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Cobalt(II) oxide

Names
IUPAC name Cobalt(II) oxide
Other names Cobaltous oxide Cobalt monoxide
Identifiers
CAS Number	1307-96-6
3D model (JSmol)	Interactive image Interactive image
ChemSpider	8117730
ECHA InfoCard	100.013.777
EC Number	215-154-6
PubChem CID	9942118
RTECS number	GG2800000
UN number	3288
CompTox Dashboard (EPA)	DTXSID6051649
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). Y verify (what is  ?) Infobox references

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
• Oxides