Iron(III) oxide

This article is about a red-colored oxide of iron. For other uses, see Red Iron.
Iron(III) oxide
Names
IUPAC name
Iron(III) oxide
Other names
Ferric oxide, Hematite, Ferric iron, Red iron oxide, Rouge, Maghemite, Colcothar, Iron sesquioxide, Rust, Ochre
Identifiers
1309-37-1 YesY
ChEBI CHEBI:50819 YesY
ChemSpider 14147 N
EC Number 215-168-2
Jmol interactive 3D Image
KEGG C19424 N
PubChem 518696
RTECS number NO7400000
UNII 1K09F3G675 YesY
Properties
Fe2O3
Molar mass 159.69 g·mol−1
Appearance Red-brown solid
Odor Odorless
Density 5.242 g/cm3[1]
Melting point 1,539–1,565 °C (2,802–2,849 °F; 1,812–1,838 K)[2]
decomposes[1]
105 °C (221 °F; 378 K)
β-dihydrate, decomposes
150 °C (302 °F; 423 K)
β-monohydrate, decomposes
50 °C (122 °F; 323 K)
α-dihydrate, decomposes
92 °C (198 °F; 365 K)
α-monohydrate, decomposes[3]
Insoluble
Solubility Soluble in diluted acids,[2] sugar solution
Trihydrate slighty soluble in aq. tartaric acid, citric acid, CH3COOH[3]
Structure
Rhombohedral, hR30 (α-form)[4]
Cubic bixbyite, cI80 (β-form)
Cubic spinel (γ-form)
Orthorhombic (ε-form)[5]
R3c, No. 161 (α-form)[4]
Ia3, No. 206 (β-form)
Pna21, No. 33 (ε-form)[5]
3m (α-form)[4]
2/m 3 (β-form)
mm2 (ε-form)[5]
Octahedral (Fe3+, α-form, β-form)[4]
Thermochemistry
103.9 J/mol·K[2]
87.4 J/mol·K[2]
−824.2 kJ/mol[2]
−742.2 kJ/mol[2]
Hazards
GHS pictograms [6]
GHS signal word Warning
H315, H319, H335[6]
P261, P305+351+338[6]
Xi
R-phrases R36/37/38
S-phrases S26
NFPA 704
5 mg/m3[2] (TWA)
Lethal dose or concentration (LD, LC):
10 g/kg (rats, oral)[1]
US health exposure limits (NIOSH):
TWA 10 mg/m3[7]
TWA 5 mg/m3[7]
2500 mg/m3[7]
Related compounds
Other anions
 Iron(III) fluoride
Other cations
 Manganese(III) oxide
Cobalt(III) oxide
Related iron oxides
 Iron(II) oxide
Iron(II,III) oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YesYN ?)
Infobox references

Iron(III) 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(II) oxide (FeO), which is rare, and iron(II,III) oxide (Fe3O4), 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 ferromagnetic, dark red, and readily attacked by acids. Iron(III) 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.

Alpha phase

α-Fe2O3 has the rhombohedral, corundum (α-Al2O3) structure and is the most common form. It occurs naturally as the mineral hematite which is mined as the main ore of iron. It is antiferromagnetic below ~260 K (Morin transition temperature), and exhibits weak ferromagnetism between 260 K and the Néel temperature, 950 K.[8] It is easy to prepare using both thermal decomposition and precipitation in the liquid phase. Its magnetic properties are dependent on many factors, e.g. pressure, particle size, and magnetic field intensity.

Gamma phase

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,[9] although ultrafine particles smaller than 10 nanometers are superparamagnetic. It can be prepared by thermal dehydratation of gamma iron(III) oxide-hydroxide, careful oxidation of iron(II,III) oxide. Another method involves the careful oxidation of Fe3O4.[9] The ultrafine particles can be prepared by thermal decomposition of iron(III) oxalate.

Other phases

Several other phases have been identified or claimed. The β-phase is cubic body centered (space group Ia3), metastable, and at temperatures above 500 °C (930 °F) converts to alpha phase. It can be prepared by reduction of hematite by carbon, pyrolysis of iron(III) chloride solution, or thermal decomposition of iron(III) 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 500 and 750 °C (930 and 1,380 °F). Can also be prepared by oxidation of iron in an electric arc or by sol-gel precipitation from iron(III) nitrate. Additionally at high pressure an amorphous form is claimed.[5] Recent research has revealed epsilon iron(III) oxide in ancient Chinese Jian ceramic glazes, which may provide insight into ways to produce that form in the lab.[10]

Hydrated iron(III) oxides

Several hydrates of Iron(III) oxide exists. When alkali is added to solutions of soluble Fe(III) salts, a red-brown gelatinous precipitate forms. This is not Fe(OH)3, but Fe2O3·H2O (also written as Fe(O)OH). Several forms of the hydrated oxide of Fe(III) exist as well. The red lepidocrocite γ-Fe(O)OH, 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 (FeIIFeIII2O4), which is known as the mineral magnetite. Fe(O)OH is soluble in acids, giving [Fe(OH2)6]3+. In concentrated aqueous alkali, Fe2O3 gives [Fe(OH)6]3−.[9]

Reactions

The most important reaction is its carbothermal reduction, which gives iron used in steel-making:

Fe2O3 + 3 CO → 2 Fe + 3 CO2

Another redox reaction is the extremely exothermic thermite reaction with aluminium.[11]

2 Al + Fe2O3 → 2 Fe + Al2O3

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 gives magnetite, a black magnetic material that contains both Fe(III) and Fe(II):[12]

3 Fe2O3 + H2 → 2 Fe3O4 + H2O

Iron(III) oxide is insoluble in water but dissolves readily in strong acid, e.g. hydrochloric and sulfuric acids. It also dissolves well in solutions of the chelating agents such as EDTA and oxalic acid.

