Calcium iodide

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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 disclaimer and 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].

[edit] Reactions

Henri Moissan first isolated pure calcium metal by reducing calcium iodide with pure sodium metal[4]:

CaI2 + 2Na → 2NaI + Ca

Calcium iodide can be formed by reacting calcium carbonate with hydroiodic acid[5]:

CaCO3 + 2HI → CaI2 + H2O + CO2

Calcium iodide slowly reacts with oxygen and carbon dioxide in the air, giving free iodine[6].

[edit] References

  1. ^ 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 
  2. ^ http://www.sciencelab.com/xMSDS-Calcium_iodide-9923259
  3. ^ 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 
  4. ^ 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 
  5. ^ 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 
  6. ^ 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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