26.2 Amines – Physical Properties

Learning Objectives

By the end of this section, you will be able to:

  • Explain why the boiling points of primary and secondary amines are higher than those of alkanes or ethers of similar molar mass but are lower than those of alcohols.
  • Compare the boiling points of tertiary amines with alcohols, alkanes, and ethers of similar molar mass.
  • Compare the solubilities in water of amines of five or fewer carbon atoms with the solubilities of comparable alkanes and alcohols in waterProperties of Amines

Properties of Amines

Primary and secondary amines have hydrogen atoms bonded to an nitrogen atom and are therefore capable of hydrogen bonding (part (a) of Figure 26.2a.), although not as strongly as alcohol molecules (which have hydrogen atoms bonded to an oxygen atom, which is more electronegative than nitrogen). These amines boil at higher temperatures than alkanes but at lower temperatures than alcohols of comparable molar mass. For example, compare the boiling point of methylamine (CH3NH2; −6°C) with those of ethane (CH3CH3; −89°C) and methanol (CH3OH; 65°C). Tertiary amines have no hydrogen atom bonded to the nitrogen atom and so cannot participate in intermolecular hydrogen bonding. They have boiling points comparable to those of ethers (Table 26.2a.).

Diagram (a) below shows a 3D molecule of an amine forming hydrogen bonds with another amine. Diagram (b) shows that an amine can also form hydrogen bonds with water molecules.
Figure 26.2a. Hydrogen Bonding. (a) Amine molecules are associated through hydrogen bonding. (b) An amine molecule can form a hydrogen bond with water molecules (credit: Intro Chem: GOB (V. 1.0).CC BY-NC-SA 3.0).
Table 26.2a. Physical Properties of Some Amines and Comparable Oxygen-Containing Compounds
Name Condensed Structural Formula Class Molar Mass Boiling Point (°C) Solubility at 25°C (g/100 g Water)
butylamine CH3CH2CH2CH2NH2 73 78 miscible
diethylamine (CH3CH2)2NH 73 55 miscible
butyl alcohol CH3CH2CH2CH2OH 74 118 8
dipropylamine (CH3CH2CH2)2NH 101 111 4
triethylamine (CH3CH2)3N 101 90 14
dipropyl ether (CH3CH2CH2)2O 102 91 0.25

Source: “15.11: Physical Properties of Amines” In Basics of GOB Chemistry (Ball et al.), CC BY-NC-SA 4.0.

All three classes of amines can engage in hydrogen bonding with water (Figure 26.2a.). Amines of low molar mass are quite soluble in water; the borderline of solubility in water is at five or six carbon atoms (Table 26.2a.).

Spotlight on Everyday Chemistry: Hazards with Amines

Amines have “interesting” odours. The simple ones smell very much like ammonia. Higher aliphatic amines smell like decaying fish. Or perhaps we should put it the other way around: Decaying fish give off odorous amines. The stench of rotting fish is due in part to two diamines: putrescine and cadaverine. They arise from the decarboxylation of ornithine and lysine, respectively, amino acids that are found in animal cells.

Aromatic amines generally are quite toxic. They are readily absorbed through the skin, and workers must exercise caution when handling these compounds. Several aromatic amines, including β-naphthylamine (Figure 26.2b.), are potent carcinogens.

 

Two heterocyclic carbon rings attached to one another with an amino group (NH2) off of one of the carbon atoms in the ring.
Figure 26.2b. Structure of beta-naphthylamine. (Credit: Intro Chem: GOB (V. 1.0).CC BY-NC-SA 3.0)

 

Cigarettes and cigarette smoke also have amine-based compounds.  Read more in Infographic 26.2a.

Infographic 26.2a.  Chemical compounds in cigarette smoke contain amines including aromatic amines. Read more about “The Chemicals in Cigarette Smoke & Their Effects” by Andy Brunning / Compound Interest, CC BY-NC-ND, or access a text-based summary of infographic 26.2a [New tab].

Exercise 26.2a

  1. Which compound has the higher boiling point, CH3CH2CH2CH2CH2NH2 or CH3CH2CH2CH2CH2CH3? Explain.

  2. Which compound is more soluble in water, CH3CH2CH2CH2CH3 or CH3CH2NHCH2CH3? Explain.

     

Check Your Answers:[1]

Spotlight on Everyday Chemistry: Scientist Dr. Nadine Borduas

Research on nitrogen-containing amine compounds in the atmosphere is explained in Infographic 26.2b.

The image and name of Dr. Nadine Borduas. Department of Chemistry, University of Toronto.

Infographic 26.2b. Read more about “RTC Week 2015 – #3: Nitrogen-Containing Atmospheric Pollutants” by Andy Brunning / Compound Interest, CC BY-NC-ND, or access a text-based summary of infographic 26.2b [New tab].

Attribution & References

Except where otherwise noted, this page is adapted by Caryn Fahey and Samantha Sullivan Sauer from


    1. CH3CH2CH2CH2CH2NH2 because the nitrogen-to-hydrogen (N–H) bonds can engage in hydrogen bonding; CH3CH2CH2CH2CH2CH3 cannot engage in hydrogen bonding
    2. CH3CH2NHCH2CH3 because amines can engage in hydrogen bonding with water; alkanes cannot engage in hydrogen bonding

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Organic and Biochemistry Supplement to Enhanced Introductory College Chemistry Copyright © 2024 by Gregory Anderson; Caryn Fahey; Adrienne Richards; Samantha Sullivan Sauer; David Wegman; and Jen Booth is licensed under a Creative Commons Attribution-NonCommercial-ShareAlike 4.0 International License, except where otherwise noted.

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