Iron(II,III) oxide

Names
IUPAC name

iron(II) iron(III) oxide

Other names

ferrous ferric oxide, ferrosoferric oxide, iron(II,III) oxide, magnetite, black iron oxide, lodestone, rust, iron(II) diiron(III) oxide

Identifiers

CAS Number

* 1317-61-9 Y

3D model (JSmol)

* Interactive image

ChEBI |

* CHEBI:50821 Y

ChEMBL |

* ChEMBL1201867 N

ChemSpider |

* 17215625 Y

PubChem CID

* 16211978

UNII |

* XM0M87F357 Y

InChI

* InChI=1S/3Fe.4O Y

Key: SZVJSHCCFOBDDC-UHFFFAOYSA-N Y

* InChI=1/3Fe.4O/rFe3O4/c1-4-2-6-3(5-1)7-2

Key: SZVJSHCCFOBDDC-QXRQKJBKAR

SMILES

* O1[Fe]2O[Fe]O[Fe]1O2

Properties

Chemical formula

| Fe3O4

FeO.Fe2O3

Molar mass | 231.533 g/mol
Appearance  | solid black powder
Density | 5 g/cm3
Melting point |  1,597 °C (2,907 °F; 1,870 K)
Boiling point |  2,623[1] °C (4,753 °F; 2,896 K)

Refractive index (nD)

| 2.42[2]
Hazards
NFPA 704 (fire diamond)  |

Thermochemistry

Std enthalpy of
formation (ΔfH⦵298)

| -1120.89 kJ·mol−1[3]

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

N verify (what is YN ?)
Infobox references

Iron(II,III) oxide, or black iron oxide, is the chemical compound with formula Fe3O4. It occurs in nature as the mineral magnetite. It is one of a number of iron oxides, the others being iron(II) oxide (FeO), which is rare, and iron(III) oxide (Fe2O3) which also occurs naturally as the mineral hematite. It contains both Fe2+ and Fe3+ ions and is sometimes formulated as FeO ∙ Fe2O3. This iron oxide is encountered in the laboratory as a black powder. It exhibits permanent magnetism and is ferrimagnetic, but is sometimes incorrectly described as ferromagnetic.[4] Its most extensive use is as a black pigment (see: Mars Black). 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.[5]

## Contents

* 1 Preparation
* 2 Reactions
* 3 Structure
* 4 Properties
* 5 Uses
* 5.1 Medical uses
* 6 Biological occurrence
* 7 References
* 8 External links

## Preparation

Heated iron metal interacts with steam to form iron oxide and hydrogen gas.

3Fe+4HA2O⟶FeA3OA4+4HA2

Under anaerobic conditions, ferrous hydroxide (Fe(OH)2) can be oxidized by water to form magnetite and molecular hydrogen. This process is described by the Schikorr reaction:

3Fe(OH)A2ferrous hydroxide⟶FeA3OA4magnetite+HA2hydrogen+2HA2Owater

This works because crystalline magnetite (Fe3O4) is thermodynamically more stable than amorphous ferrous hydroxide (Fe(OH)2 ).[6]

The Massart method of preparation of magnetite as a ferrofluid, is convenient in the laboratory: mix iron(II) chloride and iron(III) chloride in the presence of sodium hydroxide.[7]

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 FeCl3·6H2O and FeCl2·4H2O with vigorous stirring at about 2000 rpm. The molar ratio of the FeCl3:FeCl2 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 NH4OH (10 volume %). A dark precipitate of nanoparticles of magnetite forms immediately.[8]

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.

