Question

On the basis of intermolecular forces of attraction, rank the following three compounds in terms of increasing boiling point.

CH3CH2OH

CH3OCH3

CH3CH2CH3

a. (lowest bp) CH3CH2CH3 < CH3OCH3 < CH3CH2OH (highest bp)

b. (lowest bp) CH3CH2OH < CH3OCH3 < CH3CH2CH3 (highest bp)

c. (lowest bp) CH3OCH3 < CH3CH2OH < CH3CH2CH3 (highest bp)

d. (lowest bp) CH3CH2OH < CH3CH2CH3 < CH3OCH3 (highest bp)

e. (lowest bp) CH3CH2CH3 < CH3CH2OH < CH3OCH3 (highest bp)

Answer 1

Answer:

a. (lowest bp) CH3CH2CH3 < CH3OCH3 < CH3CH2OH (highest bp

Explanation:

CH3CH2OH is an alkanol. The intermolecular forces present within the molecules include dispersion forces, dipole-dipole attraction as well as hydrogen bonding which is the major intermolecular force of attraction present.

CH3OCH3 is an ether. The intermolecular forces present within the molecules are dispersion forces and dipole-dipole attraction.

CH3CH2CH3 is an alkane. The only intermolecular forces present is dispersion forces.

The order of increasing strength of these intermolecular forces is dispersion forces ,dipole-dipole forces<hydrogen bonding, the alkanol has the highest bioling point, followed by the ether and then the alkane with the lowest boiling point.

Answer 2

The ranking of the compounds in terms of increasing the boiling point is option a.

What is ethanol?

Ethanol i.e. (CH3-CH2-O-H) has three types of intermolecular interactions i.e. weak van der Waals interaction, dipole-dipole interaction, and strong intermolecular H-bonding interaction.

While on the other hand,  in dimethyl ether (CH3-O-CH3) have two types of interactions - weak van der Waals interaction, and dipole-dipole interaction.

In propane (CH3-CH2-CH3) has only weak van der Waals interaction.

So ethanol needed more energy to overcome this these interactions for the conversion to a liquid state to the gaseous state.

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