Which statement is true regarding ionic bonds?

Ionic bonds are characterized by the transfer of electrons from one atom to another. This typically occurs between atoms with significantly different electronegativities, such as metals and nonmetals. When a metal (which has a low electronegativity) loses one or more electrons, it becomes a positively charged ion, while the nonmetal (which has a high electronegativity) gains those electrons and becomes a negatively charged ion. The electrostatic attraction between these oppositely charged ions results in the formation of the ionic bond.

This process is fundamental to the structure of ionic compounds, contributing to their properties such as high melting and boiling points, as well as their ability to conduct electricity when dissolved in water. Understanding that ionic bonds are based on electron transfer clarifies why they differ from covalent bonds, which involve the sharing of electron pairs. Additionally, ionic bonds can form in various states of matter, not limited to gaseous states, allowing for a broader understanding of their occurrence in different chemical contexts.