Iron(II) oxide

Iron(II) oxide or ferrous oxide is the inorganic compound with the formula FeO. Its mineral form is known as wüstite.^[3][4] One of several iron oxides, it is a black-colored powder that is sometimes confused with rust, the latter of which consists of hydrated iron(III) oxide (ferric oxide). Iron(II) oxide also refers to a family of related non-stoichiometric compounds, which are typically iron deficient with compositions ranging from Fe_0.84O to Fe_0.95O.^[5]

Iron(II) oxide

Names
IUPAC name Iron(II) oxide
Other names Ferrous oxide, Iron monoxide, Wüstite
Identifiers
CAS Number	1345-25-1 Y
3D model (JSmol)	Interactive image
ChEBI	CHEBI:50820 Y
ChemSpider	14237 Y
ECHA InfoCard	100.014.292
Gmelin Reference	13590
PubChem CID	14945
UNII	G7036X8B5H Y
CompTox Dashboard (EPA)	DTXSID1041976
InChI InChI=1S/Fe.O Y Key: UQSXHKLRYXJYBZ-UHFFFAOYSA-N Y InChI=1/Fe.O/rFeO/c1-2 Key: UQSXHKLRYXJYBZ-WPTVXXAFAB
SMILES [Fe]=O
Properties
Chemical formula	FeO
Molar mass	71.844 g/mol
Appearance	black crystals
Density	5.745 g/cm3
Melting point	1,377 °C (2,511 °F; 1,650 K)[1]
Boiling point	3,414 °C (6,177 °F; 3,687 K)
Solubility in water	Insoluble
Solubility	insoluble in alkali, alcohol dissolves in acid
Magnetic susceptibility (χ)	+7200·10−6 cm3/mol
Refractive index (nD)	2.23
Hazards
Occupational safety and health (OHS/OSH):
Main hazards	can be combustible under specific conditions[2]
NFPA 704 (fire diamond)	1 1 0
Autoignition temperature	200 °C (392 °F; 473 K)
Safety data sheet (SDS)	ICSC 0793
Related compounds
Other anions	Iron(II) sulfide Iron(II) selenide Iron(II) telluride
Other cations	Manganese(II) oxide Cobalt(II) oxide
Related Iron oxides	Iron(II,III) oxide Iron(III) oxide
Related compounds	Iron(II) fluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Y verify (what is YN ?) Infobox references

Preparation

FeO can be prepared by the thermal decomposition of iron(II) oxalate.

FeC₂O₄ → FeO + CO₂ + CO

The procedure is conducted under an inert atmosphere to avoid the formation of iron(III) oxide (Fe₂O₃). A similar procedure can also be used for the synthesis of manganous oxide and stannous oxide.^[6][7]

Stoichiometric FeO can be prepared by heating Fe_0.95O with metallic iron at 770 °C and 36 kbar.^[8]

Reactions

FeO is thermodynamically unstable below 575 °C, tending to disproportionate to metal and Fe₃O₄:^[5]

• 4FeO → Fe + Fe₃O₄

Structure

Iron(II) oxide adopts the cubic, rock salt structure, where iron atoms are octahedrally coordinated by oxygen atoms and the oxygen atoms octahedrally coordinated by iron atoms. The non-stoichiometry occurs because of the ease of oxidation of Fe^II to Fe^III effectively replacing a small portion of Fe^II with two-thirds their number of Fe^III, which take up tetrahedral positions in the close packed oxide lattice.^[8]

In contrast to the crystalline solid, in the molten state iron atoms are coordinated by predominantly 4 or 5 oxygen atoms.^[9]

Below 200 K there is a minor change to the structure which changes the symmetry to rhombohedral and samples become antiferromagnetic.^[8][10]

Occurrence in nature

Iron(II) oxide makes up approximately 9% of the Earth's mantle. Within the mantle, it may be electrically conductive, which is a possible explanation for perturbations in Earth's rotation not accounted for by accepted models of the mantle's properties.^[11]

Uses

Iron(II) oxide is used as a pigment. It is FDA-approved for use in cosmetics and it is used in some tattoo inks. It can also be used as a phosphate remover from home aquaria.

See also

• Iron(II) hydroxide
• Iron(II)

References

1. Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
2. "Ferric(ous) Oxide, Black" (PDF). art.illinois.edu. Archived from the original (PDF) on 11 May 2019.
3. "Wüstite". www.mindat.org.
4. "List of Minerals". www.ima-mineralogy.org. March 21, 2011.
5. Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
6. H. Lux "Iron (II) Oxide" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 1497.
7. Practical Chemistry for Advanced Students, Arthur Sutcliffe, 1930 (1949 Ed.), John Murray - London
8. Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford University Press ISBN 0-19-855370-6
9. Shi, Caijuan; Alderman, Oliver; Tamalonis, Anthony; Weber, Richard; You, Jinglin; Benmore, Chris (2020). "Redox-structure dependence of molten iron oxides". Communications Materials. 1 (1): 80. Bibcode:2020CoMat...1...80S. doi:10.1038/s43246-020-00080-4.
10. Proceedings of the 5th Unconventional Resources Technology Conference. Tulsa, OK, USA: American Association of Petroleum Geologists. 2017. doi:10.15530/urtec-2017-2670073. ISBN 978-0-9912144-4-0.
11. "Science Jan 2012". Archived from the original on January 24, 2012.

External links

• Wustite Mineral Data