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Amines : Page 1
Amines Organic Bases • amines are trivalent, but with a tetrahedral arrangement of electron pairs, although the geometry of a neutral
amine is properly described as trigonal pyramidal, since unlike nuclei, the exact positions of an electron pair cannot be defined, an exception is an ammonium salt that is surrounded by 4 atoms (nuclei)
1 Nomenclature IUPAC priority: acid > ester > amide > nitrile > aldehyde > ketone > alcohol > amine > alkene > alkyne > halide • named as for alcohol, replace -ol with -amine, AMINE suffix • when an anime is a SUBSTITUENT it is an AMINO substituent
• number the chain as usual to give the amine functional group the lowest number • amines are named as alcohols except that "amine" is used in place of "ol" and so instead of propan-OL we have propan-AMINE (above), instead of pentanOL we have pentanAMINE (above) etc.
• find the longest chain that contains the maximum number of functional groups (alkene and amine) = 4 • number to give the highest priority functional group AMINE the lowest number • N comes BEFORE 3 when specifying the two methyl substituents
• REMEMBER, the common name aniline has been incorporated into IUPAC nomenclature • some common names for amines
* you NEED TO KNOW THESE TWO, piperidine seen in the Stork reaction, pyridine a common organic base
N
1° Amine 2° Amine 3° Amine QuaternaryAmmonium Salt
R HH N
R R'H N
R R'R''
R1
NR2 R3
R4
trigonal pyramidal
tetrahedral
CH3CH2CH2NH2
1-propanamine(2S)-pentanamine
NH2(S)H
123 1 2 3 45
N-ethyl-N,3-dimethylbut-2-en-1-aminelongest chain 123
4 N
Me
Me
Et
Br
NH2
3-bromo-2-chloroaniline
Cl 12
3 #1 by definition
diethylamine diisopropylamine
putrescine
NH
HN
H2N NH2 NH2H2Ncadaverine
N HNN
piperidine pyrrolepyridine 2,6-lutidine
(amines can stink!)
* *HN
Amines : Page 2
2 Amines as Bases • deciding the stronger of two acids, e.g. H-A1 and H-A2
• the stronger acid has the more stable conjugate base anion, lower energy electrons in the base • the stronger acid corresponds to the more favorable "reaction", left to right • deciding the stronger of two bases, e.g. B1 and B2
• there are no anions here, but the stronger base still has the higher energy, more chemically reactive electrons • the stronger base is stronger because the energy of the electrons go down more by getting into a bond • the stronger base has the weaker conjugate acid since it has the stronger bond Example
Acidity is Measured in terms of pKa, How is Basicity Measured? • Basicity can be measured in terms of the corresponding pKb, however, in organic chemistry we often don't do that, we specify basicity in terms of the acidity of the conjugate acid Acidity of an Amine in terms pf pKa….
Compare with (and don't confuse with) Basicity of an Amine in terms of pKa of the conjugate acid
Trends in Basicity?
H A1 H+ + – A1
H A2 H+ + – A2
higher energy electronsstronger baseweaker acid
B1 H–B1
B2 H–B2+ H+
+ H+higher energy electrons
stronger base weaker conjugate acid
+ H+
+ H+
more stable cation
less stable cation
weaker base
stronger base
more favorable
lessfavorable
D group, raises energy of
electrons on N, more reactive
W group, lowers energy of
electrons on N, less reactive
D group stabilizes positive charge on N
W group destabilizes positive charge on N
RN
R
H
H3CO
RN
R
H
O2N
RN
R
H3CO
RN
R
O2N
Amineacid
strength
+ H3ONH3pKa ~35weak acid
NH2strongbase
+ H2O
Aminebase
strength
+ H3ONH4pKa ~9
moderate acid
NH3moderate
base
+ H2O
CH3NH2
(CH3)2NH
(CH3)3N
CH3NH3
(CH3)2NH2
(CH3)3NH
increasing cationstability
but
decreasing solvation
effects cancel!!
