Metallbinding

Metallic binding, or metallic bonding, is the type of chemical bond that holds atoms together in most metals and many alloys. In this bonding, atoms release some of their valence electrons to form a mobile electron cloud, or sea, that surrounds a lattice of positively charged metal ion cores. The resulting electrostatic attraction between the cations and the delocalized electrons binds the structure while allowing electrons to move freely.

This bonding is largely non-directional, which explains why metals are typically malleable and ductile: layers of atoms can slide past one another without breaking the overall bond network. The same electron sea accounts for high electrical and thermal conductivity, as electrons can transfer energy and charge quickly through the metal. Metals also exhibit metallic luster due to the interaction of free electrons with light.

Crystalline metals typically adopt one of several close-packed arrangements, such as body-centered cubic, face-centered cubic, or hexagonal close-packed structures. The specific arrangement and the presence of alloying elements influence properties such as strength, hardness, and temperature stability.

Alloys are common in practical materials. By combining metals with other elements, properties can be tailored; examples include steel (iron with carbon and sometimes other elements), brass (copper with zinc), and bronze (copper with tin).

In summary, metallic binding is characterized by a delocalized electron sea binding positively charged ion cores in a lattice, producing conductive, malleable materials with a distinctive luster, applicable across a wide range of engineering and everyday contexts.