Cadmium sulfide

Cadmium sulfide
Names
Other names
Cadmium(II) sulfide,
Greenockite
Hawleyite
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.013.771
EC Number 215-147-8
RTECS number EV3150000
UNII
UN number 2570
Properties
CdS
Molar mass 144.47 g·mol−1
Appearance Yellow-orange to brown solid.
Density 4.826 g/cm3, solid.
Melting point 1,750 °C (3,180 °F; 2,020 K) 10 MPa
Boiling point 980 °C (1,800 °F; 1,250 K) (sublimation)
insoluble[1]
Solubility soluble in acid
very slightly soluble in ammonium hydroxide
-50.0·10−6 cm3/mol
2.529
Structure
Hexagonal, Cubic
Thermochemistry
65 J·mol−1·K−1[2]
−162 kJ·mol−1[2]
Hazards
Safety data sheet ICSC 0404
Carc. Cat. 2
Muta. Cat. 3
Repr. Cat. 3
Toxic (T)
Dangerous for the environment (N)
R-phrases (outdated) R45, R22, R48/23/25, R62, R63, R68, R50/53
S-phrases (outdated) S53, S45, S61
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gas Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
0
3
0
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
7080 mg/kg (rat, oral)
US health exposure limits (NIOSH):
PEL (Permissible)
 [1910.1027] TWA 0.005 mg/m3 (as Cd)[3]
REL (Recommended)
 Ca[3]
IDLH (Immediate danger)
 Ca [9 mg/m3 (as Cd)][3]
Related compounds
Other anions
 Cadmium oxide
Cadmium selenide
Other cations
 Zinc sulfide
Mercury 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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Infobox references

Cadmium sulfide is the inorganic compound with the formula CdS. Cadmium sulfide is a yellow solid.[4] It occurs in nature with two different crystal structures as the rare minerals greenockite and hawleyite, but is more prevalent as an impurity substituent in the similarly structured zinc ores sphalerite and wurtzite, which are the major economic sources of cadmium. As a compound that is easy to isolate and purify, it is the principal source of cadmium for all commercial applications.[4] Its vivid yellow color led to its adoption as a pigment for the yellow paint "cadmium yellow" in the 18th century.

Production

Cadmium sulfide can be prepared by the precipitation from soluble cadmium(II) salts with sulfide ion. This reaction has been used for gravimetric analysis and qualitative inorganic analysis.[5]
The preparative route and the subsequent treatment of the product, affects the polymorphic form that is produced (i.e., cubic vs hexagonal). It has been asserted that chemical precipitation methods result in the cubic zincblende form.[6]

Pigment production usually involves the precipitation of CdS, the washing of the solid precipitate to remove soluble cadmium salts followed by calcination (roasting) to convert it to the hexagonal form followed by milling to produce a powder.[7] When cadmium sulfide selenides are required the CdSe is co-precipitated with CdS and the cadmium sulfoselenide is created during the calcination step.[7]

Cadmium sulfide is sometimes associated with sulfate reducing bacteria.[8][9]

Routes to thin films of CdS

Special methods are used to produce films of CdS as components in some photoresistors and solar cells. In the chemical bath deposition method, thin films of CdS have been prepared using thiourea as the source of sulfide anions and an ammonium buffer solution to control pH:[10]

Cd2+ + H2O + (NH2)2CS + 2 NH3 → CdS + (NH2)2CO + 2 NH4+

Cadmium sulfide can be produced using metalorganic vapour phase epitaxy and MOCVD techniques by the reaction of dimethylcadmium with diethyl sulfide:[11]

Cd(CH3)2 + Et2S → CdS + CH3CH3 + C4H10

Other methods to produce films of CdS include

Reactions

Cadmium sulfide can be dissolved in acids.[17]

CdS + 2 HCl → CdCl2 + H2S

When solutions of sulfide containing dispersed CdS particles are irradiated with light hydrogen gas is generated:[18]

H2S → H2 + S ΔHf = +9.4 kcal/mol

The proposed mechanism involves the electron/hole pairs created when incident light is absorbed by the cadmium sulfide[19] followed by these reacting with water and sulfide:[18]

Production of an electron hole pair
CdS + hν → e− + hole+
Reaction of electron
2e− + 2H2O → H2 + 2OH−
Reaction of hole
2hole+ + S2− → S

Structure and physical properties

Cadmium sulfide has, like zinc sulfide, two crystal forms. The more stable hexagonal wurtzite structure (found in the mineral Greenockite) and the cubic zinc blende structure (found in the mineral Hawleyite). In both of these forms the cadmium and sulfur atoms are four coordinate.[20] There is also a high pressure form with the NaCl rock salt structure.[20]

