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Coordinate covalent bonds are where both electrons in the bond are supplied by the same atom, sometimes represented by an arrow drawn from the donator to the receiver instead of a line for regular covalent bonds.
A regular covalent bond is when two atoms both contribute one of their electrons to the bond. A coordinate covalent bond is when only one of the atoms is contributing the electrons to the bond. One example is carbon monoxide (CO) where two of its bonds are regular covalent, but the third is a coordinate covalent bond where the two electrons involved in the bond both come from oxygen.
A regular covalent bond involves the sharing of electrons between 2 species. However, a coordinate bond is formed when one species donates a lone pair of electrons to an empty orbital of another species, which means that both electrons are supplied by the same species. We usually use an arrow to indicate a coordinate bond, the arrow should be drawn from the electron donor to the electron acceptor.
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