Cadmium sulfide

Cadmium sulfide  | 3D model of the structure of hawleyite | 3D model of the structure of greenockite

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Names
Other names

cadmium(II) sulfide
greenockite
hawleyite
cadmium yellow

Identifiers

CAS Number

* 1306-23-6 Y

3D model (JSmol)

* monomer: Interactive image
* hawleyite: Interactive image
* greenockite: Interactive image
* greenockite: Interactive image

ChEBI |

* CHEBI:50833

ChemSpider |

* 7969586 Y

EC Number |

* 215-147-8

Gmelin Reference

| 13655

PubChem CID

* 14783

RTECS number |

* EV3150000

UNII |

* 057EZR4Z7Q Y

UN number | 2570

InChI

* InChI=1S/Cd.S/q+2;-2 Y

Key: FRLJSGOEGLARCA-UHFFFAOYSA-N Y

* InChI=1/Cd.S/q+2;-2

Key: FRLJSGOEGLARCA-UHFFFAOYAL

SMILES

* monomer: [S-2].[Cd+2]

* hawleyite: [SH+2]12[CdH2-2] [SH+2]3[CdH2-2] [SH+2]([CdH-2]14)[CdH-2]1[S+2]5([CdH-2]38)[Cd-2]26[SH+2]2[CdH-2]([S+2]4)[SH+2]1[CdH2-2] [SH+2]3[CdH-2]2[S+2] [CdH-2]([SH+2]6[CdH-2]([SH+2])[SH+2]68)[SH+2]([CdH2-2]6)[CdH-2]35

* greenockite: [CdH2-2]1[S+2]47[CdH-2]2[S+2] [CdH-2]3[S+2]8([CdH2-2] [SH+2]([CdH2-2]4)[CdH2-2]6)[CdH-2]4[S+2] [CdH-2]5[S+2]6([CdH2-2]6)[Cd-2]78[S+2]78[CdH-2]([SH+2]69)[SH+2]5[CdH2-2] [SH+2]4[CdH-2]7[SH+2]3[CdH2-2] [SH+2]2[CdH-2]8[SH+2]1[CdH2-2]9

* greenockite: [CdH2-2]1[SH+2]([CdH2-2]6)[CdH2-2] [SH+2]7[CdH-2]2[S+2] [Cd-2]3([S+2] [CdH-2]9[S+2]5)[S+2]18[Cd-2]45[S+2] [CdH-2]5[SH+2]6[Cd-2]78[S+2]78[CdH2-2] [SH+2]5[CdH2-2] [S+2]4([CdH2-2] [SH+2]9[CdH2-2]4)[CdH-2]7[S+2]34[CdH2-2] [SH+2]2[CdH2-2]8

Properties

Chemical formula

| 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)

Solubility in water

| insoluble[1]
Solubility | soluble in acid
very slightly soluble in ammonium hydroxide
Band gap | 2.42 eV

Magnetic susceptibility (χ)

| -50.0·10−6 cm3/mol

Refractive index (nD)

| 2.529
Structure

Crystal structure

| Hexagonal, Cubic
Thermochemistry

Std molar
entropy (S ~~o~~ 298)

| 65 J·mol−1·K−1[2]

Std enthalpy of
formation (ΔfH⦵298)

| −162 kJ·mol−1[2]
Hazards
Safety data sheet | ICSC 0404
GHS pictograms |
GHS Signal word | Danger

GHS hazard statements

| H302, H341, H350, H361, H372, H413

GHS precautionary statements

| P201, P202, P260, P264, P270, P273, P281, P301+312, P308+313, P314, P330, P405, P501
NFPA 704 (fire diamond)  |

Flash point | Non-flammable
Lethal dose or concentration (LD, LC):

LD50 (median dose)

| 7080 mg/kg (rat, oral)
NIOSH (US health exposure limits):

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).

Y verify (what is YN ?)
Infobox references

Cadmium sulfide is the inorganic compound with the formula CdS. Cadmium sulfide is a yellow salt.[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.

