Cadmium oxide

Cadmium oxide
Names
IUPAC name
Cadmium oxide
Other names
Cadmium(II) oxide,
Cadmium monoxide
Identifiers
1306-19-0 Yes
ChemSpider 14099 Yes
EC number 215-146-2
Jmol-3D images Image
PubChem 14782
RTECS number EV1925000
UN number 2570
Properties
Molecular formula
 CdO
Molar mass 128.41 g·mol−1
Appearance colorless powder (alpha form)
red-brown crystal (beta form) [1]
Odor odorless
Density 8.15 g/cm3(crystalline),
6.95 g/cm3 (amorphous)[2] solid.
Melting point 900–1,000 °C (1,650–1,830 °F; 1,170–1,270 K)
decomposition of amorphous form[3]
Boiling point 1,559 °C (2,838 °F; 1,832 K) sublimation[3]
4.8 mg/L (18 °C)[4]
Solubility soluble in dilute acid
slowly soluble in ammonium salts
insoluble in alkalies
Vapor pressure 0.13 kPa (1000 °C)
2.62 kPa (1200 °C)
61.4 kPa (1500 °C)[5]
Band gap 2.18 eV
Electron mobility 531 cm2/V·s
-3×10−5 cm3/mol
Thermal conductivity 0.7 W/m·K
2.49
Structure
Crystal structure cubic, cF8
Space group Fm3m, No. 225
Lattice constant a = 4.6958 Å
Thermochemistry
Specific
heat capacity (C)
 43.64 J/mol·K[4]
55 J/mol·K[6]
Std enthalpy of
formation (ΔfHo298)
 −258 kJ/mol[6][5]
-229.3 kJ/mol[4]
Hazards
MSDS
GHS pictograms [7]
GHS signal word Danger
H330, H341, H350, H361, H372, H410[7]
P201, P260, P273, P281, P284, P310[7]
EU Index 048-002-00-0
EU classification T+ N
Carc. Cat. 2
Muta. Cat. 3
Repr. Cat. 3
R-phrases R45, R26, R48/23/25, R62, R63, R68, R50/53
S-phrases S53, S45, S60, S61
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 4: Very short exposure could cause death or major residual injury. E.g., VX 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
4
0
Flash point Non-flammable
72 mg/kg (oral, rat)[8]
US health exposure limits (NIOSH):
TWA 0.005 mg/m3[9]
Related compounds
Other anions
 Cadmium sulfide
Cadmium selenide
Cadmium telluride
Other cations
 Zinc oxide
Mercury oxide
Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Cadmium oxide is an inorganic compound with the formula CdO. It is one of the main precursors to other cadmium compounds. It crystallizes in a cubic rocksalt lattice like sodium chloride, with octahedral cation and anion centers.[10] It occurs naturally as the rare mineral monteponite. Cadmium oxide can be found as a colorless amorphous powder or as brown or red crystals.[11] Cadmium oxide is an n-type semiconductor[12] with a band gap of 2.18 eV (2.31 eV) at room temperature (0 K).[13]

Production and structure

Since cadmium compounds are often found in association with zinc ores, cadmium oxide is a common by-product of zinc refining.[14] It is produced by burning elemental cadmium in air. Pyrolysis of other cadmium compounds, such as the nitrate or the carbonate, also affords this oxide. When pure, it is red but CdO is unusual in being available in many differing colours due to its tendency to form defect structures resulting from anion vacancies.[15] Cadmium oxide is prepared commercially by oxidizing cadmium vapor in air.[16]

Uses

Cadmium oxide is used in cadmium plating baths, electrodes for storage batteries, cadmium salts, catalyst, ceramic glazes, phosphors, and nematocide.[11] Major uses for cadmium oxide are as an ingredient for electroplating baths, and in pigments.[17]

Transparent conductor

CdO is used as a transparent conductive material,[18] which was prepared as a transparent conducting film back in 1907.[19] Cadmium oxide in the form of thin films has been used in applications such as photodiodes, phototransistors, photovoltaic cells, transparent electrodes, liquid crystal displays, IR detectors, and anti reflection coatings.[20] CdO microparticles undergo bandgap excitation when exposed to UV-A light and is also selective in phenol photodegradation.[21]

