Metallic bonding

Metallic bonding is the attraction between positively charged metal ions and delocalized valence electrons shared throughout a solid. This mobile electron cloud binds the structure and helps explain metals’ conductivity and malleability.

Electron sea model: A model of metals in which valence electrons move freely among positively charged ions. It gives a simple picture of the delocalized electrons that hold metallic structures together.
Valence electron: An electron in an atom’s outer shell that can participate in bonding. Valence electrons become delocalized in the standard account of metallic bonding.
Ionic bonding: Bonding driven by electrostatic attraction between oppositely charged ions. Unlike metallic bonding, ionic bonding centers on distinct cations and anions.
Electrical wire: A conductor, usually metal, shaped to carry electric current between locations. Wires exploit the mobility of electrons in metallic materials.
Electrical conductivity: A material’s ability to carry electric current through the movement of charge. Mobile electrons in metallic bonds carry current through the solid.
Metallic element: A chemical element whose atoms commonly form conductive solids with metallic properties. Metallic bonding is the characteristic bonding pattern in many elemental metals.
Covalent bonding: Bonding in which atoms share electron pairs, often in directional arrangements. Metallic electrons are distributed through the solid instead of confined to shared pairs.
Heat exchanger: A device that transfers heat between fluids without mixing them. Metal components conduct heat efficiently, aided by mobile electrons.
Thermal conductivity: A material’s ability to transfer thermal energy through its structure. Delocalized electrons transport energy efficiently through many metals.
Crystal lattice: A repeating three-dimensional arrangement of points representing positions in a crystalline solid. The positively charged metal ions occupy ordered sites within a lattice.

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