Iron(II,III) oxide

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
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.013.889 Edit this at Wikidata
UNII
  • InChI=1S/3Fe.4O checkY
    Key: SZVJSHCCFOBDDC-UHFFFAOYSA-N checkY
  • InChI=1/3Fe.4O/rFe3O4/c1-4-2-6-3(5-1)7-2
    Key: SZVJSHCCFOBDDC-QXRQKJBKAR
  • O1[Fe]2O[Fe]O[Fe]1O2
Properties
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)
2.42[2]
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 0: Exposure under fire conditions would offer no hazard beyond that of ordinary combustible material. E.g. sodium chlorideFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
0
0
1
OX
Thermochemistry
-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).
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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]

  1. ^ Magnetite (Fe3O4): Properties, Synthesis, and Applications Archived 2017-07-20 at the Wayback Machine 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. ^ Chase MW (1998). "NIST-JANAF Themochemical Tables". NIST (Fourth ed.): 1–1951.
  4. ^ Greenwood NN, Earnshaw A (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  5. ^ Cornell RM, Schwertmann U (2007). The Iron Oxides: Structure, Properties, Reactions, Occurrences and Uses. Wiley-VCH. ISBN 978-3-527-60644-3.