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Chapter 16: Amines and Amides

Chapter 16: Amines and Amides. AMINES Amines are derivatives of ammonia, NH 3 , where one or more hydrogen atoms have been replaced by an organic (R) group. COMMON NAMING FOR AMINES

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Chapter 16: Amines and Amides

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  1. Chapter 16:Amines and Amides

  2. AMINES Amines are derivatives of ammonia, NH3, where one or more hydrogen atoms have been replaced by an organic (R) group.

  3. COMMON NAMING FOR AMINES Alphabetically link the names of the alkyl or aromatic groups bonded to the nitrogen and attach the suffix –amine so the name is one word. Use di- or tri- prefixes for identical alkyl groups. Examples:

  4. IUPAC NAMING FOR PRIMARY AMINES The –NH2 group is treated as a chain substituent called the amino group. Examples:

  5. IUPAC NAMING FOR AMINES Name the longest chain attached to the nitrogen. Replace the final –e with –amine. Number the chain so the carbon bonded to the nitrogen has the lowest possible number. Number the other substituents on the carbon chain. An italic “N” is used as a prefix for a substituent on nitrogen. Examples:

  6. NAMING AROMATIC AMINES Aniline is the simplest aromatic amine. Compounds are named as substituted anilines. An italic “N” is used to indicate that an alkyl group is attached to the nitrogen and not to the ring. Examples:

  7. PHYSICAL PROPERTIES OF AMINES The N-H bond is not quite as polar as the O-H bond. Primary and secondary amines can form hydrogen bonds between molecules. The hydrogen bonds are not as strong as those of alcohols, so amine boiling points are somewhat lower than those of alcohols.

  8. PHYSICAL PROPERTIES OF AMINES, cont.

  9. PHYSICAL PROPERTIES, cont. Amines can hydrogen bond with water, making smaller amine molecules usually water soluble.

  10. AMINE REACTIONS All amines behave as weak bases in water (similar to ammonia) R-NH2 + H2O  R-NH3+ + OH- Examples: CH3-NH-CH2CH3 + H2O  CH3-NH2-CH2CH3+ + OH- methylethylamine methylethylammonium ion

  11. AMINE REACTIONS, cont. All amines behave as weak bases and form salts when they react with acids such as HCl. R-NH2 + HCl  R-NH3+Cl- amine acid amine salt Example:

  12. AMINE SALTS Name by changing “amine” to “ammonium” and adding the anion name. More water soluble than parent amine, a useful characteristic for administering amine drugs Can be converted back to amine form: Quaternary ammonium salts have four alkyl groups attached to the nitrogen.

  13. AMIDE FORMATION Amines react with acid chlorides or acid anhydrides to form amides.

  14. AMIDE FORMATION, cont. Primary and secondary amines can form amides. Tertiary amines do not react to form amides.

  15. Examples:

  16. POLYAMIDE FORMATION Reaction of diacid chlorides with diamines produces polyamides that, like polyesters, are condensation polymers. The repeating units in polyamides are held together by amide linkages. 3 billion pounds of nylon and related polyamides produced annually Proteins are polyamides ( e.g. silk and wool)

  17. AMINE NEUROTRANSMITTERS Neurotransmitter – a chemical bridge between nerve cells

  18. IMPORTANT AMINE NEUROTRANSMITTERS Acetylcholine Dopamine – synthesized from the amino acid tyrosine Norepinephrine – synthesized from dopamine, may be associated with mental illness Serotonin – synthesized from the amino acid tryptophan, may be associated with mental illness

  19. OTHER BIOLOGICALLY IMPORTANT AMINES Epinephrine (adrenaline) – more important as a hormone than a neurotransmitter Fight-or-flight hormone, released in response to pain, anger, or fear, increases blood glucose level for energy

  20. OTHER BIOLOGICALLY IMPORTANT AMINES, cont. Amphetamines – nervous system stimulants, similar in structure to epinephrine Abuse of amphetamines has severe detrimental effects on the body and the mind

  21. OTHER BIOLOGICALLY IMPORTANT AMINES Alkaloids – a class of nitrogen-containing organic compounds obtained from plants. Examples include: Nicotine – found in tobacco Caffeine – found in coffee and cola drinks Quinine – used to treat malaria Opium – used to make codeine (in cough medicines), morphine (pain killer), and heroin

  22. NAMING AMIDES Use the carboxylic acid’s name and drop the –ic ending (common name) or –oic ending (IUPAC name) and change to –amide. Examples:

  23. NAMING AMIDES Use N to denote alkyl groups attached to the nitrogen atom. Examples:

  24. PHYSICAL PROPERTIES OF AMIDES Hydrogen bonding between unsubstituted amides causes them to have high melting points.

  25. PHYSICAL PROPERTIES, cont. Amides can form hydrogen bonds with water, making smaller amide molecules rather water soluble.

  26. AMIDE REACTIONS Amides are neither acidic nor basic. Hydrolysis – the reverse of amide formation, an amide is cleaved to produce a carboxylic acid and an amine or ammonia Amide hydrolysis is a central reaction in the digestion of proteins and the breakdown of proteins within cells. In the body, this hydrolysis is catalyzed by enzymes.

  27. AMIDE REACTIONS – HYDROLYSIS, cont. The products of an amide hydrolysis depend on whether the reaction occurs in acidic or basic conditions.

  28. Specific Examples:

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