Copper sulfide

Copper sulfides describe a family of chemical compounds and minerals with the formula Cu_xS_y. Both minerals and synthetic materials comprise these compounds. Some copper sulfides are economically important ores.

Prominent copper sulfide minerals include Cu₂S (chalcocite) and CuS (covellite). In the mining industry, the minerals bornite or chalcopyrite, which consist of mixed copper-iron sulfides, are often referred to as "copper sulfides". In chemistry, a "binary copper sulfide" is any binary chemical compound of the elements copper and sulfur. Whatever their source, copper sulfides vary widely in composition with 0.5 ≤ Cu/S ≤ 2, including numerous non-stoichiometric compounds.

Known copper sulfides

The naturally occurring mineral binary compounds of copper and sulfur are listed below. There are probably more yet to be discovered, for example investigations of "blaubleibender covellite" (blue remaining covellite) formed by natural leaching of covellite (CuS) indicate that there are other metastable Cu-S phases still to be fully characterised.^[1]

• CuS₂, villamaninite^[2] or (Cu,Ni,Co,Fe)S₂^[3]
• CuS, covellite ^[2], copper monosulfide
• Cu₉S₈ (Cu_1.12S), yarrowite^[4]
• Cu₃₉S₂₈ (Cu_1.39S) spionkopite^[4]
• Cu₈S₅ (Cu_1.6S), geerite^[5]
• Cu₇S₄ (Cu_1.75S), anilite^[2]
• Cu₉S₅ (Cu_1.8S), digenite^[2]
• Cu₃₁S₁₆ (Cu_1.96S), djurleite^[2]
• Cu₂S, chalcocite^[2]

Classes of copper sulfides

Copper sulfides can be classified into three groups:

Monosulfides, 1.6 ≤ Cu/S ≤ 2: their crystal structures consist of isolated sulfide anions that are closely related to either hcp or fcc lattices, without any direct S-S bonds. The copper ions are distributed in a complicated manner over interstitial sites with both trigonal as well as distorted tetrahedral coordination and are rather mobile. Therefore, this group of copper sulfides shows ionic conductivity at slightly elevated temperatures. In addition, the majority of its members are semiconductors.

Mixed monosulfide and disulfide compounds of copper contain both monosulfide (S²⁻) as well as disulfide (S₂)ⁿ⁻ anions. Their crystal structures usually consist of alternating hexagonal layers of monosulfide and disulfide anions with Cu cations in trigonal and tetrahedral interstices. CuS, for example, can be written as Cu₃(S₂)S. Several nonstoichiometric compounds with Cu:S ratios between 1.0 and 1.4 also contain both monosulfide as well as disulfide ions. Depending on their composition, these copper sulfides are either semiconductors or metallic conductors.

At very high pressures, a copper disulfide, CuS₂, can be synthesized. Its crystal structure is analogous to that of pyrite, with all sulfur atoms occurring as S-S units. Copper disulfide is a metallic conductor due to the incomplete occupancy of the sulfur p band.Different stoichiometric composition can be obtained by changing the red-ox atmosphere of the synthetic environment.[6]

