physics, technology, applications
TRANSCRIPT
Physics Technology Applications
Mit Beispielen aus der Praxis
Roger Arthur Sheldon Isabel Arends and Ulf Hanefeld
Green Chemistry and Catalysis
Green Chemistryand Catalysis
Roger Arthur Sheldon
Isabel Arendsand Ulf Hanefeld
Each generation has its unique needs and aspirations When Charles Wiley firstopened his small printing shop in lower Manhattan in 1807 it was a generationof boundless potential searching for an identity And we were there helping todefine a new American literary tradition Over half a century later in the midstof the Second Industrial Revolution it was a generation focused on buildingthe future Once again we were there supplying the critical scientific technicaland engineering knowledge that helped frame the world Throughout the 20thCentury and into the new millennium nations began to reach out beyond theirown borders and a new international community was born Wiley was there ex-panding its operations around the world to enable a global exchange of ideasopinions and know-how
For 200 years Wiley has been an integral part of each generationrsquos journeyenabling the flow of information and understanding necessary to meet theirneeds and fulfill their aspirations Today bold new technologies are changingthe way we live and learn Wiley will be there providing you the must-haveknowledge you need to imagine new worlds new possibilities and new oppor-tunities
Generations come and go but you can always count on Wiley to provide youthe knowledge you need when and where you need it
William J Pesce Peter Booth WileyPresident and Chief Executive Officer Chairman of the Board
1807ndash2007 Knowledge for Generations
Physics Technology Applications
Mit Beispielen aus der Praxis
Roger Arthur Sheldon Isabel Arends and Ulf Hanefeld
Green Chemistry and Catalysis
The AuthorsProf Dr Roger SheldonDr Isabel WC E ArendsDr Ulf HanefeldBiocatalysis and Organic ChemistryDelft University of TechnologyJulianalaan 1362628 BL DelftThe Netherlands Library of Congress Card No applied for
British Library Cataloguing-in-Publication DataA catalogue record for this book is availablefrom the British Library
Bibliographic information published bythe Deutsche NationalbibliothekThe Deutsche Nationalbibliothek lists this publica-tion in the Deutsche Nationalbibliografie detailedbibliographic data are available in the Internet athttpdnbd-nbde
copy 2007 WILEY-VCH Verlag GmbH amp Co KGaAWeinheim Germany
All rights reserved (including those of translationinto other languages) No part of this book maybe reproduced in any form ndash by photoprintingmicrofilm or any other means ndash nor transmittedor translated into a machine language withoutwritten permission from the publishersRegistered names trademarks etc used in thisbook even when not specifically marked as suchare not to be considered unprotected by law
Composition K+V Fotosatz GmbH BeerfeldenPrinting betz-druck GmbH DarmstadtBookbinding Litges amp Dopf GmbH HeppenheimCover Design Schulz Grafik-Design FuszliggoumlnheimWiley Bicentennial Logo Richard J Pacifico
Printed in the Federal Republic of GermanyPrinted on acid-free paper
ISBN 978-3-527-30715-9
All books published by Wiley-VCH are carefullyproduced Nevertheless authors editors andpublisher do not warrant the information containedin these books including this book to be free oferrors Readers are advised to keep in mind thatstatements data illustrations procedural details orother items may inadvertently be inaccurate
Preface XI
Foreword XIII
1 Introduction Green Chemistry and Catalysis 111 Introduction 112 E Factors and Atom Efficiency 213 The Role of Catalysis 514 The Development of Organic Synthesis 815 Catalysis by Solid Acids and Bases 1016 Catalytic Reduction 1417 Catalytic Oxidation 1818 Catalytic CndashC Bond Formation 2319 The Question of Solvents Alternative Reaction Media 27110 Biocatalysis 29111 Renewable Raw Materials and White Biotechnology 34112 Enantioselective Catalysis 35113 Risky Reagents 38114 Process Integration and Catalytic Cascades 39
References 43
2 Solid Acids and Bases as Catalysts 4921 Introduction 4922 Solid Acid Catalysis 50221 Acidic Clays 50222 Zeolites and Zeotypes Synthesis and Structure 52223 Zeolite-catalyzed Reactions in Organic Synthesis 592231 Electrophilic Aromatic Substitutions 602232 Additions and Eliminations 652233 Rearrangements and Isomerizations 672234 Cyclizations 70224 Solid Acids Containing Surface SO3H Functionality 71225 Heteropoly Acids 75
V
Contents
23 Solid Base Catalysis 76231 Anionic Clays Hydrotalcites 76232 Basic Zeolites 80233 Organic Bases Attached to Mesoporous Silicas 8224 Other Approaches 85
References 87
3 Catalytic Reductions 9131 Introduction 9132 Heterogeneous Reduction Catalysts 92321 General Properties 92322 Transfer Hydrogenation Using Heterogeneous Catalysts 100323 Chiral Heterogeneous Reduction Catalysts 10133 Homogeneous Reduction Catalysts 104331 Wilkinson Catalyst 104332 Chiral Homogeneous Hydrogenation Catalysts and Reduction
of the C = C Double Bond 106333 Chiral Homogeneous Catalysts and Ketone Hydrogenation 111334 Imine Hydrogenation 113335 Transfer Hydrogenation using Homogeneous Catalysts 11434 Biocatalytic Reductions 116341 Introduction 116342 Enzyme Technology in Biocatalytic Reduction 119343 Whole Cell Technology for Biocatalytic Reduction 12535 Conclusions 127
References 127
4 Catalytic Oxidations 13341 Introduction 13342 Mechanisms of Metal-catalyzed Oxidations
General Considerations 134421 Homolytic Mechanisms 1364211 Direct Homolytic Oxidation of Organic Substrates 137422 Heterolytic Mechanisms 1384221 Catalytic Oxygen Transfer 139423 Ligand Design in Oxidation Catalysis 141424 Enzyme Catalyzed Oxidations 14243 Alkenes 147431 Epoxidation 1474311 Tungsten Catalysts 1494312 Rhenium Catalysts 1504313 Ruthenium Catalysts 1514314 Manganese Catalysts 1524315 Iron Catalysts 1534316 Selenium and Organocatalysts 154
ContentsVI
4317 Hydrotalcite and Alumina Systems 1564318 Biocatalytic Systems 156432 Vicinal Dihydroxylation 156433 Oxidative Cleavage of Olefins 158434 Oxidative Ketonization 159435 Allylic Oxidations 16144 Alkanes and Alkylaromatics 162441 Oxidation of Alkanes 163442 Oxidation of Aromatic Side Chains 165443 Aromatic Ring Oxidation 16845 Oxygen-containing Compounds 170451 Oxidation of Alcohols 1704511 Ruthenium Catalysts 1724512 Palladium-catalyzed Oxidations with O2 1764513 Gold Catalysts 1784514 Copper Catalysts 1794515 Other Metals as Catalysts for Oxidation with O2 1814516 Catalytic Oxidation of Alcohols with Hydrogen Peroxide 1824517 Oxoammonium Ions in Alcohol Oxidation 1834518 Biocatalytic Oxidation of Alcohols 184452 Oxidative Cleavage of 12-Diols 185453 Carbohydrate Oxidation 185454 Oxidation of Aldehydes and Ketones 1864541 Baeyer-Villiger Oxidation 187455 Oxidation of Phenols 190456 Oxidation of Ethers 19146 Heteroatom Oxidation 192461 Oxidation of Amines 1924611 Primary Amines 1924612 Secondary Amines 1934613 Tertiary Amines 1934614 Amides 194462 Sulfoxidation 19447 Asymmetric Oxidation 195471 Asymmetric Epoxidation of Olefins 196472 Asymmetric Dihydroxylation of Olefins 204473 Asymmetric Sulfoxidation 207474 Asymmetric Baeyer-Villiger Oxidation 20845 Conclusion 211
References 212
5 Catalytic CarbonndashCarbon Bond Formation 22351 Introduction 22352 Enzymes for CarbonndashCarbon Bond Formation 223521 Enzymatic Synthesis of Cyanohydrins 224
Contents VII
5211 Hydroxynitrile Lyases 2255212 Lipase-based Dynamic Kinetic Resolution 228522 Enzymatic Synthesis of -Hydroxyketones (Acyloins) 229523 Enzymatic Synthesis of -Hydroxy Acids 234524 Enzymatic Synthesis of Aldols
(-Hydroxy Carbonyl Compounds) 2355241 DHAP-dependent Aldolases 2365242 PEP- and Pyruvate-dependent Aldolases 2415243 Glycine-dependent Aldolases 2425244 Acetaldehyde-dependent Aldolases 242525 Enzymatic Synthesis of -Hydroxynitriles 24453 Transition Metal Catalysis 245531 Carbon Monoxide as a Building Block 2455311 Carbonylation of RndashX (CO ldquoInsertionR-migrationrdquo) 2455312 Aminocarbonylation 2495313 Hydroformylation or ldquoOxordquo Reaction 2505314 Hydroaminomethylation 2515315 Methyl Methacrylate via Carbonylation Reactions 253532 Heck-type Reactions 2545321 Heck Reaction 2565322 Suzuki and Sonogashira Reaction 257533 Metathesis 2585331 Metathesis involving Propylene 2595332 Ring-opening Metathesis Polymerization (ROMP) 2595333 Ring-closing Metathesis (RCM) 26054 Conclusion and Outlook 261
References 261
6 Hydrolysis 26561 Introduction 265611 Stereoselectivity of Hydrolases 266612 Hydrolase-based Preparation of Enantiopure Compounds 2686121 Kinetic Resolutions 2686122 Dynamic Kinetic Resolutions 2696123 Kinetic Resolutions Combined with Inversions 2706124 Hydrolysis of Symmetric Molecules and the ldquomeso-trickrdquo 27162 Hydrolysis of Esters 271621 Kinetic Resolutions of Esters 272622 Dynamic Kinetic Resolutions of Esters 274623 Kinetic Resolutions of Esters Combined with Inversions 276624 Hydrolysis of Symmetric Esters and the ldquomeso-trickrdquo 27863 Hydrolysis of Amides 279631 Production of Amino Acids by (Dynamic) Kinetic Resolution 2806311 The Acylase Process 2806312 The Amidase Process 281
ContentsVIII
6313 The Hydantoinase Process 2826314 Cysteine 283632 Enzyme-catalysed Hydrolysis of Amides 283633 Enzyme-catalysed Deprotection of Amines 28564 Hydrolysis of Nitriles 286641 Nitrilases 286642 Nitrile Hydratases 28765 Conclusion and Outlook 290
References 290
7 Catalysis in Novel Reaction Media 29571 Introduction 295711 Why use a solvent 295712 Choice of Solvent 296713 Alternative Reaction Media and Multiphasic Systems 29872 Two Immiscible Organic Solvents 29973 Aqueous Biphasic Catalysis 300731 Olefin Hydroformylation 302732 Hydrogenation 304733 Carbonylations 306734 Other CndashC Bond Forming Reactions 307735 Oxidations 30974 Fluorous Biphasic Catalysis 309741 Olefin Hydroformylation 310742 Other Reactions 31175 Supercritical Carbon Dioxide 313751 Supercritical Fluids 313752 Supercritical Carbon Dioxide 314753 Hydrogenation 314754 Oxidation 316755 Biocatalysis 31776 Ionic Liquids 31877 Biphasic Systems with Supercritical Carbon Dioxide 32278 Thermoregulated Biphasic Catalysis 32379 Conclusions and Prospects 323
References 324
8 Chemicals from Renewable Raw Materials 32981 Introduction 32982 Carbohydrates 332821 Chemicals from Glucose via Fermentation 333822 Ethanol 3358221 Microbial Production of Ethanol 3388222 Green Aspects 339823 Lactic Acid 340
Contents IX
824 13-Propanediol 342825 3-Hydroxypropanoic Acid 346826 Synthesizing Aromatics in Naturersquos Way 347827 Aromatic -Amino Acids 349827 Indigo the Natural Color 353828 Pantothenic Acid 355829 The -Lactam Building Block 7-Aminodesacetoxycephalosporanic
Acid 358829 Riboflavin 36183 Chemical and Chemoenzymatic Transformations of Carbohydrates
into Fine Chemicals and Chiral Building Blocks 363831 Ascorbic Acid 364832 Carbohydrate-derived C3 and C4 Building Blocks 368833 5-Hydroxymethylfurfural and Levulinic Acid 37084 Fats and Oils 372841 Biodiesel 373842 Fatty Acid Esters 37485 Terpenes 37586 Renewable Raw Materials as Catalysts 37887 Green Polymers from Renewable Raw Materials 37988 Concluding Remarks 380
References 380
9 Process Integration and Cascade Catalysis 38991 Introduction 38992 Dynamic Kinetic Resolutions by Enzymes Coupled
with Metal Catalysts 39093 Combination of Asymmetric Hydrogenation
with Enzymatic Hydrolysis 40194 Catalyst Recovery and Recycling 40295 Immobilization of Enzymes Cross-linked Enzyme Aggregates
(CLEAs) 40596 Conclusions and Prospects 406
References 407
10 Epilogue Future Outlook 409101 Green Chemistry The Road to Sustainability 409102 Catalysis and Green Chemistry 410103 The Medium is the Message 412104 Metabolic Engineering and Cascade Catalysis 413105 Concluding Remarks 413
References 414
Subject Index 415
ContentsX
The publication of books such as Silent Spring by Rachel Carson and The ClosingCircle by Barry Commoner in the late 1960s and early 1970s focused attentionon the negative side effects of industrial and economic growth on our naturalenvironment However the resulting environmental movement was not fullyendorsed by the chemical industry It was the publication two decades later in1987 of the report Our Common Future by the World Commission on Environ-ment and Development which marked a turning point in industrial and societalimpact The report emphasized that industrial development must be sustainableover time that is it must meet the needs of the present generation withoutcompromising the ability of future generations to meet their own needs Sus-tainable development has subsequently become a catch phrase of industry inthe 21st century and the annual reports and mission statements of many cor-porations endorse the concept of sustainability
At roughly the same time in the early 1990s the concept of green chemistryemerged A workable definition is Green chemistry efficiently utilizes (preferably re-newable) raw materials eliminates waste and avoids the use of toxic andor hazardousreagents and solvents in the manufacture and application of chemical products On re-flection it becomes abundantly clear that if sustainability is the goal of society inthe 21st century then green chemistry is the means to achieve it in the chemicalindustry at least A key feature is that greenness and sustainability need to be in-cluded in designing the product andor process from the outset (benign by de-sign) The basic premise of this book is that a major driver towards green chem-istry is the widespread application of clean catalytic methodologies in the manu-facture of chemicals hence its title Green Chemistry and Catalysis
The book is primarily aimed at researchers in industry or academia who areinvolved in developing processes for chemicals manufacture It could also formthe basis for an advanced undergraduate or post-graduate level course on greenchemistry Indeed the material is used by the authors for this very purpose inDelft
The main underlying theme is the application of catalytic methodologies ndashhomogeneous heterogeneous and enzymatic ndash to industrial organic synthesisThe material is divided based on the type of transformation rather than the typeof catalyst This provides for a comparison of the different methodologies egchemo- vs biocatalytic for achieving a particular conversion
XI
Preface
Chapter 1 gives an introduction to the overall theme of green chemistry andcatalysis emphasizing the importance of concepts such as atom efficiency andE factors (kg wastekg product) for assessing the environmental impact orlsquogreennessrsquo of a process In this context it is emphasized that it is not really aquestion of green vs not green but rather one of one process being greener thananother that is there are lsquomany shades of greenrsquo Chapter 2 is concerned withreplacing traditional acids and bases with solid recyclable ones thereby dramati-cally reducing the amount of waste formed Chapters 3 and 4 cover the applica-tion of catalytic methodologies to reductions and oxidations two pivotal pro-cesses in organic synthesis
Chapter 5 is concerned with C-C bond forming reactions and Chapter 6 withsolvolytic processes which mainly consist of enzyme-catalyzed transformations
Chapter 7 addresses another key topic in the context of green chemistry thereplacement of traditional environmentally unattractive organic solvents bygreener alternative reaction media such as water supercritical carbon dioxideionic liquids and perfluorous solvents The use of liquidliquid biphasic systemsprovides the additional benefit of facile catalyst recovery and recycling
Another key topic ndash renewable resources ndash is addressed in Chapter 8 The uti-lization of fossil resources as sources of energy and chemical feedstocks isclearly unsustainable and needs to be replaced by the use of renewable biomassSuch a switch is also desirable for other reasons such as biocompatibility biode-gradability and lower toxicity of the products compared to their oil-derived coun-terparts Here again the application of chemo- and biocatalysis will play an im-portant underlying role
Chapter 9 is concerned with the integration of catalytic methodologies in or-ganic synthesis and with downstream processing The ultimate green processinvolves the integration of several catalytic steps into catalytic cascade processesthus emulating the multi-enzyme processes which are occurring in the livingcell Chapter 10 consists of the Conclusions and Future Prospects
The principal literature has been covered up to 2006 and an extensive list ofreferences is included at the end of each chapter The index has been thor-oughly cross-referenced and the reader is encouraged to seek the various topicsunder more than one entry
Finally we wish to acknowledge the important contribution of our colleagueFred van Rantwijk to writing Chapter 8
Roger SheldonIsabel ArendsUlf Hanefeld
Delft November 2006
PrefaceXII
Green Chemistry was born around 1990 However it was in 1992 with the in-vention of the E-factor by Roger Sheldon that Green Chemistry really cut itsteeth For the first time Chemists had a simple metric for judging the environ-mental impact of their processes
As the subject has developed it has become increasingly clear that catalysis isone of the central tools for the greening of chemistry Catalysis not only can im-prove the selectivity of a reaction but also by doing so it can decrease or evenremove the need for downstream processing thereby reducing the material andenergy waste associated with purification This is particularly important becausethe solvent requirements for recrystallization chromatography and other purifi-cation processes are often much greater than the usage of solvent in the origi-nal reaction
Thus it gives me great pleasure to write this Foreword because this book isone of the first to bring together catalysis and Green Chemistry in a single vol-ume Furthermore it is a real book not a mere collection of separate chaptersthrown together by a whole football team of authors So as you read the bookyou can see the links the synergies and even the occasional contradictions be-tween the different topics
Roger Sheldon and his coauthors Isabel Arends and Ulf Hanefeld have avery broad knowledge of current industrial processes and this knowledge comesthrough clearly over and over again in this book This means that readers aregetting two books for the price of one firstly a detailed summary of the varioustypes of catalysis which can be applied to Green Chemistry and secondly a con-cise snapshot of new catalytic processes which have been commercialised in re-cent years Indeed it is quite possible that this snapshot will become a bench-mark by which the rate of future industrial innovation can be judged
Green Chemistry is now in its teens and like any teenager it shows promisebut has not yet reached its full potential No longer are 10 kilograms of solventrequired to make each 100 mg tablet of a leading antidepressant now we needonly 4 kilograms So there is still a long way to go till we reach truly sustainablechemical production Thus I believe that this book has a potentially muchgreater value than just describing the status quo By showing what has beenachieved it hints at what could be achieved if only chemical intuition and ima-gination were properly focussed in an attack on the dirtier aspects of current
XIII
Foreword
chemical manufacture I sincerely hope that this book will inspire a whole newgeneration of Green Chemists and enable them to realise their own vision of asustainable chemical future
Martyn PoliakoffSchool of Chemistry
The University of Nottingham UKNovember 2006
ForewordXIV
11Introduction
It is widely acknowledged that there is a growing need for more environmen-tally acceptable processes in the chemical industry This trend towards what hasbecome known as lsquoGreen Chemistryrsquo [1ndash9] or lsquoSustainable Technologyrsquo necessi-tates a paradigm shift from traditional concepts of process efficiency that focuslargely on chemical yield to one that assigns economic value to eliminatingwaste at source and avoiding the use of toxic andor hazardous substances
The term lsquoGreen Chemistryrsquo was coined by Anastas [3] of the US Environ-mental Protection Agency (EPA) In 1993 the EPA officially adopted the namelsquoUS Green Chemistry Programrsquo which has served as a focal point for activitieswithin the United States such as the Presidential Green Chemistry ChallengeAwards and the annual Green Chemistry and Engineering Conference Thisdoes not mean that research on green chemistry did not exist before the early1990s merely that it did not have the name Since the early 1990s both Italyand the United Kingdom have launched major initiatives in green chemistryand more recently the Green and Sustainable Chemistry Network was initiatedin Japan The inaugural edition of the journal Green Chemistry sponsored bythe Royal Society of Chemistry appeared in 1999 Hence we may conclude thatGreen Chemistry is here to stay
A reasonable working definition of green chemistry can be formulated as fol-lows [10] Green chemistry efficiently utilizes (preferably renewable) raw materialseliminates waste and avoids the use of toxic andor hazardous reagents and solventsin the manufacture and application of chemical products
As Anastas has pointed out the guiding principle is the design of environ-mentally benign products and processes (benign by design) [4] This concept isembodied in the 12 Principles of Green Chemistry [1 4] which can be para-phrased as1 Waste prevention instead of remediation2 Atom efficiency3 Less hazardoustoxic chemicals4 Safer products by design5 Innocuous solvents and auxiliaries
1
1Introduction Green Chemistry and Catalysis
6 Energy efficient by design7 Preferably renewable raw materials8 Shorter syntheses (avoid derivatization)9 Catalytic rather than stoichiometric reagents
10 Design products for degradation11 Analytical methodologies for pollution prevention12 Inherently safer processes
Green chemistry addresses the environmental impact of both chemical productsand the processes by which they are produced In this book we shall be con-cerned only with the latter ie the product is a given and the goal is to design agreen process for its production Green chemistry eliminates waste at sourceie it is primary pollution prevention rather than waste remediation (end-of-pipesolutions) Prevention is better than cure (the first principle of green chemistryoutlined above)
An alternative term that is currently favored by the chemical industry is Sus-tainable Technologies Sustainable development has been defined as [11] Meet-ing the needs of the present generation without compromising the ability of future gen-erations to meet their own needs
One could say that Sustainability is the goal and Green Chemistry is themeans to achieve it
12E Factors and Atom Efficiency
Two useful measures of the potential environmental acceptability of chemicalprocesses are the E factor [12ndash18] defined as the mass ratio of waste to desiredproduct and the atom efficiency calculated by dividing the molecular weight ofthe desired product by the sum of the molecular weights of all substances pro-duced in the stoichiometric equation The sheer magnitude of the waste prob-lem in chemicals manufacture is readily apparent from a consideration of typi-cal E factors in various segments of the chemical industry (Table 11)
The E factor is the actual amount of waste produced in the process definedas everything but the desired product It takes the chemical yield into accountand includes reagents solvents losses all process aids and in principle evenfuel (although this is often difficult to quantify) There is one exception wateris generally not included in the E factor For example when considering anaqueous waste stream only the inorganic salts and organic compounds con-tained in the water are counted the water is excluded Otherwise this wouldlead to exceptionally high E factors which are not useful for comparing pro-cesses [8]
A higher E factor means more waste and consequently greater negative envi-ronmental impact The ideal E factor is zero Put quite simply it is kilograms(of raw materials) in minus kilograms of desired product divided by kilograms
1 Introduction Green Chemistry and Catalysis2
of product out It can be easily calculated from a knowledge of the number oftons of raw materials purchased and the number of tons of product sold for aparticular product or a production site or even a whole company It is perhapssurprising therefore that many companies are not aware of the E factors oftheir processes We hasten to point out however that this situation is rapidlychanging and the E factor or an equivalent thereof (see later) is being widelyadopted in the fine chemicals and pharmaceutical industries (where the need isgreater) We also note that this method of calculation will automatically excludewater used in the process but not water formed
Other metrics have also been proposed for measuring the environmental ac-ceptability of processes Hudlicky and coworkers [19] for example proposed theeffective mass yield (EMY) which is defined as the percentage of product of allthe materials used in its preparation As proposed it does not include so-calledenvironmentally benign compounds such as NaCl acetic acid etc As we shallsee later this is questionable as the environmental impact of such substances isvery volume-dependent Constable and coworkers of GlaxoSmithKline [20] pro-posed the use of mass intensity (MI) defined as the total mass used in a pro-cess divided by the mass of product ie MI= E factor+ 1 and the ideal MI is 1compared with zero for the E factor These authors also suggest the use of so-called mass productivity which is the reciprocal of the MI and hence is effec-tively the same as EMY
In our opinion none of these alternative metrics appears to offer any particu-lar advantage over the E factor for giving a mental picture of how wasteful aprocess is Hence we will use the E factor in further discussions
As is clear from Table 11 enormous amounts of waste comprising primarilyinorganic salts such as sodium chloride sodium sulfate and ammonium sul-fate are formed in the reaction or in subsequent neutralization steps The E fac-tor increases dramatically on going downstream from bulk to fine chemicalsand pharmaceuticals partly because production of the latter involves multi-stepsyntheses but also owing to the use of stoichiometric reagents rather than cata-lysts (see later)
12 E Factors and Atom Efficiency 3
Table 11 The E factor
Industry segment Product tonnage a) kg waste b)kg product
Oil refining 106ndash108 lt 01Bulk chemicals 104ndash106 lt 1ndash5Fine chemicals 102ndash104 5ndashgt50Pharmaceuticals 10ndash103 25ndashgt100
a) Typically represents annual production volume of a productat one site (lower end of range) or world-wide (upper end ofrange)
b) Defined as everything produced except the desired product(including all inorganic salts solvent losses etc)
The atom utilization [13ndash18] atom efficiency or atom economy concept firstintroduced by Trost [21 22] is an extremely useful tool for rapid evaluation ofthe amounts of waste that will be generated by alternative processes It is calcu-lated by dividing the molecular weight of the product by the sum total of themolecular weights of all substances formed in the stoichiometric equation forthe reaction involved For example the atom efficiencies of stoichiometric(CrO3) vs catalytic (O2) oxidation of a secondary alcohol to the correspondingketone are compared in Fig 11
In contrast to the E factor it is a theoretical number ie it assumes a yield of100 and exactly stoichiometric amounts and disregards substances which donot appear in the stoichiometric equation A theoretical E factor can be derivedfrom the atom efficiency eg an atom efficiency of 40 corresponds to an Efactor of 15 (6040) In practice however the E factor will generally be muchhigher since the yield is not 100 and an excess of reagent(s) is used and sol-vent losses and salt generation during work-up have to be taken into account
An interesting example to further illustrate the concepts of E factors andatom efficiency is the manufacture of phloroglucinol [23] Traditionally it wasproduced from 246-trinitrotoluene (TNT) as shown in Fig 12 a perfect exam-ple of nineteenth century organic chemistry
This process has an atom efficiency of lt 5 and an E factor of 40 ie it gen-erates 40 kg of solid waste containing Cr2(SO4)3 NH4Cl FeCl2 and KHSO4 perkg of phloroglucinol (note that water is not included) and obviously belongs ina museum of industrial archeology
All of the metrics discussed above take only the mass of waste generated intoaccount However what is important is the environmental impact of this wastenot just its amount ie the nature of the waste must be considered One kg ofsodium chloride is obviously not equivalent to one kg of a chromium saltHence the term lsquoenvironmental quotientlsquo EQ obtained by multiplying the Efactor with an arbitrarily assigned unfriendliness quotient Q was introduced[15] For example one could arbitrarily assign a Q value of 1 to NaCl and say100ndash1000 to a heavy metal salt such as chromium depending on its toxicityease of recycling etc The magnitude of Q is obviously debatable and difficultto quantify but importantly lsquoquantitative assessmentrsquo of the environmental im-
1 Introduction Green Chemistry and Catalysis4
Fig 11 Atom efficiency of stoichiometric vs catalytic oxidation of an alcohol
pact of chemical processes is in principle possible It is also worth noting thatQ for a particular substance can be both volume-dependent and influenced bythe location of the production facilities For example the generation of 100ndash1000 tons per annum of sodium chloride is unlikely to present a waste prob-lem and could be given a Q of zero The generation of 10 000 tons per annumon the other hand may already present a disposal problem and would warrantassignation of a Q value greater than zero Ironically when very large quantitiesof sodium chloride are generated the Q value could decrease again as recyclingby electrolysis becomes a viable proposition eg in propylene oxide manufac-ture via the chlorohydrin route Thus generally speaking the Q value of a par-ticular waste will be determined by its ease of disposal or recycling Hydrogenbromide for example could warrant a lower Q value than hydrogen chloride asrecycling via oxidation to bromine is easier In some cases the waste productmay even have economic value For example ammonium sulfate produced aswaste in the manufacture of caprolactam can be sold as fertilizer It is worthnoting however that the market could change in the future thus creating awaste problem for the manufacturer
13The Role of Catalysis
As noted above the waste generated in the manufacture of organic compoundsconsists primarily of inorganic salts This is a direct consequence of the use ofstoichiometric inorganic reagents in organic synthesis In particular fine chemi-cals and pharmaceuticals manufacture is rampant with antiquated lsquostoichio-metricrsquo technologies Examples which readily come to mind are stoichiometricreductions with metals (Na Mg Zn Fe) and metal hydride reagents (LiAlH4
13 The Role of Catalysis 5
Fig 12 Phloroglucinol from TNT
NaBH4) oxidations with permanganate manganese dioxide and chromium(VI)reagents and a wide variety of reactions eg sulfonations nitrations halogena-tions diazotizations and Friedel-Crafts acylations employing stoichiometricamounts of mineral acids (H2SO4 HF H3PO4) and Lewis acids (AlCl3 ZnCl2BF3) The solution is evident substitution of classical stoichiometric methodolo-gies with cleaner catalytic alternatives Indeed a major challenge in (fine) che-micals manufacture is to develop processes based on H2 O2 H2O2 CO CO2
and NH3 as the direct source of H O C and N Catalytic hydrogenation oxida-tion and carbonylation (Fig 13) are good examples of highly atom efficientlow-salt processes
The generation of copious amounts of inorganic salts can similarly be largelycircumvented by replacing stoichiometric mineral acids such as H2SO4 and Le-wis acids and stoichiometric bases such as NaOH KOH with recyclable solidacids and bases preferably in catalytic amounts (see later)
For example the technologies used for the production of many substitutedaromatic compounds (Fig 14) have not changed in more than a century andare therefore ripe for substitution by catalytic low-salt alternatives (Fig 15)
An instructive example is provided by the manufacture of hydroquinone(Fig 16) [24] Traditionally it was produced by oxidation of aniline with stoichio-metric amounts of manganese dioxide to give benzoquinone followed by reduc-tion with iron and hydrochloric acid (Beacutechamp reduction) The aniline was de-rived from benzene via nitration and Beacutechamp reduction The overall processgenerated more than 10 kg of inorganic salts (MnSO4 FeCl2 NaCl Na2SO4) perkg of hydroquinone This antiquated process has now been replaced by a moremodern route involving autoxidation of p-diisopropylbenzene (produced by Frie-del-Crafts alkylation of benzene) followed by acid-catalysed rearrangement ofthe bis-hydroperoxide producing lt 1 kg of inorganic salts per kg of hydroqui-none Alternatively hydroquinone is produced (together with catechol) by tita-
1 Introduction Green Chemistry and Catalysis6
Fig 13 Atom efficient catalytic processes
nium silicalite (TS-1)-catalysed hydroxylation of phenol with aqueous hydrogenperoxide (see later)
Biocatalysis has many advantages in the context of green chemistry eg mildreaction conditions and often fewer steps than conventional chemical proce-dures because protection and deprotection of functional groups are often not re-quired Consequently classical chemical procedures are increasingly being re-placed by cleaner biocatalytic alternatives in the fine chemicals industry (seelater)
13 The Role of Catalysis 7
Fig 14 Classical aromatic chemistry
Fig 15 Non-classical aromatic chemistry
14The Development of Organic Synthesis
If the solution to the waste problem in the fine chemicals industry is so obviousndash replacement of classical stoichiometric reagents with cleaner catalytic alterna-tives ndash why was it not applied in the past We suggest that there are several rea-sons for this First because of the smaller quantities compared with bulk che-micals the need for waste reduction in fine chemicals was not widely appre-ciated
A second underlying reason is the more or less separate evolution of organicchemistry and catalysis (Fig 17) since the time of Berzelius who coined bothterms in 1807 and 1835 respectively [25] Catalysis subsequently developed as asubdiscipline of physical chemistry and is still often taught as such in univer-sity undergraduate courses With the advent of the petrochemicals industry inthe 1930s catalysis was widely applied in oil refining and bulk chemicals manu-facture However the scientists responsible for these developments which large-ly involved heterogeneous catalysts in vapor phase reactions were generally notorganic chemists
Organic synthesis followed a different line of evolution A landmark was Per-kinrsquos serendipitous synthesis of mauveine (aniline purple) in 1856 [26] whichmarked the advent of the synthetic dyestuffs industry based on coal tar as theraw material The present day fine chemicals and pharmaceutical industriesevolved largely as spin-offs of this activity Coincidentally Perkin was trying tosynthesise the anti-malarial drug quinine by oxidation of a coal tar-based rawmaterial allyl toluidine using stoichiometric amounts of potassium dichromateFine chemicals and pharmaceuticals have remained primarily the domain of
1 Introduction Green Chemistry and Catalysis8
Fig 16 Two routes to hydroquinone
synthetic organic chemists who generally speaking have clung to the use ofclassical ldquostoichiometricrdquo methodologies and have been reluctant to apply cataly-tic alternatives
A third reason which partly explains the reluctance is the pressure of timeFine chemicals generally have a much shorter lifecycle than bulk chemicalsand especially in pharmaceuticals lsquotime to marketrsquo is crucial An advantage ofmany time-honored classical technologies is that they are well-tried and broadlyapplicable and hence can be implemented rather quickly In contrast the de-velopment of a cleaner catalytic alternative could be more time consumingConsequently environmentally (and economically) inferior technologies are of-ten used to meet market deadlines Moreover in pharmaceuticals subsequentprocess changes are difficult to realise owing to problems associated with FDAapproval
There is no doubt that in the twentieth century organic synthesis hasachieved a high level of sophistication with almost no molecule beyond its cap-abilities with regard to chemo- regio- and stereoselectivity for example How-ever little attention was focused on atom selectivity and catalysis was only spor-adically applied Hence what we now see is a paradigm change under themounting pressure of environmental legislation organic synthesis and catalysisafter 150 years in splendid isolation have come together again The key towaste minimisation is precision in organic synthesis where every atom countsIn this chapter we shall briefly review the various categories of catalytic pro-
14 The Development of Organic Synthesis 9
Fig 17 Development of catalysis and organic synthesis
cesses with emphasis on fine chemicals but examples of bulk chemicals willalso be discussed where relevant
15Catalysis by Solid Acids and Bases
As noted above a major source of waste in the (fine) chemicals industry is de-rived from the widespread use of liquid mineral acids (HF H2SO4) and a vari-ety of Lewis acids They cannot easily be recycled and generally end up via ahydrolytic work-up as waste streams containing large amounts of inorganicsalts Their widespread replacement by recyclable solid acids would afford a dra-matic reduction in waste Solid acids such as zeolites acidic clays and relatedmaterials have many advantages in this respect [27ndash29] They are often trulycatalytic and can easily be separated from liquid reaction mixtures obviatingthe need for hydrolytic work-up and recycled Moreover solid acids are non-cor-rosive and easier (safer) to handle than mineral acids such as H2SO4 or HF
Solid acid catalysts are in principle applicable to a plethora of acid-promotedprocesses in organic synthesis [27ndash29] These include various electrophilic aro-matic substitutions eg nitrations and Friedel-Crafts alkylations and acylationsand numerous rearrangement reactions such as the Beckmann and Fries rear-rangements
A prominent example is Friedel-Crafts acylation a widely applied reaction in thefine chemicals industry In contrast to the corresponding alkylations which aretruly catalytic processes Friedel-Crafts acylations generally require more thanone equivalent of for example AlCl3 or BF3 This is due to the strong complexa-tion of the Lewis acid by the ketone product The commercialisation of the firstzeolite-catalysed Friedel-Crafts acylation by Rhocircne-Poulenc (now Rhodia) may beconsidered as a benchmark in this area [30 31] Zeolite beta is employed as a cat-alyst in fixed-bed operation for the acetylation of anisole with acetic anhydride togive p-methoxyacetophenone (Fig 18) The original process used acetyl chloridein combination with 11 equivalents of AlCl3 in a chlorinated hydrocarbon solventand generated 45 kg of aqueous effluent containing AlCl3 HCl solvent residuesand acetic acid per kg of product The catalytic alternative in stark contrast avoidsthe production of HCl in both the acylation and in the synthesis of acetyl chlorideIt generates 0035 kg of aqueous effluent ie more than 100 times less consistingof 99 water 08 acetic acid and lt 02 other organics and requires no solventFurthermore a product of higher purity is obtained in higher yield (gt95 vs 85ndash95) the catalyst is recyclable and the number of unit operations is reduced fromtwelve to two Hence the Rhodia process is not only environmentally superior tothe traditional process it has more favorable economics This is an important con-clusion green catalytic chemistry in addition to having obvious environmentalbenefits is also economically more attractive
Another case in point pertains to the manufacture of the bulk chemical ca-prolactam the raw material for Nylon 6 The conventional process (Fig 19) in-
1 Introduction Green Chemistry and Catalysis10
volves the reaction of cyclohexanone with hydroxylamine sulfate (or anothersalt) producing cyclohexanone oxime which is subjected to the Beckmann rear-rangement in the presence of stoichiometric amounts of sulfuric acid or oleumThe overall process generates ca 45 kg of ammonium sulfate per kg of capro-lactam divided roughly equally over the two steps
15 Catalysis by Solid Acids and Bases 11
Fig 18 Zeolite-catalysed vs classical Friedel-Crafts acylation
Fig 19 Sumitomo vs conventional process for caprolactam manufacture
Ichihashi and coworkers at Sumitomo [32 33] developed a catalytic vaporphase Beckmann rearrangement over a high-silica MFI zeolite When this iscombined with the technology developed by Enichem [34] for the ammoxima-tion of cyclohexanone with NH3H2O2 over the titanium silicalite catalyst (TS-1)described earlier this affords caprolactam in gt 98 yield (based on cyclohexa-none 93 based on H2O2) The overall process generates caprolactam and twomolecules of water from cyclohexanone NH3 and H2O2 and is essentially salt-free This process is currently being commercialised by Sumitomo in Japan
Another widely used reaction in fine chemicals manufacture is the acid-cata-lysed rearrangement of epoxides to carbonyl compounds Lewis acids such asZnCl2 or BF3 middot OEt2 are generally used often in stoichiometric amounts to per-form such reactions Here again zeolites can be used as solid recyclable cata-lysts Two commercially relevant examples are the rearrangements of -pineneoxide [35 36] and isophorone oxide [37] shown in Fig 110 The products ofthese rearrangements are fragrance intermediates The rearrangement of -pinene oxide to campholenic aldehyde was catalysed by H-USY zeolite [35] andtitanium-substituted zeolite beta [36] With the latter selectivities up to 89 inthe liquid phase and 94 in the vapor phase were obtained exceeding the bestresults obtained with homogeneous Lewis acids
As any organic chemist will tell you the conversion of an amino acid to thecorresponding ester also requires more than one equivalent of a Broslashnsted acidThis is because an amino acid is a zwitterion and in order to undergo acid cata-lysed esterification the carboxylate anion needs to be protonated with oneequivalent of acid However it was shown [38] that amino acids undergo esteri-fication in the presence of a catalytic amount of zeolite H-USY the very samecatalyst that is used in naphtha cracking thus affording a salt-free route to ami-no acid esters (Fig 111) This is a truly remarkable reaction in that a basic com-pound (the amino ester) is formed in the presence of an acid catalyst Esterifica-tion of optically active amino acids under these conditions (MeOH 100 C) un-
1 Introduction Green Chemistry and Catalysis12
Fig 110 Zeolite-catalysed epoxide rearrangements
fortunately led to (partial) racemisation The reaction could be of interest for thesynthesis of racemic phenylalanine methyl ester the raw material in the DSM-Tosoh process for the artificial sweetener aspartame
In the context of replacing conventional Lewis acids in organic synthesis it isalso worth pointing out that an alternative approach is to use lanthanide salts[39] that are both water soluble and stable towards hydrolysis and exhibit a vari-ety of interesting activities as Lewis acids (see later)
The replacement of conventional bases such as NaOH KOH and NaOMe byrecyclable solid bases in a variety of organic reactions is also a focus of recentattention [27 40] For example synthetic hydrotalcite clays otherwise known aslayered double hydroxides (LDHs) and having the general formula Mg8-xAlx(OH)16(CO3)x2 middot nH2O are hydrated aluminum-magnesium hydroxides possess-
15 Catalysis by Solid Acids and Bases 13
Fig 111 Salt-free esterification of amino acids
Fig 112 Hydrotalcite-catalysed condensation reactions
ing a lamellar structure in which the excess positive charge is compensated bycarbonate anions in the interlamellar space [41 42] Calcination transforms hy-drotalcites via dehydroxylation and decarbonation into strongly basic mixedmagnesium-aluminum oxides that are useful recyclable catalysts for inter aliaaldol [43] Knoevenagel [44 45] and Claisen-Schmidt [45] condensations Someexamples are shown in Fig 112
Another approach to designing recyclable solid bases is to attach organicbases to the surface of eg mesoporous silicas (Fig 113) [46ndash48] For exampleaminopropyl-silica resulting from reaction of 3-aminopropyl(trimethoxy)silanewith pendant silanol groups was an active catalyst for Knoevenagel condensa-tions [49] A stronger solid base was obtained by functionalisation of mesopor-ous MCM-41 with the guanidine base 157-triazabicyclo-[440]dec-5-ene (TBD)using a surface glycidylation technique followed by reaction with TBD(Fig 113) The resulting material was an active catalyst for Knoevenagel con-densations Michael additions and Robinson annulations [50]
16Catalytic Reduction
Catalytic hydrogenation perfectly embodies the concept of precision in organicsynthesis Molecular hydrogen is a clean and abundant raw material and cataly-tic hydrogenations are generally 100 atom efficient with the exception of afew examples eg nitro group reduction in which water is formed as a copro-duct They have a tremendously broad scope and exhibit high degrees of che-
1 Introduction Green Chemistry and Catalysis14
Fig 113 Tethered organic bases as solid base catalysts
mo- regio- diastereo and enantioselectivity [51 52] The synthetic prowess ofcatalytic hydrogenation is admirably rendered in the words of Rylander [51]
ldquoCatalytic hydrogenation is one of the most useful and versatile tools avail-able to the organic chemist The scope of the reaction is very broad mostfunctional groups can be made to undergo reduction frequently in high yieldto any of several products Multifunctional molecules can often be reduced se-lectively at any of several functions A high degree of stereochemical control ispossible with considerable predictability and products free of contaminatingreagents are obtained easily Scale up of laboratory experiments to industrialprocesses presents little difficultyrdquoPaul Rylander (1979)
Catalytic hydrogenation is unquestionably the workhorse of catalytic organicsynthesis with a long tradition dating back to the days of Sabatier [53] who re-ceived the 1912 Nobel Prize in Chemistry for his pioneering work in this areaIt is widely used in the manufacture of fine and specialty chemicals and a spe-cial issue of the journal Advanced Synthesis and Catalysis was recently devotedto this important topic [54] According to Roessler [55] 10ndash20 of all the reac-tion steps in the synthesis of vitamins (even 30 for vitamin E) at Hoffmann-La Roche (in 1996) are catalytic hydrogenations
Most of the above comments apply to heterogeneous catalytic hydrogenationsover supported Group VIII metals (Ni Pd Pt etc) They are equally true how-ever for homogeneous catalysts where spectacular progress has been made inthe last three decades culminating in the award of the 2001 Nobel Prize inChemistry to WS Knowles and R Noyori for their development of catalyticasymmetric hydrogenation (and to KB Sharpless for asymmetric oxidation cata-lysis) [56] Recent trends in the application of catalytic hydrogenation in finechemicals production with emphasis on chemo- regio- and stereoselectivityusing both heterogeneous and homogeneous catalysts is the subject of an excel-lent review by Blaser and coworkers [57]
A major trend in fine chemicals and pharmaceuticals is towards increasinglycomplex molecules which translates to a need for high degrees of chemo- re-gio- and stereoselectivity An illustrative example is the synthesis of an inter-mediate for the Roche HIV protease inhibitor Saquinavir (Fig 114) [55] It in-volves a chemo- and diastereoselective hydrogenation of an aromatic whileavoiding racemisation at the stereogenic centre present in the substrate
The chemoselective hydrogenation of one functional group in the presence ofother reactive groups is a frequently encountered problem in fine chemicalsmanufacture An elegant example of the degree of precision that can beachieved is the chemoselective hydrogenation of an aromatic nitro group in thepresence of both an olefinic double bond and a chlorine substituent in the aro-matic ring (Fig 115) [58]
Although catalytic hydrogenation is a mature technology that is widely ap-plied in industrial organic synthesis new applications continue to appear some-times in unexpected places For example a time-honored reaction in organic
16 Catalytic Reduction 15
synthesis is the Williamson synthesis of ethers first described in 1852 [59] Alow-salt catalytic alternative to the Williamson synthesis involving reductive al-kylation of an aldehyde (Fig 116) has been reported [60] This avoids the copro-duction of NaCl which may or may not be a problem depending on the pro-duction volume (see earlier) Furthermore the aldehyde may in some cases bemore readily available than the corresponding alkyl chloride
The Meerwein-Pondorff-Verley (MPV) reduction of aldehydes and ketones tothe corresponding alcohols [61] is another example of a long-standing technol-ogy The reaction mechanism involves coordination of the alcohol reagentusually isopropanol and the ketone substrate to the aluminum center followedby hydride transfer from the alcohol to the carbonyl group In principle the re-
1 Introduction Green Chemistry and Catalysis16
Fig 114 Synthesis of a Saquinavir intermediate
Fig 115 Chemoselective hydrogenation of a nitro group
Fig 116 Williamson ether synthesis and a catalytic alternative
action is catalytic in aluminum alkoxide but in practice it generally requiresstoichiometric amounts owing to the slow rate of exchange of the alkoxy groupin aluminum alkoxides Recently van Bekkum and coworkers [62 63] showedthat Al- and Ti-Beta zeolites are able to catalyse MPV reductions The reaction istruly catalytic and the solid catalyst can be readily separated by simple filtrationand recycled An additional benefit is that confinement of the substrate in thezeolite pores can afford interesting shape selectivities For example reduction of4-tert-butylcyclohexanone led to the formation of the thermodynamically lessstable cis-alcohol an important fragrance intermediate in high (gt95) selectiv-ity (Fig 117) In contrast conventional MPV reduction gives the thermodyna-mically more stable but less valuable trans-isomer Preferential formation ofthe cis-isomer was attributed to transition state selectivity imposed by confine-ment in the zeolite pores
More recently Corma and coworkers [64] have shown that Sn-substituted zeo-lite beta is a more active heterogeneous catalyst for MPV reductions also show-ing high cis-selectivity (99ndash100) in the reduction of 4-alkylcyclohexanones Thehigher activity was attributed to the higher electronegativity of Sn compared toTi
The scope of catalytic hydrogenations continues to be extended to more diffi-cult reductions For example a notoriously difficult reduction in organic synthe-sis is the direct conversion of carboxylic acids to the corresponding aldehydes Itis usually performed indirectly via conversion to the corresponding acid chlorideand Rosenmund reduction of the latter over PdBaSO4 [65] Rhocircne-Poulenc [30]and Mitsubishi [66] have developed methods for the direct hydrogenation of aro-matic aliphatic and unsaturated carboxylic acids to the corresponding alde-hydes over a RuSn alloy and zirconia or chromia catalysts respectively in thevapor phase (Fig 118)
Finally it is worth noting that significant advances have been made in the uti-lisation of biocatalytic methodologies for the (asymmetric) reduction of for ex-ample ketones to the corresponding alcohols (see later)
