amines - austin community · pdf filesteps r r' ho nhr" hemiaminal r r' n...
TRANSCRIPT
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Chapter 20
Amines
Ch. 20 - 1
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Ch. 20 - 2
1. Nomenclature
NH2NH2
Butylamine Cyclohexylamine
1o Amines
Butylethylamine
N
HDiethylamine
N
H
2o Amines
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Ch. 20 - 3
3o Amines
Triethylamine
N
Butylethylmethylamine
N
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Ch. 20 - 4
1A. Arylamines
Aniline N,N-Dimethylaniline
NH2 N
NH2
CH3
p-Toluidine(4-Methylbenzeneamine)
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Ch. 20 - 5
1B. Heterocyclic Amines
Aziridine Pyrrole
NN
N
N N
HH
H
Pridine
Indole Quinoline
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Ch. 20 - 6
2. Physical Properties and Structure of Amines
2A. Physical Properties
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Ch. 20 - 7
2B. Structure of Amines
NR1
R2
R3
N: sp3 hybridized
Trigonal pyramidal
Bond angles close to 109.5o
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Ch. 20 - 8
3o Amines with three different groups
N
R1
R2
R3
N
R1
R2
R3
● The two enantiomeric forms interconvert rapidly Impossible to resolve enantiomers
● Pyramidal or nitrogen inversion Barrier ~ 25 kJ/mol Enough to occur rapidly at room
temperature
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Ch. 20 - 9
Ammonium salts with four different groups
N
R1
R2
R3
N
R1
R2
R3
R4 R4
X X
enantiomerscan be resolved
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Ch. 20 - 10
3. Basicity of Amines:Amine Salts
RNH3+ + H2O RNH2 + H3O
+
Ka =[RNH2][H3O
+]
[RNH3+]
pKa = − log Ka
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Ch. 20 - 11
The aminium ion of a more basic amine will have a larger pKa than the aminium ion of a less basic amine
H
NH H
H
H
NCH3 H
H
H
NCH3CH2 H
H
Aminiumion pKa
9.26 10.64 10.75
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Ch. 20 - 12
NR H
H
+ H OH
H
NR H
H
OH2+> >
By releasing electrons, R— stabilizes the alkylaminium ion through dispersal of charge
>
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Ch. 20 - 13
(CH3)3N > (CH3)2NH > CH3NH2 > NH3
3o 2o 1o
Gas phase
(CH3)2NH > CH3NH2 > (CH3)3N > NH3
2o 1o 3o
Aqueous solution
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Ch. 20 - 14
3A. Basicity of Arylamines
H
NH H
Aminiumion pKa
10.64 4.58 5.08
H
NH H
H
NH H
CH3
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Ch. 20 - 15
NH2 NH2 NH2
NH2NH2
● Five resonance structures
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Ch. 20 - 16
NH2
+ H2O
NH3
+ OH
Aniliniumion
NH3 NH3
● Only two resonance structures
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Ch. 20 - 17
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Ch. 20 - 18
3B. Basicity of Heterocyclic Amines
N
N
N NN
H HH
Order ofBasicity: >> >
pKa of theconjugate acid: 11.2 7 5.2 0.4
(c.f. Et3N, pKa of the conjugate acid = 9.7)
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Ch. 20 - 19
N N NHH
H
H
H H
•
(lost of aromaticity)
+ H+
N
N
N
N
N
N
H H
H
H
HN
N
H
H
+ H+
(still aromatic)Imidazole(a very commonbase in organic
synthesis)
•
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Ch. 20 - 20
3C. Amines versus Amides
O
R NH2
: :
:
O
R NH2
: :
:
:
O
R NH2
: :
:Amide
N-Protonated AmideO
R NH3
: : O
R NH3
: ::
Amides are far less basic than amines (even less basic than arylamines). The pKa of the conjugate acid of a typical amide is about zero
Larger resonance
stabilization
Smaller resonance
stabilization
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Ch. 20 - 21
O
R NH2
:
O
R NH3
+ OH+ H2O
NH2
:
NH3 + OH+ H2OR R>
