Chemistry:Chromium(II) sulfide

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Chromium(II) sulfide
CrS.png
Identifiers
3D model (JSmol)
ChemSpider
Properties
CrS
Molar mass 84.061 g/mol
Appearance black crystals
Melting point 1,550 °C (2,820 °F; 1,820 K)
insoluble
Related compounds
Related compounds
 Chromium(III) sulfide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references
Tracking categories (test):

Chromium(II) sulfide is an inorganic compound of chromium and sulfur with the chemical formula CrS.[1][2][3] The compound forms black hexagonal crystals, insoluble in water.[4]

Synthesis

Chromium(II) sulfide may be formed by reaction of chromium metal with sulfur or hydrogen sulfide at high temperature. It may also be formed by reacting chromium(III) chloride with H2S, reducing chromium(III) sulfide with hydrogen, or by double replacement reaction of lithium sulfide with chromium(II) chloride.[5]

[math]\ce{ Cr + S -> CrS }[/math]
[math]\ce{ Cr + H2S -> CrS + H2 }[/math]
[math]\ce{ 2CrCl3 + 3H2S -> 2CrS + S + 6HCl }[/math]
[math]\ce{ Cr2S3 + H2 -> 2CrS + H2S }[/math]
[math]\ce{ Li2S + CrCl2 -> 2LiCl + CrS }[/math]

Physical properties

Chromium(II) sulfide forms black paramagnetic crystals of two crystalline modifications:[6]

  • α-CrS, superstructured phase, hexagonal system, cell parameters a = 1.200 nm, c = 1.152 nm.
  • β-CrS, monoclinic system, cell parameters a = 0.594 nm, b = 0.341 nm, c = 0.563 nm, β = 91.73°.

Chromium(II) sulfide is a semiconductor,[7][8] and is also used as a catalyst.[9]

Chemical properties

Chromium(II) sulfide slowly oxidizes in air:[citation needed]

[math]\ce{ 2CrS + 7O2 -> 2Cr2O3 + 4SO2 }[/math]

References

  1. ↑ Bretherick, L. (27 October 2016) (in en). Bretherick's Handbook of Reactive Chemical Hazards. Elsevier. p. 1074. ISBN 978-1-4831-6250-8. https://books.google.com/books?id=4_PJCgAAQBAJ&dq=Chromium+(II)+sulfide+CrS&pg=PA1074. Retrieved 1 November 2021. 
  2. ↑ Wiberg, Egon; Holleman, A. F.; Wiberg, Nils (2001) (in en). Inorganic Chemistry. Academic Press. p. 1372. ISBN 978-0-12-352651-9. https://books.google.com/books?id=Mtth5g59dEIC&dq=Chromium+(II)+sulfide+CrS&pg=PA1377. Retrieved 1 November 2021. 
  3. ↑ Sr, Richard J. Lewis (13 June 2008) (in en). Hazardous Chemicals Desk Reference. John Wiley & Sons. p. 670. ISBN 978-0-470-18024-2. https://books.google.com/books?id=WZeBDwAAQBAJ&dq=Chromium+(II)+sulfide&pg=PA670. Retrieved 1 November 2021. 
  4. ↑ Lide, David R. (26 June 2006) (in en). 1998 Freshman Achievement Award. CRC Press. p. 6-111. ISBN 978-0-8493-0594-8. https://books.google.com/books?id=lFjg0L-uOxoC&dq=Chromium+(II)+sulfide&pg=SA6-PA111. Retrieved 1 November 2021. 
  5. ↑ Wadhawan, Amar R.; Livi, Kenneth J.; Stone, Alan T.; Bouwer, Edward J. (2015-03-17). "Influence of oxygenation on chromium redox reactions with manganese sulfide (MnS(s))". Environmental Science & Technology 49 (6): 3523–3531. doi:10.1021/es5057165. ISSN 1520-5851. PMID 25688449. 
  6. ↑ PubChem (2002). "Chromium sulfide (CrS)" (in en). PubChem (National Library of Medicine) 40 (1): 24–26. PMID 11955372. https://pubchem.ncbi.nlm.nih.gov/compound/11955372. Retrieved 2022-09-04. 
  7. ↑ Riedel, Erwin; Janiak, Christoph (2011) (in German). Anorganische Chemie. Walter de Gruyter. p. 732. ISBN 978-3-11-022566-2. 
  8. ↑ Holleman, A. F.; Wiberg, E.; Wiberg, N. (1995) (in German). Lehrbuch der Anorganischen Chemie. 101. Auflage.. Walter de Gruyter. p. 1451. ISBN 3-11-012641-9. 
  9. ↑ Macintyre, Jane E. (23 July 1992) (in en). Dictionary of Inorganic Compounds. CRC Press. p. 3082. ISBN 978-0-412-30120-9. https://books.google.com/books?id=9eJvoNCSCRMC&dq=Chromium+(II)+sulfide+CrS&pg=PA3082. Retrieved 1 November 2021. 



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