Which type of intermolecular force is primarily responsible for the ability of metals to conduct electricity?

• A. London dispersion forces between metal ions
• B. Dipole-dipole interactions within the metal structure
• C. Hydrogen bonding between metal atoms
• D. Metallic bonding, where electrons are delocalized and free to move throughout the lattice

Answer: (D)

Verified step by step guidance

1. Understand that the question asks about the type of intermolecular force responsible for electrical conductivity in metals.
2. Recall that metals consist of a lattice of positive metal ions surrounded by a 'sea' of delocalized electrons that are free to move.
3. Recognize that London dispersion forces, dipole-dipole interactions, and hydrogen bonding are types of intermolecular forces relevant mostly to molecular or covalent substances, not metals.
4. Identify that the key to electrical conductivity in metals is the presence of delocalized electrons that can move freely, which is a characteristic of metallic bonding.
5. Conclude that metallic bonding, involving a lattice of metal cations and a sea of mobile electrons, is the primary interaction enabling metals to conduct electricity.