Amine

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For other uses, see Amine (disambiguation).
Primary amine Secondary amine Tertiary amine
primary amine secondary amine tertiary amine

In organic chemistry, amines (US: /əˈmn/ or /ˈæmin/,[1] UK: /əˈmn/, /ˈæmɪn/ or /ˈmin/)[2][3] are compounds and functional groups that contain a basic nitrogen atom with a lone pair. Amines are formally derivatives of ammonia, wherein one or more hydrogen atoms have been replaced by a substituent such as an alkyl or aryl group.[4] (These may respectively be called alkylamines and arylamines; amines in which both types of substituent are attached to one nitrogen atom may be called alkylarylamines.) Important amines include amino acids, biogenic amines, trimethylamine, and aniline; see Category:Amines for a list of amines. Inorganic derivatives of ammonia are also called amines, such as chloramine (NClH2); see Category:Inorganic amines.[5]

Compounds with a nitrogen atom attached to a carbonyl group, thus having the structure R–CO–NR′R″, are called amides and have different chemical properties from amines.

Classes of amines[edit]

An aliphatic amine has no aromatic ring attached directly to the nitrogen atom. Aromatic amines have the nitrogen atom connected to an aromatic ring as in the various anilines. The aromatic ring decreases the alkalinity of the amine, depending on its substituents. The presence of an amine group strongly increases the reactivity of the aromatic ring, due to an electron-donating effect.

Amines are organized into four subcategories:

  • Primary amines — Primary amines arise when one of three hydrogen atoms in ammonia is replaced by an alkyl or aromatic. Important primary alkyl amines include, methylamine, most amino acids, and the buffering agent tris, while primary aromatic amines include aniline.
  • Secondary amines — Secondary amines have two organic substituents (alkyl, aryl or both) bound to the nitrogen together with one hydrogen. Important representatives include dimethylamine, while an example of an aromatic amine would be diphenylamine.
  • Tertiary amines — In tertiary amines, nitrogen has three organic substituents. Examples include trimethylamine, which has a distinctively fishy smell, and EDTA.
  • Cyclic aminesCyclic amines are either secondary or tertiary amines. Examples of cyclic amines include the 3-membered ring aziridine and the six-membered ring piperidine. N-methylpiperidine and N-phenylpiperidine are examples of cyclic tertiary amines.

It is also possible to have four organic substituents on the nitrogen. These species are not amines but are quaternary ammonium cations and have a charged nitrogen center. Quaternary ammonium salts exist with many kinds of anions.

Naming conventions[edit]

Amines are named in several ways. Typically, the compound is given the prefix "amino-" or the suffix: "-amine". The prefix "N-" shows substitution on the nitrogen atom. An organic compound with multiple amino groups is called a diamine, triamine, tetraamine and so forth.

Systematic names for some common amines:

Lower amines are named with the suffix -amine.

Methylamine.svg
methylamine

Higher amines have the prefix amino as a functional group. IUPAC however does not recommend this convention, but prefers the alkanamine form, e.g. pentan-2-amine.

2-amino-pentane.png
2-aminopentane
(or sometimes: pent-2-yl-amine or pentan-2-amine)

Physical properties[edit]

Hydrogen bonding significantly influences the properties of primary and secondary amines.[6] Thus the melting point and boiling point of amines is higher than those of the corresponding phosphines, but generally lower than those of the corresponding alcohols and carboxylic acids. For example, methyl and ethyl amines are gases under standard conditions, whereas the corresponding methyl and ethyl alcohols are liquids. Amines possess a characteristic ammonia smell, liquid amines have a distinctive "fishy" smell.

The nitrogen atom features a lone electron pair that can bind H+ to form an ammonium ion R3NH+. The lone electron pair is represented in this article by a two dots above or next to the N. The water solubility of simple amines is enhanced by hydrogen bonding involving these lone electron pairs. Typically salts of ammonium compounds exhibit the following order of solubility in water: primary ammonium (RNH+
3
) > secondary ammonium (R
2
NH+
2
) > tertiary ammonium (R3NH+). Small aliphatic amines display significant solubility in many solvents, whereas those with large substituents are lipophilic. Aromatic amines, such as aniline, have their lone pair electrons conjugated into the benzene ring, thus their tendency to engage in hydrogen bonding is diminished. Their boiling points are high and their solubility in water is low.

