Covalent vs Coordinate Bond: Key Differences & Examples
A covalent bond is when two atoms share a pair of electrons equally; a coordinate (dative) bond is a special case where one atom donates both electrons to the shared pair.
People confuse them because every coordinate bond is technically covalent—textbooks often tuck it under the same chapter—so students assume “covalent” covers all sharing and overlook the donor-only twist.
Key Differences
Covalent bonds form by mutual sharing (each atom brings one electron). Coordinate bonds form when a lone-pair donor gives both electrons to an electron-deficient acceptor. Equal vs. one-sided contribution.
Examples and Daily Life
H₂O is classic covalent. The ammonium ion NH₄⁺ shows a coordinate bond: NH₃ donates its lone pair to H⁺. Your vitamin B12 cobalt complex and the O₂ carried by hemoglobin rely on metal-ligand coordinate bonds.
Is a coordinate bond stronger?
Not necessarily; strength depends on the atoms involved, not the bond type.
Can it switch to normal covalent?
Yes, once formed, the electron pair is indistinguishable from other covalent bonds.