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Ch. 20 - 22
3D. Aminium Salts and QuaternaryAmmonium Salts
R2
NR1 R3 + H Cl
R2
NR1 R3 + R4 Br
H2O
R2
NR1 R3
H(aminium salt)
Cl
R2
NR1 R3
R4
(quaternaryammonium salt)
Br
However, R4N⊕ ⊖OH are strong
bases (as strong as NaOH)
Cannot actas bases
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Ch. 20 - 23
3E. Solubility of Amines in AqueousAcids
R2
NR1 R3 + H X
R2
NR1 R3
H(water soluable)
X
O
R NH2
water-insoluableHX
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Ch. 20 - 24
3F. Amines as Resolving Agents
Enantiomerically pure amines are often used to resolve racemic forms of acidic compounds by the formation of diastereomeric salts
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Ch. 20 - 25
OH
O
HO HHO
O
OHH(R) (S)
H2N
HH3C(R)-Amine (optically pure)
+
Racemic (R,S)-acid This is the resolving agent
O
O
HO H
(R)
H3N
HH3C
(R)
O
O
OHH
(S)
H3N
HH3C
(R)separate
(R,R)-salt (S,R)-salt
OH
O
HO H(R)-Acid
HO
O
OHH(S)-Acid
H3O+ H3O
+
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Ch. 20 - 26
4. Preparation of Amines
4A. Through Nucleophilic Substitution Reactions
Alkylation of ammonia
XNH3
NH2
H
X
NH3
NH2
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Ch. 20 - 27
NH2 N
H X
X H
(over-alkylation)
NH3
N
HNH3
X
N N+
X
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Ch. 20 - 28
N N NNaN3
Alkylation of azide ion and reduction
X
NH2
Na/EtOHorLiAlH4
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Ch. 20 - 29
The Gabriel synthesis
N
O
O
H1. KOH
2.Br
N
O
O
NH2NH2EtOH, heat
N
N
O
O
H
H
H2N +
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Ch. 20 - 30
Alkylation of 3o amines
N
R
R
R Br+
(SN2)
N
R
R
R Br
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Ch. 20 - 31
4B. Preparation of Aromatic Amines through Reduction of Nitro Compounds
R
H
R
NO2
R
NH2HNO3
H2SO4
H2, catalyst
1. Fe, HCl2. NaOH
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Ch. 20 - 32
4C. Preparation of Primary, Secondary,and Tertiary Amines through Reductive Amination
O
R R'
aldehydeor
ketone
NH3
[H]
N
R R'H
H H
1o amine
R"NH2
[H]
N
R R'H
H R"
2o amine
R"R"'NH
[H]
N
R R'H
R"' R"
3o amine
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Ch. 20 - 33
O
R R'H2N R"+
Mechanismtwo
steps
R R'
HO NHR"
Hemiaminal
R R'
NR"(- H2O)
Imine
[H]
NHR"
R R'H
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Ch. 20 - 34
(1) O NH2
NH3, H2/Ni
heat &pressure
Examples
(2)O N
H1.
2. NaBH3CN
NH2
(3)O N
NH
1.
2. LiBH3CN
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Ch. 20 - 35
4D. Preparation of Primary, Secondary, or Tertiary Amines through Reduction of Nitriles, Oximes, and Amides
R C N
H
CR N
OHor[H]
RCH2NH2
O
CR N
R'
R"
RCH2N
R'
R"
[H]
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Ch. 20 - 36
(1) Br C
CH2NH2
NNaCN
DMSO
Ra NiH2Oheat
Examples
(2)O N
OHH2N OH Na
EtOH
NH2
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Ch. 20 - 37
Examples
(3)Cl
pyridine
NH
O
N
O
1. LiAlH42. H2O
N
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Ch. 20 - 38
4D. Preparation of Primary Amines through the Hofmann and Curtius Rearrangements
O
R NH2
Br2, NaOH
H2OR NH2
+ NaBr + Na2CO3
Hofmann rearrangement
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Ch. 20 - 39
(1) NH2
O
Br2
NaOH
NH2
Examples
(2)
NH2
O
NH2Br2
NaOH
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Ch. 20 - 40
MechanismO
R N
H
HOH O
R N
H
Br Br O
R N
H
Br
HO
O
R NBr
O C NR (Hofmann
rearr.)(isocyanate)
HOO C
N
OH
R
O C
N
O
R
H
+ CO2H
NR
H OHR NH2
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Ch. 20 - 41
Curtius rearrangementO
R Cl
NaN3O
R N N NO C N
R+ N2 (g)
heat
R NH2
H2O
CO2 (g) +
O
Cl 1. NaN3
2. heat3. H2O
NH2
e.g.
