Question

section 3: bonding in metals

1. how is the electrical conductivity of a metal explained by metallic bonds?
2. what are metallic bonds?

Explanation:

1. In metallic - bonding, metal atoms lose their outer - shell electrons to form a 'sea' of delocalized electrons. When a potential difference is applied, these delocalized electrons can move freely throughout the metal lattice, carrying an electric current, thus explaining electrical conductivity.
2. Metallic bonds are the electrostatic forces of attraction between the positively - charged metal ions (cations) and the delocalized electrons in a metal. The metal atoms lose their outer - shell electrons, which become free to move, while the remaining positive ions are arranged in a regular lattice structure. The delocalized electrons act as a 'glue' holding the metal ions together.

Answer:

1. In metallic bonding, delocalized electrons can move freely under a potential difference, enabling electrical conductivity.
2. Metallic bonds are the electrostatic attractions between positive metal ions and delocalized electrons.