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Iron (III) oxide is an amphoteric chemical compound that exhibits both acid and basic properties. It is an important element for the manufacture of various metals and is used as a pigment or a UV blocking agent in paints, plastics and rubber products. It is also used as a dental composite, calamine lotion and to polish glass, diamonds and precious metals.
The IUPAC name of ferric oxide is Fe2O3. This is an inorganic compound that consists of two iron atoms and three oxygen atoms with an oxidation state of +3. It is a colorless crystalline solid, and can be prepared by electrolyzing sodium bicarbonate solution with an iron anode.
Fe2O3 forms a polymorph with different coordination geometries, which vary in how many oxygen ligands are associated with each of the centers. Specifically, in the a polymorph, the iron centers are bound to six oxygen ligands; in the g polymorph, the centers have four oxygen ligands.
Various hydrated forms of iron(III) oxide exist, as well. For example, a red-brown gelatinous precipitate, known as Fe2O3*H2O, forms when alkali is added to solutions of soluble Fe(III) salts.
When these hydrates are heated, they lose their water of hydration and convert to black-colored iron(III) oxide, known as magnetite. Other forms of the hydrate include Fe2O3*H2O (also called ferrohydrite) and Fe3O4 (FeIIFeIII2O4), which is the mineral magnetite.
This compound is a strong oxidizing agent and can irritate the nose and throat, as well as cause inflammation of the eyes, stomach and mouth. It can be toxic if inhaled, and it may cause severe liver damage when ingestion is prolonged. It also combines with copper to form copper(II) nitrate, which is a common fire hazard.