Structure[edit]

Alkyl amines[edit]

Alkyl amines characteristically feature tetrahedral nitrogen centers. C-N-C and C-N-H angles approach the idealized angle of 109°. C-N distances are slightly shorter than C-C distances. The energy barrier for the nitrogen inversion of the stereocenter is about 7 kcal/mol for a trialkylamine. The interconversion has been compared to the inversion of an open umbrella into a strong wind.

Amines of the type NHRR′ and NRR′R″ are chiral: the nitrogen center bears four substituents counting the lone pair. Because of the low barrier to inversion, amines of the type NHRR′ cannot be obtained in optical purity. For chiral tertiary amines, NRR′R″ can only be resolved when the R, R′, and R″ groups are constrained in cyclic structures such as N-substituted aziridines (quaternary ammonium salts are resolvable).

Amine R-N.svg  ⇌  Amine N-R.svg
Inversion of an amine. The pair of dots represents the lone electron pair on the nitrogen atom.

Aromatic amines[edit]

In aromatic amines ("anilines"), nitrogen is often nearly planar owing to conjugation of the lone pair with the aryl substituent. The C-N distance is correspondingly shorter. In aniline, the C-N distance is the same as the C-C distances.[7]

Basicity[edit]

Like ammonia, amines are bases.[8] Compared to alkali metal hydroxides, amines are weaker (see table for examples of conjugate acid Ka values).

Alkylamine[9] or aniline[10] pKa Kb
methylamine (MeNH2) 10.62 4.17E-04
dimethylamine (Me2NH) 10.64 4.37E-04
trimethylamine (Me3N) 9.76 5.75E-05
ethylamine (EtNH2) 10.63 4.27E-04
aniline (PhNH2) 4.62 4.17E-10
4-methoxyaniline (4-MeOC6H4NH2) 5.36 2.29E-09
N,N-Dimethylaniline (PhNMe2) 5.07 1.17E-09
3-Nitroaniline (3-NO2-C6H4NH2) 2.46 2.88E-12
4-Nitroaniline (4-NO2-C6H4NH2) 1 1.00E-13
4-trifluoromethylaniline (CF3C6H4NH2) 2.75 5.62E-12

The basicity of amines depends on:

  1. The electronic properties of the substituents (alkyl groups enhance the basicity, aryl groups diminish it).
  2. The degree of solvation of the protonated amine, which includes steric hindrance by the groups on nitrogen.

Electronic effects[edit]

Owing to inductive effects, the basicity of an amine might be expected to increase with the number of alkyl groups on the amine. Correlations are complicated owing to the effects of solvation which are opposite the trends for inductive effects. Solvation effects also dominate the basicity of aromatic amines (anilines). For anilines, the lone pair of electrons on nitrogen delocalises into the ring, resulting in decreased basicity. Substituents on the aromatic ring, and their positions relative to the amine group, also affect basicity as seen in the table.

Solvation effects[edit]

Solvation significantly affects the basicity of amines. N-H groups strongly interact with water, especially in ammonium ions. Consequently, the basicity of ammonia is enhanced by 1011 by solvation. The intrinsic basicity of amines, i.e. the situation where solvation is unimportant, has been evaluated in the gas phase. In the gas phase, amines exhibit the basicities predicted from the electron-releasing effects of the organic substituents. Thus tertiary amines are more basic than secondary amines, which are more basic than primary amines, and finally ammonia is least basic. The order of pKb's (basicities in water) does not follow this order. Similarly aniline is more basic than ammonia in the gas phase, but ten thousand times less so in aqueous solution.[11]

In aprotic polar solvents such as DMSO, DMF, and acetonitrile the energy of solvation is not as high as in protic polar solvents like water and methanol. For this reason, the basicity of amines in these aprotic solvents is almost solely governed by the electronic factors.

