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{{chembox |
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| ImageFile = Magnetite.jpg |
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| verifiedrevid = 447334989 |
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| Name = |
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| IUPACName = iron(II) diiron(III) oxide |
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| ImageFile = Fe3O4.JPG |
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| OtherNames = ferrous ferric oxide, ferroso ferric oxide, iron(II,III) oxide, magnetite, black iron oxide, lodestone, rust |
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| ImageFile2 = |
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| Section1 = {{Chembox Identifiers |
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| IUPACName = iron(II) diiron(III) oxide<ref>{{nist |name=Iron(ii) diiron(iii) oxide |id=B8022203 |accessdate=2024-12-22}}</ref> |
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| OtherNames = ferrous ferric oxide, ferrosoferric oxide, iron(II,III) oxide, magnetite, black iron oxide, lodestone, rust |
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| SystematicName = |
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| Section1 = {{Chembox Identifiers |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 17215625 |
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| ChemSpiderID = 17215625 |
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| ChEBI_Ref = {{ebicite|correct|EBI}} |
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| ChEBI_Ref = {{ebicite|correct|EBI}} |
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| ChEBI = 50821 |
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| ChEBI = 50821 |
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| ChEMBL_Ref = {{ebicite|changed|EBI}} |
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| ChEMBL = 1201867 |
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| SMILES = O12OO1O2 |
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| SMILES = O12OO1O2 |
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| Section2 = {{Chembox Properties |
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| caption = Magnetite and pyrite from Piedmont Italy |
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| Formula = Fe<sub>3</sub>O<sub>4</sub><br /> |
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| Section2 = {{Chembox Properties |
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| Formula = Fe<sub>3</sub>O<sub>4</sub><br/> |
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FeO.Fe<sub>2</sub>O<sub>3</sub> |
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FeO.Fe<sub>2</sub>O<sub>3</sub> |
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| MolarMass = 231.533 g/mol |
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| MolarMass = 231.533 g/mol |
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| Appearance = black powder |
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| Appearance = solid black powder |
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| Density = 5.17 g/cm<sup>3</sup> |
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| Density = 5 g/cm<sup>3</sup> |
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| MeltingPt = 1597 °C |
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| MeltingPtC = 1597 |
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| BoilingPtC = 2623<ref> {{Webarchive|url=https://web.archive.org/web/20170720012739/http://preserve.lehigh.edu/cgi/viewcontent.cgi?article=1002&context=cas-lehighreview-vol-15 |date=2017-07-20 }} Lee Blaney, Lehigh Review 15, 33-81 (2007). See Appendix A, p.77</ref> |
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| BoilingPt = |
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| Solubility = |
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| Solubility = |
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| RefractIndex = 2.42 <ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN 0070494398</ref> |
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| RefractIndex = 2.42<ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, {{ISBN|0-07-049439-8}}</ref> |
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| Section3 = {{Chembox Hazards |
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| Section3 = {{Chembox Hazards |
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| FlashPt = |
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| FlashPt = |
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| Autoignition = |
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| AutoignitionPt = |
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| NFPA-H = 0 |
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| NFPA-F = 0 |
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| NFPA-R = 1 |
