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Metal halides are compounds between metals and halogens. Some, such as sodium chloride are ionic, while others are covalently bonded. Covalently bonded metal halides may be discrete molecules, such as uranium hexafluoride, or they may form polymeric structures, such as palladium chloride. The halogens can all react with metals to form metal halides according to the following equation: :2M + nX2 → 2MXn where M is the metal, X is the halogen, and MXn is the metal halide. File:NaCl polyhedra.png|Sodium chloride crystal structure File:Uranium-hexafluoride-unit-cell-3D-balls.png|Discrete UF6 molecules File:Alpha-palladium(II)-chloride-xtal-3D-balls.png|Infinite chains of one form of palladium chloride ==Preparation== In principle, most metal halides may be prepared by direct combination of the elements. For example, tin tetrachloride: :Sn + 2 Cl2 → SnCl4 In practice, this type of reaction may be very exothermic, hence impractical as a preparative technique. Additionally, many transition metals can adopt multiple oxidation states, which complicates matters. As the halogens are strong oxidizers, direct combination of the elements usually leads to a highly oxidized metal halide. For example, ferric chloride can be prepared thus, but ferrous chloride cannot. Heating the higher halides may produce the lower halides; this occurs by thermal decomposition or by disproportionation. For example, gold(III) chloride to gold(I) chloride:〔 :AuCl3 → AuCl + Cl2 at 160°C Metal halides are also prepared by the neutralization of a metal oxide, hydroxide, or carbonate with the appropriate halogen acid. For example, with sodium hydroxide:〔 :NaOH + HCl → NaCl + H2O Water may be removed by heat, vacuum, or the presence of anhydrous hydrohalic acid. Anhydrous metal chlorides suitable for preparing other coordination compounds may be dehydrated by treatment with thionyl chloride:〔 :MCl''n''·''x''H2O + ''x'' SOCl2 → MCl''n'' + x SO2 + 2''x'' HCl The silver and thallium(I) cations have a great affinity for halide anions in solution, and the metal halide quantitatively precipitates from aqueous solution. This reaction is so reliable that silver nitrate is used to test for the presence and quantity of halide anions. The reaction of silver cations with bromide anions: :Ag+ (aq) + Br− (aq) → AgBr (s) Some metal halides may be prepared by reacting oxides with halogenes in the presence of carbon: : 抄文引用元・出典: フリー百科事典『 ウィキペディア（Wikipedia）』 ■ウィキペディアで「Metal halides」の詳細全文を読む スポンサード リンク
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