16 Catalytic Reduction 17
Fig 117 Zeolite beta catalysed MPV reduction
Fig 118 Direct hydrogenation of carboxylic acids to aldehydes
17Catalytic Oxidation
It is probably true to say that nowhere is there a greater need for green catalyticalternatives in fine chemicals manufacture than in oxidation reactions In con-trast to reductions oxidations are still largely carried out with stoichiometric in-organic (or organic) oxidants such as chromium(VI) reagents permanganatemanganese dioxide and periodate There is clearly a definite need for catalyticalternatives employing clean primary oxidants such as oxygen or hydrogen per-oxide Catalytic oxidation with O2 is widely used in the manufacture of bulk pet-rochemicals [67] Application to fine chemicals is generally more difficult how-ever owing to the multifunctional nature of the molecules of interest Nonethe-less in some cases such technologies have been successfully applied to themanufacture of fine chemicals An elegant example is the BASF process [68] forthe synthesis of citral (Fig 119) a key intermediate for fragrances and vitaminsA and E The key step is a catalytic vapor phase oxidation over a supported sil-ver catalyst essentially the same as that used for the manufacture of formalde-hyde from methanol
This atom efficient low-salt process has displaced the traditional route start-ing from -pinene which involved inter alia a stoichiometric oxidation withMnO2 (Fig 119)
The selective oxidation of alcohols to the corresponding carbonyl compoundsis a pivotal transformation in organic synthesis As noted above there is an ur-gent need for greener methodologies for these conversions preferably employ-ing O2 or H2O2 as clean oxidants and effective with a broad range of substratesOne method which is finding increasing application in the fine chemicals in-dustry employs the stable free radical TEMPO 2266-tetramethylpiperidine-N-oxyl) as a catalyst and NaOCl (household bleach) as the oxidant [69] For exam-ple this methodology was used with 4-hydroxy TEMPO as the catalyst as thekey step in a new process for the production of progesterone from stigmasterola soy sterol (Fig 120) [70]
This methodology still suffers from the shortcomings of salt formation andthe use of bromide (10 mol) as a cocatalyst and dichloromethane as solventRecently a recyclable oligomeric TEMPO derivative PIPO derived from a com-mercially available polymer additive (Chimasorb 944) was shown to be an effec-tive catalyst for the oxidation of alcohols with NaOCl in the absence of bromideion using neat substrate or in eg methyl tert-butyl ether (MTBE) as solvent(Fig 121) [71]
Another improvement is the use of a RuTEMPO catalyst combination forthe selective aerobic oxidations of primary and secondary alcohols to the corre-sponding aldehydes and ketones respectively (Fig 122) [72] The method is ef-fective (gt99 selectivity) with a broad range of primary and secondary aliphaticallylic and benzylic alcohols The overoxidation of aldehydes to the correspond-ing carboxylic acids is suppressed by the TEMPO which acts as a radical scaven-ger in preventing autoxidation
1 Introduction Green Chemistry and Catalysis18
Another recent development is the use of water soluble palladium complexesas recyclable catalysts for the aerobic oxidation of alcohols in aqueousorganicbiphasic media (Fig 122) [73]
In the fine chemicals industry H2O2 is often the oxidant of choice because itis a liquid and processes can be readily implemented in standard batch equip-ment To be really useful catalysts should be for safety reasons effective with30 aqueous hydrogen peroxide and many systems described in the literaturedo not fulfill this requirement
17 Catalytic Oxidation 19
Fig 119 Two routes to citral
Fig 120 Key step in the production of progesterone from stigmasterol
In this context the development of the heterogeneous titanium silicalite (TS-1)catalyst by Enichem in the mid-1980s was an important milestone in oxidationcatalysis TS-1 is an extremely effective and versatile catalyst for a variety of synthe-
1 Introduction Green Chemistry and Catalysis20
Fig 121 PIPO catalysed oxidation of alcohols with NaOCl
Fig 122 Two methods for aerobic oxidation of alcohols
tically useful oxidations with 30 H2O2 eg olefin epoxidation alcohol oxidationphenol hydroxylation and ketone ammoximation (Fig 123) [74]
A serious shortcoming of TS-1 in the context of fine chemicals manufactureis the restriction to substrates that can be accommodated in the relatively small(5155 Aring2) pores of this molecular sieve eg cyclohexene is not epoxidisedThis is not the case however with ketone ammoximation which involves in situformation of hydroxylamine by titanium-catalysed oxidation of NH3 with H2O2The NH2OH then reacts with the ketone in the bulk solution which means thatthe reaction is in principle applicable to any ketone (or aldehyde) Indeed itwas applied to the synthesis of the oxime of p-hydroxyacetophenone which isconverted via Beckmann rearrangement to the analgesic paracetamol(Fig 124) [75]
TS-1 was the prototype of a new generation of solid recyclable catalysts forselective liquid phase oxidations which we called ldquoredox molecular sievesrdquo [76]A more recent example is the tin(IV)-substituted zeolite beta developed by Cor-ma and coworkers [77] which was shown to be an effective recyclable catalyst
17 Catalytic Oxidation 21
Fig 123 Catalytic oxidations with TS-1H2O2
Fig 124 Paracetamol intermediate via ammoximation
for the Baeyer-Villiger oxidation of ketones and aldehydes [78] with aqueousH2O2 (Fig 125)
At about the same time that TS-1 was developed by Enichem Venturello andcoworkers [79] developed another approach to catalysing oxidations with aque-ous hydrogen peroxide the use of tungsten-based catalysts under phase transferconditions in biphasic aqueousorganic media In the original method a tetra-alkylammonium chloride or bromide salt was used as the phase transfer agentand a chlorinated hydrocarbon as the solvent [79] More recently Noyori and co-workers [80] have optimised this methodology and obtained excellent resultsusing tungstate in combination with a quaternary ammonium hydrogen sulfateas the phase transfer catalyst This system is a very effective catalyst for the or-ganic solvent- and halide-free oxidation of alcohols olefins and sulfides with
1 Introduction Green Chemistry and Catalysis22
Fig 125 Baeyer-Villiger oxidation with H2O2 catalysed by Sn-Beta
Fig 126 Catalytic oxidations with hydrogen peroxide under phase transfer conditions
aqueous H2O2 in an environmentally and economically attractive manner(Fig 126)
Notwithstanding the significant advances in selective catalytic oxidations withO2 or H2O2 that have been achieved in recent years selective oxidation espe-cially of multifunctional organic molecules remains a difficult catalytic transfor-mation that most organic chemists prefer to avoid altogether In other wordsthe best oxidation is no oxidation and most organic chemists would prefer tostart at a higher oxidation state and perform a reduction or better still avoidchanging the oxidation state An elegant example of the latter is the use of ole-fin metathesis to affect what is formally an allylic oxidation which would benigh impossible to achieve via catalytic oxidation (Fig 127) [81]
18Catalytic CndashC Bond Formation
Another key transformation in organic synthesis is CndashC bond formation and animportant catalytic methodology for generating CndashC bonds is carbonylation Inthe bulk chemicals arena it is used for example for the production of aceticacid by rhodium-catalysed carbonylation of methanol [82] Since such reactionsare 100 atom efficient they are increasingly being applied to fine chemicalsmanufacture [83 84] An elegant example of this is the Hoechst-Celanese pro-cess for the manufacture of the analgesic ibuprofen with an annual productionof several thousands tons In this process ibuprofen is produced in two catalyticsteps (hydrogenation and carbonylation) from p-isobutylactophenone (Fig 128)with 100 atom efficiency [83] This process replaced a more classical routewhich involved more steps and a much higher E factor
In a process developed by Hoffmann-La Roche [55] for the anti-Parkinsoniandrug lazabemide palladium-catalysed amidocarbonylation of 25-dichloropyri-dine replaced an original synthesis that involved eight steps starting from 2-
18 Catalytic CndashC Bond Formation 23
Fig 127 The best oxidation is no oxidation
methyl-5-ethylpyridine and had an overall yield of 8 The amidocarbonylationroute affords lazabemide hydrochloride in 65 yield in one step with 100atom efficiency (Fig 129)
Another elegant example of palladium-catalysed amidocarbonylation thistime is the one-step 100 atom efficient synthesis of -amino acid derivativesfrom an aldehyde CO and an amide (Fig 130) [85] The reaction is used forexample in the synthesis of the surfactant N-lauroylsarcosine from formalde-hyde CO and N-methyllauramide replacing a classical route that generated co-pious amounts of salts
Another catalytic methodology that is widely used for CndashC bond formation isthe Heck and related coupling reactions [86 87] The Heck reaction [88] involvesthe palladium-catalysed arylation of olefinic double bonds (Fig 131) and pro-vides an alternative to Friedel-Crafts alkylations or acylations for attaching car-bon fragments to aromatic rings The reaction has broad scope and is currentlybeing widely applied in the pharmaceutical and fine chemical industries For ex-ample Albemarle has developed a new process for the synthesis of the anti-in-
1 Introduction Green Chemistry and Catalysis24
Fig 128 Hoechst-Celanese process for ibuprofen
Fig 129 Two routes to lazabemide
flammatory drug naproxen in which a key step is the Heck reaction shown inFig 131 [86]
The scope of the Heck and related coupling reactions was substantially broa-dened by the development in the last few years of palladiumligand combina-tions which are effective with the cheap and readily available but less reactivearyl chlorides [86 87] rather than the corresponding bromides or iodides Theprocess still generates one equivalent of chloride however Of interest in thiscontext therefore is the report of a halide-free Heck reaction which employs anaromatic carboxylic anhydride as the arylating agent and requires no base orphosphine ligands [89]
A closely related reaction that is currently finding wide application in thepharmaceutical industry is the Suzuki coupling of arylboronic acids with arylhalides [90] For example this technology was applied by Clariant scientists tothe production of o-tolyl benzonitrile an intermediate in the synthesis of angio-tensin II antagonists a novel class of antihypertensive drugs (Fig 132) [91] In-terestingly the reaction is performed in an aqueous biphasic system using awater soluble palladium catalyst which forms the subject of the next sectionthe question of reaction media in the context of green chemistry and catalysis
However no section on catalytic CndashC bond formation would be completewithout a mention of olefin metathesis [92 93] It is in many respects the epi-tome of green chemistry involving the exchange of substituents around thedouble bonds in the presence of certain transition metal catalysts (Mo W Reand Ru) as shown in Fig 133 Several outcomes are possible straight swapping
18 Catalytic CndashC Bond Formation 25
Fig 130 Palladium-catalysed amidocarbonylation
Fig 131 Heck coupling reaction
of groups between two acyclic olefins (cross metathesis CM) closure of largerings (ring closing metathesis RCM) diene formation from reaction of a cyclicolefin with an acyclic one (ring opening metathesis ROM) polymerization ofcyclic olefins (ring opening metathesis polymerization ROMP) and polymeriza-tion of acyclic dienes (acyclic diene metathesis polymerisation ADMET)
Following its discovery in the 1960s olefin metathesis was applied to bulk che-micals manufacture a prominent example being the Shell Higher Olefins Pro-cess (SHOP) [94] In the succeeding decades the development of catalysts inparticular the ruthenium-based ones that function in the presence of mostfunctional groups paved the way for widespread application of olefin metathesisin the synthesis of complex organic molecules [92 93] Indeed olefin metathe-sis has evolved into a pre-eminent methodology for the formation of CndashC bondsunder mild conditions An illustrative example is the RCM reaction shown inFig 134 [95] The ruthenium carbene complex catalyst functioned in undistilledprotic solvents (MeOHH2O) in the presence of air
1 Introduction Green Chemistry and Catalysis26
Fig 132 A Suzuki coupling
Fig 133 Olefin metathesis reactions
19The Question of Solvents Alternative Reaction Media
Another important issue in green chemistry is the use of organic solvents Theuse of chlorinated hydrocarbon solvents traditionally the solvent of choice for awide variety of organic reactions has been severely curtailed Indeed so manyof the solvents that are favored by organic chemists have been blacklisted thatthe whole question of solvent use requires rethinking and has become a pri-mary focus especially in the fine chemicals industry [96] It has been estimatedby GSK workers [97] that ca 85 of the total mass of chemicals involved inpharmaceutical manufacture comprises solvents and recovery efficiencies aretypically 50ndash80 [97] It is also worth noting that in the redesign of the sertra-line manufacturing process [98] for which Pfizer received a Presidential GreenChemistry Challenge Award in 2002 among other improvements a three-stepsequence was streamlined by employing ethanol as the sole solvent This elimi-nated the need to use distil and recover four solvents (methylene chloride tet-rahydrofuran toluene and hexane) employed in the original process Similarlyimpressive improvements were achieved in a redesign of the manufacturingprocess for sildenafil (ViagraTM) [99]
The best solvent is no solvent and if a solvent (diluent) is needed then wateris preferred [100] Water is non-toxic non-inflammable abundantly availableand inexpensive Moreover owing to its highly polar character one can expectnovel reactivities and selectivities for organometallic catalysis in water Further-more this provides an opportunity to overcome a serious shortcoming of homo-geneous catalysts namely the cumbersome recovery and recycling of the cata-lyst Thus performing the reaction in an aqueous biphasic system whereby the
19 The Question of Solvents Alternative Reaction Media 27
Fig 134 Ru-catalysed ring closing metathesis
catalyst resides in the water phase and the product is dissolved in the organicphase [101 102] allows recovery and recycling of the catalyst by simple phaseseparation
An example of a large scale application of this concept is the RuhrchemieRhocircne Poulenc process for the hydroformylation of propylene to n-butanalwhich employs a water-soluble rhodium(I) complex of trisulfonated triphenyl-phosphine (tppts) as the catalyst [103] The same complex also functions as thecatalyst in the Rhocircne Poulenc process for the manufacture of the vitamin A inter-mediate geranylacetone via reaction of myrcene with methyl acetoacetate in anaqueous biphasic system (Fig 135) [104]
Similarly Pdtppts was used by Hoechst [105] as the catalyst in the synthesis ofphenylacetic acid by biphasic carbonylation of benzyl chloride (Fig 136) as an al-ternative to the classical synthesis via reaction with sodium cyanide Although thenew process still produces one equivalent of sodium chloride this is substantiallyless salt generation than in the original process Moreover sodium cyanide isabout seven times more expensive per kg than carbon monoxide
The salt production can be circumvented by performing the selective Pdtppts-catalysed carbonylation of benzyl alcohol in an acidic aqueous biphasicsystem (Fig 136) [106] This methodology was also applied to the synthesis ofibuprofen (see earlier) by biphasic carbonylation of 1-(4-isobutylphenyl)ethanol[107] and to the biphasic hydrocarboxylation of olefins [108]
As mentioned earlier (Section 15) another example of novel catalysis in anaqueous medium is the use of lanthanide triflates as water-tolerant Lewis acidcatalysts for a variety of organic transformations in water [39]
Other non-classical reaction media [96] have in recent years attracted increas-ing attention from the viewpoint of avoiding environmentally unattractive sol-vents andor facilitating catalyst recovery and recycling Two examples whichreadily come to mind are supercritical carbon dioxide and room temperatureionic liquids Catalytic hydrogenation in supercritical CO2 for example has
1 Introduction Green Chemistry and Catalysis28
Fig 135 Manufacture of n-butanal and geranylacetone in aqueous biphasic systems
been commercialised by Thomas Swan and Co [109] Ionic liquids are similarlybeing touted as green reaction media for organic synthesis in general and cata-lytic reactions in particular [110ndash112] They exhibit many properties which makethem potentially attractive reaction media eg they have essentially no vaporpressure and cannot therefore cause emissions to the atmosphere These non-conventional reaction media will be treated in depth in Chapter 7
110Biocatalysis
Biocatalysis has many attractive features in the context of green chemistry mildreaction conditions (physiological pH and temperature) an environmentallycompatible catalyst (an enzyme) and solvent (often water) combined with highactivities and chemo- regio- and stereoselectivities in multifunctional moleculesFurthermore the use of enzymes generally circumvents the need for functionalgroup activation and avoids protection and deprotection steps required in tradi-tional organic syntheses This affords processes which are shorter generate less
110 Biocatalysis 29
Fig 136 Aqueous biphasic carbonylations
waste and are therefore both environmentally and economically more attractivethan conventional routes
The time is ripe for the widespread application of biocatalysis in industrial or-ganic synthesis and according to a recent estimate [113] more than 130 pro-cesses have been commercialised Advances in recombinant DNA techniqueshave made it in principle possible to produce virtually any enzyme for a com-mercially acceptable price Advances in protein engineering have made it possi-ble using techniques such as site directed mutagenesis and in vitro evolutionto manipulate enzymes such that they exhibit the desired substrate specificityactivity stability pH profile etc [114] Furthermore the development of effec-tive immobilisation techniques has paved the way for optimising the perfor-mance and recovery and recycling of enzymes
An illustrative example of the benefits to be gained by replacing conventionalchemistry by biocatalysis is provided by the manufacture of 6-aminopenicillanicacid (6-APA) a key raw material for semi-synthetic penicillin and cephalosporinantibiotics by hydrolysis of penicillin G [115] Up until the mid-1980s a chemi-cal procedure was used for this hydrolysis (Fig 137) It involved the use of en-vironmentally unattractive reagents a chlorinated hydrocarbon solvent (CH2Cl2)and a reaction temperature of ndash40 C Thus 06 kg Me3SiCl 12 kg PCl5 16 kgPhNMe2 02 kg NH3 841 kg of n-BuOH and 841 kg of CH2Cl2 were requiredto produce 1 kg of 6-APA [116]
In contrast enzymatic cleavage of penicillin G (Fig 137) is performed inwater at 37 C and the only reagent used is NH3 (09 kg per kg of 6-APA) to ad-just the pH The enzymatic process currently accounts for the majority of theseveral thousand tons of 6-APA produced annually on a world-wide basis
1 Introduction Green Chemistry and Catalysis30
Fig 137 Enzymatic versus chemical deacylation of penicillin G
Another advantage of biocatalysis is the high degree of chemo- regio- andstereoselectivities which are difficult or impossible to achieve by chemicalmeans A pertinent example is the production of the artificial sweetener aspar-tame The enzymatic process operated by the Holland Sweetener Company (ajoint venture of DSM and Tosoh) is completely regio- and enantiospecific(Fig 138) [117]
The above-mentioned processes employ isolated enzymes ndash penicillin G acy-lase and thermolysin ndash and the key to their success was an efficient productionof the enzyme As with chemical catalysts another key to success in biocatalyticprocesses is an effective method for immobilisation providing for efficient re-covery and re-use
In some cases it is more attractive to use whole microbial cells rather thanisolated enzymes as biocatalysts This is the case in many oxidative biotransfor-mations where cofactor regeneration is required andor the enzyme has limitedstability outside the cell By performing the reaction with growing microbialcells ie as a fermentation the cofactor is continuously regenerated from anenergy source eg glucose Lonza for example has commercialised processesfor the highly chemo- and regioselective microbial ring hydroxylation and side-chain oxidation of heteroaromatics (see Fig 139 for examples) [118] Such con-versions would clearly not be feasible by conventional chemical means
DuPont has developed a process for the manufacture of glyoxylic acid a largevolume fine chemical by aerobic oxidation of glycolic acid mediated by resting
110 Biocatalysis 31
Fig 138 Aspartame via enzymatic coupling
whole cells of a recombinant methylotrophic yeast (Fig 140) [119] The glycolicacid is readily available from acid-catalysed carbonylation of formaldehyde Tra-ditionally glyoxylic acid was produced by nitric acid oxidation of acetaldehyde orglyoxal processes with high E factors and more recently by ozonolysis ofmaleic anhydride
The key enzyme in the above process is an oxidase which utilises dioxygen asthe oxidant producing one equivalent of hydrogen peroxide without the needfor cofactor regeneration Another class of enzymes which catalyse the oxidationof alcohols comprises the alcohol dehydrogenases However in this case cofac-tor regeneration is required which is an impediment to commercialisation Re-
1 Introduction Green Chemistry and Catalysis32
Fig 139 Microbial oxidations of heteroaromatics
Fig 140 Glyoxylic acid by microbial oxidation
cently a highly enantioselective alcohol dehydrogenase showing broad substratespecificity and exceptionally high tolerance for organic solvents was isolatedfrom Rhodococcus ruber DSM 4451 [120] The enzyme maintains a high activityat concentrations of up to 20 (vv) acetone and 50 (vv) 2-propanol This en-ables the use of the enzyme conveniently as whole microbial cells as a catalystfor (enantioselective) Oppenauer oxidation of a broad range of alcohols usingacetone (20 vv in phosphate buffer at pH 8) as the oxidant (Fig 141) withsubstrate concentrations up to 18 mol lndash1 (237 g lndash1 for octan-2-ol)
Alternatively the reaction could be performed in a reduction mode using theketone as substrate and up to 50 vv isopropanol as the reductant affordingthe corresponding (S)-alcohol in 99 ee at conversions ranging from 65 to 92
Another example in which a biocatalytic transformation has replaced a chemo-catalytic one in a very simple reaction is the Mitsubishi Rayon process for the pro-duction of acrylamide by hydration of acrylonitrile (Fig 142) Whole cells of Rho-dococcus rhodocrous containing a nitrile hydratase produced acrylamide in gt 999purity at gt 999 conversion and in high volumetric and space time yields [121]The process (Fig 142) currently accounts for more than 100000 tons annual pro-duction of acrylamide and replaced an existing process which employed a coppercatalyst A major advantage of the biocatalytic process is the high product puritywhich is important for the main application of acrylamide as a specialty monomer
Similarly DuPont employs a nitrile hydratase (as whole cells of P chlororaphisB23) to convert adiponitrile to 5-cyanovaleramide a herbicide intermediate[122] In the Lonza nitrotinamide (vitamin B6) process [123] the final step(Fig 142) involves the nitrile hydratase (whole cells of Rh rhodocrous) catalysedhydration of 3-cyanopyridine Here again the very high product purity is a majoradvantage as conventional chemical hydrolysis affords a product contaminatedwith nicotinic acid which requires expensive purification to meet the specifica-tions of this vitamin
110 Biocatalysis 33
Fig 141 Biocatalytic Oppenauer oxidations and MPV reductions
111Renewable Raw Materials and White Biotechnology
Another important goal of green chemistry is the utilisation of renewable rawmaterials ie derived from biomass rather than crude oil Here again the pro-cesses used for the conversion of renewable feedstocks ndash mainly carbohydratesbut also triglycerides and terpenes ndash should produce minimal waste ie theyshould preferably be catalytic
In the processes described in the preceding section a biocatalyst ndash whole mi-crobial cells or an isolated enzyme ndash is used to catalyse a transformation (usual-ly one step) of a particular substrate When growing microbial cells are usedthis is referred to as a precursor fermentation Alternatively one can employ denovo fermentation to produce chemicals directly from biomass This has becomeknown as white biotechnology as opposed to red biotechnology (biopharmaceu-ticals) and green biotechnology (genetically modified crops) White biotechnol-ogy is currently the focus of considerable attention and is perceived as the keyto developing a sustainable chemical industry [124]
Metabolic pathway engineering [125] is used to optimise the production ofthe required product based on the amount of substrate (usually biomass-de-rived) consumed A so-called biobased economy is envisaged in which commod-ity chemicals (including biofuels) specialty chemicals such as vitamins flavorsand fragrances and industrial monomers will be produced in biorefineries (seeChapter 8 for a more detailed discussion)
De novo fermentation has long been the method of choice for the manufac-ture of many natural L-amino acids such as glutamic acid and lysine and hy-droxy acids such as lactic and citric acids More recently de novo fermentation isdisplacing existing multistep chemical syntheses for example in the manufac-ture of vitamin B2 (riboflavin) and vitamin C Other recent successes of white
1 Introduction Green Chemistry and Catalysis34
Fig 142 Industrial processes employing a nitrile hydratase
biotechnology include the biodegradable plastic polylactate produced by Car-gill-Dow and 13-propanediol a raw material for the new polyester fibre Sorona(poly-trimethylene terephthalate) developed by DuPontGenencor The latter pro-cess has become a benchmark in metabolic pathway engineering [125] Both ofthese processes employ corn-derived glucose as the feedstock
Finally an elegant example of a product derived from renewable raw materials isthe bioemulsifier marketed by Mitsubishi which consists of a mixture of sucrosefatty acid esters The product is prepared from two renewable raw materials ndash su-crose and a fatty acid ndash and is biodegradable In the current process the reaction iscatalysed by a mineral acid which leads to a rather complex mixture of mono- anddi-esters Hence a more selective enzymatic esterification (Fig 143) would haveobvious benefits Lipase-catalysed acylation is possible [126] but reaction ratesare very low This is mainly owing to the fact that the reaction for thermodynamicreasons cannot be performed in water On the other hand sucrose is sparinglysoluble in most organic solvents thus necessitating a slurry process
112Enantioselective Catalysis
Another major trend in performance chemicals is towards the development ofproducts ndash pharmaceuticals pesticides and food additives etc ndash that are moretargeted in their action with less undesirable side-effects This is also an issuewhich is addressed by green chemistry In the case of chiral molecules that ex-hibit biological activity the desired effect almost always resides in only one ofthe enantiomers The other enantiomer constitutes isomeric ballast that doesnot contribute to the desired activity and may even exhibit undesirable side-ef-fects Consequently in the last two decades there has been a marked trend to-wards the marketing of chiral pharmaceuticals and pesticides as enantiomeri-cally pure compounds This generated a demand for economical methods forthe synthesis of pure enantiomers [127]
The same reasoning applies to the synthesis of pure enantiomers as to organicsynthesis in general for economic and environmental viability processes should
112 Enantioselective Catalysis 35
Fig 143 Synthesis of a bioemulsifier from renewable raw materials
be atom efficient and have low E factors that is they should employ catalyticmethodologies This is reflected in the increasing focus of attention on enantiose-lective catalysis using either enzymes or chiral metal complexes Its importancewas acknowledged by the award of the 2001 Nobel Prize in Chemistry to KnowlesNoyori and Sharpless for their contributions to asymmetric catalysis
An elegant example of a highly efficient catalytic asymmetric synthesis is theTakasago process [128] for the manufacture of 1-menthol an important flavourand fragrance product The key step is an enantioselective catalytic isomerisa-tion of a prochiral enamine to a chiral imine (Fig 144) The catalyst is a Rh-Bi-nap complex (see Fig 144) and the product is obtained in 99 ee using a sub-stratecatalyst ratio of 8000 recycling of the catalyst affords total turnover num-bers of up to 300000 The Takasago process is used to produce several thousandtons of 1-menthol on an annual basis
An even more impressive example of catalytic efficiency is the manufactureof the optically active herbicide (S)-metolachlor The process developed by No-vartis [129] involves asymmetric hydrogenation of a prochiral imine catalysed
1 Introduction Green Chemistry and Catalysis36
Fig 144 Takasago l-menthol process
by an iridium complex of a chiral ferrocenyldiphosphine (Fig 145) Completeconversion is achieved within 4 h at a substratecatalyst ratio of gt 1 000000 andan initial TOF exceeding 1 800000 hndash1 giving a product with an ee of 80 Ahigher ee can be obtained at lower substratecatalyst ratios but is not actuallynecessary for this product The process is used to produce several thousand tonsof this optically active herbicide
The widespread application of enantioselective catalysis be it with chiral me-tal complexes or enzymes raises another issue These catalysts are often veryexpensive Chiral metal complexes generally comprise expensive noble metalsin combination with even more expensive chiral ligands A key issue is there-fore to minimise the cost contribution of the catalyst to the total cost price ofthe product a rule of thumb is that it should not be more than ca 5 Thiscan be achieved either by developing an extremely productive catalyst as in themetachlor example or by efficient recovery and recycling of the catalyst Hencemuch attention has been devoted in recent years to the development of effectivemethods for the immobilisation of metal complexes [130 131] and enzymes[132] This is discussed in more detail in Chapter 9
112 Enantioselective Catalysis 37
Fig 145 Novartis process for (S)-metalachlor
113Risky Reagents
In addition to the increasingly stringent environmental regulations with regardto the disposal of aqueous effluent and solid waste tightened safety regulationsare making the transport storage and hence use of many hazardous and toxicchemicals prohibitive The ever increasing list includes phosgene dimethyl sul-fate formaldehydehydrogen chloride (for chloromethylations) sodium azidehydrogen fluoride and even chlorine and bromine
Although it will not be possible to dispense with some of these reagents entirelytheir industrial use is likely to be confined to a small group of experts who areproperly equipped to handle and contain these materials In some cases catalyticalternatives may provide an answer such as the use of catalytic carbonylation in-stead of phosgene and solid acids as substitutes for hydrogen fluoride
Chlorine-based chemistry is a case in point In addition to the problem of saltgeneration the transport of chlorine is being severely restricted Moreoverchlorine-based routes often generate aqueous effluent containing trace levels ofchlorinated organics that present a disposal problem
Obviously when the desired product contains a chlorine atom the use ofchlorine can be avoided only by replacing the product However in many caseschlorine is a reagent that does not appear in the product and its use can be cir-cumvented How remarkably simple the solution can be once the problem hasbeen identified is illustrated by the manufacture of a family of sulfenamidesthat are used as rubber additives
Traditionally these products were produced using a three-step chlorine-basedoxidative coupling process (Fig 146) In contrast Monsanto scientists [133] de-veloped a process involving one step under mild conditions (lt 1 h at 70 C) Ituses molecular oxygen as the oxidant and activated charcoal as the catalyst(Fig 146) The alkylaminomercaptobenzothiazole product is formed in essen-tially quantitative yield and water is the coproduct We note that activated char-coal contains various trace metals which may be the actual catalyst
Another elegant example also developed by Monsanto scientists [134] is thesynthesis of p-phenylene diamine a key raw material for aramid fibres The tradi-tional process involves nitration of chlorobenzene followed by reaction of the re-sulting p-nitrochlorobenzene with ammonia to give p-nitroaniline which is hydro-genated to p-phenylenediamine Monsanto scientists found that benzamide reactswith nitrobenzene in the presence of a base and dioxygen to afford 4-nitrobenza-nilide Reaction of the latter with methanolic ammonia generates p-nitroanilineand benzamide which can be recycled to the first step (Fig 147) resulting inan overall reaction of nitrobenzene with ammonia and dioxygen to give p-nitroani-line and a molecule of water The key step in the process is the oxidation of theintermediate Meisenheimer complex by the nitrobenzene substrate resulting inan overall oxidative nucleophilic substitution The nitrosobenzene coproduct is re-oxidised by dioxygen Hence a remarkable feature of the process is that no exter-nal catalyst is required the substrate itself acts as the catalyst
1 Introduction Green Chemistry and Catalysis38
114Process Integration and Catalytic Cascades
The widespread application of chemo- and biocatalytic methodologies in themanufacture of fine chemicals is resulting in a gradual disappearance of the tra-ditional barriers between the subdisciplines of homogeneous and heterogeneouscatalysis and biocatalysis An effective integration of these catalytic technologiesin organic synthesis is truly the key to success
114 Process Integration and Catalytic Cascades 39
Fig 146 Two routes to alkylaminomercaptobenzothiazoles
Fig 147 Monsanto process for p-phenylenediamine
An elegant example is the Rhodia process for the manufacture of the flavoringredient vanillin [30] The process involves four steps all performed with aheterogeneous catalyst starting from phenol (Fig 148) Overall one equivalentof phenol H2O2 CH3OH H2CO and O2 are converted to one equivalent of va-nillin and three equivalents of water
Another pertinent example is provided by the manufacture of caprolactam[135] Current processes are based on toluene or benzene as feedstock whichcan be converted to cyclohexanone via cyclohexane or phenol More recentlyAsahi Chemical [136] developed a new process via ruthenium-catalysed selectivehydrogenation to cyclohexene followed by zeolite-catalysed hydration to cyclo-hexanol and dehydrogenation (Fig 149) The cyclohexanone is then convertedto caprolactam via ammoximation with NH3H2O2 and zeolite-catalysed Beck-mann rearrangement as developed by Sumitomo (see earlier)
Alternatively caprolactam can be produced from butadiene via homogeneousnickel-catalysed addition of HCN (DuPont process) followed by selective catalytichydrogenation of the adiponitrile product to the amino nitrile and vapor phasehydration over an alumina catalyst (Rhodia process) as shown in Fig 149 [137]
Interestingly the by-product in the above-described hydrocyanation of buta-diene 2-methylglutaronitrile forms the raw material for the Lonza process fornicotinamide (see earlier) [123] Four heterogeneous catalytic steps (hydrogena-tion cyclisation dehydrogenation and ammoxidation) are followed by an enzy-matic hydration of a nitrile to an amide (Fig 150)
The ultimate in integration is to combine several catalytic steps into a one-pot multi-step catalytic cascade process [138] This is truly emulating Naturewhere metabolic pathways conducted in living cells involve an elegant orchestra-tion of a series of biocatalytic steps into an exquisite multicatalyst cascade with-out the need for separation of intermediates
An example of a one-pot three-step catalytic cascade is shown in Fig 151[139] In the first step galactose oxidase catalyses the selective oxidation of theprimary alcohol group of galactose to the corresponding aldehyde This is fol-
1 Introduction Green Chemistry and Catalysis40
Fig 148 Rhodia vanillin process
lowed by L-proline catalysed elimination of water and catalytic hydrogenationaffording the corresponding deoxy sugar
In some cases the answer may not be to emulate Naturersquos catalytic cascadesbut rather to streamline them through metabolic pathway engineering (see ear-lier) The elegant processes for vanillin caprolactam and nicotinamide describedabove may in the longer term be superseded by alternative routes based on denovo fermentation of biomass For many naturally occurring compounds thiswill represent a closing of the circle that began more than a century ago withthe synthesis of natural products such as dyestuffs from raw materials derivedfrom coal tar It is perhaps appropriate therefore to close this chapter with amention of the dyestuff indigo Its first commercial synthesis in the nineteenthcentury [140] involved classical organic chemistry and has hardly changed since
114 Process Integration and Catalytic Cascades 41
Fig 149 Alternative routes to caprolactam
that time Mitsui Toatsu reported [141] an alternative conversion of aniline to in-digo in two catalytic steps However in the future indigo may be produced byan even greener route Genencor [142] has developed a one-step fermenatationof glucose to indigo using a recombinant E coli strain in which the tryptophanpathway has been engineered to produce high levels of indole and genes en-coding for naphthalene dioxygenase have been incorporated The latter enzymecatalyses the aerobic oxidation of indole to indigo The process (see Chapter fora more detailed discussion) is not yet commercially viable probably because of
1 Introduction Green Chemistry and Catalysis42
Fig 150 Lonza nicotinamide process
Fig 151 One-pot three-step synthesis of a deoxy sugar
relatively low volumetric (18 g lndash1) and spacendashtime yields (lt1 g lndash1 hndash1) but maybe further optimised in the future
References 43
References
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4 PT Anastas LG Heine T C William-son (Eds) Green Chemical Syntheses andProcesses American Chemical SocietyWashington DC 2000
5 PT Anastas CA Farris (Eds) Benignby Design Alternative Synthetic Design forPollution Prevention ACS Symp Ser nr577 American Chemical Society Wash-ington DC 1994
6 J H Clark D J Macquarrie Handbookof Green Chemistry and Technology Black-well Abingdon 2002
7 A S Matlack Introduction to GreenChemistry Marcel Dekker New York2001
8 M Lancaster Green Chemistry An Intro-ductory Text Royal Society of ChemistryCambridge 2002
9 J H Clark (Ed) The Chemistry of WasteMinimization Blackie London 1995
10 R A Sheldon CR Acad Sci Paris IIcChimieChemistry 2000 3 541ndash551
11 CG Brundtland Our Common FutureThe World Commission on Environmen-tal Development Oxford UniversityPress Oxford 1987
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13 R A Sheldon in Industrial Environmen-tal Chemistry DT Sawyer AE Martell(Eds) Plenum New York 1992 pp 99ndash119
14 R A Sheldon in Precision Process Tech-nology MP C Weijnen A AH Drin-kenburg (Eds) Kluwer Dordrecht 1993pp 125ndash138
15 R A Sheldon Chemtech March 199438ndash47
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17 R A Sheldon J Mol Catal A Chemical1996 107 75ndash83
18 R A Sheldon Pure Appl Chem 200072 1233ndash1246
19 T Hudlicky DA Frey L KoroniakCD Claeboe LE Brammer GreenChem 1999 1 57ndash59
20 DJ C Constable AD Curzons V LCunningham Green Chem 2002 4 521ndash527 see also A D Curzons D J C Con-stable DN Mortimer V L CunninghamGreen Chem 2001 3 1ndash6 D JC Con-stable AD Curzons LM Freitas dosSantos G R Green R E Hannah J DHayler J Kitteringham MA McGuireJ E Richardson P Smith R L Webb MYu Green Chem 2001 3 7ndash10
21 BM Trost Science 1991 254 1471ndash1477
22 BM Trost Angew Chem Int Ed 199534 259ndash281
23 T Iwata H Miki Y Fujita in UllmannrsquosEncyclopedia of Industrial Chemistry VolA19 VCH Weinheim 1991 p 347
24 PM Hudnall in Ullmannrsquos Encyclopediaof Industrial Chemistry Vol A13 VCHWeinheim 1991 p 499
25 R Larsson (Ed) Perspectives in CatalysisIn Commemoration of J J Berzelius CNKGleerup Lund Sweden 1981
26 W H Perkin J Chem Soc 1862 232Br Pat 1856 1984
27 K Tanabe W Houmllderich Appl Catal AGeneral 1999 181 399ndash434
28 R A Sheldon R S Downing Appl Cat-al A General 1999 189 163ndash183 RSDowning H van Bekkum R A Shel-don Cattech 1997 2 95ndash109
29 R A Sheldon H van Bekkum (Eds)Fine Chemicals Through HeterogeneousCatalysis Wiley-VCH Weinheim 2001Ch 3ndash7
1 Introduction Green Chemistry and Catalysis44
30 S Ratton Chem Today 1997 3ndash4 33ndash3731 M Spagnol L Gilbert D Alby in The
Roots of Organic Development J R Des-murs S Ratton (Eds) Ind Chem LibVol 8 Elsevier Amsterdam 1996pp 29ndash38
32 H Ichihashi M Kitamura Catal Today2002 73 23ndash28
33 H Ichihashi H Sato Appl Catal AGeneral 2001 221 359ndash366
34 P Roffia G Leofanti A CesanaM Mantegazza M Padovan G PetriniS Tonti P Gervasutti Stud Surf SciCatal 1990 55 43ndash50 G Bellussi CPerego Cattech 2000 4 4ndash16
35 W F Houmllderich J Roumlseler G Heit-mann A T Liebens Catal Today 199737 353ndash366
36 P J Kunkeler J C van der WaalJ Bremmer B J Zuurdeeg R S Down-ing H van Bekkum Catal Lett 199853 135ndash138
37 J A Elings HEB Lempers R A Shel-don Stud Surf Sci Catal 1997 1051165ndash1172
38 M Wegman J M Elzinga E NeelemanF van Rantwijk RA Sheldon GreenChem 2001 3 61ndash64
39 S Kobayashi S Masaharu H KitagawaL Hidetoshi W L Williams Chem Rev2002 102 2227ndash2312 W Xe Y JinPG Wang Chemtech February 199923ndash29
40 R A Sheldon H van Bekkum (Eds)Fine Chemicals Through HeterogeneousCatalysis Wiley-VCH Weinheim 2001Ch 7
41 BF Sels DE De Vos PA Jacobs CatRev Sci Eng 2001 43 443ndash488
42 A Vaccari Catal Today 1998 41 53ndash71A Vaccari Appl Clay Sci 1999 14 161ndash198
43 F Figueras D Tichit M Bennani Na-ciri R Ruiz in Catalysis of Organic Reac-tions FE Herkes (Ed) Marcel DekkerNew York 1998 pp 37ndash49
44 A Corma RM Martiacuten-Aranda ApplCatal A General 1993 105 271ndash279
45 MJ Climent A Corma S IborraJ Primo J Catal 1995 151 60ndash66
46 D Brunel A C Blanc A GalarneauF Fajula Catal Today 2002 73 139ndash152
47 A C Blanc SValle G Renard D Bru-nel D Macquarrie CR Quinn GreenChem 2000 2 283ndash288
48 DJ Macquarrie D Brunel in Fine Che-micals Through Heterogeneous CatalysisR A Sheldon H van Bekkum (Eds)Wiley-VCH Weinheim 2001 pp 338ndash349
49 D Brunel Micropor Mesopor Mater1999 27 329ndash344
50 YV Subba Rao DE De Vos PA Ja-cobs Angew Chem Int Ed 1997 362661ndash2663
51 PN Rylander Catalytic Hydrogenationover Platinum Metals Academic PressNew York 1967
52 R L Augustine Heterogeneous Catalysisfor the Synthetic Chemist Marcel DekkerNew York 1996 pp 315ndash343
53 P Sabatier A Mailhe Compt Rend1904 138 245 P Sabatier Catalysis inOrganic Chemistry (translated by EEReid) Van Nostrand Princeton 1923
54 R Noyori (Issue Ed) Adv Synth Catal2003 345 1ndash324
55 F Roessler Chimia 1996 50 106ndash10956 W S Knowles R Noyori K B Sharp-
less Nobel Lectures Angew Chem IntEd 2002 41 1998ndash2022 see also W SKnowles Adv Synth Catal 2003 3453ndash13 R Noyori Adv Synth Catal 2003345 15ndash32
57 HU Blaser C Malan B PuginF Spindler H Steiner M Studer AdvSynth Catal 2003 345 103ndash151
58 R R Bader P Baumeister HU BlaserChimia 1996 50 99ndash105
59 A W Williamson J Chem Soc 1852 4106
60 F Fache V Bethmont L Jacquot M Le-maire Recl Trav Chim Pays-Bas 1996115 231ndash238
61 CF de Graauw JA Peters H van Bek-kum J Huskens Synthesis 1994 101007ndash1017
62 E J Creyghton SD Ganeshie RSDowning H van Bekkum J Mol CatalA Chemical 1997 115 457ndash472
63 P J Kunkeler B J Zuurdeeg J C vander Waal J van Bokhoven DC Ko-ningsberger H van Bekkum J Catal1998 180 234ndash244
References 45
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65 E Mossettig R Mozingo Org React1948 4 362
66 T Yokoyama T Setoyama N FujitaM Nakajima T Maki Appl Catal AGeneral 1992 88 149ndash161
67 R A Sheldon J K Kochi Metal-Cata-lyzed Oxidations of Organic CompoundsAcademic Press New York 1981
68 A Chauvel A Delmon WF HoumllderichAppl Catal A General 1994 115 173ndash217
69 A E J de Nooy AC Besemer H vanBekkum Synthesis 1996 1153ndash1174
70 BD Hewitt in Ref 2 pp 347ndash36071 A Dijksman IW CE Arends R A
Sheldon Chem Commun 2000 271ndash272
72 A Dijksman IW CE Arends R ASheldon Chem Commun 1999 1591ndash1592
73 G J ten Brink IW CE Arends RASheldon Science 2000 287 1636ndash1639
74 B Notari Stud Surf Sci Catal 1998 37413ndash425
75 J le Bars J Dakka R A Sheldon ApplCatal A General 1996 136 69ndash80
76 IWCE Arends R A Sheldon M Wa-kau U Schuchardt Angew Chem IntEd Engl 1997 36 1144ndash1163
77 A Corma LT Nemeth M Renz S Va-lencia Nature 2001 412 423ndash425
78 A Corma V Fornes S Iborra M Mif-sud M Renz J Catal 2004 221 67ndash76
79 C Venturello E Alneri M Ricci J OrgChem 1983 48 3831ndash3833
80 R Noyori M Aoki K Sato Chem Com-mun 2003 1977ndash1986 and references ci-ted therein
81 A K Chatterjee R H Grubbs AngewChem Int Ed 2002 41 3172ndash3174
82 PM Maitlis A Haynes G J SunleyMJ Howard J Chem Soc Dalton Trans1996 2187ndash2196 D J Watson in Cataly-sis of Organic Reactions FE Herkes(Ed) Marcel Dekker New York 1998pp 369ndash380
83 V Elango MA Murhpy BL SmithK G Davenport G N Mott G L MossUS Pat 4981995 (1991) to Hoechst-Cela-nese Corp
84 M Beller AF Indolese Chimia 200155 684ndash687
85 M Beller M Eckert W A MoradiH Neumann Angew Chem Int Ed 199938 1454ndash1457 D Goumlrdes H NeumannA Jacobi van Wangelin C Fischer KDrauz HP Krimmer M Beller AdvSynth Catal 2003 345 510ndash516
86 A Zapf M Beller Top Catal 2002 19101ndash108
87 CE Tucker JG de Vries Top Catal2002 19 111ndash118
88 R F Heck Palladium Reagents in OrganicSynthesis Academic Press New York1985 and references cited therein
89 MS Stephan A J JM TeunissenG KM Verzijl J G de Vries AngewChem Int Ed 1998 37 662ndash664
90 G C Fu A F Littke Angew Chem IntEd 1998 37 3387ndash3388 and referencescited therein
91 W Bernhagen Chim Oggi (Chemistry To-day) MarchApril 1998 18
92 A Fuumlrstner R H Grubbs RR Schrock(Eds) Olefin Metathesis Issue of AdvSynth Catal 2002 344 (6+7) 567ndash793R H Grubbs (Ed) Handbook of Metathe-sis Wiley-VCH Weinheim 2003
93 TM Trnka R H Grubbs Acc ChemRes 2001 34 18ndash29 A Fuumlrstner AngewChem Int Ed 2000 39 3012ndash3043 SBlechert Pure Appl Chem 1999 711393ndash1399
94 B Reuben H Wittcoff J Chem Educ1988 65 605ndash607
95 S J Connon M Rivard M Zaja S Ble-chert Adv Synth Catal 2003 345 572ndash575
96 W Leitner KR Seddon P Wasser-scheid (Eds) Special Issue on Green Sol-vents for Catalysis Green Chem 2003 599ndash284
97 C Jiminez-Gonzalez A D CurzonsD J C Constable VL Cunningham IntJ Life Cycle Assess 2004 9 115ndash121
98 G P Taber DM Pfistere J C ColbergOrg Proc Res Dev 2004 8 385ndash388A M Rouhi CampEN April 2002 31ndash32
99 P J Dunn S Galvin K HettenbachGreen Chem 2004 6 43ndash48
1 Introduction Green Chemistry and Catalysis46
100 S Kobayashi (Ed) Special Issue onWater Adv Synth Catal 2002 344219ndash451
101 G Papadogianakis R A Sheldon inCatalysis Vol 13 Specialist PeriodicalReport Royal Society of ChemistryCambridge 1997 pp 114ndash193
102 B Cornils W A Herrmann (Eds)Aqueous Phase Organometallic CatalysisConcepts and Applications Wiley-VCHWeinheim 1998
103 B Cornils E Wiebus Recl Trav ChimPays-Bas 1996 115 211
104 C Mercier P Chabardes Pure ApplChem 1994 66 1509
105 CW Kohlpaintner M Beller J MolCatal A Chemical 1997 116 259ndash267
106 G Papadogianakis L Maat RA Shel-don J Mol Catal A Chemical 1997116 179ndash190
107 G Papadogianakis L Maat RA Shel-don J Chem Technol Biotechnol 199770 83ndash91
108 G Papadogianakis G Verspui LMaat R A Sheldon Catal Lett 199747 43ndash46
109 P Licence J Ke M Sokolova S KRoss M Poliakoff Green Chem 20035 99ndash104
110 R A Sheldon Chem Commun 20012399ndash2407
111 R D Rogers K R Seddon (Eds) IonicLiquids as Green Solvents Progress andProspects ACS Symp Ser 2003 856
112 P Wasserscheid T Welton (Eds) IonicLiquids in Synthesis Wiley-VCH Wein-heim 2003
113 A J J Straathof S Panke A SchmidCurr Opin Biotechnol 2002 13 548ndash556
114 K A Powell SW Ramer SB del Car-dayreacute W PC Stemmer MB TobinPF Longchamp G W Huisman An-gew Chem Int Ed 2001 40 3948ndash3959
115 MA Wegman MHA JanssenF van Rantwijk RA Sheldon AdvSynth Catal 2001 343 559ndash576A Bruggink EC Roos E de VroomOrg Proc Res Dev 1998 2 128ndash133
116 Ullmannrsquos Encyclopedia of IndustrialChemistry 5th edn Vol B8 VCHWeinheim 1995 pp 302ndash304
117 K Oyama in Chirality in IndustryA N Collins G N Sheldrake J Cros-by (Eds) Wiley New York 1992pp 237
118 M Petersen A Kiener Green Chem1999 1 99ndash106
119 J E Gavagan SK Fager J E SeipMS Payne D L Anton R DiCosimoJ Org Chem 1995 60 3957ndash3963
120 W Stampfer B Kosjek C MoitziW Kroutil K Faber Angew Chem IntEd 2002 41 1014ndash1017
121 M Kobayashi T Nagasawa H Yama-da Trends Biotechnol 1992 1 402ndash408M Kobayashi S Shimizu Curr OpinChem Biol 2000 4 95ndash102
122 EC Hann A Eisenberg S K FagerNE Perkins FG Gallagher SMCooper J E Gavagan B StieglitzSM Hennessey R DiCosimo BioorgMed Chem 1999 7 2239ndash2245
123 J Heveling Chimia 1996 50 114124 BE Dale J Chem Technol Biotechnol
2003 78 1093ndash1103125 CE Nakamura GM Whited Curr
Opin Biotechnol 2003 14 454ndash459126 M Woudenberg-van Oosterom F van
Rantwijk R A Sheldon BiotechnolBioeng 1996 49 328ndash333
127 R A Sheldon Chirotechnology The In-dustrial Synthesis of Optically ActiveCompounds Marcel Dekker New York1993
128 H Komobayashi Recl Trav ChimPays-Bas 1996 115 201ndash210
129 HU Blaser Adv Synth Catal 2002344 17ndash31 see also HU BlaserW Brieden B Pugin F SpindlerM Studer A Togni Top Catal 200219 3ndash16
130 DE De Vos IF J Vankelecom PAJacobs Chiral Catalyst Immobilizationand Recycling Wiley-VCH Weinheim2000
131 U Kragl T Dwars Trend Biotechnol2001 19 442ndash449
132 L Cao LM van Langen R A Shel-don Curr Opin Biotechnol 2003 14387ndash394
133 D Riley MK Stern J Ebner in TheActivation of Dioxygen and HomogeneousCatalytic Oxidation DHR Barton
References 47
A E Martell DT Sawyer (Eds) Ple-num Press New York 1993 p 31ndash44
134 MK Stern FD Hileman J K Bash-kin J Am Chem Soc 1992 1149237ndash9238
135 G Dahlhoff J PM Niederer WFHoelderich Catal Rev 2001 43 381ndash441
136 H Ishida Catal Surveys Jpn 19971 241ndash246
137 L Gilbert N Laurain P Leconte CNedez Eur Pat Appl EP 07487971996 to Rhodia
138 A Bruggink R Schoevaart T Kie-boom Org Proc Res Dev 2003 7622ndash640
139 R Schoevaart T Kieboom TetrahedronLett 2002 43 3399ndash3400
140 A Bayer Chem Ber 1878 11 1296K Heumann Chem Ber 1890 233431
141 Y Inoue Y Yamamoto H SuzukiU Takaki Stud Surf Sci Catal 199482 615
142 A Berry T C Dodge M PepsinW Weyler J Ind Microbiol Biotechnol2002 28 127ndash133
21Introduction
