Coordinate covalent bond
Coordinate Covalent Bond[edit | edit source]
A coordinate covalent bond, also known as a dative bond or coordinate bond, is a type of chemical bond in which both electrons involved in the bond are contributed by one atom. This differs from a typical covalent bond, where each atom contributes one electron to form a shared pair.
Formation[edit | edit source]
Coordinate covalent bonds are formed when one atom donates a lone pair of electrons to another atom that is electron-deficient. The atom donating the electrons is called the donor atom, while the atom accepting the electrons is called the acceptor atom. The donor atom is usually a Lewis base, capable of donating electron pairs, while the acceptor atom is typically a Lewis acid, capable of accepting electron pairs.
Examples[edit | edit source]
One common example of a coordinate covalent bond is found in the formation of the ammonium ion (NH4+). In this case, a lone pair of electrons from the nitrogen atom is donated to a hydrogen ion (H+), resulting in the formation of a coordinate covalent bond between the nitrogen and the hydrogen. The resulting ammonium ion is stabilized by the formation of this bond.
Another example is the formation of the complex ion in transition metal coordination compounds. In these compounds, a transition metal ion acts as the acceptor atom, while a ligand, such as a molecule or an ion, acts as the donor atom. The ligand donates a lone pair of electrons to the transition metal ion, forming a coordinate covalent bond.
Importance[edit | edit source]
Coordinate covalent bonds play a crucial role in many chemical reactions and biological processes. They allow for the formation of stable compounds and complexes, as well as the transfer of electrons between molecules. Additionally, they contribute to the stability and reactivity of transition metal complexes, which are widely used in catalysis and other applications.
References[edit | edit source]
See Also[edit | edit source]
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