Coordinate covalent bond
covalent bond in a coordination complex in which the shared electrons are donated by one of the atoms and also known as dative bond
In coordination chemistry, a coordinate covalent bond, also known as a dative bond, dipolar bond, or coordinate bond is a kind of two-center, two-electron covalent bond in which the two electrons derive from the same atom. The bonding of metal ions to ligands involves this kind of interaction. This type of interaction is central to Lewis acid–base theory.
Coordinate bonds are commonly found in coordination compounds.
Examples
Coordinate covalent bonding is ubiquitous. In all metal aquo-complexes [M(H2O)n]m+, the bonding between water and the metal cation is described as a coordinate covalent bond. Metal-ligand interactions in most organometallic compounds and most coordination compounds are described similarly.
The term dipolar bond is used in organic chemistry for compounds such as amine oxides for which the electronic structure can be described in terms of the basic amine donating two electrons to an oxygen atom.
R3N → O
The arrow → indicates that both electrons in the bond originate from the amine moiety. In a standard covalent bond each atom contributes one electron.
This brief starts where responsible research should: with the source description of “Coordinate covalent bond” as covalent bond in a coordination complex in which the shared electrons are donated by one of the atoms and also known as dative bond. Everything that follows is an evidence route, not borrowed authority.
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