Metallic bonding is a unique type of chemical bonding that occurs in metals. Unlike ionic or covalent bonds, metallic bonding does not involve the sharing or transfer of electrons. Instead, it is based on a sea of delocalized electrons that surround the metal atoms. These delocalized electrons are free to move within the metal lattice, giving metals their characteristic properties. For example, metals are known for their good conductivity of heat and electricity, and this is due to the presence of these mobile electrons.

The bonding in metals can be visualized as a cation surrounded by a sea of electrons. The metal cations (positively charged ions) are held together by the attraction to these mobile electrons, creating a strong, continuous network. The presence of the delocalized electrons also explains the malleability and ductility of metals, as the metal ions can slide past each other easily without breaking the bond.