Which description best captures metallic bonding?

• A. Forms discrete molecules in all states
• B. Requires full transfer of electrons
• C. Involves a lattice of cations in a sea of delocalized electrons
• D. Covalent bonds between metal and nonmetal

Answer: (C)

Metallic bonding is the electrostatic attraction between a lattice of positively charged metal ions and a surrounding sea of delocalized electrons that move freely. These electrons aren’t tied to any one atom, so they flow under an electric field, giving metals their conductivity. The cation lattice held together by this sea explains why metals are malleable and ductile—layers can slide, while the electron cloud cushions repulsion. This picture also shows why bonding in metals isn’t described as discrete molecules or as full electron transfer, and it isn’t covalent bonds between metal and nonmetal.