Iron(III) sulfide

Short description: Unstable artificial chemical compound

Iron(III) sulfide  Names

IUPAC name

Iron(III) sulfide

Other names

Iron sesquisulfide
Ferric sulfide
Diiron trisulfide

Identifiers

CAS Number

* 12063-27-3 Y

ChEBI |

* CHEBI:75899 N

PubChem CID

* 160957

UNII |

* 003Q5FW7CS Y

Properties

Chemical formula

| Fe2S3
Molar mass | 207.90 g/mol [1]
Appearance  | yellow-green [1]
Density | 4.3 g/cm3 [1]
Melting point | decomposition [1]

Solubility in water

| 0.0062g/L[1]

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

N verify (what is YN ?)
Infobox references

Iron(III) sulfide, also known as ferric sulfide or sesquisulfide (Fe2S3), is one of the several binary iron sulfides. It is a solid, black powder that degrades at ambient temperature.[2]

## Reactions

Fe2S3 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

Greigite, with the chemical formula Fe2+
Fe3+

4, 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

1. ↑ 1.0 1.1 1.2 1.3 1.4 Charles D. Hodgman, Handbook of Chemistry and Physics (1961), p.590
2. ↑ 2.0 2.1 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 1081. ISBN 978-0-08-037941-8.
3. ↑ Holleman, Wiberg (2001). Inorganic Chemistry. p. 1451. ISBN 0-12-352651-5.
4. ↑ H. Roempp, Chemie (1997), S. 1099; ISBN 3-13-734710-6
5. ↑ Vaughan, D. J.; Craig, J. R. "Mineral Chemistry of Metal Sulfides" Cambridge University Press, Cambridge: 1978. ISBN 0-521-21489-0.

* v
* t
* e

Iron compounds

Fe(-II)|

* Na2Fe(CO)4

Fe(0)|

* Fe(CO)5
* Fe2(CO)9
* Fe3(CO)12
* Fe(CO)3CH3COC2H2C6H6

Fe(I)|

* FeH

| Organoiron(I) compounds|

* (C5H5FeCO)2(CO)2

|

Fe(0,II)|

* Fe3C

Fe(II)|

* FeBr2
* FeCl2
* FeF2
* FeI2
* FeH2
* FeMoO4
* FeO
* Fe(OH)2
* FeS
* FeSO4
* FeSe
* FeSeO4
* FeSi2
* FeTiO3
* FeCO3
* FeC2O4
* Fe(C2H3O2)2
* Fe(C3H5O3)2
* FeC6H6O7
* FeC12H22O14
* Fe2CrO4
* Fe3(PO4)2
* H2Fe(CO)4
* Fe(HCO3)2
* Mg2FeH6

| Organoiron(II) compounds|

* Fe(C5H5)2
* Fe(C5H4P(C6H5)2)2
* C4H4Fe(CO)3
* C4H6Fe(CO)3

|

Fe(0,III)|

* Fe3P

Fe(II,III)|

* Fe3O4
* Fe3S4

Fe(III)|

* FeBr3
* FeCl3
* FeF3
* FeI3
* Fe(NO3)3
* Fe(acac)3
* FeOCl
* FeO(OH)
* FePO4
* Fe4(P2O7)3
* Fe2(CrO4)3
* Fe2(C2O4)3
* Fe2O3
* Fe2S3
* Fe2(SO4)3
* FeBO3
* FeB

| Organoiron(III) compounds|

* Fe(C5H5)2BF4
* C6H8O7⋅xFe3+⋅yNH3

|

Fe(VI)|

* K2FeO4
* BaFeO4

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