Cobalt(II) iodide
Names | |
---|---|
IUPAC name
Cobalt(II) iodide | |
Other names
cobaltous iodide, cobalt diiodide | |
Identifiers | |
(hexahydrate: 52595-03-6) 15238-00-3 (hexahydrate: 52595-03-6) | |
PubChem | 419951 |
Properties | |
CoI2 | |
Molar mass | 312.7421 g/mol (anhydrous) 420.83 g/mol (hexahydrate) |
Appearance | α-form: black hexagonal crystal β-form: yellow powder |
Density | α-form: 5.584 g/cm3 β-form: 5.45 g/cm3 hexahydrate: 2.79 g/cm3 |
Melting point | α-form: 515-520 °C under vacuum β-form: converts to α-form at 400 °C |
Boiling point | 570 °C (1,058 °F; 843 K) |
67.0 g/100 mL[1] | |
Hazards | |
EU classification | Harmful (Xn) |
R-phrases | R20/21/22, R36/37/38 |
S-phrases | S26, S36[2] |
NFPA 704 | |
Related compounds | |
Other anions |
Cobalt(II) fluoride Cobalt(II) chloride Cobalt(II) bromide |
Other cations |
Nickel(II) iodide Copper(I) iodide |
Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa) | |
verify (what is: / ?) | |
Infobox references | |
Cobalt(II) iodide or cobaltous iodide is the inorganic compound composed with the formula CoI2. The two forms of CoI2 and the hexahydrate CoI2(H2O)6 are the principal iodides of cobalt.[3]
Synthesis and structure
Cobalt(II) iodide is prepared by treating cobalt powder with gaseous hydrogen iodide.[3] The hydrated form (CoI2(H2O)6) can be prepared by the reaction of cobalt(II) oxide (or relate cobalt compounds) with hydroiodic acid.
Cobalt(II) iodide crystallizes in two polymorphs, the α- and β-forms. The α-polymorph consists of black hexagonal crystals which turn dark green when exposed to air. Heating samples of α-CoI2 under a vacuum at 500 C causes sublimation, yielding the β-polymorph is a yellow crystals. β-CoI2 also readily absorbs moisture from the air, converting into green droplets. Upon heating to 400 °C, β-CoI2 converts to the α-form.[3]
The hexaaquo salt consists of separated [Co(H2O)6]2+ and iodide ions as verified crystallographically.[4][5]
Reactions and applications
Anhydrous cobalt(II) iodide is sometimes used to test for the presence of water in various solvents.[6]
Cobalt(II) iodide is used as a catalyst, e.g. in carbonylations. It catalyzes the reaction of diketene with Grignard reagents, useful for the synthesis of terpenoids[7]
References
- ↑ Perry, Dale L.; Phillips, Sidney L. (1995), Handbook of Inorganic Compounds, San Diego: CRC Press, pp. 127–8, ISBN 0-8493-8671-3, retrieved 2008-06-03
- ↑ "429740 Cobalt(II) iodide anhydrous, beads, −10 mesh, 99.999%". Sigma-Aldrich. Retrieved 2008-06-03.
- ↑ 3.0 3.1 3.2 O. Glemser "Cobalt, Nickel" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 1518.
- ↑ “Structure Cristalline et Expansion Thermique de L’Iodure de Nickel Hexahydrate“ (Crystal structure and thermal expansion of nickel(II) iodide hexahydrate) Louër, Michele; Grandjean, Daniel; Weigel, Dominique Journal of Solid State Chemistry (1973), 7(2), 222-8. doi: 10.1016/0022-4596(73)90157-6
- ↑ "The crystal structure of the crystalline hydrates of transition metal salts. The structure of CoI2·6H2O" Shchukarev, S. A.; Stroganov, E. V.; Andreev, S. N.; Purvinskii, O. F. Zhurnal Strukturnoi Khimii 1963, vol. 4, pp. 63-6.
- ↑ Armarego, Wilfred L. F.; Chai, Christina L. L. (2003), Purification of Laboratory Chemicals, Butterworth-Heinemann, p. 26, ISBN 0-7506-7571-3, retrieved 2008-06-03
- ↑ Agreda, V. H.; Zoeller, Joseph R. (1992), Acetic Acid and Its Derivatives, CRC Press, p. 74, ISBN 0-8247-8792-7, retrieved 2008-06-03
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