+ H3O NH4 pKa = 9.2NH3 + H2O
+ H3O + H2O
+ H3O + H2O
+ H3O + H2O
pKa = 10.9
pKa = 10.7
pKa = 9.8
Amines : Page 3
• there are no clear trends among the aliphatic amines because of the competing effects of alkyl group donation and reduced solvation of the larger cations But
• (minor) resonance delocalization (i.e. partial bonding) stabilizes (lowers energy) of the non-bonding electrons on N, these electrons are less reactive • aromatic amines are thus MUCH less basic than aliphatic amines
• clear decrease in basicity with decreasing energy of non-bonding electrons as the hybridization of the orbitals gains more s character and less p character • the protonated nitrile is about the strongest acid that we discuss this entire course 4 Reactions of Amines 4.1 Amines a Nucleophiles Recall:
• reaction does NOT go, H2O not strong enough nucleophile
However:
• NH3 is a stronger enough nucleophile that this SN2 reaction goes! • MeNH2 is an even stronger stronger nucleophile, reaction keeps going! • clearly not very useful, due to "over-alkylation", except in the Hofmann elimination (see next reaction)
NH2 + H3O + H2ONH3
pKa ~ 42 other resonance contributors
NH2
NCH3CH3
H3CN CH3C N
sp3sp2
sp
"pKa" ~9.8 "pKa" ~5.3 "pKa" ~ -10!!!
decreasing basicity
XH3C IH
HO CH3 I
SN2H
HO
H HO
H HNH
H O
weakstrong intermediatenucleophilicity
H
HN H3C I
HH N CH3 IH
H
H HNH
H
HN CH3
H3C ICH3
H N CH3H
etc. etc.
CH3H3C N CH3
CH3
"exhaustive" alkylation product
H HNH
H3C
HN CH3
slightly stronger nucleophile
SN2
Amines : Page 4
4.2 Hofmann Elimination Revist a Concept we Have Seen Many Times Now:
This reaction ALSO doesn't work (poor leaving group)
However, this one does (better leaving group)
Example
Overall
• the reaction is overall E2 ELIMINATION, forming an alkene with a neutral amine as the leaving group
XC CH
OHCC
+ OH2
+ OHBase
no reaction : poor leaving group
reaction goes : better leaving group
C CH
OH2
CCBase
E2
E2
XC CH
NH2
CC + NH2Base
no reaction : poor leaving group
E2
+ NR3
reaction goes : better leaving group
C CH
NMe3
CCBase E2
C CH
NH2
excess Me-Iexhaustivemethylation
NH2H3C NMe3H3CNMe3H2C
HOH
CH2Excess Ag2O
H2O
Heat
converts from iodideto hydroxide anion = good base
CH3I
I
+ AgI (ppt.) E2
exhaustivemethylation
1. XS CH3I
2. Ag2O/H2O
3. Heat
NH2H3C
MajorHofmann
MinorSayetzeff
+
Amines : Page 5
• HOWEVER, the LEAST substituted alkene is the major product (Hofmann product), not the more substituted Saytzeff (Zaitsev) alkene Why is this? There are TWO reasons, the first is a STERIC EFFECT, the second is an ELECTRONIC EFFECT Reason #1: The steric effect of the bulky -NR3 leaving group
• the –NMe3
+ group is LARGE (bulky), it is roughly the same size as a t-butyl group • therefore the E2 conformation for Hofmann elimination is lower in energy than the E2 conformation for Sayetzeff elimination for steric reasons (fewer gauche interactions) • therefore elimination in the Hofmann conformation is more likely because the structure spends more time in that lower energy conformation Reason #2: electronic effect • NH3 is a good leaving group, but not as good as Br–, I– etc. • at this point we need a more sophisticated and subtle look at the transition state that goes beyond conventional general organic chemistry, the transition state is not really "symmetrical", in that although all of the bonds are made and broken in one continuous process, as required for all concerted reactions, the bonds are not all broken and made at EXACTLY the same time • the proton "leaves" earlier than the NH3, which means that in the transition