Synthesis[edit]

Alkylation[edit]

The most industrially significant amines are prepared from ammonia by alkylation with alcohols:

ROH + NH3 → RNH2 + H2O

These reactions require catalysts, specialized apparatus, and additional purification measures since the selectivity can be problematic. The same amines can be prepared by treatment of haloalkanes with ammonia and amines:

RX + 2 R′NH2 → RR′NH + [RR′NH2]X

Such reactions, which are most useful for alkyl iodides and bromides, are rarely employed because the degree of alkylation is difficult to control.[5] Selectivity can be improved via the Delépine reaction, although this is rarely employed on an industrial scale.

Reductive routes[edit]

Via the process of hydrogenation, nitriles are reduced to amines using hydrogen in the presence of a nickel catalyst. Reactions are sensitive to acidic or alkaline conditions, which can cause hydrolysis of the –CN group. LiAlH4 is more commonly employed for the reduction of nitriles on the laboratory scale. Similarly, LiAlH4 reduces amides to amines. Many amines are produced from aldehydes and ketones via reductive amination, which can either proceed catalytically or stoichiometrically.

Aniline (C6H5NH2) and its derivatives are prepared by reduction of the nitroaromatics. In industry, hydrogen is the preferred reductant, whereas in the laboratory, tin and iron are often employed.

Specialized methods[edit]

Many laboratory methods exist for the preparation of amines, many of these methods being rather specialized.

Reaction name Substrate Comment
Gabriel synthesis Organohalide Reagent: potassium phthalimide
Staudinger reduction Azide This reaction also takes place with a reducing agent such as lithium aluminium hydride.
Schmidt reaction Carboxylic acid
Aza-Baylis–Hillman reaction Imine Synthesis of allylic amines
Birch reduction Imine Useful for reactions that trap unstable imine intermediates, such as Grignard reactions with nitriles.[12]
Hofmann degradation Amide This reaction is valid for preparation of primary amines only. Gives good yields of primary amines uncontaminated with other amines.
Hofmann elimination Quaternary ammonium salt Upon treatment with strong base
Amide reduction amide
Nitrile reduction Nitriles Either accomplished with reducing agents or by electrosynthesis
Reduction of nitro compounds Nitro compounds Can be accomplished with elemental zinc, tin or iron with an acid.
Amine alkylation Haloalkane
Delepine reaction Organohalide reagent Hexamine
Buchwald–Hartwig reaction Aryl halide Specific for aryl amines
Menshutkin reaction Tertiary amine Reaction product a quaternary ammonium cation
Hydroamination Alkenes and alkynes
Oxime reduction Oximes
Leuckart reaction Ketones and aldehydes Reductive amination with formic acid and ammonia via an imine intermediate
Hofmann–Löffler reaction Haloamine
Eschweiler–Clarke reaction Amine Reductive amination with formic acid and formaldehyde via an imine intermediate

Reactions[edit]

Alkylation, acylation, and sulfonation[edit]

Aside from their basicity, the dominant reactivity of amines is their nucleophilicity.[13] Most primary amines are good ligands for metal ions to give coordination complexes. Amines are alkylated by alkyl halides. Acyl chlorides and acid anhydrides react with primary and secondary amines to form amides (the "Schotten–Baumann reaction").

Amide formation

Similarly, with sulfonyl chlorides, one obtains sulfonamides. This transformation, known as the Hinsberg reaction, is a chemical test for the presence of amines.

Because amines are basic, they neutralize acids to form the corresponding ammonium salts R3NH+. When formed from carboxylic acids and primary and secondary amines, these salts thermally dehydrate to form the corresponding amides.

