Iron ( III ) oxide - wikipedia 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 CAS Number 1309 - 37 - 1 3D model ( JSmol ) Interactive image ChEBI CHEBI : 50819 ChemSpider 14147 ECHA InfoCard 100.013. 790 EC Number 215 - 168 - 2 E number E172 ( ii ) ( colours ) Gmelin Reference 11092 KEGG C19424 PubChem CID 518696 RTECS number NO7400000 UNII 1K09F3G675 InChI InChI = 1S / 2Fe. 3O Key : JEIPFZHSYJVQDO - UHFFFAOYSA - N InChI = 1 / 2Fe. 3O / rFe2O3 / c3 - 1 - 4 - 2 ( 3 ) 5 - 1 Key : JEIPFZHSYJVQDO - ZVGCCQCPAC SMILES O1 ( Fe ) 2O ( Fe ) 1O2 Properties Chemical formula Fe O Molar mass 159.69 g mol Appearance Red - brown solid Odor Odorless Density 5.242 g / cm Melting point 1,539 -- 1,565 ° C ( 2,802 -- 2,849 ° F ; 1,812 -- 1,838 K ) decomposes 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 Solubility in water Insoluble Solubility Soluble in diluted acids, sugar solution Trihydrate slightly soluble in aq. tartaric acid, citric acid, CH COOH Magnetic susceptibility ( χ ) + 3586.0 10 cm / mol Structure Crystal structure Rhombohedral, hR30 ( α - form ) Cubic bixbyite, cI80 ( β - form ) Cubic spinel ( γ - form ) Orthorhombic ( ε - form ) Space group R3c, No. 161 ( α - form ) Ia 3, No. 206 ( β - form ) Pna2, No. 33 ( ε - form ) Point group 3m ( α - form ) 2 / m 3 ( β - form ) mm2 ( ε - form ) Coordination geometry Octahedral ( Fe, α - form, β - form ) Thermochemistry Specific heat capacity ( C ) 103.9 J / mol K Std molar entropy ( S ) 87.4 J / mol K Std enthalpy of formation ( Δ H ) − 824.2 kJ / mol Gibbs free energy ( Δ G  ̊ ) − 742.2 kJ / mol Hazards GHS pictograms GHS signal word Warning GHS hazard statements H315, H319, H335 GHS precautionary statements P261, P305 + 351 + 338 NFPA 704 0 0 OX Threshold limit value 5 mg / m ( TWA ) Lethal dose or concentration ( LD, LC ) : LD ( median dose ) 10 g / kg ( rats, oral ) US health exposure limits ( NIOSH ) : PEL ( Permissible ) TWA 10 mg / m REL ( Recommended ) TWA 5 mg / m IDLH ( Immediate danger ) 2500 mg / m 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 ? ) Infobox references Iron ( III ) oxide or ferric oxide is the inorganic compound with the formula Fe O. 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 ( Fe O ), which also occurs naturally as the mineral magnetite. As the mineral known as hematite, Fe O is the main source of iron for the steel industry. Fe O is ferromagnetic, dark red, and readily attacked by acids. Iron ( III ) oxide is often called rust, and is acidic in nature 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. Contents 1 Structure 1.1 Alpha phase 1.2 Gamma phase 1.3 Other phases 2 Hydrated iron ( III ) oxides 3 Reactions 4 Preparation 5 Uses 5.1 Iron industry 5.2 Polishing 5.3 Pigment 5.4 Magnetic recording 5.5 Photocatalysis 5.6 Medicine 6 See also 7 References 8 External links Structure Fe O 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 - Fe O has the rhombohedral, corundum ( α - Al O ) 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. 