state the partial bond to the departing hydrogen atom is LONG and WEAK, but the leaving group leaves "later", which means that in the transition state the bond to the leaving group is still comparatively SHORT and STRONG, as illustrated below • because the proton leaves "earlier", a partial negative charge starts to develop on the carbon atom that the proton is attached to, and in the Hofmann elimination this carbon is less substituted: RECALL: negative charges are LESS STABLE on more substituted carbons, thus the transition state for the Hofmann elimination has the partial negative charge on the less substituted carbon, this transition state is lower in energy, it is thus formed faster (under kinetic control), the Hofmann alkene is thus the major product
NH2
Major Hofmann Minor Sayetzeff
+
H
NMe3
H3CH2C
H
HH
H
H
NMe3
H3C
H
HS
CH3
HHHS
1. XS CH3I
2. Ag2O/H2O
3. Heat
lowerenergy
conformation
H and leaving group are anti-
coplanar gaucheinteraction
bulky bulky
excess
NMe3
HHHSOHHO
NMe3
HS
OHHHHofmann
Sayetzeff
‡
NMe3
HS
HH
‡
HO
partial negative developing on 1° carbon
+ H2O + NH3
+ H2O + NH3
δ
δ
leaving "later"
leaving "later"
leaving "earlier"
leaving "earlier"
partial negative developing on 2° carbon
higherenergy ‡
lowerenergy ‡
faster
slower
Amines : Page 6
• this is a rather subtle advanced organic chemistry concept, but it is important that you are exposed to this thinking as we get towards the end of our general organic chemistry course Example Problem 1
• there are TWO possible elimination products once the ammonium ion has been form in the reaction with CH3-I, the reaction that forms the least substituted (Hofmann) alkene is fastest, the Hofmann alkene is the major alkene product, together with its associated amine • in some cases the amine leaving group will be a substantial major organic structure on its own Example Problem 2
Example Problem 3
3 Synthesis of Amines Amines are made in REDUCTION REACTIONS, several of which we have ALREADY SEEN
NH
N
N1. Excess CH3I
+
+ Major, Hofmann
Minor, Sayetzeff
HeatN
2. Ag2O/H2O
HHO
HeatN
HO H
HN N+1. Excess CH3I
2. Ag2O/H2ONHHO
heat
mono-substituted alkene formed
NH2NMe
MeMe
1. Excess CH3I+
2. Ag2O/H2O3. Heat
NMe3
HHO
NO2 NH2/Pd/C
addition of H, removal of O
RCO
NHR' R C NHR'amide
1. LiAlH4
2. H3O
nitro
addition of H, removal of O
R C N R C Nnitrile
1. LiAlH4
2. H3Oaddition of H
seen
before
H
H
H H
H H H
H
amine
amine
amine
Amines : Page 7
• In reality there are lots of different ways of doing these reductions (many different sets of reagents/conditions work), but here we use reagents/conditions that we already know for simplicity., no need to learn even more new reagents at this point 3.1 Amine Synthesis by Reduction of Azides: Synthesis of PRIMARY amines AGAIN, the reactions we already know in a synthetic context, AND A NEW ONE
• 1°, 2° or 3° amines can be made by reducing an amide, which in turn comes from an acid chloride, which in turn comes form a carboxylic acid • a 1° amine can be made from a nitrile, which can be made in an SN2 reaction from an appropriate alkyl bromide, ONE CARBON ATOM IS ADDED COMPARED TO THE STARTING ALKYL BROMIDE • a 1° amine can be made from an azide, which can be made in an SN2 reaction from an appropriate alkyl bromide, ZERO CARBON ATOMS ARE ADDED COMPARED TO THE STARTING ALKYL BROMIDE A New Reagent
Examples • Synthesize these two PRIMARY amines
OR...R
CN
RIMINE
1. LiAlH4 2. H3Oaddition of H
R'
RCN
R
R' H
H amineH2/Pd/C
OR...AZIDE 1. LiAlH4 2. H3O
addition of HH2/Pd/C
R CH2 N3 R CH2 NH
Hamine
new
BUT
related!