Diazotization[edit]

Amines react with nitrous acid to give diazonium salts. The alkyl diazonium salts are of little synthetic importance because they are too unstable. The most important members are derivatives of aromatic amines such as aniline ("phenylamine") (A = aryl or naphthyl):

Anilines and naphthylamines form more stable diazonium salts, which can be isolated in the crystalline form.[14] Diazonium salts undergo a variety of useful transformations involving replacement of the N2 group with anions. For example, cuprous cyanide gives the corresponding nitriles:

Aryldiazonium couple with electron-rich aromatic compounds such as a phenol to form azo compounds. Such reactions are widely applied to the production of dyes.[15]

Conversion to imines[edit]

Imine formation is an important reaction. Primary amines react with ketones and aldehydes to form imines. In the case of formaldehyde (R′ = H), these products typically exist as cyclic trimers.

RNH2 + R′2C=O → R′2C=NR + H2O

Reduction of these imines gives secondary amines:

R′2C=NR + H2 → R′2CH–NHR

Similarly, secondary amines react with ketones and aldehydes to form enamines:

R2NH + R′(R″CH2)C=O → R″CH=C(NR2)R′ + H2O

Overview[edit]

An overview of the reactions of amines is given below:

Reaction name Reaction product Comment
Amine alkylation Amines Degree of substitution increases
Schotten–Baumann reaction Amide Reagents: acyl chlorides, acid anhydrides
Hinsberg reaction Sulfonamides Reagents: sulfonyl chlorides
Amine–carbonyl condensation Imines
Organic oxidation Nitroso compounds Reagent: peroxymonosulfuric acid
Organic oxidation Diazonium salt Reagent: nitrous acid
Zincke reaction Zincke aldehyde Reagent: pyridinium salts, with primary and secondary amines
Emde degradation Tertiary amine Reduction of quaternary ammonium cations
Hofmann–Martius rearrangement Aryl-substituted anilines
Von Braun reaction Organocyanamide By cleavage (tertiary amines only) with cyanogen bromide
Hofmann elimination Alkene Proceeds by β-elimination of less hindered carbon
Cope reaction Alkene Similar to Hofmann elimination
carbylamine reaction Isonitrile Primary amines only
Hoffmann's mustard oil test Isothiocyanate CS2 and HgCl2 are used. Thiocyanate smells like mustard.

Biological activity[edit]

Amines are ubiquitous in biology. The breakdown of amino acids releases amines, famously in the case of decaying fish which smell of trimethylamine. Many neurotransmitters are amines, including epinephrine, norepinephrine, dopamine, serotonin, and histamine. Protonated amino groups (–NH+
3
) are the most common positively charged moieties in proteins, specifically in the amino acid lysine.[16] The anionic polymer DNA is typically bound to various amine-rich proteins.[17] Additionally, the terminal charged primary ammonium on lysine forms salt bridges with carboxylate groups of other amino acids in polypeptides, which is one of the primary influences on the three-dimensional structures of proteins.[18]

Application of amines[edit]

Dyes[edit]

Primary aromatic amines are used as a starting material for the manufacture of azo dyes. It reacts with nitrous acid to form diazonium salt, which can undergo coupling reaction to form azo compound. As azo-compounds are highly coloured, they are widely used in dyeing industries, such as:

Drugs[edit]

Many drugs are designed to mimic or to interfere with the action of natural amine neurotransmitters, exemplified by the amine drugs:

Gas treatment[edit]

Aqueous monoethanolamine (MEA), diglycolamine (DGA), diethanolamine (DEA), diisopropanolamine (DIPA) and methyldiethanolamine (MDEA) are widely used industrially for removing carbon dioxide (CO2) and hydrogen sulfide (H2S) from natural gas and refinery process streams. They may also be used to remove CO2 from combustion gases and flue gases and may have potential for abatement of greenhouse gases. Related processes are known as sweetening.[19]

Safety[edit]

Low molecular weight amines, such as ethylamine, are toxic, and some are easily absorbed through the skin. Many higher molecular weight amines are, biologically, highly active.[citation needed]

See also[edit]

External links[edit]

References[edit]

