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An ionic bond forms when one atom transfers electrons to another atom, creating oppositely charged ions that attract each other electrostatically. This electron transfer typically occurs between a metal and a nonmetal, where the metal loses electrons to become a positively charged cation and the nonmetal gains electrons to become a negatively charged anion. The strong electrostatic attraction between these opposite charges holds the compound together.

Cations are positively charged ions formed when an atom loses electrons, while anions are negatively charged ions formed when an atom gains electrons. In ionic compounds, cations and anions combine in specific ratios to achieve electrical neutrality. The number of electrons transferred determines the charge on each ion and the overall stability of the resulting ionic compound.

Metals readily lose valence electrons because they have low ionization energy, while nonmetals readily gain electrons because they have high electron affinity. This difference in electron behavior makes electron transfer favorable between these element types. When a metal donates electrons to a nonmetal, both atoms achieve stable electron configurations, forming a strong ionic bond.

Valence electrons are the outermost electrons that participate in ionic bonding. Atoms transfer valence electrons to achieve a stable electron configuration, typically matching the nearest noble gas. The number of valence electrons an atom has determines how many electrons it will lose or gain, which directly affects the charge of the resulting ion and the formula of the ionic compound.

Ionic compounds consist of discrete cations and anions held together by electrostatic attraction, forming crystalline solids with repeating three-dimensional patterns. Covalent bonds, by contrast, involve shared electrons between atoms forming distinct molecules. Ionic compounds typically have higher melting points and conduct electricity when dissolved or melted, whereas covalent compounds are often molecular with lower melting points.

The chemical formula of an ionic compound is determined by the charges of the cation and anion. Ions combine in ratios that balance their charges to achieve electrical neutrality. For example, a cation with a +2 charge combines with two anions each with a -1 charge. This charge-balancing principle ensures the compound has no net electrical charge.

Electrostatic attraction is the force between oppositely charged ions that holds an ionic bond together. The strength of this attraction depends on the magnitude of the charges and the distance between ions. Stronger charges and closer proximity result in stronger ionic bonds. This electrostatic force is responsible for the high melting points and solid crystalline structure characteristic of ionic compounds.