RCO
Cl RCO
NHR'R CH2 NHR'
R X
R C N
R N3 R NH2
R'NH2
Na+ –CN adds 1 carbon
does not add carbonNaN3
amide
R CH2 NH2
1. LiAlH4
2. H3O
SN2
acid chloride makes a 1°, 2° or 3° alkyl aminedoes not add a carbon
1° aminenitrilealkyl halide
azideSN2
R X1. LiAlH4
2. H3O
1. LiAlH4
2. H3O 1° amine
RCO
OH
SOCl2
acid
alkyl halideNEW
Na NNNsodium azide = Na+ –N3 =Very good nucleophilesmall "bullet" shaped
similar to the cyanide anionNC
cyanide anionazide anion
NaN3
Br
N3 NH2
NaCNC
NNH2
1. LiAlH4
2. H3O
1. LiAlH4
2. H3O
NBS/hνSN2
must add THIS carbon atom
no additional carbon atoms
adds carbon atom
Amines : Page 8
3.2 Synthesis of Substituted Amines by Reduction of an Imine: Reductive Amination • Addition of nitrogen to a carbonyl to form an imine, FOLLOWED BY reduction to form an amine
• So now we have a new reaction name: Reductive Amination, but is basically chemistry we already know • We already knew that we could react an amine with an aldehyde/ketone to form an imine (also known as a Schiff base), and it is no great surprise that the C=N bond of the imine (Schiff base) can be reduced by addition of H2 addition similarly to a C=O bond, we can even use the SAME REDUCING REAGENTS we already know! • reduction of C=N is actually somewhat easier than reduction of C=O, N is less electronegative and the C-N pi-bond is thus a bit weaker than the C-O p-bond INDIRECT Reductive Amination combines these reactions in sequence: Example 1
Example 2
DIRECT Reductive Amination COMBINES formation of the imine and the reduction in one reaction
• "in situ" means formed in the reaction, reaction "in situ" means that the imine reacts as it is formed • NEW REDUCING AGENT, NaBH3CN Recall NaBH4:
/H (cat.)
RC
R
NR'
RC
R
NR' H
H 2° amine
imine
RC
R
O
RC
R
OH
HOR...1. LiAlH4 2. H3O
H2/Pd/C
RNH2
OR...1. LiAlH4 2. H3O
H2/Pd/Creductiveamination
HCO
H (cat.) H2/Pd/CH
NCH3
CH2
NCH3H
+1° amine
CH3-NH2
HCO
1. CH3CH2NH2/H+ cat.
2. LiAlH43. H3O+
NH
CO
H
NaBH3CN
CN H
CHN HH
reduced in situ
+ NH3ammonia
1° amine
new!!
organic acidLBLA
HBH
HH
LB/Nucleophile
CO
CN
H
slower
faster
strongerπ-bondO more
electronegative
Na+ –BH4
Amines : Page 9
Compare NaBH3CN:
• The -CN withdrawing group makes the -BH3CN anion less nucleophilic, it reacts slower with carbonyls (C=O) and imines (C=N), but the reaction with C=O is slow enough that it does not happen under reductive amination conditions, Na+ –BH3CN is a selective reducing agent for imines • remember, "no reaction" doesn’t really mean no reaction at all, reactivity is not black and white, it means that the reaction with the C=O is now slow enough and the reaction with C=N fast enough to be useful in the reaction • another subtle point, EtOH may not be required as a solvent to provide the protons that go with the hydride, since the acid that is used to catalyze the reaction may also supply these protons
Example of an INDIRECT reductive amination
Example of a DIRECT reductive amination
• note that the selective reducing agent NaBH3CN is included in the reagent/conditions in a "one pot" reaction Example in Reverse • how can we make the provided amine using a reductive amination?