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Ch. 20 - 42
5. Reactions of Amines
H Cl+Et3N
Acid-base reactions
Et3N H + Cl
+ BrNH2
Alkylation
BrN
H
H
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Ch. 20 - 43
+N
H
Cl
O Acylation
N
O(- HCl)
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Ch. 20 - 44
NH2 NH2 NH2
E
E
E+
Electrophilic aromatic substitution
NH2: powerful activating group, ortho-para director
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Ch. 20 - 45
5A. Oxidation of Amines
R3N O
(a tertiaryamine oxide)
R3NH2O2 or
R OO
H
O
(per acid)
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Ch. 20 - 46
6. Reactions of Amines withNitrous Acid
Nitrous acid (HONO) is a weak, unstable acid
HCl(aq) + NaNO2(aq) HONO(aq) + NaCl(aq)
H2SO4(aq) + 2 NaNO2(aq)
2 HONO(aq) + Na2SO4(aq)
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Ch. 20 - 47
6A. Reactions of Primary Aliphatic Amines with Nitrous Acid
1o aliphatic amineR NH2
R N N X
NaNO2HX (HONO)
RX alkyl halides
alcoholsH2O
- H+alkenes
(aliphatic diazonium salt)
(highly unstable)
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Ch. 20 - 48
6B. Reactions of Primary Arylamines with Nitrous Acid
N N
XNaNO2
HX
R
NH2
R
(arenediazonium salt)(stable at <5oC)
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Ch. 20 - 49
H
NAr
H
N O
NAr
H
N OH
HONO + H3O+ + A:−
Mechanism
H2O NO + H2O
+ 2 H2ON O
H
NAr
H
OH2
- H3O+
NAr
H
N OH A
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Ch. 20 - 50
- HA + HA
NAr N OH2
Mechanism (Cont'd)NAr
H
N OH
A
NAr N OH- HA
+ HADiazohydroxide
NAr NNAr NH2O +
diazonium ion
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Ch. 20 - 51
6C. Reactions of Secondary Amines with Nitrous Acid
NaNO2
HCl, H2ON H N N O
N
H
N
NO
NaNO2
HCl, H2O
N-Nitroso-amines
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Ch. 20 - 52
6D. Reactions of Tertiary Amines with Nitrous Acid
NaNO2
HCl, H2O
8oC
N N N O
NaNO2
HCl, H2OEt3N + Et3N N O ClEt3NH Cl
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Ch. 20 - 53
7. Replacement Reactions of Arenediazonium Salts
N NHONO
0 - 5oC
R
NH2
R
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Ch. 20 - 54
7A. Syntheses Using Diazonium Salts
NN
R
R
OHCu2O, Cu2-
H2O
R
ClCuCl
CuBr
R
Br
R
CNCuCN
KI
R
I
1. HBF4
2. heat
R
F
H3PO2, H2O
R
H
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Ch. 20 - 55
7B. The Sandmeyer Reaction: Replacement of the Diazonium Group by -Cl, -Br, or -CN
CuCl
15 - 60oC
HCl, NaNO2
H2O
0 - 5oC
N2Cl
CH3
NH2
CH3
CH3
Cl
+N2
o-Toluidine
o-Chlorotoluene(74-79% overall)
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Ch. 20 - 56
CuBr
100oC
HBr, NaNO2
H2O
0 - 10oC
N2BrNH2
Br
+N2
m-Chloroaniline
m-Bromochlorobenzene(70% overall)
Cl Cl
Cl
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Ch. 20 - 57
CuCN
90 - 100oC
HCl, NaNO2
H2Oroom temp.