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| NFPA-S = OX |
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|Section4={{Chembox Thermochemistry |
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| DeltaHf = -1120.89 kJ·mol<sup>−1</sup><ref>{{Cite journal|url=https://webbook.nist.gov/cgi/cbook.cgi?ID=C1309382&Units=SI&Mask=2|title=NIST-JANAF Themochemical Tables | edition = Fourth |year=1998|pages=1–1951| vauthors = Chase MW |journal=NIST }}</ref> |
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| Section5 = |
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'''Iron(II,III) oxide''' is the chemical compound with formula Fe<sub>3</sub>O<sub>4</sub>. It is one of a number of ]. It occurs in nature as the mineral ]. It contains both Fe<sup>2+</sup> and Fe<sup>3+</sup> ions and is sometimes formulated as FeO ∙ Fe<sub>2</sub>O<sub>3</sub>. This iron oxide is encountered in the laboratory as a black powder. It exhibits permanent magnetism and is ], but is sometimes incorrectly described as ].<ref name = "Greenwood">{{Greenwood&Earnshaw}}</ref> Its most extensive use is as a black pigment which is synthesised rather than being extracted from the naturally occurring mineral as the particle size and shape can be varied by the method of production.<ref name = "Cornell">Rochelle M. Cornell, Udo Schwertmann 2007 ''The Iron Oxides: Structure, Properties, Reactions, Occurrences and Uses'' Wiley-VCH ISBN 3527606440</ref> |
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| Section6 = |
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}} |
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'''Iron(II,III) oxide''', or black iron oxide, is the chemical compound with formula Fe<sub>3</sub>O<sub>4</sub>. It occurs in nature as the mineral ]. It is one of a number of ], the others being ] (FeO), which is rare, and ] (Fe<sub>2</sub>O<sub>3</sub>) which also occurs naturally as the mineral ]. It contains both Fe<sup>2+</sup> and Fe<sup>3+</sup> ions and is sometimes formulated as FeO ∙ Fe<sub>2</sub>O<sub>3</sub>. This iron oxide is encountered in the laboratory as a black powder. It exhibits permanent magnetism and is ], but is sometimes incorrectly described as ].<ref name = "Greenwood">{{Greenwood&Earnshaw|name-list-style = vanc }}</ref> Its most extensive use is as a black pigment (see: ]). For this purpose, it is synthesized rather than being extracted from the naturally occurring mineral as the particle size and shape can be varied by the method of production.<ref name = "Cornell">{{cite book | vauthors = Cornell RM, Schwertmann U | date = 2007 | title = The Iron Oxides: Structure, Properties, Reactions, Occurrences and Uses | publisher = Wiley-VCH | isbn = 978-3-527-60644-3 }}</ref> |
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==Preparation== |
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==Preparation== |
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Heated iron metal interacts with steam to form iron oxide and hydrogen gas. |
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Pigment quality Fe<sub>3</sub>O<sub>4</sub>, so called synthetic magnetite, can be prepared using processes that utilise industrial wastes, scrap iron or solutions containing iron salts (e.g. those produced as by-products in industrial processes such as the acid vat treatment (]) of steel): |
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:<chem>3Fe + 4H2O->Fe3O4 + 4H2 </chem> |
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Under ] conditions, ] (Fe(OH)<sub>2</sub>) can be oxidized by water to form magnetite and molecular ]. This process is described by the ]: |
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:<chem>\underset{ferrous\ hydroxide}{3Fe(OH)2} -> \underset{magnetite}{Fe3O4} + \underset{hydrogen}{H2} + \underset{water}{2H2O}</chem> |
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This works because crystalline magnetite (Fe<sub>3</sub>O<sub>4</sub>) is thermodynamically more stable than amorphous ferrous hydroxide (Fe(OH)<sub>2</sub> ).<ref>{{cite journal | vauthors = Ma M, Zhang Y, Guo Z, Gu N | title = Facile synthesis of ultrathin magnetic iron oxide nanoplates by Schikorr reaction | journal = Nanoscale Research Letters | volume = 8 | issue = 1 | pages = 16 | date = January 2013 | pmid = 23294626 | pmc = 3598988 | doi = 10.1186/1556-276X-8-16 | bibcode = 2013NRL.....8...16M | doi-access = free }}</ref> |
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The ] of preparation of magnetite as a ], is convenient in the laboratory: mix ] and ] in the presence of ].<ref>{{cite journal| vauthors = Massart R |title=Preparation of aqueous magnetic liquids in alkaline and acidic media|journal=IEEE Transactions on Magnetics|date=1981|volume=17|issue=2|pages=1247–1248|doi=10.1109/TMAG.1981.1061188|bibcode=1981ITM....17.1247M}}</ref> |