• Break bond "backwards", the benzene ring cannot carry a C=O, the carbonyl must be the fragment on the "right" • You can use EITHER the DIRECT or the INDIRECT reductive amination methods in a synthesis problem
HBH
HCNwithdrawing
LESS nucleophilic, less reactive
CO
CN
Hweakerπ-bondN less
electronegativeXNa+ –BH3CN
2° amine
ON
+
HN
NaBH3CN
1° amine
HN
iminereduced in situ
H
HTFA
or other organic acid
EtOH
LBLA
2° amineH
ON+ NaBH3CN
1° amineH H
N
iminiumreduced in situ
HCN
HTsOH
or other organic acid
EtOH
LA LB
NHEt
H
O+ NEt
H
1. HCl cat.
2. H2/Pd/CLALB
NHH
H H
O+
H
H2N
NaBH3CN
TsOH
EtOH
LB
LA
XNH2
O+NH
NaBH3CN O H2N+
obviously can't have thisA B
can't make bond A
CAN make bond B
H+
EtOH
Amines : Page 10
5 Some Final Synthesis Problems 5.1 Synthesis of Amines Common Methods of Synthesizing Amines (this is not all of the methods, see Section 3 of these notes
Example Problem 1
• MDMA = N,a-dimethyl-1,3-benzodioxole-5-ethenamine = Ecstacy : 5g ~ 20 years!! • this is a secondary amine, which can in principle be synthesized either by reduction of an amide or by reductive amination, however, in this case only reductive amination would work • Trying to make the amine via amide reduction in this case obviously doesn't work because the relevant amide can't exist
OCH3NH2/H+ (cat.)
NaBH3CNNH
N
O1. LiAlH4
2. H3O+N
2. LiAlH4Br
3. H3O+
NH2
1. NaCN
2. LiAlH4Br
3. H3O+
NH2
reductive amination
amide reduction
azide reduction
nitrile reduction
1°, 2° or 3°
1°, 2° or 3°
1° only
1° only + 1 carbon atom1C 2C
1. NaN3
HN
(±)
H3C NH2
TsOH CatNaBH3CN
O
O
O
O
O
O OH
O
O O
O
O
Osamething
PCC
1. H2O/Hg(OAc)22. NaBH4
reductiveamination
MDMA
HNO
O (±)
HNO
O O
1. LiAlH4
can't exist2. H3O+
amide reductioncan't work here
Amines : Page 11
Example Problem 2
• in this case the strategy again is to note that we need to make a tertiary amine, which requires either a reductive amination or reduction of a tertiary amide, in this case either of these two routes would work, as shown Example Final Exam Synthesis Problems Involving Amines Problem 1: Difficulty = "moderate": Synthesize methamphetamine (meth) from benzene
• again, the strategy again is to note that we need to make a tertiary amine, which requires either a reductive amination or reduction of a tertiary amide, in this case only the reductive amination works • This is not the normal method of synthesizing meth, this is just an organic chemistry exercise! Problem 2: Difficulty = "easy"
CO2H
COCl CO
N
N
1. LiAlH42. H3O+
HNSOCl2
1. KMnO4/–OH/boil
2. H3O+
CO
H
HN H+ cat.NaBH3CN
Br
OH
Na+ –OH
(SN2) PCC
HN
(±)
H3C NH2
TsOH Cat
O
OH
PCC
Br2/FeBr3 NaBH3CN
meth
Br
MgBr1.
