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Revision as of 16:37, 23 July 2011

Cobalt(II) oxide
Cobalt(II) oxide
Names
IUPAC name Cobalt(II) oxide
Other names Cobaltous oxide
Cobalt monoxide
Identifiers
CAS Number
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.013.777 Edit this at Wikidata
EC Number
  • 215-154-6
PubChem CID
RTECS number
  • GG2800000
UN number 3288
CompTox Dashboard (EPA)
InChI
  • InChI=1S/Co.O/q+2;-2Key: IUYLTEAJCNAMJK-UHFFFAOYSA-N
  • InChI=1/Co.O/rCoO/c1-2Key: IVMYJDGYRUAWML-NNYFCMOLAO
  • InChI=1/Co.O/q+2;-2Key: IUYLTEAJCNAMJK-UHFFFAOYAY
SMILES
  • =O
  • .
Properties
Chemical formula CoO
Molar mass 74.9326 g/mol
Appearance black powder
Odor odorless
Density 6.44 g/cm
Melting point 1,933 °C (3,511 °F; 2,206 K)
Solubility in water insoluble in water
Structure
Crystal structure cubic, cF8
Space group Fm3m, No. 225
Hazards
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
LD50 (median dose) 202 mg/kg
Related compounds
Other anions Cobalt(II) sulfide
Cobalt(II) hydroxide
Other cations Iron(II) oxide
Nickel(II) oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). checkY verify (what is  ?) Infobox references
Chemical compound

Cobalt(II) oxide or cobalt monoxide is an inorganic compound that appears as olive-green to red crystals, or as a greyish or black powder. It is used extensively in the ceramics industry as an additive to create blue colored glazes and enamels as well as in the chemical industry for producing cobalt(II) salts.

Structure and properties

CoO crystals adopt the periclase (rock salt) structure with a lattice constant of 4.2615Å.

It is antiferromagnetic below 16°C .

Preparation

Cobalt(II,III) oxide decomposes to cobalt(II) oxide at 950 °C:

2 Co3O4 → 6 CoO + O2

Though commercially available, cobalt(II) oxide may be prepared in the laboratory by electrolyzing a solution of cobalt(II) chloride:

CoCl2 + H2O → CoO + H2 + Cl2

It may also be prepared by precipitating the hydroxide, followed by thermal decomposition:

CoX + 2 NaOH → Co(OH)2 + Na2X
Co(OH)2 → CoO + H2O

Reactions

As can be expected, cobalt(II) oxide reacts with mineral acids to form the corresponding cobalt salts:

CoO + 2 HX → CoX2 + H2O

Applications

Cobalt(II) oxide has for centuries used as a coloring agent on kiln fired pottery; the earliest examples go back to 12th century German pottery. The additive provides a deep shade of blue named Cobalt blue. The band gap (CoO) is around 2.4 eV. It also is used in cobalt blue glass.

References

  1. Patnaik, Pradyot (2003). Handbook of Inorganic Chemical Compounds. McGraw-Hill. ISBN 0070494398. Retrieved 2009-06-06.
  2. http://www.alfa.com/content/msds/german/44354.pdf
  3. "Safety (MSDS) data for cobalt oxide". The Physical and Theoretical Chemistry Laboratory, Oxford University. Retrieved 2008-11-11.
  4. Kannan, R.; Seehra, Mohindar S. (1987). "Percolation effects and magnetic properties of the randomly diluted fcc system CopMg1-pO". Physical Review B. 35: 6847. doi:10.1103/PhysRevB.35.6847.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  5. Silinsky, P. S.; Seehra, Mohindar S. (1981). "Principal magnetic susceptibilities and uniaxial stress experiments in CoO". Physical Review B. 24: 419. doi:10.1103/PhysRevB.24.419.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  6. Process for making a cobalt oxide catalyst, James, Leonard E. (Richmond, VA) Crescentini, Lamberto (Chester, VA) Fisher, William B. (Chester, VA) 1983. http://www.freepatentsonline.com/4389339.html
  7. Kern, S.; J. Chem. Soc.; 1876. Part 1. p880.
  8. Zamek, Jeff: "A Problem With Cobalt?" Ceramics Today http://www.ceramicstoday.com/articles/zamek_cobalt.htm
Cobalt compounds
Cobalt(I)
Cobalt(II)
Cobalt(0,III)
Cobalt(II,III)
Cobalt(III)
Cobalt(III,IV)
Cobalt(IV)
Cobalt(V)
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