Which describes metallic bonding?

• A. Metal + metal
• B. Covalent bonding between nonmetals
• C. Ionic bonding between metals and nonmetals
• D. Hydrogen bonding

Answer: (A)

Metallic bonding is the electrostatic attraction that holds metal atoms together in a solid by a sea of delocalized electrons. In this model, metal atoms release some of their electrons, which become free to move among the positively charged metal ions arranged in a lattice. The mobile electrons cling to all the ions, producing a strong, non-directional bond throughout the structure. This explains why metals conduct electricity, are malleable, and are lustrous—the electron sea enables easy movement of charge and deformation of the lattice without breaking distinct bonds.

This bonding description is distinct from covalent bonding (where atoms share electron pairs between nonmetals), ionic bonding (transfer of electrons creating oppositely charged ions between metals and nonmetals), and hydrogen bonding (an intermolecular attraction involving hydrogen bound to highly electronegative atoms like nitrogen, oxygen, or fluorine). The metal–metal interaction with a delocalized electron cloud best matches metallic bonding.