Which statement correctly explains how polarizability affects intermolecular forces?

• A. Lower polarizability results in stronger dipole-dipole interactions.
• B. Polarizability only affects ionic bonds and not intermolecular forces.
• C. Greater polarizability leads to stronger London dispersion forces between molecules.
• D. Greater polarizability leads to weaker hydrogen bonding between molecules.

Answer: (C)

Verified step by step guidance

1. Understand that polarizability refers to how easily the electron cloud around a molecule or atom can be distorted by an external electric field.
2. Recognize that London dispersion forces are a type of intermolecular force that arise due to temporary dipoles created when electron clouds fluctuate and become unevenly distributed.
3. Know that greater polarizability means the electron cloud is more easily distorted, which enhances the temporary dipoles and thus strengthens London dispersion forces.
4. Recall that dipole-dipole interactions depend on permanent dipoles, not directly on polarizability, so lower polarizability does not lead to stronger dipole-dipole interactions.
5. Understand that polarizability does not affect ionic bonds (which are strong electrostatic attractions between ions) or hydrogen bonding (which depends on specific interactions involving hydrogen and electronegative atoms), so statements about polarizability weakening hydrogen bonding or only affecting ionic bonds are incorrect.