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A more efficient method of preparing magnetite without troublesome residues of sodium, is to use ammonia to promote chemical co-precipitation from the iron chlorides: first mix solutions of 0.1 M FeCl<sub>3</sub>·6H<sub>2</sub>O and FeCl<sub>2</sub>·4H<sub>2</sub>O with vigorous stirring at about 2000 rpm. The molar ratio of the FeCl<sub>3</sub>:FeCl<sub>2</sub> should be about 2:1. Heat the mix to 70 °C, then raise the speed of stirring to about 7500 rpm and quickly add a solution of NH<sub>4</sub>OH (10 volume %). A dark precipitate of nanoparticles of magnetite forms immediately.<ref>{{cite journal| vauthors = Keshavarz S, Xu Y, Hrdy S, Lemley C, Mewes T, Bao Y |title=Relaxation of Polymer Coated Fe<sub>3</sub>O<sub>4</sub> Magnetic Nanoparticles in Aqueous Solution|journal=IEEE Transactions on Magnetics|date=2010|volume=46|issue=6|pages=1541–1543|doi=10.1109/TMAG.2010.2040588|s2cid=35129018}}</ref> |
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In both methods, the precipitation reaction relies on rapid transformation of acidic iron ions into the spinel iron oxide structure at pH 10 or higher. |
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Controlling the formation of magnetite nanoparticles presents challenges: the reactions and phase transformations necessary for the creation of the magnetite spinel structure are complex.<ref>{{cite journal | vauthors = Jolivet JP, Chanéac C, Tronc E | title = Iron oxide chemistry. From molecular clusters to extended solid networks | journal = Chemical Communications | issue = 5 | pages = 481–7 | date = March 2004 | pmid = 14973569 | doi = 10.1039/B304532N }}</ref> The subject is of practical importance because magnetite particles are of interest in bioscience applications such as ] (MRI), in which iron oxide magnetite nanoparticles potentially present a non-toxic alternative to the gadolinium-based ] currently in use. However, difficulties in controlling the formation of the particles, still frustrate the preparation of superparamagnetic magnetite particles, that is to say: magnetite nanoparticles with a coercivity of 0 A/m, meaning that they completely lose their permanent magnetisation in the absence of an external magnetic field. The smallest values currently reported for nanosized magnetite particles is ''Hc'' = 8.5 A m<sup>−1</sup>,<ref>{{cite journal| vauthors = Ström V, Olsson RT, Rao KV |title=Real-time monitoring of the evolution of magnetism during precipitation of superparamagnetic nanoparticles for bioscience applications|journal=Journal of Materials Chemistry|date=2010|volume=20|issue=20|pages=4168|doi=10.1039/C0JM00043D}}</ref> whereas the largest reported magnetization value is 87 Am<sup>2</sup> kg<sup>−1</sup> for synthetic magnetite.<ref>{{cite journal| vauthors = Fang M, Ström V, Olsson RT, Belova L, Rao KV |title=Rapid mixing: A route to synthesize magnetite nanoparticles with high moment|journal=Applied Physics Letters |date=2011 |volume=99 |issue=22 |pages=222501 |doi=10.1063/1.3662965 |bibcode=2011ApPhL..99v2501F }}</ref><ref>{{cite journal | vauthors = Fang M, Ström V, Olsson RT, Belova L, Rao KV | title = Particle size and magnetic properties dependence on growth temperature for rapid mixed co-precipitated magnetite nanoparticles | journal = Nanotechnology | volume = 23 | issue = 14 | pages = 145601 | date = April 2012 | pmid = 22433909 | doi = 10.1088/0957-4484/23/14/145601 | bibcode = 2012Nanot..23n5601F | s2cid = 34153665 }}</ref> |
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Pigment quality Fe<sub>3</sub>O<sub>4</sub>, so called synthetic magnetite, can be prepared using processes that use industrial wastes, scrap iron or solutions containing iron salts (e.g. those produced as by-products in industrial processes such as the acid vat treatment (]) of steel): |
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*Oxidation of Fe metal in the Laux process where ] is reacted with iron metal using FeCl<sub>2</sub> as a catalyst to produce ]<ref name = "Cornell"/> : |
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*Oxidation of Fe metal in the Laux process where ] is treated with iron metal using FeCl<sub>2</sub> as a catalyst to produce ]:<ref name = "Cornell"/> |
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:C<sub>6</sub>H<sub>5</sub>NO<sub>2</sub> + 3 Fe + 2 H<sub>2</sub>O → C<sub>6</sub>H<sub>5</sub>NH<sub>2</sub> + Fe<sub>3</sub>O<sub>4</sub> |
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:C<sub>6</sub>H<sub>5</sub>NO<sub>2</sub> + 3 Fe + 2 H<sub>2</sub>O → C<sub>6</sub>H<sub>5</sub>NH<sub>2</sub> + Fe<sub>3</sub>O<sub>4</sub> |
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*Oxidation of Fe<sup>II</sup> compounds, e.g. the precipitation of iron(II) salts as hydroxides followed by oxidation by aeration where careful control of the pH determines the oxide produced.<ref name = "Cornell"/> |
