Back كبريتيد النحاس الثنائي Arabic پاخیر مونوسولفید AZB Sulfur de coure(II) Catalan Sulfid měďnatý Czech Kupfer(II)-sulfid German Sulfuro de cobre(II) Spanish مس مونوسولفید Persian Kuparisulfidi Finnish Monosulfure de cuivre French कापर(II) सल्फाइड Hindi

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 Cu+3S(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.
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