Copper monosulfide

Copper monosulfide
Names
IUPAC name
Copper sulfide
Other names
Covellite
Copper(II) sulfide
Cupric sulfide
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.013.884 Edit this at Wikidata
EC Number
  • 215-271-2
RTECS number
  • GL8912000
UNII
  • InChI=1S/Cu.S checkY
    Key: BWFPGXWASODCHM-UHFFFAOYSA-N checkY
  • InChI=1/Cu.S/rCuS/c1-2
    Key: BWFPGXWASODCHM-BLKBWTQCAT
  • [Cu]=S
Properties
CuS
Molar mass 95.611 g/mol
Appearance black powder or lumps
Density 4.76 g/cm3
Melting point above 500 °C (932 °F; 773 K) (decomposes)[2]
0.000033 g/100 ml (18 °C)
6 x 10−37[1]
Solubility soluble in HNO3, NH4OH, KCN
insoluble in HCl, H2SO4
-2.0·10−6 cm3/mol
1.45
Structure
hexagonal
Hazards
GHS labelling:
GHS09: Environmental hazard
H413
P273, P501
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 1 mg/m3 (as Cu)[3]
REL (Recommended)
 TWA 1 mg/m3 (as Cu)[3]
IDLH (Immediate danger)
 TWA 100 mg/m3 (as Cu)[3]
Related compounds
Other anions
 Copper(II) oxide
Other cations
 zinc 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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Copper monosulfide is a chemical compound of copper and sulfur. It was initially thought to occur in nature as the dark indigo blue mineral covellite. However, it was later shown to be rather a cuprous compound, formula Cu3S(S2).[4] CuS is a moderate conductor of electricity.[5] A black colloidal precipitate of CuS is formed when hydrogen sulfide, H2S, is bubbled through solutions of Cu(II) salts.[6] It is one of a number of binary compounds of copper and sulfur (see copper sulfide for an overview of this subject), and has attracted interest because of its potential uses in catalysis[7] and photovoltaics.[8]

  1. ^ Rollie J. Myers (1986). "The new low value for the second dissociation constant for H2S: Its history, its best value, and its impact on the teaching of sulfide equilibria". J. Chem. Educ. 63 (8): 687. Bibcode:1986JChEd..63..687M. doi:10.1021/ed063p687.
  2. ^ Blachnik, R.; Müller, A. (2000). "The formation of Cu2S from the elements I. Copper used in form of powders". Thermochimica Acta. 361 (1–2): 31–52. doi:10.1016/S0040-6031(00)00545-1.
  3. ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH).
  4. ^ Liang, W., Whangbo, M.H. (1993) Conductivity anisotropy and structural phase transition in Covellite CuS Solid State Communications, 85(5), 405-408
  5. ^ Wells A.F. (1962) Structural Inorganic Chemistry 3d edition Oxford University Press
  6. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  7. ^ Kuchmii, S.Y.; Korzhak A.V.; Raevskaya A.E.; Kryukov A.I. (2001). "Catalysis of the Sodium Sulfide Reduction of Methylviologene by CuS Nanoparticles". Theoretical and Experimental Chemistry. 37 (1). New York: Springer: 36–41. doi:10.1023/A:1010465823376. S2CID 91893521.
  8. ^ Mane, R.S.; Lokhande C.D. (June 2000). "Chemical deposition method for metal chalcogenide thin films". Materials Chemistry and Physics. 65 (1): 1–31. doi:10.1016/S0254-0584(00)00217-0.