Iron(II) oxide

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Iron(II) oxide
Iron(II) oxide
Identifiers
CAS number 1345-25-1 YesY
PubChem 14945
ChemSpider 14237 YesY
UNII G7036X8B5H YesY
ChEBI CHEBI:50820 YesY
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 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
Refractive index (nD) 2.23
Hazards
MSDS ICSC 0793
EU Index Not listed
Main hazards can be pyrophoric
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 0: Exposure under fire conditions would offer no hazard beyond that of ordinary combustible material. E.g., sodium chloride Reactivity (yellow): no hazard code Special hazards (white): no codeNFPA 704 four-colored diamond
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
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

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.[2]

Preparation[edit]

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[edit]

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

4FeO → Fe + Fe3O4

Structure[edit]

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]

Occurrence in nature[edit]

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.[4]

Uses[edit]

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 for filtering phosphates from home aquaria.

References[edit]

  1. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
  2. ^ a b c Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0080379419. 
  3. ^ a b c Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford University Press ISBN 0-19-855370-6
  4. ^ Science Jan 2012

External links[edit]