Aluminium
Start with the big picture
Aluminium has the electron configuration [Ne]3s²3p¹ and commonly forms Al³⁺. In water, this strongly Lewis-acidic ion undergoes hydrolysis. Aluminium and its oxide and hydroxide are amphoteric: they react with acids and bases, producing Al³⁺ or [Al(OH)₄]⁻, respectively. A thin, adherent Al₂O₃ layer helps protect the metal from corrosion. Industrially, alumina is obtained from bauxite by the Bayer process and converted to aluminium by Hall–Héroult electrolysis. The topic also links aluminium chemistry to thermite reduction, corundum and gemstones, AlCl₃ catalysis, water-treatment salts, alloys, and selected pharmaceutical uses. These examples show how structure and reactivity help explain aluminium’s practical importance.
What you'll learn
- Relate aluminium’s electron configuration and periodic position to its common oxidation state.
- Explain the Lewis acidity and hydrolysis of aqueous Al³⁺.
- Distinguish aluminium’s reactions with acids and bases using its amphoteric character.
- Describe how passivation and industrial processing affect aluminium’s behavior and availability.
- Identify selected aluminium compounds and their analytical, pharmaceutical, and engineering uses.
Continue your study
Work through the complete notes and reinforce the topic with the study tools available in the full lesson.
