Magnesium iodide
| Magnesium iodide |
|
| 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) |
| 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) |
| Structure |
| Crystal structure |
Hexagonal (anhydrous)
Monoclinic (hexahydrate)
Orthorhombic (octahydrate) |
| Hydrates |
Hexahydrate, Octahydrate[1] |
| Hazards |
| R/S statement |
R: R36 R38 R42 R43 R61
S: S22 S36/37/39 S45 S53[2] |
| Supplementary data page |
| Related compounds |
| Other anions |
Magnesium fluoride
Magnesium bromide
Magnesium chloride |
| Other cations |
beryllium iodide
calcium iodide |
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]:
- MgO + 2 HI → MgI2 + H2O
- Mg(OH)2 + 2 HI → MgI2 + 2 H2O
- MgCO3 + 2 HI → MgI2 + CO2 + H2O
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].
References
 |
- ^ Perry, Dale L. & Phillips, Sidney L., , CRC Press, pp. 240, ISBN 0849386713, <http://books.google.com/books?id=0fT4wfhF1AsC&pg=PA240&dq=%22magnesium+iodide%22&as_brr=3&ei=jDZcR--DA4fQiwGJ9MGwAw&ie=ISO-8859-1&sig=OczmUrZd3qb3uYKwOHfdAoOKqyA>. Retrieved on 2007-12-09
- ^ http://ptcl.chem.ox.ac.uk/MSDS/MA/magnesium_iodide.html
- ^ Patnaik, Pradyot, , McGraw-Hill Professional, pp. 527-528, ISBN 0070494398, <http://books.google.com/books?id=Xqj-TTzkvTEC&pg=RA1-PA527&dq=%22magnesium+iodide%22&as_brr=3&ei=5DVcR4uFPKXQiQGOiemkAw&ie=ISO-8859-1&sig=QOvcMUABsG5Kn7NshePb2P0VMFg#PRA1-PA527,M1>. Retrieved on 2007-12-09
- ^ N. T. M., Wilsmore (1891). "Note on Magnesium Iodide". James Hector Report of the Third Meeting of the Australasian Association for the Advancement of Science: 116, Sydney: The Association. Retrieved on 2007-12-09.
- ^ Tietze, Lutz-Friedjan; Brasche, Gordon & Gericke, Kersten, , Wiley-VCH, pp. 59, ISBN 3527290605, <http://books.google.com/books?id=qijhLyZ6SokC&pg=PA59&dq=%22magnesium+iodide%22+reactions&as_brr=3&ei=m0BcR4HgAYq-igGB5sH6Aw&ie=ISO-8859-1&sig=hKziWjoeftgwxNyZMTGY5508YZc#PPA59,M1>. Retrieved on 2007-12-09
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