Coordinate covalent bond

A covalent bond in which both shared electrons originate from one atom. Once formed, it behaves like other covalent bonds.

Lewis acid–base theory: A theory that defines acids as electron-pair acceptors and bases as electron-pair donors. The donor–acceptor description of this bond is expressed directly as a Lewis acid–base interaction.
Covalent bond: A chemical bond formed when atoms share one or more pairs of electrons. A coordinate covalent bond is a specific way a covalent bond can form.
Coordination complex: A structure with a central metal atom or ion bonded to surrounding ligands through coordinate bonds. Ligands commonly donate electron pairs to metal centers to form these structures.
Ionic bond: An electrostatic attraction between oppositely charged ions. Unlike an ionic bond, a coordinate covalent bond involves a shared electron pair.
Lewis structure: A diagram showing valence electrons and bonds in a molecule or ion. Lewis structures depict the donated pair as a bond between the donor and acceptor.
Valence electron: An electron in an atom's outer shell that can participate in chemical bonding. The donated pair consists of valence electrons from the donor atom.
Ammonium ion: The polyatomic cation NH₄⁺, formed when ammonia accepts a proton. In its formation, nitrogen donates a lone pair to H⁺.
Ordinary covalent bond: A covalent bond described as forming when each bonded atom contributes one electron to the shared pair. This contrast concerns the pair's origin during formation, not a lasting difference in the finished bond.
Lone pair: A pair of valence electrons localized on one atom and not shared in a bond. The bond begins as a lone pair on the atom that supplies both electrons.
Octet rule: A chemical guideline that atoms often form bonds to attain eight valence electrons. Coordinate donation can help an acceptor complete its valence shell.

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