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Magnesium bromide

\n{{Cite book\n| last = Lide\n| first = David R.\n| year = 1998\n| title = Handbook of Chemistry and Physics\n| edition = 87\n| location = Boca Raton, Florida\n| publisher = CRC...

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Magnesium bromide are inorganic compounds with the chemical formula MgBr2(H2O)x, 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.[2][3]

Synthesis

Magnesium bromide can be synthesized by treating magnesium oxide (and related basic salts) with hydrobromic acid.[3] It can also be made by reacting magnesium carbonate and hydrobromic acids, and collecting the solid left after evaporation.[2]

As suggested by its easy conversion to various hydrates, anhydrous MgBr2 is a Lewis acid. In the coordination polymer with the formula MgBr2(dioxane)2, Mg2+ adopts an octahedral geometry.[4]

Uses and reactions

Magnesium bromide is used as a Lewis acidcatalyst in some organic synthesis, e.g., in aldol reaction.[5]

Magnesium bromide also has been used as a tranquilizer[2] and as an anticonvulsant for treatment of nervous disorders.[6]

Magnesium bromide modifies the catalytic properties of palladium on charcoal.[7]

Magnesium bromide hexahydrate has properties as a flame retardant.[8]

Treatment of magnesium bromide with chlorine gives magnesium chloride. This reaction is employed in the production of magnesium chloride from brines.[9]

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.[10]

References

  1. ↑Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, Florida: CRC Press. pp. 4–67. ISBN 0-8493-0594-2.
  2. 123Gruyter, W. Concise Encyclopedia Chemistry, Walter de Gruyter & Company: Berlin, 1993; 612
  3. 1 2 Lewis, RJ Diccionario Químico Condensado de Hawley, 15.ª ed.; John Wiley & Sons Inc.: Nueva York, 2007; 777
  4. ↑ Fischer, Reinald; Görls, Helmar; Meisinger, Philippe R.; Suxdorf, Regina; Westerhausen, Matthias (2019). " Relación estructura-solubilidad de complejos de 1,4-dioxano de di(hidrocarbil)magnesio" . Chemistry – A European Journal . 25 (55): 12830– 12841. doi : 10.1002/chem.201903120 . PMC 7027550. PMID 31328293 .  
  5. ↑ Evans, David A.; Tedrow, Jason S.; Shaw, Jared T.; Downey, C. Wade (2002). "Reacciones anti-aldólicas diastereoselectivas catalizadas por haluros de magnesio de N-aciloxazolidinonas quirales". Journal of the American Chemical Society . 124 (3): 392– 393. doi : 10.1021/ja0119548 . PMID 11792206 . 
  6. ↑ Pradyot Patnaik. Manual de productos químicos inorgánicos . McGraw-Hill, 2002, ISBN 0-07-049439-8
  7. ↑ Bouzide, Abderrahim (2002). "Hidrogenación heterogénea altamente diastereoselectiva de olefinas mediada por bromuro de magnesio". Organic Letters . 4 (8): 1347– 50. doi : 10.1021/ol020032m . PMID 11950359 . 
  8. ↑ Mostashari, SM; Fayyaz, F. (2008). "Caracterización por XRD de las cenizas de un tejido celulósico quemado impregnado con hexahidrato de bromuro de magnesio como retardante de llama". Journal of Thermal Analysis and Calorimetry . 92 (3): 845. doi : 10.1007/s10973-007-8928-4 . S2CID 94416902 . 
  9. ↑ Seeger, Margarete; Otto, Walter; Flick, Wilhelm; Bickelhaupt, Friedrich; Akkerman, Otto S. (2000). «Compuestos de magnesio». Enciclopedia de química industrial de Ullmann . doi : 10.1002/14356007.a15_595 . ISBN 3-527-30673-0.
  10. ↑Hennings, Erik; Schmidt, Horst; Voigt, Wolfgang (2013). "Crystal Structures of Hydrates of Simple Inorganic Salts. I. Water-Rich Magnesium Halide Hydrates MgCl2·8H2O, MgCl2·12H2O, MgBr2·6H2O, MgBr2·9H2O, MgI2·8H2O and MgI2·9H2O". Acta Crystallographica Section C Crystal Structure Communications. 69 (11): 1292–1300. doi:10.1107/S0108270113028138. PMID 24192174.