Explain boiling point and volatility trends using intermolecular forces.

Boiling point and volatility trends can be explained by the strength of intermolecular forces present in a substance. Stronger intermolecular forces, such as hydrogen bonds or dipole-dipole interactions, require more energy to overcome, resulting in higher boiling points. Conversely, substances with weaker London dispersion forces tend to have lower boiling points and higher volatility, as they evaporate more easily. For example, water, which exhibits hydrogen bonding, has a higher boiling point compared to methane, which only has London dispersion forces. Thus, the type and strength of intermolecular forces directly influence the boiling point and volatility of substances.