Multiple Choice
Which statement best describes the movement of molecules in liquids compared to solids and gases?
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13. Liquids, Solids & Intermolecular Forces
Intermolecular Forces and Physical Properties
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Which of the following correctly ranks the boiling points of the molecules CH\(_3\)CH\(_2\)OH, CH\(_3\)OCH\(_3\), and CH\(_4\) from highest to lowest?
A
CH\(_3\)OCH\(_3\) > CH\(_4\) > CH\(_3\)CH\(_2\)OH
B
CH\(_3\)CH\(_2\)OH > CH\(_3\)OCH\(_3\) > CH\(_4\)
C
CH\(_4\) > CH\(_3\)CH\(_2\)OH > CH\(_3\)OCH\(_3\)
D
CH\(_3\)OCH\(_3\) > CH\(_3\)CH\(_2\)OH > CH\(_4\)
Verified step by step guidance1
Identify the types of intermolecular forces present in each molecule, as boiling points depend largely on these forces.
For CH\(_3\)CH\(_2\)OH (ethanol), recognize that it can form hydrogen bonds due to the -OH group, which are strong intermolecular forces that increase boiling point.
For CH\(_3\)OCH\(_3\) (dimethyl ether), note that it has dipole-dipole interactions because of the polar C-O-C bond, but it cannot hydrogen bond like ethanol.
For CH\(_4\) (methane), understand that it is nonpolar and only exhibits weak London dispersion forces, resulting in the lowest boiling point among the three.
Rank the boiling points based on the strength of intermolecular forces: hydrogen bonding (ethanol) > dipole-dipole (dimethyl ether) > London dispersion forces (methane).
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