Chemistry:Calcium iodide
From HandWiki
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| IUPAC name
calcium iodide
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3D model (JSmol)
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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). | |
 verify (what is   ?)
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| 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:[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
- ↑ 1.0 1.1 Turner, Jr., Francis M., ed. (1920), The Condensed Chemical Dictionary (1st ed.), New York: Chemical Catalog Co., pp. 127, https://books.google.com/books?id=y8y0XE0nsYEC&q=%22calcium+iodide%22+properties&pg=PA127, retrieved 2007-12-08
- ↑ 2.0 2.1 R. J. Lewis (1993), Hawley's Condensed Chemical Dictionary 12th edition
- ↑ Mellor, Joseph William (1912), Modern Inorganic Chemistry, Longmans, Green, and Co, pp. 334, 6909989325689, https://books.google.com/books?id=wEoJAAAAIAAJ&q=%22calcium+iodide%22+subject:%22Chemistry,+Inorganic%22&pg=PA334, retrieved 2007-12-08
- ↑ Gooch, Frank Austin; Walker, Claude Frederic (1905), Outlines of Inorganic Chemistry, New York: Macmillan, pp. 340, https://books.google.com/books?id=q8MMAAAAYAAJ&q=%22calcium+iodide%22+subject:%22Chemistry,+Inorganic%22&pg=RA1-PA340, retrieved 2007-12-08
- ↑ Jones, Harry Clary (1906), Principles of Inorganic Chemistry, New York: Macmillan, pp. 365, https://books.google.com/books?id=zWE6AAAAMAAJ&q=%22calcium+iodide%22+subject:%22Chemistry,+Inorganic%22&pg=PA365, retrieved 2007-12-08
| HI | He | ||||||||||||||||
| LiI | BeI2 | BI3 | CI4 | NI3 | I2O4, I2O5, I4O9 |
IF, IF3, IF5, IF7 |
Ne | ||||||||||
| NaI | MgI2 | AlI3 | SiI4 | PI3, P2I4 |
S | ICl, ICl3 |
Ar | ||||||||||
| KI | CaI2 | Sc | TiI4 | VI3 | CrI3 | MnI2 | FeI2 | CoI2 | NiI2 | CuI | ZnI2 | Ga2I6 | GeI2, GeI4 |
AsI3 | Se | IBr | Kr |
| RbI | SrI2 | YI3 | ZrI4 | NbI5 | Mo | Tc | Ru | Rh | Pd | AgI | CdI2 | InI3 | SnI4, SnI2 |
SbI3 | TeI4 | I | Xe |
| CsI | BaI2 | HfI4 | TaI5 | W | Re | Os | Ir | Pt | AuI | Hg2I2, HgI2 |
TlI | PbI2 | BiI3 | Po | AtI | Rn | |
| Fr | RaI2 | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |
| ↓ | |||||||||||||||||
| La | Ce | Pr | Nd | Pm | SmI2 | Eu | Gd | TbI3 | Dy | Ho | Er | Tm | Yb | Lu | |||
| Ac | ThI4 | Pa | UI3, UI4 |
Np | Pu | Am | Cm | Bk | Cf | EsI3 | Fm | Md | No | Lr | |||
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