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*Oxidation of Fe<sup>II</sup> compounds, e.g. the precipitation of iron(II) salts as hydroxides followed by oxidation by aeration where careful control of the pH determines the oxide produced.<ref name = "Cornell"/> |
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Reduction of Fe<sub>2</sub>O<sub>3</sub> with hydrogen:<ref>US patent 2596954, 1947, Process for reduction of iron ore to magnetiteHeath T.D.</ref><ref>{{cite journal | title = Kinetics of reduction of iron oxides by H2 Part I: Low temperature reduction of hematite | author = A. Pineau, N. Kanari, I. Gaballah | journal = ] | volume = 447 | issue = 1 | pages = 89–100 | year = 2006 | doi=10.1016/j.tca.2005.10.004}}</ref> |
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Reduction of Fe<sub>2</sub>O<sub>3</sub> with hydrogen:<ref>{{cite patent | country = US | number = 2596954 | gdate = 13 May 1952 | title = Process for reduction of iron ore to magnetite | inventor = Heath TD | assign1 = Dorr Company }}</ref><ref>{{cite journal | title = Kinetics of reduction of iron oxides by H2 Part I: Low temperature reduction of hematite | vauthors = Pineau A, Kanari N, Gaballah I | journal = Thermochimica Acta | volume = 447 | issue = 1 | pages = 89–100 | year = 2006 | doi=10.1016/j.tca.2005.10.004}}</ref> |
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:3Fe<sub>2</sub>O<sub>3</sub> + H<sub>2</sub> → 2Fe<sub>3</sub>O<sub>4</sub> +H<sub>2</sub>O |
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:3Fe<sub>2</sub>O<sub>3</sub> + H<sub>2</sub> → 2Fe<sub>3</sub>O<sub>4</sub> +H<sub>2</sub>O |
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Reduction of Fe<sub>2</sub>O<sub>3</sub> with CO:<ref>{{cite journal | title = The effects of nucleation and growth on the reduction of Fe<sub>2</sub>O<sub>3</sub> to Fe<sub>3</sub>O<sub>4</sub> | author = Hayes P. C., Grieveson P. | journal = ] B | year = 1981 | volume = 12 | issue = 2 | pages = 319–326 | doi = 10.1007/BF02654465}}</ref> |
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Reduction of Fe<sub>2</sub>O<sub>3</sub> with CO:<ref>{{cite journal | title = The effects of nucleation and growth on the reduction of Fe<sub>2</sub>O<sub>3</sub> to Fe<sub>3</sub>O<sub>4</sub> | vauthors = Hayes PC, Grieveson P | journal = Metallurgical and Materials Transactions B | year = 1981 | volume = 12 | issue = 2 | pages = 319–326 | doi = 10.1007/BF02654465|bibcode=1981MTB....12..319H |s2cid=94274056 }}</ref> |
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:3Fe<sub>2</sub>O<sub>3</sub> + CO → 2Fe<sub>3</sub>O<sub>4</sub> + CO<sub>2</sub> |
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:3Fe<sub>2</sub>O<sub>3</sub> + CO → 2Fe<sub>3</sub>O<sub>4</sub> + CO<sub>2</sub> |
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Production of nano-particles can be performed chemically by taking for example mixtures of Fe<sup>II</sup> and Fe<sup>III</sup> salts and mixing them with alkali to precipitate colloidal Fe<sub>3</sub>O<sub>4</sub>. The reaction conditions are critical to the process and determine the particle size.<ref>Arthur T. Hubbard (2002) ''Encyclopedia of Surface and Colloid Science'' CRC Press, ISBN 0824707966</ref> |
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Production of nano-particles can be performed chemically by taking for example mixtures of Fe<sup>II</sup> and Fe<sup>III</sup> salts and mixing them with alkali to precipitate colloidal Fe<sub>3</sub>O<sub>4</sub>. The reaction conditions are critical to the process and determine the particle size.<ref>Arthur T. Hubbard (2002) ''Encyclopedia of Surface and Colloid Science'' CRC Press, {{ISBN|0-8247-0796-6}}</ref> |
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] can also be thermally decomposed into Iron(II,III):<ref>{{Cite web |title=FeCO3 = Fe3O4 + CO2 + CO {{!}} The thermal decomposition of iron(II) carbonate |url=https://chemiday.com/en/reaction/3-1-0-5222 |access-date=2022-10-14 |website=chemiday.com}}</ref> |
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: {{Chem2|3FeCO3 → Fe3O4 + 2CO2 + CO}} |
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==Reactions== |
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==Reactions== |
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Reduction of magnetite ore by ] in a ] is used to produce iron as part of steel production process:<ref name = "Greenwood"/> |
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Reduction of magnetite ore by ] in a ] is used to produce iron as part of steel production process:<ref name = "Greenwood"/> |
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:Fe<sub>3</sub>O<sub>4</sub> + 4CO → 3Fe + 4CO<sub>2</sub> |
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:<chem>{Fe3O4} + 4CO -> {3Fe} + 4CO2</chem> |
