Copper(I) thiocyanate

Source: Wikipedia, the free encyclopedia.
Copper(I) thiocyanate

Copper(I) thiocyanate
Names
Other names
Cuprous thiocyanate
Identifiers
ChemSpider
ECHA InfoCard
 100.012.894 Edit this at Wikidata
UNII
Properties
CuSCN
Molar mass 121.628 g/mol[1]
Appearance white powder
Density 2.88 g/cm3[2]
Melting point 1,084[1] °C (1,983 °F; 1,357 K)
8.427·10−7 g/L (20 °C)
1.77×10−13[3]
-48.0·10−6 cm3/mol
Related compounds
Other anions
 Copper(I) iodide, copper(I) cyanide
Other cations
 Ammonium thiocyanate
Potassium thiocyanate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Copper(I) thiocyanate (or cuprous thiocyanate) is a coordination polymer with formula CuSCN. It is an air-stable, white solid used as a precursor for the preparation of other thiocyanate salts.

Structure

At least two

polymorphs have been characterized by X-ray crystallography. They both feature copper(I) in a characteristic tetrahedral coordination geometry. The sulfur end of the SCN- ligand is triply bridging so that the coordination sphere for copper is CuS3N.[2][4]

Synthesis

Copper(I) thiocyanate forms from the spontaneous decomposition of black copper(II) thiocyanate, releasing

sulphurous acid is added and then a soluble thiocyanate is added (preferably slowly, while stirring[7]). Copper(I) thiocyanate is precipitated as a white powder.[8] Alternatively, a thiosulfate
solution may be used as a reducing agent.

Double salts

Copper(I) thiocyanate forms one double salt with the group 1 elements, CsCu(SCN)2. The double salt only forms from concentrated solutions of CsSCN, into which CuSCN dissolves. From less concentrated solutions, solid CuSCN separates reflecting its low solubility.[9] When brought together with potassium, sodium or barium thiocyanate, and brought to crystallisation by concentrating the solution, mixed salts will crystallise out. These are not considered true double salts. As with CsCu (SNC)2, copper(I) thiocyanate separates out when these mixed salts are redissolved or their solutions diluted.[10]

Uses

Copper(I) thiocyanate is a

P-type semiconductor and as a solid-state electrolyte. It is often used in dye-sensitized solar cells. Its hole conductivity is however relatively poor (0.01 S·m−1). This can be improved by various treatments, e.g. exposure to gaseous chlorine or doping with (SCN)2.[12]

CuSCN with NiO act synergically as a smoke suppressant additive in polyvinyl chloride (PVC).

CuSCN precipitated on carbon support can be used for conversion of aryl halides to aryl thiocyanates.[13]

Copper thiocyanate is used in some

cuprous oxide include that the compound is white and a more efficient biocide
.

References

  1. ^ a b "Properties of Copper(I) thiocyanate". Chemspider. Alfa Aesar 40220. Retrieved 5 January 2016.
  2. ^
    doi:10.1107/S0567740882004361
  3. ISBN 978-1138561632
    .
  4. doi:10.1016/S0020-1693(00)81976-3
    .
  5. ISSN 0020-1650
    .
  6. doi:10.1021/ed070p174.3.PDF copy
  7. PMID 5771673.PDF copy
  8. ^ Reece H. Vallance, Douglas F. Twiss and Miss Annie R. Russell (1931). J. Newton Friend (ed.). A text-book of inorganic chemistry, volume VII, part II. Charles Griffin & Company Ltd. p. 282.
  9. ^ H.L.Wells (1902). "On some double and triple thiocyanates". American Chemical Journal. 28: 245–284 (263).
  10. ^ Herbert E. Williams (1915). The chemistry of cyanogen compounds. J. & A. Churchill, London. pp. 202–203.
  11. ISBN 9780080914237
    . Retrieved 14 January 2017.
  12. ISBN 9781849731652
    . Retrieved 14 January 2017.
  13. ISBN 9780471187790
    . Retrieved 14 January 2017.
  14. ^ "Copper in Antifouling". Archived from the original on 2017-04-27. Retrieved 2017-04-25.
  15. ^ V.F. Vetere et al, "Solubility and Toxic Effect of the Cuprous Thiocyanate Antifouling Pigment on Barnacle Larvae", Journal of Coatings Technology, 69:39 (March 1997)
Retrieved from "https://en.wikipedia.org/w/index.php?title=Copper(I)_thiocyanate&oldid=1191385710"