What defines ionic bonding?

Ionic bonding is primarily defined by the electrostatic attraction between ions of opposite charges. When one atom donates an electron to another atom, it forms a positively charged ion (cation) and a negatively charged ion (anion). The ionic bond is the strong attraction that occurs between these oppositely charged ions, resulting in the formation of a stable ionic compound.

In contrast, other options describe different types of bonding. The sharing of electrons equally between atoms indicates covalent bonding, not ionic bonding. Similarly, the idea of ions being held together by covalent bonds misinterprets the nature of ionic interactions; covalent bonds involve shared electrons rather than interaction through charge. Lastly, the concept of molecules formed by overlapping atomic orbitals pertains to covalent bonding as well, where electrons are shared rather than transferred as in ionic bonding.

Thus, the defining feature of ionic bonding is indeed the attraction between ions of different elements that are held together by their opposite charges.