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Controlled oxidation of Fe<sub>3</sub>O<sub>4</sub> is used to produce brown pigment quality ] (]):<ref name = "Buxbaum">Gunter Buxbaum, Gerhard Pfaff (2005) ''Industrial Inorganic Pigments'' 3d edition Wiley-VCH {{ISBN|3-527-30363-4}}</ref> |
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:<math chem>\ce{\underbrace{2Fe3O4}_{magnetite} + {1/2O2} ->}\ {\color{Brown}\ce{\underbrace{3(\gamma-Fe2O3)}_{maghemite}}}</math> |
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More vigorous calcining (roasting in air) gives red pigment quality ] (]):<ref name = "Buxbaum"/> |
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:<math chem>\ce{\underbrace{2Fe3O4}_{magnetite} + {1/2O2} ->}\ {\color{BrickRed}\ce{\underbrace{3(\alpha-Fe2O3)}_{hematite}}}</math> |
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== Structure == |
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Controlled oxidation of Fe<sub>3</sub>O<sub>4</sub> is used to produce brown pigment quality ] (]):<ref name = "Buxbaum">Gunter Buxbaum, Gerhard Pfaff (2005) ''Industrial Inorganic Pigments'' 3d edition Wiley-VCH ISBN 3527303634</ref> |
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Fe<sub>3</sub>O<sub>4</sub> has a cubic inverse ] structure which consists of a cubic close packed array of oxide ions where all of the Fe<sup>2+</sup> ions occupy half of the octahedral sites and the Fe<sup>3+</sup> are split evenly across the remaining octahedral sites and the tetrahedral sites. |
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Both ] and ] have a similar cubic close packed array of oxide ions and this accounts for the ready interchangeability between the three compounds on oxidation and reduction as these reactions entail a relatively small change to the overall structure.<ref name="Greenwood"/> Fe<sub>3</sub>O<sub>4</sub> samples can be ].<ref name="Greenwood"/> |
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:2Fe<sub>3</sub>O<sub>4</sub> + ½ O<sub>2</sub> → 3(γ-Fe<sub>2</sub>O<sub>3</sub>) |
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More vigorous calcining, (roasting in air), gives red pigment quality ] (]):<ref name = "Buxbaum"/> |
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:2Fe<sub>3</sub>O<sub>4</sub> + ½ O<sub>2</sub> → 3(α-Fe<sub>2</sub>O<sub>3</sub>) |
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==Structure== |
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Fe<sub>3</sub>O<sub>4</sub> has a cubic inverse ] structure which consists of a cubic close packed array of oxide ions where all of the Fe<sup>2+</sup> ions occupy half of the octahedral sites and the Fe<sup>3+</sup> are split evenly across the remaining octahedral sites and the tetrahedral sites. |
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Both ] and ] have a similar cubic close packed array of oxide ions and this accounts for the ready interchangeability between the three compounds on oxidation and reduction as these reactions entail a relatively small change to the overall structure.<ref name ="Greenwood"/> Fe<sub>3</sub>O<sub>4</sub> samples can be ].<ref name ="Greenwood"/> |
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The ] of Fe<sub>3</sub>O<sub>4</sub> arises because the electron spins of the Fe<sup>II</sup> and Fe<sup>III</sup> ions in the octahedral sites are coupled and the spins of the Fe<sup>III</sup> ions in the tetrahedral sites are coupled but anti-parallel to the former. The net effect is that the magnetic contributions of both sets are not balanced and there is a permanent magnetism.<ref name = "Greenwood"/> |
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The ] of Fe<sub>3</sub>O<sub>4</sub> arises because the electron spins of the Fe<sup>II</sup> and Fe<sup>III</sup> ions in the octahedral sites are coupled and the spins of the Fe<sup>III</sup> ions in the tetrahedral sites are coupled but anti-parallel to the former. The net effect is that the magnetic contributions of both sets are not balanced and there is a permanent magnetism.<ref name = "Greenwood"/> |
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In the molten state, experimentally constrained models show that the iron ions are coordinated to 5 oxygen ions on average.<ref name="ShiFeOx2020">{{cite journal | vauthors = Shi C, Alderman OL, Tamalonis A, Weber R, You J, Benmore CJ |title=Redox-structure dependence of molten iron oxides |journal=Communications Materials |date=2020 |volume=1 |issue=1 |page=80 |doi=10.1038/s43246-020-00080-4 |bibcode=2020CoMat...1...80S |s2cid=226248368 |ref=ShiFeOx2020|doi-access=free }}</ref> There is a distribution of coordination sites in the liquid state, with the majority of both Fe<sup>II</sup> and Fe<sup>III</sup> being 5-coordinated to oxygen and minority populations of both 4- and 6-fold coordinated iron. |
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==Properties== |
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==Properties== |
