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Amines.pptx

This chapter discusses the structure, classification, nomenclature, physical properties and reactions of amines. Amines are classified as primary, secondary or tertiary depending on the number of carbon groups bonded to the nitrogen atom. The chapter describes various amine structures including aliphatic, aromatic, heterocyclic aliphatic and heterocyclic aromatic amines. It also discusses IUPAC nomenclature rules for naming amines and provides examples of common amine names. The chapter notes that amines are polar compounds that can form hydrogen bonds. It describes amines as weak bases and explains how their basicity depends on their structure. The chapter concludes by giving an example reaction of an amine reacting with an acid to

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Chapter 15 Amines
Structure & Classification • Amines are classified as 1°, 2°, or 3° depending on the number of carbon groups bonded to nitrogen. • aliphatic amine: All carbons bonded to nitrogen are derived from alkyl groups. • aromatic amine: One or more of the groups bonded to nitrogen are aryl groups. CH3 -NH2 CH3 -N-CH3 H CH3 -N-CH3 CH3 Methylamine (a 1° amine) Dimethylamine (a 2° amine) Trimethylamine (a 3° amine) NH2 N-CH3 H CH2-N-CH3 CH3 Aniline (a 1° aromatic amine) N-Methylaniline (a 2° aromatic amine) Benzyldimethylamine (a 3° aliphatic amine)
Structure & Classification • heterocyclic amine: An amine in which the nitrogen atom is part of a ring. • heterocyclic aliphatic amine: A heterocyclic amine in which the ring is saturated (has no C=C bonds). • heterocyclic aromatic amine: The amine nitrogen is part of an aromatic ring. Piperidine Pyrrolidine Pyridine (heterocyclic aliphatic amines) (heterocyclic aromatic amines) N H N H N N N Pyrimidine N N Imidazole N N N N H Purine H
Nomenclature • IUPAC names • We derive IUPAC names for aliphatic amines just as we did for alcohols. • Drop the final -e of the parent alkane and replace it by - amine. • Use a number to locate the amino group on the parent chain. CH3 CHCH3 NH2 NH2 H2 N NH2 1,6-Hexanediamine Cyclohexanamine 2-Propanamine
Nomenclature • IUPAC names (cont’d) • IUPAC nomenclature retains the common name aniline for C6H5NH2, the simplest aromatic amine. • Name simple derivatives of aniline by using numbers to locate substituents or, alternatively, use the prefixes ortho (o), meta (m), and para (p). • Several derivatives of aniline have common names that are still widely used; among them is toluidine: NH2 CH3 NH2 NO2 NH2 3-Methylaniline (m-Toluidine) Aniline 4-Nitroaniline (p-Nitroaniline)
Nomenclature • IUPAC names (cont’d) • Name unsymmetrical secondary and tertiary amines as N-substituted primary amines. • Take the largest group bonded to nitrogen as the parent amine. • Name the smaller group(s) bonded to nitrogen, and show their location on nitrogen by using the prefix N- (indicating that they are bonded to nitrogen). N CH3 CH3 NHCH3 N,N-Dimethyl- cyclopentanamine N-Methylaniline
Nomenclature • Common names • For most aliphatic amines, list the groups bonded to nitrogen in alphabetical order in one word ending in the suffix -amine. Diethylmethylamine sec-Butylamine N NH2 NH2 Cyclohexylamine NH2 Propylamine
Nomenclature • Amine salts • When four atoms or groups of atoms are bonded to a nitrogen atom, as for example CH3NH3 +, nitrogen bears a positive charge and is associated with an anion as a salt. • Name the compound as a salt of the corresponding amine. • Replace the ending -amine (or aniline or pyridine or the like) by -ammonium (or anilinium or pyridinium or the like) and add the name of the anion. ( CH3 CH2 )3 NH+ Cl- Triethylammonium chloride
Physical Properties • Like ammonia, low-molecular-weight amines have very sharp, penetrating odors. • Trimethylamine, for example, is the pungent principle in the smell of rotting fish. • Two other particularly pungent amines are 1,4- butanediamine (putrescine) and 1,5-pentanediamine (cadaverine). H2N NH2 1,5-Pentanediamine (Cadaverine) NH2 H2N 1,4-Butanediamine (Putrescine)
Physical Properties • Amines are polar compounds: • Both 1° and 2° amines have N-H bonds, and can form hydrogen bonds with one another. • 3° amines have no N-H bond and cannot form hydrogen bonds with one another.