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 - Fe O 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 ( III ) oxide - hydroxide. Another method involves the careful oxidation of iron ( II, III ) oxide ( Fe O ). 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. 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. 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 ), but Fe O H O ( 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 Fe O H O is heated, it loses its water of hydration. Further heating at 1670 K converts Fe O to black Fe O ( Fe Fe O ), which is known as the mineral magnetite. Fe ( O ) OH is soluble in acids, giving ( Fe ( OH ) ). In concentrated aqueous alkali, Fe O gives ( Fe ( OH ) ). Reactions The most important reaction is its carbothermal reduction, which gives iron used in steel - making : Fe O + 3 CO → 2 Fe + 3 CO Another redox reaction is the extremely exothermic thermite reaction with aluminium. 2 Al + Fe O → 2 Fe + Al O 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 ( III ) and Fe ( II ) : 3 Fe O + H → 2 Fe O + H O 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 chelating agents such as EDTA and oxalic acid. Heating iron ( III ) oxides with other metal oxides or carbonates yields materials known as ferrates : ZnO + Fe O → Zn ( FeO ) 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 O + 2 H O → 4 FeO ( OH ) The resulting hydrated iron ( III ) oxide, written here as Fe ( O ) OH, dehydrates around 200 ° C. 2 FeO ( OH ) → Fe O + H O 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. 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 ; they are useful as pigments. Iron ( III ) 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 ( FDA ) 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 ( 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 ). Its use in computer disks was superseded by cobalt alloy, enabling thinner magnetic films with higher storage density. Photocatalysis Because its acidic in nature ( 1.9 - 2.2 eV ) lies in an intense region of the solar spectrum, α - Fe O has been studied as a photoanode for solar water oxidation. However, its efficacy is limited by a short diffusion length ( 2 - 4 nm ) 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 Fe O using nanostructuring, surface functionalization, or by employing alternate crystal phases such as β - Fe O. 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 Iron oxides Chalcanthum References ^ Jump up to : `` SDS of Iron ( III ) oxide '' ( PDF ). KJLC. England : Kurt J Lesker Company Ltd. 2012 - 01 - 05. Retrieved 2014 - 07 - 12. ^ Jump up to : Lide, David R., ed. ( 2009 ). CRC Handbook of Chemistry and Physics ( 90th ed. ). Boca Raton, Florida : CRC Press. ISBN 978 - 1 - 4200 - 9084 - 0. ^ Jump up to : Comey, Arthur Messinger ; Hahn, Dorothy A. ( February 1921 ). A Dictionary of Chemical Solubilities : Inorganic ( 2nd ed. ). New York : The MacMillan Company. p. 433. ^ Jump up to : Ling, Yichuan ; Wheeler, Damon A. ; Zhang, Jin Zhong ; Li, Yat ( 2013 ). Zhai, Tianyou ; Yao, Jiannian, eds. One - Dimensional Nanostructures : Principles and Applications. John Wiley & Sons, Inc. Hoboken, New Jersey : John Wiley & Sons, Inc. p. 167. ISBN 978 - 1 - 118 - 07191 - 5. ^ Jump up to : 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 ). Univerzity Palackého. Czech. Retrieved 2014 - 07 - 12. ^ Jump up to : Sigma - Aldrich Co., Iron ( III ) oxide. Retrieved on 2014 - 07 - 12. ^ Jump up to : `` NIOSH Pocket Guide to Chemical Hazards # 0344 ''. National Institute for Occupational Safety and Health ( NIOSH ). Jump up ^ Greedon, J.E. ( 1994 ). `` Magnetic oxides ''. In King, R. Bruce. Encyclopedia of Inorganic chemistry. New York : John Wiley & Sons. ISBN 0 - 471 - 93620 - 0. ^ Jump up to :. Housecroft, Catherine E. ; Sharpe, Alan G. ( 2008 ). `` Chapter 22 : d - block metal chemistry : the first row elements ''. Inorganic Chemistry ( 3rd ed. ). Pearson. p. 716. ISBN 978 - 0 - 13 - 175553 - 6. Jump up ^ ( ( 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 ) ) Jump up ^ Adlam ; Price ( 1945 ). Higher School Certificate Inorganic Chemistry. Leslie Slater Price. ^ Jump up to : Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 1661. ^ Jump up to : Greenwood, N.N. ; Earnshaw, A. ( 1997 ). Chemistry of the Element ( 2nd ed. ). Oxford : Butterworth - Heinemann. ISBN 0 - 7506 - 3365 - 4. Jump up ^ Paint and Surface Coatings : Theory and Practice. William Andrew Inc. ISBN 1 - 884207 - 73 - 1. Jump up ^ 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. Jump up ^ S.N. Piramanayagam, J. Appl. Phys. 102, 011301 ( 2007 ). ^ Jump up to : Kay, A., Cesar, I. and Grätzel, M., J. Am. Chem. Soc. 2006, 128, 15714 - 15721 Jump up ^ Kennedy, J.H. and Frese, K.W., J. Electrochem. Soc. 1978, 125, 709 - 714 Jump up ^ Le Formal, F. et al., J. Am. Chem. Soc. 2014, 136, 2564 - 2574 Jump up ^ Zhong, D.K. and Gamelin, D.R., J. Am. Chem. Soc. 2010, 132, 4202 - 4207 Jump up ^ Emery, J.D. et al., ACS Appl. Mater. Interfaces 2014, 6, 21894 - 21900 External links Wikimedia Commons has media related to Iron ( III ) oxide. NIOSH Pocket Guide to Chemical Hazards Iron compounds Fe ( - II ) Na Fe ( CO ) Fe ( 0 ) Fe ( CO ) Fe ( CO ) Fe ( CO ) Fe ( CO ) CH COC H C H Fe ( I ) FeH Organoiron ( I ) compounds ( C H FeCO ) ( CO ) Fe ( 0, II ) Fe C Fe ( II ) FeBr FeCl FeF FeI FeH FeMoO FeO Fe ( OH ) FeS FeSO FeSe FeSeO FeSi FeTiO FeCO FeC O Fe ( C H O ) Fe ( C H O ) FeC H O FeC H O Fe CrO Fe ( PO ) FeH ( CO ) Fe ( HCO ) Mg FeH Organoiron ( II ) compounds Fe ( C H ) Fe ( C H P ( C H ) ) C H Fe ( CO ) Fe ( 0, III ) Fe P Fe ( II, III ) Fe O Fe S Fe ( III ) FeBr FeCl FeF FeI Fe ( NO ) FeOCl FeO ( OH ) FePO Fe ( P O ) Fe ( CrO ) Fe ( C O ) Fe O Fe S Fe ( SO ) FeBO FeB Organoiron ( III ) compounds Fe ( C H ) BF C H O ⋅ xFe ⋅ yNH Fe ( VI ) K FeO BaFeO Oxides Mixed oxidation states Antimony tetroxide ( Sb O ) Cobalt ( II, III ) oxide ( Co O ) Europium ( II, III ) oxide ( Eu O ) Iron ( II, III ) oxide ( Fe O ) Lead ( II, IV ) oxide ( Pb O ) Manganese ( II, III ) oxide ( Mn O ) Silver ( I, III ) oxide ( Ag O ) Triuranium