2. H3O+
O (±)
(±)
Mg.THF
C
1. LiAlH42. H3O+
Br NaCNN
NH2
NBS/hν
Amines : Page 12
• in this case we need to make a primary amine AND we need to add one carbon atom compared to the starting structure, the nitrile reduction method works well here Problem 3: Difficulty = "difficult"
• this one is tricky because you have to construct the amine from which to make the amide • it is also tricky because the "order" of the reactants to make the amide are reversed, usually we make the acid chloride and react it with an amine on the reagent arrow, here we make an amine and have the acid chloride on the reagent arrow
N
O
Ph
N
O
PhO
H
H+ cat.NaBH3CNX
does not work for an amide
NH
O
PhCl
ignore stereochemistry
OOH
Br
MgBr
PCC
NBS/hν
Mg.THF
2. H3O+
1. H
ON
H
HH+ cat.NaBH3CN
Amines : Page 13
5.2 Different Types of Synthesis problems for the Final Exam Synthesis is hard because the strategy is often difficult and there are simply a lot of reactions to know. Synthesis problems on the final exam will be of two kinds. The first includes all of the major reactions we have learned this semester. The second kind of synthesis problem will include only a "minimal set" of reactions, that everybody should know. The idea here is these problems test your synthesis problem solving skills rather than your ability to learn a lot of reactions. There are two parts to this "minimal set: of reactions, the first are a set of basic functional group interconversions, the second includes the most basic carbon-carbon bond forming reactions, i.e. the Grignard and acetylide reactions. These two sets of reactions are summarized below, and also on the class website.
Example Synthesis Problems that Include Only Reactions from the "Minimal Set" Problem 1
PCCNBS/hν
MgBr
O
Br Mg.THF
OH
2. H3O+
1. H
O
Amines : Page 14
Problem 2
Problem 3
NBS/hν
Br
1.
O
OH
Ph
MCPBA2. H3O+
PhMgBr
Na+ –OH
Br2 Na/NH3(l)
Br
Br
Na
1. Excess NaNH2/heat2. H2O
NaNH2
Br
Amines : Page 15
6 Summary of Reactions Involving Amines Do NOT start studying by trying to memorize the reactions here! Work as many problems as you can, with this list of reactions in front of you if necessary, so that you can get through as many problems as you can without getting stuck on the reagents/conditions, and so that you can learn and practice solving reaction problems. Use this list AFTER you have worked all of the problems, and just before an exam. By then you will have learned a lot of the reagents/conditions just by using them and you will only have to memorize what you haven't learned yet. Then do the following: • Cover the entire page of reagents/conditions with a long vertical strip of paper, see if you can write down the reagents/conditions for each reaction, check to see which you get correct, if COMPLETELY correct, circle Y, if incorrect or even slightly incorrect, circle N. In this way you keep track of what you know and what you don't know. • Keep coming back to this list and so the same thing only for those reactions you circled N, until all are circled Y. Knowing the reagents/conditions on this page is INSUFFICIENT to do well on an exam since you will ALSO need to recognize how to use and solve reaction problems in different contexts, this page ONLY helps you to learn the reagents/conditions that you have not YET learned by working problems.
You have seen PARTS of some of these reactions in earlier sections!
1. NaN32. LiAlH4
Br
3. H3O+
NH2
1. NaCN2. LiAlH4
Br3. H3O+
NH2
NO2 H2/Pd/C NH2
1. NH3/H+ (cat.)O NH2
amphetamine
OCH3NH2/H+ (cat.)NaBH3CN/EtOH
NH
H(CH3)2NH/H+ (cat.)
O N
2. H2/Pd/C
INDIRECT reductive amination
NO 1. LiAlH4
2. H3O+N
amine synthesis
HN 1. XS CH3I
2. Ag2O / H2O/Heat
N
1°
2°
3°
Hofmann eliminationNaBH3CN/EtOH
Y / N
Y / N
Y / N
Y / N
Y / N
Y / N
Y / N
Y / N
DIRECT reductive amination