Processes catalyzed by acids and bases play a key role in the oil refining andpetrochemical industries and in the manufacture of a wide variety of specialtychemicals such as pharmaceuticals agrochemicals and flavors and fragrancesExamples include catalytic cracking and hydrocracking alkylation isomeriza-tion oligomerization hydrationdehydration esterification and hydrolysis and avariety of condensation reactions to name but a few [1 2] Many of these pro-cesses involve the use of traditional Broslashnsted acids (H2SO4 HF HCl p-toluene-sulfonic acid) or Lewis acids (AlCl3 ZnCl2 BF3) in liquid-phase homogeneoussystems or on inorganic supports in vapor phase systems Similarly typicalbases include NaOH KOH NaOMe and KOBut Their subsequent neutraliza-tion leads to the generation of inorganic salts which ultimately end up in aque-ous waste streams Even though only catalytic amounts are generally but not al-ways used in the oil refining and petrochemical industries the absolute quanti-ties of waste generated are considerable owing to the enormous production vol-umes involved In contrast in the fine and specialty chemical industries theproduction volumes are much smaller but acids and bases are often used instoichiometric quantities eg in Friedel-Crafts acylations and aldol and relatedcondensations respectively [3]
An obvious solution to this salt generation problem is the widespread replace-ment of traditional Broslashnsted and Lewis acids with recyclable solid acids andbases [3ndash7] This will obviate the need for hydrolytic work-up and eliminate thecosts and environmental burden associated with the neutralization and disposalof eg liquid acids such as H2SO4 The use of solid acids and bases as catalystsprovides additional benefits Separation and recycling is facilitated resulting in a simpler process which
translates to lower production costs Solid acids are safer and easier to handle than their liquid counterparts eg
H2SO4 HF that are highly corrosive and require expensive construction ma-terials
Contamination of the product by trace amounts of (neutralized) catalyst isgenerally avoided when the latter is a solid
49
2Solid Acids and Bases as Catalysts
22Solid Acid Catalysis
Acid-catalyzed processes constitute one of the most important areas for the ap-plication of heterogeneous catalysis A wide variety of solid catalysts are usedThey include mixed oxides such as silicandashalumina and sulfated zirconia acidicclays [8ndash10] zeolites [11ndash14] supported heteropoly acids [15] organic ion ex-change resins [16 17] and hybrid organicndashinorganic materials such as mesopor-ous oxides containing pendant organic sulfonic acid moieties [18 19] For thepurpose of our further discussion of this topic we can conveniently divide solidacid catalysts into three major categories amorphous mixed oxides typified bythe acidic clays the crystalline zeolites and related materials (zeotypes) and sol-id acids containing surface sulfonic acid groups The latter category embracesorganic and inorganic cationic exchange resins and the above-mentioned hybridorganicndashinorganic materials Zeolites definitely occupy center stage and will bethe major focus of our discussion but the use of (acidic) clays as catalysts is ofearlier vintage so we shall begin with this interesting class of materials
221Acidic Clays
Clays are naturally occurring minerals that are produced in enormous quanti-ties and find a wide variety of applications including their use as catalysts [8ndash10 20 21] They were widely used as solid acid catalysts in oil refining fromthe 1930s until the mid 1960s when they were replaced by the zeolites whichexhibited better activity and selectivity
Clays are amorphous layered (alumino)silicates in which the basic buildingblocks ndash SiO4 tetrahedra and MO6 octahedra (M= Al3+ Mg2+ Fe3+ Fe2+ etc) ndashpolymerize to form two-dimensional sheets [8ndash10 20] One of the most com-monly used clays is montmorillonite in which each layer is composed of an oc-tahedral sheet sandwiched between two tetrahedral silicate sheets (see Fig 21)Typically the octahedral sheet comprises oxygens attached to Al3+ and somelower valence cations such as Mg2+ The overall layer has a net negative chargewhich is compensated by hydrated cations occupying the interlamellar spacesImmersion in water results in a swelling of the clay and exposure of the interca-lated cations making them accessible for cation exchange The interlamellar ca-tions are largely responsible for the clayrsquos Broslashnsted andor Lewis acidity Themore electronegative the cation the stronger the acidity and both the amountand strength of Broslashnsted and Lewis acid sites can be enhanced by cation ex-change or treatment with a mineral acid eg H2SO4
An Al3+-exchanged montmorillonite for example is as active as concentratedsulfuric acid in promoting acid-catalyzed reactions Sulfuric acid treatment ofnatural montmorillonite similarly affords the much more active and widely usedacid catalyst known as K-10 or KSF (from Sud-Chemie or Fluka respectively)
2 Solid Acids and Bases as Catalysts50
For example K-10 has been successfully used as a Friedel-Crafts alkylation cata-lyst (see Fig 22) [22]
Clays or acid-treated clays are also effective supports for Lewis acids such asZnCl2 or FeCl3 [23] Montmorillonite-supported zinc chloride known as Clayzichas been extensively studied as a catalyst for eg Friedel-Crafts alkylations [2425] (see Fig 22)
A serious shortcoming of clays however is their limited thermal stability Heat-ing of exchanged clays results in a loss of water accompanied by collapse of theinterlamellar region thereby dramatically decreasing the effective surface areaThis problem was addressed by developing so-called pillared clays (PILCs) [26ndash28] in which the layered structure is intercalated with pillaring agents whichact as lsquomolecular propsrsquo Inorganic polyoxocations such as [Al13O4(OH)24
(H2O)12]7+ are popular pillaring agents but a variety of organic and organometallic
22 Solid Acid Catalysis 51
Fig 21 Structure of montmorillonite clay
Fig 22 Friedel-Crafts alkylations
pillaring agents have also been used Pillaring with Al13 provides an interlamellarspace of ca 08 nm which remains after drying The major goal of the pillaringprocess is to produce novel inexpensive materials with properties (pore shapeand size acidity etc) complementary to zeolites (see next section)
222Zeolites and Zeotypes Synthesis and Structure
Zeolites are crystalline aluminosilicates comprising corner-sharing SiO4 andAlO4
ndash terahedra and consisting of a regular system of pores (channels) and cav-ities (cages) with diameters of molecular dimensions (03 to 14 nm) [11ndash14] Alarge number of zeolites are known some of which are naturally occurring butmost of which have been synthesized [29] Analogous structures containing TO4
tetrahedra composed of Si Al or P as well as other main group and transitionelements eg B Ga Fe Ge Ti V Cr Mn and Co have also been synthesisedand are generically referred to as zeotypes They include for example AlPOsSAPOs and MeAPOs [30] As with amorphous aluminosilicates zeolites containan extraframework cation usually Na+ to maintain electroneutrality with theAlO4
ndash moiety These extraframework cations can be replaced by other cations byion exchange Since zeolites react with acids the proton-exchanged species (H-form) is best prepared by ion exchange with an ammonium ion followed bythermal dissociation affording ammonia and the acid form of the zeolite TheBroslashnsted acid strength of the latter which is of the same order as that of con-centrated sulfuric acid is related to the SiAl ratio Since an AlO4
ndash moiety is un-stable when attached to another AlO4
ndash unit it is necessary that they are sepa-rated by at least one SiO4 unit ie the SiAl ratio cannot be lower than one (theH-form is depicted in Fig 23) The number of proton donor hydroxy groupscorresponds to the number of aluminum atoms present in the structure Themore isolated this silanol species the stronger the acid ie the acid strength in-creases with decreasing aluminum content or increasing SiAl ratio (but notethat complete replacement of aluminum affords a material with lower acidity)
2 Solid Acids and Bases as Catalysts52
Fig 23 The acid form of zeolites
Zeolites are prepared by so-called hydrothermal synthesis a simplified schemeof which is shown in Fig 24 The basic ingredients ndash SiO2 Na2SiO3 or Si(OR)4
and Al2O3 NaAlO2 or Al(OR)3 ndash together with a structure directing agent (tem-plate) usually an amine or tetraalkylammonium salt are added to aqueous alka-li (pH 8ndash12) This results in the formation of a solndashgel comprising monomericand oligomeric silicate species Gradual heating of this mixture up to ca 200 Cresults in dissolution of the gel to form clusters of SiO4AlO4
ndash units which con-stitute the building blocks for the zeolite structure In the presence of the tem-plate these building blocks undergo polymerization to form the zeolite whichcrystallizes slowly from the reaction mixture At this point the zeolite still con-tains the occluded organic template This is subsequently removed by calcina-tion ie heating in air at 400ndash600 C to burn out the template and evaporatewater
Similarly zeotype molecular sieves are synthesized by mixing the basic ingre-dients with the organic template eg aluminophosphates are prepared fromalumina and phosphoric acid Other main group or transition elements can beincorporated into the framework by adding them to the initial solndashgel Alterna-tively different elements can be introduced by post-synthesis modification (seelater) eg by dealumination followed by insertion of the new elements into theframework position [31]
The most important feature of zeolites (and zeotypes) in the context of cataly-sis is not their range of acidndashbase properties since that is also available withamorphous alumino-silicates It is the presence of a regular structure containing
22 Solid Acid Catalysis 53
Fig 24 Simplified zeolite synthesis scheme
molecular sized cavities and channels that make them unique as shape selectivecatalysts for a wide variety of organic transformations
Representation of zeolite structures is different to that used by organic che-mists The intersection of lines represents either an SiO4 or an AlO4
ndash tetrahedronand the line itself represents an O atom joining the two tetrahedra In Fig 25eight TO4 octahedra are joined together in a ring commonly referred to as the8-ring structure as there are eight oxygen atoms in the ring These basic ring struc-tures are combined to form three dimensional arrangements which constitute thebuilding blocks for the zeolite For example one of these building units is the so-dalite cage a truncated octahedron with four-membered rings made during trun-cation and six-membered rings as part of the original octahedron
In zeolites derived from the sodalite unit these cages are joined togetherthrough extensions of either the 4-ring or the 6-ring Zeolite A (see Fig 26) isan example of the former The center of the structure comprises a supercagewith a diameter of 114 nm surrounded by eight sodalite cages Access to thesecages is via the six mutually perpendicular 8-ring openings having a diameterof 042 nm enabling linear hydrocarbons to enter The SiAl ratio is 1ndash12 mak-ing zeolite A among the least acidic of all zeolites
Faujasites are naturally occurring zeolites composed of sodalite cages joinedthrough extensions of their 6-ring faces An internal supercage of ca 13 nm diam-eter is accessed by four 12-ring openings with a diameter of 074 nm The latterprovide access for relatively large aliphatic and aromatic molecules eg naphtha-lene The synthetic zeolites X and Y have the same crystal structure as faujasite butdiffer in their SiAl ratios In zeolites X and Y the SiAl ratio is 1ndash15 and 15ndash3respectively while faujasite has a SiAl ratio of ca 22
Mordenite is a naturally occurring zeolite with a SiAl ratio of ca 10 and astructure composed of 12-ring and 8-ring tunnels with diameters of 039 nmand ca 07 nm respectively extending through the entire framework (Fig 27)Every framework atom forms a part of the walls of these tunnels and is accessi-ble to substrate molecules diffusing through them
The synthetic zeolite ZSM-5 is a highly siliceous material with a SiAl ratiofrom 25 up to 2000 [32] As shown in Fig 27 it consists of a three-dimensionalnetwork of two intersecting 10-ring tunnel systems of 055ndash06 nm diameterOne of these resembles the 12-ring tunnels passing through mordenite (see
2 Solid Acids and Bases as Catalysts54
Fig 25 Basic units in zeolites
above) while the other follows a sinusoidal path perpendicular to and intersect-ing with the first The basic structural unit of this zeolite is the pentasil unitcomposed of fused 5-rings (Fig 28)
Zeolites are conveniently divided into groups on the basis of their pore sizesndash small medium large and ultra large ndash which are determined by the ring size
22 Solid Acid Catalysis 55
Fig 26 Structures of zeolite A and faujasite
Fig 27 Structures of mordenite and ZSM-5
of the pore openings Examples of commonly used zeolites and zeotypes are col-lected in Table 21
Obviously the pore size determines which molecules can access the acidicsites inside the zeolite framework (molecular sieving effect) and is responsiblefor the shape selectivity observed with these materials (see later) The catalyticactivity is also influenced by the acid strength of these sites which is deter-mined by the SiAl ratio (see above) The latter can be increased by post-synthe-sis removal of Al atoms Dealumination can be achieved by treatment with a
2 Solid Acids and Bases as Catalysts56
Fig 28 The pentasil unit
Table 21 Pore dimensions of molecular sieves
Ring size Structure type Isotopic frameworkstructures
Pore size(nm)
Dimensionality
Small pore8 LTA Zeolite A 41 3
Medium pore10 MFI ZSM-5
silicalite5653 3
10 MEL ZSM-11 5453 310 AEL AlPO-11
SAPO-116339 1
Large pore12 FAU X Y 74 312 MOR Mordenite 7065 212 BEA Beta 7557 312 LTL L 71 112 AFI AlPO-5 73 1
Extra large pore14 AlPO-8 8779 118 VFI VPI-5 121 120 Cloverite 13260 3Unknown M41S MCM-41 40ndash100 1
strong acid or a chelating agent such as EDTA or by steaming It results in theformation of lsquosilanol nestsrsquo with retention of the framework structure (Fig 29)
The wide range of pore sizes available coupled with their tunable acidity en-dows the zeolites with unique properties as tailor-made (acid) catalysts Theseimportant features of zeolites (and zeotypes) may be summarized as follows regular microenvironment and uniform internal structure large internal surface area pores of molecular dimensions (shape selectivity) control of pore size and shape by choice of template andor post synthesis
modification control of pore hydrophobicityhydrophilicity control of acidity by adjusting constitution (SiAl ratio) ion exchange or post-
synthesis modification framework substitution by transition elements the presence of strong electric fields within the confined space of the chan-
nels and cavities can serve to activate substrate molecules
The earliest applications of zeolites utilized the molecular sieving properties ofsmall pore zeolites eg zeolite A in separation and purification processes suchas drying and linearbranched alkane separation [33] In 1962 Mobil Oil intro-duced the use of synthetic zeolite X an FCC (fluid catalytic cracking) catalyst inoil refining In the late sixties the WR Grace company introduced the ldquoultra-
22 Solid Acid Catalysis 57
Fig 29 Formation of a silanol nest by dealumination
stablerdquo zeolite Y (USY) as an FCC catalyst produced by steaming of zeolite Ywhich is still used today The use of zeolite A as a replacement for phosphatesin detergents was first introduced by Henkel in 1974 Although their synthesishad already been reported by Mobil in the late 1960s extensive studies of cataly-tic applications of the high-silica zeolites typified by ZSM-5 and beta were notconducted until the 1980s and 1990s ZSM-5 was first applied as an FCC addi-tive to generate high octane gasoline by taking advantage of its shape selectivityin cracking linear rather than branched alkanes ZSM-5 was subsequently ap-plied as a shape selective acid catalyst in a wide variety of organic transforma-tions (see later)
The 1980s also witnessed the explosive development of a wide variety of zeo-types notably the aluminophosphate (AlPO) based family of molecular sieves[30] The early 1990s saw the advent of a new class of mesoporous molecularsieves the ordered mesoporous (alumino)silicates synthesized with the help ofsurfactant micelle templates (see Fig 210) [34ndash37] Exemplified by the MobilM415 materials of which MCM-41 is the most well-known these micelle-tem-plated silicas contain uniform channels with tunable diameters in the range of15 to 10 nm and a greater uniformity of acid sites than other amorphous mate-rials According to the IUPAC definition microporous materials are those hav-ing pores lt 2 nm in diameter and mesoporous solids those with pore diametersin the range 2 to 50 nm
As noted above one of the most important characteristics of zeolites is theirability to discriminate between molecules solely on the basis of their size Thisfeature which they share with enzymes is a consequence of them having poredimensions close to the kinetic diameter of many simple organic moleculesHence zeolites and zeotypes have sometimes been referred to as mineral en-zymes This so-called shape selectivity can be conveniently divided into threecategories substrate selectivity product selectivity and transition state selectivityExamples of each type are shown in Fig 211
In substrate selectivity access to the catalytically active site is restricted to oneor more substrates present in a mixture eg dehydration of a mixture of n-buta-nol and isobutanol over the small pore zeolite CaA results in dehydration ofonly the n-butanol [38] while the bulkier isobutanol remains unreacted Product
2 Solid Acids and Bases as Catalysts58
Fig 210 Synthesis of mesoporous micelle-templated molecular sieves
selectivity is a result of differences in the size of products formed in a reversibleprocess inside a molecular sieve For example when methanol is allowed to re-act with toluene over H-ZSM-5 p-xylene is formed almost exclusively becausethis molecule can easily diffuse out of the molecular sieve The bulkier o- andm-isomers in contrast cannot pass easily through the pores and consequentlyundergo isomerization via demethylation to the p-isomer Restricted transitionstate selectivity is observed when the zeolite discriminates between two differenttransformations on the basis of the bulk of their transition states In the exam-ple shown the disproportionation of o-xylene to trimethylbenzene and tolueneinvolves a bulky diaryl species in the transition state whereas isomerization tom- or p-xylene does not Hence disproportionation is not observed over H-ZSM-5 Most applications of zeolites as acid catalysts involve one or more of thesetypes of shape selectivity as we shall see in the following section
223Zeolite-catalyzed Reactions in Organic Synthesis
Pertinent examples of zeolite-catalyzed reactions in organic synthesis includeFriedel-Crafts alkylations and acylations and other electrophilic aromatic substi-tutions additions and eliminations cyclizations rearrangements and isomeriza-tions and condensations
22 Solid Acid Catalysis 59
Fig 211 Shape selective catalysis with zeolites
2231 Electrophilic Aromatic SubstitutionsFriedel-Crafts alkylations are widely used in both the bulk and fine chemical in-dustries For example ethylbenzene (the raw material for styrene manufacture)is manufactured by alkylation of benzene with ethylene (Fig 212)
The original process developed in the 1940s involved traditional homoge-neous catalysis by AlCl3 This process was superseded by one employing a het-erogeneous catalyst consisting of H3PO4 or BF3 immobilized on a support(UOP process) This system is highly corrosive and because of the enormousproduction volumes involved generates substantial amounts of acidic waste Amajor breakthrough in FC alkylation technology was achieved in 1980 with theapplication of the medium pore zeolite H-ZSM-5 as a stable recyclable catalystfor ethylbenzene manufacture (Mobil-Badger process) An added benefit of thisprocess is the suppression of polyalkylation owing to the shape selective proper-ties of the catalyst
This process marked the beginning of an era of intensive research whichcontinues to this day on the application of zeolites in the manufacture of petro-chemicals and more recently fine chemicals
Zeolite-based processes have gradually displaced conventional ones involvingsupported H3PO4 or AlCl3 as catalysts in the manufacture of cumene the rawmaterial for phenol production [1 6 39] A three-dimensional dealuminatedmordenite (3-DDM) catalyst was developed by Dow Chemical for this purpose[39] Dealumination using a combination of acid and thermal treatments in-creases the SiAl ratio from 10ndash30 up to 100ndash1000 and at the same timechanges the total pore volume and pore-size distribution of the mordenite The
2 Solid Acids and Bases as Catalysts60
Fig 212 Zeolite-catalyzed Friedel-Crafts alkylations
3-DDM catalysts have a new pore structure consisting of crystalline domains of8- and 12-ring pores connected by mesopores (5ndash10 nm) The presence of thelatter enhances accessibility to the micropore regions without seriously compro-mising the shape-selective character of the catalyst This combination ofchanges in acidity and pore structure transforms synthetic mordenites intohighly active stable and selective alkylation catalysts
Dow Chemical also pioneered the shape-selective dialkylation of polyaro-matics eg naphthalene and biphenyl (see Fig 212) using the same type of 3-DDM catalyst [39] The products are raw materials for the production of the cor-responding dicarboxylic acids which are important industrial monomers for avariety of high performance plastics and fibres
Zeolites are also finding wide application as catalysts for FC alkylations and re-lated reactions in the production of fine chemicals For example a H-MOR typecatalyst with a SiAl ratio of 18 was used for the hydroxyalkylation of guaiacol(Fig 213) to p-hydroxymethylguaiacol the precursor of vanillin [40] Aromatic hy-droxyalkylation with epoxides is of importance in the production of fine chemicalseg the fragrance 2-phenylethanol from benzene and ethylene oxide (Fig 213)Attempts to replace the conventional process which employs stoichiometricamounts of AlCl3 with a zeolite-catalyzed conversion met with little success [641] This was largely due to the large polarity difference between the aromatic sub-strate and the epoxide alkylating agent which leads to unfavorable adsorption ra-tios between substrate and reagent This adsorption imbalance is avoided by hav-ing the aromatic and epoxide functions in the same molecule ie in an intramo-lecular hydroxyalkylation For example H-MOR and H-Beta were shown to be ef-fective catalysts for the cyclialkylation of 4-phenyl-1-butene oxide (Fig 213) [41]
The Pechmann synthesis of coumarins via condensation of phenols with -keto esters also involves an intramolecular hydroxyalkylation following initial
22 Solid Acid Catalysis 61
Fig 213 Hydroxyalkylation of aromatics
transesterification and subsequent dehydration It was found that H-Beta couldsuccessfully replace the sulfuric acid conventionally used as catalyst For exam-ple reaction of resorcinol with ethyl acetoacetate afforded methylumbelliferone(Fig 214) a perfumery ingredient and insecticide intermediate [42] Other ex-amples of the synthesis of coumarin derivatives via zeolite-catalyzed intramole-cular alkylations have also been described (Fig 214) [6 43]
Friedel-Crafts acylation of aromatics generally requires a stoichiometricamount of a Lewis acid such as AlCl3 It further shares with hydroxyalkylationthe problem of widely differing polarities of the substrate acylating agent andthe product which makes it difficult to achieve a favorable adsorption ratio ofsubstrate and reagent Moreover favored reagents such as the carboxylic acid oranhydride produce water and carboxylic acid respectively which may also bepreferentially adsorbed Hence heterogeneous catalysis of Friedel-Crafts acyla-tion is much more difficult than the related alkylations and poses a formidablechallenge As in the case of hydroxyalkylation intramolecular processes such asthe cycliacylation of 4-phenylbutyric acid to -tetralone over a H-Beta catalystproved to be more tractable (Fig 215) [44] As already noted in Chapter 1 thecommercialization of the first zeolite-catalyzed FC acylation by Rhodia consti-tutes a benchmark in this area [45 46] The process employs H-Beta or HY infixed-bed operation for the acylation of activated aromatics such as anisolewith acetic anhydride (Fig 215) It avoids the production of HCl from acetylchloride in the classical process in addition to circumventing the generation ofstoichiometric quantities of AlCl3 waste
Furthermore very high para-selectivities are observed as a result of the shape-selective properties of the zeolite catalyst
Similarly acylation of isobutylbenzene with acetic anhydride over H-Beta at140 C afforded p-acetylisobutylbenzene (Fig 215) an intermediate in the syn-
2 Solid Acids and Bases as Catalysts62
Fig 214 Zeolite-catalyzed synthesis of coumarins
thesis of the antiinflammatory drug ibuprofen in 80 yield and 96 para-selec-tivity [47]
Pioneering work in zeolite-catalyzed FC acylations was reported by Genesteand coworkers in 1986 [48] They showed that a Ce3+-exchanged zeolite Y cata-lyzed the acylation of toluene and xylenes with carboxylic acids (Fig 216) Thisdemonstrated that relatively mild acidity was sufficient to catalyze the reactionand that the free carboxylic acid could be used as the acylating agent The reac-tion exhibited a very high para-selectivity However only the more lipophilichigher carboxylic acids were effective which can be ascribed to differences inpreferential adsorption of substrate and acylating agent in the pores of the cata-lyst ie the adsorption imbalance referred to above
22 Solid Acid Catalysis 63
Fig 215 Zeolite-catalyzed Friedel-Crafts acylations
Fig 216 Acylation of toluene over Ce3+-exchanged zeolite Y
Subsequently Corma and coworkers [49] reported the acylation of anisole withphenacetyl chloride over H-Beta and H-Y The FC acylation of electron-rich hetero-aromatics such as thiophene and furan with acetic anhydride over modified ZSM-5 catalysts (Fig 217) in the gas phase [50] or liquid phase [51] was also reported
Almost all of the studies of zeolite-catalyzed FC acylations have been con-ducted with electron-rich substrates There is clearly a commercial need there-fore for systems that are effective with electron-poor aromatics In this contextthe reports [52] on the acylation of benzene with acetic acid over H-ZSM-5 inthe gas phase are particularly interesting These results suggest that the adsorp-tion ratios of substrate acylating agent and product are more favorable in thegas phase than in the liquid phase
Zeolites have also been investigated as heterogeneous catalysts for other elec-trophilic aromatic substitutions eg nitration [53] and halogenation [54] Aro-matic nitration for example traditionally uses a mixture of sulfuric and nitricacids which leads to the generation of copious quantities of spent acid wasteDealuminated mordenite (see earlier) is sufficiently robust to function effec-tively as a catalyst for the vapor phase nitration of benzene with 65 aqueousnitric acid [55] The advantage of using vapor phase conditions is that the wateris continuously removed Although these results are encouraging aromatic ni-tration over solid acid catalysts is still far from commercialization
An interesting example of aromatic halogenation in the context of greenchemistry is the production of 26-dichlorobenzonitrile an agrochemical inter-mediate The conventional process involves a series of reactions (see Fig 218)with Cl2 HCN and POCl3 as stoichiometric reagents having an atom efficiencyof 31 and generating substantial amounts of salts as waste The new processdeveloped by Toray [56] involves vapor phase chlorination of toluene over a Ag-H-Mordenite catalyst to give a mixture of dichlorotoluene isomers The required26-isomer is separated by adsorption in faujasite or AlPO-11 and the other iso-mers are returned to the chlorination reactor where equilibration occurs The26-dichlorotoluene can be subsequently converted to 26-dichlorobenzonitrile byvapour phase ammoxidation over an oxide catalyst
2 Solid Acids and Bases as Catalysts64
Fig 217 Acylation of heteroaromatics over zeolite catalysts
2232 Additions and EliminationsZeolites have been used as (acid) catalysts in hydrationdehydration reactions Apertinent example is the Asahi process for the hydration of cyclohexene to cyclo-hexanol over a high silica (SiAl gt 20) H-ZSM-5 type catalyst [57] This processhas been operated successfully on a 60 000 tpa scale since 1990 although manyproblems still remain [57] mainly due to catalyst deactivation The hydration ofcyclohexanene is a key step in an alternative route to cyclohexanone (and phe-nol) from benzene (see Fig 219) The conventional route involves hydrogena-tion to cyclohexane followed by autoxidation to a mixture of cyclohexanol and
22 Solid Acid Catalysis 65
Fig 218 Two processes for 26-dichlorobenzonitrile
cyclohexanone and subsequent dehydrogenation of the former A serious disad-vantage of this process is that the autoxidation gives reasonable selectivities (75ndash80) only at very low conversions (ca 5) thus necessitating the recycle of en-ormous quantities of cyclohexane The Asahi process involves initial partial hy-drogenation of benzene to cyclohexene over a heterogeneous ruthenium cata-lyst The cyclohexane byproduct is recycled by dehydrogenation back to benzeneThe cyclohexene hydration proceeds with gt 99 selectivity at 10ndash15 conver-sion If the ultimate product is adipic acid the cyclohexanone can be by-passedby subjecting cyclohexanol to oxidation (see Fig 219) [57]
2 Solid Acids and Bases as Catalysts66
Fig 219 Two processes for cyclohexanone
Fig 220 Two processes for tert-butylamine
Similarly zeolites can catalyze the addition of ammonia to an olefinic doublebond as is exemplified by the BASF process for the production of tert-butylamineby reaction of isobutene with ammonia in the vapor phase over a rare earth ex-changed ZSM-5 or Y zeolite (Fig 220) [58 59] This process has an atom efficiencyof 100 and replaced a conventional synthesis via a Ritter reaction which em-ploys HCN and sulfuric acid and generates formate as a coproduct
2233 Rearrangements and IsomerizationsAs already discussed in Chapter 1 the commercialization by Sumitomo [60ndash64] of a vapor phase Beckmann rearrangement of cyclohexanone oxime to capro-lactam over a high-silica MFI (ZSM-5 type) zeolite (Fig 221) is another bench-mark in zeolite catalysis The process which currently operates on a 90 000 tpascale replaces a conventional one employing stoichiometric quantities of sulfu-ric acid and producing ca 2 kg of ammonium sulfate per kg of caprolactam
Interestingly the activity of the catalyst was proportional to its external sur-face area This together with the fact that caprolactam does not fit easily intothe pores of the zeolite strongly suggests that the reaction takes place on theexternal surface possibly at the pore openings Ichihashi and coworkers [61]proposed that the reaction takes place in a silanol nest resulting from dealumi-nation (see earlier) as was also suggested by Hoelderich and coworkers [65]
The Friedel-Crafts acylation of phenols proceeds via initial esterification fol-lowed by Fries rearrangement of the resulting aryl ester to afford the hydroxyaryl
22 Solid Acid Catalysis 67
Fig 221 Zeolite-catalyzed Beckmann rearrangement
ketone For example phenylacetate affords a mixture of o- and p-hydroxyaceto-phenone (see Fig 222) The latter is a key intermediate in the Hoechst Cela-nese process for the manufacture of the analgesic paracetamol
Traditionally the Fries rearrangement is conducted with stoichiometricamounts of mineral (H2SO4 HF) or Lewis acids (AlCl3 ZnCl2) and generateslarge amounts of inorganic salts as by-products ie it suffers from the samedisadvantages as standard Friedel-Crafts acylations Substitution of these corro-sive polluting and non-regenerable catalysts by regenerable solid acid catalystshas obvious environmental benefits Consequently a variety of solid acids par-ticularly zeolites have been studied as catalysts for the Fries rearrangementboth in the vapor and liquid phases [66] Most studies were performed withphenyl acetate as the substrate prepared ex situ or formed in situ from phenoland acetic anhydride or acetic acid A variety of zeolites have been used eg H-Y H-ZSM-5 and H-beta generally affording o-hydroxyacetophenone as the ma-jor product often in very high selectivity [67] None of these processes has beenbrought to commercialization presumably because they produce the commer-cially less interesting isomer as the product
Another example of commercial interest is the Fries rearrangement of thebenzoate ester of resorcinol to afford 24-dihydroxybenzophenone the precursorof the UV-absorbent 4-O-octyl-2-hydroxybenzophenone Reaction of benzoic acidwith one equivalent of resorcinol (see Fig 222) over various solid catalysts inchlorobenzene as solvent with continuous removal of water was investigated byHoefnagel and van Bekkum [68] H-Beta was slightly less active than the ion-ex-
2 Solid Acids and Bases as Catalysts68
Fig 222 Fries rearrangement over zeolites
change resin Amberlyst 15 but gave less by-product formation and has the ad-vantage of being regenerable by simple air burn-off It would appear to have en-vironmental benefits compared to the existing industrial process which gener-ates substantial amounts of chloride waste (see Fig 222)
Epoxide rearrangements are key steps in the manufacture of numerous syn-thetic intermediates in the fine chemical industry They are generally performedwith conventional Broslashnsted or Lewis acids or strong bases as catalysts often instoichiometric amounts Here again replacement by recyclable solid catalystshas obvious benefits [69]
For example rearrangement of -pinene oxide produces among the ten or somajor products campholenic aldehyde the precursor of the sandalwood fra-grance santalol The conventional process employs stoichiometric quantities ofzinc chloride but excellent results have been obtained with a variety of solid acidcatalysts (see Fig 223) including a modified H-USY [70] and the Lewis acid Ti-Beta [71] The latter afforded campholenic aldehyde in selectivities up to 89 inthe liquid phase and 94 in the vapor phase
Similarly the rearrangement of substituted styrene oxides to the correspond-ing phenylacetaldehydes (see Fig 223) affords valuable intermediates for fra-grances pharmaceuticals and agrochemicals Good results were obtained usingzeolites eg H-ZSM-5 in either the liquid or vapor phase [69] The solid Lewisacid titanium silicalite-1 (TS-1) also gave excellent results eg styrene oxidewas converted to phenylacetaldehyde in 98 selectivity at 100 conversion in1ndash2 h at 70 C in acetone as solvent Other noteworthy epoxide rearrangements
22 Solid Acid Catalysis 69
Fig 223 Zeolite-catalyzed epoxide rearrangements
are the conversion of isophorone oxide to the keto aldehyde (see Fig 223) overH-mordenite [72] or H-US-Y (SiAl = 48) [69] and 23-dimethyl-2-butene oxide topinacolone [73] The mechanistically related pinacol rearrangement eg of pina-col to pinacolone has also been conducted over solid acid catalysts includingacidic clays and zeolites [74]
2234 CyclizationsZeolites have also been shown to catalyze a variety of acid-promoted cycliza-tions Many of these involve the formation of N-heterocycles via intramolecularamination reactions [75ndash77] Some examples are shown in Fig 224
Reaction of ammonia with various combinations of aldehydes over solid acidcatalysts in the vapor phase is a convenient route for producing pyridines [77]For example amination of a formaldehydeacetaldehyde mixture affords pyri-dine and 3-picoline (Fig 225) Mobil scientists found that MFI zeolites such asH-ZSM-5 were particularly effective for these reactions
Alternatively 3-picoline is produced by vapor phase cyclization of 2-methyl-pentane-15-diamine (Fig 225) over for example H-ZSM-5 followed by palla-dium-catalyzed dehydrogenation [78] This diamine is a by-product of the manu-facture of hexamethylenediamine the raw material for nylon 66 and these tworeactions are key steps in the Lonza process for nicotinamide production (seeChapter 1) [79]
2 Solid Acids and Bases as Catalysts70
Fig 224 Zeolite-catalyzed cyclizations
Other examples of zeolite-catalyzed cyclizations include the Fischer indolesynthesis [80] and Diels-Alder reactions [81]
224Solid Acids Containing Surface SO3H Functionality
This category encompasses a variety of solid acids with the common feature ofa sulfonic acid moiety attached to the surface ie they are heterogeneousequivalents of the popular homogeneous catalysts p-toluenesulfonic and metha-nesulfonic acids The cross-linked polystyrene-based macroreticular ion ex-change resins such as Amberlystreg-15 are probably the most familiar examplesof this class They are the catalysts of choice in many industrial processes andin laboratory scale organic syntheses eg esterifications etherifications andacetalizations [2 16 17] However a serious shortcoming of conventional poly-styrene-based resins is their limited thermal stability Reactions requiring ele-vated temperatures can be conducted with the more thermally stable Nafionreg
resins which consist of a perfluorinated Teflon-like polymeric backbone func-tionalized with terminal SO3H groups [2 82ndash85] These materials (see Fig 226for structure) were originally developed by DuPont for application as mem-branes in electrochemical processes based on their inertness to corrosive envi-ronments Nafion is commercially available as Nafion NR50 (DuPont) in the
22 Solid Acid Catalysis 71
Fig 225 Synthesis of pyridines via zeolite-catalyzed cyclizations
Fig 226 Structures of polystyrene- and perfluorocarbon-based ion exchange resins
form of relatively large (2ndash3 mm) beads or as a 5 solution in a mixture of alower alcohol and water Other major differences with the polystyrene-based re-sins are their superior acid strength and higher number of acid sites As a con-sequence of their highly electron-withdrawing perfluoroalkyl backbone Nafion-H has an acidity comparable with that of 100 sulfuric acid ie an acidityfunction (Ho) of ndash11 to ndash13 compared with ndash22 for Amberlyst-15 It also hasfive times as many acid sites as the latter This superacidity coupled with ther-mal stability (up to 280 C) make Nafion-H an attractive catalyst for a variety ofprocesses [2 16 17] Thus reactions not requiring especially strong acidity andor high temperatures are usually conducted with the less expensive polystyrene-based resins while those that require higher acidity andor temperatures can beperformed better with the more robust Nafion-H
However Nafion-H NR50 beads have one serious drawback they have a verylow surface area (lt 002 m2 gndash1) To overcome this disadvantage DuPont research-ers developed Nafion-silica composites consisting of small (20ndash60 nm) Nafion re-sin particles embedded in a porous silica matrix [86] The microstructure can beregarded as a porous silica network containing a large number of lsquopocketsrsquo of verystrong acid sites (the Nafion polymer) in domains of ca 10ndash20 nm The surfacearea is increased by several orders of magnitude and the catalytic activity per unitweight is up to 1000 times that of the pure Nafion They are prepared by a solndashgeltechnique and are available as SAC 13 which contains 13 (ww) Nafion The im-proved accessibility to the active sites makes this material a particularly attractivesolid acid catalyst [2 84] for a variety of reactions such as Friedel-Crafts alkylations[86 87] and Friedel-Crafts acylations [2] The latter are effective only with electron-rich aromatics such as anisole The Nafion-silica composite was compared withthe pure polymer and Amberlyst-15 in the alkylation of p-cresol with isobutene[2] The results are shown in Table 22
Nafion-silica composites were compared with zeolites such as H-Beta H-USYand H-ZSM-5 in the Fries rearrangement of phenyl acetate (see earlier) Thehighest conversion was observed with H-Beta [88]
Another class of thermally stable polymers containing surface SO3H function-alities comprises the sulfonated polysiloxanes (see Fig 227) [89] They are bestprepared by a solndashgel technique involving copolymerization of functionalizedand non-functionalized silanes eg 3-(tris-hydroxysilyl)propyl sulfonic acid withtetraethoxysilane This solndashgel process affords material with a high surface area(300ndash600 m2 gndash1) high porosity and large mesopores (gt 20 nm) Although theyhave excellent chemical and thermal stability and have been marketed underthe trade name Deloxanreg industrial applications have not yet been forthcom-ing probably owing to their relatively high price
Similarly perfluoroalkylsulfonic acid moieties can be covalently attached to asilica matrix by grafting a silica surface with (EtO)3Si(CH2)3(CF2)2O(CF2)2SO3H(see Fig 227) or by using the latter in a solndashgel synthesis [18 90]
More recently attention has shifted to the preparation of hybrid organicndashinor-ganic ordered mesoporous silicas eg of the M41S type (see earlier) bearingpendant alkylsulfonic acid moieties [18 91ndash96] These materials combine a high
2 Solid Acids and Bases as Catalysts72
surface area high loading and acid strength with excellent site accessibility andregular mesopores of narrow size distribution This unique combination ofproperties makes them ideal solid acid catalysts for in particular reactions in-volving relatively bulky molecules as reactants andor products They are pre-pared by grafting of preformed MCM-41 with for example 3-mercaptopropyltri-methoxysilane (MPTS) followed by oxidation of the pendant thiol groups toSO3H with hydrogen peroxide (Fig 228) [18] Alternatively direct co-condensa-tion of tetraethoxysilane (TEOS) with MPTS in the presence of a surfactant tem-plating agent such as cetyltrimethylammonium bromide or dodecylamine af-fords functionalized MCM-41 or HMS (hexagonal mesoporous silica) respec-tively [18 91ndash96] Non-ionic surfactants eg the poly(ethylene oxide)ndashpoly(pro-pylene oxide) block copolymer commercially available as Pluronic 123 have
22 Solid Acid Catalysis 73
Table 22 Acid catalyzed alkylation of p-cresol
Catalyst Conv () Selectivity () Rate(mMgndash1 cat middothndash1)
Ether Alkylates
13 NafionSiO2 826 06 994 5810
Nafion NR50 195 282 718 548
Amberlyst-15 624 145 855 1710
Fig 227 Synthesis of SO3H-functionalized silicas
been used under acidic conditions [91 92 96] When hydrogen peroxide isadded to the solndashgel ingredients the SH groups are oxidized in situ affordingthe SO3H-functionalized mesoporous silica in one step [91 92] Alternativelyco-condensation of TEOS with 2-(4-chlorosulfonylphenyl)ethyltrimethoxysilanein the presence of Pluronic 123 as template afforded a mesoporous materialcontaining pendant arenesulfonic acid moieties (see Fig 228) [91 92]
These mesoporous SO3H-functionalized silicas are attractive recyclable acidcatalysts for reactions involving molecules that are too large to access the smal-ler pores of conventional molecular sieves or those affording bulky productsThe additional option of modifying their hydrophobicityhydrophilicity balanceby introducing varying amounts of alkyltrialkoxysilanes eg CH3CH2CH2
Si(OEt)3 into the solndashgel synthesis provides an opportunity to design tailor-made solid acid catalysts [94] These organicndashinorganic materials have been usedas acid catalysts in for example esterifications of polyols with fatty acids [1894 95] Friedel-Crafts acylations [97] and bisphenol-A synthesis [93] The latteris an important raw material for epoxy resins and is manufactured by reactionof phenol with acetone (see Fig 229) using ion exchange resins such as Amber-lystreg-15 as catalyst However thermal stability and fouling are major problemswith these catalysts and there is a definite need for thermally stable recyclablesolid acid catalysts A sulfonic acid functionalized MCM-41 produced by graft-ing of preformed MCM-41 with MPTS and subsequent H2O2 oxidation exhib-ited a superior activity and selectivity compared with various zeolites Unfortu-nately the crucial comparison with Amberlyst-15 was not reported
Finally the functionalization of mesoporous silicas with perfluoroalkylsulfonicacid groups by grafting with 122-trifluoro-2-hydroxy-1-trifluoromethylethane
2 Solid Acids and Bases as Catalysts74
Fig 228 Synthesis of ordered mesoporous silicas containing pendant SO3H groups
sulfonic acid -sultane (see Fig 230) was recently reported [98] The resultingmaterials displayed a higher activity than commercial Nafionreg silica composites(see earlier) in the esterification of ethanol with octanoic acid [98]
225Heteropoly Acids
Heteropoly acids (HPAs) are mixed oxides composed of a central ion or lsquohet-eroatomrsquo generally P As Si or Ge bonded to an appropriate number of oxygenatoms and surrounded by a shell of octahedral MO6 units usually whereM= Mo W or V HPAs having the so-called Keggin structure are quite com-mon and consist of a central tetrahedron XO4 (X = P As Si Ge etc) sur-rounded by 12 MO6 octahedra (M= Mo W V) arranged in four groups of threeedge-sharing M3O13 units (see Fig 231)
Many HPAs exhibit superacidity For example H3PW12O40 has a higher acidstrength (Ho = ndash1316) than CF3SO3H or H2SO4 Despite their rather dauntingformulae they are easy to prepare simply by mixing phosphate and tungstate inthe required amounts at the appropriate pH [99] An inherent drawback of
22 Solid Acid Catalysis 75
Fig 229 Bisphenol-A synthesis over MCM-SO3H
Fig 230 Mesoporous silica grafted with perfluoroalkylsulfonic acid groups
HPAs however is their solubility in polar solvents or reactants such as wateror ethanol which severely limits their application as recyclable solid acid cata-lysts in the liquid phase Nonetheless they exhibit high thermal stability andhave been applied in a variety of vapor phase processes for the production ofpetrochemicals eg olefin hydration and reaction of acetic acid with ethylene[100 101] In order to overcome the problem of solubility in polar media HPAshave been immobilized by occlusion in a silica matrix using the solndashgel tech-nique [101] For example silica-occluded H3PW12O40 was used as an insolublesolid acid catalyst in several liquid phase reactions such as ester hydrolysis es-terification hydration and Friedel-Crafts alkylations [101] HPAs have also beenwidely applied as catalysts in organic synthesis [102]
23Solid Base Catalysis
Examples of the application of recyclable solid base catalysts are far fewer thanfor solid acids [103] This is probably because acid-catalyzed reactions are muchmore common in the production of commodity chemicals The various catego-ries of solid bases that have been reported are analogous to the solid acids de-scribed in the preceding sections and include anionic clays basic zeolites andmesoporous silicas grafted with pendant organic bases
231Anionic Clays Hydrotalcites
Anionic clays are natural or synthetic lamellar mixed hydroxides with interlayerspaces containing exchangeable anions [10 104] The generic terms layered dou-ble hydroxides (LDHs) or hydrotalcites are widely used the latter because exten-
2 Solid Acids and Bases as Catalysts76
Fig 231 Keggin structure of [PW12O40]3ndash
P-atoms W-atoms O-atoms
sive characterization has been performed on hydrotalcite (a MgAl hydroxy-carbonate) which is both inexpensive and easy to synthesize
Hydrotalcite is a natural mineral of ideal formula Mg6Al2(OH)16CO3 middot 4H2Ohaving a structure similar to brucite Mg(OH)2 In hydrotalcite the Mg cationsare partially replaced with Al3+ and the resulting positive charge is compensatedby anions typically carbonate in the interlamellar space between the brucite-like sheets When hydrotalcite is calcined at ca 500 C it is decarbonated anddehydrated to afford a strongly basic mixed MgAl oxide Rehydration restoresthe original hydrotalcite structure and creates Broslashnsted base sites (OHndash) in theinterlamellar space
Activated hydrotalcites prepared in this way have been used as solid base cata-lysts in for example the aldol and related reactions [105] The aldol condensa-tion is a key step in the production of several commodity chemicals includingthe solvent methylisobutylketone (MIBK) and 2-ethylhexanol the precursor ofthe PVC plasticizer dioctylphthalate (see Fig 232) More than 1 million tons ofthese chemicals are produced worldwide on an annual basis using homoge-neous bases such as 30 aqueous caustic (NaOH) [106] Major problems are as-sociated with the safe handling of the 30 caustic and treatment of caustic con-taminated waste streams About 1 kg of spent catalyst is generated per 10 kg ofproduct and it has been estimated that 30 of the selling price is related toproduct recovery purification and waste treatment Hence there is a definite in-centive to replace these homogeneous bases with recyclable solid bases and hy-drotalcites have been used to catalyze the aldol condensation of n-butyraldehydein the liquid phase and acetone in the vapor phase to give 2-ethylhexenal andmesityl oxide respectively [105] Hydrogenation of the aldol condensation prod-ucts yields 2-ethylhexanol and MIBK respectively (Fig 232) Impregnation of
23 Solid Base Catalysis 77
Fig 232 Synthesis of MIBK and 2-ethylhexanol via aldol condensations
the hydrotalcite with Pd or Ni affords bifunctional catalysts which are able tomediate the one-pot reductive aldol condensation of n-butyraldehyde or acetoneto 2-ethylhexanol or MIBK respectively [105]
Aldol and related condensation reactions such as Knoevenagel and Claisen-Schmidt condensations are also widely used in the fine chemicals and specialtychemicals eg flavors and fragrances industries Activated hydrotalcites havebeen employed as solid bases in many of these syntheses Pertinent examplesinclude the aldol condensation of acetone and citral [107 108] the first step inthe synthesis of ionones and the Claisen-Schmidt condensation of substituted2-hydroxyacetophenones with substituted benzaldehydes [109] the synthetic
2 Solid Acids and Bases as Catalysts78
Fig 233 Hydrotalcite-catalyzed aldol and Claisen-Schmidt condensations
route to flavonoids (see Fig 233) The diuretic drug Vesidryl was similarlysynthesized by condensation of 24-dimethoxyacetophenone with p-anisaldehyde(see Fig 233) [109]
Excellent results were also obtained using activated hydrotalcite as a solidbase catalyst in the Knoevenagel condensation of benzaldehyde with ethylcya-noacetate [110] ethylacetoacetate [111] or malononitrile [112] (see Fig 234)Similarly citronitrile a perfumery compound with a citrus-like odor wassynthesized by hydrotalcite-catalyzed condensation of benzylacetone with ethyl-cyanoacetate followed by hydrolysis and decarboxylation (Fig 234) [113]
Other reactions which have been shown to be catalyzed by hydrotalcites in-clude Michael additions cyanoethylations and alkylations of eg 13-dicarbonyl
23 Solid Base Catalysis 79
Fig 234 Hydrotalcite-catalyzed Knoevenagel condensations
Fig 235 Hydrotalcite-catalyzed oxidations with H2O2
compounds [105 114] Another interesting application is as a solid base catalystin oxidations (Fig 235) involving the hydroperoxide anion HOndash
2 [115] eg theepoxidation of electron deficient olefins with H2O2 [116] and the epoxidation ofelectron-rich olefins with PhCNH2O2 [117] The latter reaction involves the per-oxycarboximidate (Payne reagent) as the active oxidant producing one equiva-lent of the amide as a co-product Subsequent studies showed that carboxylicamides also act as catalysts in this reaction (Fig 235) isobutyramide being par-ticularly effective [118] In this case one equivalent of the ammonium carboxy-late is formed as the co-product
Interesting recent developments are the use of hydrotalcite supported on car-bon nanofibers [119] to facilitate recovery of the catalyst by filtration and theuse of synthetic hydroxyapatite Ca10(PO4)6(OH)2 as a solid base catalyst in avariety of reactions including Michael additions [120] The supported hydrotal-cite exhibited higher activities and selectivities than the conventional unsup-ported material in the aldol condensation of citral with acetone [119]
