Coordinate covalent bond

Definition

A coordinate covalent bond is a type of covalent bond in which one atom provides both electrons for the shared pair. This often occurs between a Lewis base and a Lewis acid.

5 Must Know Facts For Your Next Test

1. In a coordinate covalent bond, the electron donor is typically called the Lewis base and the electron acceptor is called the Lewis acid.
2. Once formed, a coordinate covalent bond behaves like any other covalent bond.
3. Coordinate covalent bonds are common in complex ions and coordination compounds.
4. The formation of this bond can be represented with an arrow pointing from the donor to the acceptor.
5. An example of a coordinate covalent bond is found in the ammonium ion (NH4+), where nitrogen donates a pair of electrons to hydrogen.

Review Questions

• What distinguishes a coordinate covalent bond from a regular covalent bond?
• How does the concept of Lewis acids and bases relate to coordinate covalent bonds?
• Provide an example of a molecule or ion that contains a coordinate covalent bond.

Related terms

Lewis Acid:

A species that accepts an electron pair during the formation of a coordinate covalent bond.

Lewis Base:

A species that donates an electron pair during the formation of a coordinate covalent bond.

Complex Ion:

An ion consisting of a central metal atom or ion bonded to surrounding molecules or anions through coordinate covalent bonds.