Controlling the formation of magnetite nanoparticles presents challenges: the reactions and phase transformations necessary for the creation of the magnetite spinel structure are complex.[9] The subject is of practical importance because magnetite particles are of interest in bioscience applications such as magnetic resonance imaging (MRI), in which iron oxide magnetite nanoparticles potentially present a non-toxic alternative to the gadolinium-based contrast agents 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−1,[10] whereas the largest reported magnetization value is 87 Am2 kg−1 for synthetic magnetite.[11][12]

Pigment quality Fe3O4, 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 (pickling) of steel):

* Oxidation of Fe metal in the Laux process where nitrobenzene is treated with iron metal using FeCl2 as a catalyst to produce aniline:[5]

C6H5NO2 \+ 3 Fe + 2 H2O → C6H5NH2 \+ Fe3O4

* Oxidation of FeII 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.[5]

Reduction of Fe2O3 with hydrogen:[13][14]

3Fe2O3 \+ H2 → 2Fe3O4 +H2O

Reduction of Fe2O3 with CO:[15]

3Fe2O3 \+ CO → 2Fe3O4 \+ CO2

Production of nano-particles can be performed chemically by taking for example mixtures of FeII and FeIII salts and mixing them with alkali to precipitate colloidal Fe3O4. The reaction conditions are critical to the process and determine the particle size.[16]

Iron(II) carbonate can also be thermally decomposed into Iron(II,III):[17]

3FeCO
3 → Fe

4 \+ 2CO
2 \+ CO

## Reactions

Reduction of magnetite ore by CO in a blast furnace is used to produce iron as part of steel production process:[4]

Fe3O4+4CO⟶3Fe+4COA2

Controlled oxidation of Fe3O4 is used to produce brown pigment quality γ-Fe2O3 (maghemite):[18]

2FeA3OA4⏟magnetite+1/2O2⟶ 3(γ-FeA2OA3)⏟maghemite

More vigorous calcining (roasting in air) gives red pigment quality α-Fe2O3 (hematite):[18]

2FeA3OA4⏟magnetite+1/2O2⟶ 3(α-FeA2OA3)⏟hematite

## Structure

Fe3O4 has a cubic inverse spinel group structure which consists of a cubic close packed array of oxide ions where all of the Fe2+ ions occupy half of the octahedral sites and the Fe3+ are split evenly across the remaining octahedral sites and the tetrahedral sites.

Both FeO and γ-Fe2O3 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.[4] Fe3O4 samples can be non-stoichiometric.[4]

The ferrimagnetism of Fe3O4 arises because the electron spins of the FeII and FeIII ions in the octahedral sites are coupled and the spins of the FeIII 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.[4]

In the molten state, experimentally constrained models show that the iron ions are coordinated to 5 oxygen ions on average.[19] There is a distribution of coordination sites in the liquid state, with the majority of both FeII and FeIII being 5-coordinated to oxygen and minority populations of both 4- and 6-fold coordinated iron.

## Properties

Sample of magnetite, naturally occurring Fe3O4.

Fe3O4 is ferrimagnetic with a Curie temperature of 858 K (585 °C). There is a phase transition at 120 K (−153 °C), called Verwey transition where there is a discontinuity in the structure, conductivity and magnetic properties.[20] This effect has been extensively investigated and whilst various explanations have been proposed, it does not appear to be fully understood.[21]

While it has much higher electrical resistivity than iron metal (96.1 nΩ m), Fe3O4's electrical resistivity (0.3 mΩ m [22]) is significantly lower than that of Fe2O3 (approx kΩ m). This is ascribed to electron exchange between the FeII and FeIII centres in Fe3O4.[4]

## Uses

FerumoxytolClinical data

Trade names| Feraheme, Rienso
AHFS/Drugs.com| Monograph
MedlinePlus| a614023
License data|

* EU EMA: by INN
* US DailyMed: Ferumoxytol

Pregnancy
category|

* US: N (Not classified yet)[23]

Routes of
administration| Intravenous infusion
ATC code|

* None

Legal status
Legal status|

* US: ℞-only [24]
* EU: Rx-only [25]

Identifiers

IUPAC name

* iron(2+);iron(3+);oxygen(2-)

