Textbook Question
In each pair, choose the compound you would expect to have the highest boiling/melting point.
(a)
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2. Molecular Representations
Intermolecular Forces
Multiple Choice
The structure of which of the following compounds suggests that it has the highest boiling point?
A
(chloromethane)
B
(dimethyl ether)
C
(methanol)
D
(methane)
Verified step by step guidance1
Identify the types of intermolecular forces present in each compound, as boiling point is largely influenced by these forces.
For chloromethane (CH\_3Cl), consider dipole-dipole interactions due to the polar C-Cl bond, along with London dispersion forces.
For dimethyl ether (CH\_3OCH\_3), recognize that it has dipole-dipole interactions because of the polar C-O-C linkage, plus London dispersion forces, but it cannot hydrogen bond because it lacks an O-H bond.
For methanol (CH\_3OH), note that it can form hydrogen bonds due to the presence of the O-H group, in addition to dipole-dipole and London dispersion forces, which significantly increases its boiling point.
For methane (CH\_4), only London dispersion forces are present, which are the weakest intermolecular forces among these compounds, leading to the lowest boiling point.
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