Iron oxide or ferric oxide is the inorganic compound with the formula Fe2O3. It is one of the three main oxides of iron, the other two being iron oxide, which is rare; and iron oxide, which also occurs naturally as the mineral magnetite. As the mineral known as hematite, Fe2O3 is the main source of iron for the steel industry. Fe2O3 is readily attacked by acids. Iron oxide is often called rust, and to some extent this label is useful, because rust shares several properties and has a similar composition. To a chemist, rust is considered an ill-defined material, described as hydrated ferric oxide.
Structure
Fe2O3 can be obtained in various polymorphs. In the main ones, α and γ, iron adopts octahedral coordination geometry. That is, each Fe center is bound to six oxygen ligands.
γ-Fe2O3 has a cubic structure. It is metastable and converted from the alpha phase at high temperatures. It occurs naturally as the mineral maghemite. It is ferromagnetic and finds application in recording tapes, although ultrafine particles smaller than 10 nanometers are superparamagnetic. It can be prepared by thermal dehydratation of gamma iron oxide-hydroxide. Another method involves the careful oxidation of iron oxide. The ultrafine particles can be prepared by thermal decomposition of iron oxalate.
Other phases
Several other phases have been identified or claimed. The β-phase is cubic body-centered, metastable, and at temperatures above converts to alpha phase. It can be prepared by reduction of hematite by carbon, pyrolysis of iron chloride solution, or thermal decomposition of iron sulfate. The epsilon phase is rhombic, and shows properties intermediate between alpha and gamma, and may have useful magnetic properties. Preparation of the pure epsilon phase has proven very challenging due to contamination with alpha and gamma phases. Material with a high proportion of epsilon phase can be prepared by thermal transformation of the gamma phase. This phase is also metastable, transforming to the alpha phase at between. Can also be prepared by oxidation of iron in an electric arc or by sol-gel precipitation from iron nitrate. Additionally at high pressure an amorphous form is claimed. Recent research has revealed epsilon iron oxide in ancient Chinese Jian ceramic glazes, which may provide insight into ways to produce that form in the lab.
Hydrated iron(III) oxides
Several hydrates of Iron oxide exists. When alkali is added to solutions of soluble Fe salts, a red-brown gelatinous precipitate forms. This is not Fe3, but Fe2O3·H2O. Several forms of the hydrated oxide of Fe exist as well. The red lepidocrocite γ-FeOH, occurs on the outside of rusticles, and the orange goethite, which occurs internally in rusticles. When Fe2O3·H2O is heated, it loses its water of hydration. Further heating at 1670 K converts Fe2O3 to black Fe3O4, which is known as the mineral magnetite. FeOH is soluble in acids, giving 3+. In concentrated aqueous alkali, Fe2O3 gives 3−.
Reactions
The most important reaction is its carbothermal reduction, which gives iron used in steel-making: Another redox reaction is the extremely exothermicthermite reaction with aluminium. This process is used to weld thick metals such as rails of train tracks by using a ceramic container to funnel the molten iron in between two sections of rail. Thermite is also used in weapons and making small-scale cast-iron sculptures and tools. Partial reduction with hydrogen at about 400 °C produces magnetite, a black magnetic material that contains both Fe and Fe: Iron oxide is insoluble in water but dissolves readily in strong acid, e.g. hydrochloric and sulfuric acids. It also dissolves well in solutions of chelating agents such as EDTA and oxalic acid. Heating iron oxides with other metal oxides or carbonates yields materials known as ferrates :
Preparation
Iron oxide is a product of the oxidation of iron. It can be prepared in the laboratory by electrolyzing a solution of sodium bicarbonate, an inert electrolyte, with an iron anode: The resulting hydrated iron oxide, written here as FeO, dehydrates around 200 °C.
Uses
Iron industry
The overwhelming application of iron oxide is as the feedstock of the steel and iron industries, e.g. the production of iron, steel, and many alloys.
Polishing
A very fine powder of ferric oxide is known as "jeweler's rouge", "red rouge", or simply rouge. It is used to put the final polish on metallic jewelry and lenses, and historically as a cosmetic. Rouge cuts more slowly than some modern polishes, such as cerium oxide, but is still used in optics fabrication and by jewelers for the superior finish it can produce. When polishing gold, the rouge slightly stains the gold, which contributes to the appearance of the finished piece. Rouge is sold as a powder, paste, laced on polishing cloths, or solid bar. Other polishing compounds are also often called "rouge", even when they do not contain iron oxide. Jewelers remove the residual rouge on jewelry by use of ultrasonic cleaning. Products sold as "stropping compound" are often applied to a leather strop to assist in getting a razor edge on knives, straight razors, or any other edged tool.
Pigment
Iron oxide is also used as a pigment, under names "Pigment Brown 6", "Pigment Brown 7", and "Pigment Red 101". Some of them, e.g. Pigment Red 101 and Pigment Brown 6, are approved by the US Food and Drug Administration for use in cosmetics. Iron oxides are used as pigments in dental composites alongside titanium oxides. Hematite is the characteristic component of the Swedish paint color Falu red.
Magnetic recording
Iron oxide was the most common magnetic particle used in all types of magnetic storage and recording media, including magnetic disks and magnetic tape. Its use in computer disks was superseded by cobalt alloy, enabling thinner magnetic films with higher storage density.
Photocatalysis
α-Fe2O3 has been studied as a photoanode for solar water oxidation. However, its efficacy is limited by a short diffusion length of photo-excited charge carriers and subsequent fast recombination, requiring a large overpotential to drive the reaction. Research has been focused on improving the water oxidation performance of Fe2O3 using nanostructuring, surface functionalization, or by employing alternate crystal phases such as β-Fe2O3.
Medicine
lotion, used to treat mild itchiness, is chiefly composed of a combination of zinc oxide, acting as astringent, and about 0.5% iron oxide, the product's active ingredient, acting as antipruritic. The red color of iron oxide is also mainly responsible for the lotion's widely familiar pink color.
