Chromium(II) sulfide

Chromium(II) sulfide

Identifiers
CAS Number	12018-06-3
3D model (JSmol)	Interactive image
ChemSpider	10129648
PubChem CID	11955372
CompTox Dashboard (EPA)	DTXSID10923256
InChI InChI=1S/Cr.S/q+2;-2 Key: LXEAUGDQDABWTN-UHFFFAOYSA-N
SMILES [S-2].[Cr+2]
Properties
Chemical formula	CrS
Molar mass	84.061 g/mol
Appearance	Black crystals
Melting point	1,550 °C (2,820 °F; 1,820 K)
Solubility in water	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

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] It is a semiconductor, ^{[5] [6]} and is also used as a catalyst. ^[7]

Structure

Chromium(II) sulfide forms black paramagnetic crystals of two crystalline modifications: ^[8]

• 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°.

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. ^[9]

Cr + S → CrS

Cr + H₂S → CrS + H₂

2 CrCl₃ + 3 H₂S → 2 CrS + S + 6 HCl

Cr₂S₃ + H₂ → 2 CrS + H₂S

Li₂S + CrCl₂ → 2 LiCl + CrS

Reactions

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

2 CrS + 7 O₂ → 2 Cr₂O₃ + 4 SO₂

References

1. Bretherick, L. (27 October 2016). Bretherick's Handbook of Reactive Chemical Hazards. Elsevier. p. 1074. ISBN   978-1-4831-6250-8 . Retrieved 1 November 2021.
2. Wiberg, Egon; Holleman, A. F.; Wiberg, Nils (2001). Inorganic Chemistry. Academic Press. p. 1372. ISBN   978-0-12-352651-9 . Retrieved 1 November 2021.
3. Sr, Richard J. Lewis (13 June 2008). Hazardous Chemicals Desk Reference. John Wiley & Sons. p. 670. ISBN   978-0-470-18024-2 . Retrieved 1 November 2021.
4. Lide, David R. (26 June 2006). 1998 Freshman Achievement Award. CRC Press. p. 6-111. ISBN   978-0-8493-0594-8 . Retrieved 1 November 2021.
5. Riedel, Erwin; Janiak, Christoph (2011). Anorganische Chemie (in German). Walter de Gruyter. p. 732. ISBN   978-3-11-022566-2.
6. Holleman, A. F.; Wiberg, E.; Wiberg, N. (1995). Lehrbuch der Anorganischen Chemie. 101. Auflage (in German). Walter de Gruyter. p. 1451. ISBN   3-11-012641-9.
7. Macintyre, Jane E. (23 July 1992). Dictionary of Inorganic Compounds. CRC Press. p. 3082. ISBN   978-0-412-30120-9 . Retrieved 1 November 2021.
8. PubChem (2002). "Chromium sulfide (CrS)". PubChem . 40 (1). National Library of Medicine: 24–26. PMID   11955372. Archived from the original on 2022-09-04. Retrieved 2022-09-04.
9. 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.