Describe the intermolecular forces that must be overcome to...

Describe the intermolecular forces that must be overcome to convert these substances from a liquid to a gas: (a) $\mathrm{SO}_{2}$, (b) $\mathrm{CH}_{3} \mathrm{COOH}_{\text {, }}$ (c) $\mathrm{H}_{2} \mathrm{~S}$.

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Key Concepts

Intermolecular Forces

These are the forces of attraction between molecules that determine many physical properties of substances, such as boiling and melting points. In the process of converting a liquid to a gas, the energy provided must overcome these forces to allow molecules to separate from one another.

London Dispersion Forces

These are weak, temporary attractive forces that arise due to momentary fluctuations in electron density in all molecules, but are particularly significant in non-polar molecules. They increase with the size and polarizability of the molecule and must be overcome during vaporization.

Dipole-Dipole Interactions

These are forces that occur between molecules with permanent dipoles, where the positive end of one molecule is attracted to the negative end of another. Their strength depends on the magnitude of the dipoles and the arrangement of molecules, and they are key in determining the energy required for phase changes in polar substances.

Hydrogen Bonding

A strong type of dipole-dipole interaction, hydrogen bonding occurs when hydrogen is directly bonded to highly electronegative atoms like oxygen, nitrogen, or fluorine. These bonds significantly increase the boiling point of substances, and breaking them requires more energy when moving from a liquid to a gas.

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