Antimony pentasulfide
Names
Other names
Antimony red
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.013.869 Edit this at Wikidata
EC Number
  • 215-255-5
UNII
  • InChI=1S/5S.2Sb checkY
    Key: PPKVREKQVQREQD-UHFFFAOYSA-N checkY
  • S=[Sb](=S)S[Sb](=S)=S
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:
GHS02: FlammableGHS07: Exclamation markGHS09: Environmental hazard
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)
 TWA 0.5 mg/m3 (as Sb)[1]
REL (Recommended)
 TWA 0.5 mg/m3 (as Sb)[1]
Related compounds
Related compounds
 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

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

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

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

  1. ^ a b NIOSH Pocket Guide to Chemical Hazards. "#0036". National Institute for Occupational Safety and Health (NIOSH).
  2. ^ Arnold F. Holleman, Nils Wiberg: Lehrbuch der Anorganischen Chemie, 102nd edition, de Gruyter, Berlin 2007, p. 849, ISBN 978-3-11-017770-1.
  3. ^ Strem MSDS
  4. ^ 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.
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