octoxide ( U O ) Carbon suboxide ( C O ) Mellitic anhydride ( C O ) Praseodymium ( III, IV ) oxide ( Pr O ) Terbium ( III, IV ) oxide ( Tb O ) + 1 oxidation state Copper ( I ) oxide ( Cu O ) Dicarbon monoxide ( C O ) Dichlorine monoxide ( Cl O ) Gallium ( I ) oxide ( Ga O ) Lithium oxide ( Li O ) Potassium oxide ( K O ) Rubidium oxide ( Rb O ) Silver oxide ( Ag O ) Thallium ( I ) oxide ( Tl O ) Sodium oxide ( Na O ) Water ( hydrogen oxide ) ( H O ) + 2 oxidation state Aluminium ( II ) oxide ( Al O ) Barium oxide ( Ba O ) Beryllium oxide ( Be O ) Cadmium oxide ( Cd O ) Calcium oxide ( Ca O ) Carbon monoxide ( CO ) Chromium ( II ) oxide ( Cr O ) Cobalt ( II ) oxide ( Co O ) Copper ( II ) oxide ( Cu O ) Europium ( II ) oxide ( Eu O ) Germanium monoxide ( Ge O ) ) Iron ( II ) oxide ( Fe O ) Lead ( II ) oxide ( Pb O ) Magnesium oxide ( Mg O ) Manganese ( II ) oxide ( Mn O ) Mercury ( II ) oxide ( Hg O ) Nickel ( II ) oxide ( Ni O ) Nitric oxide ( N O ) Palladium ( II ) oxide ( Pd O ) Silicon monoxide ( Si O ) Strontium oxide ( Sr O ) Sulfur monoxide ( S O ) Disulfur dioxide ( S O ) Tin ( II ) oxide ( Sn O ) Titanium ( II ) oxide ( Ti O ) Vanadium ( II ) oxide ( V O ) Zinc oxide ( Zn O ) + 3 oxidation state Aluminium oxide ( Al O ) Antimony trioxide ( Sb O ) Arsenic trioxide ( As O ) Bismuth ( III ) oxide ( Bi O ) Boron trioxide ( B O ) Cerium ( III ) oxide ( Ce O ) Dibromine trioxide ( Br O ) Chromium ( III ) oxide ( Cr O ) Dinitrogen trioxide ( N O ) Dysprosium ( III ) oxide ( Dy O ) Erbium ( III ) oxide ( Er O ) Europium ( III ) oxide ( Eu O ) Gadolinium ( III ) oxide ( Gd O ) Gallium ( III ) oxide ( Ga O ) Holmium ( III ) oxide ( Ho O ) Indium ( III ) oxide ( In O ) Iron ( III ) oxide ( Fe O ) Lanthanum oxide ( La O ) Lutetium ( III ) oxide ( Lu O ) Manganese ( III ) oxide ( Mn O ) Neodymium ( III ) oxide ( Nd O ) Nickel ( III ) oxide ( Ni O ) Phosphorus trioxide ( P O ) Praseodymium ( III ) oxide ( Pr O ) Promethium ( III ) oxide ( Pm O ) Rhodium ( III ) oxide ( Rh O ) Samarium ( III ) oxide ( Sm O ) Scandium oxide ( Sc O ) Terbium ( III ) oxide ( Tb O ) Thallium ( III ) oxide ( Tl O ) Thulium ( III ) oxide ( Tm O ) Titanium ( III ) oxide ( Ti O ) Tungsten ( III ) oxide ( W O ) Vanadium ( III ) oxide ( V O ) Ytterbium ( III ) oxide ( Yb O ) Yttrium ( III ) oxide ( Y O ) + 4 oxidation state Americium dioxide ( Am O ) Carbon dioxide ( C O ) Carbon trioxide ( C O ) Cerium ( IV ) oxide ( Ce O ) Chlorine dioxide ( Cl O ) Chromium ( IV ) oxide ( Cr O ) Dinitrogen tetroxide ( N O ) Germanium dioxide ( Ge O ) Hafnium ( IV ) oxide ( Hf O ) Lead dioxide ( Pb O ) Manganese dioxide ( Mn O ) Neptunium ( IV ) oxide ( Np O ) Nitrogen dioxide ( N O ) Osmium dioxide ( Os O ) Plutonium ( IV ) oxide ( Pu O ) Praseodymium ( IV ) oxide ( Pr O ) Protactinium ( IV ) oxide ( Pa O ) Rhodium ( IV ) oxide ( Rh O ) Ruthenium ( IV ) oxide ( Ru O ) Selenium dioxide ( Se O ) Silicon dioxide ( Si O ) Sulfur dioxide ( S O ) Tellurium dioxide ( Te O ) Terbium ( IV ) oxide ( Tb O ) Thorium dioxide ( Th O ) Tin dioxide ( Sn