Calcium iodide
Names | |
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IUPAC name
calcium iodide
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Identifiers | |
10102-68-8 13640-62-5 (tetrahydrate) |
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ChemSpider | 59629 |
Jmol 3D model | Interactive image |
PubChem | 66244 |
RTECS number | EV1300000 |
UNII | 8EKI9QEE2H |
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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[1] |
Melting point | 779 °C (1,434 °F; 1,052 K) (tetrahydrate) with decomposition |
Boiling point | 1,100 °C (2,010 °F; 1,370 K) |
64.6 g/100 mL (0 °C) 66 g/100 mL (20 °C) 81 g/100 mL (100 °C) |
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Solubility | soluble in acetone and alcohols |
Structure | |
Rhombohedral, hP3 | |
P-3m1, No. 164 | |
octahedral | |
Vapor pressure | {{{value}}} |
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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verify (what is ?) | |
Infobox references | |
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
Henri Moissan first isolated pure calcium in 1898 by reducing calcium iodide with pure sodium metal:[2]
Calcium iodide can be formed by treating calcium carbonate, calcium oxide, or calcium hydroxide with hydroiodic acid:[3]
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.[4]
- 2 CaI2 + 2 CO2 + O2 → 2 CaCO3 + 2 I2
References
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- Calcium compounds
- Iodides
- Metal halides
- Deliquescent substances
- Inorganic compound stubs