What distinguishes an ionic bond from a covalent bond?

An ionic bond is characterized by the transfer of electrons from one atom to another, typically occurring between a metal and a non-metal. In this process, one atom (usually the metal) loses one or more electrons, becoming a positively charged ion, while the other atom (usually the non-metal) gains those electrons, becoming a negatively charged ion. The resulting electrostatic attraction between these oppositely charged ions forms the ionic bond.

In contrast, a covalent bond is formed when two atoms share electrons. This sharing allows each atom to attain the electron configuration of a noble gas, leading to stability. Furthermore, covalent bonds can occur between non-metals and non-metals, rather than restricting themselves to metals.

The other choices provide incorrect or misleading information about bonds. For instance, stating that an ionic bond involves sharing electrons misrepresents the essential characteristic of ionic bonding. Similarly, claiming that covalent bonds only occur between metals overlooks the fundamental nature of these bonds. Lastly, asserting that both types of bonds involve equal sharing of electrons does not accurately reflect ionic bonds, where electrons are not shared but transferred. Thus, identifying that an ionic bond involves the transfer of electrons encapsulates the key distinction between ionic and covalent bonding.