ionic compound

ionic compound, any of a large group of chemical compounds consisting of oppositely charged ions, wherein electron transfer, or ionic bonding, holds the atoms together. Ionic compounds usually form when a metal reacts with a nonmetal, where the metallic atoms lose an electron or electrons, becoming cations (positively charged ions), and the nonmetallic atoms gain an electron or electrons, becoming anions (negatively charged ions). Once the ions form, if they are in close proximity, their opposite charges attract, forming an ionic compound. Such compounds are characterized by ionic lattice structures, wherein the force of attraction between ions determines the compound’s chemical and physical properties.

Stable ions of atoms in group IA (the first column) of the periodic table form by losing one electron, taking on a +1 charge (usually written as ⁺ beside the atom designation, as in H⁺ or Li⁺). Atoms in group IIA lose two electrons to form stable ions with a charge of +2 (e.g., Mg²⁺ or Ca²⁺). Likewise, atoms in group IIIA lose three electrons to form stable ions with a +3 charge (e.g., Al³⁺). All the electrons that are lost are located in the outermost shell of the atom and are known as valence electrons. Once the valence electrons are lost, the now outermost shell of electrons is full, creating a stable ion.

Larger metal atoms require a more complicated process to lose electrons and achieve a stable ionic form. Some atoms, such as lead, iron, chromium, mercury, tin, and nickel, have more than one stable ionic form. Iron, for example, can be stable whether it loses two or three electrons, forming ions of Fe²⁺ or Fe³⁺. For group VIIA, stable ions form when the atoms gain one electron, forming ions with a −1 charge (e.g., Cl⁻). Atoms from group VIA form stable ions when they gain two electrons, forming ions with a −2 charge (e.g., O²⁻). Atoms from group VA form stable ions when they gain three electrons, forming ions with a −3 charge (e.g., N³⁻); this gain in electrons fills the outer shell of electrons for these atoms, forming a stable ion with a negative charge.

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chemical bonding: Ionic and covalent compounds

When positive and negative ions join to form an ionic compound, the total number of electrons lost must be equal to the total number of electrons gained. Thus, there must be a net zero charge when the atoms combine. For example, in order for aluminum (Al³⁺) to form an ionic compound with an ion of oxygen (O²⁻; also known as an oxide ion), aluminum must lose six electrons, and oxygen must gain six electrons; this requires two ions of aluminum and three ions of oxygen, resulting in the ionic compound aluminum oxide (Al₂O₃). (Ionic compounds are named according to the element that loses electrons, followed by the name of the element that gains electrons, with a modified -ide ending.)

Ionic compounds can also form when metals and polyatomic ions interact. A polyatomic ion is an ion made up of more than one atom; examples include nitrate (NO₃⁻¹) and chlorite (ClO₂⁻¹). Similar to ionic compounds that contain two types of atoms, the total positive charge must be equal to the total negative charge in a polyatomic ion. For example, in magnesium nitrate, the magnesium ion has a +2 charge, while nitrate (NO₃⁻¹) has a −1 charge. Thus, two nitrate polyatomic ions are needed to balance the ionic charge of the magnesium ion, resulting in the formula Mg(NO₃)₂.