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], naturally occurring Fe<sub>3</sub>O<sub>4</sub>.]] |
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Fe<sub>3</sub>O<sub>4</sub> is ] with a ] of 858 K. There is a phase transition at 120K, the so-called '''Verwey transition''' where there is a discontinuity in the structure, conductivity and magnetic properties.<ref>{{cite journal | title = Electronic Conduction of Magnetite (Fe<sub>3</sub>O<sub>4</sub>) and its Transition Point at Low Temperatures | author = Verwey E. J. W. | journal = ] | volume = 144 | pages = 327–328 (1939) | doi = 10.1038/144327b0 | year = 1939 | issue=3642}}</ref> This effect has been extensively investigated and whilst various explanations have been proposed, it does not appear to be fully understood.<ref>{{cite journal | title = The Verwey transition - a topical review | author = Walz F. | journal = ] | year = 2002 | volume = 14 | pages = 285–340 | doi = 10.1088/0953-8984/14/12/203}}</ref> |
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Fe<sub>3</sub>O<sub>4</sub> is ] with a ] of {{Convert|858|K|C}}. There is a phase transition at {{Convert|120|K|C}}, called ] where there is a discontinuity in the structure, conductivity and magnetic properties.<ref>{{cite journal |title = Electronic Conduction of Magnetite (Fe<sub>3</sub>O<sub>4</sub>) and its Transition Point at Low Temperatures | vauthors = Verwey EJ |journal = ] |volume = 144 |pages = 327–328 (1939) |doi = 10.1038/144327b0 |year = 1939 | issue=3642|bibcode = 1939Natur.144..327V |s2cid = 41925681 }}</ref> This effect has been extensively investigated and whilst various explanations have been proposed, it does not appear to be fully understood.<ref>{{cite journal| vauthors = Walz F |title=The Verwey transition - a topical review |journal=Journal of Physics: Condensed Matter |date=2002 |volume=14 |issue=12 |pages=R285–R340 |doi=10.1088/0953-8984/14/12/203|s2cid=250773238 }}</ref> |
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Fe<sub>3</sub>O<sub>4</sub> is an electrical conductor with a conductivity is significantly higher (X 10<sup>6</sup>) than ], and this is ascribed to electron exchange between the Fe<sup>II</sup> and Fe<sup>III</sup> centres.<ref name = "Greenwood"/> |
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While it has much higher ] than iron metal (96.1 nΩ m), Fe<sub>3</sub>O<sub>4</sub>'s electrical resistivity (0.3 mΩ m <ref>{{cite journal| vauthors = Itai R |title=Electrical resistivity of Magnetite anodes |journal=Journal of the Electrochemical Society |date=1971 |volume=118 |issue=10 |page=1709 |doi=10.1149/1.2407817 |bibcode=1971JElS..118.1709I |url=http://www.chlorates.exrockets.com/magnetite/jes1971.html}}</ref>) is significantly lower than that of ] (approx kΩ m). This is ascribed to electron exchange between the Fe<sup>II</sup> and Fe<sup>III</sup> centres in Fe<sub>3</sub>O<sub>4</sub>.<ref name = "Greenwood"/> |
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==Uses== |
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==Uses== |
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{{Infobox drug |
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Fe<sub>3</sub>O<sub>4</sub> is used as a black pigment and is known as '''C.I pigment black 11''' (C.I. No.77499).<ref name = "Buxbaum"/> |
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| drug_name = Ferumoxytol |
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| INN = |
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<!-- Clinical data --> |
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Fe<sub>3</sub>O<sub>4</sub> is used as a catalyst in the ] and in the ].<ref name = "Lee">Sunggyu Lee (2006) Encyclopedia of Chemical Processing CRC Press ISBN 0824755634</ref> The latter uses an HTS (high temperature shift catalyst) of iron oxide stabilised by chromium oxide.<ref name = "Lee"/> This iron-chrome catalyst is reduced at reactor start up to generate Fe<sub>3</sub>O<sub>4</sub> from α-Fe<sub>2</sub>O<sub>3</sub> and Cr<sub>2</sub>O<sub>3</sub> to CrO<sub>3</sub>.<ref name = "Lee"/> |
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| pronounce = |
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| tradename = Feraheme, Rienso |
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| Drugs.com = {{drugs.com|monograph|ferumoxytol}} |
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| MedlinePlus = a614023 |
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| licence_CA = <!-- Health Canada may use generic or brand name (generic name preferred) --> |
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| licence_EU = Yes |
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| DailyMedID = Ferumoxytol |
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| licence_US = <!-- FDA may use generic or brand name (generic name preferred) --> |
