Topic 4.4: Metallic Bonding

4.4.1 Describe the metallic bond as the electrostatic attraction between a lattice of positive ions and delocalized electrons.

In the elemental state, when there is no other element present to accept the electron and form an ionic compound, the outer electrons held only loosely by atom's nucleus tend to 'wander off' or, more correctly, become delocalized. This means that in metals they will no longer be associated closely with any one atomic nucleus but instead can spread themselves through the metals structure. The metal atoms without these electrons become positively charged ions and form a regular lattice structure which electrons can move freely.

4.4.2 Explain the electrical conductivity and malleability of metals

Metals are good conductors of electricity because the delocalized electrons are highly mobile and can move through the metal structure in response to an applied voltage. This mobility of electrons is responsible for the fact that they are also very good conductors. The unduly change in the confirmation of the metal through applied pressure. This property means that metals can be shaped under pressure so they are said to be malleable. A related property is that metals are ductile, meaning that they can be drawn out into threads.