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How does a coordinate-covalent bond differ from an ordinary covalent bond?

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Two diagrams show the three-dimensional structure of a methane molecule: panel A uses a ball-and-stick model with a central carbon atom connected to four hydrogen atoms in a tetrahedral arrangement, while panel B illustrates the bond angle of 109.5 degrees and bond length of 1.09 angstroms between carbon and hydrogen atoms. — chemical compound Methane, in which four hydrogen atoms are bound to a single carbon atom, is an example of a basic chemical compound. The structures of chemical compounds are influenced by complex factors, such as bond angles and bond length.

A coordinate-covalent bond (also known as a coordinate bond or dative bond) is often described as a type of covalent bond where both electrons in the shared pair are supplied by only one of the two atoms involved. In contrast, in an ordinary covalent bond, each atom typically contributes one electron to the shared bonding pair.123

However, it is important to note that modern chemical theory suggests this distinction is largely a matter of historical nomenclature rather than a fundamental difference in the nature of the bonds themselves. Once a bond is formed, the electrons are shared between the nuclei, and there is no physical difference between a bond formed from two separate electrons and one formed from a lone pair. Consequently, the idea that a coordinate-covalent bond differs fundamentally from an ordinary covalent bond has fallen into disfavor among chemists, as both are simply covalent bonds consisting of shared electron pairs.32