AluminumIII

AluminumIII, often referred to as aluminum(III) or simply aluminum in contexts where other oxidation states are less common, represents the most stable and prevalent oxidation state of the element aluminum. In this state, an aluminum atom has lost three of its valence electrons, resulting in a positive charge of +3. This configuration, Al³⁺, is characteristic of aluminum in most of its chemical compounds.

Aluminum(III) compounds are ubiquitous in nature and industry. Aluminum oxide (Al₂O₃), also known as alumina, is a prime example, forming the basis of minerals like corundum, ruby, and sapphire. Aluminum hydroxide (Al(OH)₃) is another common compound, found in bauxite ore, the primary source for aluminum production. In solution, aluminum typically exists as the hydrated ion, [Al(H₂O)₆]³⁺.

The Al³⁺ ion is small and highly charged, which leads to significant polarizing power. This influences the properties of aluminum(III) compounds, often resulting in covalent character in their bonding. Aluminum(III) chemistry is diverse, encompassing salts, oxides, hydroxides, and organometallic compounds. Its amphoteric nature, meaning it can react with both acids and bases, is a key characteristic of its hydroxide and oxide. Industrially, aluminum(III) compounds are vital, serving as catalysts, abrasives, refractories, and in the production of ceramics and glass.