232Basic Zeolites
In contrast with the widespread application of zeolites as solid acid catalysts(see earlier) their use as solid base catalysts received scant attention until fairlyrecently [121] This is probably because acid-catalyzed processes are much morecommon in the oil refining and petrochemical industries Nonetheless basiczeolites and related mesoporous molecular sieves can catalyze a variety of reac-tions such as Knoevenagel condensations and Michael additions which are keysteps in the manufacture of flavors and fragrances pharmaceuticals and otherspecialty chemicals [121] Indeed the Knoevenagel reaction of benzaldehydewith ethyl cyanoacetate (Fig 236) has become a standard test reaction for solidbase catalysts [121]
Two approaches have been used to prepare basic zeolites by post-synthesismodification (i) ion exchange of protons by alkali metal or rare earth cationsand (ii) generation of nanoparticles of alkali metal or alkaline earth metal oxideswithin the zeolite channels and cavities (see later) In zeolites Lewis basicity isassociated with the negatively charged framework oxygens and as expected in-creases with the size of the counter cation ie Lilt Na lt Ka lt Cs Alkali-ex-changed zeolites contain a large number of relatively weak basic sites capable ofabstracting a proton from molecules having a pKa in the range 9ndash11 and a fewmore basic ones (up to pKa = 133) [121] This corresponds with the basic
2 Solid Acids and Bases as Catalysts80
Fig 236 Knoevenagel reaction
strength required to catalyze many synthetically useful reactions such as theKnoevenagel and Michael reactions referred to above The use of the ion-ex-changed zeolites as base catalysts has the advantage that they are stable towardsreaction with moisture andor carbon dioxide
Cesium-exchanged zeolite X was used as a solid base catalyst in the Knoeve-nagel condensation of benzaldehyde or benzyl acetone with ethyl cyanoacetate[121] The latter reaction is a key step in the synthesis of the fragrance mole-cule citronitrile (see Fig 237) However reactivities were substantially lowerthan those observed with the more strongly basic hydrotalcite (see earlier) Simi-larly Na-Y and Na-Beta catalyzed a variety of Michael additions [122] and K-Yand Cs-X were effective catalysts for the methylation of aniline and phenylaceto-nitrile with dimethyl carbonate or methanol respectively (Fig 237) [123] Theseprocedures constitute interesting green alternatives to classical alkylations usingmethyl halides or dimethyl sulfate in the presence of stoichiometric quantitiesof conventional bases such as caustic soda
Alkali-exchanged mesoporous molecular sieves are suitable solid base catalystsfor the conversion of bulky molecules which cannot access the pores of zeolitesFor example Na- and Cs-exchanged MCM-41 were active catalysts for the Knoe-venagel condensation of benzaldehyde with ethyl cyanoacetate (pKa = 107) butlow conversions were observed with the less acidic diethyl malonate (pKa = 133)[123] Similarly Na-MCM-41 catalyzed the aldol condensation of several bulkyketones with benzaldehyde including the example depicted in Fig 238 inwhich a flavonone is obtained by subsequent intramolecular Michael-type addi-tion [123]
As noted above the basic sites generated by alkali metal exchange in zeolitesare primarily weak to moderate in strength Alkali and alkaline earth metal oxi-des in contrast are strong bases and they can be generated within the poresand cavities of zeolites by over-exchanging them with an appropriate metal salteg an acetate followed by thermal decomposition of the excess metal salt toafford highly dispersed basic oxides occluded in the pores and cavities For ex-ample cesium oxide loaded faujasites exhibiting super-basicities were preparedby impregnating CsNa-X or CsNa-Y with cesium acetate and subsequent ther-mal decomposition [124 125] They were shown to catalyze inter alia Knoeve-nagel condensations eg of benzaldehyde with ethyl cyanoacetate [126] A simi-
23 Solid Base Catalysis 81
Fig 237 Alkylations catalyzed by basic zeolites
larly prepared Cs oxide loaded MCM-41 was an active catalyst for the Michaeladdition of diethylmalonate to chalcone (Fig 239) [127]
A serious drawback of these alkali metal oxide loaded zeolites and mesopor-ous molecular sieves is their susceptibility towards deactivation by moistureandor carbon dioxide which severely limits their range of applications
233Organic Bases Attached to Mesoporous Silicas
Analogous to the attachment of organic alkyl(aryl)sulfonic acid groups to thesurface of organic or inorganic polymers (see earlier) recyclable solid base cata-lysts can be prepared by grafting eg amine moieties to the same supportsAnion exchange resins such as Amberlyst are composed of amine or tetraalky-lammonium hydroxide functionalities grafted to cross-linked polystyrene resinsand they are widely used as recyclable basic catalysts [128] As with the cationexchange resins a serious limitation of these materials is their lack of thermalstability under reaction conditions in this case a strongly alkaline medium Thisproblem can be circumvented by grafting basic moieties to inorganic polymersthat are thermally stable under reaction conditions
The use of silica-grafted primary and tertiary amines as solid base catalysts inKnoevenagel condensations was reported already in 1988 Yields were high butactivities were rather low owing to the relatively low loadings (lt 1 mmol gndash1) Adecade later the groups of Brunel [129ndash131] Macquarrie [132ndash135] and Jacobs[136] obtained much higher loadings (up to 5 mmol gndash1) and activities by at-
2 Solid Acids and Bases as Catalysts82
Fig 238 Na-MCM-41 catalyzed flavonone synthesis
Fig 239 Cesium oxide loaded MCM-41 as a catalyst for the Michael addition
taching amine functionalities to mesoporous silicas thus taking advantage oftheir high surface areas (ca 1000 m2 gndash1) Two strategies were used for theirpreparation (i) grafting of pre-formed micelle templated silicas (MTS) withamine functionalities or with other functionalities eg halide epoxide whichcan be subsequently converted to amines by nucleophilic displacement (seeFig 240) and (ii) direct incorporation by co-condensation of (EtO)4Si with anappropriately functionalized silane in a solndashgel synthesis
For example Brunel and coworkers [137] anchored primary amine groups tothe surface of mesoporous silica by grafting with 3-aminopropyltriethoxysilaneAnchoring of tertiary amine functionality was achieved by grafting with chloro-or iodopropyltriethoxysilane followed by nucleophilic displacement of halidewith piperidine Both materials were active catalysts for the Knoevenagel con-densation of benzaldehyde with ethyl cyanoacetate at 80 C in dimethyl sulfox-ide The primary amine was more active which was explained by invoking a dif-ferent mechanism imine formation with the aldehyde group rather than classi-cal base activation of the methylene group in the case of the tertiary amine
Stronger solid base catalysts can be prepared by grafting guanidine bases tomesoporous silicas For example the functionalization of MCM-41 with 157-triazabicyclo[440]dec-5-ene (TBD) as shown in Fig 240 afforded a material(MCM-TBD) that was an effective catalyst for Michael additions with ethylcya-noacetate or diethylmalonate (Fig 241) [136]
In a variation on this theme a bulky guanidine derivative NNN-tricyclohex-ylguanidine was encapsulated by assembly within the supercages of hydrophobiczeolite Y The resulting lsquoship-in-a-bottlersquo catalyst was active in the aldol reaction of
23 Solid Base Catalysis 83
Fig 240 Methods for attachment of organic bases to micelle templated silicas
acetone with benzaldehyde giving 4-phenyl-4-hydroxybutan-2-one (Fig 242)[138] The catalyst was stable and recyclable but activities were relatively low pre-sumably owing to diffusion restrictions Grafting of the same guanidine ontoMCM-41 afforded a more active catalyst but closer inspection revealed that leach-ing of the base from the surface occurred Similarly diamine functionalizedMCM-41 [139] and a tetraalkylammonium hydroxide functionalized MCM-41[140] were shown to catalyze aldol condensations (Fig 242)
2 Solid Acids and Bases as Catalysts84
Fig 241 Michael reactions catalyzed by MCM-TBD
Fig 242 Aldol reactions catalyzed by various solid bases
24Other Approaches
In Section 21 we discussed the use of solid Broslashnsted acids as recyclable alterna-tives to classical homogeneous Broslashnsted and Lewis acids In the case of Lewisacids alternative strategies for avoiding the problems associated with their usecan be envisaged The need for greener alternatives for conventional Lewis acidssuch as AlCl3 and ZnCl2 derives from the necessity for decomposing the acidndashbase adduct formed between the catalyst and the product This is generallyachieved by adding water to the reaction mixture Unfortunately this also leadsto hydrolysis of the Lewis acid thus prohibiting its re-use and generating aque-ous effluent containing copious amounts of inorganic salts Since the product isoften more basic than the substrate eg in Friedel-Crafts acylations (see earlier)Lewis acid catalyzed processes often require stoichiometric amounts of catalyst
One approach is to incorporate Lewis acids into for example zeolites or me-soporous silicas [141] For example incorporation of Sn(IV) into the frameworkof zeolite beta afforded a heterogeneous water-tolerant Lewis acid [142] Itproved to be an effective catalyst for the intramolecular carbonyl-ene reaction ofcitronellal to isopulegol [143] (Fig 243) in batch or fixed bed operation Hydro-genation of the latter affords menthol (Fig 243)
Another approach is to design homogeneous Lewis acids which are water-compatible For example triflates of Sc Y and lanthanides can be prepared inwater and are resistant to hydrolysis Their use as Lewis acid catalysts in aque-ous media was pioneered by Kobayashi and coworkers [144ndash146] The catalyticactivity is dependent on the hydrolysis constant (Kh) and water exchange rateconstant (WERC) for substitution of inner sphere water ligands of the metal cat-ion [145] Active catalysts were found to have pKh values in the range 4ndash10 Cat-ions having a pKh of less than 4 are easily hydrolyzed while those with a pKh
greater than 10 display only weak Lewis aciditySc(OTf)3 and lanthanide triflates particularly Yb(TOTf)3 have been shown to
catalyze a variety of reactions in aqueousorganic cosolvent mixtures [145 146]For example they catalyze the nitration of aromatics with 69 aqueous nitricacid the only by-product being water [147]
24 Other Approaches 85
Fig 243 Sn-Beta catalyzed carbonyl-ene reaction
The lanthanide triflate remains in the aqueous phase and can be re-used afterconcentration From a green chemistry viewpoint it would be more attractive toperform the reactions in water as the only solvent This was achieved by addingthe surfactant sodium dodecyl sulfate (SDS 20 mol) to the aqueous solutionof eg Sc(OTf)3 (10 mol) [145] A further extension of this concept resulted inthe development of lanthanide salts of dodecyl sulfate so-called Lewis acidndashsur-factant combined catalysts (LASC) which combine the Lewis acidity of the cat-ion with the surfactant properties of the anion [148] These LASCs eg Sc(DS)3exhibited much higher activities in water than in organic solvents They wereshown to catalyze a variety of reactions such as Michael additions and a threecomponent -aminophosphonate synthesis (see Fig 244) in water [145]
Another variation on this theme is the use of a scandium salt of a hydropho-bic polystyrene-supported sulfonic acid (PS-SO3H) as an effective heterogeneousLewis acid catalyst in aqueous media [149]
Ishihara and Yamamoto and coworkers [150] reported the use of 1 mol ofZrOCl2middot8 H2O and HfOCl2middot8 SH2O as water-tolerant reusable homogeneouscatalysts for esterification
Finally it should be noted that Lewis acids and bases can also be used inother non-conventional media as described in Chapter 7 eg fluorous solventssupercritical carbon dioxide and ionic liquids by designing the catalyst eg forsolubility in a fluorous solvent or an ionic liquid to facilitate its recovery and re-use For example the use of the ionic liquid butylmethylimidazolium hydroxide[bmim][OH] as both a catalyst and reaction medium for Michael additions(Fig 245) has been recently reported [151]
2 Solid Acids and Bases as Catalysts86
Fig 244 Sc(DS)3 catalyzed reactions in water
It is clear that there are many possibilities for avoiding the use of classicalacid and base catalysts in a wide variety of chemical reactions Their applicationwill result in the development of more sustainable processes with a substantialreduction in the inorganic waste produced by the chemical industry Particularlynoteworthy in this context is the use of chemically modified expanded cornstarches containing pendant SO3H or NH2 groups as solid acid or base cata-lysts respectively [152] In addition to being recyclable these catalysts are biode-gradable and derived from renewable raw materials (see Chapter 8)
References 87
Fig 245 Michael additions catalyzed by [bmim][OH]
References
1 K Tanabe WF Houmllderich Appl CatalA General 1999 181 399
2 M Harmer in Handbook of Green Chem-istry and Technology J Clark D Macquar-rie (Eds) Blackwell Oxford 2002pp 86ndash119
3 R A Sheldon H van Bekkum (Eds)Fine Chemicals through HeterogeneousCatalysis Wiley-VCH Weinheim 2001
4 W Houmllderich Catal Today 2000 62115
5 A Corma H Garcia Chem Rev 2003103 4307
6 R A Sheldon R S Downing ApplCatal A General 1999 189 163
7 A Mitsutani Catal Today 2002 73 578 M Campanati A Vaccari in Ref [3]
pp 61ndash799 A Vaccari Catal Today 1998 41 53
10 A Vaccari Appl Clay Sci 1999 14 16111 H van Bekkum E M Flanigen
J C Jansen (Eds) Introduction to Zeolite
Science and Practice Elsevier Amster-dam 1991
12 A Corma in Ref [3] pp 80ndash9113 A Corma J Catal 2003 216 29814 A Corma Chem Rev 1995 95 55915 Y Izumi in Ref [3] pp 100ndash10516 MM Sharma React Funct Polym
1995 26 317 A Chakrabarti MM Sharma React
Funct Polym 1993 20 118 W van Rhijn D De Vos PA Jacobs in
Ref [3] pp 106ndash11319 MH Valkenberg W F Houmllderich Catal
Rev 2002 44 (2) 32120 Y Izumi K Urabe M Onaka Zeolite
Clay and Heteropoly Acids in OrganicReactions VCH Weinheim 1992
21 In Ref [20] p 5322 O Sieskind P Albrecht Tetrahedron
Lett 1993 34 119723 A Cornelis P Laszlo SynLett 1994 3
155
2 Solid Acids and Bases as Catalysts88
24 J H Clark A P Kybett D J MacquarrieS J Barlow J Chem Soc Chem Com-mun 1989 1353
25 S J Barlow TW Bastock J H ClarkSR Cullen J Chem Soc Perkin Trans1994 2 411
26 T J Pinnavaia Science 1983 220 459527 F Figueras Catal Rev Sci Eng 1988
30 45728 J Sterte Catal Today 1988 2 21929 SL Suib Chem Rev 1993 93 80330 ST Wilson in Ref [11] pp 137ndash15131 R Szostak in Ref [11] pp 153ndash19932 G T Kokotailo SL Lawton DH Olsen
W M Meijer Nature 1978 272 43733 For a historical account see E M Flani-
gen in Ref [11] pp 31ndash3434 A Corma Chem Rev 1997 97 237335 CT Kresge ME Leonowicz WJ Roth
J C Vartuli JS Beck Nature 1992 359710
36 J S Beck J C Vartuli W J RothME Leonowicz et al J Am ChemSoc 1992 114 10834
37 D Macquarrie in Handbook of GreenChemistry and Technology J Clark DMacquarrie (Eds) Blackwell Oxford2002 pp 120ndash147
38 PB Weisz Pure Appl Chem 1980 522091
39 G R Meima G S Lee JM Garces inRef [3] pp 151ndash160
40 P Meacutetivier in Ref [3] pp 173ndash17741 J A Elings R S Downing R A Sheldon
Stud Surf Sci Catal 1997 105 112542 EA Gunnewegh A J Hoefnagel
R S Downing H van Bekkum ReclTrav Chim Pays-Bas 1996 115 226
43 EA Gunnewegh A J Hoefnagel H vanBekkum J Mol Catal 1995 100 87
44 EA Gunnewegh R S DowningH van Bekkum Stud Surf Sci Catal1995 97 447
45 M Spagnol L Gilbert D Alby inThe Roots of Organic DevelopmentJ R Desmurs S Ratton (Eds) IndChem Lib Vol 8 Elsevier Amsterdam1996 pp 29ndash38 S Ratton Chem Today1997 3ndash4 33
46 P Meacutetivier in Ref [3] pp 161ndash17247 A Vogt A Pfenninger EP0701987A1
1996 to Uetikon AG
48 B Chiche A Finiels C GauthierP Geneste J Graille D Pioch J OrgChem 1986 51 2128
49 A Corma MJ Ciment H GarciaJ Primo Appl Catal 1989 49 109
50 W Houmllderich M Hesse F NaumannAngew Chem 1988 27 226
51 A Finiels A Calmettes P GenesteP Moreau Stud Surf Sci Catal 199378 595 J J Fripiat Y Isaev J Catal1999 182 257
52 A K Pandey AP Singh Catal Lett1997 44 129 R Sreekumar R Padma-kumar Synth Commun 1997 27 777
53 A Kogelbauer HW Kouwenhoven inRef [3] pp 123ndash132
54 P Ratnasamy A P Singh in Ref [3]pp 133ndash150
55 L Bertea HW Kouwenhoven R PrinsAppl Catal A General 1995 129 229
56 K Iwayama S Yamakawa M KatoH Okino Eur Pat Appl EP9489881999 to Toray
57 H Ishida Catal Surveys Jpn 1997 1 24158 W F Houmllderich Stud Surf Sci Catal
1993 75 127 W F Houmllderich inComprehensive Supramolecular ChemistryJ-M Lehn et al (Eds) 1996 Vol 7pp 671ndash692
59 A Chauvel B Delmon WF HoumllderichAppl Catal A 1994 115 173
60 H Ichihashi M Ishida A Shiga M Ki-tamura T Suzuki K Suenobu K SugitaCatal Surveys Asia 2003 7 (4) 261
61 H Ichihashi H Sato Appl Catal AGeneral 2001 221 359 H IchihashiM Kitamura Catal Today 2002 73 23
62 H Sato Catal Rev Sci Eng 1997 39395
63 T Tatsumi in Ref [3] pp 185ndash20464 For a discussion of by-product free
routes to caprolactam see G DahlhoffJ PM Niederer WF Houmllderich CatalRev 2001 43 381
65 G P Heitmann G DahlhoffW F Houmllderich J Catal 1999 186 12
66 M Guisnet G Perot in Ref [3]pp 211ndash216 and references cited therein
67 I Nicolai A Aguilo US 4652683 1987BBG Gupta US 4668826 1987 toHoechst-Celanese
68 A J Hoefnagel H van Bekkum ApplCatal A General 1993 97 87
References 89
69 W F Houmllderich U Barsnick in Ref [3]pp 217ndash231
70 W F Houmllderich J Roumlseler G HeitmanA T Liebens Catal Today 1997 37 353
71 P J Kunkeler J C van der WaalJ Bremmer B J Zuurdeeg R S Down-ing H van Bekkum Catal Lett 199853 135
72 J A Elings HEB LempersR A Sheldon Eur J Org Chem 20001905
73 R A Sheldon J A Elings S K LeeHE B Lempers RS Downing J MolCatal A 1998 134 129
74 A Molnar in Ref [3] pp 232ndash23975 R A Budnik MR Sanders Eur Pat
Appl EP158310 1985 to Union Carbide76 M Hesse W Houmllderich E Gallei Chem
Ing Tech 1991 63 100177 CHMcAteer EFV Scriven in Ref [3]
pp 275ndash28378 CD Chang W H Lang US 4220783
1980 to Mobil Oil Corp79 J Heveling Chimia 1996 50 11480 R S Downing P J Kunkeler in Ref [3]
pp 178ndash183 and references cited therein81 G J Meuzelaar R A Sheldon in Ref
[3] pp 284ndash29482 MA Harmer W E Farneth Q Sun
Adv Mater 2001 221 4583 MA Harmer Q Sun Appl Catal A
General 2001 221 4584 A EW Beers T A Nijhuis F Kapteijn
in Ref [3] pp 116ndash12185 G A Olah PS Iyer G K Prakash
Synthesis 1986 7 51386 MA Harmer W E Farneth Q Sun
J Am Chem Soc 1996 118 770887 MA Harmer Q Sun A J Vega
W E Farneth A Heidekum WF Hoel-derich Green Chem 2000 6 7
88 A Heidekum MA HarmerW F Houmllderich J Catal 1998 176 260
89 S Wieland P Panster in Ref [3]pp 92ndash99
90 MA Harmer Q Sun MJ MichalczykZ Yang Chem Commun 1997 1803
91 D Margolese JA Melero SC Chris-tiansen BF Chmelka G D StuckyChem Mater 2000 12 2448
92 J A Melero G D Stucky R van GriekenG Morales J Mater Chem 2002 121664
93 D Das J F Lee S Cheng ChemCommun 2001 2178
94 I Diaz C Marquez-Alvarez F Mohi-no J Perez-Pariente E Sastre Micro-por Mesopor Mater 2001 44ndash45 295
95 W M van Rhijn DE De Vos BFSels W D Bossaert PA JacobsChem Commun 1998 317 W DBossaert DE De Vos W M vanRhijn J Bullen P J Grobet PA Ja-cobs J Catal 1999 182 156
96 R Richer L Mercier Chem Commun1998 1775
97 J A Melero R van Grieken G Mor-ales V Nuno Catal Commun 20045 131
98 M Alvaro A Corma D Das V For-nes H Garcia Chem Commun 2004956
99 MT Pope Heteropoly and Isopoly Oxo-metalates Springer Berlin 1983
100 N Mizuno M Misono Chem Rev1998 98 199
101 Y Izumi in Ref [3] pp 100ndash105102 For reviews see IV Kozhevnikov
Catal Rev Sci Eng 1995 37 311I V Kozhevnikov Chem Rev 1998 98171 T Okuhara N Mizuno M MisonoAdv Catal 1996 41 113 M MisonoI Ono G Koyano A Aoshima PureAppl Chem 2000 72 1305
103 H Hattori Chem Rev 1995 95 537104 F Cavani F Trifiro A Vaccari Catal
Today 1991 11 173105 BF Sels D E De Vos P A Jacobs
Catal Rev 2001 43 392106 G J Kelly F King M Kett Green
Chem 2002 4 392107 F Figueras J Lopez in Ref [3]
pp 327ndash337108 J C Roelofs A J van Dillen
K P de Jong Catal Today 2000 60297
109 MJ Climent A Corma S IborraJ Primo J Catal 1995 151 60
110 F Figueras D Tichit M BennaniNaciri R Ruiz in Catalysis of OrganicReactions FE Herkes (Ed) MarcelDekker New York 1998 p 37
111 A Corma V Fornes RM Martin-Aranda F Rey J Catal 1992 134 58
112 A Corma R M Martin-Aranda ApplCatal A General 1993 105 271
2 Solid Acids and Bases as Catalysts90
113 A Corma S Iborra J Primo F ReyAppl Catal A General 1994 114 215
114 C Cativiela F Figueras J I GarciaJ A Mayoral M M Zurbano SynthCommun 1995 25 1745
115 K Kaneda K Yamaguchi K MoriT Mizugaki K Ebitani Catal SurveysJapan 2000 4 31 K Kaneda S UenoK Ebitani Curr Top Catal 1997 191
116 C Cativiela F Figueras JM FraileJ I Garcia JA Mayoral TetrahedronLett 1995 36 4125
117 S Ueno K Yamaguchi K YoshidaK Ebitani K Kaneda Chem Com-mun 1998 295
118 K Yamaguchi K Ebitani K KanedaJ Org Chem 1999 64 2966
119 F Winter A J van Dillen KP deJong Chem Commun 2005 3977
120 M Zahouily Y Abrouki B BahlaouanA Rayadh S Sebti Catal Commun2003 4 521
121 A Corma S Iborra in Ref [3]pp 309ndash326
122 R Streekumar P Rugmini R Padma-kumar Tetrahedron Lett 1997 386557
123 Y Ono CATTECH March 1997 31124 K R Kloetstra H van Bekkum Chem
Soc Chem Commun 1995 1005125 PA Hathaway ME Davis J Catal
1989 116 263 and 279126 I Rodriguez H Cambon D Brunel
M Lasperas J Mol Catal A Chemical1998 130 95
127 K R Kloetstra H van Bekkum StudSurf Sci Catal 1997 105 431
128 E Angeletti C Canepa G MartinettiP Venturello Tetrahedron Lett 198818 2261 see also E AngelettiC Canepa G Martinelli P VenturelloJ Chem Soc Perkin Trans 1989 1105
129 M Lasperas T Llorett L ChavesI Rodriguez A Cauvel D BrunelStud Surf Sci Catal 1997 108 75
130 A Cauvel G Renard D BrunelJ Org Chem 1997 62 749
131 D Brunel Micropor Mesopor Mat1999 329
132 DJ Macquarrie D Brunel in Ref [3]pp 338ndash348
133 DJ Macquarrie in Ref [2] pp 120ndash149
134 DB Jackson D J Macquarrie ChemCommun 1997 1781
135 DJ Macquarrie Green Chem 1999 1195
136 YV Subba Rao DE De VosPA Jacobs Angew Chem Int Ed1997 36 2661
137 M Lasperas T Lloret L ChavesI Rodriguez A Cauvel D BrunelStud Surf Sci Catal 1997 108 75
138 R Sercheli A LB Ferreira MCGuerreiro R M Vargas R A SheldonU Schuchardt Tetrahedron Lett 199738 1325
139 BM Choudry M Lakshmi-Kantam PSreekanth T Bandopadhyay F Fig-ueras A Tuel J Mol Catal 1999142 361
140 I Rodriguez S I Iborra A Corma FRey J J Jorda Chem Commun 1999593
141 A Corma H Garcia Chem Rev 2002102 3837 A Corma H Garcia ChemRev 2003 103 4307
142 A Corma LT Nemeth M Renz SValencia Nature 2001 412 423
143 A Corma M Renz Chem Commun2004 550
144 S Kobayashi Chem Lett 1991 2187145 S Kobayashi K Manabe Acc Chem
Res 2002 35 209146 S Kobayashi M Sugiura H Kitagawa
W W L Lam Chem Rev 2002 1022227
147 F J Waller A G M Barrett DC Brad-dock D Ramprasad Chem Commun1997 613
148 S Kobayashi T Wakabayashi Tetrahe-dron Lett 1998 39 5389
149 S Imura K Manabe S KobayashiTetrahedron 2004 60 7673
150 M Nakayama A Sato K Ishihara HYamamoto Adv Synth Catal 2004346 1275
151 BC Ranu S Banerjee Org Lett2005 7 3049
152 S Doi J H Clark D J MacquarrieK Milkowski Chem Commun 20022632
31Introduction
Catalytic hydrogenation ndash using hydrogen gas and heterogeneous catalysts ndash canbe considered as the most important catalytic method in synthetic organicchemistry on both laboratory and production scales Hydrogen is withoutdoubt the cleanest reducing agent and heterogeneous robust catalysts havebeen routinely employed Key advantages of this technique are (i) its broadscope many functional groups can be hydrogenated with high selectivity (ii)high conversions are usually obtained under relatively mild conditions in theliquid phase (iii) the large body of experience with this technique makes it pos-sible to predict the catalyst of choice for a particular problem and (iv) the pro-cess technology is well established and scale-up is therefore usually straightfor-ward The field of hydrogenation is also the area where catalysis was first widelyapplied in the fine chemical industry Standard hydrogenations of olefins andketones and reductive aminations using heterogeneous catalysts have beenroutinely performed for more than two decades [1] These reactions are usuallyfast and catalyst separation is easy Catalysts consist of supported noble metalsRaney nickel and supported Ni or Cu However once enantioselectivity is calledfor homogeneous catalysis and biocatalysis generally become the methods ofchoice The field of homogeneous asymmetric catalysis had a major break-through with the discovery of ligands such as BINAP DIPAMP and DIOP (forstructures see later) designed by the pioneers in this field Noyori Knowles andKagan [2ndash4] These ligands endow rhodium ruthenium and iridium with theunique properties which allow us nowadays to perform enantioselective reduc-tion of a large number of compounds using their homogeneous metal com-plexes Besides homogeneous and heterogeneous catalysis the potential of bio-catalytic reduction is still growing and has already delivered some interestingapplications [5] Reduction of many secondary carbonyl compounds can be per-formed using enzymes as catalysts yielding chiral compounds with high enan-tioselectivities [6] Use of new genetic engineering techniques is rapidly expand-ing the range of substrates to be handled by enzymes The issue of cofactor-re-cycling often denoted as the key problem in the use of biocatalytic reductionsis nowadays mainly a technological issue which can be solved by applying a
91
3Catalytic Reductions
substrate or enzyme coupled approach in combination with novel reactor con-cepts In this chapter all three catalytic methods heterogeneous homogeneousand biocatalytic reductions will be separately described and illustrated with in-dustrial examples Enantioselective hydrogenation applications which aremainly the domain of homogeneous and enzymatic catalysts will constitute amain part of this chapter
32Heterogeneous Reduction Catalysts
321General Properties
The classical hydrogenation catalysts for preparative hydrogenation are sup-ported noble metals Raney nickel and supported Ni and Cu all of which areable to activate hydrogen under mild conditions [1] Because only surface atomsare active the metal is present as very small particles in order to give a highspecific surface area It is generally accepted that the catalytic addition of hydro-gen to an X= Y bond does not occur in a concerted manner but stepwise Inother words the HndashH bond has to be cleaved first giving intermediate MndashHspecies which are then added stepwise to the X= Y bond This is depicted sche-matically in Fig 31 for a metallic surface for the hydrogenation of ethylene [7]The first step is called dissociative adsorption and the newly formed MndashHbonds deliver the energetic driving force for the cleavage of the strong HndashHbond The metal surface also forms complexes with the X= Y most probably viaa -bond thereby activating the second reactant and placing it close to the MndashHfragments allowing the addition to take place There is consensus that the H isadded to the complexed or adsorbed X= Y from the metal side leading to anoverall cis-addition [7] The outcome of a diastereoselective hydrogenation canthus also be rationalized For substrate coordination to the surface preferentialadsorption of the less hindered face will take place preferentially due to repul-sive interactions Furthermore if anchoring groups are present in the moleculesuch as OH sulfide or amine repulsive interactions can be overruled and theopposite stereoisomer will be obtained
It is important to realize that even today it is not possible to adequately char-acterize a preparative heterogeneous catalyst on an atomic level Most researchin heterogeneous hydrogenation took place in the 1970s to 1980s and the re-sults thereof can be found in the pioneering monographs of Rylander [1] Au-gustine [8] and Smith [9] Catalysts are still chosen on an empirical basis bytrial and error and it is rarely understood why a given catalyst is superior to an-other one The factors which influence the reactivity and selectivity are (i) Typeof metal noble metals (Pd Pt Rh Ru) versus base metals (Ni and Cu) Bimetal-lic catalysts are also applied (ii) Type of support charcoal versus aluminas or si-licas (iii) Type of catalyst supported on carrier fine powders Ni as Raney nickel
3 Catalytic Reductions92
and Cu as Cu chromite (iv) Metal loading In a slurry reactor typically 1ndash10loading is employed while in a fixed-bed reactor loadings of 01ndash1mol areused (v) Dispersion crystallite size etc (vi) Modifiers and promoters Classical ex-amples are the use of sulfur phosphorus or nitrogen compounds as partial de-activating agents eg for the selective hydrogenation of halogenated aromaticnitro compounds (see below) (vii) Solvent Commonly employed solvents whichhave a large impact on the final outcome of the reaction are water methanolethanol acetic acid ethyl acetate or methoxyethanol The preferred catalysts fordifferent conversions are shown in Fig 32 Experimental details for a wide vari-ety of conversions can be found in the monographs [1ndash3] mentioned earlier Re-cent progress is highlighted by Blaser and coworkers [10]
The selective semi-hydrogenation of alkynes is an important reaction in thecontext of fine chemicals manufacture The acyetylenic group is used for theformation of new carbonndashcarbon bonds in substitution reactions Selectivehydrogenation to the alkene further enhances its synthetic utility eg in thesynthesis of insect sex pheromones and vitamins [11ndash13] Overall palladium of-fers the best combination of activity and selectivity at reasonable cost and forthese reasons has become the basis of the most successful commercial alkynehydrogenation catalysts to date Because of their inherently high activity thesecatalysts contain typically less than 05 of active metal in order to preserve se-lectivity at high alkyne conversion The best known alkyne semi-hydrogenationcatalyst is that developed by Lindlar which comprises calcium carbonate-sup-ported palladium with Pb and quinoline promoters [14] Selective hydrogena-tion of 1-bromo-11-hexadecyne has been shown to occur in high yield and with-out hydrogenolysis of the carbonndashbromine bond over Lindlarrsquos catalyst treatedwith aromatic amine oxides such as pyridine N-oxide [15] Utilization of lead as
32 Heterogeneous Reduction Catalysts 93
Fig 31 Mechanism of heterogeneous hydrogenation
a promoter has been developed further by formulation of true PdndashPb alloys inthe hydrogenation of 11-hexadecynyl acetate which is an insect pheromone tothe corresponding cis-olefin (Fig 33a) [12] Modification by addition of quino-line is reported to benefit the selective production of cis-vitamin D (Fig 33b)
3 Catalytic Reductions94
Fig 32 Preferred heterogeneous catalysts for different functional group reductions
[16] More examples can be found in a recent monograph by Bailey and King[17]
The selective hydrogenation of cinnamaldehyde to produce cinnamyl alcoholis an important reaction and it represents an often encountered selectivity prob-lem namely the selective hydrogenation of aldehydes in the presence of a car-bonndashcarbon double bond The major application of cinnamyl alcohol is as abase for perfumes and therefore high selectivities and conversions are vital Irand Pt catalysts (Fig 34) seem to give the best results [18 19] Alternatively ahomogeneous catalyst can be applied (see below)
A reaction which deserves extra attention in view of its greenness is the re-duction of carboxylic acid derivatives to the corresponding aldehydes in onestep This is quite difficult to achieve with classical hydrogenation catalysts be-cause the product is in general more easily hydrogenated than the substrateOn a small scale this conversion can be carried out by the Rosenmund reduc-tion of acid chlorides over a palladium catalyst However during high tempera-ture processes using either RuSn catalysts (Rhodia) [20] or ZrO2 or CrO3 (Mit-subishi Chemical Corporation) (Fig 35) [21] stable aldehydes can be produceddirectly from the corresponding acids in good yields Mitsubishi has success-fully commercialized the production of p-tert-butylbenzaldehyde m-phenoxyben-zaldehyde p-methylbenzaldehyde 10-undecanal and dodecanal by reduction ofthe corresponding acids By use of this technology ca 2000 t yndash1 of aldehydehave been manufactured since 1988 [22]
Hydrogenation of aromatic nitro compounds with heterogeneous catalysts isoften the method of choice for the production of the corresponding anilines As
32 Heterogeneous Reduction Catalysts 95
Fig 33 Selective semi-hydrogenation of alkynes to cis-olefins
Fig 34 Selective hydrogenation of cinnamyl alcohol
a general rule commercial heterogeneous catalysts are well suited to the reduc-tion of simple nitroarenes However recent progress has expanded the technol-ogy to the technical reduction of functionalized nitroarenes Until recently onlythe Beacutechamp reduction (stoichiometric Fe) was available for the technical reduc-tion of nitroarenes with additional easily reducible functional groups (eg ha-lide C = C or C= O) The team of Ciba-Geigy developed two new catalytic sys-tems that can perform the selective reduction of a nitroallyl ester as shown inFig 36 [23] In the first process a newly developed PtndashPbndashCaCO3 catalyst wasused In the second process H3PO2 was used as process modifier for a commer-cial PtndashC catalyst In the latter system VO(acac)2 is added to suppress the accu-mulation of hydroxylamines Both catalyst systems have a wide scope for relatedsystems They are able to hydrogenate aromatic nitro compounds containingfunctional groups such as iodide C = C CN and even CC with high yieldand selectivity
The catalytic hydrogenation of nitriles is one of the basic methods to obtainprimary amines Diamines especially are of high industrial importance Manydifferent catalytic systems have been studied and two recent reviews give an ex-cellent overview of this rather scattered area [24 25] Reactions are often carriedout at temperatures up to 100 C and pressures up to 100 bar with Raney nickel(often in combination with Cr Fe or Mo) or Raney cobalt as industrially pre-ferred catalysts Pd and Pt are also suitable catalysts Besides the usually desiredprimary amines condensation of reaction intermediates leads to secondary andtertiary amines Addition of ammonia or less toxic bases such as NaOH andLiOH [26 27] can be used to improve the selectivity for primary amines Forfine chemicals applications functional group tolerance is an important issueThe selective hydrogenation of CN groups in the presence of C = C bonds aparticularly difficult task has recently been studied in the hydrogenation of cin-namonitrile see Fig 37 It is possible to selectively hydrogenate cinnamonitrileto 3-phenylallylamine with selectivities up to 80 in the presence of RaNi orRaCo catalysts in methanolic ammonia solution [28]
3 Catalytic Reductions96
Fig 35 Selective reduction of 10-undecylenic acid to the aldehyde in one step
Fig 36 Chemoselective hydrogenation of a nitroallylester
The field of arene hydrogenation is almost 100 years old The initial work ofSabatier on the interaction of finely divided nickel with ethylene and hydrogengas led to the development of the first active catalyst for the hydrogenation ofbenzene [29] In the last two decades arene hydrogenation has also become im-portant for the area of fine chemistry Traditionally it is accomplished by use ofa Group VIII metal with the rate of hydrogenation depending on the metalused ie Rh gt Ru gt Pt gt Nigt Pd gt Co [1] Hydrogenation of multiply substitutedaromatic rings can lead to the formation of a variety of stereoisomers Hydroge-nation of functionalized arenes usually leads predominantly to the cis-substi-tuted product The nature of carrier type of metal solvent temperature andpressure determine the exact amount of stereochemical induction In Fig 38the use of RuC enables hydrogenation of tri-substituted benzoic acid into thecorresponding cis-product with high stereoselectivity [30]
The partial hydrogenation of an arene to its cyclohexene derivative is difficultto achieve because complete hydrogenation to cyclohexane tends to occur Oftenthe use of a RuC catalyst can solve this problem because Ru is not very effec-tive at hydrogenating olefinic double bonds Alternatively PtC and RhC can beused [31] The Asahi Corporation has developed a benzene-to-cyclohexene pro-cess involving a liquidndashliquid two-phase system (benzenendashwater) with a solidruthenium catalyst dispersed in the aqueous phase The low solubility of cyclo-hexene in water promotes rapid transfer towards the organic phase An 80 000tonsyear plant using this process is in operation [32] Another way to scavengethe intermediate cyclohexene is to support the metal hydrogenation catalysts onan acidic carrier (eg silicandashalumina) On such a bifunctional catalyst the cyclo-hexene enters the catalytic alkylation of benzene to yield cyclohexylbenzene [33]The latter can be converted with high selectivity by oxidation and rearrange-ment reactions into phenol and cyclohexanone [34] The complete reaction cycleis shown in Fig 39
32 Heterogeneous Reduction Catalysts 97
Fig 37 Selective cinnamonitrile hydrogenation to 3-phenylallylamine
Fig 38 Selective hydrogenation of a tri-substituted aromatic ring
Another example of catalytic hydrogenation which demonstrates the flexibil-ity of this method is the hydrogenation of nitrogen-containing aromatic ringsystems For example isoquinoline ring saturation can be directed towardseither or both of the two rings (Fig 310) When a platinum catalyst was usedin acetic acid the hydrogenation of isoquinoline results in saturation of the ni-trogen-containing aromatic ring Changing the solvent to methanolic hydrogenchloride results in hydrogenation of the other aromatic ring and use of ethanolin combination with sulfuric acid results in saturation of both aromatic ringsUnder the latter reaction conditions especially when using Ru catalysts the cis-product is formed preferentially [32]
Additional reactions which need to be highlighted are the reductive alkylationof alcohols and amines with aldehydes leading to the green synthesis of ethersand amines These reactions are generally catalyzed by palladium [35] This re-action can replace the classical Williamsonrsquos synthesis of ethers which requiresan alcohol and an alkyl halide together with a base and always results in theconcomitant production of salt The choice of PdC as catalyst is due to the lowefficiency of this metal for the competitive carbonyl reduction Analysis of the
3 Catalytic Reductions98
Fig 39 Partial hydrogenation of benzene and production of phenol
Fig 310 Influence of solvents on the PtC catalyzed selective hydrogenation of isoquinoline
supposed reaction mechanism indicates that the first step of the reaction is theformation of the hemiketal which is favored by the use of one of the reactants(the alcohol or the aldehyde) as solvent (Fig 311) After hydrogenolysis underH2 pressure ethers are produced in high yields after simple filtration of the cat-alyst and evaporation of the solvent
In reductive amination the alkylation is performed under hydrogen in thepresence of a catalyst and an aldehyde or ketone as the alkylating agent Themethod was developed for anilines and extended to amide N-alkylation [36] Anotable example is the use of nitro derivatives as aniline precursors in a one-potreduction of the nitro group and subsequent reductive alkylation of the result-ing aniline (Fig 312)
N- and O-benzyl groups are among the most useful protective groups in syn-thetic organic chemistry and the method of choice for their removal is catalytichydrogenolysis [37] Recently the most important reaction conditions were iden-tified [38] Usually 5ndash20 PdC the best solvents are alcoholic solvents or aceticacid acids promote debenzylation whereas amines can both promote and hin-der hydrogenolysis Chemoselectivity can mainly be influenced by modifyingthe classical PdC catalysts
32 Heterogeneous Reduction Catalysts 99
Fig 311 Catalytic alternative to the Williamsonrsquos synthesis of ethers
Fig 312 Reductive amination of nitro derivatives leading tonon-natural amino acid derivatives
322Transfer Hydrogenation Using Heterogeneous Catalysts
On a small scale it can be advantageous to perform a transfer hydrogenation inwhich an alcohol such as isopropanol serves as hydrogen donor The advantageof this technique is that no pressure equipment is needed to handle hydrogen andthat the reactions can be performed under mild conditions without the risk of re-ducing other functional groups The so-called Meerwein-Ponndorf-Verley (MPV)reduction of aldehydes and ketones is a hydrogen-transfer reaction using easilyoxidizable alcohols as reducing agents Industrial applications of the MPV-reac-tions are found in the fragrance and pharmaceutical industries MPV reactionsare usually performed by metal alkoxides such as Al(O-iPr)3 The activity of thesecatalysts is related to their Lewis-acidic character in combination with ligand ex-changeability Naturally a heterogeneous catalyst would offer the advantage ofeasy separation from the liquid reaction mixture Many examples of heteroge-neously catalyzed MPV reactions have now been reported [39] The catalysts com-prise (modified) metal oxides which have either Lewis acid or base properties Themechanism involves the formation of an alkoxide species in the first step and inthe second step a cyclic six-membered transition state (see Fig 313) Examples arethe use of alumina ZrO2 and immobilized zirconium complexes magnesium oxi-des and phosphates and MgndashAl hydrotalcites
Especially worth mentioning in a green context is the use of mesoporous ma-terials and zeolites as stable and recyclable catalysts for MPV reductions Highactivity was obtained by using zeolite-beta catalysts Beta zeolites have a largepore three-dimensional structure with pores of size 7664 Aring2 which makesthem suitable for a large range of substrates Al Ti- and Sn-beta zeolite have allbeen used as catalysts for the selective reduction of cyclohexanones [40ndash42] The
3 Catalytic Reductions100
Fig 313 Mechanism of MPV reduction catalyzed by Al-beta zeolite
Fig 314 MPV reductions catalyzed by Sn- and Al-zeolite beta
reaction is shown in Fig 314 In terms of both activity and selectivity Sn-beta(containing 2 SnO2) seems to be superior This can be ascribed to the interac-tion of the carbonyl group with the Sn-center which is stronger than with Tiand more selective than with Al-centers [42] Additionally shape-selectivity ef-fects can be observed for all three zeolites When using 4-tert-butylcyclohexa-none as the substrate the selectivity for the cis-isomer easily reaches 99 Thisis clear proof that the reaction occurs within the pores of the zeolite and thatthe active tin centers are not at the external surface of the zeolite or in solution
323Chiral Heterogeneous Reduction Catalysts
Despite the fact that enantioselective hydrogenation is largely the domain of homo-geneous catalysts some classical examples of heterogeneous reduction catalystsneed to be mentioned In this case the metal surface is modified by a (natural) chir-al additive The first successful attempts were published about 60 years ago anddespite a large effort in this field only three examples have shown success theRaney nickel system for -functionalized ketones Pt catalysts modified withcinchona alkaloids for -functionalized ketones and Pd catalysts modified withcinchona alkaloids for selected activated C = C bonds [43 44] The Raney-Nindashtar-taric acidndashNaBr catalyst system known as the Izumi system [45] affords goodto high enantioselectivity in the hydrogenation of -functionalized ketones and rea-sonable results have also been obtained for unfunctionalized ketones Besides Ra-ney nickel Ni powder and supported nickel are almost as good precursors In theoptimized preparation procedure RaNi undergoes ultrasonication in water fol-lowed by modification with tartaric acid and NaBr at 100 C and pH 32 The mod-ification procedure is highly corrosive and produces large amounts of nickel- andbromide-containing waste This together with its low activity (typical reaction timeis 48 h) hampers its industrial application Examples are given in Fig 315 [43]
For the hydrogenation of -functionalized ketones the Pt on alumina systemmodified with cinchonidine or its simple derivative 1011-dihydro-O-methyl-cinchonidine is the best catalyst [43 44 46] This so-called Orito system [47] is
32 Heterogeneous Reduction Catalysts 101
Fig 315 Best results for the enantioselective hydrogenationof -functionalized ketones and non-functionalized ketonesusing the Izumi system
most well known for the hydrogenation of -ketoesters Acetic acid or toluene assolvent close to ambient temperature and medium to high pressure (10ndash70 bar)are sufficient to ensure high enantioselectivities of 95 to 975 (see Fig 316)The highest ee has been obtained after reductive heat treatment of PtAl2O3 andsubsequent sonochemical pretreatment at room temperature [48] In recentyears the substrate range of cinchona-modified Pt has been extended to the hy-drogenation of selected activated ketones including ketopantolactone -ketoacids linear and cyclic -keto amides -keto acetals and trifluoroacetophenone[43 44] Examples are shown in Fig 316
Up to 72 ee has been achieved in the hydrogenation of a diphenyl-substitutedreactant (trans)--phenylcinnamic acid with a PdTiO2 catalyst and cinchonidineat 1 bar in strongly polar solvent mixtures [49] For aliphatic -unsaturated acidsthe enantioselectivities that can be attained are much lower Therefore for thesetype of substrates homogeneous metal-catalysts are preferred
Another approach towards asymmetric heterogeneous catalysts is the immobi-lization of chiral homogeneous complexes via different methods In this waythe advantages of homogeneous catalysts (high activity and selectivity) and het-erogeneous catalysts (easy recovery) can be combined For a complete overviewof this active research field the reader is referred to several reviews on this topic[50 51] The practical applicability of these catalysts is hampered by the fact thatsevere demands of recyclability and stability need to be obeyed In certain casespromising results have been obtained as outlined here
1 The use of solid and soluble catalysts with covalently attached ligandsThe covalent anchoring of ligands to the surface or to a polymer is a conven-tional approach which often requires extensive modification of the already ex-pensive ligands The advantage is that most catalysts can be heterogenized bythis approach and various supports can be used An illustrative example is theuse of the BINAP ligand that has been functionalized using several different
3 Catalytic Reductions102
Fig 316 The Ptcinchona alkaloid system for the enantio-selective hydrogenation of -functionalized ketones
methods followed by attachment to supports such as polystyrene (see Fig 317)[52] or polyethyleneglycol [53] Alternatively it was rendered insoluble by oligo-merization [54] or co-polymerized with a chiral monomer [55] The resulting cat-alysts have catalytic performances that are comparable to their soluble analogsThe latter soluble catalyst (see Fig 317) achieved even better activities than theparent Ru-BINAP which was attributed to a cooperative effect of the polymericbackbone Alternatively the ligand can be covalently attached to a ldquosmartrdquo poly-mer which is soluble at the reaction temperature and which precipitates by cool-ing or heating the reaction mixture (see Chapter 7) In this way the reactioncan be conducted homogeneously under optimum mass transport conditionsand phase separation can be induced by changing the temperature [56]
2 Catalysts immobilized on support via ionic interactionThis is an attractive method since it does not require the functionalization ofthe ligand Augustine et al [57] developed heteropolyacids (HPA) notably phos-photungstates as a ldquomagic gluerdquo to attach cationic Rh and Ru complexes to var-ious surfaces The interaction of the heteropolyacid is thought to occur directly
32 Heterogeneous Reduction Catalysts 103
Fig 317 Heterogenization of Ru-BINAP catalysts by covalentmodification according to Refs [52 55]
with the metal ion The most promising catalyst seems to be Rh-DIPAMP (forstructure of ligand see Fig 323 below) attached to HPA-clay due to the highstability of the DIPAMP ligand This catalyst hydrogenated methyl acetami-doacrylic acid (MAA) with 97 ee (TON 270 TOF up to 400 hndash1) Recently amesoporous Al-containing material was used to attach various cationic chiralrhodium complexes to its anionic surface In this way a stable material was ob-tained which showed excellent recyclability over five cycles and which couldeven be applied in water [58] Best results were obtained by using Rh-monophos(see Fig 318)
3 Catalysts entrapped or occluded in polymer matricesWhile the entrapment in rigid matrices such as zeolites usually leads to a signifi-cant rate decrease the occlusion in polyvinylalcohol (PVA) or polydimethylsilane(PDMS) looks more promising but is still far from being practically useful Leach-ing of the metal complex is often observed in solvents which swell the organic ma-trix Rh-DUPHOS (see Fig 323 below) was occluded in PVA or PDMS and wasapplied for the hydrogenation of methyl acetamidoacrylic acid Activities and selec-tivities in this case (TON 140 TOF ca 15 hndash1 ee 96) [59] were significantly lowerthan for the homogeneous complex (ee 99 TOF 480 hndash1)
33Homogeneous Reduction Catalysts
331Wilkinson Catalyst
In 1965 Wilkinson invented the rhodium-tris(triphenylphosphine) catalyst as ahydrogenation catalyst [60] It still forms the basis for many of the chiral hydro-genations performed today The most effective homogeneous hydrogenation cat-alysts are complexes consisting of a central metal ion one or more (chiral) li-gands and anions which are able to activate molecular hydrogen and to add thetwo H atoms to an acceptor substrate Experience has shown that low-valent Ru
3 Catalytic Reductions104
Fig 318 Immobilization through ionic interaction Rh-Mono-phos on mesoporous Al-TUD1
Rh and Ir complexes stabilized by tertiary (chiral) phosphorus ligands are themost active and the most versatile catalysts Although standard hydrogenationsof olefins ketones and reductive aminations are best performed using heteroge-neous catalysts (see above) homogeneous catalysis becomes the method ofchoice once selectivity is called for An example is the chemoselective hydroge-nation of -unsaturated aldehydes which is a severe test for the selectivity ofcatalysts
The use of a tris(triphenyl) ruthenium catalyst resulted in a high selectivity tothe desired unsaturated alcohol ndash prenol ndash in the hydrogenation of 3-methyl-2-buten-1-al (Fig 319) [61] Thus the double C = C bond stays intact while the al-dehyde group is hydrogenated The latter product is an intermediate for the pro-duction of citral In this case RuCl3 was used in combination with water-solubletris-sulfonated triphenylphosphine (TPPTS) ligands and in this way the wholereaction could be carried out in a two-phase aqueousorganic system (see Chap-ter 7) This allowed easy recycling of the catalyst by phase separation [61] Thecatalytic cycle for the Wilkinson catalyst according to Halpern is depicted inFig 320 [62]
The catalytic cycle starts with the dissociation of one ligand P which is re-placed eg by a solvent molecule An oxidative addition reaction of dihydrogen
33 Homogeneous Reduction Catalysts 105
Fig 319 Chemoselective hydrogena-tion of 3-methyl-2-buten-1-al
Fig 320 Catalytic cycle of Wilkinson catalyst
