Which bond is characterized by the sharing of an electron pair between non-metals?

A covalent bond is indeed characterized by the sharing of an electron pair between non-metal atoms. In this type of bond, each atom contributes one electron to the pair, which allows them to achieve a more stable electronic configuration similar to that of noble gases. This shared pair of electrons helps to hold the atoms together, creating a strong bond that is essential in forming molecules.

The strength and properties of covalent bonds can vary depending on the number of shared electron pairs (single, double, or triple bonds), but the fundamental concept remains the same—non-metals typically bond this way because they have similar electronegativities and thus tend to share electrons rather than transfer them.

Other types of bonds mentioned do not fit this description. Ionic bonds involve the complete transfer of electrons from one atom to another, leading to the attraction between charged ions. Dative covalent bonds involve one atom providing both electrons for the shared pair, but still fundamentally function like typical covalent bonds. Metallic bonds involve a "sea of electrons," where electrons are not shared between specific atoms but move freely throughout the metallic structure.