Iron(II) oxide

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Iron(II) oxide
Iron(II) oxide
Manganese(II)-oxide-xtal-3D-vdW.png
Identifiers
CAS number1345-25-1 YesY
PubChem14945
ChemSpider14237 YesY
UNIIG7036X8B5H YesY
ChEBICHEBI:50820 YesY
Jmol-3D imagesImage 1
Properties
Molecular formulaFeO
Molar mass71.844 g/mol
Appearanceblack crystals
Density5.745 g/cm3
Melting point1,377 °C (2,511 °F; 1,650 K)[1]
Boiling point3,414 °C (6,177 °F; 3,687 K)
Solubility in waterInsoluble
Solubilityinsoluble in alkali, alcohol
dissolves in acid
Refractive index (nD)2.23
Hazards
MSDSICSC 0793
EU IndexNot listed
Main hazardscan be pyrophoric
NFPA 704
Autoignition temperaturevariable
Related compounds
Other anionsiron(II) fluoride, iron(II) sulfide, iron(II) selenide, iron(II) telluride
Other cationsmanganese(II) oxide, cobalt(II) oxide
Related compoundsIron(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)
 YesY (verify) (what is: YesY/N?)
Infobox references
 
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Iron(II) oxide
Iron(II) oxide
Manganese(II)-oxide-xtal-3D-vdW.png
Identifiers
CAS number1345-25-1 YesY
PubChem14945
ChemSpider14237 YesY
UNIIG7036X8B5H YesY
ChEBICHEBI:50820 YesY
Jmol-3D imagesImage 1
Properties
Molecular formulaFeO
Molar mass71.844 g/mol
Appearanceblack crystals
Density5.745 g/cm3
Melting point1,377 °C (2,511 °F; 1,650 K)[1]
Boiling point3,414 °C (6,177 °F; 3,687 K)
Solubility in waterInsoluble
Solubilityinsoluble in alkali, alcohol
dissolves in acid
Refractive index (nD)2.23
Hazards
MSDSICSC 0793
EU IndexNot listed
Main hazardscan be pyrophoric
NFPA 704
Autoignition temperaturevariable
Related compounds
Other anionsiron(II) fluoride, iron(II) sulfide, iron(II) selenide, iron(II) telluride
Other cationsmanganese(II) oxide, cobalt(II) oxide
Related compoundsIron(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)
 YesY (verify) (what is: YesY/N?)
Infobox references

Iron(II) oxide is the inorganic compound with the formula FeO. Its mineral form is known as wüstite. One of several iron oxides, it is a black-colored powder that is sometimes confused with rust, 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 Fe0.84O to Fe0.95O.[2]

Preparation[edit]

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

FeC2O4 → FeO + CO2 + CO

The procedure is conducted a protective atmosphere to avoid the formation of ferric oxide. A similar procedure can also be used for the synthesis of manganous oxide and stannous oxide.[3][4]

Stoichiometric FeO can be prepared by heating Fe0.95O with metallic iron at 770 °C and 36 kbar.[5]

Reactions[edit]

FeO is thermodynamically unstable below 575 °C, tending to disproportionate 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.[5]

Below 200 K there is a minor change to the structure which changes the symmetry to rhombohedral and samples become antiferromagnetic.[5]

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.[6]

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 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0080379419. 
  3. ^ 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.
  4. ^ Practical Chemistry for Advanced Students, Arthur Sutcliffe, 1930 (1949 Ed.), John Murray - London
  5. ^ a b c Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford University Press ISBN 0-19-855370-6
  6. ^ Science Jan 2012

External links[edit]