A coordinate covalent bond is described as forming by donation of a lone pair from one partner into an acceptor orbital of the other. This formation description does not imply that the final electrons remain distinguishable by origin.
An electron-pair interaction represented as donation from a metal-base fragment into an orbital of a metal-acid fragment. electron counting must avoid adding a new pair twice to an already occupied donor orbital.
Donation from an occupied ligand orbital into a metal orbital of pi symmetry relative to the metal–ligand axis. It differs from metal-to-ligand pi backbonding.
Pi backbonding is donation from occupied metal orbitals into ligand acceptor orbitals with pi symmetry about the metal–ligand axis. In a carbonyl ligand, occupation of CO weakens C–O while strengthening metal–carbon bonding. Lower CO stretching spectroscopic wavenumber is therefore a useful comparative probe, with electrostatic and mode-coupling qualifications.
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A coordinate covalent bond, also known as a dative bond, is a type of chemical bond in which one atom provides both electrons that are shared in the bond with another atom. This contrasts with a typical covalent bond, where each atom contributes one electron to the bond. In a coordinate covalent bond, the atom donating the pair of electrons is usually a Lewis base, while the atom accepting the electron pair is typically a Lewis acid.