Bonding in solids

Bonding in solids is the set of attractive interactions that hold atoms, ions, or molecules together in a solid, shaping its structure and properties.

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Ionic bonding: Electrostatic attraction between oppositely charged ions formed through electron transfer. It holds many salts together in extended lattices of positive and negative ions.
Coulomb's law: The law describing the electrostatic force between charged particles. Its attractions and repulsions underpin ionic bonding and contribute to other solid-state interactions.
Electrical conductivity: A measure of how readily electric charge moves through a material. Mobile electrons in metallic solids contrast with localized charge in many ionic and covalent solids.
Ionic crystal: A crystalline solid whose structure is built chiefly from oppositely charged ions. It is a clear case of electrostatic bonding in an extended solid.
Covalent bonding: A chemical bond formed when atoms share one or more pairs of electrons. Shared electrons link atoms into molecules or extended solid networks.
Band theory: A quantum-mechanical model describing allowed electron energy ranges in solids. Bonding and atomic orbital overlap produce bands that help explain solid conductivity.
Elastic modulus: A measure of a material's resistance to elastic deformation under applied stress. Bond stiffness helps set how much a solid deforms under load.
Covalent network solid: A solid whose atoms form an extended network of covalent bonds. It contrasts with solids built from discrete molecules or alternating ions.
Metallic bonding: Attraction between positive metal ions and delocalized valence electrons in a metal. Delocalized electrons bind metal atoms while allowing electrical conduction.
Electron localization function: A measure used to map regions where electrons are likely to be localized in a material. It helps distinguish localized bonds from more delocalized electronic structures.