metallic bond

In metallic bonding, metal ions are tightly packed with their outer shell electrons overlap, so each electron becomes detached from its parent atom (delocalized). The metal is held together by the strong forces of attraction between the positive nuclei and the surrounding sea of delocalized electrons.

Force of attraction operating in a metal that holds the atoms together in a metallic structure. In metallic bonding, metal atoms form a close-packed, regular arrangement. The atoms lose their outer-shell electrons to become positive ions. The outer electrons become a ‘sea’ of mobile electrons surrounding a lattice of positive ions. The lattice is held together by the strong attractive forces between the mobile electrons and the positive ions.

The properties of metals can be explained in terms of metallic bonding. Metals conduct electricity as the electrons are free to move. Conduction of heat occurs by vibration of the positive ions as well as via the mobile electrons. Metals are both ductile and malleable because the bonding is not broken when metals are deformed; instead, the metal ions slide over each other to new lattice positions.