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| pregnancy_AU = <!-- A / B1 / B2 / B3 / C / D / X --> |
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| pregnancy_AU_comment = |
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| pregnancy_US = N |
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| pregnancy_US_comment = <ref name="Drugs.com pregnancy">{{cite web | title=Ferumoxytol (Feraheme) Use During Pregnancy | website=Drugs.com | date=15 May 2020 | url=https://www.drugs.com/pregnancy/ferumoxytol.html | access-date=14 September 2020}}</ref> |
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| routes_of_administration = ] |
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| ATC_prefix = None |
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<!-- Legal status --> |
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Nano particles of Fe<sub>3</sub>O<sub>4</sub> are used as contrast agents in ]<ref>{{cite journal | title = Synthesis of Iron Oxide Nanoparticles Used as MRI Contrast Agents: A Parametric Study | author = Babes L, Denizot B, Tanguy G, Le Jeune J.J., Jallet P. | journal = ] | volume = 212 | issue = 2 | year = 1999 | pages = 474–482 | doi = 10.1006/jcis.1998.6053 | pmid = 10092379}}</ref> |
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| legal_AU = <!-- S2, S3, S4, S5, S6, S7, S8, S9 or Unscheduled --> |
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| legal_BR = <!-- OTC, A1, A2, A3, B1, B2, C1, C2, C3, C4, C5, D1, D2, E, F --> |
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| legal_CA = <!-- OTC, Rx-only, Schedule I, II, III, IV, V, VI, VII, VIII --> |
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| legal_DE = <!-- Anlage I, II, III or Unscheduled --> |
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| legal_NZ = <!-- Class A, B, C --> |
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| legal_UK = <!-- GSL, P, POM, CD, CD Lic, CD POM, CD No Reg POM, CD (Benz) POM, CD (Anab) POM or CD Inv POM / Class A, B, C --> |
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| legal_US = Rx-only |
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| legal_US_comment = <ref name="Feraheme FDA label">{{cite web | title=Feraheme- ferumoxytol injection | website=DailyMed | date=9 July 2020 | url=https://dailymed.nlm.nih.gov/dailymed/drugInfo.cfm?setid=32b0e320-a739-11dc-a704-0002a5d5c51b | access-date=14 September 2020}}</ref> |
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| legal_EU = Rx-only |
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| legal_EU_comment = <ref name="Rienso EPAR">{{cite web | title=Rienso EPAR | website=European Medicines Agency | date=17 September 2018 | url=https://www.ema.europa.eu/en/medicines/human/EPAR/rienso | access-date=14 September 2020}}</ref> |
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| legal_UN = <!-- N I, II, III, IV / P I, II, III, IV --> |
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| legal_status = <!-- For countries not listed above --> |
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<!-- Pharmacokinetic data --> |
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Along with ] and ], it is an ingredient in ] a specific type of ] useful for cutting steel. |
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<!-- Identifiers --> |
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] is a ] process that produces a layer of Fe<sub>3</sub>O<sub>4</sub> on the surface of steel to protect it from rust. |
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| CAS_number_Ref = {{cascite|correct|CAS}} |
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| CAS_number = 1309-38-2 |
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| DrugBank = DB06215 |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII = CLH5FT6412 |
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| KEGG = D04177 |
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| ChEBI = 46726 |
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<!-- Chemical and physical data --> |
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==Biological Occurrence== |
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| IUPAC_name = iron(2+);iron(3+);oxygen(2-) |
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Magnetite has been found as nano-crystals in ] (42-45 nm)<ref name = "Cornell"/> and in homing pigeon beak tissue<ref>{{cite journal | author = Hanzlik M., Heunemann C., Holtkamp-Rötzler E., Winklhofer M., Petersen N., Fleissner G | journal = ] | year = 2000 | volume = 13 | issue = 4 | pages = 325–331 | doi = 10.1023/A:1009214526685 | title =Superparamagnetic Magnetite in the Upper Beak Tissue of Homing Pigeons | pmid=11247039}}</ref> |
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| Fe = 3 | O = 4 |
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| SMILES = ...... |