CAS Number|

* 1309-38-2 Y

DrugBank|

* DB06215

UNII|

* CLH5FT6412

KEGG|

* D04177

ChEBI|

* CHEBI:46726

Chemical and physical data
Formula| Fe3O4
Molar mass| 231.531 g·mol−1
3D model (JSmol)|

* Interactive image

SMILES

* [O-2].[O-2].[O-2].[O-2].[Fe+2].[Fe+3].[Fe+3]

InChI

* InChI=1S/3Fe.4O/q+2;2*+3;4*-2

* Key:WTFXARWRTYJXII-UHFFFAOYSA-N

Fe3O4 is used as a black pigment and is known as C.I pigment black 11 (C.I. No.77499) or Mars Black.[18]

Fe3O4 is used as a catalyst in the Haber process and in the water-gas shift reaction.[26] The latter uses an HTS (high temperature shift catalyst) of iron oxide stabilised by chromium oxide.[26] This iron–chrome catalyst is reduced at reactor start up to generate Fe3O4 from α-Fe2O3 and Cr2O3 to CrO3.[26]

Bluing is a passivation process that produces a layer of Fe3O4 on the surface of steel to protect it from rust. Along with sulfur and aluminium, it is an ingredient in steel-cutting thermite.[citation needed]

### Medical uses

Nano particles of Fe3O4 are used as contrast agents in MRI scanning.[27]

Ferumoxytol, sold under the brand names Feraheme and Rienso, is an intravenous Fe3O4 preparation for treatment of anemia resulting from chronic kidney disease.[24][25][28][29] Ferumoxytol is manufactured and globally distributed by AMAG Pharmaceuticals.[24][29]

## Biological occurrence

Magnetite has been found as nano-crystals in magnetotactic bacteria (42–45 nm)[5] and in the beak tissue of homing pigeons.[30]

