Lewis base

A chemical species that donates an electron pair to form a covalent bond with an electron-pair acceptor, called a Lewis acid.

Lewis acid: A chemical species that accepts an electron pair to form a covalent bond. It receives the pair donated by a Lewis base, completing the defining interaction.
Valence electron: An electron in an atom's outer shell that can participate in chemical bonding. Lewis-base behavior depends on the availability of valence electrons for donation.
Coordination complex: A compound in which a central metal atom or ion is bonded to surrounding ligands. Ligands commonly bind metal centers by donating Lewis-base electron pairs.
Brønsted base: A species that accepts a proton in a Brønsted–Lowry acid–base reaction. A Lewis base need not accept a proton; it can donate to other electron-pair acceptors.
Coordinate covalent bond: A covalent bond whose shared electron pair is supplied by one atom. A Lewis base forms this bond by supplying both bonding electrons.
Lewis structure: A diagram showing valence electrons as bonds and lone pairs in a molecule or ion. Lewis structures reveal the lone pairs that can act as donor sites.
Ligand: An ion or molecule that binds to a central atom or ion in a coordination complex. A ligand often functions as a Lewis base at its metal-binding site.
Nucleophilicity: A measure of how rapidly a reagent attacks an electrophile to form a bond. Lewis basicity is an equilibrium-oriented affinity, while nucleophilicity concerns reaction rate.
Lone pair: A pair of valence electrons localized on one atom and not shared in a bond. A lone pair is the usual source of electrons donated by a Lewis base.
Covalent bond: A chemical bond formed when atoms share electron pairs. Lewis donation creates a shared pair, placing the interaction within covalent bonding.

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