Iron(II) oxide

Iron(II) oxide
IUPAC name

Iron(II) oxide
Other names

Ferrous oxide
Identifiers
CAS number 1345-25-1 Y
PubChem 14945
ChemSpider 14237 Y
UNII G7036X8B5H Y
ChEBI CHEBI:50820 Y
Jmol-3D images Image 1
Properties
Molecular formula FeO
Molar mass 71.844 g/mol
Appearance black crystals
Density 5.745 g/cm3
Melting point

1377 °C, 1650 K, 2511 °F ([1])
Boiling point

3414 °C, 3687 K, 6177 °F
Solubility in water Insoluble
Solubility insoluble in alkali, dissolves in acid
Hazards
MSDS ICSC 0793
EU Index Not listed
Main hazards can be pyrophoric
Autoignition
temperature		 variable
Related compounds
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
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Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Iron(II) oxide, also known as ferrous oxide, 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.[2]

Contents

Preparation

FeO can be prepared by heating iron(II) oxalate in vacuo:[2]

FeC2O4 → FeO + CO + CO2

Stoichiometric FeO can be prepared by heating Fe0.95O with metallic iron at 770 °C and 36 kbar.[3]

Reactions

FeO is thermodynamically unstable below 575 °C, disproportionating to metal and Fe3O4:[2]

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 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.[3]

Below 200 K there is a minor change to the structure which changes the symmetry to rhombohedral and samples become antiferromagnetic.[3]

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.

References

  1. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0070494398
  2. ^ a b c Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Oxford: Butterworth-Heinemann. ISBN 0080379419. 
  3. ^ a b c Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford University Press ISBN 0198553706

External links