What characterizes a covalent bond?

A covalent bond is characterized by the sharing of electrons between atoms. This type of bond typically occurs between nonmetal atoms that have similar electronegativities, allowing them to achieve a more stable electron configuration together without fully transferring electrons. When atoms share electrons equally, it is often referred to as a nonpolar covalent bond. However, even in cases where atoms share electrons unequally (which leads to polar covalent bonds), the fundamental nature of covalent bonding is rooted in the sharing of electrons rather than any other interactions.

The other options illustrate different bonding concepts. The transfer of electrons is indicative of ionic bonds, where one atom gives up one or more electrons to another atom. Atoms attracting through ionic charge describes the electrostatic force that holds ions together in an ionic bond, not covalent. Being chemically inert typically relates to noble gases, which do not form covalent bonds due to their full valence shell, rather than defining covalent bonding itself. Therefore, the defining feature of covalent bonds remains primarily established through the sharing of electrons.