then takes place This occurs in a cis fashion and can be promoted by the sub-stitution of more electron-rich phosphines on the rhodium complex The nextstep is the migration of hydride forming the alkyl group Reductive eliminationof alkane completes the cycle Obviously the rate of this step can be increasedby using electron-withdrawing ligands The function of the ligand besides influ-encing the electronic properties of the metal is to determine the geometryaround the metal core This forms the basis for the enantioselective propertiesof these catalysts (see below)
332Chiral Homogeneous Hydrogenation Catalysts and Reductionof the C= C Double Bond
The foundation for the development of catalysts for asymmetric hydrogenationwas the concept of replacing the triphenylphosphane ligand of the Wilkinson cat-alyst with a chiral ligand This was demonstrated in the work of the early pioneersHorner [63] and Knowles [64] With these new catalysts it turned out to be possi-ble to hydrogenate prochiral olefins Important breakthroughs were provided bythe respective contributions of Kagan and Dang [65] and the Monsanto groupheaded by Knowles [66] Chelating chiral phosphorus atoms played a central rolein this selectivity and this culminated in the development of the PAMP and laterits corresponding dimer the bidentate DIPAMP ligand [67] The DIPAMP ligandled to high enantioselectivities in the rhodium catalyzed hydrogenation of pro-tected dehydroaminoacids On an industrial scale this catalyst is used for the mul-ti-ton scale production of the anti-Parkinson drug L-DOPA [68] (Fig 321)
It must be noted that the enantioselectivity reached by the catalyst does nothave to be absolute for industrial production In this case 100 enantioselectiv-ity of the product was obtained by crystallization In the past Selke in the for-mer GDR independently developed a sugar based bis-phosphinite as a ligandwhich formed the basis for the L-DOPA process by the company VEB-Isis [69
3 Catalytic Reductions106
Fig 321 Monsantorsquos L-DOPA process
70] see Fig 322 The process was introduced in 1985 and it ended in 1990 oneyear after the collapse of the socialist system
A breakthrough in ligand design was achieved by the work of Kagan whodemonstrated that phosphorus ligands with chirality solely in the backbonewhich are much easier to synthesize led to even better enantioselectivities [4]This was the beginning in the 1990s of a still-ongoing period in which manynew bisphosphines were invented and tested in a variety of enantioselective hy-drogenations [71] Selected examples of chiral bisphosphine ligands have beencollected in Fig 323
Ligands based on ferrocenes have been developed extensively by Hayashi Tog-ni and the Ciba-Geigy catalysis group (now operating as part of Solvias AG)[72] An example is found in Lonzarsquos new biotin process (Fig 324) in which Rhcatalyzed hydrogenation of the olefinic double bond of the substrate takes placewith 99 de [73 74] Another example of the use of this class of ferrocene-de-rived ligands is the use of Josiphos ligand with Ru for the production of (+) cis-methyl dihydrojasmonate (Fig 325) [75]
Especially worth mentioning is the use of bis-phospholane DUPHOS as a li-gand [76] A wide variety of substrates notably enamides vinylacetic acid deriva-tives and enol acetates can be reduced with high enantioselectivities A recentapplication is the rhodium catalyzed enantioselective hydrogenation of the -unsaturated carboxylic ester in Fig 326 which is an intermediate for PfizerrsquosCandoxatril a new drug for the treatment of hypertension and congestive heartfailure [77] Other examples are the diastereoselective hydrogenation leading toPharmacia amp Upjohnrsquos Tipranavir [78] (Fig 327) an HIV protease inhibitor andthe manufacture of -amino acid derivatives [79] Both processes were developedby Chirotech (now part of Dow) For the production of -amino acids the exam-ple of N-Boc-(S)-3-fluorophenylalanine is given in Fig 328 However many deri-vatives have been produced using the same methodology It is noteworthy thatthe use of Rh-MeDUPHOS catalysts is accompanied by using a biocatalytic de-protection of the resulting amide using acylase enzymes (see Fig 328)
One of the drawbacks of the use of bisphosphines is the elaborate synthesesnecessary for their preparation Many efforts have been directed towards the de-velopment of bis-phosphonites and bis-phosphites However surprisingly mono-dentate phosphinates phosphates and phosphoramidates recently emerged aseffective alternatives for bidentate phosphines (Fig 329) This constitutes animportant breakthrough in this area as these can be synthesized in one or twosteps and the cost of these ligands is an order of magnitude lower Monophoscan be made in a single step from BINOL and HMPT
33 Homogeneous Reduction Catalysts 107
Fig 322 ldquoSelkersquosrdquo ligand for the productionof L-DOPA
All of the above examples involve an extra coordinating group such as ena-mide acid or ester in the substrate This is necessary for optimum coordinationto the metal Asymmetric hydrogenation of olefins without functional groups isan emerging area [80]
3 Catalytic Reductions108
Fig 323 Selected examples of chiral ligands used in homogeneous hydrogenation catalysts
Fig 324 Lonzarsquos biotin process using Rh-Xyliphos-type ligands
According to the mechanism of the enantioselective reduction a concept hasbeen evolved termed the ldquoquadrant rulerdquo [81 82] This model addresses howthe chiral ligand influences the preferential addition of hydrogen either to there- or si-face of a C = X bond As visualized in Fig 330 upon coordination ofthe ligands to the metal atom the substituents are oriented in such a way that
33 Homogeneous Reduction Catalysts 109
Fig 325 Production of (+) cis-methyl dihydrojasmonate usingRu-Josiphos catalyzed hydrogenation
Fig 326 Rh-MeDUPHOS catalyzed hydrogenation in the production of Candoxatril
Fig 327 Rh-MeDUPHOS for production of Tipranavir
3 Catalytic Reductions110
Fig 328 Production of N-Boc-(S)-3-fluorophenylalanine usingChirotechrsquos Rh-MeDUPHOS technology
Fig 329 Use of monodentate ligands for the reduction of prochiral olefins
Fig 330 The quadrant model used to predict enantioselectiv-ity in homogeneous hydrogenation
a chiral array is formed where two diagonal quadrants are blocked by bulky sub-stituents The situation is visualized for DIOP a diphosphine with two PAr2
moieties attached to a flexible chiral backbone When the substrate coordinatesto the metal atom it will orient in such a way that steric repulsion is minimalIn many cases this simple model is able to predict the sense of inductionHowever it will not be able to predict more complex situations [83]
333Chiral Homogeneous Catalysts and Ketone Hydrogenation
Enantiopure alcohols can be produced using chiral hydrogenation catalysts forthe reduction of ketones A major breakthrough in this area was achieved in themid-1980s by Takaya and Noyori following the initial work of Ikariyarsquos group[84] on the development of the BINAP ligand for Ru-catalyzed hydrogenations[85] The ruthenium-BINAP ligand is famous for its broad reaction scope manydifferent classes of ketones can be hydrogenated with very high enantioselectiv-ities BINAP is a chiral atropisomeric ligand and its demanding synthesis hasbeen optimized [86] The Japanese company Takasago has commercialized var-ious Ru-BINAP processes [87] Drawbacks of the Ru-BINAP procedure are therelatively high pressures and temperatures in combination with long reactiontimes This can be circumvented by adding small amounts of strong acids [88]or turning to Rh-DUPHOS type complexes Furthermore unlike rhodium com-plexes most ruthenium bisphosphines have to be preformed for catalysis
An example of the hydrogenation of a -ketoester is the dynamic kinetic reso-lution of racemic 2-substituted acetoacetates [89] In this process one of the twoenantiomeric acetoacetates is hydrogenated with very high diastereoselectivepreference and in high enantioselectivity At the same time the undesired acet-oacetate undergoes a continuous racemization This has found application inthe hydrogenation of the intermediate for the carbapenem antibiotic intermedi-ate Imipenem on a scale of 120 tonyear [90] The reaction is shown inFig 331 Ru-BINAP is also suitable for the enantioselective hydrogenation of -substituted ketones In Fig 332 the reduction of acetol leading to the (R)-12-propane-diol is denoted This diol is an intermediate for the antibiotic Levofloxa-cin [87 90]
33 Homogeneous Reduction Catalysts 111
Fig 331 Hydrogenation of a -ketoester for the production of Imipenem
Another breakthrough was made by Noyori for the enantioselective hydroge-nation of aromatic ketones by introducing a new class of Ru-BINAP (diamine)complexes [91] In this case hydrogen transfer is facilitated by ligand assistanceThe company Takasago used this catalyst for the production of (R)-1-phenyletha-nol in 99 ee using only 4 bar of hydrogen [86] (see Fig 333) (R)-1-phenyletha-nol as its acetate ester is sold as a fragrance and has a floral fresh green note
3 Catalytic Reductions112
Fig 332 Enantioselective hydrogenation of acetol intermediate for Levofloxacin
Fig 333 Bifunctional Ru-BINAP(diamine) complexes for en-antioselective hydrogenation of simple ketones
There is consensus that the transfer of the two H atoms occurs in a concertedmanner as depicted in Fig 333 [91ndash94] This hypothesis explains the need foran NndashH moiety in the ligand
334Imine Hydrogenation
The asymmetric hydrogenation of imines is an important application because itgives access to enantiopure amines For a long period the development of asym-metric imine hydrogenation lagged behind the impressive progress made inasymmetric olefin and ketone hydrogenation [95 96] It was difficult to achievegood results both in terms of rate and selectivity The best results were obtainedwith rhodium and bisphosphines However rhodium-based catalysts required70 bar of hydrogen which hampered their industrial application The largestasymmetric catalytic process nowadays however involves imine hydrogenationas the key step (see Fig 334) Ciba-Geigy (now Syngenta) produces the herbi-cide (S)-metolachlor on a scale of 10000 tonyear The use of iridium instead ofrhodium finally resulted in the required activity TOFs with this catalyst are inexcess of 100000 hndash1 and TONs of more than 1106 were reached [97] As a li-gand xyliphos a ferrocenyl-type bisphosphine was used in combination with io-dide and acetic acid as promoters The enantioselectivity for this process is ca80 which can be easily increased by lowering the substratecatalyst ratioHowever this is not necessary as 80 ee is sufficient Compared to the firstgeneration process which produced racemic metolachlor an environmental bur-den reduction of 89 could be realized
33 Homogeneous Reduction Catalysts 113
Fig 334 Ir-Xyliphos based process for the production of (S)-metolachlor
335Transfer Hydrogenation using Homogeneous Catalysts
For small scale production the use of hydrogen at elevated pressure imposespractical problems related to reactor design and safety issues An attractive alter-native is the use of alcohols or formate as a reductant (see also below for bioca-talytic reductions) The MeerweinndashPonndorfndashVerley (MPV) reaction has alreadybeen mentioned above and is traditionally performed using stoichiometricamounts of aluminim salts or zeolites [98] In particular for enantioselectivetransformations a wide variety of Ru- Rh- and Ir-based homogeneous catalystsare now known and the technique of transfer hydrogenation seems to find ap-plication in industry [99ndash101] Whereas complexes containing chiral phosphineligands are the catalysts of choice for hydrogenation reactions with H2 Ru Rhand Ir complexes with chiral NN or NO ligands have been shown to be very ef-fective for asymmetric transfer hydrogenations (Fig 335) These complexes arenot able to activate molecular hydrogen Especially in the case of aryl ketonesand ketimines transfer hydrogenation can be potentially interesting becausethe ruthenium hydrogenation technology in this case is limited by mediumTONs and TOFs [10]
A plethora of ligands has been reported in the literature but the most effectiveones are 12-amino alcohols monotosylated diamines and selected phosphine-oxazoline ligands The active structures of the complexes reported are half-sand-
3 Catalytic Reductions114
Fig 335 Structure of the most effective Ru and Rhprecursors used in transfer hydrogenations
wich -complexes Ru-arene and Rh (or Ir)-cyclopentadiene complexes (seeFig 335) [10] The introduction of these catalysts in 1995 by Noyori [100] was abreakthrough because it led to a great improvement in terms of both reactionrate and enantioselectivity For a discussion of the bifunctional mechanism oper-ating in this case see the discussion above and Ref [94] These catalysts havebeen developed with acetophenone as model substrate However many functio-nalized acetophenones aryl ketones acetylenic ketones as well as cyclic aryl ke-tones give very good results Imine reduction can also be performed highly effi-ciently using this technique An example is shown in Fig 336 where a TOF of1000 hndash1 was reached [102]
Furthermore Avecia has developed the Rh-cyclopentadienyl complexes inFig 336 for the large scale production of 1-tetralol and substituted 1-phenyl-ethanol [102] The challenge in this area is to increase the activity of the catalystRecently Andersson and co-workers reported an azanorbornane-based ligandwhich can reach a TOF up to 3680 hndash1 for acetophenone hydrogenation (see
33 Homogeneous Reduction Catalysts 115
Fig 336 Transfer hydrogenation of imine as developed by Avecia
Fig 337 Azanorbornane-based ligands form complexes withRu which are the most effective complexes reported today fortransfer hydrogenation
Fig 337) [103] The combined introduction of a dioxolane in the backbone anda methyl group in the -position to the OH group proved essential to reach thisactivity The ligand without these functionalities resulted in 10 times lowerTOFs
34Biocatalytic Reductions
341Introduction
Oxidoreductases play a central role in the metabolism and energy conversion ofliving cells About 25 of the presently known enzymes are oxido reductases[104] The classification of oxidoreductases is presented in Fig 338 The groupsof oxidases monooxygenases and peroxidases ndash dealing with oxidations ndash willbe described in Chapter 4
For industrial applications the group of alcohol dehydrogenases otherwiseknown as carbonyl-reductases is of prime interest The natural substrates of theenzymes are alcohols such as ethanol lactate glycerol etc and the correspond-ing carbonyl compounds However unnatural ketones can also be reduced en-antioselectively In this way chiral alcohols hydroxy acids and their esters oramino acids respectively can be easily generated An excellent overview of thisfield up to 2004 can be found in Refs [105ndash108] The advantages of biocatalyticreductions are that the reactions can be performed under mild conditions lead-ing to excellent enantioselectivities A vast reservoir of wild-type microorganismshas been screened for new enzymes and tested with numerous substrates Anumber of alcohol dehydrogenases are commercially available These includebakerrsquos yeast and the alcohol dehydrogenases from Bakerrsquos yeast Thermoanaero-bium brockii horse liver and the hydroxysteroid dehydrogenase from Pseudome-nas testosterone and Bacillus spherisus [105 106] Table 31 gives a selection of wellknown alcohol dehydrogenases Genetic engineering tools can be applied to
3 Catalytic Reductions116
Fig 338 Classification of oxidoreductases
make enzymes available in larger quantities and at lower costs in recombinanthosts Furthermore by directed evolution tailor-made catalysts can be gener-ated The scientific knowledge in this field is increasing rapidly and in the fu-ture more tailor-made enzymes will be used in industrial processes [109 110]
The vast majority of alcohol dehydrogenases require nicotanimide cofactorssuch as nicotinamide adenine dinucleotide (NADH) and its respective phos-phate NADPH The structure of NADNADP is shown in Fig 339 Hydrogenand two electrons are transferred from the reduced nicotinamide to the carbonylgroup to effect a reduction of the substrate (see Fig 339)
The mechanism of horse liver dehydrogenase has been described in great de-tail In this case the alcohol is coordinated by a Zn ion and Serine Both the al-cohol and the cofactor are held in position via a three-point attachment and effi-cient hydrogen transfer takes place [111 112] The alcohol dehydrogenases canbe used to reduce a variety of ketones to alcohols with high enantioselectivityunder mild conditions In Fig 340 a number of examples is shown using Lacto-bacillus kefir [113] During the course of the reaction the enzyme delivers thehydride preferentially either from the si or the re-side of the ketone to give for
34 Biocatalytic Reductions 117
Table 31 Examples of commonly used alcohol dehydrogenases
Dehydrogenase Specificity Cofactor
Yeast-ADH Prelog NADHHorse liver-ADH Prelog NADHThermoanaerobium brockii-ADH Prelog NADPHHydroxysteroid-DH Prelog NADHCandida parapsilosis Prelog NADHRhodococcus erythropolis Prelog NADHLactobacillus kefir-ADH Anti-Prelog NADPHMucor javanicus-ADHa) Anti-Prelog NADPHPseudomenas sp-ADHa) Anti-Prelog NADH
a) Not commercially available
Fig 339 Mechanism of biocatalytic ketone reduction
simple systems the (R)- or (S)-alcohols respectively For most cases the stereo-chemical course of the reaction which is mainly dependent on the steric re-quirements of the substrate may be predicted from a simple model which isgenerally referred to as the ldquoPrelogrdquo rule [106 114] As shown in Fig 340 Lac-tobacillus kefir leads to anti-Prelog selectivity Obviously the enzymatic reductionis most efficient when the prochiral center is adjoined by small and largegroups on either side (Fig 340)
The cofactors are relatively unstable molecules and expensive if used in stoi-chiometric amounts In addition they cannot be substituted by less expensivesimple molecules Since it is only the oxidation state of the cofactor whichchanges during the reaction it may be regenerated in situ by using a second re-dox reaction to allow it to re-enter the reaction cycle Thus the expensive cofac-tor is needed only in catalytic amounts leading to a drastic reduction in costs[115] Much research effort in the field of alcohol dehydrogenases is thereforedirected towards cofactor recycling (see below) Cofactor recycling is no problemwhen whole microbial cells are used as biocatalysts for redox reactions Manyexamples have been described using ldquofermenting yeastrdquo as a reducing agent[116] In this case cheap sources of redox equivalents such as carbohydratescan be used since the microorganism possesses all the enzymes and cofactorswhich are required for the metabolism In Fig 341 an example of the produc-tion of a pharmaceutically relevant prochiral ketone is given using fermentationtechnology [117]
However from the standpoint of green chemistry the use of isolated enzymes(or dead whole cells) is highly preferred because it avoids the generation of co-pious amounts of biomass It must be emphasized that the productivity of mi-crobial conversions is usually low since non-natural substrates are only toler-ated at concentrations as low as 01ndash03 [106] The large amount of biomasspresent in the reaction medium causes low overall yields and makes product re-covery troublesome Therefore the E-factors for whole cell processes can be ex-tremely high Moreover the use of wild-type cells often causes problems becausean array of enzymes is present which can interfere in the reduction of a specificketone (giving opposite selectivities) The use of recombinant techniques how-ever which only express the desired enzyme can overcome this problem [108]
3 Catalytic Reductions118
Fig 340 Examples of ketone reduction and the Prelog rule
Much higher productivities can be obtained using isolated enzymes or cell ex-tracts [118] This approach is therefore highly preferred Because of the impor-tance of whole cell technology for biocatalytic reduction a few examples will begiven However the main part of this chapter will be devoted to industrial exam-ples of bioreduction involving isolated enzymes and cofactor recycling
342Enzyme Technology in Biocatalytic Reduction
To keep the amount of biomass involved to a minimum the use of isolated en-zymes or cell extracts is highly preferable In this case for their efficient recy-cling two strategies are feasible [106] These are depicted in Fig 342 In thefirst case the substrate-coupled approach only one enzyme is needed and addi-tional alcohol is needed to complete the reduction In terms of overall reactionthese coupled substrate-systems bear a strong resemblance to transition-metaltransfer hydrogenation the so-called Meerwein-Ponndorf-Verley reaction seeabove In the second approach [106ndash108] a large variety of reducing agents canbe used such as formate glucose H2 or phosphite in combination with a sec-ond enzyme namely formate dehydrogenase glucose dehydrogenase hydroge-nase [119] or phosphite dehydrogenase [120] respectively Industrial processes(see below) commonly use glucose or formate as coreductants
In the first approach one enzyme is needed to convert both substrate (ke-tone) and co-substrate (alcohol) The second alcohol needs to afford a ketonewhich can be easily removed by distillation eg acetone to drive the reductionto completion For most alcohol-dehydrogenases however the enzyme can only
34 Biocatalytic Reductions 119
Fig 341 Whole cell technology for biocatalytic reduction example adapted from Ref [117]
tolerate certain levels of alcohols and aldehydes and therefore these coupled-sub-strate systems are commonly impeded by cosubstrate-inhibition [121] Engineer-ing solutions performed by Liese and coworkers were found to address thisproblem in situ product removal accompanied by constant addition of reducingalcohol can improve the yields using isopropanol as the reductant
To push the productivity limits of coupled-substrate systems even further themaximum tolerable concentration of isopropanol applied for cofactor-regenera-tion with different alcohol dehydrogenases (as isolated enzymes or in prepara-tions) has been constantly increased in the period 2000ndash2002 by using evenmore chemostable enzyme preparations [108] In general bacterial alcohol dehy-drogenases dominate the stability ranking and the best results up till now werereached using Rhodococcus ruber DSM 44541 [122] Elevated concentrations ofisopropanol up to 50 (vv) using whole cells not only shift the equilibriumtoward the product-side but also enhance the solubility of lipophilic substratesin the aqueousorganic medium (Fig 343) The alcohol dehydrogenases fromRhodococcus ruber employed as a whole cell preparation tolerate substrate con-centrations of approximately 1ndash2 M Using this system a variety of methyl ke-tones ethyl ketones and chloromethyl ketones could be reduced with Prelogpreference It is also worth noting that this system has been used in a reductionas well as an oxidation mode (see Chapter 4)
3 Catalytic Reductions120
Fig 342 Cofactor recycling during bioreduction processes
To circumvent the drawback of thermodymanic equilibrium limitations andcosubstrate-inhibition cofactor recycling can be performed completely indepen-dently by using a second irreversible reaction and another enzyme This is theso-called coupled-enzyme approach In this case a variety of reducing agentshas been used The most advanced regeneration systems make use of innocu-ous hydrogen as reductant An example has been demonstrated where hydroge-nase from Pyrococcus furiosus was used to recycle the NADP+ cofactor showinga turnover frequency up to 44 hndash1 [119 123] In nature this enzyme ndash which op-erates under thermophilic conditions ndash is able to reversibly cleave the heterolyticcleavage of molecular hydrogen It contains both Ni and Fe in the active siteUnfortunately the enhanced activity of the enzyme at elevated temperature(maximum 80 C) could not be used due to the thermal instability of NADPHand reactions were performed at 40 C This system despite the oxygen sensitiv-ity of hydrogenase I represents an elegant example of green chemistry andbears significant potential (see Fig 344)
One of the prominent industrial bioreduction processes run by cofactor re-generation is performed by leucine dehydrogenase This enzyme can catalyzethe reductive amination of trimethylpyruvic acid using ammonia (see Fig 345)For this process the cofactor regeneration takes place by using formate as thereductant and formate dehydrogenase as the second enzyme The advantage of
34 Biocatalytic Reductions 121
Fig 343 6-Methyl-hept-5-en-2-one reduction andsimultaneous NAD+ regeneration using alcoholdehydrogenase from Rhodococcus rubber
Fig 344 Cofactor recycling using Hydrogenase I from Pyrococcus furiosus
this concept is that the cofactor-regeneration is practically irreversible since car-bon dioxide is produced which can be easily removed Although the substratescope of this enzyme is not too good a number of other substrates have beenscreened [124 125]
Another industrial example albeit on a lower scale of the use of formate asformal reductant is represented by the synthesis of (R)-3-(4-fluorophenyl)-2-hy-droxy propionic acid which is a building block for the synthesis of Rupintrivir arhinovirus protease inhibitor currently in human clinical trials to treat the com-mon cold [126] The chiral 2-hydroxy-acid A can in principle be readily pre-pared by asymmetric reduction of the -keto acid salt B (see Fig 346) [127]Chemocatalysts such as Ru(II)-BINAP and Rh(I)-NORPHOS gave unsatisfac-tory results for this substrate However using d-lactate dehydrogenase (d-LDH)the keto acid salt B could be stereoselectively reduced to the corresponding -hy-droxy acid by NADH with high ee and high conversion For scaling up an en-zyme coupled approach was chosen where formate was used as the stoichio-metric reductant The process is depicted in Fig 346 A relatively simple contin-uous membrane reactor was found to satisfactorily produce -hydroxy acid witha productivity of 560 g Lndash1 dndash1 Enzyme deactivation was a key factor in deter-mining the overall cost of the process In a period of nine days without addingfresh d-LDH and FDH the rate of reaction decreased slowly and the enzymeslost their activity at a rate of only 1 per day Therefore the reactor was chargedwith new enzymes periodically to maintain a high conversion of above 90
An example of glucose coupled ketone reduction is the continuous mode re-duction using whole (dead) cells of Lactobacillus kefir for the enantioselective re-duction of 25-hexanedione to (2R5R)-hexanediol ndash a popular chiral ligand for
3 Catalytic Reductions122
Fig 345 L-tert-leucine production by cofactor-dependent reductive amination
transition metal catalyzed asymmetric hydrogenations In this case the biocataly-tic process is superior to its chemical counterpart because the degt 995 andeegt 995 are difficult to achieve with chemical catalysts [128] While substrateand glucose for cofactor regeneration were constantly fed to a stirred tank reac-tor the product was removed in situ Using this technique the productivitycould be increased to 64 g Lndash1 dndash1 (Fig 347) [129]
Another example for biocatalytic reduction using glucose as the reductant isthe production of (R)-ethyl-444-trifluoro-3-hydroxybutanoate by Lonza [130] Itis a building block for pharmaceuticals such as Befloxatone an anti-depressantmonoamine oxidase-A inhibitor from Synthelabo The process uses whole cellsof Escheria coli that contain two plasmids One carries an aldehyde reductase
34 Biocatalytic Reductions 123
Fig 346 Formate coupled production of chiral -hydroxy acid
Fig 347 Glucose coupled biocatalytic production of (2R5R)-hexanediol
gene from the yeast Sporobolomyces salmonicolor which catalyzes the reductionof ethyl-444-trifluoroacetoacetate and the second carries a glucose dehydroge-nase gene from Bacillus megaterium to generate NADPH from NADP+
(Fig 348) By this ldquoco-expressionrdquo approach the desired enzymes can be pro-duced together in one fermentation The cells can be stored frozen before usein the biotransformation The Lonza process is carried out in a waterbutyl ace-tate two-phase system to avoid inhibition of the reductase by the substrate andproduct An advantage of the two-phase system is that the cells are permeabi-lized allowing the transfer of NADP+ and NADHP through the cell wall Thiswhole-cell biocatalyst was originally constructed for the stereoselective reductionof 4-chloro-3-oxobutanoate (a precursor for l-carnitine) in which case productiv-ities of up to 300 g Lndash1 and ee values of up to 92 were reported [131]
The enantioselective reduction of alkyl-4-chloroacetoacetates is an importantarea because it leads to an intermediate for the side chain of statins Statins arecholesterol-lowering drugs and the market thereof is the largest in the pharma-ceutical sector In 2003 revenues of US$ 92 billion and US$ 61 billion were re-corded for astorvastatin and simvastatin respectively [132] The established strat-egy of enantioselective reduction of alkyl-4-chloroacetoacetates has been opti-mized Alcohol dehydrogenase from Candida magnoliae and glucose dehydro-genase from Bacillus megatorium were used in a biphasic organic solventaqueous buffer system for the production of ethyl (S)-4-chloro-3-hydroxybutano-
3 Catalytic Reductions124
Fig 348 Stereoselective reduction of (R)-ethyl-444-trifluoro-acetoacetate by aldehyde reductase
Fig 349 Biocatalytic production of ethyl (S)-4-chloro-3-hydroxybutanoate using alcohol dehydrogenase fromCandida magnoliae
ate in enantiopure form (see Fig 349) Product concentrations of 63 g Lndash1 wereobserved in the organic phase and the product was isolated in 95 yield [133]
When the enantioselective reduction of ethyl 4-chloroacetoacetate was carriedout with alcohol dehydrogenase from Candida parapsilosis the other enantiomerwas produced ethyl (R)-4-chloro-3-hydroxybutanoate [134] This product is a keyintermediate in a synthesis of (R)-carnitine In this case a substrate coupledapproach was chosen The enzyme also has a strong oxidation activity for 2-pro-panol which was therefore selected as the cosubstrate The situation is depictedin Fig 350 Under optimized conditions the yield of (R)-ethyl-4-chloro-3-hydroxy-butanoate reached 366 g Lndash1 (gt 99 ee 95 yield) on a 30 L scale
343Whole Cell Technology for Biocatalytic Reduction
For small-scale reductions on a laboratory scale the use of (dead cells of) bakerrsquosyeast is a cheap alternative It results in Prelog face reduction of a large varietyof aliphatic and aromatic ketones to give the (S)-alcohols in good optical purities[106] Examples were given above On a larger scale the use of fermenting yeastcan also be attractive [116] An example is the production of a natural ldquogreennoterdquo flavor compound [104] Natural flavors have high consumer appeal andare desired in the food industry Products obtained by fermentation or enzy-matic catalysis usually qualify for the label ldquonaturalrdquo and can be sold at higherprices than nature identical flavors derived by chemical synthesis The greennotes are a mixture of hexenal hexan-1-ol trans-2-hexenal trans-2-hexen-1-oland cis-3-hexen-1-ol The latter dominates the impact of freshness The flavorcompany Firmenich SA Geneva CH [135] developed a process starting frompolyunsaturated fatty acids which are converted to six-carbon hexenals and hex-anal by a combined action of lipoxygenase and hydroperoxide lyase In the sec-ond conversion the aldehydes were reduced employing a 20 bakerrsquos yeast sus-pension This process is operated on the ton scale Separation in this case is rel-atively facile because the flavor compounds are sufficiently volatile to be isolatedby distillation The yeast is discarded after the biotransformation
Another example is the microbial reduction of 34-methylene-dioxyphenylace-tone to the corresponding (S) alcohol at Lilly Research Laboratories [136] (see
34 Biocatalytic Reductions 125
Fig 350 Preparation of ethyl (R)-4-chloro-3-hydroxybutanoateby using alcohol dehdyrogenase from Candida parapsilosis
Fig 351) The chiral alcohol is a key intermediate in the synthesis of an anti-convulsant drug The yeast Zygosaccharomyces rouxii employed for this processis hampered by substrate and product toxicity at levels of gt 6 g Lndash1 This wassolved by using in situ adsorption on Amberlite XAD-7 In this way in situ prod-uct removal could be achieved At the end of the process (8ndash12 h) 75ndash80 g ofthe alcohol is found on the resin and about 2 g Lndash1 remains in the aqueousphase Finally an isolated yield of 85ndash90 could be obtained with an eegt 999
Screening for the novel enzyme although the classical method is still one ofthe most powerful tools for finding biocatalytic reduction systems [108] Enzymesources used for the screening can be soil samples commercial enzymes cul-ture sources a clone bank etc Their origin can be microorganisms animals orplants In most of the examples mentioned above the biocatalyst was chosenafter an extensive screening program A third example of a fermenting processwhich illustrates the importance of screening is shown in Fig 352 The key in-termediate in the synthesis of Montelukast an anti-asthma drug was preparedfrom the corresponding ketone by microbial transformation [137] After screen-ing 80 microorganisms the biotransforming organism Microbacterium campo-quemadoensis (MB5614) was identified which was capable of reducing the com-plex ketone to the (S) alcohol
3 Catalytic Reductions126
Fig 351 Asymmetric reduction of 34-methylene-dioxyphenylacetone
Fig 352 Fermenting process for the production of Montelukast
35Conclusions
Summarizing it is evident that catalytic reduction is an important technologythat is widely applied for the production of fine chemicals It is a key exampleof green technology due to the low amounts of catalysts required in combina-tion with the use of hydrogen (100 atom efficient) as the reductant In gener-al if chirality is not required heterogeneous supported catalysts can be used incombination with hydrogen Apart from the standard reductions such as ketoneand nitro reductions reductive aminations etc the Pd-catalyzed reductive alky-lation of alcohols and amines with aldehydes leading to the green synthesis ofethers and amines needs to be mentioned Once selectivity and chirality iscalled for homogeneous catalysts and biocatalysts are required The use and ap-plication of chiral Ru Rh and Ir catalysts has become a mature technology Itallows a large variety of transformations imines and functionalized ketones andalkenes can be converted with high selectivity in most cases The enantioselec-tive reduction of non-functionalized and non-aromatic alkenes is still an area ofdevelopment
Biocatalysis is developing rapidly Especially in the area of ketone reductionbiocatalytic reduction is often the method of choice due to the high purities ofproduct that can be achieved (gt 99) In these cases alcohol formate or glucoseare used as the reductants Significant progress can be expected in this area dueto the advancement in enzyme production technologies and the possibility oftailor-made enzymes In the future more applications of catalytic reduction willcertainly come forward for new chemical entities as well as for the replacementof current less-green technologies
References 127
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2 W S Knowles Adv Synth Catal 2003345 3
3 R Noyori Adv Synth Catal 2003 34515
4 HB Kagan in Asymmetric Synthesis Vol5 Chiral Catalysis J D Morrison (Ed)Academic Press New York 1985
5 A J J Straathof S Panke A SchmidCurr Opin Biotechnol 2002 13 548
6 K Nakamura R Yamanaka T Matsudaand T Harada Tetrahedron Asym 200314 2659
7 G A Somorjai K McCrea Appl CatalA General 2001 222 3 G A SomorjaiTop Catal 2002 18 157
8 R L Augustine Heterogeneous Catalysisfor the Synthetic Chemist CRC PressNew York 1995
9 G V Smith F Notheisz HeterogeneousCatalysis in Organic Chemistry AcademicPress San Diego 1999
10 H-U Blaser C Malan B Pugin FSpindler H Steiner M Studer AdvSynth Catal 2003 345 103
11 EN Marvell T Li Synthesis 1973 45712 J Sobczak T Boleslawska M Pawlowska
W Palczewska in Heterogeneous Catalysisand Fine Chemicals M Guisnet et al(Eds) Elsevier Amsterdam 1988 p 197
3 Catalytic Reductions128
13 R A Raphael in Acetylenic Compounds inOrganic Synthesis Butterworths London1955 p 26
14 H Lindlar Helv Chim Acta 1952 35446
15 CA Drake US Pat 4596783 and4605797 1996 to Philips PetroleumCompany
16 LA Sarandeses J L Mascarenas LCastedo A Mourino Tetrahedron Lett1992 33 5445
17 S Bailey F King in Fine Chemicalsthrough Heterogeneous CatalysisR A Sheldon H van Bekkum (Eds)Wiley-VCH Weinheim 2001 p 351
18 A Giroir-Fendler D Richard P GallezotStud Surf Sci Catal 1988 41 171
19 A Giroir-Fendler D Richard P GallezotCatal Lett 1990 5 175
20 S Ratton Chem Today MarchApril 19833ndash37
21 T Yokohama T Setoyama N FujitaM Nakajima T Maki Appl Catal 199288 149
22 T Yokoyama T Setoyama in FineChemicals through Heterogeneous CatalysisR A Sheldon H van Bekkum (Eds)Wiley-VCH Weinheim 2001 p 370
23 U Siegrist P Baumeister H-U BlaserM Studer Chem Ind 1998 75 207
24 C De Bellefon P Fouilloux Catal Rev1994 36 459
25 S Gomez J A Peters T MaschmeyerAdv Synth Catal 2002 344 1037
26 A M Allgeier MW Duch Chem Ind2001 82 229
27 SN Thomas-Pryor TA Manz Z LiuTA Koch S K Sengupta W N DelgassChem Ind 1998 75 195
28 P Kukula M Studer H-U Blaser AdvSynth Catal 2004 346 1487
29 P Sabatier Ind Eng Chem 1926 181004
30 SN Balasubrahmanyam N Balasubrah-manyam Tetrahedron 1973 29 683
31 H van Bekkum HMA Buurmans Gvan Minnen-Pathuis BM Wepster ReclTrav Chim Pays-Bas 1969 88 779
32 J G Donkervoort EG M Kuijpers inFine Chemicals through HeterogeneousCatalysis R A Sheldon H van Bekkum(Eds) Wiley-VCH Weinheim 2001p 407
33 LH Slaugh J A Leonard J Catal1969 13 385
34 IWCE Arends M SasidharanA Kuumlhnle M Duda C JostR A Sheldon Tetrahedron 2002 589055
35 J Muzart Tetrahedron 2005 61 595536 F Fache F Valot M Lemaire in Fine
Chemicals through Heterogeneous CatalysisR A Sheldon H van Bekkum (Eds)Wiley-VCH Weinheim 2001 p 461
37 TW Greene P GM Wuts in ProtectiveGroups in Organic Synthesis 2nd ednWiley New York 1991
38 H-U Blaser H Steiner M Studer inTransition Metals for Organic SynthesisVol 2 C Bolm M Beller (Eds)Wiley-VCH Weinheim 1998 p 97
39 E J Creyghton JC van der Waal inFine Chemicals through HeterogeneousCatalysis R A Sheldon H van Bekkum(Eds) Wiley-VCH Weinheim 2001p 438
40 E J Creyghton SD GaneshieR S Downing H van Bekkum J ChemSoc Chem Commun 1995 1859E J Creyghton SD GaneshieR S Downing H van Bekkum J MolCatal A Chemical 1997 115 457
41 J C van der Waal K Tan H van BekkumCatal Lett 1996 41 63
42 A Corma ME Domine L NemethS Valencia J Am Chem Soc 2002124 3194
43 M Studer H-U Blaser C Exner AdvSynth Catal 2003 346 45 H-U BlaserHP Jalett M Muumlller M Studer CatalToday 1997 37 441
44 T Mallat A Baiker in Fine Chemicalsthrough Heterogeneous CatalysisR A Sheldon H van Bekkum (Eds)Wiley-VCH Weinheim 2001 p 449
45 Y Izumi Adv Catal 1983 32 21546 A Baiker J Mol Catal A Chemical
1997 115 47347 Y Orito S Imai S Niwa J Chem Soc
Jpn 1979 111848 B Toumlroumlk K Balagravezsik G Szoumllloumlsi
K Felfoumlldi M Bartoacutek Chirality 199911 470
49 Y Nitta K Kobiro Chem Lett 1996897
References 129
50 H-U Blaser B Pugin M Studer inChiral Catalyst Immobilization and Recy-cling D E De Vos I F J VankelecomPA Jacobs (Eds) Wiley-VCH Wein-heim 2000 p 1
51 K Fodor SG A KolmschotR A Sheldon Enantiomer 1999 4 497and references cited therein
52 T Ohkuma H Takeno Y Honda RNoyori Adv Synth Catal 2001 343 369
53 P Guerreiro V Rato-Velomanana-ViadlJ-P Genet P Dellis Tetrahedron Lett2001 42 3423
54 T Lamouille C Saluzzo R ter HalleF Le Guyader M Lemaire TetrahedronLett 2001 42 663
55 Q Fan C Ren C Yeung W HuA SC Chan J Am Chem Soc 1999121 7407
56 DE Bergbreiter Chem Rev 2002 1023345
57 R L Augustine S K TanielyanS Anderson H Yang Y Gao ChemInd 2001 82 497
58 C Simons U Hanefeld IW CE ArendsR A Sheldon T Maschmeyer Chem EurJ 2004 5839 C Simons U HanefeldIWCE Arends R A SheldonT Maschmeyer Chem Commun 20042830
59 A Wolfson S Geresh M GottliebM Herskowitz Tetrahedron Asym 200213 465
60 FH Jardine JA Osborn G WilkinsonJ F Young Chem Ind 1965 560J Chem Soc (A) 1966 1711
61 J M Grosselin C Mercier G AllmangF Grass Organometallics 1991 10 2126
62 J Halpern Pure Appl Chem 2001 73209
63 L Horner H Buthe H Siegel Tetrahe-dron Lett 1968 4923
64 W S Knowles M J Sabacky J ChemSoc Chem Commun 1968 1445
65 TP Dang HB Kagan J Am ChemSoc 1972 94 6429
66 W S Knowles M J Sabacky BD Vine-yard J Chem Soc Chem Commun1972 10
67 W S Knowles Acc Chem Res 1983 16106
68 W S Knowles in Asymmetric Catalysis onan Industrial Scale H-U Blaser E
Schmidt (Eds) Wiley-VCH Weinheim2004 p 23
69 R Selke H Pracejus J Mol Catal1986 37 213
70 R Selke in Asymmetric Catalysis on anIndustrial Scale H-U Blaser E Schmidt(Eds) Wiley-VCH Weinheim 2004p 39
71 For a recent overview of chiral ligandssee eg Ref [10]
72 R R Bader P Baumeister H-U BlaserChimia 1996 50 86
73 J McGarrity F Spindler R Fux M Eyer EP 624587 1994 to Lonza
74 R Imwinkelried Chimia 1997 51 30075 DA Dobbs K PM Vanhessche
E Brazi V Rautenstrauch J-Y LenoirJ-P Genecirct J Wiles SH BergensAngew Chem Int Ed 2000 39 1992
76 MJ Burk F Bienewald in AppliedHomogeneous Catalysis with Organometal-lic Compounds Vol 2 B CornilsW A Herrmann (Eds) VCH Weinheim1996 p 13
77 MJ Burk F Bienewald S ChallengerA Derrick JA Ramsden J Org Chem1999 64 3290
78 H-U Blaser F Spindler M StuderAppl Catal A General 2001 221 119
79 CJ Cobley NB Johnson IC LennonR McCague JA Ramsden A Zanotti-Gerosa in Asymmetric Catalysis on anIndustrial Scale H-U Blaser E Schmidt(Eds) Wiley-VCH Weinheim 2004p 269
80 R L Balterman in Comprehensive Asym-metric Catalysis Vol 1 EN JacobsenA Pfaltz H Yamamoto (Eds) SpringerBerlin 1999 p 183
81 K E Koenig MJ Sabacky G L BachmanW C Christopfel HD BarnstoffR B Friedman W S Knowles BR StultsBD Vineyard D J Weinkauff Ann NYAcad Sci 1980 333 16
82 H Brunner A Winter J BreuJ Organomet Chem 1998 553 285
83 S Feldgus CR Landis J Am ChemSoc 2000 122 12714
84 T Ikarya Y Ishii H Kawano T AraiM Saburi S Yoshikawa S AkutagawaJ Chem Soc Chem Commun 1985922
3 Catalytic Reductions130
85 R Noyori M Ohta Y HsiaoM Kitamura T Ohta H TakayaJ Am Chem Soc 1986 108 7117R Noyori H Takaya Acc Chem Res1990 23 345
86 H Kumobayashi T Miura N SayoT Saito X Zhang Synlett 2001 1055
87 H Kumobayashi Recl Trav ChimPays-Bas 1996 115 201
88 SA King A S Thompson AO KingTR Verhoeven J Org Chem 199257 6689
89 R Noyori T Ikeda T OhkumaM Widhalm M Kitamura H TakayaS Akutagawa N Sayo T SaitoT Taketomi H Kumobayashi J AmChem Soc 1989 111 9134
90 R Noyori Acta Chem Scand 1996 50380
91 R Noyori T Ohkuma Angew ChemInt Ed 2001 40 41
92 R Hartmann P Chen Angew ChemInt Ed 2001 40 3581
93 K Abdur-Rashid M Faatz A J LoughR H Morris J Am Chem Soc 2001123 7473
94 M Yamakawa H Ito R NoyoriJ Am Chem Soc 2000 122 1466
95 H-U Blaser F Spindler in Compre-hensive Asymmetric Catalysis Vol 1EN Jacobsen A Pfaltz H Yamamoto(Eds) Springer Berlin 1999 p 248
96 T Ohkuma M Kitamura R Noyoriin Catalytic Asymmetric Synthesis 2ndedn I Ojima (Ed) VCH PublishersNew York 2000 p 1
97 H-U Blaser R Hanreich H-DSchneider F Spindler B Steinacherin Asymmetric Catalysis on an IndustrialScaleH-U Blaser E Schmidt (Eds)Wiley-VCH Weinheim 2004 p 55
98 CF de Graauw J A Peters H vanBekkum J Huskens Synthesis 19941007
99 G Zassinovich G Mestroni S Gladia-li Chem Rev 1992 92 1051
100 R Noyori S Hashiguchi Acc ChemRes 1997 30 97
101 M Wills Tetrahedron Asymmetry 199910 2045
102 J Blacker J Martin in AsymmetricCatalysis on an Industrial Scale
H-U Blaser E Schmidt (Eds) Wiley-VCH Weinheim 2004 p 201
103 S J M Nordin P Roth T TarnaiDA Alonso P Brandt P G AnderssonChem Eur J 2001 7 1431
104 Enzyme Nomenclature Academic PressNew York 1992
105 M-R Kula U Kragl in StereoselectiveBiocatalysis RN Patel (Ed) MarcelDekker New York 2000 p 839
106 K Faber Biotransformations in OrganicChemistry 4th edn Springer Berlin2000
107 W Kroutil H Mang K EdeggerK Faber Curr Opin Chem Biol 20048 120
108 K Nakamura R Yamanaka T MatsudaT Harada Tetrahedron Asymmetry 200314 2659
109 For an introduction to the area ofdirected evolution see K A PowellSW Ramer S B del CardayreacuteW PC Stemmer MB TodinPF Longchamp G W HuismanAngew Chem Int Ed 2001 40 3948
110 MT Reetz Angew Chem Int Ed2001 40 284
111 A Fersht Structure and Mechanism inProtein Science Freeman and CompanyNew York 1999
112 J K Rubach BV Plapp Biochemistry2003 42 2907 and references citedtherein
113 CW Bradshaw W HummelCH Wong J Org Chem 1992 571532
114 V Prelog Pure Appl Chem 1964 9119
115 U Kragl D Vasic-Racki C WandreyBioproc Eng 1996 14 291
116 S Servi in Biotechnology 2nd ednVol 8a HJ Rehm G Reed (Eds)Wiley-VCH Weinheim 1998 p 363
117 M Chartrain R Greasham J MooreP Reider D Robinson B BucklandJ Mol Catal B Enzymatic 2001 11503
118 For selected examples see Ref [5]119 R Mertens L Greiner E CD van den
Ban HBCM Haaker A Liese JMol Catal B Enzymatic 2003 24--2539
References 131
120 J M Vrtis AK White W M MetcalfW A van der Donk Angew Chem IntEd 2002 41 3257
121 T Stillger M Boumlnitz M Villela FilhoA Liese Chem Ing Technol 2002 741035
122 W Stampfer B Kosjek C MoitziW Kroutil K Faber Angew Chem IntEd 2002 41 1014
123 L Greiner D H Muumlller E CD vanden Ban J Woumlltinger C WandreyA Liese Adv Synth Catal 2003 345679
124 G Krix A S Bommarius K DrauzM Kottenhan M SchwarmM-R Kula J Biotechnol 1997 53 29
125 H Groger K Drauz in AsymmetricCatalysis on an Industrial ScaleH-U Blaser E Schmidt (Eds) Wiley-VCH Weinheim 2004 p 131
126 J Tao K McGee in Asymmetric Catalysison an Industrial Scale H-U BlaserE Schmidt (Eds) Wiley-VCH Wein-heim 2004 p 323
127 M-J Kim G M Whitesides J AmChem Soc 1988 110 2959
128 J Haberland A KriegesmannE Wolfram W Hummel A LieseAppl Microb Biotechnol 2002 58 595
129 J Haberland W Hummel T DausmanA Liese Org Proc Res Dev 2002 6458
130 NM Shaw KT Robbins A KienerAdv Synth Catal 2003 345 425
131 S Shimizu M Kataoka A MorishitaM Katoh T Morikawa T MiyoshiH Yamada Biotechnol Lett 1990 12593
132 M Muumlller Angew Chem Int Ed 200544 362
133 Y Yasohara N Kizaki J HasegawaM Wada M Kataoka S Shimizu Tet-rahedron Asym 2001 12 1713N Kizaki Y Yasohara J HasegawaM Wada M Kataoka S ShimizuAppl Microbiol Biotechnol 2001 55590
134 H Yamamoto A MatsuyamaY Kobayashi Biosci Biotechnol Bio-chem 2002 66 925
135 BL Muller C Dean I M WhiteheadSymposium Plant Enzymes in the FoodIndustry 1994 26 Lausanne
136 BA Anderson MM HansenA R Harkness CL Henry J T VicenziMJ Zmijewski J Am Chem Soc 1995117 12358 MJ Zmijewski J VicenziBE Landen W Muth P MarlerB Anderson Appl Microbiol Biotechnol1997 47 162 J T VicenziMJ Zmijewski MR ReinhardBE Landen WL Muth P G MarlerEnzyme Microbial Technol 1997 20494
137 A Shafiee H Motamedi A KingAppl Microbiol Biotechnol 1998 49709
41Introduction
The controlled partial oxidation of hydrocarbons comprising alkanes alkenesand (alkyl)aromatics is the single most important technology for the conversionof oil- and natural gas-based feedstocks to industrial organic chemicals [1ndash3]For economic reasons these processes predominantly involve the use of mole-cular oxygen (dioxygen) as the primary oxidant Their success depends largelyon the use of metal catalysts to promote both the rate of reaction and the selec-tivity to partial oxidation products Both gas phase and liquid phase oxidationsemploying heterogeneous and homogeneous catalysts respectively are used in-dustrially in a ca 5050 ratio (see Table 41)
The pressure of increasingly stringent environmental regulation is also pro-viding a stimulus for the deployment of catalytic oxidations in the manufactureof fine chemicals Traditionally the production of many fine chemicals involvedoxidations with stoichiometric quantities of for example permanganate or di-chromate resulting in the concomitant generation of copious amounts of inor-ganic salt-containing effluent Currently there is considerable pressure there-fore to replace these antiquated technologies with cleaner catalytic alternatives[3 4] In practice this implies an implementation of catalytic technologies whichallow the use of oxygen and hydrogen peroxide (which produces water as theside product) as stoichiometric oxidants Therefore this chapter will focus oncatalysts which use either O2 or H2O2 as oxidants In some cases eg in thecase of stereoselective conversion where a highly added benefit of the productprevails the use of other oxidants will be considered as well
In principle homogeneous as well as heterogeneous and bio-catalysts can bedeployed in liquid phase oxidations but in practice the overwhelming majorityof processes are homogeneous ie they involve the use of soluble metal salts orcomplexes as the catalyst Pivotal examples of the potential of selective catalyzedoxidations have already been mentioned in Chapter 1 For example in the oxi-dation of alcohols and epoxidation of olefins enormous progress has beenachieved over the last decade towards green methods notably using homoge-neous metal complexes However also in the field of biocatalytic transforma-tions industrial applications start to appear notably in the field of aromatic side
133
4Catalytic Oxidations
chain oxidation of heteroaromatics [5] In the next section the basics of mecha-nisms in metal-catalyzed oxidations ndash homolytic versus heterolytic ndash will be pre-sented The fundamentals of redox catalysis by enzymes will also be given Thegreen methodologies for converting different classes of substrates will then betreated consecutively
42Mechanisms of Metal-catalyzed Oxidations General Considerations
The ground state of dioxygen is a triplet containing two unpaired electrons withparallel spins The direct reaction of 3O2 with singlet organic molecules to givesinglet products is a spin forbidden process with a very low rate Fortunatelythis precludes the spontaneous combustion of living matter a thermodynami-cally very favorable process
One way of circumventing this activation energy barrier involves a free radicalpathway in which a singlet molecule reacts with 3O2 to form two doublets (freeradicals) in a spin-allowed process (Fig 41 Reaction (1)) This process is how-ever highly endothermic (up to 50 kcal molndash1) and is observed at moderate tem-peratures only with very reactive molecules that afford resonance stabilized radi-cals eg reduced flavins (Fig 41 Reaction (2)) It is no coincidence therefore
4 Catalytic Oxidations134
Table 41 Bulk chemicals via catalytic oxidation
Product Feedstock OxidantProcess a)
StyreneTerephthalic acidFormaldehydeEthene oxidePhenol
Acetic acid
Propene oxideAcrylonitrileVinyl acetateBenzoic acidAdipic acid-CaprolactamPhthalic anhydrideAcrylic acidMethyl methacrylateMaleic anhydride
Benzeneethenep-XyleneMethanolEthenea Benzenepropeneb Toluenea n-Butaneb EthenePropenePropeneEtheneTolueneBenzeneBenzeneo-XylenePropeneIsobutenen-Butane
NoneG (O2L) b)
O2LO2GO2GO2L
O2L
RO2HLO2GO2L GO2LO2LO2LO2GO2GO2GO2G
a) L = liquid phase G =gas phaseb) Styrene from propene epoxidation with EBHP
that this is the key step in the activation of dioxygen by flavin-dependent oxyge-nases
A second way to overcome this spin conservation obstacle is via reaction of3O2 with a paramagnetic (transition) metal ion affording a superoxometal com-plex (Fig 41 Reaction (3)) Subsequent inter- or intramolecular electron-transferprocesses can lead to the formation of a variety of metalndashoxygen species(Fig 42) which may play a role in the oxidation of organic substrates
Basically all (catalytic) oxidations with dioxygen or peroxide reagents eitherunder homogeneous or heterogeneous conditions can be divided into two typeson the basis of their mechanism homolytic and heterolytic The former involvefree radicals as reactive intermediates Such reactions can occur with most or-ganic substrates and dioxygen in the presence or absence of metal catalystsThis ubiquity of free radical processes in dioxygen chemistry renders mechanis-tic interpretation more difficult than in the case of hydrogenations or carbonyla-tions where there is no reaction in the absence of the catalyst
