Question

shown below are the lewis structures of two molecules (nonbonding electrons omitted for clarity), pentanol and pentane. which intermolecular force is primarily responsible for the difference in their boiling points? hydrogen bonding, dipole - dipole intermolecular forces, london (induced dipole) dispersion forces

Explanation:

Pentanol has a hydroxyl (-OH) group. Hydrogen bonding occurs when a hydrogen atom is bonded to a highly - electronegative atom (such as O, N, or F). In pentanol, hydrogen bonds can form between the -OH groups of different molecules. These hydrogen bonds are stronger intermolecular forces compared to the London (induced - dipole) dispersion forces present in non - polar pentane. Stronger intermolecular forces require more energy to break, resulting in a higher boiling point for pentanol.

Answer:

Hydrogen bonding