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Calcium iodide
Identifiers
CAS number 10102-68-8 Yes check.svgY
13640-62-5 (tetrahydrate)
PubChem 66244
ChemSpider 59629
RTECS number EV1300000
SMILES
InChI
InChI key UNMYWSMUMWPJLR-NUQVWONBAC
Properties
Molecular formula 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 (tetrahydrate) with decomposition

Boiling point

1100 °C

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
Structure
Crystal structure Rhombohedral, hP3, SpaceGroup = P-3m1, No. 164
Coordination
geometry
octahedral
Hazards
EU Index Not listed
NFPA 704
NFPA 704.svg
0
2
1
Related compounds
Other anions calcium fluoride
calcium chloride
calcium bromide
Other cations magnesium iodide
strontium iodide
barium iodide
 Yes check.svgY (what is this?)  (verify)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Calcium iodide is the inorganic compound with the formula CaI2. This colourless deliquescent solid is highly soluble in water. Its properties are similar to those for related salts, such as calcium chloride. It is used in photography[1].

Reactions

Henri Moissan first isolated pure calcium metal by reducing calcium iodide with pure sodium metal[2]:

CaI2 + 2 Na → 2 NaI + Ca

Calcium iodide can be formed by treating calcium carbonate with hydroiodic acid:[3]

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.[4]

2 CaI2 + 2 CO2 + O2 → 2 CaCO3 + I2

References

  1. ^ a b Turner, Jr., Francis M., ed. (1920), The Condensed Chemical Dictionary (1st ed.), New York: Chemical Catalog Co., pp. 127, http://books.google.com/books?id=y8y0XE0nsYEC&pg=PA127&dq=%22calcium+iodide%22+properties&as_brr=1&ei=lUhbR8iyIpDIiQHsqKW7BA, retrieved 2007-12-08 
  2. ^ Mellor, Joseph William (1912), 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 2007-12-08 
  3. ^ Gooch, Frank Austin; Walker, Claude Frederic (1905), 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 2007-12-08 
  4. ^ Jones, Harry Clary (1906), 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 2007-12-08 
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