How is a covalent bond defined?

A covalent bond is defined as the force that holds two neighboring nuclei together by sharing electrons. This occurs when two atoms come close enough for their atomic orbitals to overlap, allowing electrons to be shared between them. The sharing of electrons enables both atoms to achieve a more stable electron configuration, often resembling that of noble gases, which typically involves having a full outer electron shell. This is particularly common in nonmetal elements, where atoms have similar electronegativities and are more likely to share electrons rather than transfer them.

The concept of sharing electrons distinguishes a covalent bond from ionic bonds, where electrons are completely transferred from one atom to another, leading to the formation of charged ions. The other options reflect different types of interactions or bonding mechanisms that do not accurately describe the nature of covalent bonds. For example, attraction between opposite charges typically describes ionic bonds, while temporary interactions between molecules can refer to forces like van der Waals or hydrogen bonds, which are different from the stable and directional nature of covalent bonds.