Calcium iodide
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IUPAC name calcium iodide | |
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ECHA InfoCard | 100.030.238 ![]() |
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InChI
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Properties | |
Chemical formula | 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] |
Solubility in water | 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 |
Magnetic susceptibility (χ) | -109.0·10−6 cm3/mol |
Structure | |
Crystal structure | Rhombohedral, hP3 |
P-3m1, No. 164 | |
octahedral | |
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NFPA 704 (fire diamond) | ![]() 2 0 1 |
Related compounds | |
Other anions | calcium fluoride calcium chloride calcium bromide |
Other cations | 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). ![]() ![]() ![]() Infobox references |
Chemical compound
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:[3]
Calcium iodide can be formed by treating calcium carbonate, calcium oxide, or calcium hydroxide with hydroiodic acid:[4]
- CaCO3 + 2 HI → CaI2 + H2O + CO2
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
- ^ 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
- v
- t
- e
- CaH2
- CaF2
- CaCl2
- Ca(ClO)2
- Ca(ClO3)2
- Ca(ClO4)2
- CaBr2
- Ca(BrO3)2
- CaI2
- Ca(IO3)2
- CaICl
- CaC2
- Ca(CN)2
- CaCN2
- CaCO3
- Ca(HCO3)2
- CaSi
- CaSi2
- Ca2SiO4
- Ca3(BO3)2
- CaAl2O4
- Ca3Al2O6
- Ca(MnO4)2
- CaCrO4
- CaTiO3
- CaC2O4
- Ca(HCO2)2
- Ca(CH3CO2)2
- Ca(C3H5O2)2
- CaC4H2O4
- Ca3(C6H5O7)2
- C3H7CaO6P
- Ca(C6H5O5S)2
- Ca(C6H7O6)2
- C10H11CaN4O8P
- CaC10H12O4N5PO4
- C10H16CaN2O8
- C12H22CaO14
- C14H26CaO16
- C18H32CaO19
- C36H70CaO4
- C24H40B2CaO24