What is the formal charge for a coordinate covalent bond?

 A coordinate covalent bond (also known as a dative covalent bond or a coordinate bond) is a type of covalent bond formed when one atom provides both bonding electrons. In a coordinate covalent bond, one atom donates a pair of electrons to another atom, which then shares the electrons with another atom.

The formal charge of a coordinate covalent bond is the charge that an atom would have if the electrons in the bond were assigned to only one atom. In a coordinate covalent bond, the electron pair is shared between two atoms, so the formal charge of each atom is zero. Formal charge is calculated by the following formula:

Formal Charge = [number of valence electrons in free atom] - [number of non-bonding electrons] - [1/2 * number of bonding electrons]

When it comes to a coordinate covalent bond, since there is no transfer of electrons from one atom to another, the formal charge of each atom is zero. In other words, a coordinate covalent bond does not affect the formal charge of the atoms involved.

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