Metallic bonding

Metallic bonding is the bonding within metals. It involves the delocalised sharing of free electrons between a lattice of metal atoms.

Metallic Bonding does NOT form any molecules or macromolecules. The outcome is described as "giant structure" or "giant lattice".

Delocalised electrons are often refered to as a 'Sea of Electrons' or sometimes a 'Fog of Electrons'.

Metal atoms have 1, 2 or 3 electrons in the outer shell (Energy Level). These become Delocalised and form a 'Sea of Electrons' surrounding a giant lattice of +ve ions.

Metallic bonding, as with covalent bonding is non-polar, in that there is no (for pure elemental metals) or very little (for alloys) electronegativity difference among the atoms participating in the bonding interaction, and the electrons involved in that interaction are delocalized across the crystalline structure of the metal.

The metallic bond accounts for many physical characteristics of metals, such as strength, malleability, ductility, conduction of heat and electricity, and luster. See also chemical bond.

Metallic bonding is the electrostatic attraction between the ions and the delocalised electrons. Which is why atoms or layers are allowed to slide pass each other, making the characteristic of malleable and ductile. The delocalised electrons allow conductivity of electricity both when solid and molten.