Oxidation states of copper and sulfur

The bonding in copper sulfides cannot be correctly described in terms of a simple oxidation state formalism because the Cu-S bonds are somewhat covalent rather than ionic in character, and have a high degree of delocalization resulting in complicated electronic band structures. Although many textbooks (e.g. ^[6]) give the mixed valence formula (Cu⁺)₂(Cu²⁺)(S^2–)(S₂)^2– for CuS, X-ray photoelectron spectroscopic data give strong evidence that, in terms of the simple oxidation state formalism, all the known copper sulfides should be considered as purely monovalent copper compounds, and more appropriate formulae would be (Cu⁺)₃(S^2–)(S₂)^– for CuS, and (Cu⁺)(S₂)⁻ for CuS₂, respectively.^{[7][8] [9][10]} Further evidence that the assignment of the so-called "valence hole" should be to the S₂ units in these two formulae is the length of the S-S bonds, which are significantly shorter in CuS (0.207 nm) and CuS₂ (0.203 nm) than in the "classical" disulfide Fe²⁺(S₂)²⁻ (0.218 nm). This bond length difference has been ascribed to the higher bond order in (S-S)⁻ compared to (S-S)²⁻ due to electrons being removed from a π* antibonding orbital.^[8] NMR studies on CuS show that there are two distinct species of copper atom, one with a more metallic nature than the other.^[11] and this apparent discrepancy with the X-ray photo-electron spectrum data simply highlights the problem that NMR has in assigning oxidation states in a mixed-valence compound. The issue of the valence of copper in sulfides (as well as selenides an tellurides) continues to be revisited in the literature. A good example is a 2009 study of the ternary compound CuCo₂S₄^[12] (a spinel mineral known as carrollite) that "was undertaken primarily to establish unequivocally the oxidation state of the Cu in the mineral" and concluded "that the experimental and simulated Cu L2,3 absorption spectra established an unequivocal oxidation state of CuI in the carrollite bulk".

References

• J.C.W. Folmer Holes in the valence band of copper chalcogenides Thesis 1981 Groningen State University (Neth).

1. ^ Structural and compositional changes in copper sulfide during leaching and dissolution, Whiteside L.S, Goble R.J, The Canadian Mineralogist; (1986);. 24; 2; 247-258
2. ^ ^{a b c d e f} Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6
3. ^ http://rruff.geo.arizona.edu/doclib/hom/villamaninite.pdf Handbook of Mineralogy
4. ^ ^{a b} Copper sulfides from Alberta; yarrowite Cu₉S₈ and spionkopite Cu₃₉S₂₈ R. J. Goble, The Canadian Mineralogist; (1980); 18; 4; 511-518
5. ^ Geerite, Cu_1.60S, a new copper sulfide from Dekalb Township, New York, Goble R.J., Robinson G.,The Canadian Mineralogist;(1980),18,4,519-523
6. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Oxford: Butterworth-Heinemann. ISBN 0080379419. 
7. ^ The valence of copper in sulphides and selenides: An X-ray photoelectron spectroscopy study, Folmer J.C.W., Jellinek F., Journal of the Less Common Metals, 76, 1-2, ( 1980), 153-162, doi:10.1016/0022-5088(80)90019-3
8. ^ ^{a b} The electronic structure of pyrites, particularly CuS₂ and Fe1−xCu_xSe₂: An XPS and Mössbauer study, Folmer J.C.W., Jellinek F., Calis G.H.M, Journal of Solid State Chemistry, 72, 1, (1988),137-144, doi:10.1016/0022-4596(88)90017-5
9. ^ Siew Wei Goh, Buckley A.N., Lamb R.N: Copper(II) sulfide?, Min. Eng.,19', 204 (2006), doi:10.1016/j.mineng.2005.09.003
10. ^ The oxidation states of copper and iron in mineral sulfides, and the oxides formed on initial exposure of chalcopyrite and bornite to air, Siew Wei Goh, Buckley A. N. Lamb R.N., Rosenberg R. A., Moran D., Geochimica et Cosmochimica Acta, 70, 9, 2006, 2210-2228, doi:10.1016/j.gca.2006.02.007
11. ^ ⁶³Cu NMR studies of copper sulfide Shin-hachiro Saito, Hideki Kishi, Kohji Nié, Hisakazu Nakamaru, Fumihiko Wagatsuma, Takeshi Shinohara, Phys. Rev. B 55, (1997), 21, 14527 - 14535 doi:10.1103/PhysRevB.55.14527
12. ^ Electronic environments in carrollite, CuCo2S4, determined by soft X-ray photoelectron and absorption spectroscopy
    Alan N. Buckleya, , , William M. Skinnerb, Sarah L. Harmerb, Allan Pringc and Liang-Jen Fand
    Geochimica et Cosmochimica Acta Volume 73, Issue 15, 1 August 2009, Pages 4452-4467

See also

• Copper(I) sulfide
• Copper(II) sulfide

External links

• Copper sulfides mineral information and data