Cadmium sulfide is a direct band gap semiconductor (gap 2.42 eV[19]). The magnitude of its band gap means that it appears coloured.[4]
As well as this obvious property other properties result:

Applications

Pigment

Yellow cadmium sulfide- pigment

CdS is used as pigment in plastics, showing good thermal stability, light and weather fastness, chemical resistance and high opacity.[7] As a pigment, CdS is known as cadmium yellow.[4] (CI pigment yellow 37[31]) About 2000 tons are produced annually as of 1982, representing about 25% of the cadmium processed commercially.[32]

Historical use in art

The general commercial availability of cadmium sulfide from the 1840s led to its adoption by artists, notably Van Gogh, Monet (in his London series and other works) and Matisse (Bathers by a river 1916–1919).[33] The presence of cadmium in paints has been used to detect forgeries in paintings alleged to have been produced prior to the 19th century.[34]

CdS-CdSe solutions

CdS and CdSe form solid solutions. Increasing amounts of cadmium selenide, gives pigments verging toward red, for example CI pigment orange 20 and CI pigment red 108.[31]
Such solid solutions are components of photoresistors (light dependent resistors) sensitive to visible and near infrared light.

Safety

Cadmium sulfide is toxic, especially when inhaled as dust, and cadmium compounds general are classified as carcinogenic.[35] Problems of biocompatibility have been reported when CdS is used as colors in tattoos.[36]

