| Names | |
|---|---|
| IUPAC name
Iron(III) sulfide
| |
| Other names
Iron sesquisulfide
Ferric sulfide Diiron trisulfide | |
| Identifiers | |
| ChEBI | |
PubChem CID
|
|
| UNII | |
CompTox Dashboard (EPA)
|
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| Properties | |
| Fe2S3 | |
| Molar mass | 207.90 g/mol [1] |
| Appearance | yellow-green [1] |
| Density | 4.3 g/cm3 [1] |
| Melting point | decomposition [1] |
| 0.0062g/L[1] | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
| |
Iron(III) sulfide, also known as ferric sulfide or sesquisulfide (Fe
2S
3), is one of the several binary iron sulfides. It is a solid, black powder that degrades at ambient temperature.[2]
Reactions
[edit]Fe
2S
3 precipitates from solutions containing its respective ions:[2]
- 2Fe3+ + 3S2− → Fe2S3
The resulting solid decays at a temperature over 20 °C into iron(II) sulfide (FeS) and elemental sulfur:[3]
- Fe2S3 → 2 FeS + S
With hydrochloric acid it decays according to the following reaction equation:[4]
- Fe2S3 + 4 HCl → 2 FeCl2 + 2 H2S + S
Greigite
[edit]Greigite, with the chemical formula Fe2+Fe3+2S4, is a mixed valence compound containing both Fe(III) and Fe(II). It is the sulfur equivalent of the iron oxide magnetite (Fe3O4). As established by X-ray crystallography, the S anions form a cubic close-packed lattice, and the Fe cations occupy both tetrahedral and octahedral sites.[5]
References
[edit]- ^ a b c d e Charles D. Hodgman, Handbook of Chemistry and Physics (1961), p.590
- ^ a b Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 1081. ISBN 978-0-08-037941-8.
- ^ Holleman, Wiberg (2001). Inorganic Chemistry. p. 1451. ISBN 0-12-352651-5.
- ^ H. Roempp, Chemie (1997), S. 1099; ISBN 3-13-734710-6
- ^ Vaughan, D. J.; Craig, J. R. "Mineral Chemistry of Metal Sulfides" Cambridge University Press, Cambridge: 1978. ISBN 0-521-21489-0.
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