Metallic bond - definition
Metallic bond - definition
A metallic bond is a type of chemical bond occurring between metal atoms, characterised by a specific electronic structure in which the external valence electrons form what is known as an electron gas moving freely throughout the crystal structure of the metal. These electrons are not assigned to a specific positive ion, but form a common electron field, responsible for the cohesion and physicochemical properties of the material.
The mechanism of metallic bonding involves an electrostatic interaction between positively charged atomic cores (metal cations) and a negatively charged electron gas. This delocalisation of electrons causes metals to exhibit high electrical and thermal conductivity, high plasticity and a characteristic surface sheen. The free movement of electrons promotes easy energy and charge transfer, making metals materials of particular importance in electrical engineering, electronics and materials engineering.
Metallic bonding occurs not only in pure metals, but also in their alloys, where a structure based on a common electron field is maintained despite the presence of different elements. Its strength depends on the number of valence electrons and the packing density of the ions in the crystal lattice, which translates into mechanical properties such as hardness, elasticity or resistance to deformation.
In the band model, metallic bonding is explained by the overlap of energy levels of atoms and the formation of a conduction band in which electrons can move freely. The presence of incompletely filled energy bands underlies the electrical conductivity of metals and distinguishes them from dielectrics and Semiconductors. This bond, although not spatially localised like covalent bonds, plays a key role in shaping the structure and function of engineering and functional materials in technology and industry.
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