References

  1. ↑ Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, FL: CRC Press. pp. 4–67; 1363. ISBN 0-8493-0594-2.
  2. 1 2 Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A21. ISBN 0-618-94690-X.
  3. 1 2 3 "NIOSH Pocket Guide to Chemical Hazards #0087". National Institute for Occupational Safety and Health (NIOSH).
  4. 1 2 3 4 Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0-12-352651-5
  5. ↑ Fred Ibbotson (2007), The Chemical Analysis of Steel-Works' Materials,Read Books, ISBN 1-4067-8113-4
  6. ↑ Paul Klocek (1991), Handbook of Infrared Optical Materials, CRC Press ISBN 0-8247-8468-5
  7. 1 2 3 Hugh MacDonald Smith (2002). High Performance Pigments. Wiley-VCH. ISBN 3-527-30204-2.
  8. ↑ Larry L. Barton 1995 Sulfate reducing bacteria, Springer, ISBN 0-306-44857-2
  9. ↑ Sweeney, Rozamond Y.; Mao, Chuanbin; Gao, Xiaoxia; Burt, Justin L.; Belcher, Angela M.; Georgiou, George; Iverson, Brent L. (2004). "Bacterial Biosynthesis of Cadmium Sulfide Nanocrystals". Chemistry & Biology. 11 (11): 1553–9. PMID 15556006. doi:10.1016/j.chembiol.2004.08.022.
  10. ↑ Oladeji, I.O.; Chow, L. (1997). "Optimization of Chemical Bath Deposited Cadmium Sulfide". J. Electrochem. Soc. 144: 7.
  11. ↑ Uda, H; Yonezawa, H; Ohtsubo, Y; Kosaka, M; Sonomura, H (2003). "Thin CdS films prepared by metalorganic chemical vapor deposition". Solar Energy Materials and Solar Cells. 75 (1–2): 219. doi:10.1016/S0927-0248(02)00163-0.
  12. ↑ Reisfeld, R (2002). "Nanosized semiconductor particles in glasses prepared by the sol–gel method: their optical properties and potential uses". Journal of Alloys and Compounds. 341 (1–2): 56. doi:10.1016/S0925-8388(02)00059-2.
  13. ↑ Moon, B; Lee, J; Jung, H (2006). "Comparative studies of the properties of CdS films deposited on different substrates by R.F. sputtering". Thin Solid Films. 511-512: 299. Bibcode:2006TSF...511..299M. doi:10.1016/j.tsf.2005.11.080.
  14. ↑ Goto, F; Shirai, Katsunori; Ichimura, Masaya (1998). "Defect reduction in electrochemically deposited CdS thin films by annealing in O2". Solar Energy Materials and Solar Cells. 50 (1–4): 147. doi:10.1016/S0927-0248(97)00136-0.
  15. ↑ U.S. Patent 4,086,101 Photovoltaic cells, J.F. Jordan, C.M. Lampkin Issue date: April 25, 1978
  16. ↑ U.S. Patent 3,208,022, High performance photoresistor, Y.T. Sihvonen, issue date: September 21, 1965
  17. ↑ Wanrooij, P. H. P.; Agarwal, U. S.; Meuldijk, J.; Kasteren, J. M. N. van; Lemstra, P. J. (2006). "Extraction of CdS pigment from waste polyethylene". Journal of Applied Polymer Science. 100 (2): 1024. doi:10.1002/app.22962.
  18. 1 2 Mario Schiavello (1985) Photoelectrochemistry, Photocatalysis, and Photoreactors: Fundamentals and Developments Springer ISBN 90-277-1946-2
  19. 1 2 3 D. Lincot, Gary Hodes Chemical Solution Deposition of Semiconducting and Non-Metallic Films: Proceedings of the International Symposium The Electrochemical Society, 2006 ISBN 1-56677-433-0
  20. 1 2 Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6
  21. ↑ Antonio Luque, Steven Hegedus, (2003), Handbook of Photovoltaic Science and Engineering John Wiley and Sons ISBN 0-471-49196-9
  22. ↑ Reynolds, D.; Leies, G.; Antes, L.; Marburger, R. (1954). "Photovoltaic Effect in Cadmium Sulfide". Physical Review. 96 (2): 533. Bibcode:1954PhRv...96..533R. doi:10.1103/PhysRev.96.533.
  23. ↑ C. Fouassier,(1994), Luminescence in Encyclopedia of Inorganic Chemistry, John Wiley & Sons ISBN 0-471-93620-0
  24. ↑ Minkus, Wilfred (1965). "Temperature Dependence of the Pyroelectric Effect in Cadmium Sulfide". Physical Review. 138 (4A): A1277. Bibcode:1965PhRv..138.1277M. doi:10.1103/PhysRev.138.A1277.
  25. ↑ Smith, Roland (1957). "Low-Field Electroluminescence in Insulating Crystals of Cadmium Sulfide". Physical Review. 105 (3): 900. Bibcode:1957PhRv..105..900S. doi:10.1103/PhysRev.105.900.
  26. ↑ Akimov, Yu A; Burov, A A; Drozhbin, Yu A; Kovalenko, V A; Kozlov, S E; Kryukova, I V; Rodichenko, G V; Stepanov, B M; Yakovlev, V A (1972). "KGP-2: AN ELECTRON-BEAM-PUMPED CADMIUM SULFIDE LASER". Soviet Journal of Quantum Electronics. 2 (3): 284. Bibcode:1972QuEle...2..284A. doi:10.1070/QE1972v002n03ABEH004443.
  27. ↑ Agarwal, Ritesh; Barrelet, Carl J.; Lieber, Charles M. (2005). "Lasing in Single Cadmium Sulfide Nanowire Optical Cavities". Nano Letters. 5 (5): 917–920. Bibcode:2005NanoL...5..917A. PMID 15884894. arXiv:cond-mat/0412144v1 Freely accessible. doi:10.1021/nl050440u.
  28. ↑ H. Zhao et al, "The effect of impurities on the doping and VOC of CdTe/CdS thin film solar cells", Thin Solid Films, Vol. 517, No. 7 (2009) pp. 2365-2369, doi:10.1016/j.tsf.2008.11.041
  29. ↑ P.K. Weimar, "The TFT a new thin-film transistor", Proc. IRE, Vol. 50, No. 6 (1962) pp. 1462-1469, doi:10.1109/JRPROC.1962.288190
  30. ↑ Zhang, Jun (24 January 2013). "Laser cooling of a semiconductor by 40 kelvin.". Nature. 493 (7433): 504–508. doi:10.1038/nature11721.
  31. 1 2 R. M. Christie 2001 Colour Chemistry, p. 155 Royal Society of Chemistry ISBN 0-85404-573-2
  32. ↑ Karl-Heinz Schulte-Schrepping, Magnus Piscator "Cadmium and Cadmium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, 2007 Wiley-VCH, Weinheim. doi:10.1002/14356007.a04_499.
  33. ↑ Sidney Perkowitz, 1998, Empire of Light: A History of Discovery in Science and Art Joseph Henry Press, ISBN 0-309-06556-9
  34. ↑ W. Stanley Taft, James W. Mayer, Richard Newman, Peter Kuniholm, Dusan Stulik (2000) The Science of Paintings, Springer, ISBN 0-387-98722-3
  35. ↑ CDC International Chemical Safety Card - Cadmium Sulfide
  36. ↑ Bjornberg, A (Sep 1963). "Reactions to light in yellow tattoos from cadmium sulfide". Arch Dermatol. 88: 267–71. PMID 14043617. doi:10.1001/archderm.1963.01590210025003.
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