## Contents

* 1 Production
* 1.1 Routes to thin films of CdS
* 2 Reactions
* 3 Structure and physical properties
* 4 Applications
* 4.1 Pigment
* 4.2 Historical use in art
* 4.3 CdS-CdSe solutions
* 5 Safety
* 6 References
* 7 External links

## 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

* Sol–gel techniques[12]
* Sputtering[13]
* Electrochemical deposition[14]
* Spraying with precursor cadmium salt, sulfur compound and dopant[15]
* Screen printing using a slurry containing dispersed CdS[16]

## 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− \+ h+
Reaction of electron

2e− \+ 2H2O → H2 \+ 2OH−
Reaction of hole

2h+ \+ 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 proximity of its band gap to visible light wavelengths gives it a coloured appearance.[4]
As well as this obvious property other properties result:

* the conductivity increases when irradiated,[19] (leading to uses as a photoresistor)
* when combined with a p-type semiconductor it forms the core component of a photovoltaic (solar) cell and a CdS/Cu2S solar cell was one of the first efficient cells to be reported (1954)[21][22]
* when doped with for example Cu+ ("activator") and Al3+ ("coactivator") CdS luminesces under electron beam excitation (cathodoluminescence) and is used as phosphor[23]
* both polymorphs are piezoelectric and the hexagonal is also pyroelectric[24]
* electroluminescence[25]
* CdS crystals can act as a gain medium in solid state laser[26][27]
* In thin-film form, CdS can be combined with other layers for use in certain types of solar cells.[28] CdS was also one of the first semiconductor materials to be used for thin-film transistors (TFTs).[29] However interest in compound semiconductors for TFTs largely waned after the emergence of amorphous silicon technology in the late 1970s.
* Thin films of CdS can be piezoelectric and have been used as transducers which can operate at frequencies in the GHz region.
* Nanoribbons of CdS show a net cooling due annihilation of phonons, during anti-Stokes luminescence at ~510 nm. As a result, a maximum temperature drop of 40 and 15 K has been demonstrated when the nanoribbons are pumped with a 514 or 532 nm laser.[30]

## 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 (CI pigment yellow 37).[4][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 with each other. 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.[citation needed]

## Safety

Cadmium sulfide is toxic, especially dangerous when inhaled as dust, and cadmium compounds in general are classified as carcinogenic.[35] Problems of biocompatibility have been reported when CdS is used as colors in tattoos.[36] CdS has an LD50 of approximately 7,080 mg/kg in rats - which is higher than other cadmium compounds due to its low solubility.[37]

## References

1. ↑ Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, FL: CRC Press. pp. 4–67; 1363. ISBN 978-0-8493-0594-8.
2. ↑ 2.0 2.1 Zumdahl, Steven S. (2009). Chemical Principles 6th Ed.. Houghton Mifflin Company. p. A21. ISBN 978-0-618-94690-7.
3. ↑ 3.0 3.1 3.2 NIOSH Pocket Guide to Chemical Hazards. "#0087". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0087.html.
4. ↑ 4.0 4.1 4.2 4.3 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. ↑ 7.0 7.1 7.2 Hugh MacDonald Smith (2002). High Performance Pigments. Wiley-VCH. ISBN 978-3-527-30204-8.
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. doi:10.1016/j.chembiol.2004.08.022. PMID 15556006.
10. ↑ Oladeji, I.O.; Chow, L. (1997). "Optimization of Chemical Bath Deposited Cadmium Sulfide". J. Electrochem. Soc. 144 (7): 7. doi:10.1149/1.1837815.
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. doi:10.1016/j.tsf.2005.11.080. Bibcode: 2006TSF...511..299M.
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. ↑ 18.0 18.1 Mario Schiavello (1985) Photoelectrochemistry, Photocatalysis, and Photoreactors: Fundamentals and Developments Springer ISBN 90-277-1946-2
19. ↑ 19.0 19.1 19.2 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. ↑ 20.0 20.1 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. doi:10.1103/PhysRev.96.533. Bibcode: 1954PhRv...96..533R.
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–A1287. doi:10.1103/PhysRev.138.A1277. Bibcode: 1965PhRv..138.1277M.
25. ↑ Smith, Roland (1957). "Low-Field Electroluminescence in Insulating Crystals of Cadmium Sulfide". Physical Review 105 (3): 900. doi:10.1103/PhysRev.105.900. Bibcode: 1957PhRv..105..900S.
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 et al. (1972). "KGP-2: An Electron-Beam-Pumped Cadmium Sulfide Laser". Soviet Journal of Quantum Electronics 2 (3): 284. doi:10.1070/QE1972v002n03ABEH004443. Bibcode: 1972QuEle...2..284A.
27. ↑ Agarwal, Ritesh; Barrelet, Carl J.; Lieber, Charles M. (2005). "Lasing in Single Cadmium Sulfide Nanowire Optical Cavities". Nano Letters 5 (5): 917–920. doi:10.1021/nl050440u. PMID 15884894. Bibcode: 2005NanoL...5..917A.
28. ↑ Zhao, H.; Farah, Alvi; Morel, D.; Ferekides, C.S. (2009). "The effect of impurities on the doping and VOC of Cd Te/CDS thin film solar cells". Thin Solid Films 517 (7): 2365–2369. doi:10.1016/j.tsf.2008.11.041. Bibcode: 2009TSF...517.2365Z.
29. ↑ Weimer, Paul (1962). "The TFT A New Thin-Film Transistor". Proceedings of the IRE 50 (6): 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. PMID 23344360. Bibcode: 2013Natur.493..504Z.
31. ↑ 31.0 31.1 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 - CADMIUM SULFIDE - International Chemical Safety Cards - NIOSH". June 26, 2018. https://www.cdc.gov/niosh/ipcsneng/neng0404.html.
36. ↑ Bjornberg, A (Sep 1963). "Reactions to light in yellow tattoos from cadmium sulfide". Arch Dermatol 88 (3): 267–71. doi:10.1001/archderm.1963.01590210025003. PMID 14043617.
37. ↑ "Sicherheitsdatenblatt". http://www.alfa.com/content/msds/german/A14544.pdf.