## References

1. ↑ Magnetite (Fe3O4): Properties, Synthesis, and Applications Lee Blaney, Lehigh Review 15, 33-81 (2007). See Appendix A, p.77
2. ↑ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
3. ↑ "NIST-JANAF Themochemical Tables". NIST: 1–1951. 1998. https://webbook.nist.gov/cgi/cbook.cgi?ID=C1309382&Units=SI&Mask=2.
4. ↑ 4.0 4.1 4.2 4.3 4.4 4.5 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
5. ↑ 5.0 5.1 5.2 5.3 The Iron Oxides: Structure, Properties, Reactions, Occurrences and Uses. Wiley-VCH. 2007. ISBN 978-3-527-60644-3.
6. ↑ "Facile synthesis of ultrathin magnetic iron oxide nanoplates by Schikorr reaction". Nanoscale Research Letters 8 (1): 16. January 2013. doi:10.1186/1556-276X-8-16. PMID 23294626. Bibcode: 2013NRL.....8...16M.
7. ↑ "Preparation of aqueous magnetic liquids in alkaline and acidic media". IEEE Transactions on Magnetics 17 (2): 1247–1248. 1981. doi:10.1109/TMAG.1981.1061188. Bibcode: 1981ITM....17.1247M.
8. ↑ "Relaxation of Polymer Coated Fe3O4 Magnetic Nanoparticles in Aqueous Solution". IEEE Transactions on Magnetics 46 (6): 1541–1543. 2010. doi:10.1109/TMAG.2010.2040588.
9. ↑ "Iron oxide chemistry. From molecular clusters to extended solid networks". Chemical Communications (5): 481–7. March 2004. doi:10.1039/B304532N. PMID 14973569.
10. ↑ "Real-time monitoring of the evolution of magnetism during precipitation of superparamagnetic nanoparticles for bioscience applications". Journal of Materials Chemistry 20 (20): 4168. 2010. doi:10.1039/C0JM00043D.
11. ↑ "Rapid mixing: A route to synthesize magnetite nanoparticles with high moment". Applied Physics Letters 99 (22): 222501. 2011. doi:10.1063/1.3662965. Bibcode: 2011ApPhL..99v2501F.
12. ↑ "Particle size and magnetic properties dependence on growth temperature for rapid mixed co-precipitated magnetite nanoparticles". Nanotechnology 23 (14): 145601. April 2012. doi:10.1088/0957-4484/23/14/145601. PMID 22433909. Bibcode: 2012Nanot..23n5601F.
13. ↑ Heath TD, "Process for reduction of iron ore to magnetite", US patent 2596954, issued 13 May 1952, assigned to Dorr Company
14. ↑ "Kinetics of reduction of iron oxides by H2 Part I: Low temperature reduction of hematite". Thermochimica Acta 447 (1): 89–100. 2006. doi:10.1016/j.tca.2005.10.004.
15. ↑ "The effects of nucleation and growth on the reduction of Fe2O3 to Fe3O4". Metallurgical and Materials Transactions B 12 (2): 319–326. 1981. doi:10.1007/BF02654465. Bibcode: 1981MTB....12..319H.
16. ↑ Arthur T. Hubbard (2002) Encyclopedia of Surface and Colloid Science CRC Press, ISBN 0-8247-0796-6
17. ↑ "FeCO3 = Fe3O4 + CO2 + CO | The thermal decomposition of iron(II) carbonate". https://chemiday.com/en/reaction/3-1-0-5222.
18. ↑ 18.0 18.1 18.2 Gunter Buxbaum, Gerhard Pfaff (2005) Industrial Inorganic Pigments 3d edition Wiley-VCH ISBN 3-527-30363-4
19. ↑ "Redox-structure dependence of molten iron oxides". Communications Materials 1 (1): 80. 2020. doi:10.1038/s43246-020-00080-4. Bibcode: 2020CoMat...1...80S.
20. ↑ "Electronic Conduction of Magnetite (Fe3O4) and its Transition Point at Low Temperatures". Nature 144 (3642): 327–328 (1939). 1939. doi:10.1038/144327b0. Bibcode: 1939Natur.144..327V.
21. ↑ "The Verwey transition - a topical review". Journal of Physics: Condensed Matter 14 (12): R285–R340. 2002. doi:10.1088/0953-8984/14/12/203.
22. ↑ "Electrical resistivity of Magnetite anodes". Journal of the Electrochemical Society 118 (10): 1709. 1971. doi:10.1149/1.2407817. Bibcode: 1971JElS..118.1709I. http://www.chlorates.exrockets.com/magnetite/jes1971.html.
23. ↑ "Ferumoxytol (Feraheme) Use During Pregnancy". 15 May 2020. https://www.drugs.com/pregnancy/ferumoxytol.html.
24. ↑ 24.0 24.1 24.2 "Feraheme- ferumoxytol injection". 9 July 2020. https://dailymed.nlm.nih.gov/dailymed/drugInfo.cfm?setid=32b0e320-a739-11dc-a704-0002a5d5c51b.
25. ↑ 25.0 25.1 "Rienso EPAR". 17 September 2018. https://www.ema.europa.eu/en/medicines/human/EPAR/rienso.
26. ↑ 26.0 26.1 26.2 Sunggyu Lee (2006) Encyclopedia of Chemical Processing CRC Press ISBN 0-8247-5563-4
27. ↑ "Synthesis of Iron Oxide Nanoparticles Used as MRI Contrast Agents: A Parametric Study". Journal of Colloid and Interface Science 212 (2): 474–482. April 1999. doi:10.1006/jcis.1998.6053. PMID 10092379. Bibcode: 1999JCIS..212..474B.
28. ↑ "Ferumoxytol: a new intravenous iron preparation for the treatment of iron deficiency anemia in patients with chronic kidney disease". Pharmacotherapy 30 (1): 70–79. January 2010. doi:10.1592/phco.30.1.70. PMID 20030475. http://www.medscape.com/viewarticle/715178.
29. ↑ 29.0 29.1 "Drug Approval Package: Feraheme (Ferumoxytol) Injection NDA #022180". https://www.accessdata.fda.gov/drugsatfda_docs/nda/2009/022180s000TOC.cfm.
"Application Number: 22-180". Center for Drug Evaluation and Research. June 23, 2009. https://www.accessdata.fda.gov/drugsatfda_docs/nda/2009/022180s000_SumR.pdf.
30. ↑ "Superparamagnetic magnetite in the upper beak tissue of homing pigeons". Biometals 13 (4): 325–31. December 2000. doi:10.1023/A:1009214526685. PMID 11247039.