Physical Properties • An N-H---N hydrogen bond is weaker than an O-H---O hydrogen bond, because the difference in electronegativity between N and H (3.0 - 2.1 = 0.9) is less than that between O and H (3.5 - 2.1 = 1.4). • We see the effect of hydrogen bonding between molecules of comparable molecular weight by comparing the boiling points of ethane, methanamine, and methanol. CH3 OH CH3 CH3 CH3 NH2 -6.3 65.0 32.0 31.1 MW (amu) bp (°C) 30.1 -88.6
Physical Properties • All classes of amines form hydrogen bonds with water and are more soluble in water than are hydrocarbons of comparable molecular weight. • Most low-molecular-weight amines are completely soluble in water. • Higher-molecular-weight amines are only moderately soluble in water or are insoluble.
Basicity of Amines • Like ammonia, amines are weak bases, and aqueous solutions of amines are basic. • The acid-base reaction between an amine and water involves transfer of a proton from water to the amine. CH3-N H H H-O-H CH3-N-H H H O-H Methylammonium hydroxide Methylamine (a base) + + - : : : : : :
Basicity of Amines • The base dissociation constant, Kb, for the reaction of an amine with water has the following form, illustrated for the reaction of methylamine with water to give methylammonium hydroxide. • pKb is defined as the negative logarithm of Kb Kb = = 4.37 x 10-4 [ CH3 NH3 + ] [ OH - ] [ CH3 NH2 ] pKb = - log 4.37 x 10 -4 = 3.36
Basicity of Amines • Aliphatic amines have about the same base strength, and are slightly stronger bases than NH3. • Aromatic and heterocyclic aromatic amines are considerably weaker bases than aliphatic amines. • Note that while aliphatic amines are weak bases by comparison with inorganic bases such as NaOH, they are strong bases among organic compounds. C6 H5 NH2 CH3 CH2 NH2 Aliphatic Ammonia Aromatic 3.0 - 4.0 4.74 8.5 - 9.5 Class pKb Example Name Ethanamine Aniline Stronger base Weaker base
Basicity of Amines • Assume that the amine, RNH2, has a pKb of 3.50 and that it is dissolved in blood, pH 7.40 (pOH 6.60). • We first write the base dissociation constant for the amine and then solve for the ratio of RNH3 + to RNH2. • substituting values for Kb and OH- gives: RNH2 H2 O RNH3 + OH- + + [RNH3 + ] [OH- ] [ RNH2 ] Kb = [RNH3 + ] [RNH2 ] [OH - ] Kb = [ RNH3 + ] [ RNH2 ] 3.2 x 10-4 2.5 x 10-7 = = 1300
Basicity of Amines • Given the basicities of amines, we can determine which form of an amine exists in body fluids, say blood. • In a normal, healthy person, the pH of blood is approximately 7.40, which is slightly basic. • If an aliphatic amine is dissolved in blood, it is present predominantly as its protonated (conjugated acid) form. HO HO NH2 Dopamine HO HO NH3 + Conjugate acid of dopamine (the major form present in blood plasma)
Reactions of Amines • The most important chemical property of amines is their basicity. • Amines, whether soluble or insoluble in water, react quantitatively with strong acids to form water-soluble salts. HO H NH2 HO HO HCl H2 O HO HO NH3 + Cl - H HO (R)-Norepinephrine hydrochloride (a water-soluble salt) + (R)-Norepinephrine (only slightly soluble in water)
Reactions of Amines • example: Complete each acid-base reaction and name the salt formed. ( CH3 CH2 )2 NH HCl N CH3 COOH + (a) (b) +
Reactions of Amines • example: Complete each acid-base reaction and name the salt formed. • solution: (CH3 CH2 ) 2 NH HCl N CH3 COOH N H (CH3 CH2 ) 2 NH2 + Cl - CH3 COO- Diethylammonium chloride + Pyridinium acetate + (a) (b) +
End Chapter 15 Amines