A coordinate covalent bond, also known as a dative bond or a coordinate bond, is a type of chemical bond between two atoms in which one atom donates a pair of electrons to a shared bonding orbital, which is typically located on the other atom. This results in the formation of a shared electron pair between the two atoms involved in the bond.
In a coordinate covalent bond, one atom acts as the electron pair donor, referred to as the Lewis base, while the other atom acts as the electron pair acceptor, referred to as the Lewis acid. The Lewis base donates the lone pair of electrons to the vacant orbital on the Lewis acid, creating a shared bonding pair that holds the atoms together in the molecule.
This type of bond is distinct from a typical covalent bond, where the electrons are shared equally between the two atoms involved. In a coordinate covalent bond, the shared electron pair is provided entirely by one atom, resulting in a slightly more polar bond.
Coordinate covalent bonds are commonly seen in coordination compounds, where a central metal atom or ion coordinates with ligands that donate electron pairs. They are also observed in other chemical species such as Lewis acids and bases, complex ions, and molecules with multiple resonance structures, among others.
Overall, coordinate covalent bonds play a crucial role in the formation and stability of various chemical compounds, contributing to the wide range of chemical reactions and interactions observed in nature.