## External links

* "Ferumoxytol". Drug Information Portal. U.S. National Library of Medicine. https://druginfo.nlm.nih.gov/drugportal/rn/1309-38-2.

* v
* t
* e

Iron compounds

Fe(-II)|

* Na2Fe(CO)4

Fe(0)|

* Fe(CO)5
* Fe2(CO)9
* Fe3(CO)12
* Fe(CO)3CH3COC2H2C6H6

Fe(I)|

* FeH

| Organoiron(I) compounds|

* (C5H5FeCO)2(CO)2

|

Fe(0,II)|

* Fe3C

Fe(II)|

* FeBr2
* FeCl2
* FeF2
* FeI2
* FeH2
* FeMoO4
* FeO
* Fe(OH)2
* FeS
* FeSO4
* FeSe
* FeSeO4
* FeSi2
* FeTiO3
* FeCO3
* FeC2O4
* Fe(C2H3O2)2
* Fe(C3H5O3)2
* FeC6H6O7
* FeC12H22O14
* Fe2CrO4
* Fe3(PO4)2
* H2Fe(CO)4
* Fe(HCO3)2
* Mg2FeH6

| Organoiron(II) compounds|

* Fe(C5H5)2
* Fe(C5H4P(C6H5)2)2
* C4H4Fe(CO)3
* C4H6Fe(CO)3

|

Fe(0,III)|

* Fe3P

Fe(II,III)|

* Fe3O4
* Fe3S4

Fe(III)|

* FeBr3
* FeCl3
* FeF3
* FeI3
* Fe(NO3)3
* Fe(acac)3
* FeOCl
* FeO(OH)
* FePO4
* Fe4(P2O7)3
* Fe2(CrO4)3
* Fe2(C2O4)3
* Fe2O3
* Fe2S3
* Fe2(SO4)3
* FeBO3
* FeB

| Organoiron(III) compounds|

* Fe(C5H5)2BF4
* C6H8O7⋅xFe3+⋅yNH3

|

Fe(VI)|

* K2FeO4
* BaFeO4

* v
* t
* e

Oxides

Mixed oxidation states|

* Antimony tetroxide (Sb2O4)
* Cobalt(II,III) oxide (Co3O4)
* Europium(II,III) oxide (Eu3O4)
* Iron(II,III) oxide (Fe<sub>3O4)
* Lead(II,IV) oxide (Pb3O4)
* Manganese(II,III) oxide (Mn3O4)
* Silver(I,III) oxide (Ag2O2)
* Triuranium octoxide (U3O8)
* Carbon suboxide (C3O2)
* Mellitic anhydride (C12O9)
* [[Chemistry:Praseodymium(III,IV) Praseodymium(III,IV) oxide]] (Pr6O11)
* Terbium(III,IV) oxide (Tb4O7)

+1 oxidation state|

* Copper(I) oxide (Cu<sub>2O)
* Caesium oxide (Cs2O)
* Dicarbon monoxide (C2O)
* Dichlorine monoxide (Cl2O)
* Gallium(I) oxide (Ga2O)
* Lithium oxide (Li2O)
* Potassium oxide (K2O)
* Rubidium oxide (Rb2O)
* Silver oxide (Ag2O)
* Thallium(I) oxide (Tl2O)
* Sodium oxide (Na2O)
* Water (hydrogen oxide) (H2O)

