Question

section 3: bonding in metals

1. how is the electrical conductivity of a metal explained by metallic bonds?
2. what are metallic bonds? the electrostatic attractions between positive metal ions and delocalized electrons.

Explanation:

1. In metals, metallic bonds involve a sea of delocalized electrons. When an electric field is applied, these delocalized electrons can move freely throughout the metal lattice, which allows for the conduction of electricity.
2. Metallic bonds are the electrostatic attractions between positively - charged metal ions (cations) and a sea of delocalized electrons. The metal atoms lose their outer - shell electrons to form cations, and these electrons are then shared among all the metal ions in the lattice.

Answer:

1. The electrical conductivity of a metal is explained by metallic bonds because the delocalized electrons in metallic bonds can move freely under an electric field, facilitating the flow of electric current.
2. Metallic bonds are the electrostatic attractions between positive metal ions and a sea of delocalized electrons.