Editing Delocalized electron (section)

== Electrical conduction ==
{{main|Metallic bonding}}
Delocalized electrons also exist in the structure of solid metals. Metallic structure consists of aligned positive [[ion]]s ([[cation]]s) in a "sea" of delocalized electrons. This means that the electrons are free to move throughout the structure, and gives rise to properties such as [[electrical conductivity|conductivity]].

In [[diamond]] all four outer electrons of each [[carbon]] atom are 'localized' between the atoms in covalent bonding. The movement of electrons is restricted and diamond does not conduct an electric current. In [[graphite]], each carbon atom uses only 3 of its 4 outer energy level electrons in covalently bonding to three other carbon atoms in a plane. Each carbon atom contributes one electron to a delocalized system of electrons that is also a part of the chemical bonding. The delocalized electrons are free to move throughout the plane. For this reason, graphite conducts electricity along the planes of carbon atoms, but does not conduct in a direction at [[right angle]]s to the plane.