What type of bond is formed when two atoms share a pair of electrons?

A bond formed when two atoms share a pair of electrons is classified as a covalent bond. In this type of bond, the shared pair of electrons allows each atom to achieve greater stability, often resembling the electron configuration of noble gases.

When the sharing of electrons is equal, it leads to a nonpolar covalent bond. This typically occurs between atoms of the same element or atoms with similar electronegativities, meaning that neither atom has a significantly stronger pull on the shared electrons. As a result, the charge distribution remains even, and the molecule, as a whole, does not have distinct poles.

In contrast, a polar covalent bond involves an unequal sharing of electrons between two atoms with different electronegativities; one atom attracts the shared electrons more strongly than the other, resulting in a slight charge difference across the molecule. Hydrogen bonds are not covalent but rather a type of intermolecular attraction involving a hydrogen atom bonded to a highly electronegative atom. An ionizing bond, often referred to within the context of ionic bonds, does not involve sharing electrons at all but rather the transfer of electrons from one atom to another, leading to the formation of charged ions.