|Jmol-3D images||Image 1|
|Molar mass||71.844 g/mol|
1377 °C, 1650 K, 2511 °F ()
3414 °C, 3687 K, 6177 °F
|Solubility in water||Insoluble|
|Solubility||insoluble in alkali, alcohol
dissolves in acid
|Refractive index (nD)||2.23|
|EU Index||Not listed|
|Main hazards||can be pyrophoric|
|Other anions||iron(II) fluoride, iron(II) sulfide, iron(II) selenide, iron(II) telluride|
|Other cations||manganese(II) oxide, cobalt(II) oxide|
|Related compounds||Iron(III) oxide, Iron(II,III) oxide|
| (what is: / ?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Iron(II) oxide, also known by its former name ferrous oxide or informally as iron monoxide, is one of the iron oxides. It is a black-colored powder with the chemical formula FeO. It consists of the chemical element iron in the oxidation state of 2 bonded to oxygen. Its mineral form is known as wüstite. Iron(II) oxide should not be confused with rust, which usually consists of hydrated iron(III) oxide (ferric oxide). The term may be used more loosely for a non-stoichiometric compound as the ratio of the elements iron and oxygen can vary; samples are typically iron deficient with compositions ranging from Fe0.84O to Fe0.95O.
- FeC2O4 → FeO + CO + CO2
Stoichiometric FeO can be prepared by heating Fe0.95O with metallic iron at 770 °C and 36 kbar.
- 4FeO → Fe + Fe3O4
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 FeII to FeIII effectively replacing a small portion of FeII with two thirds their number of FeIII, which take up tetrahedral positions in the close packed oxide lattice.
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.
- Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
- Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth–Heinemann. ISBN 0080379419.
- Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford University Press ISBN 0-19-855370-6
- Science Jan 2012