+2 oxidation state|

* Aluminium(II) oxide (AlO)
* Barium oxide (BaO)
* Beryllium oxide (BeO)
* Cadmium oxide (CdO)
* Calcium oxide (CaO)
* Carbon monoxide (CO)
* Chromium(II) oxide (CrO)
* Cobalt(II) oxide (CoO)
* Copper(II) oxide (CuO)
* Europium(II) oxide (EuO)
* Germanium monoxide (GeO))
* Iron(II) oxide (FeO)
* Lead(II) oxide (PbO)
* Magnesium oxide (MgO)
* Manganese(II) oxide (MnO)
* Mercury(II) oxide (HgO)
* Nickel(II) oxide (NiO)
* Nitric oxide (NO)
* Palladium(II) oxide (PdO)
* Silicon monoxide (SiO)
* Strontium oxide (SrO)
* Sulfur monoxide (SO)
* Disulfur dioxide (S2O2)
* Thorium monoxide (ThO)
* Tin(II) oxide (SnO)
* Titanium(II) oxide (TiO)
* Vanadium(II) oxide (VO)
* Zinc oxide (ZnO)

+3 oxidation state|

* Aluminium oxide (Al<sub>2O3)
* Antimony trioxide (Sb2O3)
* Arsenic trioxide (As2O3)
* Bismuth(III) oxide (Bi2O3)
* Boron trioxide (B2O3)
* Cerium(III) oxide (Ce2O3)
* Dibromine trioxide (Br2O3)
* Chromium(III) oxide (Cr2O3)
* Dinitrogen trioxide (N2O3)
* Dysprosium(III) oxide (Dy2O3)
* Erbium(III) oxide (Er2O3)
* Europium(III) oxide (Eu2O3)
* Gadolinium(III) oxide (Gd2O3)
* Gallium(III) oxide (Ga2O3)
* Holmium(III) oxide (Ho2O3)
* Indium(III) oxide (In<sub>2O3)
* Iron(III) oxide (Fe2O3)
* Lanthanum oxide (La2O3)
* Lutetium(III) oxide (Lu2O3)
* Manganese(III) oxide (Mn2O3)
* Neodymium(III) oxide (Nd2O3)
* Nickel(III) oxide (Ni2O3)
* Phosphorus trioxide (P4O6)
* Praseodymium(III) oxide (Pr2O3)
* Promethium(III) oxide (Pm2O3)
* Rhodium(III) oxide (Rh2O3)
* [[Chemistry:Samarium(III) Samarium(III) oxide]] (Sm2O3)
* Scandium oxide (Sc2O3)
* Terbium(III) oxide (Tb2O3)
* Thallium(III) oxide (Tl2O3)
* Thulium(III) oxide (Tm2O3)
* Titanium(III) oxide (Ti2O3)
* Tungsten(III) oxide (W2O3)
* Vanadium(III) oxide (V2O3)
* Ytterbium(III) oxide (Yb2O3)
* Yttrium(III) oxide (Y2O3)

+4 oxidation state|

* Americium dioxide (AmO2)
* Carbon dioxide (CO2)
* Carbon trioxide (CO3)
* Cerium(IV) oxide (CeO2)
* Chlorine dioxide (ClO2)
* Chromium(IV) oxide (CrO<sub>2)
* Dinitrogen tetroxide (N2O4)
* Germanium dioxide (GeO<sub>2)
* [[Chemistry:Hafnium(IV) Hafnium(IV) oxide]] (HfO2)
* Lead dioxide (PbO2)
* Manganese dioxide (MnO2)
* Neptunium(IV) oxide (NpO2)
* Nitrogen dioxide (NO2)
* Osmium dioxide (OsO2)
* Plutonium(IV) oxide (PuO2)
* Praseodymium(IV) oxide (PrO2)
* Protactinium(IV) oxide (PaO2)
* Rhodium(IV) oxide (RhO2)
* Ruthenium(IV) oxide (RuO<sub>2)
* Selenium dioxide (SeO2)
* Silicon dioxide (SiO2)
* Sulfur dioxide (SO2)
* Tellurium dioxide (TeO<sub>2)
* [[Chemistry:Terbium(IV) Terbium(IV) oxide]] (TbO2)
* Thorium dioxide (ThO2)
* Tin dioxide (SnO2)
* Titanium dioxide (TiO<sub>2)
* Tungsten(IV) oxide (WO2)
* Uranium dioxide (UO2)
* Vanadium(IV) oxide (VO2)
* Zirconium dioxide (ZrO2)

