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| Calcium iodide | |
|---|---|
| IUPAC name | calcium iodide |
| Identifiers | |
| CAS number | [10102-68-8] |
| RTECS number | EV1300000 |
| Properties | |
| Molecular formula | CaI2 |
| Molar mass | 293.89 g/mol, anhydrous |
| Appearance | white to light yellow solid |
| Density | 3.956 g/cm³[1] |
| Melting point |
740 °C |
| Boiling point |
1100 °C |
| Solubility in water | ? |
| Hazards | |
| NFPA 704 |
 0
1
0
|
| S-phrases | S24, S25, S28, S37, S45 [2] |
| Related compounds | |
| Other anions | calcium fluoride calcium bromide calcium chloride |
| Other cations | magnesium iodide strontium iodide |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox references |
|
Calcium iodide (CaI2) is an ionic compound of calcium and iodine. It is highly soluble in water and it is deliquescent. It is a salt that is solid at room temperature, and it behaves as a typical ionic halide. Because of its hygroscopic nature, it must be kept in tightly-sealed containers. It is similar to calcium chloride in many respects[3]. It is used in photography[1].
Reactions
Henri Moissan first isolated pure calcium metal by reducing calcium iodide with pure sodium metal[4]:
Calcium iodide can be formed by reacting calcium carbonate with hydroiodic acid[5]:
Calcium iodide slowly reacts with oxygen and carbon dioxide in the air, giving free iodine[6].
References
- ^ a b Turner, Jr., Francis M., ed., The Condensed Chemical Dictionary (First ed.), New York: The Chemical Catalog Company, pp. 127, <http://books.google.com/books?id=y8y0XE0nsYEC&pg=PA127&dq=%22calcium+iodide%22+properties&as_brr=1&ei=lUhbR8iyIpDIiQHsqKW7BA>. Retrieved on 8 December 2007
- ^ http://www.sciencelab.com/xMSDS-Calcium_iodide-9923259
- ^ Mendeleyev, Dmitry Ivanovich & Kamensky, George, The Principles of Chemistry, New York: P. F. Collier, pp. 604, <http://books.google.com/books?id=BrE93bC50wAC&pg=RA4-PA604&dq=%22calcium+iodide%22&as_brr=1&ei=LUdbR5OfIYmMiQHcjLCvBA>. Retrieved on 2007-12-08
- ^ Mellor, Joseph William, Modern Inorganic Chemistry, New York: Longmans, Green, and Co, pp. 334, <http://books.google.com/books?id=wEoJAAAAIAAJ&pg=PA334&dq=%22calcium+iodide%22+subject:%22Chemistry,+Inorganic%22&as_brr=1&ei=ZUJbR7CEA5vOiQGmn-2GBA>. Retrieved on 2007-12-08
- ^ Gooch, Frank Austin & Walker, Claude Frederic, Outlines of Inorganic Chemistry, New York: Macmillan, pp. 340, <http://books.google.com/books?id=q8MMAAAAYAAJ&pg=RA1-PA340&dq=%22calcium+iodide%22+subject:%22Chemistry,+Inorganic%22&as_brr=1&ei=uEJbR832JJPuiQGqzqWKBA>. Retrieved on 2007-12-08
- ^ Jones, Harry Clary, Principles of Inorganic Chemistry, New York: Macmillan, pp. 365, <http://books.google.com/books?id=zWE6AAAAMAAJ&pg=PA365&dq=%22calcium+iodide%22+subject:%22Chemistry,+Inorganic%22&as_brr=1&ei=RUJbR4z9I4yEiQGaw5X3Aw>. Retrieved on 2007-12-08
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