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|Section2= |Section3= |Section7= |Section8= }} Sulfur dichloride is the chemical compound with the formula SCl2. This cherry-red liquid is the simplest sulfur chloride and one of the most common. It is used as a precursor to organosulfur compounds.〔Schmidt, M.; Siebert, W. "Sulphur" ''Comprehensive Inorganic Chemistry'' Vol. 2, ed. A.F. Trotman-Dickenson. 1973.〕 ==Chlorination of sulfur== SCl2 is produced by the chlorination of either elemental sulfur or disulfur dichloride.〔F. Fehér "Dichloromonosulfane" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 370.〕 The process occurs in a series of steps, some of which are: ::S8 + 4 Cl2 → 4 S2Cl2; ''ΔH'' = −58.2 kJ/mol ::S2Cl2 + Cl2 → 2 SCl2; ''ΔH'' = −40.6 kJ/mol The addition of Cl2 to S2Cl2 has been proposed to proceed via a mixed valence intermediate Cl3S-SCl. SCl2 undergoes even further chlorination to give SCl4, but this species is unstable at near room temperature. It is likely that several SxCl2 exist where x > 2. Disulfur dichloride, S2Cl2, is the most common impurity in SCl2. Separation of SCl2 from S2Cl2 is possible via distillation with PCl3 to form an azeotrope of 99% purity, however sulfur dichloride loses chlorine slowly at room temperature and reverts to disulfur dichloride. Pure samples may be stored in sealed glass ampules which develop a slight positive pressure of chlorine, halting the decomposition. 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「Sulfur dichloride」の詳細全文を読む スポンサード リンク
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