42 Mechanisms of Metal-catalyzed Oxidations General Considerations 135
Fig 41 Reactions of triplet oxygen
Fig 42 Metalndashoxygen species
Heterolytic oxidations generally involve the (metal-mediated) oxidation of asubstrate by an active oxygen compound eg H2O2 or RO2H Alternatively stoi-chiometric oxidation of a substrate by a metal ion or complex is coupled withthe reoxidation of the reduced metal species by the primary oxidant (eg O2 orH2O2)
421Homolytic Mechanisms
As noted above dioxygen reacts with organic molecules eg hydrocarbons viaa free radical pathway The corresponding hydroperoxide is formed in a free rad-ical chain process (Fig 43) The reaction is autocatalytic ie the alkyl hydroper-oxide accelerates the reaction by undergoing homolysis to chain initiating radi-cals and such processes are referred to as autoxidations [1]
The susceptibility of any particular substrate to autoxidation is determined bythe ratio kp(2kt)
12 which is usually referred to as its oxidizability [6] The oxi-dizabilities of some typical organic substrates are collected in Table 42
The reaction can be started by adding an initiator which undergoes homolyticthermolysis at the reaction temperature to produce chain-initiating radicals Theinitiator could be the alkyl hydroperoxide product although relatively high tem-peratures (gt 100 C) are required for thermolysis of hydroperoxides Alterna-tively chain-initiating radicals can be generated by the reaction of trace amountsof hydroperoxides with variable valence metals eg cobalt manganese iron cer-ium etc The corresponding alkoxy and alkylperoxy radicals are produced inone-electron transfer processes (Fig 44)
In such processes the metal ion acts (in combination with ROOH) as an initi-ator rather than a catalyst It is important to note that homolytic decompositionof alkyl hydroperoxides via one-electron transfer processes is generally a com-
4 Catalytic Oxidations136
Fig 43 Mechanism of autoxidation
peting process even with metal ions that catalyze heterolytic processes with hy-droperoxides (see above) Since dioxygen can be regenerated via subsequentchain decomposition of the alkyl hydroperoxide this can lead to competing freeradical autoxidation of the substrate Generally speaking this has not been rec-ognized by many authors and can lead to a misinterpretation of results
4211 Direct Homolytic Oxidation of Organic SubstratesAnother class of metal catalyzed autoxidations involves the direct one-electronoxidation of the substrate by the oxidized form of the metal catalyst For exam-ple the autoxidation of alkylaromatics in acetic acid in the presence of relativelyhigh concentrations (01 M) of cobalt(III) acetate involves rate-limiting oneelectron transfer oxidation of the alkylbenzene to the corresponding cation radi-cal (Fig 45) This is followed by elimination of a proton to afford the corre-sponding benzylic radical which subsequently forms a benzylperoxy radical byreaction with dioxygen The primary products from substituted toluenes are thecorresponding aldehydes formed by reaction of benzylperoxy radicals with co-balt(II) (which simultaneously regenerates the cobalt(III) oxidant) The usual re-action of alkylperoxy radicals with the toluene substrate (see Fig 43) is largely
42 Mechanisms of Metal-catalyzed Oxidations General Considerations 137
Table 42 Oxidizabilities of organic compounds at 30 Ca)
Substrate kp(2kt)12103 (Mndash12 sndash12)
IndeneCyclohexene1-OcteneCumeneEthylbenzeneToluenep-XyleneBenzaldehyde b)
Benzyl alcoholDibenzyl ether
2842300615021001005
29008571
a) Data taken from Ref [6]b) At 0 C
Fig 44 Metal initiated and mediated autoxidation
2 RO2H RO2
circumvented by the efficient trapping of the benzylperoxy radical with the rela-tively high concentration of cobalt(II) present The aldehyde product undergoesfacile autoxidation to the corresponding carboxylic acid and metal-catalyzed aut-oxidation of methylaromatics is a widely used method for the production of car-boxylic acids (see below) Since cobalt is usually added as cobalt(II) reactive sub-strates such as aldehydes or ketones are often added as promoters to generatethe high concentrations of cobalt(III) necessary for initiation of the reaction
422Heterolytic Mechanisms
Catalytic oxidations with dioxygen can also proceed via heterolytic pathwayswhich do not involve free radicals as intermediates They generally involve atwo-electron oxidation of a (coordinated) substrate by a metal ion The oxidizedform of the metal is subsequently regenerated by reaction of the reduced formwith dioxygen Typical examples are the palladium(II)-catalyzed oxidation of al-kenes (Wacker process) and oxidative dehydrogenation of alcohols (Fig 46)
In a variation on this theme which pertains mainly to gas phase oxidationsan oxometal species oxidizes the substrate and the reduced form is subse-quently re-oxidized by dioxygen (Fig 47) This is generally referred to as theMars-van Krevelen mechanism [7]
A wide variety of oxidations mediated by monooxygenase enzymes are similar-ly thought to involve oxygen transfer from a high-valent oxoiron intermediate tothe substrate (although the mechanistic details are still controversial) [8ndash11]However in this case a stoichiometric cofactor is necessary to regenerate the re-duced form of the enzyme resulting in the overall stoichiometry shown inFig 48
Indeed the holy grail in oxidation chemistry is to design a lsquosuprabioticrsquo cata-lyst capable of mediating the transfer of both oxygen atoms of dioxygen to or-
4 Catalytic Oxidations138
Fig 45 Direct homolytic oxidation of benzylic compounds
ganic substrates such as alkenes and alkanes [12] This would obviate the needfor a stoichiometric cofactor as a sacrificial reductant ie it would amount to aMars-van Krevelen mechanism in the liquid phase
4221 Catalytic Oxygen TransferAnother way to avoid the need for a sacrificial reductant is to use a reducedform of dioxygen eg H2O2 or RO2H as a single oxygen donor Such a reactionis referred to as a catalytic oxygen transfer and can be described by the generalequation shown in Fig 49
Catalytic oxygen transfer processes are widely applicable in organic synthesisVirtually all of the transition metals and several main group elements areknown to catalyze oxygen transfer processes [13] A variety of single oxygen do-nors can be used (Table 43) in addition to H2O2 or RO2H Next to price and
42 Mechanisms of Metal-catalyzed Oxidations General Considerations 139
Fig 46 Wacker oxidation and oxidative dehydrogenation of alcohols
Fig 47 Mars-van Krevelen mechanism
Fig 48 Stoichiometry in oxidations mediated by monooxygenases
Fig 49 Catalytic oxygen transfer
ease of handling two important considerations which influence the choice ofoxygen donor are the nature of the co-product and the weight percentage ofavailable oxygen The former is important in the context of environmental ac-ceptability and the latter bears directly on the volumetric productivity (kg prod-uct per unit reactor volume per unit time) With these criteria in mind it isreadily apparent that hydrogen peroxide which affords water as the co-productis generally the preferred oxidant The co-product from organic oxidants suchas RO2H and amine oxides can be recycled via reaction with H2O2 The overallprocess produces water as the co-product but requires one extra step comparedto the corresponding reaction with H2O2 With inorganic oxygen donors envi-ronmental considerations are relative Sodium chloride and potassium bisulfateare obviously preferable to the heavy metal salts (Cr Mn etc) produced in clas-sical stoichiometric oxidations Generally speaking inorganic oxidants are moredifficult to recycle in an economic manner than organic ones Indeed the easeof recycling may govern the choice of oxidant eg NaOBr may be preferred overNaOCl because NaBr can in principle be re-oxidized with H2O2 As noted ear-lier a disadvantage of H2O2 and RO2H as oxygen donors is possible competi-tion from metal-catalyzed homolytic decomposition leading to free radical oxida-tion pathways andor low selectivities based on the oxidant
Heterolytic oxygen transfer processes can be divided into two categories basedon the nature of the active oxidant an oxometal or a peroxometal species(Fig 410) Catalysis by early transition metals (Mo W Re V Ti Zr) generallyinvolves high-valent peroxometal complexes whereas later transition metals (RuOs) particularly first row elements (Cr Mn Fe) mediate oxygen transfer via oxo-metal species Some elements eg vanadium can operate via either mecha-nism depending on the substrate Although the pathways outlined in Fig 410
4 Catalytic Oxidations140
Table 43 Oxygen donors
Donor Active Oxygen Coproduct
H2O2
N2OO3
CH3CO3Htert-BuO2HHNO3
NaOClNaO2ClNaOBrC5H11NO2
b)
KHSO5
NaIO4
PhIO
470 (141) a)
3643332111782542163561341371057573
H2ON2
O2
CH3CO2Htert-BuOHNOx
NaClNaClNaBrC5H11NOKHSO4
NaIO3
PhI
a) Figure in parentheses refers to 30 aq H2O2b) N-Methylmorpholine-N-oxide (NMO)
pertain to peroxidic reagents analogous schemes involving M=O or MOX(X = ClO IO4 HSO5 R3NO etc) as the active oxidant can be envisaged forother oxygen donors Reactions that typically involve peroxometal pathways arealkene epoxidations alcohol oxidations and heteroatom (N and S) oxidationsOxometal species on the other hand are intermediates in the oxidation of al-kane benzylic and allylic CndashH bonds and the dihydroxylation and oxidativecleavage of olefins in addition to the above-mentioned transformations
For the sake of completeness we also note that oxygen transfer processes canbe mediated by organic catalysts which can be categorized on the same basis asmetal catalysts For example ketones catalyze a variety of oxidations with mono-peroxysulfate (KHSO5) [14] The active oxidant is the corresponding dioxiraneand hence the reaction can be construed as involving a lsquoperoxometalrsquo pathwaySimilarly TEMPO-catalyzed oxidations of alcohols with hypochlorite [15 16] in-volve an oxoammonium salt as the active oxidant ie an lsquooxometalrsquo pathway
423Ligand Design in Oxidation Catalysis
In the majority of catalytic oxidations simple metal salts are used as the cata-lysts In contrast oxidations mediated by redox enzymes involve metal ions co-ordinated to complex ligands amino acid residues in a protein or a prostheticgroup eg a porphyrin ligand in heme-dependent enzymes Indeed many ofthe major challenges in oxidation chemistry involve demanding oxidations suchas the selective oxidation of unactivated CndashH bonds which require powerful oxi-dants This presents a dilemma if an oxidant is powerful enough to oxidize anunactivated CndashH bond then by the same token it will readily oxidize most li-gands which contain CndashH bonds that are more active than the CndashH bonds ofthe substrate The low operational stability of for example heme-dependent en-zymes is a direct consequence of the facile oxidative destruction of the porphyr-in ring Nature solves this problem in vivo by synthesizing fresh enzyme to re-place that destroyed In vitro this is not a viable option In this context it isworth bearing in mind that many simple metal complexes that are used as cata-
42 Mechanisms of Metal-catalyzed Oxidations General Considerations 141
Fig 410 Peroxometal versus oxometal pathways
lysts in oxidation reactions contain ligands eg acetylacetonate that are rapidlydestroyed under oxidizing conditions This fact is often not sufficiently recog-nized by authors of publications on catalytic oxidations
Collins [17] has addressed the problem of ligand design in oxidation catalysisin some detail and developed guidelines for the rational design of oxidatively ro-bust ligands Although progress has been achieved in understanding ligand sen-sitivity to oxidation the ultimate goal of designing metal complexes that are bothstable and exhibit the desired catalytic properties remains largely elusive Wenote in this context that an additional requirement has to be fulfilled the de-sired catalytic pathway should compete effectively with the ubiquitous free radi-cal autoxidation pathways
One category of oxidations deserves special mention in the context of liganddesign enantioselective oxidations It is difficult to imagine enantioselective oxi-dations without the requirement for (chiral) organic ligands Here again thetask is to design ligands that endow the catalyst with the desired activity and(enantio-)selectivity and at the same time are (reasonably) stable
In the following sections oxidative transformations of a variety of functionalgroups will be discussed from both a mechanistic and a synthetic viewpoint
424Enzyme Catalyzed Oxidations
Oxidations by enzymes are performed by the group of oxidoreductases An over-view of the classification of oxidoreductases is given in Fig 411
The alcohol dehydrogenases were already described in Chapter 3 These en-zymes are cofactor dependent and in the active site hydrogen transfer takesplace from NADH or NADPH In the reverse way they can however be appliedfor the oxidation of alcohols in some cases (see below) Oxidases are very appeal-ing for biocatalytic purposes because they use oxygen as the only oxidant with-out the need for a cofactor Oxidases usually have flavins (glucose oxidase alco-hol oxidase) or copper (examples galactose oxidase laccase and tyrosinase) inthe active site [18] The mechanism for glucose oxidase (GOD) is denoted in
4 Catalytic Oxidations142
Fig 411 Classes of oxidoreductases
Fig 412 GOD oxidases the oxidation of -D-glucose to D-glucone--lactone areaction which has attracted the attention of generations of analytical scientistsdue to its possible applicability in glucose sensors for diabetes control
Galactose oxidase exhibits a mononuclear copper-active site which is flankedby a tyrosinyl radical In a single step a two-electron oxidation of alcohols canbe performed by this enzyme where one electron is extracted by copper andthe other by the tyrosine residue [19]
In the case of oxygenases catalytic oxygen transfer has to take place andmany of the principles described above are operative here as well A combina-tion of oxygen and NADH or NADPH is supplied to the active site which re-sults in net transfer of ldquoOrdquo and H2O as the by-product Thus NAD(P)H is re-quired as sacrificial reductant and only one of the two oxygen atoms in oxygenends up in the product An exception is the dioxygenases where both oxygenatoms can end up in the product Oxygenases can be classified depending ontheir redox-active cofactor (Table 44) The active site commonly contains eithera heme-iron non-heme-iron flavin or copper (mono- or binuclear) as redox-ac-tive group
42 Mechanisms of Metal-catalyzed Oxidations General Considerations 143
Fig 412 Aerobic oxidation of D-glucose catalyzed by flavin-dependent glucose oxidase
Table 44 Classification of oxygenases
Type Examples Substrates
Heme-iron aromatics Cytochrome-P450 alkanes alkenesNon-heme-iron Methane monooxygenase alkanes alkenes
Rieske dioxygenases aromatics alkenesLipoxygenase alkenes
Flavin Hydroxybiphenyl monooxygenase aromaticsStyrene monooxygenase styrenesCyclohexane monooxygenase Baeyer-Villiger
Copper Tyrosinase phenolicDopamine -monooxygenase benzylic CndashH
A pivotal class of oxygenases are the so-called iron heme-proteins from theCytochrome P450 family in which the iron is ligated by a porphyrin moiety [1120 21] In the first case an oxometal-type mechanism is operative where a pu-tative P+Fe(IV)=O (P = porphyrin) species transfers oxygen directly to the sub-strate (see Fig 413) The exact identity is still a matter of controversy Generallya Fe(IV)=O species stabilized by a cationic radical porphyrin moiety seems to befavored instead of a formally Fe(V)=O species Especially intriguing is the poten-tial of these types of enzymes to perform a stereoselective hydroxylation of non-activated alkanes ndash a reaction which is still very rare in the case of metal-cata-lysed oxidations A so-called rebound mechanism has been proposed in thiscase which involves a [FendashOH R] transient species (see Fig 414) Iron-heme-type enzymes are the enzymes which have the broadest substrate spectrumThey are capable of performing oxygenation on a wide range of compoundsfrom alkanes and fatty acids to alkenes and alcohols Due to the instability ofthe heme group and the requirement for a cofactor these enzymes are com-monly employed under microbial whole cell conditions [22]
Another important class of oxygenases are the flavin-dependent oxygenasesnotably in Baeyer-Villiger oxidation and epoxidation [23 24] The mechanism forBaeyer-Villiger conversion of cyclic ketones into esters by the enzyme cyclohex-ane monooxygenase is shown in Fig 415 [25] The prosthetic group FADwhich is tightly bound to the active site of the enzyme is reduced to FADH2 byNADPH Rapid reaction between FADH2 and molecular oxygen (see Fig 41Reaction (2)) affords 4-hydroperoxyflavin which is a potent oxidizing agent Ad-dition of 4-hydroperoxyflavin to the carbonyl group of cyclohexanone creates atetrahedral intermediate which rearranges to give FAD-4-OH and -caprolac-tone Finally a water molecule is eliminated from FAD-4-OH to regenerate
4 Catalytic Oxidations144
Fig 413 Fe-porphyrins and the peroxide shunt pathway
FAD ready for a subsequent catalytic cycle This enzyme catalyzed Baeyer-Villi-ger oxidation bears great resemblance to the analogous chemical reaction per-formed by peroxides or peracids which act as nucleophiles Globally these fla-vin-enzymes can perform the same reactions as peracids ie epoxidationsBaeyer-Villiger-reactions and nucleophilic heteroatom oxidation [26ndash28]
Within the group of non-heme-iron monooxygenases two notable classes can beidentified The binuclear non-heme monooxygenases and the mononuclear diox-ygenases [29 30] The most important example of the first group methane mono-oxygenase is capable of mediating the oxidation of a broad range of substrates in-cluding methane at ambient temperature [31] In this enzyme a non-heme di-ironcore is present in which the two-irons are connected through two carboxylatebridges and coordinated by histidine residues (see Fig 416) [32] Also in this caseFe(IV)=O species have been proposed as the active intermediates
42 Mechanisms of Metal-catalyzed Oxidations General Considerations 145
Fig 414 Fe-porphyrins and the oxygen-rebound mechanism
Fig 415 Mechanism of the Baeyer-Villiger oxidation ofcyclohexanone using flavin-dependent monooxygenase
The class of mononuclear dioxygenases [30] can eg perform hydroperoxida-tion of lipids the cleavage of catechol and dihydroxylation of aromatics A pro-minent example is naphthalene dioxygenase which was the first identified byits crystal structure It contains iron and a Rieske (2Fendash2S) cluster and is com-monly referred to as a Rieske-type dioxygenase [33] The iron in this case isflanked by two histidines and one aspartic acid residue Among the mononuc-lear iron enzymes the 2-His-1-carboxylate is a common motif which flanksone-side of the iron in a triangle and plays an important role in dioxygen activa-tion [34] (Fig 417)
Alternatively copper is capable of H-atom abstraction leading to aliphatic hy-droxylation The enzyme dopamine -monooxygenase is an example thereof andthe reaction is exemplified in Fig 418 [35] Recently it has been disclosed thatthe two copper centers in the enzyme are far apart and not coupled by any mag-netic interaction [36] The binding and activation of dioxygen thus takes place ata single Cu-center which can provide one electron to generate a superoxo CuIIndashO2
ndash intermediate This superoxo intermediate is supposed to be capable of H-atom abstraction
All the above examples of monooxygenases are dependent on cofactors Theenzymes are usually composed of several subunits which in a series of cas-cades provide the reducing equivalents to the iron-active site The need for a co-
4 Catalytic Oxidations146
Fig 416 Structure of the MMO-iron site and its catalytic cyle
Fig 417 (a) The 2-His-1-carboxylate facial triad innaphthalene dioxygenase (NDO) (b) Reaction catalyzed byNDO
factor is circumvented in the case of peroxidases where H2O2 acts as the oxidantIn this case the addition of hydrogen peroxide results in a shunt pathway whichdirectly recovers the [Fe(IV)=O][P+] species from Fe(III) (see Fig 413) Besidesiron-heme-dependent peroxidases [37] vanadate-dependent peroxidases are alsoknown which can catalyze sulfide oxidations and which exhibit much higherstabilities [38]
43Alkenes
Various combinations of metal catalyst and single oxygen donor have been usedto effect different oxidative transformations of olefins epoxidation dihydroxyla-tion oxidative cleavage ketonization and allylic oxidation The most extensivelystudied example is undoubtedly olefin epoxidation [39]
431Epoxidation
The epoxidation of propene with tert-butylhydroperoxide (TBHP) or ethylben-zene hydroperoxide (EBHP) for example accounts for more than one milliontons of propene oxide production on an annual basis (Fig 419)
The reaction in Fig 419 is catalyzed by compounds of high-valent early tran-sition metals such as Mo(VI) W(VI) V(V) and Ti(IV) Molybdenum compoundsare particularly effective homogeneous catalysts and are used in the ARCO pro-cess in combination with TBHP or EBHP In the Shell process on the otherhand a heterogeneous Ti(IV)SiO2 catalyst is used with EBHP in a continuous
43 Alkenes 147
Fig 418 Hydroxylation of dopamine by the non-coupledbinuclear copper center in dopamine--monooxygenase
Fig 419 Epoxidation of propylene using RO2H as oxidant
fixed-bed operation Alkyl hydroperoxides in combination with homogeneous(Mo W V Ti) or heterogeneous (Ti(IV)SiO2) catalysts can be used for the selec-tive epoxidation of a wide variety of olefins [40] Chiral titanium complexes areused as catalysts for enantioselective epoxidations with alkyl hydroperoxides (seebelow)
The epoxidation of olefins with RO2H or H2O2 (see above) catalyzed by earlytransition elements involves as would be expected a peroxometal mechanismin which the rate-limiting step is oxygen transfer from an electrophilic (alkyl)peroxometal species to the nucleophilic olefin (Fig 420) The metal center doesnot undergo any change in oxidation state during the catalytic cycle It functionsas a Lewis acid by withdrawing electrons from the OndashO bond and thus in-creased the electrophilic character of the coordinated peroxide Active catalystsare metals that are strong Lewis acids and relatively weak oxidants (to avoid oneelectron oxidation of the peroxide) in their highest oxidation state
Neither the homogeneous Mo nor the heterogeneous Ti(IV)SiO2 catalysts areeffective with hydrogen peroxide as the oxygen donor Indeed they are severelyinhibited by strongly coordinating molecules such as alcohols and particularlywater Because of the strong interest in the use of H2O2 as the primary oxidantparticularly in the context of fine chemicals production much effort has beendevoted to developing epoxidation catalysts that are effective with aqueous hy-drogen peroxide
In the mid-1980s two approaches were followed to achieve this goal Enichemscientists developed a titanium(IV)-silicalite catalyst (TS-1) that is extremely ef-fective for a variety of synthetically useful oxidations including epoxidation with
4 Catalytic Oxidations148
Fig 420 Peroxometal mechanism in theepoxidation
Fig 421 Epoxidation catalyzed by TS-1
30 aqueous H2O2 (Fig 421) [41] The unique activity of TS-1 derives from thefact that silicalite is a hydrophobic molecular sieve in contrast to Ti(IV)SiO2
which is hydrophilic Consequently hydrophobic substrates are preferentiallyadsorbed by TS-1 thus precluding the strong inhibition by water observed withTi(IV)SiO2 However a serious limitation of TS-1 in organic synthesis is thatits scope is restricted to relatively small molecules eg linear olefins which areable to access the micropores (5355 Aring2) This provoked a flurry of activityaimed at developing titanium-substituted molecular sieves with larger poreswhich as yet has not produced catalysts with comparable activity to TS-1 [42]
4311 Tungsten CatalystsAt the same time Venturello and coworkers [43] followed a different approachThey showed that a mixture of tungstate and phosphate in the presence of a tet-raalkylammonium salt as a phase transfer agent catalyzed epoxidations withH2O2 in a two-phase dichloroethanewater medium Since its discovery in 1983this system has been extensively studied [44 45] in particular with regard to theexact nature of the active phosphotungstate catalyst [46] More recently Noyoriand coworkers reported [47] a significant improvement of the original systemAn appropriate choice of phase transfer catalyst containing a sufficiently lipo-philic tetraalkylammonium cation and a bisulfate (HSO4
ndash) anion in combinationwith catalytic amounts of H2NCH2PO3H2 and sodium tungstate produced an ef-fective system for the epoxidation of olefins with H2O2 in toluenewater or inthe absence of an organic solvent (Fig 422) The type of ammonium salt usedwith phosphatetungstic acid catalyst is important For example n-octylammo-nium hydrogen sulfate is critical in Noyorirsquos work chloride causes deactivationand other ammonium hydrogen sulfates produce catalysts that are not as effec-tive or are even completely inactive
Subsequently the Noyori-system was shown [48] to be an effective system forthe oxidative cleavage of cyclic olefins to dicarboxylic acids (Fig 423) using 4equivalents of H2O2 via the intermediate formation of the epoxide For exam-ple cyclohexene afforded adipic acid in 93 isolated yield thus providing alsquogreen routersquo to adipic acid Although the economics may be prohibitive for adi-pic acid manufacture owing to the consumption of 4 equivalents of H2O2 themethod has general utility for the selective conversion of a variety of cyclic ole-fins to the corresponding dicarboxylic or keto-carboxylic acids
The success of tungstate as catalyst has stimulated a wealth of research inthis area Recently it was shown that a silicotungstate compound synthesized
43 Alkenes 149
Fig 422 Halide- and halogenated solvent-free biphasic epoxidationwith 30 aqueous H2O2 using tungstate catalysts
by protonation of a divalent lacunary Keggin-type compound exhibits high cata-lytic performance for epoxidations with H2O2 For example propene could beoxidized to propylene oxide with gt 99 selectivity at 305 K in acetonitrile using015 mol catalyst (15 mol W) in 10 h (Fig 424) [49] This catalyst could berecovered and reused at least five times
ldquoGreenrdquo versions of the Venturello system have been developed A smart re-coverable phosphatetungstic acid was obtained by using tributylphosphate as acosolvent in combination with a quaternary ammonium cetylpyridinium cation-[C5H5NC16H33]3[PO4(WO3)4] [50] This soluble material oxidizes propene with30 H2O2 at 35 C and the reduced catalyst precipitates out once hydrogen per-oxide is consumed Heterogeneous versions of the Venturello-catalyst [51] havebeen obtained by direct support on ion-exchange resins [52] Another approachis to heterogenize the quaternary ammonium functions that charge-balance theanionic W-catalysts as in PW4-amberlite [52] Other peroxotungstates can also beimmobilized cetylpyridium-dodecatungstates were immobilized on fluoroapatiteand employed under anhydrous solvent-free conditions [53] Furthermore perox-otungstate was immobilized on ionic liquid-modified silica and used as a cata-lyst in acetonitrile [54] In general these catalysts are subject to low productiv-ities A much more active heterogeneous W-system was obtained by combininga [WO4]2ndash-exchanged LDH catalyst with NH4Br [55] In this case W catalyzes theoxidation of the bromide ions The thus formed bromohydrin is converted intothe epoxide Interesting activities could be observed for eg -methylstyrenewith H2O2 in the presence of NH4Br at 40 C which produces almost 50 g ofepoxide per g [WO4]2ndash-LDH catalyst within 5 h with 95 epoxide selectivity [55]
4312 Rhenium CatalystsIn the early 1990s Herrmann and coworkers [56] reported the use of methyl-trioxorhenium (MTO) as a catalyst for epoxidation with anhydrous H2O2 in tert-butanol In the initial publication cyclohexene oxide was obtained in 90 yieldusing 1 mol MTO at 10 C for 5 h At elevated temperatures (82 C) the corre-
4 Catalytic Oxidations150
Fig 423 Oxidative cleavage of cyclohexene using tungstate catalyst
Fig 424 Silicotungstate as recyclable catalyst for epoxidation
sponding trans-diol was obtained (97 yield) owing to the acidity of the systempromoting ring opening of the epoxide Subsequently the groups of Herrmann[57] and Sharpless [58] significantly improved the synthetic utility of MTO byperforming reactions in the presence of 10ndash12 mol of heterocyclic bases egpyridine [58] 3-cyanopyridine [58] and pyrazole [57] in a dichloromethanewatermixture For example using the MTO-pyrazole system high activities and epox-ide selectivities were obtained [57] with a variety of olefins using 35 aqueousH2O2 and 05 mol MTO The use of 222-trifluoroethanol further enhancesthe catalytic performance of the MTObasehydrogen peroxide system by athree- to ten-fold increase in TOF [59 60] In the epoxidation of cyclohexeneturnover numbers of over 10 000 could be achieved by slow addition of the sub-strate Notably the use of perfluorinated alcohols in the absence of catalysts al-ready leads to significant epoxidation [60 61] This observation that fluorinatedalcohols are able to activate hydrogen peroxide is tentatively attributed to thecharacteristic feature of highly fluorinated alcohols owing to the strong elec-tron-withdrawing effect of the perfluoroalkyl groups the hydroxy group is veryelectron poor and unable to accept a hydrogen bond but at the same time easi-ly donates a hydrogen bond In this way the perfluorinated alcohol acts as a Le-wis acid and increases the electrophilicity of the hydrogen peroxide
MTO-catalyzed epoxidations proceed via a peroxometal pathway involving a di-peroxorhenium(VII) complex as the active oxidant (see Fig 425) Major disad-vantages of MTO are its limited stability under basic H2O2 conditions [62] andits rather difficult and hence expensive synthesis
4313 Ruthenium CatalystsThe systems described above all involve peroxometal species as the active oxi-dant In contrast ruthenium catalysts involve a ruthenium-oxo complex as theactive oxidant [1] Until recently no Ru-catalysts were known that were able toactivate H2O2 rather then to decompose it However in 2005 Beller and co-work-ers recognized the potential of the Ru(terpyridine)(26-pyridinedicarboxylate) cat-alyst [63] for the epoxidation of olefins with H2O2 [64] The result is a very effi-cient method for the epoxidation of a wide range of alkyl substituted or allylicalkenes using as little as 05 mol Ru In Fig 426 details are given Terminal
43 Alkenes 151
Fig 425 MTO-Catalyzed epoxidations with H2O2
olefins are not very active under these conditions This system can be operatedunder neutral conditions which makes it suitable for the synthesis of acid-sen-sitive epoxides as well
4314 Manganese CatalystsManganese-based catalysts probably involve an oxomanganese(V) complex as theactive oxidant Montanari and coworkers [65] described the use of a mangane-se(III) complex of a halogenated porphyrin in the presence of hexylimidazoleand benzoic acid for epoxidations with 30 H2O2 in dichloromethanendashwaterMore recently Hage and coworkers [66] showed that a manganese(II) complexof trimethyl-147-triazacyclononane (tmtacn) originally developed as a bleach ac-tivator for application in detergents is a highly active catalyst for epoxidations withH2O2 in aqueous methanol In the original publication a vast excess of H2O2 wasneeded owing to competing manganese-catalyzed decomposition of the H2O2Subsequent detailed investigations of this system by Jacobs and De Vos and co-workers [67] culminated in the development of an optimized system comprisingMn(II)-tmtacn (01 mol) in the presence of oxalate buffer (03 mol) with 35H2O2 (15 eq) in acetonitrile at 5 C This system is an extremely active catalyst forthe epoxidation of even relatively unreactive olefins Mechanistic details are uncer-tain but it would seem likely that the active oxidant is an oxomanganese(IV) or (V)[68] complex containing one tmtacn and one oxalate ligand (see Fig 427)
Recently it has been shown that simple manganese sulfate in the presence ofsodium bicarbonate is reasonably effective in promoting the epoxidation of alkeneswith aqueous H2O2 using DMF or t-BuOH as solvents [69] In this system peroxo-carbonate is formed in situ thus minimizing the catalase activity of the Mn saltFollowing this discovery Chan and coworkers introduced an imidazole-based ionic
4 Catalytic Oxidations152
Fig 426 Ru(terpyridine)(26-pyridinedicarboxylate) catalysed epoxidations
liquid in the Mnbicarbonate system in order to overcome the requirements of vol-atile organic cosolvents (see Fig 428) [70] A major disadvantage of these Mn saltsystems is that 10 equivalents of H2O2 are still required to reach substantial con-versions Moreover simple terminal olefins cannot be oxidized in this way
In addition recently it was found that by using peracetic acid as the oxidantMnII(bipy)2 becomes an extremely active catalyst A turnover frequency over200000 hndash1 was found for 1-octene using 2 equivalents of peracetic acid in acet-onitrile [71] In spite of this high activity the system above with Mn-tacn andH2O2 would be preferred because of the safety issues associated with peraceticacid and the coproduction of acetic acid
4315 Iron CatalystsMechanistically related to Mn is the use of Fe as an epoxidation catalyst Re-cently iron complexes with a tetradentate amine core were reported that werecapable of activating H2O2 without the involvement of hydroxyl radicals [72]For a variety of substituted as well as terminal alkenes effective epoxidation
43 Alkenes 153
Fig 427 Mn-tmtacn catalyzed epoxidation with H2O2
Fig 428 Mnbicarbonate system for epoxidation in ionic liquid
was described using 3 mol of Fe 30 mol acetic acid and 15 eq of 50H2O2 (see Fig 429) [73] For a variety of substituted as well as terminal alkenescomplete conversion of the alkene was obtained leading to 77ndash85 isolatedyields Acetic acid was essential to obtain high epoxide yields Investigationsshowed that under reaction conditions with the acid peracetic acid is formedand that the iron(II) complex self-assembled into a -oxo carboxylate bridgeddiiron(III) complex resembling the diiron(III) core found in the active site ofthe oxidized enzyme methane monooxygenase (MMO) The results obtained byJacobsen are amongst the best obtained so far in epoxidation using iron cata-lysts and hydrogen peroxide At the same time Que showed that analogs of thisiron complex led to asymmetric cis-dihydroxylation of olefins (see below) [74]In addition it was found that in situ prepared iron catalysts from ferric perchlo-rate or ferric nitrate and phenanthroline ligands are very active catalysts withperacetic acid as the oxidant and acetonitrile as solvent [75] TOFs of the orderof 5000 hndash1 were obtained for a variety of terminal and internal olefins A majordisadvantage is of course the requirement for peracetic acid (see above for Mn)
4316 Selenium and OrganocatalystsFinally organic compounds and arylseleninic acids have been described as cata-
lysts for epoxidations with H2O2 Perfluoroheptadecan-9-one was shown [76] tobe a recyclable catalyst for the epoxidation of relatively reactive olefins with 60aqueous H2O2 in 222-trifluoroethanol The discovery that hydrogen peroxidecan be used in conjunction with catalytic amounts of peroxyseleninic acidsdates from 1978 [77] Recently 35-bis(trifluoromethyl)benzeneseleninic acid wasused as the catalyst and even sensitive epoxides could be formed in nearlyquantitative yields using SC ratios as high as 200 (see Fig 430 and Table 45)[78] In these reactions bis(35-bis(trifluoromethyl)phenyl)-diselenide is the start-ing compound which under reaction conditions gives the seleninic acid (seeFig 430) Under these optimised conditions turnover frequencies of over1000 hndash1 were observed at room temperature
It is clear from the preceding discussion that several systems are now avail-able for epoxidations with aqueous H2O2 The key features are compared in Ta-ble 45 for epoxidation of cyclohexene and a terminal olefin They all have theirlimitations regarding substrate scope eg TS-1 is restricted to linear olefins and
4 Catalytic Oxidations154
Fig 429 Fe-tetradentate amine complexes as catalysts inepoxidation with H2O2acetic acid
43 Alkenes 155
Fig 430 Aromatic seleninic acids as catalysts for epoxidation
Table 45 Catalytic epoxidation with H2O2 state of the art
CatalystRef
Mn a)
67W b)
48Re c)
57Re d)
59Se e)
78Ru f)
64Ti g)
41SCSolventTemp (C)1-AlkeneYield ()TOF (hndash1) i)
CyclohexeneYield ()TOF (hndash1) i)
666CH3CN5
992000
83550
50PhCH3
90
8112
j)
j)
200CH2Cl225
9914
99198
1000CF3CH2OH25
9948
992000
200CF3CH2OH20
2513
981000
200TAA h)
25
ndashndash
84 k)
14
100CH3OH25
74108
ll
a) Mn(tmtacn)oxalate bufferb) WO4
2ndashH2NCH2PO3H2(C8H17)3MeN+HSO4ndash
c) CH3ReO3pyrazole (12 mol)d) CH3ReO3pyrazole (10 mol)e) 025 mol bis(35-bis(trifluoromethyl) phenyldiselenidef) Ru(terpyridine)(pyridinedicarboxylate)g) TS-1 (=titanosilicalite)h) TAA = tert-amylalcoholi) mol productmol cathj) Gives adipic acid via ring openingk) Activity for 1-methyl-cyclohexene This substrate is more nu-
cleophilic and therefore more reactive [l] Essentially noreaction
W gives ring opening with acid-sensitive epoxides or the solvent required forgood results eg dichloromethane (MTO) and acetonitrile (Mn-tmtacn) Hencethe quest for even better systems continues
4317 Hydrotalcite and Alumina SystemsRelatively simple solid materials like hydrotalcites and clays can also act as cata-lysts for epoxidation in the presence of H2O2 In the case of anionic clays likeMg10Al2(OH)24CO3 these materials are basic enough to promote nucleophilicepoxidations [79] For ldquonormalrdquo electrophilic epoxidation nitrile and amide addi-tives are required [80] It must however be recognized that these materials arepolynuclear-alumina clays and simple alumina will also catalyze this reactionswithout additives [81] A variety of alumina-materials can absorb hydrogen per-oxide onto that surface forming an active oxidant (alumina-OOH) Reactionscould be carried out using ethylacetate as the solvent which is a cheap and en-vironmentally attractive solvent The major limitation of this system is the lowtolerance towards water and to overcome this problem reactions need to be car-ried out under Dean-Stark conditions Furthermore selectivities are usually inthe 70ndash90 range Notably the epoxide of -pinene which is very unstable wasalso obtained in a reasonable 69 yield [81]
4318 Biocatalytic SystemsA variety of monooxygenases (see above) can perform epoxidations Some bio-
catalytic methods come into sight which will become attractive for industrialuse In these cases chiral epoxides are the targeted products and therefore thissubject will be dealt with in Section 46
432Vicinal Dihydroxylation
The osmium-catalyzed vicinal dihydroxylation of olefins with single oxygen do-nors typically TBHP or N-methylmorpholine-N-oxide (NMO) has been knownfor more than two decades [82] and forms the basis for the Sharpless asym-metric dihydroxylation of olefins (see below) The reaction involves an oxometalmechanism in which it is generally accepted that oxoosmium(VIII) undergoesan initial 2 + 2 cycloaddition to the olefin to give an oxametallocycle which sub-sequently rearranges to an osmium(VI)-diol complex (Fig 431) [83] This is fol-lowed by rate-limiting reaction with the oxidant to afford the diol product withconcomitant regeneration of osmium tetroxide Recently the scope of this meth-od was extended to electron-deficient olefins such as -unsaturated amides byperforming the reaction at acidic pH Citric acid (25 mol) was identified asthe additive of choice and 11 equivalent of NMO was required as oxidant [84]
Beller and coworkers [85] showed that osmium-catalyzed dihydroxylations canbe performed successfully with dioxygen as the primary oxidant (Fig 432)
4 Catalytic Oxidations156
Using potassium osmate (05ndash2 mol) in the presence of an organic base egquinuclidine in aqueous tert-butanol at pH 104 a variety of olefins was con-verted to the corresponding vic-diols in high yield Apparently reoxidation of os-mium(VI) to osmium(VIII) with dioxygen is possible under alkaline conditionsWhen chiral bases were used asymmetric dihydroxylation was observed (seeSection 47) albeit with moderate enantioselectivities
43 Alkenes 157
Fig 431 Mechanism of osmium-catalyzed vicinal dihydroxylation of olefins
Fig 432 Osmium-catalyzed dihydroxylations using air as the oxidant
Fig 433 Heterogeneous acid-catalyzed dihydroxylation of olefins
Osmium is unrivalled as catalyst for the asymmetric cis-dihydroxylation ofolefins However Sato and coworkers reported that the perfluorosulfonic acidresin Nafionreg (see Chapter 2) is an effective catalyst for the trans-dihydroxyla-tion of olefins with H2O2 [86] The method is organic solvent-free and the cata-lyst can be easily recycled (see Fig 433) The first step of this reaction is epoxi-dation which is probably carried out by resin-supported peroxysulfonic acidformed in situ This is followed by acid-catalyzed epoxide-ring opening
433Oxidative Cleavage of Olefins
It has long been known that oxidative cleavage of olefinic double bonds occurswith stoichiometric amounts of the powerful oxidant rutheniumtetroxide [87]Ruthenium-catalyzed oxidative cleavage has been described with various oxygendonors eg NaIO4 [88 89] and NaOCl [90] as the primary oxidant The presumedcatalytic cycle in which RuO4 is the active oxidant is shown in Fig 434 Variousattempts have been made to introduce a green element in this reaction ie recycl-able heterogenous Ru-nanoparticles [91] and environmentally acceptable solvents[92] but the main problem of the oxidant has not been solved
From an economic viewpoint it would obviously be advantageous if hydrogenperoxide or even dioxygen could be used as the primary oxidant Unfortunatelyruthenium compounds generally catalyze rapid non-productive decompositionof hydrogen peroxide [93] However a bimetallic system comprising MoO3RuCl3 for the oxidative cleavage of olefins with H2O2 in tert-butanol has beendescribed [94] For optimum performance a small amount of a carboxylic acidwhich could be the product of the oxidative cleavage was added Presumablythe reaction involves initial molybdenum-catalyzed conversion to the vic-diol viathe epoxide followed by ruthenium-catalyzed oxidative cleavage of the diol
4 Catalytic Oxidations158
Fig 434 A catalytic cycle forruthenium-catalyzed oxidativecleavage of olefins
Methodologies for the oxidative cleavage of olefins still in our opinion leavesomething to be desired Bearing in mind the osmium-catalyzed aerobic dihy-droxylation of olefins (see Section 432) and the ruthenium-catalyzed aerobicoxidations of alcohols and cleavage of diols (see below) one cannot help wonder-ing if conditions cannot be designed for the ruthenium-catalyzed aerobic oxida-tive cleavage of olefins Indeed for compounds like styrene and stilbene up to80 yield can be obtained for oxidative cleavage at 130 C using 0004 mol ofa RuCl2ndashPNNP complex [95] Alternatively a combination of osmium and ruthe-nium might be expected to have this capability
Another possibility is the use of tungsten which has led to excellent resultsfor the conversion of cyclohexene to adipic acid (see Fig 423) [48] For linearolefins using the Venturello-system oxidative cleavage products can be obtainedin around 80 yield [96]
434Oxidative Ketonization
The selective aerobic oxidations of ethene to acetaldehyde and terminal alkenesto the corresponding methyl ketones in the presence of a PdCl2CuCl2 catalystare collectively referred to as Wacker oxidations [97] The reaction involves hy-droxypalladation of the olefin via nucleophilic attack of coordinating hydroxideon a palladiumndasholefin complex followed by a -hydride shift to give the acetal-dehyde (or methyl lketone) product and palladium(0) (Fig 435) The latter un-dergoes copper-catalyzed reoxidation with dioxygen The presence of chlorideions at acidic pH is necessary for a reasonable rate of reoxidation and to preventthe formation of palladium clusters
A major disadvantage of the Wacker system is the extremely corrosive natureof (acidic) aqueous solutions of PdCl2 and CuCl2 which necessitates the use ofcostly titanium alloys as materials of construction With higher olefins oxidationrates are lower and complex mixtures are often formed as a result of competingpalladium-catalyzed isomerization of the olefin Research has been focused ondeveloping acid-free PdCl2CuCl2 catalyzed Wacker oxidations using ionic liquid[98] ionic liquidScCO2 [99] and heterogeneous Pd montmorillonite [100]
However all these systems suffer from high concentrations of chloride ionso that substantial amounts of chlorinated by-products are formed For thesereasons there is a definite need for chloride- and copper-free systems for Wackeroxidations One such system has been recently described viz the aerobic oxida-tion of terminal olefins in an aqueous biphasic system (no additional solvent)
43 Alkenes 159
Fig 435 PdCl2CuCl2 catalyzed Wacker oxidation
catalyzed by water-soluble palladium complexes of bidentate amines such as sul-fonated bathophenanthroline (see Fig 436) [101]
Moreover it was disclosed that PdCl2 in combination with NN-dimethylaceta-mide (DMA) solvent could offer a simple and efficient catalyst system for acid-and Cu-free Wacker oxidation [102] The reaction is illustrated in Fig 437 Awide range of terminal olefins could be oxidized to form the correspondingmethyl ketones in high yields reaching a TOF up to 17 hndash1 The Pd-DMA cata-lyst layer could be recycled Furthermore this system is also capable of per-
4 Catalytic Oxidations160
Fig 436 Water-soluble palladium complexes for Wacker oxidation
Fig 437 PdCl2NN-dimethylacetamide system for Wacker oxidation of olefins
Fig 438 PdCl2NN-dimethylacetamide system forregioselective acetoxylation of terminal olefins
forming regioselective acetoxylation of terminal olefins to linear allylic acetates(see Fig 438) This system shows a strong resemblance to the Baumlckvall system(see below and Fig 441) [103]
In this context it is also worth mentioning that Showa Denko has developed anew process for the direct oxidation of ethene to acetic acid using a combinationof palladium(II) and a heteropoly acid [104] However the reaction probably in-volves heteropoly acid-catalyzed hydration followed by palladium-catalyzed aerobicoxidation of ethanol to acetic acid rather than a classical Wacker mechanism
435Allylic Oxidations
Classical (metal-catalyzed) autoxidation of olefins is facile but not syntheticallyuseful owing to competing oxidation of allylic CndashH bonds and the olefinic doublebond leading to complex product mixtures [105] Nonetheless the synthetic che-mist has a number of different tools for the allylic oxidation of olefins available
Stoichiometric oxidation with SeO2 became more attractive after Sharplessshowed that the reaction could be carried out with catalytic amounts of SeO2
and TBHP as the (re)oxidant [106] The reaction involves an oxometal mecha-nism (see Fig 439) The use of fluorous seleninic acids with iodoxybenzene asoxidant introduces the possibility of recycling the catalyst [107]
Allylic oxidation (acyloxylation) can also be achieved with copper catalysts andstoichiometric amounts of peresters or an alkylhydroperoxide in a carboxylicacid as solvent [108] via a free radical mechanism (Fig 440) The use of water-soluble ligands [109] or fluorous solvents [110] allows recycling of the coppercatalyst In view of the oxidants required this reaction is economically viableonly when valuable (chiral) products are obtained using asymmetric copper cata-lysts [111ndash113] The scope of the reaction is rather limited however
Arguably the best or at least the most versatile allylic oxidation method isbased on Pd [114] Since the intermediates are palladium-allyl complexes ratherthan free radicals the number of by-products is limited compared to the preced-ing examples (Fig 441) Furthermore a large number of nucleophiles (aminesalcohols stabilized carbanions carboxylates or halides) may attack the palla-dium-allyl complex giving a wide variety of products
43 Alkenes 161
Fig 439 Selenium-catalyzed allylic oxidation of olefins
Fig 440 The KharaschndashSosnovsky reaction for allylic oxidation of olefins
In the group of Baumlckvall a method was developed involving palladium andbenzoquinone as cocatalyst (Fig 442) [103] The difficulty of the catalytic reac-tion lies in the problematic reoxidation of Pd(0) which cannot be achieved by di-oxygen directly (see also Wacker process) To overcome this a number of elec-tron mediators have been developed such as benzoquinone in combinationwith metal macrocycles heteropolyacids or other metal salts (see Fig 442) Al-ternatively a bimetallic palladium(II) air oxidation system involving bridgingphosphines can be used which does not require additional mediators [115]This approach would also allow the development of asymmetric Pd-catalyzedallylic oxidation
44Alkanes and Alkylaromatics
One of the remaining ldquoholy grailsrdquo in catalysis is undoubtedly the selective oxi-dation of unfunctionalized hydrocarbons such as alkanes [116] Generallyspeaking the difficulty lies in the activation of the poorly reactive CndashH bondsand stabilization of a product which is often more reactive than the starting ma-terial There are few notable exceptions eg the gas phase oxidation of butaneto maleic anhydride (a highly stable product) and isobutane to tert-butylhydro-peroxide (a highly reactive tertiary CndashH bond) The aerobic oxidation of cyclo-
4 Catalytic Oxidations162
Fig 441 Pd-catalyzed allylic oxidation of olefins
Fig 442 The Pdmediator approach for allylic oxidation of olefins
hexane to cyclohexanolcyclohexanone ndash the starting material for adipic acidused on a million tonnes scale for the manufacture of nylon-66 ndash is more chal-lenging [117] Since the substrate lacks reactive CndashH bonds and the productcannot be stabilized the reaction is stopped at lt 10 conversion to preventfurther oxidation affording a roughly 1 1 mixture of cyclohexanolcyclohexa-none in ca 80 selectivity
As noted in Section 42 the selective oxidation of unreactive CndashH bonds withdioxygen is fraught with many problems eg the oxidative destruction of organ-ic ligands and competition with free radical oxidation pathways For this reasonmost biomimetic systems employ sacrificial reductants or a reduced form of di-oxygen eg H2O2 [118] One extensively studied class of biomimetic catalystscomprises the so-called Gif-systems [119] which were believed to involve directinsertion of high-valent oxoiron(V) species into CndashH bonds However more re-cent results suggest that classical free radical mechanisms may be involved[120]
441Oxidation of Alkanes
Classical autoxidation of tertiary CndashH bonds in alkanes can afford the corre-sponding hydroperoxides in high selectivities This is applied industrially in theconversion of pinane to the corresponding hydroperoxide an intermediate inthe manufacture of pinanol (Fig 443)
More reactive hydroperoxides can be converted selectively to alcohols via themethod of Bashkirov (Fig 444) where a boric acid ester protects the productfrom further oxidation and thus increases the selectivity [121] The method isused to convert C10ndashC20 paraffins to alcohols which are used as detergents andsurfactants for the oxidation of cyclohexane (see elsewhere) and cyclododecaneto cyclododecanol (cyclododecanone) for the manufacture of nylon-12
44 Alkanes and Alkylaromatics 163
Fig 443 Selective oxidation of pinane
Fig 444 Bashkirov method for conversion of alkanes to alcohols
