Magnesium bromide
Template:Chembox Magnesium bromide are inorganic compounds with the chemical formula Template:Chem2, where x can range from 0 to 9. They are all white deliquescent solids. Some magnesium bromides have been found naturally as rare minerals such as: bischofite and carnallite.[1][2]
Synthesis
Magnesium bromide can be synthesized by treating magnesium oxide (and related basic salts) with hydrobromic acid.[2] It can also be made by reacting magnesium carbonate and hydrobromic acids, and collecting the solid left after evaporation.[1]
As suggested by its easy conversion to various hydrates, anhydrous Template:Chem2 is a Lewis acid. In the coordination polymer with the formula MgBr2(dioxane)2, Mg2+ adopts an octahedral geometry.[3]
Uses and reactions
Magnesium bromide is used as a Lewis acid catalyst in some organic synthesis, e.g., in aldol reaction.[4]
Magnesium bromide also has been used as a tranquilizer[1] and as an anticonvulsant for treatment of nervous disorders.[5]
Magnesium bromide modifies the catalytic properties of palladium on charcoal.[6]
Magnesium bromide hexahydrate has properties as a flame retardant.[7]
Treatment of magnesium bromide with chlorine gives magnesium chloride. This reaction is employed in the production of magnesium chloride from brines.[8]
Structure
Two hydrates are known, the hexahydrate and the nonahydrate. Several reports claim a decahydrate, but X-ray crystallography confirmed that it is a nonahydrate. The hydrates feature [Mg(H2O)6]2+ ions.<ref>Script error: No such module "Citation/CS1".</ref it can also cause violently convulsing and potential release of bowels
References
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- ↑ a b c Gruyter, W. Concise Encyclopedia Chemistry, Walter de Gruyter & Company: Berlin, 1993; 612
- ↑ a b Lewis, R.J. Hawley’s Condensed Chemical Dictionary, 15th ed.; John Wiley & Sons Inc.:New York, 2007; 777
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- ↑ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, Template:ISBN
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Template:Magnesium compounds Template:Bromides Template:Bromine compounds