Cadmium plating

Most commercial electroplating of cadmium is done by electrodeposition from cyanide baths. These cyanide baths consist of cadmium oxide and sodium cyanide in water, which likely form cadmium cyanide and sodium hydroxide. A typical formula is 32 g/L cadmium oxide and 75 g/L sodium cyanide. The cadmium concentration may vary by as much as 50%. Brighteners are usually added to the bath and the plating is done at room temperature with high purity cadmium anodes.[22]

Reactivity

CdO is a basic oxide and is thus attacked by aqueous acids to give solutions of [Cd(H2O)6]2+. Upon treatment with strong alkaline solutions, [Cd(OH)
4]2−
 forms. A thin coat of cadmium oxide forms on the surface of cadmium in moist air at room temperature.[11] Cadmium will oxidize at room temperatures to form CdO.[22] Cadmium vapor and steam will form CdO and hydrogen in a reversible reaction.[22]

References

  1. ↑ Patnaik, Pradyot (2003). Handbook of Inorganic Chemical Compounds. McGraw-Hill. ISBN 0-07-049439-8.
  2. ↑ "NIOSH Pocket Guide to Chemical Hazards". Retrieved 2007-02-16.
  3. ↑ 3.0 3.1 "INCHEM: Chemical Safety Information from Intergovernmental Organizations". Retrieved 2007-02-16.
  4. ↑ 4.0 4.1 4.2 http://chemister.ru/Database/properties-en.php?dbid=1&id=500
  5. ↑ 5.0 5.1 Cadmium oxide in Linstrom, P.J.; Mallard, W.G. (eds.) NIST Chemistry WebBook, NIST Standard Reference Database Number 69. National Institute of Standards and Technology, Gaithersburg MD. http://webbook.nist.gov (retrieved 2014-05-23)
  6. ↑ 6.0 6.1 Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A21. ISBN 0-618-94690-X.
  7. ↑ 7.0 7.1 7.2 Sigma-Aldrich Co., Cadmium oxide. Retrieved on 2014-05-23.
  8. ↑ http://chem.sis.nlm.nih.gov/chemidplus/rn/1306-19-0
  9. ↑ "NIOSH Pocket Guide to Chemical Hazards #0088". National Institute for Occupational Safety and Health (NIOSH).
  10. ↑ Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
  11. ↑ 11.0 11.1 11.2 Lewis, Richard J., Sr., Hawley's condensed chemical dictionary, 13th ed., 1997, p. 189
  12. ↑ T. L. Chu and Shirley S. Chu (1990). "Degenerate cadmium oxide films for electronic devices". Journal of Electronic Materials 19 (9): 1003–1005. doi:10.1007/BF02652928.
  13. ↑ S. K. Vasheghani Farahani et al. (2013). "Temperature dependence of the direct bandgap and transport properties of CdO". Applied Physics Letters 102 (2): 022102. doi:10.1063/1.4775691.
  14. ↑ "Cadmium and compounds fact sheet". Archived from the original on 2006-12-10. Retrieved 2007-02-16.
  15. ↑ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
  16. ↑ Hampel, C. A. and Hawley, G. G. (1973). The encyclopedia of Chemistry (3rd ed.). p. 169.
  17. ↑ Clifford A. Hampel and Gessner G. Hawley, The encyclopedia of Chemistry, 3rd Ed., 1973, p. 169
  18. ↑ Varkey, A (1994). "Transparent conducting cadmium oxide thin films prepared by a solution growth technique". Thin Solid Films 239 (2): 211. doi:10.1016/0040-6090(94)90853-2.
  19. ↑ Dou, Y (1998). "N-type doping in CdO ceramics: a study by EELS and photoemission spectroscopy". Surface Science 398: 241. doi:10.1016/S0039-6028(98)80028-9.
  20. ↑ Lokhande, B (2004). "Studies on cadmium oxide sprayed thin films deposited through non-aqueous medium". Materials Chemistry and Physics 84 (2–3): 238. doi:10.1016/S0254-0584(03)00231-1.
  21. ↑ Karunakaran, C; Dhanalakshmi, R (2009). "Selectivity in photocatalysis by particulate semiconductors". Central European Journal of Chemistry 7 (1): 134. doi:10.2478/s11532-008-0083-7.
  22. ↑ 22.0 22.1 22.2 Clifford A. Hampel, Rare Metals Handbook, 1954, p. 87-103

External links

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