  1. ^ "amine". The American Heritage Dictionary of the English Language (5th ed.). Boston: Houghton Mifflin Harcourt. 2014. Retrieved 19 April 2017. 
  2. ^ "Amine definition and meaning". Collins English Dictionary. Retrieved 2017-03-28. 
  3. ^ "amine - definition of amine in English". Oxford Dictionaries. Retrieved 2017-03-28. 
  4. ^ McMurry, John E. (1992), Organic Chemistry (3rd ed.), Belmont: Wadsworth, ISBN 0-534-16218-5 
  5. ^ a b Eller, Karsten; Henkes, Erhard; Rossbacher, Roland; Höke, Hartmut (2000). "Amines, Aliphatic". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a02_001. ISBN 3527306730. 
  6. ^ Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5. 
  7. ^ G. M. Wójcik "Structural Chemistry of Anilines" in Anilines (Patai's Chemistry of Functional Groups), S. Patai, Ed. 2007, Wiley-VCH, Weinheim. doi:10.1002/9780470682531.pat0385
  8. ^ J. W. Smith (1968). S. Patai, ed. "Basicity and complex formation". Patai's Chemistry of Functional Groups. doi:10.1002/9780470771082.ch4. 
  9. ^ Hall, H. K. (1957). "Correlation of the Base Strengths of Amines". Journal of the American Chemical Society. 79 (20): 5441–5444. doi:10.1021/ja01577a030. 
  10. ^ Kaljurand, I.; Kütt, A.; Sooväli, L.; Rodima, T.; Mäemets, V.; Leito, I.; Koppel, I. A. (2005). "Extension of the Self-Consistent Spectrophotometric Basicity Scale in Acetonitrile to a Full Span of 28 pKa Units: Unification of Different Basicity Scales". The Journal of Organic Chemistry. 70 (3): 1019–1028. doi:10.1021/jo048252w. PMID 15675863. 
  11. ^ Smith, Michael B.; March, Jerry (2007), Advanced Organic Chemistry: Reactions, Mechanisms, and Structure (6th ed.), New York: Wiley-Interscience, ISBN 0-471-72091-7 
  12. ^ Weiberth, Franz J.; Hall, Stan S. (1986). "Tandem alkylation-reduction of nitriles. Synthesis of branched primary amines". Journal of Organic Chemistry. 51 (26): 5338–5341. doi:10.1021/jo00376a053. 
  13. ^ March, Jerry (1992), Advanced Organic Chemistry: Reactions, Mechanisms, and Structure (4th ed.), New York: Wiley, ISBN 0-471-60180-2 
  14. ^ A. N. Nesmajanow (1943). "β-Naphthylmercuric chloride". Org. Synth. ; Coll. Vol., 2, p. 432 
  15. ^ Hunger, Klaus; Mischke, Peter; Rieper, Wolfgang; Raue, Roderich; Kunde, Klaus; Engel, Aloys (2000). "Azo Dyes". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a03_245. ISBN 3527306730. 
  16. ^ Andrade, Miguel A.; O'Donoghue, Seán I.; Rost, Burkhard (1998). "Adaptation of protein surfaces to subcellular location". Journal of Molecular Biology. 276 (2): 517–25. CiteSeerX 10.1.1.32.3499Freely accessible. doi:10.1006/jmbi.1997.1498. PMID 9512720. 
  17. ^ Nelson, D. L.; Cox, M. M. (2000). Lehninger, Principles of Biochemistry (3rd ed.). New York: Worth Publishing. ISBN 1-57259-153-6. 
  18. ^ Dill, Ken A. (1990). "Dominant forces in protein folding". Biochemistry. 29 (31): 7133–55. doi:10.1021/bi00483a001. PMID 2207096. 
  19. ^ Hammer, Georg; Lübcke, Torsten; Kettner, Roland; Davis, Robert N.; Recknagel, Herta; Commichau, Axel; Neumann, Hans-Joachim; Paczynska-Lahme, Barbara (2000). "Natural Gas". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a17_073. ISBN 3527306730.