Structure: regular giant lattice made of close-packed metal cations surrounded by a sea of delocalised electrons

Electrons shared between cations, not associated with one particular nucleus of a metal

Metallic bond = the electrostatic attraction between a lattice of positive ions and delocalised electrons

Strength of metallic bond:

Relatively strong. Depends on:

1. # valance electrons that can be delocalised (more = stronger)

2. charge on metal ion (higher charge = stronger)

3. ionic radius of metallic cation (larger radius = weaker)

Properties:

Metal atoms can slide past each other and not break (= ductile & malleable) (ions can slide past and stay connected)
Good conductors of heat and electricity (because electrons can flow)

Alloys:

Mixture of different types of metal ions. Disrupts properties (becomes more brittle)

	Created by Annebelle Rombach about 6 years ago

From booklets teacher gave us.

Bonding SL & HL content