For less reactive hydrocarbons more drastic measures are required High va-lent metal compounds especially ruthenium compounds [122] can react withhydrocarbons but usually more than stoichiometric amounts of peracids or per-oxides are required to reach the high oxidation state of the metal (eg RuVI)One of the very few examples in which a clean oxidant (H2O2 or O2) is usedwas reported by Drago et al using a cis-dioxoruthenium complex (Fig 445 a)In both cases a free radical mechanism could not be excluded however [123]In a variation on this theme Catalytica researchers described the direct oxidationof methane to methanol using a platinum-bipyrimidine complex in concen-trated sulfuric acid (Fig 445 b) [124] Analogous to the Bashkirov method thesulfuric acid protects the methanol via esterification from overoxidation to(eventually) CO2 and H2O which is a highly thermodynamically favorable pro-cess
Recently the CoMnN-hydroxyphthalimide (NHPI) systems of Ishii havebeen added to the list of aerobic oxidations of hydrocarbons including both aro-matic side chains and alkanes For example toluene was oxidized to benzoicacid at 25 C [125] and cyclohexane afforded adipic acid in 73 selectivity at73 conversion [126] see Fig 446 A related system employing N-hydroxysac-charine instead of NHPI was reported for the selective oxidation of large ringcycloalkanes [127]
4 Catalytic Oxidations164
Fig 445 Approaches for selective conversion of methane tomethanol using O2 or H2O2 as oxidants
a)
b)
The role of NHPI seems to be analogous to that of bromide ions during aut-oxidation processes Bromide ion has a pronounced synergistic effect on metal-catalyzed autoxidations [128ndash130] This results from a change in the chain-pro-pagation step from hydrogen abstraction by alkylperoxy radicals to the energeti-cally more favorable hydrogen abstraction by bromine atoms (Fig 447) Thebromine atoms are formed by one-electron oxidation of bromide ions by for ex-ample cobalt(III) or manganese(III) generally a more favorable process thanone-electron oxidation of the hydrocarbon substrate
442Oxidation of Aromatic Side Chains
The power of lsquogreen chemistryrsquo is nicely illustrated by reference to the produc-tion of aromatic acids Classical methods using chlorine or nitric acid have beenlargely displaced by catalytic oxidations with dioxygen (see Fig 448) This leadsto high atom utilization low-salt technology no chloro- or nitro-compounds asby-products and the use of a very cheap oxidant
Oxidation of hydrocarbons with dioxygen is more facile when the CndashH bondis activated through aromatic or vinylic groups adjacent to it The homolytic CndashH bond dissociation energy decreases from ca 100 kcal molndash1 (alkyl CndashH) to ca85 kcal molndash1 (allylic and benzylic CndashH) which makes a number of autoxidationprocesses feasible The relative oxidizability is further increased by the presenceof alkyl substituents on the benzylic carbon (see Table 46) The autoxidation ofisopropylbenzene (Hock process Fig 449) accounts for the majority of theworld production of phenol [131]
In the AmocoMC process terephthalic acid (TPA) is produced by aerobic oxi-dation of p-xylene This bulk chemical (gt 10106 t andash1) is chiefly used for poly-
44 Alkanes and Alkylaromatics 165
Fig 446 NHPI as cocatalyst for aerobic oxidation of toluene and cyclohexane
Fig 447 Synergistic effect of bromide ions and NHPI compared
etheneterephthalate (PET a polymer used in eg plastic bottles) The solvent ofchoice is acetic acid which shows a high solubility for substrates and low forproducts is safe recyclable (up to 40 times) has a wide temperature range andis relatively inert [132] although some solvent is ldquoburntrdquo into CO2 and H2O(Fig 450)
The rather drastic conditions are required because in this particular case theCOOH group deactivates the intermediate p-toluic acid towards further oxidationand some p-carboxybenzaldehyde is found as a side-product which is hydroge-nated back to p-toluic acid Other than that a large number of functional groupsare tolerated (see Table 47) [129] The combination of cobalt manganese and bro-mide ions is essential for optimum performance The benzylic radicals are bestgenerated with bromine atoms (see above) which in turn are more easily produced
4 Catalytic Oxidations166
Fig 448 Classical versus lsquogreenrsquo aromatic side-chain oxidation
Table 46 Relative oxidizability of aromatic side-chains
Substrate Rel Oxidizability
PhCH3 10PhCH2CH3 15PhCH(CH3)2 107
Fig 449 Hock process for production of phenol
by reaction of bromide with MnIII rather than CoIII (see Fig 451) The resultingperacid however is more easily reduced by CoII than by MnII In the Eastman Ko-dak and related processes fairly large amounts of eg acetaldehyde (021 tt) areused as additives instead of bromide leading to less corrosion
The use of manganese catalysts maintains a low concentration of Co(III) whichis important since the latter promotes extensive decarboxylation of acetic acid at Tgt 130 C A somewhat similar process which operates under biphasic conditionsrather than in acetic acid also gives high conversions and selectivities [133]
44 Alkanes and Alkylaromatics 167
Fig 450 AmocoMC process for the production of terephthalic acid
Table 47 Tolerance of functional groups in CoMnBr-catalyzed aerobic oxidation of substituted toluenes a)
Complete conversion90ndash98 yield
Side reactions30ndash70 yield
Total radical consumptionno yield
F Cl Br (omp) OAc (mp) I (omp)OCH3 (p) OCH3 (om) OH (omp)OPh (mp) NHAc (mp) NH2 (omp)COOH (mp) COOH (o) OPh (o)NO2 (mp) Ph (o) NO2 (o)Ph (mp) SO2NH2 (o)COPh (omp)SO2NH2 (mp)SO2R (mp)POR2 (omp)
a) Taken from Ref [129]
Fig 451 Mechanism for the aerobic oxidation of aromatic side-chains
Lonza has succesfully developed a biocatalytic method for the oxidation of alkylgroups on aromatic heterocycles [5] The oxidation is carried out in a fermenterusing Pseudomonas putida grown on xylenes as the microorganism Product con-centrations of up to 24 g Lndash1 could be reached Another microorganism Pseudome-nas oleoverans grown on n-octane could be used for the terminal oxidation of ethylgroups (see Fig 452) These are important examples of industrial biocatalystic ap-plications where the high selectivity and activity demonstrated by enzymes forthese difficult alkane transformations has a clear advantage The reactions needto be carried out with living cells because the monoxygenase enzymes which car-ry out these transformations are cofactor-dependent (see Chapter 1 Section 12)The success of this methodology is related to the relatively high water-solubilityof these heterocycles which makes them more amenable to oxidation by enzymes
Another example of industrially viable biooxidation of N-heterocycles sidechain oxidation is the oxidation of 2-methylquinoxaline to 2-quinoxalinecar-boxylic acid by Pfizer [134]
443Aromatic Ring Oxidation
Oxidation of aromatic rings is quite complicated for a number of reasonsFirstly radical intermediates preferentially abstract hydrogen atoms from thearomatic side chain rather than the nucleus (the dissociation energies of theArndashH bond and the ArCR2ndashH bond are 110 kcal molndash1 and 83 kcal molndash1respectively) Secondly the phenol products are much more reactive towards oxi-dation than the hydrocarbon substrates Recently a solution was found to theproblem of over-oxidation by using aqueous-organic solvent mixtures The opti-mum conditions are represented in Fig 453 As catalyst FeSO4 which is a con-ventional Fenton catalyst was applied in the presence of 5-carboxy-2-methylpyr-azine N-oxide as ligand and trifluoroacetic acid as cocatalyst [135] The choice ofthe NO ligand turned out to be crucial Using 10-fold excess of benzene to hy-drogen peroxide 97 selectivity of phenol (relative to benzene) could beachieved at almost full conversion of H2O2 Similar results could be obtained byusing aqueous-ionic liquid biphasic mixtures and iron-dodecanesulfonate saltsas catalyst [136]
4 Catalytic Oxidations168
Fig 452 Biocatalytic oxidation of alkyl groups on aromatic heterocycles
This technology could also be applied for the oxidation of methane (70 C5 Mpa) to formic acid (46 selectivity based on hydrogen peroxide) Anothercatalyst which can be applied for the direct oxidation of benzene with H2O2 isthe TS-1 catalyst as described above for propylene epoxidation [41] Conversionis generally kept low because introduction of a hydroxy group activates the aro-matic nucleus to further oxidation to hydroquinone catechol and eventually totarry products [137]
Arguable the best technology ndash due to its simplicity ndash for directly convertingbenzene to phenol is represented by the Fe-ZSM-5N2O gas phase technologyas developed by Panov and coworkers [138] Nitrous oxide is the terminal oxi-dant and MFI-type zeolite-containing low amounts (lt10 wt) of iron acts asthe catalyst The use of N2O instead of oxygen circumvents the occurrence offree radical reactions In this way highly selective conversion to phenol (gt 95)could be reached at 350 C (Fig 454) The technology was adopted by Monsan-to but no chemical plant was built Oxidation of other aromatics and alkenesusing this technology generally leads to low selectivities
For the direct hydroxylation of N-heterocycles a microbial oxidation is mostsuitable Lonza developed a process to produce 6-hydroxynicotinic acid on a10 tonnes scale [5] The enzymatic production is carried out in two-steps FirstlyAchromobacter xylosoxydans LK1 biomass is produced which possesses a highly
44 Alkanes and Alkylaromatics 169
Fig 453 Direct oxidation of benzene to phenol using H2O2
Fig 454 Direct oxidation of benzene to phenol using N2O as the terminal oxidant
Fig 455 Hydroxylation of nicotinic acid
active nicotinic acid hydroxylase In the second step the biomass is used for thehydroxylation (Fig 455) The impressive yield of gt 99 is due to the selectivityof the enzyme involved
45Oxygen-containing Compounds
451Oxidation of Alcohols
The oxidation of primary and secondary alcohols into the corresponding carbon-yl compounds plays a central role in organic synthesis [1 139 140] Traditionalmethods for performing such transformations generally involve the use of stoi-chiometric quantities of inorganic oxidants notably chromium(VI) reagents[141] However from both an economic and environmental viewpoint atom effi-cient catalytic methods that employ clean oxidants such as O2 and H2O2 aremore desirable
The catalytic oxidation of alcohols is a heavily studied field where many me-tals can be applied New developments in the 21st century can be discernedsuch as the use of nanocatalysts (notably Pd and Au) which combine high sta-bility with a high activity Furthermore catalysis in water and the use of non-no-ble metals such as copper are important green developments Thus both homo-geneous and heterogeneous catalysts are employed In addition biocatalysis ison the rise In combination with a mediator the copper-dependent oxidase lac-case is very promising for alcohol oxidation Furthermore alcohol dehydro-genases can also be employed for (asymmetric) alcohol oxidation by using acet-one as a cosubstrate It should be noted that hydrogen peroxide is not reallyneeded for alcohol conversion compared to the use of oxygen it has little advan-tage The focus in this section will therefore be on molecular oxygen For acomplete overview in this field the reader is referred to reviews on this topic[142ndash144] We will start with some mechanistic aspects and a separate sectionhighlighting the green aspects of using industrially important oxoammoniumions as catalyst The latter methodology is widely used in industrial batch pro-cesses
As discussed above metal-catalyzed oxidations with hydrogen peroxide or al-kyl hydroperoxide can be conveniently divided into two categories involving per-oxometal and oxometal species respectively as the active oxidant [13] This is il-lustrated for alcohol oxidations in Fig 456 [4] In the peroxometal pathway themetal ion does not undergo any change in oxidation state during the catalyticcycle and no stoichiometric oxidation is observed in the absence of H2O2 Incontrast oxometal pathways involve a two-electron change in oxidation state ofthe metal ion and a stoichiometric oxidation is observed with the oxidized stateof the catalyst in the absence of H2O2 Indeed this is a test for distinguishingbetween the two pathways
4 Catalytic Oxidations170
In aerobic oxidations of alcohols a third pathway is possible with late transi-tion metal ions particularly those of Group VIII elements The key step in-volves dehydrogenation of the alcohol via -hydride elimination from the metalalkoxide to form a metal hydride (see Fig 457) This constitutes a commonlyemployed method for the synthesis of such metal hydrides The reaction is of-ten base-catalyzed which explains the use of bases as cocatalysts in these sys-tems In the catalytic cycle the hydridometal species is reoxidized by O2 possi-bly via insertion into the MndashH bond and formation of H2O2 Alternatively an al-koxymetal species can afford a proton and the reduced form of the catalysteither directly or via the intermediacy of a hydridometal species (see Fig 457)Examples of metal ions that operate via this pathway are Pd(II) Ru(III) andRh(III) We note the close similarity of the -hydride elimination step in thispathway to the analogous step in the oxometal pathway (see Fig 456) Somemetals eg ruthenium can operate via both pathways and it is often difficult todistinguish between the two
45 Oxygen-containing Compounds 171
Fig 456 Oxometal versus peroxometal pathways for alcohol oxidation
Fig 457 Mechanism for metal catalyzed aerobic oxidation of alcohols
4511 Ruthenium CatalystsRuthenium compounds have been extensively studied as catalysts for the aero-bic oxidation of alcohols [142] They operate under mild conditions and offerpossibilities for both homogeneous and heterogeneous catalysts The activity ofcommon ruthenium precursors such as RuCl2PPh3 can be increased by theuse of ionic liquids as solvents (Fig 458) Tetramethylammoniumhydroxide andaliquatreg 336 (tricaprylylmethylammonium chloride) were used as solvent andrapid conversion of benzyl alcohol was observed [145] Moreover the tetra-methylammonium hydroxideRuCl2(PPh3)3 could be reused after extraction ofthe product
Ruthenium compounds are widely used as catalysts for hydrogen transfer re-actions These systems can be readily adapted to the aerobic oxidation of alco-hols by employing dioxygen in combination with a hydrogen acceptor as a coca-talyst in a multistep process These systems demonstrate high activity For ex-ample Baumlckvall and coworkers [146] used low-valent ruthenium complexes incombination with a benzoquinone and a cobalt-Schiffrsquos base complex Optimiza-tion of the electron-rich quinone combined with the so-called ldquoShvordquo Ru-cata-lyst led to one of the fastest catalytic systems reported for the oxidation of sec-ondary alcohols (Fig 459)
The regeneration of the benzoquinone can also be achieved with dioxygen inthe absence of the cobalt cocatalyst Thus Ishii and coworkers [147] showed thata combination of RuCl2(Ph3P)3 hydroquinone and dioxygen in PhCF3 as sol-vent oxidized primary aliphatic allylic and benzylic alcohols to the correspond-ing aldehydes in quantitative yields
Another example of a low-valent ruthenium complex is the combination ofRuCl2(Ph3P)3 and the stable nitroxyl radical 2266-tetramethylpiperidine-N-oxyl (TEMPO) This system is a remarkably effective catalyst for the aerobic oxi-dation of a variety of primary and secondary alcohols giving the correspondingaldehydes and ketones respectively in gt 99 selectivity [148] The best resultswere obtained using 1 mol of RuCl2(Ph3P)3 and 3 mol of TEMPO(Fig 460) Primary alcohols give the corresponding aldehydes in high selectiv-ity eg 1-octanol affords 1-octanal in gt 99 selectivity Over-oxidation to the cor-responding carboxylic acid normally a rather facile process is completely sup-pressed in the presence of a catalytic amount of TEMPO TEMPO suppressesthe autoxidation of aldehydes by efficiently scavenging free radical intermediates
4 Catalytic Oxidations172
Fig 458 Ruthenium salts in ionic liquids as catalysts for oxidation of alcohols
resulting in the termination of free radical chains ie it acts as an antioxidantAllylic alcohols were selectively converted to the corresponding unsaturated al-dehydes in high yields
Perruthenate catalysts ie TPAP are superior Ru-catalysts which are air-stable non-volatile and soluble in a wide range of organic solvents It wasshown that TPAP is an excellent catalyst for the selective oxidation of a widevariety of alcohols using N-methylmorpholine-N-oxide (NMO) or oxygen as thestoichiometric oxidant [139 149ndash151] In particular polymer-supported perruthe-nate (PSP) prepared by anion exchange of KRuO4 with a basic anion exchangeresin (Amberlyst A-26) has emerged as a versatile catalyst for the aerobic oxida-tion (Fig 461) of alcohols [152] However the activity was ca 4 times lower thanhomogeneous TPAP and this catalyst could not be recycled which was attrib-
45 Oxygen-containing Compounds 173
Fig 459 Low-valent ruthenium complexes in combination with benzoquinone
Fig 460 RutheniumTEMPO catalyzed oxidation of alcohols
uted to oxidative degradation of the polystyrene support PSP displays a markedpreference for primary versus secondary alcohol functionalities [152] The prob-lem of deactivation was also prominent for the homogeneous TPAP oxidationwhich explains the high (10 mol) loading of catalyst required
Recently two heterogeneous TPAP-catalysts were developed which could berecycled successfully and displayed no leaching In the first example the tetra-alkylammonium perruthenate was tethered to the internal surface of mesopor-ous silica (MCM-41) and was shown [153] to catalyze the selective aerobic oxida-tion of primary and secondary allylic and benzylic alcohols Surprisingly bothcyclohexanol and cyclohexenol were unreactive although these substrates caneasily be accommodated in the pores of MCM-41 The second example involvesstraightforward doping of methyl modified silica denoted as ormosil with tetra-propylammonium perruthenate via the solndashgel process [154] A serious disad-vantage of this system is the low-turnover frequency (10 and 18 hndash1) observedfor primary aliphatic alcohol and allylic alcohol respectively
Many examples of heterogeneous ruthenium systems are available One ofthe more promising seems to be ruthenium on alumina which is an active andrecyclable catalyst [155] This system displayed a large substrate scope (seeFig 462) and tolerates the presence of sulfur and nitrogen groups Only pri-mary aliphatic alcohols required the addition of hydroquinone Turnover fre-quencies in the range of 4 hndash1 (for secondary allylic alcohols) to 18 hndash1 (for 2-oc-tanol) were obtained in trifluorotoluene while in the solvent-free oxidation at150 C a TOF of 300 hndash1 was observed for 2-octanol
Ruthenium-exchanged hydrotalcites were shown by Kaneda and coworkers[156] to be heterogeneous catalysts for the aerobic oxidation of reactive allylicand benzylic alcohols Ruthenium could be introduced in the Brucite layer byion exchange [156] The activity of the ruthenium-hydrotalcite was significantlyenhanced by the introduction of cobalt(II) in addition to ruthenium(III) in theBrucite layer [157 ] For example cinnamyl alcohol underwent complete conver-sion in 40 min in toluene at 60 C in the presence of RuCo-HT compared with31 conversion under the same conditions with Ru-HT A secondary aliphatic
4 Catalytic Oxidations174
Fig 461 TPAP catalyzed oxidation of alcohols
alcohol 2-octanol was smoothly converted into the corresponding ketone butprimary aliphatic alcohols eg 1-octanol exhibited extremely low activity Theresults obtained in the oxidation of representative alcohols with Ru-HT and RuCo-HT are compared in Table 48
Other examples of heterogeneous ruthenium catalysts are a ruthenium-basedhydroxyapatite catalyst [158] a ferrite spinel-based catalyst MnFe15Ru035
Cu015O4 [159] and Ru supported on CeO2 [160] which all gave lower activitiesAnother class of ruthenium catalysts which has attracted considerable inter-
est due to their inherent stability under oxidative conditions are the polyoxome-talates [161] Recently Mizuno et al [162] reported that a mono-ruthenium-sub-stituted silicotungstate synthesized by the reaction of the lacunary polyoxometa-late [SiW11O39]8ndash with Ru3+ in an organic solvent acts as an efficient heteroge-neous catalyst with high turnover frequencies for the aerobic oxidation ofalcohols (see Fig 463) Among the solvents used 2-butyl acetate was the most
45 Oxygen-containing Compounds 175
Fig 462 Ru on alumina for aerobic alcohol oxidation
Table 48 Oxidation of various alcohols to their correspondingaldehydes or ketones with Ru-hydrotalcites using molecularoxygen a)
Substrate Ru-Mg-Al-CO3-HT b) Ru-Co-Al-CO3-HTc)
Timeh Yield () Timeh Yield ()
PhCH=CHCH2OH 8 95 067 94PhCH2OH 8 95 1 96PhCH(CH3)OH 18 100 15 100n-C6H13CH(CH3)OH 2 97
a) 2 mmol substrate 03 g hydrotalcite (14 mol) in toluene60 C 1 bar O2
b) Ref [156]c) Ref [157]
effective and this Ru-heteropolyanion could be recycled The low loading usedresulted in very long reaction times of gt 2 days and low selectivities
4512 Palladium-catalyzed Oxidations with O2
Much effort has been devoted to finding synthetically useful methods for the pal-ladium-catalyzed aerobic oxidation of alcohols For a detailed overview the readeris referred to several excellent reviews [163] The first synthetically useful systemwas reported in 1998 when Peterson and Larock showed that simple Pd(OAc)2 incombination with NaHCO3 as a base in DMSO as solvent catalyzed the aerobicoxidation of primary and secondary allylic and benzylic alcohols to the correspond-ing aldehydes and ketones respectively in fairly good yields [164 165] Recently itwas shown that replacing the non-green DMSO by an ionic liquid (imidazole-type)resulted in a three times higher activity of the Pd-catalyst [166]
Uemura and coworkers [167 168] reported an improved procedure involvingthe use of Pd(OAc)2 (5 mol) in combination with pyridine (20 mol) and 3 Aringmolecular sieves in toluene at 80 C This system smoothly catalyzed the aerobicoxidation of primary and secondary aliphatic alcohols to the corresponding alde-hydes and ketones respectively in addition to benzylic and allylic alcoholsAlthough this methodology constitutes an improvement on those previously re-ported turnover frequencies were still generally lt 10 hndash1 and hence there isconsiderable room for further improvement Recent attempts to replace eitherpyridine by triethylamine [169] or Pd(OAc)2 by palladacycles [170] all resultedin lower activities Notably the replacement of pyridine by pyridine derivativeshaving a 2345 tetraphenyl substitutent completely suppressed the Pd black for-mation using only 1 atm air [171] However the reaction times in this case wererather long (3ndash4 days)
A much more active catalyst is constituted by a water-soluble palladium(II)complex of sulfonated bathophenanthroline as a stable recyclable catalyst forthe aerobic oxidation of alcohols in a two-phase aqueous-organic medium egin Fig 464 [16 172 173] Reactions were generally complete in 5 h at 100 C30 bar air with as little as 025 mol catalyst No organic solvent is required(unless the substrate is a solid) and the product ketone is easily recovered byphase separation The catalyst is stable and remains in the aqueous phasewhich can be recycled to the next batch
A wide range of alcohols were oxidized with TOFs ranging from 10 hndash1 to100 hndash1 depending on the solubility of the alcohol in water (since the reactionoccurs in the aqueous phase the alcohol must be at least sparingly soluble inwater) Representative examples of primary and secondary alcohols that were
4 Catalytic Oxidations176
Fig 463 Ru-HPA catalysed oxidation of alcohols
smoothly oxidized using this system are collected in Fig 464 The correspond-ing ketones were obtained in gt 99 selectivity in virtually all cases
Primary alcohols afforded the corresponding carboxylic acids via further oxida-tion of the aldehyde intermediate eg 1-hexanol afforded 1-hexanoic acid in95 yield It is important to note however that this was achieved without therequirement of one equivalent of base to neutralize the carboxylic acid product(which is the case with supported noble metal catalysts) In contrast when1 mol TEMPO (4 equivalents per Pd) was added the aldehyde was obtainedin high yield eg 1-hexanol afforded 1-hexanal in 97 yield Under cosolventconditions using waterethylene carbonate Pd-neocuproine was found to beeven more active (Fig 465) [174] This system is exceptional because of its activ-ity (TOF gtgt 500 hndash1 could be reached for 2-octanol) and functional group toler-ance such as C=C bonds CC bonds halides -carbonyls ethers amines etcThereby this system is expected to have a broad synthetic utility
45 Oxygen-containing Compounds 177
Fig 464 Pd-bathophenanthroline as catalyst for alcohol oxidation in water
Fig 465 Pd-neocuproine as catalyst for alcohol oxidation in watercosolvent mixtures
In the context of heterogeneous palladium catalysts PdC catalysts are com-monly used for water-soluble substrates ie carbohydrates [175] Palladium canalso be introduced in the brucite-layer of the hydrotalcite [176] As with RuCo-hydrotalcite (see above) besides benzylic and allylic also aliphatic and cyclic al-cohols are smoothly oxidized using this palladium-hydrotalcite However a ma-jor shortcoming is the necessity of at least 5 mol catalyst and the co-additionof 20ndash100 mol pyridine A seemingly very active heterogeneous catalyst isPdCl2(PhCN)2 on hydroxyapatite [177] Using trifluorotoluene as the solventvery high TONs (gt 20 000) could be obtained for benzyl alcohol However for ali-phatic alcohols long reaction times were needed (24 h)
Major trends can be discerned for Pd-catalysts aimed at increasing the stabilityand activity First is the use of palladium-carbene complexes [178] Although activ-ities are still modest much can be expected in this area Second is the synthesisand use of palladium nanoparticles For example the giant palladium clusterPd561phen60(OAc)180 [179] was shown to catalyze the aerobic oxidation of primaryallylic alcohols to the corresponding -unsaturated aldehydes (Fig 466) [180]
Some other recent examples are the use of palladium nanoparticles entrappedin aluminum hydroxide [181] resin-dispersed Pd nanoparticles [182] and poly(ethylene glycol)-stabilized palladium nanoparticles in scCO2 [183] Although insome cases the activities for activated alcohols obtained with these Pd-nanoparti-cles are impressive the conversion of aliphatic alcohols is still rather slow
4513 Gold CatalystsRecently gold has emerged as one of the most active catalysts for alcohol oxida-tion and is especially selective for poly alcohols In 2005 Corma [184] and Tsu-kuda [185] independently demonstrated the potential of gold nanoparticles forthe oxidation of aliphatic alcohols For example in the case of gold nanoparti-cles deposited on nanocrystalline cerium oxide [184] a TOF of 12 500 hndash1 wasobtained for the conversion of 1-phenylethanol into acetophenone at 160 C(Fig 467) Moreover this catalyst is fully recyclable Another example of a goldcatalyst with exceptional activity is a 25 Aundash25 PdTiO2 as catalyst [186] Inthis case for 1-octanol a TOF of 2000 hndash1 was observed at 160 C (reaction with-out solvent Fig 467)
As reported below Au is now considered as the catalyst of choice for carbohy-drate oxidation Similarly glycerol can be oxidized to glyceric acid with 100 se-
4 Catalytic Oxidations178
Fig 466 Alcohol oxidation by giant palladium clusters
lectivity using either 1 Aucharcoal or 1 Augraphite catalyst under mild re-action conditions (60 C 3 h water as solvent) [187]
4514 Copper CatalystsCopper would seem to be an appropriate choice of metal for the catalytic oxida-tion of alcohols with dioxygen since it comprises the catalytic centre in a varietyof enzymes eg galactose oxidase which catalyze this conversion in vivo [188189] Several catalytically active biomimetic models for these enzymes have beendesigned which are seminal examples in this area [190ndash193] A complete over-view of this field can be found in a review [194]
Marko and coworkers [195 196] reported that a combination of Cu2Cl2(5 mol) phenanthroline (5 mol) and di-tert-butylazodicarboxylate DBAD(5 mol) in the presence of 2 equivalents of K2CO3 catalyzes the aerobic oxida-tion of allylic and benzylic alcohols (Fig 468) Primary aliphatic alcohols eg 1-decanol could be oxidized but required 10 mol catalyst for smooth conversion
45 Oxygen-containing Compounds 179
Fig 467 Au nanoparticles for alcohol oxidation
Fig 468 Cu-phenanthroline-DBAD catalyzed aerobic oxidation of alcohols
O
An advantage of the system is that it tolerates a variety of functional groupsSerious drawbacks of the system are the low activity the need for two equiva-lents of K2CO3 (relative to substrate) and the expensive DBAD as a cocatalystAccording to a later report [197] the amount of K2CO3 can be reduced to 025equivalents by changing the solvent to fluorobenzene The active catalyst is het-erogeneous being adsorbed on the insoluble K2CO3 (filtration gave a filtrate de-void of activity) Besides fulfilling a role as a catalyst support the K2CO3 acts asa base and as a water scavenger In 2001 Marko et al reported a neutral variantof their CuICl(phen)ndashDBADH2ndashbase system [198] Furthermore it was foundthat 1-methylimidazole as additive in the basic system dramatically enhancedthe activity [199]
The use of Cu in combination with TEMPO also affords an attractive catalyst[200 201] The original system however operates in DMF as solvent and is onlyactive for activated alcohols Knochel et al [202] showed that CuBrMe2S withperfluoroalkyl substituted bipyridine as the ligand and TEMPO as cocatalystwas capable of oxidizing a large variety of primary and secondary alcohols in afluorous biphasic system of chlorobenzene and perfluorooctane (see Fig 469)In the second example Ansari and Gree [203] showed that the combination ofCuCl and TEMPO can be used as a catalyst in 1-butyl-3-methylimidazoliumhexafluorophosphate an ionic liquid as the solvent However in this case turn-over frequencies were still rather low even for benzylic alcohol (around 13 hndash1)
Recently an alternative to the catalytic system described above was reported[204] The new catalytic procedure for the selective aerobic oxidation of primaryalcohols to aldehydes was based on a CuIIBr2(Bpy)ndashTEMPO system (Bpy = 22-bipyridine) The reactions were carried out under air at room temperature andwere catalyzed by a [copperII(bipyridine ligand)] complex and TEMPO and base(KOtBu) as co-catalysts (Fig 470)
Several primary benzylic allylic and aliphatic alcohols were successfully oxi-dized with excellent conversions (61ndash100) and high selectivities The systemdisplays a remarkable selectivity towards primary alcohols This selectivity for
4 Catalytic Oxidations180
Fig 469 Fluorous CuBr2-bipy-TEMPO system for alcohol oxidation
the oxidation of primary alcohols resembles that encountered for certain copper-dependent enzymes In the mechanism proposed TEMPO coordinates side-onto the copper during the catalytic cycle
4515 Other Metals as Catalysts for Oxidation with O2
Co(acac)3 in combination with N-hydroxyphthalimide (NHPI) as cocatalystmediates the aerobic oxidation of primary and secondary alcohols to the corre-sponding carboxylic acids and ketones respectively eg Fig 471 [205] By ana-logy with other oxidations mediated by the CoNHPI catalyst studied by Ishiiand coworkers [206 207] Fig 471 probably involves a free radical mechanismWe attribute the promoting effect of NHPI to its ability to efficiently scavengealkylperoxy radicals suppressing the rate of termination by combination of al-kylperoxy radicals (see above for alkane oxidation)
After their leading publication on the osmium-catalyzed dihydroxylation ofolefins in the presence of dioxygen [208] Beller et al [209] recently reported thatalcohol oxidations could also be performed using the same conditions The reac-tions were carried out in a buffered two-phase system with a constant pH of104 Under these conditions a remarkable catalyst productivity (TON up to 16600 for acetophenone) was observed The pH value is critical in order to ensurethe reoxidation of Os(VI) to Os(VIII) The scope of this system seems to be lim-ited to benzylic and secondary alcohols
As heterogeneous oxidation catalyst 5 Pt 1 BiC has been identified asan efficient catalyst for the conversion of 2-octanol to 2-octanone and 1-octanolto octanoic acid (see Fig 472) [210] Also manganese-substituted octahedral mo-
45 Oxygen-containing Compounds 181
Fig 470 CuBr2(bipy)-TEMPO catalyzed oxidation of alcohols
Fig 471 CoNHPI catalyzed oxidation of alcohols
lecular sieves have been reported [211] In this case benzylic and allylic alcoholscould be converted within 4 h However 50 mol of catalyst was needed toachieve this
Scant attention has been paid to vanadium-catalyzed oxidation of alcohols de-spite its ability to act according to the oxometal mechanism Punniyamurthy re-cently reported that indeed vanadium turns out to be a remarkably simple andselective catalyst with a wide substrate scope which requires few additives [212]albeit the activities are still rather low
4516 Catalytic Oxidation of Alcohols with Hydrogen PeroxideThe use of tungsten affords a highly active catalytic system for the oxidation ofalcohols Noyori and coworkers [213 214] have achieved substantial improve-ments in the sodium tungstate-based biphasic system by employing a phasetransfer agent containing a lipophilic cation and bisulfate as the anion egCH3(n-C8H17)3NHSO4 This system requires 11 equivalents of 30 aq H2O2
in a solvent-free system For example 1-phenylethanol was converted to aceto-phenone with turnover numbers up to 180000 As with all Mo- and W-basedsystems the Noyori system shows a marked preference for secondary alcoholseg Fig 473
Titanium silicalite (TS-1) an isomorphously substituted molecular sieve [215]is a truly heterogeneous catalyst for oxidations with 30 aq H2O2 includingthe oxidation of alcohols [216]
4 Catalytic Oxidations182
Fig 472 PtBi on carbon as effective catalyst for alcohol oxidation
Fig 473 Tungsten catalyzed alcohol oxidation with hydrogen peroxide
4517 Oxoammonium Ions in Alcohol OxidationIn addition a very useful and frequently applied method in the fine chemical in-dustry to convert alcohols into the corresponding carbonyl compounds is theuse of oxoammonium salts as oxidants [15] These are very selective oxidants foralcohols which operate under mild conditions and tolerate a large variety offunctional groups
The oxoammonium is generated in situ from its precursor TEMPO (or deriva-tives thereof) which is used in catalytic quantities see Fig 474 Various oxi-dants can be applied as the final oxidant In particular the TEMPO-bleach pro-tocol using bromide as cocatalyst introduced by Anelli et al is finding wide ap-plication in organic synthesis [217] TEMPO is used in concentrations as lowas 1 mol relative to substrate and full conversion of substrates can commonlybe achieved within 30 min The major drawbacks of this method are the use ofNaOCl as the oxidant the need for addition of bromine ions and the necessityto use chlorinated solvents Recently a great deal of effort has been devoted to-wards a greener oxoammonium-based method by eg replacing TEMPO by het-erogeneous variations or replacing NaOCl with a combination of metal as coca-talyst and molecular oxygen as oxidant Examples of heterogeneous variants ofTEMPO are anchoring TEMPO to solid supports such as silica [218 219] andthe mesoporous silica MCM-41 [220] or by entrapping TEMPO in solndashgel [221]Alternatively an oligomeric TEMPO can be used [222]
Alternatively TEMPO can be reoxidized by metal salts or enzyme In oneapproach a heteropolyacid which is a known redox catalyst was able to gener-ate oxoammonium ions in situ with 2 atm of molecular oxygen at 100 C [223]In the other approach a combination of manganese and cobalt (5 mol) wasable to generate oxoammonium ions under acidic conditions at 40 C [224] Re-sults for both methods are compared in Table 49 Although these conditionsare still open to improvement both processes use molecular oxygen as the ulti-mate oxidant are chlorine free and therefore valuable examples of progress inthis area Alternative Ru and CuTEMPO systems where the mechanism is me-
45 Oxygen-containing Compounds 183
Fig 474 Oxoammonium salts asactive intermediates in alcoholoxidation
tal-based rather than oxoammonium based and which display higher activitywill be discussed below Another approach to generate oxoammonium ions insitu is an enzymatic one Laccase that is an abundant highly potent redox en-zyme is capable of oxidizing TEMPO to the oxoammonium ion (Table 49)[225] A recent report shows that 15 mol TEMPO and 5 h reaction time canlead to similar results using laccase from Trametes versicolor [226]
4518 Biocatalytic Oxidation of AlcoholsEnzymatic methods for the oxidation of alcohols are becoming more importantAn excellent overview of biocatalytic alcohol oxidation is given in a review [227]Besides the already mentioned oxidases (laccase see above and eg glucose oxi-dase) the enzymes widespread in nature for (asymmetric) alcohol dehydrogena-tion are the alcohol dehydrogenases However their large scale application haspredominantly been impeded by the requirement for cofactor-recycling The vastmajority of dehydrogenases which oxidize alcohols require NAD(P)+ as cofactorare relatively unstable and too expensive when used in molar amounts Re-cently a stable NAD+-dependent alcohol dehydrogenase from Rhodococcus rubberwas reported which accepts acetone as co-substrate for NAD+ regeneration andat the same time performs the desired alcohol oxidation (Fig 475) Alcohol con-centrations up to 50vv could be applied [228] However it must be realizedthat this oxidation generally results in kinetic resolution Only one of the enan-
4 Catalytic Oxidations184
Table 49 Aerobic oxoammonium-based oxidation of alcohols
Substrate Aldehyde or ketone yield a)
2 mol Mn(NO3)2
2 mol Co(NO3)2
10 mol TEMPOacetic acid 40 C1 atm O2
b)
1 mol H5PMo10V2O40
3 mol TEMPOacetone 100C2 atm O2
c)
Laccase (3 Uml)Water pH 4530 mol TEMPO25 C 1 atm O2
d)
n-C6H13-CH2OH 97 (6 h)n-C7H15-CH2OH 98 (18 h)n-C9H19-CH2OH 15 (24 h)n-C7H15-CH(CH3)OH 100 (5 h)n-C6H13-CH(CH3)OH 96 (18 h)PhCH2OH 98 (10 h) e) 100 (6 h) 92 (24 h)PhCH(CH3)OH 98 (6 h) e)
cis-C3H7-CH=CHndashCH2OH 100 (10 h)PhndashCH=CHndashCH2OH 99 (3 h) 94 (24 h)
a) GLC yieldsb) Minisci et al Ref [224]c) Neumann et al Ref [223]d) Fabbrini et al Ref [225]e) Reaction performed at 20 C with air
tiomers is converted For example for 2-octanol maximum 50 conversion isobtained and the residual alcohol has an ee of gt 99 On the other hand for 2-butanol no chiral discrimination occurs and 96 conversion was observedAlso steric requirements exist while cyclohexanol is not oxidized cyclopentanolis a good substrate
452Oxidative Cleavage of 12-Diols
The oxidation of vic-diols is often accompanied by cleavage of the CndashC bond toyield ketones andor aldehydes Especially the clean conversion of (cyclohexeneto) 12-cyclohexanediol to adipic acid (Fig 476) has received tremendous inter-est [229]
453Carbohydrate Oxidation
Carbohydrate oxidations are generally performed with dioxygen in the presenceof heterogeneous catalysts such as PdC or PtC [230] An example of homoge-neous catalysis is the ruthenium-catalyzed oxidative cleavage of protected man-nitol with hypochlorite (Fig 477) [231]
Glucose oxidation to gluconate is carried out using glucose oxidase fromAspergillus niger mould [232] Very recently it was found that unsupported goldparticles in aqueous solution with an average diameter of 3ndash5 nm show a sur-
45 Oxygen-containing Compounds 185
Fig 475 Biocatalytic oxidation of alcohol using acetone for cofactor recycling
Fig 476 Formation of adipic acid via 12-cyclohexanediol cleavage
prisingly high activity in the aerobic oxidation of glucose not far from that ofan enzymatic system [233] Both gold and glucose oxidase share the commonstoichiometric reaction producing gluconate and hydrogen peroxideC6H12O6 + O2 + H2OC6H12O7 + H2O2 In both cases the hydrogen peroxide isdecomposed either through alkali-promoted decomposition or catalase-pro-moted decomposition
454Oxidation of Aldehydes and Ketones
Aldehydes undergo facile autoxidation (see Fig 478) which is frequently usedto form peracids in situ The peracid itself will react with aldehydes in a Baeyer-Villiger (BV) reaction to form carboxylic acids [6]
The reaction is used commercially in the oxidation of acetaldehyde to perace-tic acid [234] acetic anhydride [235] and acetic acid [236] respectively (Fig 479)In the production of acetic anhydride copper(II) salt competes with dioxygenfor the intermediate acyl radical affording acetic anhydride via the acyl cation
Also heterogeneous catalysts can be employed such as Pd or Pt on carbon[237] Recently it was found that gold supported on a mesoporous CeO2 matrix
4 Catalytic Oxidations186
Fig 477 Rutheniumhypochlorite for oxidation of protected mannitol
Fig 478 Autoxidation of aldehydes
Fig 479 Production of acetic acid and acetic anhydride starting from acetaldehyde
catalyzes the selective aerobic oxidation of aliphatic and aerobic aldehydes betterthan other heterogeneous reported materials [238] The activity is due to the na-nomeric particle size of Au and CeO2
4541 Baeyer-Villiger OxidationThe Baeyer-Villiger reaction is the oxidation of a ketone or aldehyde to the cor-responding ester The mechanism of the reaction is relatively straightforward(see Fig 480) In the first step a peracid undergoes a nucleophilic attack on thecarbonyl group to give the so-called Criegee intermediate [239] In the secondstep a concerted migration of one of the alkyl groups takes place with the re-lease of the carboxylate anion
The reaction has a broad scope and is widely used in organic synthesis Theoxidant is usually an organic peracid although in principle any electrophilicperoxide can be used A large number of functional groups are tolerated and avariety of carbonyl compounds may react ketones are converted into esters cy-clic ketones into lactones benzaldehydes into phenols or carboxylic acids and -diketones into anhydrides The regiochemistry of the reaction is highly predict-able and the migrating group generally retains its absolute configuration Thesecharacteristic features are best illustrated by the reaction in Fig 481 in which anumber of functional groups are left intact [240]
Dioxygen can be used as the oxidant in combination with a ldquosacrificialrdquo alde-hyde [241] in which case the aldehyde first reacts with dioxygen and the result-ing peracid is the oxidant This is similar to the classical Baeyer-Villiger oxida-tion
A large number of catalysts have been shown to be active in the oxidation ofcycloalkanones to lactones using only hydrogen peroxide as the oxidant Methyl-trioxorhenium (MTO) is moderately active in the oxidation of linear ketones[242] or higher cycloalkanones [243] but it is particularly active in the oxidationof cyclobutanone derivatives (Fig 482) which are oxidized faster with MTOthan with other existing methods [244]
45 Oxygen-containing Compounds 187
Fig 480 Mechanism of the Baeyer-Villiger reaction
With lt 1 mol MTO cyclobutanones are fully converted within one hour An-other approach consists of the use of a fluorous Sn-catalyst under biphasic con-ditions [245] A perfluorinated tin(IV) compound Sn[NSO2C8F17]4 was recentlyshown to be a highly effective catalyst for BV oxidations of cyclic ketones with35 hydrogen peroxide in a fluorous biphasic system (Fig 483) The catalystwhich resides in the fluorous phase could be easily recycled without loss of ac-tivity
Migration of hydrogen can yield carboxylic acids as the product of BV-oxida-tion of aldehydes SeO2 is especially good for oxidation of linear aldehydes toacids but also of heteroaromatic aldehydes to acids [246] To avoid contamina-tion of the products with selenium catalysts Knochel [247] immobilised 24-bis(perfluorooctyl)phenyl butyl selenide in a fluorous phase The system was im-proved slightly by using the 35-bis(perfluorooctyl)phenyl butyl selenide isomerof the catalyst and by using the more polar dichloroethane as a co-solvent sys-tem instead of benzene (Fig 484) [248] The latter selenium isomer is slightlymore difficult to synthesize but both catalysts could be recycled without seriousloss of activity
A (lipophilic) quaternary ammonium salt has been shown to catalyze theBeayer-Villiger reaction of aldehydes under halide-and metal-free conditionswith aqueous H2O2 (Fig 485) [249]
4 Catalytic Oxidations188
Fig 481 Functional group tolerance in Baeyer-Villiger oxidation
Fig 482 MTO-catalyzed oxidation of cycloalkanones
Fig 483 Use of a fluorous Sn-catalyst for BV oxidations in a fluorous biphasic system
Heterogeneous catalysts are also active for the Baeyer-Villiger oxidation withH2O2 One of the best ndash based on 16 wt tin in zeolite beta ndash was developedin the group of Corma [250 251] It provides a green method for BV oxidationsin that it utilizes hydrogen peroxide as the oxidant a recyclable catalyst andavoids the use of chlorinated hydrocarbon solvents It is believed that the Sn Le-wis acid sites solely activate the ketone for BV-reaction and leave hydrogen per-oxide non-activated Corma proposed that in this way side-reactions such asepoxidation which require electrophilic activation of hydrogen peroxide arelargely avoided Oxidation of bicyclo[320]hept-2-en-6-one with hydrogen perox-ide in the presence of tin zeolite beta gave selective oxidation of the ketoneleaving the olefin intact The tin catalyst may be particularly effective because itcan expand its coordination sphere to 6 thereby providing room for coordina-tion of both the ketone and the hydroxide leaving group
Surprisingly both in the oxidation of bicyclo[320]hept-2-en-6-one and of di-hydrocarvone (not shown) isomeric lactones formed by migration of the second-ary carbon as is usual in Baeyer-Villiger reactions were not observed Other
45 Oxygen-containing Compounds 189
Fig 484 Fluorous phase BV-oxidation using fluorous selenium catalysts
Fig 485 Quaternary ammonium salts as catalyst for BV-oxidation with H2O2
ketones (eg cyclohexanone Fig 486) were oxidized with remarkable selectivity(gt 98) considering the reaction conditions and the catalyst was recycled severaltimes without loss of activity Dioxane or the more attractive methyl-tert-butylether were used as solvents in these transformations
Also very important is the asymmetric version of the BV-reaction In this areabiocatalysts are very promising see Section 47
455Oxidation of Phenols
The aerobic oxidation of phenols in the presence of cobalt-Schiffrsquos base com-plexes as catalysts is facilitated by (electron-donating) alkyl substituents in thering and affords the corresponding p-quinones eg the Vitamin E intermediatedrawn in Fig 487 When the para-position is occupied the reaction may be di-rected to the ortho-position [252 253] Copper compounds also mediate this typeof oxidation eg the Mitsubishi Gas process for the Vitamin E intermediate[254]
Phenol undergoes hydroxylation with H2O2 in the presence of Broslashnsted(HClO4 H3PO4) or Lewis acid (TS-1) catalysts affording a mixture of catecholand hydroquinone [255] The reaction proceeds via a heterolytic mechanism in-volving an electrophilic TindashOOH species or in the case of Broslashnsted acids per-haps even a hydroxy cation On the other hand catalysis by FeIICoII (Brichimaprocess) involves a homolytic mechanism and hydroxyl radical intermediates[255] (see Table 410)
4 Catalytic Oxidations190
Fig 486 Sn-Beta catalyzed BV-oxidation
Fig 487 Aerobic oxidation of phenols
456Oxidation of Ethers
Ethers are readily autoxidized at the -position to the corresponding -hydroper-oxyethers which is of no synthetic utility but important to realize when ethersare evaporated to leave an explosive residue of -hydroperoxyethers behindEthers are oxidized with stoichiometric amounts of high valent metal oxidessuch as RuO4 [256] CrO3 [257] and KMnO4 [258] but very few catalytic oxida-tions are known and these generally pertain to activated eg benzylic sub-strates One example is the NHPI [259] catalyzed oxidation of methyl benzylether to the corresponding acetate (Fig 488)
Recently a convenient and selective Ruhypochlorite oxidation protocol for theselective transformation of a series of ethers and alcohols was reported [260]The catalytic systems described in the literature especially regarding ether oxi-dation have limited reproducibility andor require an excess of terminal oxi-dant ie NaOCl solutions (household bleach) When the pH is maintained at9ndash95 the reactions proceed smoothly using the theoretical amount of hypo-chlorite with fast complete conversion of substrate and high selectivity to thetarget molecules at low concentration of Ru precursor A variety of Ru precur-sors can be used although it was found that [Pr4N][RuO4] (TPAP) gave the bestresults The catalyst can also be recycled with negligible loss of selectivity andminimum loss of activity which can be further optimised by scale-up In theoxidation of dibutyl ether only 025 mol of TPAP was used in ethyl acetate asthe solvent leading to 95 yield and 97 selectivity towards butyl butyrate(Fig 489)
45 Oxygen-containing Compounds 191
Table 410 Comparison of phenol conversion processes [255]
Process(catalyst)
Rhone-Poulenc(HClO4 H3PO4)
Brichima(FeIICoII)
Enichem(TS-1)
Phenol conversion 5 10 25Selectivity on phenol 90 80 90Selectivity on H2O2 70 50 70Catecholhydroquinone 14 23 10
Fig 488 NHPI catalyzed oxidation of ethers
46Heteroatom Oxidation
Autoxidations of substrates containing heteroatoms tend to be complex andnon-selective processes Nonetheless a number of selective catalytic reactionswith hydrogen peroxide are known
461Oxidation of Amines
A large number of different nitrogen-containing compounds such as primarysecondary and tertiary amines NN-dimethylhydrazones hydroxylamines pyri-dines etc can be oxidized with eg hydrogen peroxide leading to an equallyvast number of different products The presence of an -hydrogen may have amajor influence on the outcome of the reaction Furthermore a distinction canbe made between oxidations involving high-valent peroxometal or oxometal spe-cies and oxidative dehydrogenations mediated by low-valent transition metal cat-alysts Nonetheless with the right choice of solvent and equivalents of oxidantsthe reactions can be directed to a certain extent
4611 Primary AminesPrimary amines are dehydrogenated by high-valent oxometal species to give ni-triles or imines depending on the number of available -hydrogens Oxidationof the amine via peroxometal-intermediates (eg with MTO Na2MoO4
4 Catalytic Oxidations192
Fig 489 Green protocol for TPAPNaOCl catalyzed oxidation of ethers
Fig 490 Oxidation of primary amines
Na2WO4 NaVO3 in combination with H2O2) leads to the formation of oximes[261 262] or in the absence of -hydrogens even to nitro-compounds (Fig 490)[263]
4612 Secondary AminesPeroxometal-forming catalysts eg MTO SeO2 or Na2WO4 catalyze the oxida-tion of secondary amines to nitrones via the corresponding hydroxylaminesFig 491 a [262] In the absence of -hydrogens these substrates will also givenitroxides (R2NO) see Fig 491 b [263] Here again oxometal complexes reactdifferently giving the dehydrogenated imine rather than the nitrone [122 264]as is illustrated in Fig 492
4613 Tertiary AminesSimilarly for tertiary amines a distinction can be made between oxometal andperoxometal pathways Cytochrome P450 monooxygenases catalyze the oxidativeN-demethylation of amines in which the active oxidant is a high-valent oxoironspecies This reaction can be mimicked with some oxometal complexes(RuV=O) while oxidation via peroxometal complexes results in oxidation of theN atom (Fig 493 a and b) [261] A combination of MTOhydrogen peroxide can
46 Heteroatom Oxidation 193
Fig 491 MTO catalyzed oxidation of secondary amines
Fig 492 Oxidation of secondary amines via Ru and W catalysts
