Barium iodide
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Barium iodide
| Barium iodide[1] | |
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Barium iodide |
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Other names
Barium iodide, anhydrous |
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| Identifiers | |
| CAS number | 13718-50-8, (anhydrous) [7787-33-9] (dihydrate) |
| PubChem | 5462836 |
| ChemSpider | 75507  |
| Jmol-3D images | Image 1 |
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| Properties | |
| Molecular formula | BaI2 (anhydrous) BaI2·2H2O (dihydrate) |
| Molar mass | 391.136 g/mol (anhydrous) 427.167 g/mol (dihydrate) |
| Appearance | White orthorhombic crystals (anhydrous) colorless crystals (dihydrate) |
| Density | 5.15 g/cm3 (anhydrous) 5.0 g/cm3 (dihydrate) |
| Melting point |
711°C (anhydrous) |
| Solubility in water | 221 g/100 mL |
| Solubility | soluble in ethanol, acetone |
| Structure | |
| Crystal structure | Orthorhombic, oP12, SpaceGroup = Pnma, No. 62 |
| Thermochemistry | |
| Std enthalpy of formation ΔfH |
-602.1 kJ·mol-1 |
| Hazards | |
| Main hazards | toxic |
| Related compounds | |
| Other anions | barium fluoride barium chloride barium bromide |
| Other cations | beryllium iodide magnesium iodide calcium iodide strontium iodide |
 (verify) (what is:  / ?)Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) |
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| Infobox references | |
Barium iodide is an inorganic compound with the formula BaI2. The compound exists as an anhydrous and a hydrate (BaI2(H2O)2), both of which are white solids. When heated, hydrated barium iodide converts to the anhydrous salt. The hydrated form is freely soluble in water, ethanol, and acetone.
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Contents
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Structure
The structure of the anhydrous form resembles that of lead(II) chloride with each Ba center bound to nine iodide ligands[2] and has a crystalline packing structure that is quite similar to BaCl2.[3]
Reactions
Anhydrous BaI2 can be prepared by treating Ba metal with 1,2-diiodoethane in ether.[4].
BaI2 reacts with alkyl potassium compounds to form organobarium compounds.[5]
BaI2 can be reduced with lithium biphenyl, to give a highly active form of barium metal.[6]
Safety
Like other soluble salts of barium, barium iodide is toxic.
References
- ^ Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, FL: CRC Press, pp. 4–44, ISBN 0-8493-0594-2
- ^ Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
- ^ Brackett, E. B.; Brackett, T. E.; Sass, R. L.; The Crystal Structures of Barium Chloride, Barium Bromide, and Barium Iodide. J. Phys. Chem., 1963, volume 67, 2132 – 2135
- ^ Duval, E.; Zoltobroda, G.; Langlois, Y.; A new preparation of BaI2: application to (Z)-enol ether synthesis. Tetrahedron Letters, 2000, 41, 337-339
- ^ Walter, M. D.; Wolmershauser, G.; Sitzmann, H.; Calcium, Strontium, Barium, and Ytterbium Complexes with Cyclooctatetraenyl or Cyclononatetraenyl Ligands. J. Am. Chem. Soc., 2005, 127 (49), 17494 – 17503.
- ^ Yanagisawa, A.; Habaue, S.; Yasue, K.; Yamamoto, H.; Allylbarium Reagents: Unprecedented Regio- and Stereoselective Allylation Reactions of Carbonyl Compounds. J. Am. Chem. Soc.1994, 116,6130-6141
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