Which type of bond involves the sharing of electron pairs between atoms?

The bond that involves the sharing of electron pairs between atoms is a covalent bond. In a covalent bond formation, two atoms, typically nonmetals, come together and share one or more pairs of electrons to achieve a more stable electronic configuration, similar to that of noble gases. This mutual sharing allows each atom to attain a full outer shell of electrons, thereby enhancing stability.

Covalent bonds can be single (sharing one pair of electrons), double (sharing two pairs), or triple (sharing three pairs) depending on how many electrons are shared between the atoms. This type of bonding is fundamental to the structure of many compounds, particularly organic molecules, where the sharing of electrons plays a crucial role in the formation of molecules like water, carbon dioxide, and larger organic compounds.

In contrast, an ionic bond involves the transfer of electrons from one atom to another, resulting in the formation of charged ions. A metallic bond is characterized by a sea of delocalized electrons shared among a lattice of metal atoms. Hydrogen bonds are a specific type of attraction between a hydrogen atom covalently bonded to a highly electronegative atom and another electronegative atom; they do not involve the sharing of electron pairs in the way covalent bonds do.