Cobalt(II) oxide

Cobalt(II) oxide
Names
IUPAC name
Cobalt(II) oxide
Other names
Cobaltous oxide
Cobalt monoxide
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.013.777
EC Number 215-154-6
RTECS number GG2800000
UN number 3288
Properties
CoO
Molar mass 74.9326 g/mol
Appearance black powder
Odor odorless
Density 6.44 g/cm3 [1]
Melting point 1,933 °C (3,511 °F; 2,206 K)
insoluble in water[2]
+4900.0·10−6 cm3/mol
Structure
cubic, cF8
Fm3m, No. 225
Hazards
Main hazards Toxic (T)

Harmful (Xn)
Dangerous for the environment (N)

Safety data sheet ICSC 1551
T Xn N
R-phrases (outdated) R22, R43, R50/53
S-phrases (outdated) (S2), S24, S37, S60, S61
NFPA 704
Flammability code 0: Will not burn. E.g., waterHealth code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gasReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogenSpecial hazards (white): no codeNFPA 704 four-colored diamond
0
3
0
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
202 mg/kg
Related compounds
Other anions
 Cobalt(II) sulfide
Cobalt(II) hydroxide
Other cations
 Iron(II) oxide
Nickel(II) oxide
Related compounds
 Cobalt(II,III) oxide
Cobalt(III) oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☑Y verify (what is ☑Y☒N ?)
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.[3] 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 4.2615 Å.[4]

It is antiferromagnetic below 16 °C.[5]

Preparation

Cobalt(II,III) oxide decomposes to cobalt(II) oxide at 950 °C:[6]

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.[7]

CoCl2 + H2O → CoO + H2 + Cl2

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

CoX + 2 KOH → Co(OH)2 + K2X
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 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.

See also

References

  1. ↑ Patnaik, Pradyot (2003). Handbook of Inorganic Chemical Compounds. McGraw-Hill. ISBN 0-07-049439-8. Retrieved 2009-06-06.
  2. ↑ Advanced Search – Alfa Aesar – A Johnson Matthey Company. Alfa.com. Retrieved on 2011-11-19.
  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 (13): 6847–6853. doi:10.1103/PhysRevB.35.6847.
  5. ↑ Silinsky, P. S.; Seehra, Mohindar S. (1981). "Principal magnetic susceptibilities and uniaxial stress experiments in CoO". Physical Review B. 24: 419–423. doi:10.1103/PhysRevB.24.419.
  6. ↑ US 4389339, James, Leonard E.; Crescentini, Lamberto & Fisher, William B., "Process for making a cobalt oxide catalyst"
  7. ↑ Kern, S. (1876). "Inorganic chemistry". J. Chem. Soc. 29: 880. doi:10.1039/JS8762900876.
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