Cobalt(II) iodide
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Cobalt(II) iodide | |
---|---|
IUPAC name | Cobalt(II) iodide |
Other names | cobaltous iodide, cobalt diiodide |
Identifiers | |
CAS number | [15238-00-3] |
Properties | |
Molecular formula | CoI2 |
Molar mass | 312.742 g/mol |
Appearance | α-form: black hexagonal crystal β-form: yellow powder |
Density | α-form: 5.584 g/cm³ β-form: 5.45 g/cm³ |
Melting point |
α-form: 515-520°C under vacuum |
Solubility in water | 67.0 g/100 mL[1] |
Hazards | |
EU classification | Harmful (Xn) |
NFPA 704 | |
R-phrases | R20/21/22, R36/37/38 |
S-phrases | S26, S36[2] |
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 are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references |
Cobalt(II) iodide or cobaltous iodide is the chemical compound composed of cobalt and iodine with the formula CoI2. This hygroscopic crystalline solid is a laboratory reagent used to test for the presence of water in organic solvents or in the atmosphere[3]. When anhydrous cobalt(II) iodide is added to solvents such as alcohols, ketones, and nitriles, it will turn pick in the presence of water[4].
[edit] Forms
Cobalt(II) iodide exists in two distinct forms, the α- and β-forms. The α-form consists of black hexagonal crystals which turn dark green when exposed to air. The β-form is a yellow powder which readily absorbs moisture from the air, converting into green droplets. When placed in a vacuum, the α-form sublimes, forming the β-form. When the β-form is heated to 400°C, it converts to the α-form.
[edit] Reactions
Cobalt(II) iodide is formed by heating elemental cobalt in the presence of gaseous hydrogen iodide or elemental iodine vapor[3].
Cobalt(II) iodide has been used as a catalyst in the reaction of diketene with Grignard reagents in the synthesis of terpenoids[5].
[edit] References
- ^ Perry, Dale L. & Phillips, Sidney L., Handbook of Inorganic Compounds, San Diego: CRC Press, pp. 127-8, ISBN 0849386713, <http://books.google.com/books?id=0fT4wfhF1AsC&pg=PA128&dq=%22Cobalt(II)+iodide%22&sig=xjN_iy-hte1LQmDXwd0lZ9DOIQw#PPA127,M1>. Retrieved on 2007-06-03
- ^ 429740 Cobalt(II) iodide anhydrous, beads, −10 mesh, 99.999%. Sigma-Aldrich. Retrieved on 2008-06-03.
- ^ a b Patnaik, Pradyot, Handbook of Inorganic Chemicals, Amsterdam: McGraw-Hill Professional, pp. 244, ISBN 0070494398, <http://books.google.com/books?id=Xqj-TTzkvTEC&pg=PA244&dq=%22Cobalt(II)+iodide%22&sig=kAuO8lJeq0SqAE46x7n4sm1iT0E>. Retrieved on 2007-06-03
- ^ Armarego, Wilfred L. F. & Chai, Christina L. L., Purification of Laboratory Chemicals, Butterworth-Heinemann, pp. 26, ISBN 0750675713, <http://books.google.com/books?id=SYzm1tx2z3QC&pg=PA26&dq=%22Cobalt(II)+iodide%22&as_brr=3&sig=TDGFmkL7UvLsU_zYK2MbVZiJYRI>. Retrieved on 2007-06-03
- ^ Agreda, V. H. & Zoeller, Joseph R., Acetic Acid and Its Derivatives, CRC Press, pp. 74, ISBN 0824787927, <http://books.google.com/books?id=3MjdGp1v1YIC&pg=RA1-PA784&dq=%22Cobalt(II)+iodide%22&as_brr=3&sig=hWuarTAI7M-FW8DbBJRRX6SiUmE>. Retrieved on 2007-06-03