What is ionic bonding characterized by?

Ionic bonding is characterized by the electrostatic attraction between charged particles, specifically between positively charged cations and negatively charged anions. In the formation of ionic bonds, atoms transfer electrons, resulting in the generation of ions. For example, when sodium (Na) loses an electron, it becomes a positively charged ion (Na⁺), while chlorine (Cl) gains that electron and becomes a negatively charged ion (Cl⁻). The opposite charges of these ions create a strong electrostatic attraction, which is the essence of ionic bonding.

This fundamental interaction leads to the formation of ionic compounds, which typically exhibit high melting and boiling points due to the strong forces of attraction between the ions. The stability of such compounds originates from the significant energy released during the formation of ionic bonds, which is much greater compared to other types of bonding, such as covalent bonds where electrons are shared rather than transferred.

In contrast, covalent bonding involves sharing electrons, the other choice refers to weak interactions, and attraction between neutral atoms is not typical of ionic bonding as it involves charged species. Thus, the distinct nature of ionic bonds lies in the strong attractions formed between ions of opposite charges.