N2Cl
NO2
NH2
NO2
NO2
Cl
+N2
o-Nitroaniline
o-Nitrobenzonitrile(65% overall)
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Ch. 20 - 58
7C. Replacement by —I
KIH2SO4, NaNO2
H2O
0 - 5oC
NO2NO2 NO2
+ N2
p-Nitroaniline p-Iodonitrobenzene(81% overall)
NH2 N2HSO4 I
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Ch. 20 - 59
7D. Replacement by —FCH3CH3
CH3
BF3 + N2 +
m-Toluidine
m-Fluorotoluene(69%)
NH2 N2BF4
F
(1) HONO, H+
(2) HBF4
m-Toluenediazoniumfluoroborate
(79%)
heat
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Ch. 20 - 60
7E. Replacement by —OH
CH3 CH3
p-Toluenediazoniumhydrogen sulfate
p-Cresol(93%)
N2HSO4 OH
Cu2O
Cu2+, H2O
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Ch. 20 - 61
7F. Replacement by Hydrogen: Deamination by Diazotization
CH3CH3 CH3
N2 +
p-Toluidine 65%(from p-Toluidine)
NH2 HN NH2
O
O2
(1) Br2(2) OH−, H2O
Brheat
H2SO4, NaNO2
H2O, 0 - 5oC
H2O, 25oC
O
H3PO2
CH3
N2
Br
CH3
Br
m-Bromotoluene(85% from 2-bromo-
4-methylaniline)
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Ch. 20 - 62
8. Coupling Reactions of Arenediazonium Salts
N N X + Q
N N Q
(Q = NR2 or OH)
(azo dyes)
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Ch. 20 - 63
(1)
N2 Cl OH
+
NN
OH
NaOH
H2O, 0oC
(orange solid)
Examples
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Ch. 20 - 64
(2)
N2 Cl N
+
NN
N
NaOAc
H2O, 0oC
(yellow solid)
Me
Me
Me
Me
Examples
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Ch. 20 - 65
(3)
N2 Cl OH
+
NN
NaOHH2O
Me
HO
Me
Examples
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Ch. 20 - 66
9. Reactions of Amines with Sulfonyl Chlorides
+
R"
NR' H Cl S Ar
O
O
R"
NR' S Ar
O
O
+ HCl
1. H3O+, heat
2. NaOH
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Ch. 20 - 67
9A. The Hinsberg Test
Sulfonamide formation is the basis for a chemical test, called the Hinsberg test, that can be used to demonstrate whether an amine is primary, secondary, or tertiary
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Ch. 20 - 68
1o Amine
+
H
NR H Cl S
O
O
H
NR S
O
O
H
NR S
O
O
OH−
(-HCl)
HClNR S
O
O
K
water insoluable(precipitate)
water-soluable salt(clear solution)
KOH
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Ch. 20 - 69
2o Amine
+
R2
NR1 H Cl S
O
O
R2
NR1 S
O
O
OH−
(-HCl)
water insoluable(precipitate)
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Ch. 20 - 70
3o Amine
+
R2
NR1 R3 Cl S
O
O
R2
NR1 R3
NaOH
H3O+
water soluable
No apparentchange
H
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Ch. 20 - 71
10. Synthesis of Sulfa Drugs
NH2
O
HNO
O2
O
HN
SO2Cl
2 HOSO2Cl
80oC
H2N R
(-HCl)
O
HN
SO2NHR
NH2
SO2NHR
1. dilute HCl, heat
2. HCO3−
(-H2O)
Aniline Acetanilide
Sulfanilamide
p-Acetamidobenzene-sulfonyl chloride
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Ch. 20 - 72
11. Analysis of Amines
11A. Chemical Analysis
Dissolve in dilute aqueous acid Moist pH paper
⇒ basic Hinsberg test 1o aromatic amines
⇒ azo dye formation with 2-naphthol
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Ch. 20 - 73
11B. Spectroscopic Analysis
IR● 1o amines
3300 – 3555 cm-1 (N–H)⇒ two bands
● 2o amines 3300 – 3555 cm-1 (N–H)
⇒ one band only● 3o amines
No bands at 3300 – 3555 cm-1
region
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Ch. 20 - 74
● Aliphatic amines 1020 – 1220 cm-1 (C–N)
● Aromatic amines 1250 – 1360 cm-1 (C–N)
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Ch. 20 - 75
