Calcium iodide
(Redirected from CaI2)
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| Names | |
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| IUPAC name
calcium iodide
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| Identifiers | |
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3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.030.238 |
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PubChem CID
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| UNII | |
CompTox Dashboard (EPA)
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| Properties | |
| CaI2 | |
| Molar mass | 293.887 g/mol (anhydrous) 365.95 g/mol (tetrahydrate) |
| Appearance | white solid |
| Density | 3.956 g/cm3 (anhydrous)[1] |
| Melting point | 779 °C (1,434 °F; 1,052 K) (anhydrous) [2] |
| Boiling point | 1,100 °C (2,010 °F; 1,370 K)[2] |
| 64.6 g/100 mL (0 °C) 66 g/100 mL (20 °C) 81 g/100 mL (100 °C) | |
| Solubility | soluble in acetone and alcohols |
| -109.0·10−6 cm3/mol | |
| Structure | |
| Rhombohedral, hP3 | |
| P-3m1, No. 164 | |
| octahedral | |
| Hazards | |
| NFPA 704 (fire diamond) | |
| Related compounds | |
Other anions
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calcium fluoride calcium chloride calcium bromide |
Other cations
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beryllium iodide magnesium iodide strontium iodide barium iodide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Calcium iodide (chemical formula CaI2) is the ionic compound of calcium and iodine. This colourless deliquescent solid is a salt that is highly soluble in water. Its properties are similar to those for related salts, such as calcium chloride. It is used in photography.[1] It is also used in cat food as a source of iodine.
Reactions
[edit]Henri Moissan first isolated pure calcium in 1898 by reducing calcium iodide with pure sodium metal:[3]
Calcium iodide can be formed by treating calcium carbonate, calcium oxide, or calcium hydroxide with hydroiodic acid:[4]
Calcium iodide slowly reacts with oxygen and carbon dioxide in the air, liberating iodine, which is responsible for the faint yellow color of impure samples.[5]
- 2 CaI2 + 2 CO2 + O2 → 2 CaCO3 + 2 I2
References
[edit]- ^ a b Turner, Jr., Francis M., ed. (1920), The Condensed Chemical Dictionary (1st ed.), New York: Chemical Catalog Co., p. 127, retrieved 2007-12-08
- ^ a b R. J. Lewis (1993), Hawley's Condensed Chemical Dictionary 12th edition
- ^ Mellor, Joseph William (1912), Modern Inorganic Chemistry, New York: Longmans, Green, and Co, p. 334, 6909989325689, retrieved 2007-12-08
- ^ Gooch, Frank Austin; Walker, Claude Frederic (1905), Outlines of Inorganic Chemistry, New York: Macmillan, p. 340, retrieved 2007-12-08
- ^ Jones, Harry Clary (1906), Principles of Inorganic Chemistry, New York: Macmillan, p. 365, retrieved 2007-12-08