## External links

* Cadmium(II) sulphide information at Webelements
* IARC Monograph: "Cadmium and Cadmium Compounds" Last access November 2005.
* International Chemical Safety Card 0404
* National Pollutant Inventory - Cadmium and compounds
* Defence Internet | About Defence | Zinc Cadmium Sulphide Dispersion Trials Report by the Academy of Medical Sciences to the Chief Scientific Adviser, Ministry of Defence on the zinc cadmium sulphide dispersion trials undertaken in the United Kingdom between 1953 and 1964.

* v
* t
* e

Cadmium compounds

Cadmium(I)|

* Cd2(AlCl4)2

Cadmium(II)|

* Cd(BF4)2
* CdF2
* CdCl2
* CdBr2
* CdI2
* Cd(CN)2
* CdH2
* CdO
* CdS
* CdSe
* CdTe
* Cd(OH)2
* Cd(NO3)2
* CdSO4
* CdWO4
* Cd3As2
* CsCdCl3
* CsCdBr3

* v
* t
* e

Sulfides

| H2S
H2S2 |  |  |  |  |  |  |  |  |  |  |  |  |  |  |  |  | He

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Li2S | BeS |  |  |  |  |  |  |  |  |  |  | B2S3 | CS2
COS | (NH4)SH | O | F | Ne
Na2S
Na2Sx | MgS |  |  |  |  |  |  |  |  |  |  | Al2S3 | SiS
SiS2 | PxSy | S | Cl | Ar
K2S | CaS | Sc2S3 | TiS2 | V | CrS
Cr2S3 | MnS
MnS2 | FeS
Fe3S4 | CoS | NiS | Cu2S
CuS | ZnS | GaS
Ga2S3 | GeS
GeS2 | As2S3
As4S3 | SeS2 | Br | Kr
Rb2S | SrS | Y2S3 | ZrS2 | NbS2 | MoS2 | Tc | Ru | Rh2S3 | PdS | Ag2S | CdS | In2S3 | SnS
SnS2 | Sb2S3
Sb2S5 | TeS2 | I | Xe
Cs2S | BaS | *  | HfS2 | TaS2 | WS2
WS3 | ReS2
Re2S7 | Os | Ir2S3
IrS2 | PtS
PtS2 | Au2S
Au2S3 | HgS | Tl2S | PbS
PbS2 | Bi2S3 | Po | At | Rn
Fr | Ra | **  | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og |  |  |  |  |  |  |  |
|  | ↓ |  |  |  |  |  |  |  |  |  |  |  |  |  |  |
| * | La2S3 | CeS
Ce2S3 | Pr2S3 | Nd2S3 | Pm2S3 | SmS
Sm2S3 | Eu2S3 | Gd2S3 | Tb2S3 | Dy2S3 | Ho2S3 | Er2S3 | Tm2S3 | Yb2S3 | Lu2S3 |
| ** | Ac | ThS2 | Pa | US2 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr |

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*[H341]: Suspected of causing genetic defects
*[H350]: May cause cancer
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