1H NMR spectra● 1o and 2o amines
N–H δ (0.5 – 5 ppm), usually broad, exact position depends on the solvent, concentration, purity and temperature
● N–H protons are not usually coupled to protons on adjacent carbons
● Protons on the α carbon of an aliphatic amine are deshielded by the electron-withdrawing effect of the nitrogen and absorb typically in the δ 2.2–2.9 region
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Ch. 20 - 76
● Protons on the β carbon are not deshielded as much and absorb in the range δ 1.0–1.7
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Ch. 20 - 77
13C NMR spectra
NH223.0 34.0
14.3 29.7 42.5
13C NMR chemical shifts (δ)
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Ch. 20 - 78
Mass spectra● The molecular ion in the mass spectrum
of an amine has an odd number mass (unless there is an even number of nitrogen atoms in the molecule)
● The peak for the molecular ion is usually strong for aromatic and cyclic aliphatic amines but weak for acyclic aliphatic amines
● Cleavage between the α and β carbons of aliphatic amines is a common mode of fragmentation
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Ch. 20 - 79
12. Eliminations Involving Ammonium Compounds
12A. The Hofmann Elimination
H
NR3
A quaternaryammoniumhydroxide
OH
HOH
+
heat
NR3
+
An alkene
A tertiaryamine
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Ch. 20 - 80
A quaternaryammonium
halide
RNMe3X
Ag2O
H2O
+ 2 AgX
A quaternaryammoniumhydroxide
RNMe3HO
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Ch. 20 - 81
Although most eliminations involving neutral substrates tend to follow the Zaitsev rule, eliminations with charged substrates tend to follow what is called the Hofmann rule and yield mainly the least substituted alkene
75%Br
+ NaBr + EtOH+EtONa
EtOH
25oC25%
5%NMe3
+ NMe3 + H2O+−OH
150oC95%
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Ch. 20 - 82
H
NMe3
Carbanion-liketransition state
(gives Hofmann orientation)
HOδ−
δ− H
Br
HOδ−
δ−
Alkene-liketransition state
(gives Zaitsev orientation)
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Ch. 20 - 83
12B. The Cope Elimination
+N
Me
O150oCMe
R
H
RO N
H
Me
Me
A tertiaryamine oxide
An alkene N,N-Dimethyl-hydroxylamine
H
N
Oe.g.
heatN OH+
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Ch. 20 - 84
13. Summary of Preparations and Reactions of Amines
Preparation of amines
R NH2
N
O
O
H
1. KOH2. R-X3. NH2NH2, EtOH, heat
R Br
1. NaN32. LiAlH4
R Br
NH3R NO2
H2, cat. or1. Fe, HCl2. NaOH
O
R1 R2R =
R1 R2
NH3[H]
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Ch. 20 - 85
R NH2
N
R1 R2R =
R1 R2
OH
NaEtOH
1. LiAlH42. H2O
C NR
O
R NH2
1. LiAlH42. H2O
(R = R1CH2)
O
R NH2
Br2NaOH
1. NaN32. heat3. H2O
O
R Cl
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Ch. 20 - 86
Reactions of amines
R NH2
H X
RNH3 X
R N
H
S
O
O
Ar
ClS
O
O
Ar1. , NaOH
2. HCl
O
R' Cl
O
R'NR
base
H
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Ch. 20 - 87
Ar NH2
N2
Q
NN
Q
(Q = NR2 or OH)
HONO
0-5oCAr N2
Ar OHH2O
Cu2O, Cu2+
Ar ClCuCl
Ar BrCuBr
Ar CNCuCN
Ar IKI
Ar F1. HBF4
2. heat
Ar HH3PO2
H2O
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Ch. 20 - 88
H
NR3
+ H2O + NR3heat
OH+
Hofmann Elimination
Cope Elimination
NMe
H OMe
syn elimination
heat
MeN
Me
OH
+
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Ch. 20 - 89
END OF CHAPTER 21