also oxidize pyridines to pyridine N-oxides as was recently published by Sharp-less et al [265] A rare example of clean oxidation of tertiary amines withoutmetal compounds was reported by Baumlckvall et al [266] using flavin as the cata-lyst (Fig 493 d)
4614 AmidesRuthenium oxo compounds catalyze the oxidation of amides eg -lactams atthe position to the nitrogen using peracetic acid as the oxidant presumablyvia oxoruthenium intermediates [264]
462Sulfoxidation
Dialkyl sulfides are readily oxidized by eg H2O2 in the presence of metal cata-lysts to give the corresponding sulfoxides In turn the sulfoxides can be furtheroxidized to the corresponding sulfones RndashS(O)2ndashR with excess peroxide Due tothe polarity of the SndashO bond the second oxidation step is more difficult for elec-trophilic oxidation catalysts This is especially important in the oxidative destruc-tion of mustard gas where the corresponding sulfoxide is relatively harmlessbut the sulfone quite toxic again [267] In order to see which catalyst is likely togive ldquooveroxidationrdquo of the sulfoxide the thianthrene 5-oxide (see Fig 494) is anexcellent probe to test catalysts active in oxygen transfer reactions for whether
4 Catalytic Oxidations194
Fig 493 Oxidation of tertiary amines
they are nucleophilic or electrophilic in character Catalytic oxidations with hy-drogen peroxide are generally performed with early transition elements egMo(VI) [268] W(VI) Ti(IV) V(V) Re(V) [269] and Re(VII) (=MTO Fig 495)[270] or seleninic acids as catalysts [271] and involve peroxometal pathways Sul-fides can also be oxidized with dioxygen using a cerium (IV)cerium (III) redoxcouple [271] via a homolytic mechanism involving a sulfonium radical cationintermediate (Fig 496)
47Asymmetric Oxidation
Owing to the instability of many (chiral) ligands under oxidative reaction condi-tions asymmetric oxidation is not an easy reaction to perform However muchprogress has been achieved over the last decades Because of the relatively lowvolumes and high added value of the products asymmetric oxidation allows theuse of more expensive and environmentally less attractive oxidants such as hy-pochlorite and N-methylmorpholine-N-oxide (NMO)
47 Asymmetric Oxidation 195
Fig 494 Nucleophilic vs electrophilic S oxidation pathways
Fig 495 MTOH2O2 catalyzed sulfide oxidation
Fig 496 Sulfide oxidation using air as the oxidant
471Asymmetric Epoxidation of Olefins
Chiral epoxides are important intermediates in organic synthesis A benchmarkclassic in the area of asymmetric catalytic oxidation is the Sharpless epoxidationof allylic alcohols in which a complex of titanium and tartrate salt is the activecatalyst [273] Its success is due to its ease of execution and the ready availabilityof reagents A wide variety of primary allylic alcohols are epoxidized in gt 90optical yield and 70ndash90 chemical yield using tert-butyl hydroperoxide as theoxygen donor and titanium-isopropoxide-diethyltartrate (DET) as the catalyst(Fig 497) In order for this reaction to be catalytic the exclusion of water is ab-solutely essential This is achieved by adding 3 Aring or 4 Aring molecular sieves Thecatalytic cycle is identical to that for titanium epoxidations discussed above (seeFig 420) and the actual catalytic species is believed to be a 2 2 titanium(IV) tar-trate dimer (see Fig 498) The key step is the preferential transfer of oxygenfrom a coordinated alkylperoxo moiety to one enantioface of a coordinatedallylic alcohol For further information the reader is referred to the many re-views that have been written on this reaction [274 275]
The applicability of the ldquoSharplessrdquo asymmetric epoxidation is however lim-ited to functionalized alcohols ie allylic alcohols (see Table 411) The bestmethod for non-functionalized olefins is the Jacobsen-Kaksuki method Only afew years after the key publication of Kochi and coworkers on salen-manganesecomplexes as catalysts for epoxidations Jacobsen and Kaksuki independently de-scribed in 1990 the use of chiral salen manganese(III) catalysts for the synthe-sis of optically active epoxides [276 277] (Fig 499) Epoxidations can be carriedout using commercial bleach (NaOCl) or iodosylbenzene as terminal oxidantsand as little as 05 mol of catalyst The active oxidant is an oxomanganese(V)species
Over the years further tuning of the ligand by varying the substituents in thearomatic ring has led to gt 90 ee for a number of olefins [278] Improvementswere also achieved by adding amine-N-oxides such as 4-phenylpyridine-N-oxide
4 Catalytic Oxidations196
Fig 497 The ldquoSharplessrdquo catalytic asymmetric epoxidation
which serve as axial ligands in the active oxomanganese(V) species The methodgenerally gives good results for cis-disubstituted olefins whereas trans-disubsti-tuted olefins are less suitable substrates (see Table 412) On the other hand chro-mium-salen complexes catalyze the asymmetric epoxidation of trans-substitutedolefins in reasonable ees (see Fig 4100) using iodosylarenes as oxidants [279]
47 Asymmetric Oxidation 197
Fig 498 The catalytic cycle of the ldquoSharplessrdquo catalytic asymmetric epoxidation
Table 411 Sharpless asymmetric epoxidation of allylic alcohols a)
Substrate Yield () ee ()
65 90
70 96
89 gt98
50 gt95
40 95
a) Results with 5 mol of catalyst see Ref [273]
4 Catalytic Oxidations198
Fig 499 The Jacobsen-Katsuki asymmetric epoxidation of unfunctionalized olefins
Table 412 Jacobsen-Katsuki asymmetric epoxidation of unfunctionalized olefins
Olefin Method a) Equiv catalyst Isolated yield () ee ()
A 004 84 92
A 001 80 88
B 004 67 88
A 002 87 98
B 015 63 94
B 008 67 97
a) Method A NaOCl pH 113 CH2Cl2 0 C Method B sameas A +02 eq 4-phenylpyridine-N-oxide
The recent reports of Katsuki and Beller using Ti- [280 281] and Ru-based[282] complexes for asymmetric epoxidation with H2O2 have however changedthe state-of-the-art in the area of metal-catalyzed asymmetric epoxidations Espe-cially for titanium in combination with reduced salen-type ligands excellentstereochemical control was achieved for terminal olefins using hydrogen perox-ide as the oxidant (see Fig 4101) Also with ruthenium notorious for its cata-lase activity excellent yields and enantioselectivities were obtained for cis- andactivated olefins In Table 413 an overview is given of the performance of tita-nium and ruthenium complexes as catalysts with hydrogen peroxide
For titanium only 1 mol of catalyst Ti(salalen) (Table 413) and 105 eqH2O2 are required to obtain high yields and selectivities 12-Dihydronaphtha-lene is an activated cis-olefin which obviously gives the best results (yield andenantioselectivity of over 98) using little or no excess of hydrogen peroxideHowever also for simple styrene 93 ee can be achieved using this chiral tita-nium complex What is most striking is the result obtained for 1-octene Forthis simple non-activated olefin a reasonable 82 ee could be attained Tita-nium-salan (see Table 413) as a catalyst requires higher loadings (5 mol) butits ease of synthesis and in situ synthesis from Ti(OiPr)4 and salan ligandmakes this a very promising catalyst for practical applications
47 Asymmetric Oxidation 199
Fig 4100 Cr-salen catalyzedasymmetric epoxidation
Fig 4101 Ti-catalyzed asymmetric epoxidation of olefinsusing aqueous hydrogen peroxide as the oxidant
Mukaiyama has reported the use of manganese complexes for chiral epoxida-tions using a combination of molecular oxygen and an aldehyde as the oxidant[283] With salen-manganese(III) complexes and pivaldehydeoxygen the corre-sponding epoxides of several 12-dihydronaphthalenes were obtained in verygood yields (77 to 92 ee) in the presence of N-alkyl imidazole as axial ligandAltering the ligand structure from salen derivatives to optically active -keto-imine-type ligands gave the novel manganese catalysts in Fig 4102 which oxi-dize phenyl-conjugated olefins such as dihydronaphthalenes and cis--methylstyrene in 53 to 84 ee [284] The enantiofacial selection in these manganese-catalyzed epoxidations is opposite to that obtained with sodium hypochlorite oriodosylbenzene as the primary oxidant in the Jacobsen-Katsuki epoxidation Ap-parently the catalytically active species differs from the putative oxomangane-se(V) complex in the latter processes An acylperoxomanganese complex wasproposed as the active oxidant ie a peroxometal rather than an oxometal mech-anism
4 Catalytic Oxidations200
Table 413 Comparison of metal catalysts for the asymmetric epoxidation of alkenes using aqueous H2O2
Substrate Catalyst Catalystloading (mol)
Eq 30aqueous H2O2
Yield epoxide()
ee epoxide()
Ref
Ti(salalen)-1 a)
Ti(salan)-2 b)
Ru(pyboxazine)(pydic)-3 c) d)
155
105153
904785
938259
280281282
Ti(salalen)-1 a)
Ti(salan)-2 b)15
10515
7025
8255
280281
Ti(salalen)-1 a)
Ti(salan)-2 b)15
10515
9987
9996
280281
Ru(pyboxazine)(pydic)-3 c)
5 3 95 72 282
a) RT 12ndash48 h CH2Cl2 as solventb) 25 C 6ndash24 h CH2Cl2 as solventc) RT 12 h 2-methylbutan-2-ol as solventd) 20 mol acetic acid was added
A very different non-metal based approach for the synthesis of trans-disub-stituted chiral epoxides is the use of the highly reactive chiral dioxiranes(Fig 4103) These oxidants can be generated in situ by using potassium persul-fate as the primary oxidant Although this method requires the use of 20ndash30 mol of dioxirane precursor the reaction proceeds with high chemical yieldsand ees over 90 for a wide variety of trans-disubstituted olefines [285] Themechanism is given in Fig 4104 and involves a spiro transition state More re-cently it was shown that the persulfate can be replaced by H2O2 in CH3CNwhich generates the peroxyimidic acid (Payne reagent) in situ [286]
Another method is to use poly-L-amino acids as catalysts in alkaline media(Julia-Colanna epoxidation) for the asymmetric epoxidation of chalcones andother electron-poor olefins with H2O2 [287] SmithKline Beecham workers usedthis method (see Fig 4105) as a key step in the synthesis of a leukotriene an-tagonist although it required 20 equivalents of H2O2 and 12 equivalents ofNaOH based on substrate [288] The mechanism probably involves the asym-
47 Asymmetric Oxidation 201
Fig 4102 Enantioselective epoxidation of phenyl-conjugatedolefins employing aldehyde and molecular oxygen as theoxidant
Fig 4103 Efficient asymmetric epoxidation of trans-alkenes
metric addition of a hydroperoxy anion (HOOndash) to the olefinic double bond fol-lowed by epoxide ring closure The poly-L-amino acid acts as a chiral phasetransfer catalyst and may be considered as a synthetic enzyme mimic Furtherimprovements of the Julia-Colonna epoxidation have been achieved by using so-dium percarbonate as the oxidant and recyclable silica-supported polyaminoacids as catalysts in dimethoxyethane as solvent [289]
Finally enzymes themselves can be used for the direct epoxidation of olefinsAs already outlined in Section 42 peroxidases (which can directly apply hydro-gen peroxide as the oxidant) as well as monooygenases are available Because ofits ease of application chloroperoxidase (CPO) from Caldariomyces fumago isvery promising It is commercially available and displays a reasonable substraterange [290] The main problem is its instability under reaction conditions andthe sluggish reaction rates Typical turnover rates are 01ndash2 sndash1 The epoxidationof styrene in the presence of 08 of surfactant is at 55 sndash1 the fastest on re-cord [291] The advantage is that the ees in most cases are always good to excel-
4 Catalytic Oxidations202
Fig 4104 Catalytic cycle of asymmetric epoxidation via chiral dioxiranes
Fig 4105 Asymmetric epoxidation of chalcones
lent For example 2-heptene could be oxidized with 1700 turnovers relative toenzyme in 30 t-BuOH The ee of the resulting epoxide was 96 The totalturnover number could be further increased in this reaction (from 1700 to11500) when the hydrogen peroxide was generated in situ by the glucose oxi-dase-mediated reaction of glucose and oxygen A wide range of 2-methyl-1-al-kenes could also be oxidized with ees ranging from 95 to 50 [292] 1-Alkeneswith the exception of styrene are suicide reactants that alkylate the heme in na-tive CPO The latter problem can be circumvented by using certain mutants[293] Styrene resulted in only 49 ee for this substrate the styrene monooxy-genases seem to be better suited
Recently the first asymmetric cell-free application of styrene monooxygenase(StyAB) from Pseudomonas sp VLB120 was reported [294] StyAB catalyses theenantiospecific epoxidation of styrene-type substrates and requires the presenceof flavin and NADH as cofactor This two-component system enzyme consistsof the actual oxygenase subunit (StyA) and a reductase (StyB) In this case thereaction could be made catalytic with respect to NADH when formate togetherwith oxygen were used as the actual oxidant and sacrificial reductant respec-tively The whole sequence is shown in Fig 4106 The total turnover numberon StyA enzyme was around 2000 whereas the turnover number relative toNADH ranged from 66 to 87 Results for individual substrates are also given inFig 4106 Excellent enantioselectivities are obtained for - and -styrene deriva-tives
Recently it was shown that the flavin (FAD in Fig 4106) could be directly re-generated by the organometallic complex CpRh(bpy)(H2O)]2+ and formate In
47 Asymmetric Oxidation 203
Fig 4106 Biocatalytic epoxidation with styrenemonooxygenase including cofactor regeneration
this way the reaction becomes simpler because only enzyme (StyA) FAD andRh-complex are required The resulting turnover number on Rh ranged from 9to 18 depending on the substrate [295]
472Asymmetric Dihydroxylation of Olefins
Following their success in asymmetric epoxidation Sharpless and coworkers de-veloped an efficient method for the catalytic asymmetric dihydroxylation of ole-fins The method employs catalytic amounts of OsO4 and derivatives of cincho-na alkaloids as chiral ligands together with N-methylmorpholine-N-oxide (NMO)as the primary oxidant see Fig 4107 [296] The use of osmium(VIII) complexesas catalysts leads to stereospecific 12-cis addition of two OH groups to the ole-fin The reaction greatly benefits from ligand accelerated catalysis ie the liga-tion of osmium by the alkaloid enhances the rate of reaction with the alkene byone to two orders of magnitude relative to the reaction without ligand The reac-tion is complicated by the fact that two catalytic cycles are possible seeFig 4108 [297] The primary cycle proceeds with high face selectivity and in-volves the chiral ligand in its selectivity determining step the formation of theosmium(VI)glycolate The latter is oxidized by the primary oxidant to the os-mium(VIII)glycolate which is hydrolyzed to the product diol with concomitant
4 Catalytic Oxidations204
Fig 4107 Asymmetric dihydroxylation of alkenes
generation of the catalyst In the second catalytic cycle the osmium(VIII)glyco-late reacts with a second molecule of olefin displacing the chiral ligand and re-sulting in poor overall enantioselectivity The desired pathway involves hydroly-sis of the osmium(VI)glycolate in competition with coordination of another ole-fin molecule Therefore slow addition of olefin is essential to obtain high ees
Alternatively the process can be performed with K3Fe(CN)6 as the stoichio-metric oxidant in tert-butanolwater mixtures [298] In this case the olefin osmy-lation and osmium reoxidation steps are uncoupled since they occur in differ-ent phases resulting in improved enantioselectivities However from a practicalpoint of view the improved enantioselectivities (about 5ndash10 ee) are probablyoffset by the use of a less attractive oxidant
When using NMO as the oxidant on the other hand the reduced form isreadily recycled by oxidation with H2O2 The asymmetric dihydroxylation is suc-cessful with a broad range of substrates in contrast to the Sharpless asym-metric epoxidation which is only suitable for allylic alcohols (Table 414)Further development of the system has led to the formulation of a reagent mix-ture called AD-mix based on phthalazine-type ligands which contains all theingredients for the asymmetric dihydroxylation under heterogeneous conditionsincluding OsO4 [299] see Fig 4109 One equivalent of methanesulfonamide isadded to accelerate the hydrolysis of the osmium(VI)glycolate and thus toachieve satisfactory turnover rates
Beller et al [85] recently described the aerobic dihydroxylation of olefins cata-lyzed by osmium at basic pH as mentioned above When using the hydroquini-dine and hydroquinine bases they were able to obtain reasonable enantioselec-tivities (54 ee to 96 ee) for a range of substrates An alternative route towardsenantiopure diols is the kinetic resolution of racemic epoxides via enantioselec-tive hydrolysis catalyzed by a Co(III)salen acetate complex developed by Jacob-
47 Asymmetric Oxidation 205
Fig 4108 Mechanism of asymmetric dihydroxylation
sen [300] In this case the maximum theoretical yield of the enantiomericallypure diol is 50 compared with 100 in the asymmetric dihydroxylation meth-od Nonetheless its simplicity makes it a synthetically useful methodology
4 Catalytic Oxidations206
Table 414 Comparison of asymmetric epoxidation (AE) and asymmetricdihydroxylation (AD) according to refs [273] and [299]
Alkene Substrate for
AD AE
gt 95 ee NR
80 ee gt 95 ee
gt 95 ee 30ndash50 ee
X=OAc OCH2Ph N3 Cl gt 95 ee NR
gt 95 ee NR
gt 95 ee NR
gt 95 ee NR
NR =non-relevant
Fig 4109 Ligands used in commercial catalysts for asymmetric dihydroxylation
473Asymmetric Sulfoxidation
In the area of metal catalyzed asymmetric sulfoxidation there is still much roomfor improvement The most successful examples involve titanium tartrates butat the same time often require near stoichiometric quantities of catalysts [301302] Recently this methodology has been successfully used for the productionof (S)-Omeprazole by AstraZeneca [303] (see Fig 4110) A modified Kagan-pro-cedure [302] was applied using cumene hydroperoxide as the oxidant Anotherexample is the sulfoxidation of an aryl ethyl sulfide which was in developmentby Astra Zeneca as a candidate drug for the treatment of schizophrenia In thiscase the final ee could be improved from 60 to 80 by optimising the Titar-trate ratio [304]
From a practical viewpoint the recently discovered vanadium-based and iron-based asymmetric sulfoxidation with hydrogen peroxide is worth mentioning[305 306] For vanadium in principle as little as 001 mol of catalyst can beemployed (Fig 4111) With tridentate Schiff-bases as ligands formed fromreadily available salicylaldehydes and (S)-tert-leucinol ees of 59ndash70 were ob-tained for thioanisole [305] 85 ee for 2-phenyl-13-dithiane [305] and 82ndash91ee for tert-butyl disulfide [307] For iron similar results were obtained using4 mol of an iron catalyst synthesized in situ from Fe(acac)3 and the same typeof Schiff base ligands as in Fig 4111 (see Ref [306] for details)
47 Asymmetric Oxidation 207
Fig 4110 Production of (S)-Omeprazole
Fig 4111 Vanadium catalyzed asymmetric sulfoxidation
Finally but certainly not least we note that the enzyme chloroperoxidase(CPO) catalyzes the highly enantioselective (gt 98 ee) sulfoxidation of a rangeof substituted thioanisoles [308] In contrast to the epoxidation of alkenes whereturnover frequencies were low (see above) in the case of sulfoxidation of thioa-nisole a turnover frequency of around 16 sndash1 and a total turnover number of125000 could be observed A selection of data is represented in Fig 4112 Be-sides aryl alkyl sulfides also dialkylsulfides could be oxidized with reasonableenantioselectivities [27]
Another class of peroxidases which can perform asymmetric sulfoxidationsand which have the advantage of inherently higher stabilities because of theirnon-heme nature are the vanadium peroxidases It was shown that vanadiumbromoperoxidase from Ascophyllum nodosum mediates the production of (R)-methyl phenyl sulfoxide with a high 91 enantiomeric excess from the corre-sponding sulfide with H2O2 [38] The turnover frequency of the reaction wasfound to be around 1 minndash1 In addition this enzyme was found to catalyse thesulfoxidation of racemic non-aromatic cyclic thioethers with high kinetic resolu-tion [309]
474Asymmetric Baeyer-Villiger Oxidation
The area of asymmetric catalytic Baeyer-Villiger oxidation was recently reviewed[310] It was concluded that biocatalytic methods in this case would seem tohave the edge with respect to enantioselectivity regiochemistry and functionalgroup selectivity Baeyer-Villiger monooxgenases (BVMOs) are versatile biocata-lysts that have been widely used in synthetic biotransformations The cyclohexa-none monooxygenase (CHMO) from Acinetobacter calcoaceticus NCIMB is thebest characterized and most studied of these enzymes [311] They contain a fla-vin moiety as the prosthetic group and utilize NAD(P)H as a stoichiometric co-factor (see Fig 4113)
In view of the requirement for cofactor regeneration these reactions are gen-erally performed with whole microbial cells in a fermentation mode Degrada-
4 Catalytic Oxidations208
Fig 4112 Sulfoxidation reactions mediated by CPO
tion of the lactone product can be circumvented by the addition of hydrolase in-hibitors andor heterologous expression Several CHMOs are now commerciallyavailable eg from Fluka and they are easy to use even for non-specialists Adisadvantage of the methodology is the low volume yield (concentrations aretypically 10 mM compared to 1 M solutions in homogeneous catalysis) Further-more many organic substrates have limited solubility in water This problemcould possibly be solved by performing the reactions in organic media [312]The generally accepted mechanism for BV oxidations catalyzed by BVMOs waspreviously discussed in Section 42 (see Fig 415) The state-of-the-art with re-gard to scale-up of BVMO catalyzed oxidations has been recently reviewed [313]The reaction suffers from both substrate and product inhibition and the opti-mum ketone concentration was shown to be 02 to 04 g lndash1 and at product con-centrations above 45 to 5 g lndash1 the activity of the whole cell biocatalyst fell tozero This suggests that a fed-batch operation with continuous product removalby adsorption on a solid resin is necessary in order to obtain reasonable volu-metric yields In this way volumetric yields up to 20 g lndash1 could be obtained
In principle the use of the isolated enzyme should allow the reaction to beperformed at higher substrate concentrations avoid side reactions and facilitatedownstream processing However this requires an ancillary enzymatic cofactorregeneration system Encouraging results have been obtained by couplingCHMO-catalyzed BV oxidation to cofactor regeneration mediated by anNADPH-dependent formate dehydrogenase (Fig 4114) [314 315] The overallreaction constitutes an enantioselective BV oxidation with stoichiometric con-sumption of O2 and formate to give water and carbon dioxide as the coproductsThe reaction was carried to complete conversion with a 40 mM substrate con-centration and the enzymes separated by ultrafiltration and re-used
The enzyme catalyzed hydrolysis of the lactone and subsequent oxidation areunwanted side-reactions obviously Several yeasts [316] and E coli [317] have
47 Asymmetric Oxidation 209
Fig 4113 BV reactions catalyzed by BVMOs
Fig 4114 CHMO catalyzed BVreaction coupled to cofactorregeneration by formatedehydrogenase
been engineered to convert the ketone to the lactone exclusively Thus 2-substi-tuted [316] and 4-substituted (or prochiral) [317 318] cyclohexanones can beconverted with high selectivity (Fig 4115) [319] The (racemic) 3-substituted[320] cyclohexanones are synthetically less interesting as they can yield two re-gioisomeric lactones each in two enantiomers For small substituents there islittle discrimination by the enzyme
The first example of a dynamic kinetic resolution involving a CHMO-cata-lyzed BV oxidation was recently reported (Fig 4116) [321] The reaction wasperformed with whole cells of CHMO-containing recombinant E coli sp at pH9 Under these conditions the ketone substrate underwent facile racemization
4 Catalytic Oxidations210
Fig 4115 Enzyme catalyzed asymmetric BV oxidation of 2- 3- and 4-ethylcyclohexanones
Fig 4116 Dynamic kinetic resolution of ketones using CHMO-containing recombinant E coli
via ketondashenol tautomerism and the lactone product was obtained in 85 yieldand 96 ee
Homogeneous catalysts can also be used for asymmetric BV oxidation [310]One of the best catalysts appears to be 1 mol of a chiral copper catalyst withoxazoline ligands (see Fig 4117) cyclobutanone derivatives are readily oxidizedto give optically active lactones The most promising results were obtained in re-actions using benzene solutions under an atmosphere of dioxygen (1 atm) withpivaldehyde as co-reductant at ambient temperature [322] In general 2-aryl sub-stituted cyclohexanones give good results In the example of Fig 4117 metalcatalyzed oxidation of rac-1 gave isomeric -lactones 2 and 3 in a ratio of 3 1(61 yield) with enantiomeric excesses of 67 and 92 respectively [323]
45Conclusion
Summarizing it is evident that catalytic oxidation is a mature technology whichis still under strong development Every day the performance of catalysts thatuse O2 or H2O2 as green oxidants increases This is illustrated by two keyareas the oxidation of alcohols and alkenes In the first case the oxidation of al-cohols no longer requires stoichiometric use of heavily polluting metals Manyhomogeneous and heterogeneous catalysts are available which use molecularoxygen as the oxidant Especially promising seems to be the use of gold nano-particles as catalysts for alcohol and carbohydrate oxidation The turnover fre-quencies obtained in this case overwhelm all results obtained so far In the areaof asymmetric epoxidation the use of hydrogen peroxide now seems to give asgood results as the more established methods using alkylhydroperoxide or hypo-chlorite as the oxidant
When comparing homogeneous and heterogeneous catalysts clearly homoge-neous systems take the lead In addition heterogeneous systems have the disad-
45 Conclusion 211
Fig 4117 Asymmetric copper-catalyzed BV oxidation of cyclobutanones
vantage that the leaching of metals in solution is always a possible complicationin the reaction and therefore they have to be subjected to a rigorous test of het-erogeneity
When comparing chemical and biocatalytic methods one could say that espe-cially for asymmetric oxidations enzymatic methods enter the scene This ismost evident in the area of asymmetric Baeyer-Villiger oxidation where biocata-lysts take the lead and homogeneous chiral catalysts lag far behind in terms ofee values Significant progress can be expected in the area of biocatalysis due tothe advancement in enzyme production technologies and the possibility of tai-lor-made enzymes
Despite the huge effort put into research towards green and catalytic oxida-tion the number of applications in the fine chemical industry is limited For in-dustrial batch processes simple robust and reliable methods are required Foroxidations this is in general less straightforward than for reductions Howevermuch is to be gained in this area and therefore elegance should be a leadingprinciple for all newly designed chemical oxidation processes
4 Catalytic Oxidations212
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267 Y-U Yang J A Baker JR WardChem Rev 1992 92 1729
268 HS Schultz HB Freyermuth S RBuc J Org Chem 1963 28 1140
269 HQ N Gunaratne MA McKervey SFeutren J Finlay J Boyd TetrahedronLett 1998 39 5655
270 W Adam CM Mitchell CR Saha-Moumlller Tetrahedron 1994 50 13121
271 HJ Reich F Chow SL Peake Syn-thesis 1978 299
272 DP Riley MR Smith PE CorreaJ Am Chem Soc 1988 110 177
273 T Katsuki KB Sharpless J AmChem Soc 1980 102 5974
274 R A Johnson K B Sharpless in Cata-lytic Asymmetric Synthesis I Ojima(ed) VCH Berlin 1993 p 103
275 K B Sharpless Janssen Chim Acta1988 6(1) 3
276 W Zhang JL Loebach SR WilsonEN Jacobsen J Am Chem Soc 1990112 2801
277 R Irie K Noda Y Ito T Katsuki Tet-rahedron Lett 1991 32 1055
278 EN Jacobsen in Catalytic AsymmetricSynthesis I Ojima (ed) VCH Berlin1993 p 159
279 C Bousquet DG Gilheany Tetrahe-dron Lett 1995 36 7739
280 K Matsumoto Y Sawada B Saito KSakai T Katsuki Angew Chem Int Ed2005 44 4935
281 Y Sawada K Matsumoto S KondoH Watanabe T Ozawa K Suzuki BSaito T Katsuki Angew Chem Int Ed2006 45 3478
282 MK Tse C Doumlbler S Bhor M Kla-wonn W Maumlgerlein H Hugl M Bel-ler Angew Chem Int Ed 2004 435255 MK Tse S Bhor M KlawonnG Anilkumar H Jiao A Spannen-berg C Doumlbler W Maumlgerlein HHugl M Beller Chem Eur J 2006 121875
283 T Yamada K Imagawa T Nagata TMukaiyama Chem Lett 1992 2231
284 T Mukaiyama T Yamada T NagataK Imagawa Chem Lett 1993 327
285 Y Tu ZX Wang Y Shi J Am ChemSoc 1996 118 9806 ZX Wang Y TuM Frohn JR Zhang Y Shi J AmChem Soc 1997 119 11224
286 L Shu Y Shi Tetrahedon Lett 199940 8721
287 S Julia J Guixer J Masana J RocaS Colonna R Annunziata H Moli-nari J Chem Soc Perkin Trans I1982 1314
288 I Lantos V Novack in Chirality inDrug Design and Synthesis C Brown(ed) Academic Press New York 1990pp 167ndash180
289 K H Dranz personal communication290 F van Rantwijk RA Sheldon Curr
Opin Biotechnol 2000 11 554291 J-B Park DS Clark Biotechn Bioeng
2006 94 189292 F J Lakner K P Cain LP Hager
J Am Chem Soc 1997 119 443 AFDexter F J Lakner R A CampbellLP Hager J Am Chem Soc 1995117 6412
293 G P Rai Q Zong LP Hager Isr JChem 2000 40 63
294 K Hofstetter J Lutz I Lang B With-olt A Schmid Angew Chem Int Ed2004 43 2163
295 F Hollmann P-C Lin B Witholt ASchmid J Am Chem Soc 2003 1258209
296 EN Jacobsen I Marko WS MungallG Schroumlder K B Sharpless J AmChem Soc 1988 110 1968
References 221
297 J SM Wai I Marko J S SvendsenMG Finn EN Jacobsen KB Sharp-less J Am Chem Soc 1989 111 1123
298 HL Kwong C Sorato Y Ogino HChen K B Sharpless Tetrahedron Lett1990 31 2999
299 K B Sharpless W Amberg YL Ben-nani GA Crispino J Hartung K-SJeong H-L Kwong K MorikawaZ-M Wang D Xu X-L ZhangJ Org Chem 1992 57 2768 HCKolb K B Sharpless in Transition me-tals for Organic Synthesis M Beller CBolm (eds) Wiley-VCH WeinheimGermany 1998 p 219
300 M Tokunaga J F Larrow EN Jacob-sen Science 1997 277 936
301 V Conte F Di Furia G Licini GModena in Metal Promoted Selectivityin Organic Synthesis AF Noels MGraziani AJ Hubert (eds) KluwerAmsterdam 1991 p 91 F Di FuriaG Modena R Seraglia Synthesis1984 325
302 HB Kagan in Catalytic AsymmetricSynthesis I Ojima (ed) VCH Berlin1993 p 203
303 M Larsson lecture presented at ChiralEurope 2000 26ndash27 Oct 2000 Malta
304 P J Hogan PA Hopes WO MossG E Robinson I Patel Org Proc ResDev 2002 6 225
305 C Bolm F Bienewald Angew ChemInt Ed Engl 1995 34 2640
306 J Legros C Bolm Angew Chem IntEd 2003 42 5487
307 G Liu DA Cogan J A EllmanJ Am Chem Soc 1997 119 9913
308 MP J van Deurzen I J RemkesF van Rantwijk RA Sheldon J MolCatal A Chemical 1997 117 329
309 HB ten Brink HL Holland HESchoenmaker H van Lingen R We-ver Tetrahedron Asymm 1999 10 4563
310 G-J ten Brink IWCE Arends RASheldon Chem Rev 2004 104 4105
311 J D Stewart Curr Org Chem 1998 2195
312 G Carrea S Riva Angew Chem IntEd 2000 39 2226
313 V Alphand G Carrea R Wohlge-muth R Furstoss J M WoodleyTrends Biotechnol 2003 21 318
314 S Rissom U Schwarz-Linek M Vo-gel V I Tishkov U Kragl TetrahedronAsymm 1997 8 2523
315 K Seelbach B Riebel W HummelMR Kula V I Tishkov C WandreyU Kragl Tetrahedron Lett 1996 91377
316 J D Stewart K W Reed J Zhu GChen MM Kayser J Org Chem1996 61 7652 K Saigo A KasaharaS Ogawa H Nohiro Tetrahedron Lett1983 511
317 MD Mihovilovic G Chen S WangB Kyte FRochon M Kayser J DStewart J Org Chem 2001 66 733
318 MJ Taschner D J Black Q-Z ChenTetrahedron Asymm 1993 4 1387 M JTaschner L Peddadda J Chem SocChem Commun 1992 1384 USchwartz-Linek A Krodel F-A Lud-wig A Schulze S Rissom U KraglV I Tishkov M Vogel Synthesis 2001947
319 Usually 2-or 3-substituted cyclopenta-nones are converted with considerablylower enantioselectivities MM KayserG Chen J D Stewart J Org Chem1998 63 7103
320 J D Stewart K W Reed CA Marti-nez J Zhu G Chen MM KayserJ Am Chem Soc 1998 120 3541
321 N Berezina V Alphand R FurstossTetrahedron Asymm 2002 13 1953
322 C Bolm G Schlingloff K WeickhardtAngew Chem Int Ed Engl 1994 331848
323 C Bolm G Schlingloff J Chem SocChem Commun 1995 1247
51Introduction
The formation of carbonndashcarbon bonds is central to organic chemistry indeedto chemistry in general The preparation of virtually every product be it finechemical or bulk chemical will include a carbonndashcarbon bond formation atsome stage in its synthesis The importance of carbonndashcarbon bond forming re-actions can therefore not be overemphasized Consequently they have been a fo-cus of interest ever since chemists made their first attempts at synthesis In thecourse of the last 150 years many very selective and efficient reactions for theformation of carbonndashcarbon bonds have been introduced too many for thescope of this book At the same time carbonndashcarbon bond forming reactions areoften textbook examples of wastefulness The Nobel prize winning Wittig reac-tion being a particularly good illustration of why green chemistry is necessary[1] At the same time it also becomes obvious how much there still remains tobe done before chemistry is green since not even the equally Nobel prize win-ning metathesis can completely replace the Wittig reaction
This chapter focuses on the application of transition metal catalysts and en-zymes for the formation of carbonndashcarbon bonds Transition metal-catalyzed car-bonndashcarbon bond formations are not always very green but they often replaceeven less favorable conventional approaches The key to making them reallygreen is that they have to be easily separable and reusable Several of these reac-tions such as the hydroformylation oligomerisation carbonylation of alcoholsand the metathesis are therefore also treated in Chapter 1 Section 18 andChapter 7 since their greener variations are performed in novel reaction media
52Enzymes for CarbonndashCarbon Bond Formation
The synthesis of carbonndashcarbon bonds in nature is performed by a vast varietyof enzymes however the bulk of the reactions are performed by a rather limitednumber of them Indeed for the synthesis of fatty acids just one carbonndashcarbonbond forming enzyme is necessary Contrary to expectation virtually none of
223
5Catalytic CarbonndashCarbon Bond Formation
the enzymes that nature designed for building up molecules are used in organicsynthesis This is because they tend to be very specific for their substrate andcan therefore not be broadly applied Fortunately an ever increasing number ofenzymes for the formation of carbonndashcarbon bonds are available [2ndash4] Many ofthem are lyases and in an indirect approach hydrolases These classes of en-zymes were designed by nature not for making but for breaking down mole-cules By reversing the equilibrium reactions that these enzymes catalyze in thenatural substrates they can be applied to the synthesis of carbonndashcarbon bondsAs reagents that were designed by nature for degrading certain functionalgroups they are robust but not very substrate specific However they are specif-ic for the functional group they destroy in nature and generate in the laboratoryor factory Equally important they are very stereoselective Hence these enzymesare ideal for the application in organic synthesis
521Enzymatic Synthesis of Cyanohydrins
Cyanohydrins are versatile building blocks that are used in both the pharmaceu-tical and agrochemical industries [2ndash9] Consequently their enantioselective syn-thesis has attracted considerable attention (Scheme 51) Their preparation bythe addition of HCN to an aldehyde or a ketone is 100 atom efficient It ishowever an equilibrium reaction The racemic addition of HCN is base-cata-lyzed thus the enantioselective enzymatic cyanide addition should be per-formed under mildly acidic conditions to suppress the undesired backgroundreaction While the formation of cyanohydrins from aldehydes proceeds readilythe equilibrium for ketones lies on the side of the starting materials The latterreaction can therefore only be performed successfully by either bio- or chemo-cat-
5 Catalytic CarbonndashCarbon Bond Formation224
Scheme 51 Cyanohydrins are versatile building blocks
alysis when an excess of HCN is employed or when the product is constantly re-moved from the equilibrium The only advantage of this unfavorable equilibriumis that the liquid acetone cyanohydrin can replace the volatile HCN in the labora-tory It releases HCN during the synthesis of an aldehyde-based cyanohydrin im-proving safety in the laboratory significantly At the same time the atom efficiencyof the reaction is however greatly reduced Alternative methods for the safe han-dling of cyanides on a laboratory scale are for instance to use cyanide salts in solu-tion again generating waste In order to achieve high yields an excess of HCN orof the other cyanide sources is commonly used This excess cyanide needs to bedestroyed with iron (II) sulfate or bleach in the laboratory It is much easier to han-dle HCN on an industrial scale and to regain any HCN In general all work involv-ing cyanide (enzyme-catalyzed or not) must be performed in well-ventilated la-boratories and HCN detectors have to be used [6]
5211 Hydroxynitrile LyasesFor the synthesis of cyanohydrins nature provides the chemist with R- and S-se-lective enzymes the hydroxynitrile lyases (HNL) [4ndash7] These HNLs are alsoknown as oxynitrilases and their natural function is to catalyze the release ofHCN from natural cyanohydrins like mandelonitrile and acetone cyanohydrinThis is a defense reaction of many plants It occurs if a predator injures theplant cell The reaction also takes place when we eat almonds Ironically thebenzaldhyde released together with the HCN from the almonds is actually theflavor that attracts us to eat them
Since the release of HCN is a common defense mechanism for plants the num-ber of available HNLs is large Depending on the plant family they are isolatedfrom they can have very different structures some resemble hydrolases or carbox-ypeptidase while others evolved from oxidoreductases Although many of theHNLs are not structurally related they all utilize acidndashbase catalysis No co-factorsneed to be added to the reactions nor do any of the HNL metallo-enzymes requiremetal salts A further advantage is that many different enzymes are available R- orS-selective [10] For virtually every application it is possible to find a stereoselectiveHNL (Table 51) In addition they tend to be stable and can be used in organic sol-vents or two-phase systems in particular in emulsions
The R-selective Prunus amygdalus HNL is readily available from almonds Ap-proximately 5 g of pure enzyme can be isolated from 1 kg of almonds alterna-tively crude defatted almond meal has also been used with great success Thisenzyme has already been used for almost 100 years and it has successfully beenemployed for the synthesis of both aromatic and aliphatic R-cyanohydrins(Scheme 52) [11] More recently it has been cloned into Pichea pastoris guaran-teeing unlimited access to it and enabling genetic modifications of this versatileenzyme [12]
Prunus amygdalus HNL can be employed for the bulk production of (R)-o-chloromandelonitrile however with a modest enantioselectivity (ee= 83) [9]When replacing alanine 111 with glycine the mutant HNL showed a remarkably
52 Enzymes for CarbonndashCarbon Bond Formation 225
high enantioselectivity towards o-chlorobenzaldehyde and the corresponding cya-nohydrin was obtained with an ee of 965 [12] Hydrolysis with conc HClyields the enantiopure (S)-o-chloromandelic acid an intermediate for the anti-thrombotic drug clopidogrel (Scheme 53)
Recently it was described that site directed mutagenesis has led to a Prunusamygdalus HNL that can be employed for the preparation of (R)-2-hydroxy-4-phe-nylbutyronitrile with excellent enantioselectivity (ee gt 96) This is a chiralbuilding block for the enantioselective synthesis of ACE inhibitors such as ena-lapril (Scheme 54) [13]
The unmodified enzyme has also been used in ionic liquids expanding thescope of its application even further Significant rate enhancement in particularfor substrates that otherwise react only sluggishly was observed [14]
The discovery of the S-selective HNLs is more recent The application of the S-selective Hevea brasiliensis HNL was first described in 1993 [15] The potential of thisenzyme was immediately recognized and already four years after describing it for
5 Catalytic CarbonndashCarbon Bond Formation226
Table 51 Commonly used hydroxynitrile lyases (HNL)
Name and origin Natural substrate Stereoselectivity
Prunus amygdalusHNL Almonds (R)-mandelonitrile R
Linum usitatissimumHNL Flax seedlings (R)-butanone cyanohydrin
and acetone canohydrinR
Hevea brasiliensisHNL Rubber-tree leaves acetone cyanohydrin S
Sorghum bicolorHNL Millet seedlings (S)-4-hydroxy-mandelonitrile S
Manihot esculentaHNL Manioc leaves acetone cyanohydrin S
Scheme 52 Application of Prunus amygdalus HNL for thesynthesis of R-cyanohydrins
the first time it has been cloned and overexpressed making it available for large-scale applications [16] Indeed this enzyme is not only a versatile catalyst in thelaboratory industrially it is used to prepare (S)-m-phenoxymandelonitrile with highenantiopurity (ee gt 98) [9] This is a building block for the pyrethroid insecticidesdeltamethrin and cypermethrin and is used on a multi-ton scale (Scheme 55) TheHNL-based process replaced another enzymatic process that was used earlier forthe production of the enantiopure cyanohydrin the kinetic resolution of m-phen-oxymandelonitrile acetate with a hydrolase from Arthrobacter globiformis [17]
As mentioned above the synthesis of cyanohydrins from ketones is difficultdue to the unfavorable equilibrium However it can be achieved When methylketones were treated with only 15 equivalents of HCN in an emulsion of citratebuffer (pH 40) and MTBE the S-selective Manihot esculenta HNL catalyzed thesynthesis of the corresponding cyanohydrins with good yields (85ndash97) and en-antioselectivities (69ndash98) The corresponding esters were then used in a sec-ond carbonndashcarbon bond forming reaction Since cyanohydrins from ketonescannot be deprotonated adjacent to the nitrile group the esters could be selec-tively deprotonated and then a ring closing attack on the nitrile function yieldedthe unsaturated lactones (Scheme 56) When the nitrile function was first con-
52 Enzymes for CarbonndashCarbon Bond Formation 227
Scheme 53 Modified Prunus amygdalus HNL is applied forthe synthesis of enantiopure R-o-chloromandelonitrile aprecursor for the synthesis of clopidogrel
Scheme 54 Modified Prunus amygdalus HNL catalyzes theenantioselective formation of potential precursors for ACEinhibitors
verted into an ester via a Pinner reaction the intramolecular Claisen reactiongave chiral tetronic acids [18]
5212 Lipase-based Dynamic Kinetic ResolutionA completely different enzyme-catalyzed synthesis of cyanohydrins is the lipase-catalyzed dynamic kinetic resolution (see also Chapter 6) The normally unde-sired racemic base-catalyzed cyanohydrin formation is used to establish a dy-namic equilibrium This is combined with an irreversible enantioselective ki-netic resolution via acylation For the acylation lipases are the catalysts ofchoice The overall combination of a dynamic carbonndashcarbon bond formingequilibrium and a kinetic resolution in one pot gives the desired cyanohydrinsprotected as esters with 100 yield [19ndash22]
This methodology was employed to prepare many heterocyclic cyanohydrinacetates in high yields and with excellent enantioselectivities Candida antarcticalipase A (CAL-A) being the lipase of choice (Scheme 57) [23] A recent detailedstudy of the reaction conditions revealed that the carrier on which the lipase isimmobilised is important generally Celite should be used for aromatic sub-strates With Celite R-633 as support for Candida antarctica lipase B (CAL-B)
5 Catalytic CarbonndashCarbon Bond Formation228
Scheme 55 Hevea brasiliensis HNL catalyzes a key step in theenantioselective synthesis of pyrethroid insecticides
Scheme 56 HNL-catalyzed formation of cyanohydrins fromketones and their application in synthesis
mandelonitrile acetate was synthesised in 97 yield and ee= 98 (Scheme 58)[24 25] Drawbacks of this approach are that an R-selective variant has so farnot been developed and most lipases do not accept sterically demanding acidsConsequently attempts at preparing the pyrethroid insecticides in one step viathis approach were not successful
522Enzymatic Synthesis of -Hydroxyketones (Acyloins)
The bifunctional nature and the presence of a stereocenter make -hydroxyketones(acyloins) amenable to further synthetic transformations There are two classicalchemical syntheses for these -hydroxyketones the acyloin condensation andthe benzoin condensation In the acyloin condensation a new carbonndashcarbon bondis formed by a reduction for instance with sodium In the benzoin condensationthe new carbonndashcarbon bond is formed with the help of an umpolung induced bythe formation of a cyanohydrin A number of enzymes catalyze this type of reac-tion and as might be expected the reaction conditions are considerably milder [2ndash4 26 27] In addition the enzymes such as benzaldehyde lyase (BAL) catalyze theformation of a new carbonndashcarbon bond enantioselectively Transketolases (TK)
52 Enzymes for CarbonndashCarbon Bond Formation 229
Scheme 57 CAL-A-catalyzed formation of chiral cyanohydrins
Scheme 58 Synthesis of enantiopure mandelonitrile acetate via a dynamic kinetic resolution
and decarboxylases such as benzoylformate decarboxylase (BFD) catalyze the acy-loin formation efficiently too Like the chemical benzoin reaction the latter twobreak a carbonndashcarbon bond while forming a new one This making and breakingof bonds involves a decarboxylation in both the TK and the decarboxylase-catalyzedreactions When TK is applied it might also involve the discarding of a ketone andnot only CO2 [27 28] The atom efficiency of these enzymes is therefore limited Incontrast to TK BFD can however also catalyze the formation of new carbonndashcar-bon bonds without decarboxylation (Scheme 59)
All of the enzymes that catalyze the acyloin formation from two carbonyl groupsrely on a cofactor thiamin diphosphate The unphosphorylated thiamin is alsoknown as vitamin B1 deficiency thereof is the cause of the disease Beriberi Thia-min diphosphate induces an umpolung of the carbonyl group similar to the cya-nide in the benzoin condensation After deprotonation its ylide attacks the carbo-nyl group of the aldehyde Shifting of the negative charge from the alcoholate tothe carbanion initiates this umpolung This enables the nucleophilic attack on thesecond aldehyde stereoselectively forming the carbonndashcarbon bond for the -hy-droxyketones Another shift of the charge and elimination releases the desired acy-loin and the ylide is available for further action (Scheme 510)
In the decarboxylase- and TK-catalyzed reactions the ylide attacks the ketofunction of -keto acids to form an intermediate carboxylate ion Decarboxyla-tion ie carbonndashcarbon bond fragmentation leads to the same reactive carba-nion as in the BAL-catalyzed reaction (Scheme 510) Once again it enantiose-lectively forms the new carbonndashcarbon bond of the desired -hydroxyketone TKrequires not only thiamin diphosphate but also a second co-factor Mg2+ [28]
The enantioselective synthesis of -hydroxyketones via a carbonndashcarbon bondforming reaction has received a significant impulse during recent years Fourdifferent enzymes are commonly used for this reaction BAL BFD pyruvatedecarboxylase (PDC) and TK Many different compounds can be prepared with
5 Catalytic CarbonndashCarbon Bond Formation230
Scheme 59 BAL BFD and TK catalyze the formation of -hydroxyketones (acyloins)
S
their aid however not every stereoisomer is accessible yet Moreover it is stilldifficult to perform the reaction of two different aldehydes to obtain the mixedacyloins in a predictable manner
The R-selective BAL accepts either two aromatic aldehydes or an aliphatic andan aromatic aldehyde as substrates This enables enantioselective access to avariety of biologically active compounds and natural products such as Cytoxa-zone a metabolite from Streptomyces sp (Scheme 511) [29] If formaldehyde isused instead of prochiral acetaldehyde or its derivatives achiral hydroxyacetophe-nones are obtained [30]
Both BAL and BFD can be applied for R-selective cross coupling reactions be-tween two aromatic aldehydes (Scheme 512) This opens a direct access to ahuge variety of compounds Their stereoselectivity in these reactions is identicaltheir substrate specificity however is not Of particular interest is that BFD isonly R-selective for the coupling of two aromatic aldehydes For the coupling of
52 Enzymes for CarbonndashCarbon Bond Formation 231
Scheme 510 Catalytic cycle in thiamin diphosphate basedcarbonndashcarbon bond forming enzymes
Scheme 511 BAL-catalyzed synthesis of carbonndashcarbon bonds
two aliphatic aldehydes or of aliphatic aldehydes with aromatic aldehydes BFDis S-selective (Schemes 59 and 512) Consequently BAL and BFD complementeach otherrsquos stereoselectivity in coupling reactions between an aromatic and ali-phatic aldehyde widening the scope of the cross coupling approach [31 32]
In the above-described cross coupling reactions between an aromatic and an ali-phatic aldehyde the keto group of the product is always adjacent to the benzene ring(Schemes 59 and 512) With pyruvate decarboxylase (PDC) this selectivity is turnedaround It catalyzes the reaction of pyruvate with benzaldehyde After decarboxyla-tion of the pyruvate a new carbonndashcarbon bond is formed Fortunately acetaldehydecan be used instead of pyruvate improving the atom efficiency of the reaction Witheither pyruvate or acetaldehyde the cross coupling with benzaldehyde yields (R)-phenylacetylcarbinol in good optical purity This process has been performed onan industrial scale since the 1930s Whole yeast cells are used and pyruvate is em-ployed as a starting material together with benzaldehyde This acyloin is convertedvia a platinum-catalyzed reductive amination on a commercial scale into (ndash)-ephe-drine (Scheme 513) [26 33] The newest development for the industrial applicationis the introduction of the PDC from Zymomonas mobilis a bacterial PDC [33 34]This PDC accepts acetaldehyde instead of the significantly more expensive pyru-vate While the industrial synthesis of (R)-phenylacetylcarbinol with PDC was verysuccessful PDC has not been used for many other acyloin syntheses
The sugar metabolism is a source of many enzymes the transketolase (TK)being one of them TK transfers an -hydroxy carbonyl fragment from D-xylu-lose-5-phosphate onto D-ribose-5-phosphate forming D-sedoheptulose-7-phos-phate and D-glyceraldehyde-3-phosphate (Scheme 514) Since this reaction is anequilibrium reaction and starting materials and products are of similar stabilityit is not very versatile for organic synthesis Fortunately TK also accepts pyru-vate instead of xylulose Under these modified circumstances carbon dioxide
5 Catalytic CarbonndashCarbon Bond Formation232
Scheme 512 BAL and BFD-catalyzed cross coupling reactionsbetween two aromatic aldehydes
and not D-glyceraldehyde-3-phosphate is the leaving group This renders the re-action irreversible and considerably more atom efficient [28] More interestingstill is the recent observation that yeast TK can activate the two-carbon unit gly-colaldehyde No decarboxylation occurs and the atom efficiency of this couplingreaction yielding erythrulose (Scheme 515) is 100 [35] This result demon-strated that TK can be employed similar to an aldolase and the path is nowopen for efficient cross coupling reactions
52 Enzymes for CarbonndashCarbon Bond Formation 233
Scheme 513 The PDC-catalyzed synthesis of (R)-phenylacetyl-carbinol induces the stereochemistry in the industrialsynthesis of (ndash)-ephedrine
Scheme 514 In nature TK catalyzes an equilibrium reaction
Scheme 515 TK can be employed like an aldolase in a 100atom efficient reaction