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Why is the term coordinate covalent bond used less often in modern chemistry?

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Diagram showing the formation of a polar covalent bond in a water molecule, with two hydrogen atoms bonding to one oxygen atom to form H2O, illustrating shared electrons and chemical reaction. — covalent bond In polar covalent bonds, such as that between hydrogen and oxygen atoms, the electrons are not transferred from one atom to the other as they are in an ionic bond. Instead, some outer electrons merely spend more time in the vicinity of the other atom. The effect of this orbital distortion is to induce regional net charges that hold the atoms together, such as in water molecules.

The term "coordinate covalent bond" (or dative bond) is used less frequently in modern chemistry because it creates a misleading distinction between types of covalent bonds.

In older chemical formulations, a distinction was made based on the origin of the shared electrons: a standard covalent bond was viewed as one electron being supplied by each atom, while a coordinate covalent bond was described as both electrons being supplied by a single atom. However, modern chemistry recognizes that once a bond is formed, there is no physical difference between the electrons regardless of their origin.1

The continued use of the term has fallen into disfavor for two primary reasons:
* It is difficult and often unnecessary to track the specific origin of bonding electrons in complex molecules.1
* It incorrectly implies that a coordinate covalent bond is fundamentally different from a standard covalent bond, when in reality, they are identical in nature.1

While the term is still occasionally referenced in specific contexts—such as valence bond theory—the modern understanding emphasizes that all covalent bonds consist of shared electron pairs.123