Magnesium iodide: Difference between revisions
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== References == | == References == | ||
{{reflist|2}} | |||
[[Category:Iodides]] | [[Category:Iodides]] | ||
Latest revision as of 19:23, 4 September 2012
| Template:Chembox header | Magnesium iodide | |
|---|---|
| Magnesium iodide | |
| Template:Chembox header | General | |
| Systematic name | Magnesium iodide |
| Molecular formula | MgI2 (anhydrous) MgI2.6H2O (hexahydrate) MgI2.8H2O (octahydrate) |
| Molar mass | 278.114 g/mol (anhydrous) 386.2005 g/mol (hexahydrate) 422.236 g/mol (octahydrate) |
| Appearance | white crystalline solid |
| CAS number | 10377-58-9 (anhydrous) 75535-11-4 (hexahydrate) 7790-31-0 (octahydrate) |
| Template:Chembox header | Properties | |
| Density and phase | 4.43 g/cm³ (anhydrous solid) 2.353 g/cm³ (hexahydrate solid) 2.098 g/cm³ (octahydrate solid) |
| Solubility in water | 54.7 g/100 cm³ (anhydrous, 0 °C) 81 g/100 cm³ (octahydrate, 20 °C) |
| Melting point | 637 °C (anhydrous, decomposes) 41 °C (octahydrate, decomposes) |
| Template:Chembox header | Structure | |
| Crystal structure | Hexagonal (anhydrous) Monoclinic (hexahydrate) Orthorhombic (octahydrate) |
| Hydrates | Hexahydrate, Octahydrate[1] |
| Template:Chembox header | Hazards | |
| R/S statement | R: Template:R36 Template:R38 Template:R42 Template:R43 Template:R61 S: Template:S22 Template:S36/37/39 Template:S45 Template:S53[2] |
| Template:Chembox header | Supplementary data page | |
| Template:Chembox header | Related compounds | |
| Other anions | Magnesium fluoride Magnesium bromide Magnesium chloride |
| Other cations | beryllium iodide calcium iodide |
| Template:Chembox header | Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references | |
Magnesium iodide is the name for the chemical compounds with the formulas MgI2 and its various hydrates MgI2(H2O)x. These salts are typical ionic halides, being highly soluble in water. Magnesium iodide has few commercial uses but can be used to prepare compounds for organic synthesis.
Reactions
Magnesium iodide can be prepared from magnesium oxide, magnesium hydroxide, and magnesium carbonate by treatment with hydroiodic acid[3]:
Magnesium iodide is stable at high heat under a hydrogen atmosphere, but decomposes in air at normal temperatures, turning brown from the release of elemental iodine. When heated in air, it decomposes completely to magnesium oxide [4].
Usage of magnesium iodide in the Baylis-Hillman reaction tends to give (Z)-vinyl compounds [5].
Template:Inorganic-compound-stub
References
- ↑
Perry, Dale L.; Phillips, Sidney L. (1995), Handbook of Inorganic Compounds, CRC Press, p. 240, ISBN 0849386713, retrieved 2007-12-09 Check date values in:
|accessdate=(help) - ↑ http://ptcl.chem.ox.ac.uk/MSDS/MA/magnesium_iodide.html
- ↑
Patnaik, Pradyot (2003), Handbook of Inorganic Chemicals, McGraw-Hill Professional, pp. 527–528, ISBN 0070494398, retrieved 2007-12-09 Check date values in:
|accessdate=(help) - ↑ N. T. M., Wilsmore (1891). "Note on Magnesium Iodide". In James Hector. Report of the Third Meeting of the Australasian Association for the Advancement of Science. Sydney: The Association. p. 116. Retrieved 2007-12-09.
- ↑
Tietze, Lutz-Friedjan; Brasche, Gordon; Gericke, Kersten (2006), Domino Reactions in Organic Synthesis, Wiley-VCH, p. 59, ISBN 3527290605, retrieved 2007-12-09 Check date values in:
|accessdate=(help)