O ) Titanium dioxide ( Ti O ) Tungsten ( IV ) oxide ( W O ) Uranium dioxide ( U O ) Vanadium ( IV ) oxide ( V O ) Zirconium dioxide ( Zr O ) + 5 oxidation state Antimony pentoxide ( Sb O ) Arsenic pentoxide ( As O ) Dinitrogen pentoxide ( N O ) Niobium pentoxide ( Nb O ) Phosphorus pentoxide ( P O ) Protactinium ( V ) oxide ( Pa O ) Tantalum pentoxide ( Ta O ) Vanadium ( V ) oxide ( V O ) + 6 oxidation state Chromium trioxide ( Cr O ) Molybdenum trioxide ( Mo O ) Rhenium trioxide ( Re O ) Selenium trioxide ( Se O ) Sulfur trioxide ( S O ) Tellurium trioxide ( Te O ) Tungsten trioxide ( W O ) Uranium trioxide ( U O ) Xenon trioxide ( Xe O ) Iridium trioxide ( Ir O ) + 7 oxidation state Dichlorine heptoxide ( Cl O ) Manganese heptoxide ( Mn O ) Rhenium ( VII ) oxide ( Re O ) Technetium ( VII ) oxide ( Tc O ) + 8 oxidation state Osmium tetroxide ( Os O ) Ruthenium tetroxide ( Ru O ) Xenon tetroxide ( Xe O ) Iridium tetroxide ( Ir O ) Hassium tetroxide ( Hs O ) Related Oxocarbon Suboxide Oxyanion Ozonide Peroxide Superoxide Oxides are sorted by oxidation state. Category : Oxides Metabolism : Metal metabolism Transition metal Iron metabolism Absorption in Duodenum Iron ( II ) oxide : DMT1 ( SLC11A2 ) Ferritin Hephaestin / Ferroportin ( SLC11A3 / SLC40A1 ) Transferrin to Transferrin receptor TFR1 TFR2 Iron ( III ) oxide : Duodenal cytochrome B Integrin Calreticulin / mobilferrin Ferritin Other Iron - binding proteins : Ferritin Hepcidin / HAMP Hemojuvelin Iron - responsive element - binding protein Aconitase Ceruloplasmin HFE Hemosiderin Lactoferrin Copper metabolism ATP7A ATP7B Ceruloplasmin SLC31A1 ATOX1 Zinc metabolism TMC6 TMC8 SLC30A1 SLC39A4 Electrolyte Sodium metabolism Na / K - ATPase Phosphate metabolism Phosphoric acids and phosphates Magnesium metabolism Magnesium transporter Calcium metabolism Calcium - sensing receptor Calcium - binding protein Retrieved from `` https://en.wikipedia.org/w/index.php?title=Iron(III)_oxide&oldid=834360333 '' Categories : Iron compounds Oxides Iron oxide pigments Sesquioxides Hidden categories : Articles with changed ChemSpider identifier ECHA InfoCard ID from Wikidata E number from Wikidata Articles with changed KEGG identifier Chembox having GHS data Articles containing unverified chemical infoboxes All articles with unsourced statements Articles with unsourced statements from July 2017 Articles with unsourced statements from November 2016 Articles with unsourced statements from July 2011 Use dmy dates from July 2011 Talk Contents About Wikipedia Asturianu تۆرکجه Català Čeština Deutsch Eesti Español فارسی Français 한국어 Hrvatski Ido Bahasa Indonesia Italiano Magyar Bahasa Melayu Nederlands 日本 語 Norsk Polski Português Română Русский සිංහල Simple English Slovenčina Slovenščina Српски / srpski Srpskohrvatski / српскохрватски Suomi Svenska Українська Tiếng Việt 中文 26 more Edit links This page was last edited on 5 April 2018, at 09 : 25. 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Question: is iron iii oxide a solid liquid or gas
Answer: mineral