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Chromium(II) sulfide
Identifiers
ChemSpider
InChI=1S/Cr.S/q+2;-2
Key: LXEAUGDQDABWTN-UHFFFAOYSA-N
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).
Chemical compound
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 H2 S, reducing
chromium(III) sulfide with
hydrogen , or by
double replacement reaction of
lithium sulfide with
chromium(II) chloride .
[5]
Cr
+
S
⟶
CrS
{\displaystyle {\ce {Cr + S -> CrS}}}
Cr
+
H
2
S
⟶
CrS
+
H
2
{\displaystyle {\ce {Cr + H2S -> CrS + H2}}}
2
CrCl
3
+
3
H
2
S
⟶
2
CrS
+
S
+
6
HCl
{\displaystyle {\ce {2CrCl3 + 3H2S -> 2CrS + S + 6HCl}}}
Cr
2
S
3
+
H
2
⟶
2
CrS
+
H
2
S
{\displaystyle {\ce {Cr2S3 + H2 -> 2CrS + H2S}}}
Li
2
S
+
CrCl
2
⟶
2
LiCl
+
CrS
{\displaystyle {\ce {Li2S + CrCl2 -> 2LiCl + CrS}}}
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 ]
2
CrS
+
7
O
2
⟶
2
Cr
2
O
3
+
4
SO
2
{\displaystyle {\ce {2CrS + 7O2 -> 2Cr2O3 + 4SO2}}}
References
^ 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 .
^ Wiberg, Egon; Holleman, A. F.; Wiberg, Nils (2001).
Inorganic Chemistry .
Academic Press . p. 1372.
ISBN
978-0-12-352651-9 . Retrieved 1 November 2021 .
^ 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 .
^ 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 .
^ 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 .
^ 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 .
^ Riedel, Erwin; Janiak, Christoph (2011). Anorganische Chemie (in German). Walter de Gruyter. p. 732.
ISBN
978-3-11-022566-2 .
^ 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 .
^ Macintyre, Jane E. (23 July 1992).
Dictionary of Inorganic Compounds .
CRC Press . p. 3082.
ISBN
978-0-412-30120-9 . Retrieved 1 November 2021 .
Chromium(0) Organochromium(0) compounds
Chromium(I) Organochromium(I) compounds
Chromium(II) Organochromium(II) compounds
Chromium(II, III) Chromium(III) Chromium(IV) Chromium(V)
Chromium(VI)
Polyatomic ion