| Names | |
|---|---|
| Other names
Antimony red
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| Identifiers | |
3D model (JSmol)
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| ChEBI | |
| ChemSpider | |
| ECHA InfoCard | 100.013.869 |
| EC Number |
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PubChem CID
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| UNII | |
CompTox Dashboard (EPA)
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| Properties | |
| Sb2S5 | |
| Molar mass | 403.82 g·mol−1 |
| Appearance | Red powder |
| Density | 4.12 g/cm 3 |
| Melting point | 135 °C (275 °F; 408 K) (decomposes) |
| insoluble | |
| Solubility | soluble in HCl, alkalis, ammonium hydrosulfide |
| Pharmacology | |
| R05CA07 (WHO) | |
| Hazards | |
| GHS labelling: | |
  
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| Warning | |
| H228, H302, H332, H411 | |
| P210, P240, P241, P261, P264, P270, P271, P273, P280, P301+P312, P304+P312, P304+P340, P312, P330, P370+P378, P391, P501 | |
| Flash point | flammable |
| NIOSH (US health exposure limits): | |
PEL (Permissible)
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TWA 0.5 mg/m3 (as Sb)[1] |
REL (Recommended)
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TWA 0.5 mg/m3 (as Sb)[1] |
| Related compounds | |
Related compounds
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Antimony(III) sulfide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Antimony pentasulfide is an inorganic compound of antimony and sulfur, also known as antimony red. It is a nonstoichiometric compound with a variable composition. Its structure is unknown.[2] Commercial samples are contaminated with sulfur, which may be removed by washing with carbon disulfide in a Soxhlet extractor.
Production[edit]
Antimony pentasulfide can be produced by the reaction of antimony with sulfur at a temperature from 250 to 400 °C in an inert atmosphere.
Uses[edit]
It may be used as a red pigment and is one possible precursor to Schlippe's salt, Na3SbS4·9H2O, which can be prepared according to the equation:
- 3 Na2S + Sb2S5 + 9 H2O → 2 Na3SbS4·9H2O
It is also used in the vulcanization of rubber to produce red rubber.
Physical chemistry[edit]
Like many sulfides, this compound liberates hydrogen sulfide upon treatment with strong acids such as hydrochloric acid.[3]
- 6 HCl + Sb2S5 → 2 SbCl3 + 3 H2S + 2 S
Analysis by Mössbauer spectroscopy indicates that this compound is a derivative antimony(III),[4] explaining the production of antimony(III) chloride, rather than antimony(V) chloride, upon acidification. It is, therefore, not analogous to the phosphorus(V) compound phosphorus pentasulfide.
References[edit]
- ^ a b NIOSH Pocket Guide to Chemical Hazards. "#0036". National Institute for Occupational Safety and Health (NIOSH).
- ^ Arnold F. Holleman, Nils Wiberg: Lehrbuch der Anorganischen Chemie, 102nd edition, de Gruyter, Berlin 2007, p. 849, ISBN 978-3-11-017770-1.
- ^ Strem MSDS
- ^ G. G. Long; J. G. Stevens; L. H. Bowen; S. L. Ruby (1969). "The oxidation number of antimony in antimony pentasulfide". Inorganic and Nuclear Chemistry Letters. 5 (1): 21–25. doi:10.1016/0020-1650(69)80231-X.