+5 oxidation state|

* Antimony pentoxide (Sb2O5)
* Arsenic pentoxide (As2O5)
* Dinitrogen pentoxide (N2O5)
* Niobium pentoxide (Nb2O5)
* Phosphorus pentoxide (P2O5)
* Protactinium(V) oxide (Pa2O5)
* Tantalum pentoxide (Ta2O5)
* Vanadium(V) oxide (V2O5)

+6 oxidation state|

* Chromium trioxide (CrO3)
* Molybdenum trioxide (MoO3)
* Rhenium trioxide (ReO3)
* Selenium trioxide (SeO3)
* Sulfur trioxide (SO3)
* Tellurium trioxide (TeO3)
* Tungsten trioxide (WO3)
* Uranium trioxide (UO3)
* Xenon trioxide (XeO3)
* Iridium trioxide (IrO3)

+7 oxidation state|

* Dichlorine heptoxide (Cl2O7)
* Manganese heptoxide (Mn2O7)
* [[Chemistry:Rhenium(VII) Rhenium(VII) oxide]] (Re2O7)
* Technetium(VII) oxide (Tc2O7)

+8 oxidation state|

* Osmium tetroxide (OsO4)
* Ruthenium tetroxide (RuO4)
* Xenon tetroxide (XeO4)
* Iridium tetroxide (IrO4)
* Hassium tetroxide (HsO4)

Related|

* Oxocarbon
* Suboxide
* Oxyanion
* Ozonide
* Peroxide
* Superoxide

Oxides are sorted by oxidation state. Category:Oxides

* v
* t
* e

Oxygen compounds

* AgO
* Al2O3
* AmO2
* Am2O3
* As2O3
* As2O5
* Au2O3
* B2O3
* BaO
* BeO
* Bi2O3
* BiO2
* Bi2O5
* BrO2
* Br2O3
* Br2O5
* CO
* CO2
* C2O3
* CaO
* CaO2
* CdO
* CeO2
* Ce3O4
* Ce2O3
* ClO2
* Cl2O
* Cl2O3
* Cl2O4
* Cl2O6
* Cl2O7
* CoO
* Co2O3
* Co3O4
* CrO3
* Cr2O3
* Cr2O5
* Cr5O12
* CsO2
* Cs2O3
* CuO
* D2O
* Dy2O3
* Er2O3
* Eu2O3
* FeO
* Fe2O3
* Fe3O4
* Ga2O
* Ga2O3
* GeO
* GeO2
* H2O
* H218O
* H2O2
* HfO2
* HgO
* Hg2O
* Ho2O3
* I2O4
* I2O5
* I2O6
* I4O9
* In2O3
* IrO2
* KO2
* K2O2
* La2O3
* Li2O
* Li2O2
* Lu2O3
* MgO
* Mg2O3
* MnO
* MnO2
* Mn2O3
* Mn2O7
* MoO2
* MoO3
* Mo2O3
* NO
* NO2
* N2O
* N2O3
* N2O4
* N2O5
* NaO2
* Na2O
* Na2O2
* NbO
* NbO2
* Nd2O3
* OF2
* O2F2
* O3F2
* O4F2
* O2PtF6

Chemical formulas

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Original source: https://en.wikipedia.org/wiki/Iron(II,III) oxide. Read more

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