Final answer:
The compound CH2CO2H, known as acetic acid, is influenced by hydrogen bonding due to the presence of a hydroxyl group, which facilitates this strong intermolecular force.
Step-by-step explanation:
The intermolecular force influencing the compound CH2CO2H is hydrogen bonding. This compound, also known as acetic acid, has a hydroxyl group (-OH) that can participate in hydrogen bonding with other molecules of acetic acid or with water. Hydrogen bonding is a strong type of dipole-dipole interaction that occurs when a hydrogen atom bonded to a strongly electronegative atom like oxygen, nitrogen, or fluorine is attracted to another electronegative atom in a nearby molecule. The carboxyl group (-CO2H) in acetic acid has this feature, thus facilitating hydrogen bonding, which greatly influences its physical properties such as boiling point and solubility.