Heating iron(III) oxides with other metal oxides or carbonates yields materials known as ferrates:[12]

ZnO + Fe2O3 → Zn(FeO2)2

Preparation

Iron(III) 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:

4 Fe + 3 O2 + 2 H2O → 4 FeO(OH)

The resulting hydrated iron(III) oxide, written here as Fe(O)OH, dehydrates around 200 °C.[12][13]

2 FeO(OH) → Fe2O3 + H2O

It can also be prepared by the thermal decomposition of iron(III) hydroxide under temperature above 200 °C.

2 Fe(OH)3 → Fe2O3 + 3H2O

Uses

Iron industry

The overwhelming application of iron(III) oxide is as the feedstock of the steel and iron industries, e.g. the production of iron, steel, and many alloys.[13]

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(IV) 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 (with a wax or grease binder). 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

Two different colors at different hydrate phase (α = red, β = yellow) of iron(III) oxide hydrate[3] and they are useful as a pigment.

Iron(III) oxide is also used as a pigment, under names "Pigment Brown 6", "Pigment Brown 7", and "Pigment Red 101".[14] Some of them, e.g. Pigment Red 101 and Pigment Brown 6, are Food and Drug Administration (FDA)-approved for use in cosmetics. Iron oxides are used as pigments in dental composites alongside titanium oxides.[15]

Hematite is the characteristic component of the Swedish paint color Falu red.

Magnetic recording

Iron(III) oxide was the most common magnetic particle used in all types of magnetic storage and recording media, including magnetic disks (for data storage) and magnetic tape (used in audio and video recording as well as data storage). However, modern magnetic storage media - in particular, the hard disk drives - use more advanced thin film technology, which may consist of a stack of 15 layers or more.[16]

Photocatalyst

α-Fe2O3 has been studied as a photoanode for the water-splitting reaction for over 25 years.[17]

Medicine

A mixture of zinc oxide with about 0.5% iron(III) oxide is called calamine, which is the active ingredient of calamine lotion.

See also

References

  1. 1 2 3 4 "SDS of Iron(III) oxide" (PDF). http://www.lesker.com. England: Kurt J Lesker Company Ltd. 2012-01-05. Retrieved 2014-07-12. External link in |website= (help)
  2. 1 2 3 4 5 6 7 Lide, David R., ed. (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. ISBN 978-1-4200-9084-0.
  3. 1 2 3 Comey, Arthur Messinger; Hahn, Dorothy A. (1921-02). A Dictionary of Chemical Solubilities: Inorganic (2nd ed.). New York: The MacMillan Company. p. 433. Check date values in: |date= (help)
  4. 1 2 3 4 Ling, Yichuan; Wheeler, Damon A.; Zhang, Jin Zhong; Li, Yat (2013). Zhai, Tianyou; Yao, Jiannian, eds. One-Dimensional Nanostructures: Principles and Applications. http://www.wiley.com (Hoboken, New Jersey: John Wiley & Sons, Inc.). p. 167. ISBN 978-1-118-07191-5. External link in |website= (help)
  5. 1 2 3 4 Vujtek, Milan; Zboril, Radek; Kubinek, Roman; Mashlan, Miroslav. "Ultrafine Particles of Iron(III) Oxides by View of AFM – Novel Route for Study of Polymorphism in Nano-world" (PDF). http://atmilab.upol.cz. Czech. Retrieved 2014-07-12. External link in |website= (help)
  6. 1 2 3 Sigma-Aldrich Co., Iron(III) oxide. Retrieved on 2014-07-12.
  7. 1 2 3 "NIOSH Pocket Guide to Chemical Hazards #0344". National Institute for Occupational Safety and Health (NIOSH).
  8. ↑ Greedon, J. E. (1994). "Magnetic oxides". In King, R. Bruce. Encyclopedia of Inorganic chemistry. New York: John Wiley & Sons. ISBN 0-471-93620-0.
  9. 1 2 3 .Housecroft, Catherine E.; Sharpe, Alan G. (2008). "Chapter 22: d-block metal chemistry: the first row elements". Inorganic Chemistry, 3rd Edition. Pearson. p. 716. ISBN 978-0-13-175553-6.
  10. ↑ {{Learning from the past: Rare ε-Fe2O3 in the ancient black-glazed Jian (Tenmoku) wares Catherine Dejoie, Philippe Sciau, Weidong Li, Laure Noé, Apurva Mehta, Kai Chen, Hongjie Luo, Martin Kunz,Nobumichi Tamura & Zhi Liu Scientific Reports 4, Article number: 4941 doi:10.1038/srep04941 Received 20 February 2014 Accepted 15 April 2014 Published 13 May 2014}}
  11. ↑ Adlam; Price (1945). Higher School Certificate Inorganic Chemistry. Leslie Slater Price.
  12. 1 2 3 Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 1661.
  13. 1 2 Greenwood, N. N.; Earnshaw, A. (1997). Chemistry of the Element (2nd ed.). Oxford: Butterworth-Heinemann. ISBN 0-7506-3365-4.
  14. ↑ Paint and Surface Coatings: Theory and Practice. William Andrew Inc. ISBN 1-884207-73-1.
  15. ↑ Banerjee, Avijit (2011). Pickard's Manual of Operative Dentistry. United States: Oxford University Press Inc., New York. p. 89. ISBN 978-0-19-957915-0.
  16. ↑ S.N. Piramanayagam, J. Appl. Phys. 102, 011301 (2007).
  17. ↑ Kay, A., Cesar, I. and Gratzel, M, Journal of the American Chemical Society 2006, 128, 15714-15721

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