Predict the chemical formula of the ionic compound formed between the following pairs of elements: (d) Mg and N

Key Concepts

Ionic Bonding

Ionic bonding occurs when atoms transfer electrons to achieve full outer electron shells, resulting in the formation of charged ions. Metals, like magnesium (Mg), tend to lose electrons and form cations, while nonmetals, like nitrogen (N), gain electrons to form anions. The electrostatic attraction between these oppositely charged ions creates a stable ionic compound.

Charge of Ions

The charge of ions is determined by the number of electrons lost or gained by an atom. Magnesium typically loses two electrons to form a Mg²⁺ ion, while nitrogen gains three electrons to form an N³⁻ ion. Understanding the charges of the ions is crucial for predicting the correct ratio of ions in the resulting ionic compound.

Empirical Formula

The empirical formula of an ionic compound represents the simplest whole-number ratio of the ions present. For magnesium and nitrogen, the charges of Mg²⁺ and N³⁻ must be balanced to determine the formula. The least common multiple of the charges (6) indicates that two magnesium ions and three nitrogen ions combine to form the compound, resulting in the empirical formula Mg3N2.