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| StdInChI = 1S/3Fe.4O/q+2;2*+3;4*-2 |
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| StdInChI_comment = |
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| StdInChIKey = WTFXARWRTYJXII-UHFFFAOYSA-N |
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Fe<sub>3</sub>O<sub>4</sub> is used as a black pigment and is known as ''C.I pigment black 11'' (C.I. No.77499) or ].<ref name = "Buxbaum"/> |
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==See also== |
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*] |
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Fe<sub>3</sub>O<sub>4</sub> is used as a catalyst in the ] and in the ].<ref name = "Lee">Sunggyu Lee (2006) Encyclopedia of Chemical Processing CRC Press {{ISBN|0-8247-5563-4}}</ref> The latter uses an HTS (high temperature shift catalyst) of iron oxide stabilised by ].<ref name = "Lee"/> This iron–chrome catalyst is reduced at reactor start up to generate Fe<sub>3</sub>O<sub>4</sub> from α-Fe<sub>2</sub>O<sub>3</sub> and Cr<sub>2</sub>O<sub>3</sub> to CrO<sub>3</sub>.<ref name = "Lee"/> |
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==References== |
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] is a ] process that produces a layer of Fe<sub>3</sub>O<sub>4</sub> on the surface of steel to protect it from rust. Along with sulfur and aluminium, it is an ingredient in steel-cutting ].{{citation needed|date=September 2020}} |
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=== Medical uses === |
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Nano particles of Fe<sub>3</sub>O<sub>4</sub> are used as contrast agents in ].<ref>{{cite journal | vauthors = Babes L, Denizot B, Tanguy G, Jallet P | title = Synthesis of Iron Oxide Nanoparticles Used as MRI Contrast Agents: A Parametric Study | journal = Journal of Colloid and Interface Science | volume = 212 | issue = 2 | pages = 474–482 | date = April 1999 | pmid = 10092379 | doi = 10.1006/jcis.1998.6053 | bibcode = 1999JCIS..212..474B }}</ref> |
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Ferumoxytol, sold under the brand names Feraheme and Rienso, is an ] Fe<sub>3</sub>O<sub>4</sub> preparation for treatment of ] resulting from ].<ref name="Feraheme FDA label"/><ref name="Rienso EPAR"/><ref name="schwenk2010">{{cite journal |vauthors=Schwenk MH |title=Ferumoxytol: a new intravenous iron preparation for the treatment of iron deficiency anemia in patients with chronic kidney disease |journal= Pharmacotherapy |volume=30 |issue=1 |pages=70–79 |date=January 2010 |pmid=20030475 |doi=10.1592/phco.30.1.70 |s2cid=7748714 |url=http://www.medscape.com/viewarticle/715178}}</ref><ref name="FDA approval">{{cite web |title=Drug Approval Package: Feraheme (Ferumoxytol) Injection NDA #022180 |website=U.S. ] (FDA) |url=https://www.accessdata.fda.gov/drugsatfda_docs/nda/2009/022180s000TOC.cfm |access-date=14 September 2020}}<br/>{{cite web | vauthors = Rieves D |date=June 23, 2009 |title=Application Number: 22-180 |publisher=Center for Drug Evaluation and Research |type=Summary Review |url=https://www.accessdata.fda.gov/drugsatfda_docs/nda/2009/022180s000_SumR.pdf}}</ref> Ferumoxytol is manufactured and globally distributed by ].<ref name="Feraheme FDA label"/><ref name="FDA approval"/> |
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==Biological occurrence== |
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Magnetite has been found as nano-crystals in ] (42–45 nm)<ref name = "Cornell"/> and in the beak tissue of ]s.<ref>{{cite journal | vauthors = Hanzlik M, Heunemann C, Holtkamp-Rötzler E, Winklhofer M, Petersen N, Fleissner G | title = Superparamagnetic magnetite in the upper beak tissue of homing pigeons | journal = Biometals | volume = 13 | issue = 4 | pages = 325–31 | date = December 2000 | pmid = 11247039 | doi = 10.1023/A:1009214526685 | s2cid = 39216462 }}</ref> |
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{{clear}} |
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== References == |
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{{reflist}} |
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{{reflist}} |
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== External links == |
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* {{cite web | url = https://druginfo.nlm.nih.gov/drugportal/rn/1309-38-2 | publisher = U.S. National Library of Medicine | work = Drug Information Portal | title = Ferumoxytol }} |
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{{Iron compounds}} |
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{{Iron compounds}} |
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{{Oxides}} |
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{{oxygen compounds}} |
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{{Portal bar | Medicine}} |
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