copyright 2002 © mark brandt, ph.d. addition reactions
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Copyright 2002 © Mark Brandt, Ph.D.
Addition Reactions
Copyright 2002 © Mark Brandt, Ph.D.
Exam III
• Nucleophilic substitution– Reaction mechanisms
• SN1
• SN2
– Stereochemistry– Leaving groups– Nucleophiles– Substrates– Solvent effects– Products
Copyright 2002 © Mark Brandt, Ph.D.
Exam III
• Elimination reactions– Reaction mechanisms
• E1• E2• Dehydration
– Stereochemistry– Leaving groups– Nucleophiles– Substrates– Solvent effects– Products
Copyright 2002 © Mark Brandt, Ph.D.
Exam III
• Factors controlling competition between reaction types– E2 vs SN2 vs SN1 vs E1
• Rearrangement reactions– Reaction mechanisms
• Methyl and alkyl shifts• Hydride shifts
– Products• Dihalide reactions
– Synthesizing dihalides– Synthesizing alkenes and alkynes
Copyright 2002 © Mark Brandt, Ph.D.
Exam III
• Nomenclature• Spartan problem?• Mechanism• Energy profile diagram• Fill in the blank
• Relative carbocation stability• Relative alkene stability• Review session Wednesday 7 PM
CH3
Br KOC(CH3)3
CH3 CH3
+
Major Minor
Copyright 2002 © Mark Brandt, Ph.D.
Hydrogenation(Alkene Reduction)
• Platinum or Palladium catalysts allow conversion of alkenes or alkynes to alkanes.
• The catalyst has a large surface area. Under high pressure the H2 will dissociate to atomic hydrogen adsorbed to catalyst surface.
• The H will add to the same face of the alkene (syn addition).
CH3
CH3
H2/PtCH3
CH3
H
H
Copyright 2002 © Mark Brandt, Ph.D.
Addition Reactions
• Alkenes are substrates for reactions in which groups add across the double bond.
• An example is the addition of a halogen molecule (e.g. Br2) to form a vicinal dibromide.
R
CR
C
R
R
A B R C C R
R
B
R
A
+
Copyright 2002 © Mark Brandt, Ph.D.
Reactivity of Alkenes
• The bond of an alkene is weaker than typical bonds. Replacing a bond with a bond usually results in a lower energy state.
• The orbitals of a double bond are exposed to attack. Steric hindrance is minimal.
• The orbitals contain relatively loosely associated electrons, and are subject to electrophilic attack.
• Electrophile = “electron-loving”
Copyright 2002 © Mark Brandt, Ph.D.
General Mechanism
• An alkene can act as a Lewis base.
• Carbocations are Lewis acids.
R
CR
C
R
R
A B
R
CR C+
R
RA
B
R C C R
R
B
R
A
Copyright 2002 © Mark Brandt, Ph.D.
Hydrogen Halide Addition
• Markovnikov’s rule – the hydrogen adds to the carbon that has more hydrogens.
• Markovnikov’s rule – the addition occurs to yield the more stable carbocation intermediate.
• This is an example of regioselectivity – the predictable preference of one product over others.
H
CH
C
CH3
CH3
H Br
H
CH C+
CH3
CH3H
Br
H C C CH3
CH3
Br
H
H
Copyright 2002 © Mark Brandt, Ph.D.
Hydrogen Halide Addition
• Hydrogen halide addition may result in the creation of a stereocenter.
• The products form as a racemic mixture.
H
CH
C
H
CH2 CH3
H I
H C C CH2
H
I
H
H
CH3C C
+H
CH2 CH3H
H
H
Copyright 2002 © Mark Brandt, Ph.D.
Sulfuric Acid Addition
• Although hydrogen sulfate ion is a poor nucleophile, in the absence of other nucleophiles, it will attack carbocations.
H
CH
C
H
CH2 CH3
H C C CH2
H
OSO3H
H
H
CH3C C
+H
CH2 CH3H
H
H
S
O
OO
O
HH S
O
OO
O
H OH2
H2SO4
H C C CH2
H
OH
H
H
CH3
+_
Conc.H2SO4
Copyright 2002 © Mark Brandt, Ph.D.
Alcohol Synthesis
• Alcohols may be synthesized directly.
• The reaction is the reverse of the dehydration reaction.
• Rearrangement is a problem, whenever a more stable carbocation can be formed.
H
CH
C
H
CH2 CH3
H C C CH2
H
OH
H
H
CH3 OH C CH3
CH3
CH3
OH2
H2SO4 +
Copyright 2002 © Mark Brandt, Ph.D.
Alcohol Synthesis
• Because the reaction is reversible, it is difficult to get the reaction to go to completion; dilute acid is used.
• The dehydration reaction is more useful, because the product can be removed by distillation during the reaction.
• The conjugate base of the acid must be a poor nucleophile (e.g. sulfate or phosphate) to prevent SN1 and other reactions.
Copyright 2002 © Mark Brandt, Ph.D.
Alkenes and Halogens
• Alkenes react readily with halogen molecules.
• The reaction must be performed in a non-polar solvent to prevent other nucleophilic reactions.
CCCH3
H H
CH3
Br2CCCH3
H H
CH3
BrBrCCl4
Copyright 2002 © Mark Brandt, Ph.D.
Halohydrin Formation
• If a halogen molecule reaction with an alkene in water, the product is a halohydrin.
CCCH3
H CH3
CH3
Br2
OH2
Br Br
CCCH3
H CH3
CH3
Br+
Bromonium ion
O
H
H
CCCH3
H
CH3
CH3
Br
O+
H
H
O
H
H
CCCH3
H
CH3
CH3
Br
OH
Copyright 2002 © Mark Brandt, Ph.D.
Halonium Ions
• The properties of the cyclic halonium ion have two consequences:– The second attack occurs anti to the first.
– The second attack occurs at the more substituted carbon (unless the more substituted carbon is too sterically hindered).
CCCH3
H CH3
CH3
Br+
O
H
H
+
Cl2
OH2
Cl+ Cl
OH2
+
Cl
OH
Copyright 2002 © Mark Brandt, Ph.D.
Alkyne Addition
• Halogens add across triple bonds in the same way as across double bonds.
CH3 C CHCCl4
Br2CH3 C CH
Br Br
CCl4
Br2CH3 C CH
Br Br
Br Br
Copyright 2002 © Mark Brandt, Ph.D.
Alkyne Addition
• Hydrohalogen addition across triple bonds is also similar to addition across double bonds. Addition follows Markovnikov’s rule.
CH3 C CHCCl4
BrHCH3 C CH
Br H
CCl4
BrHCH3 C CH
Br H
Br H
Copyright 2002 © Mark Brandt, Ph.D.
Alkene Oxidation
MnO O
O O
H H
OH OH
coldKMnO4
OH2
OH
MnO O
O O
Copyright 2002 © Mark Brandt, Ph.D.
Alkene Oxidation
MnO O
O O
heatKMnO4
OH2
OHOHOH
O O
Copyright 2002 © Mark Brandt, Ph.D.
Carbenes
• A carbene is a highly unstable compound containing a carbon with two bonds.
CH2 N+
N N N:CH2 +heat
CHCl3KOC(CH3)3
C Cl
Cl
Cl Cl:CCl2 +
CH2I2 Zn(Cu) ICH2ZnI+
Copyright 2002 © Mark Brandt, Ph.D.
Carbene Reactions
• Carbenes react readily with double bonds, by forming a three membered ring.
ICH2ZnI
H H
+