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|Section2= |Section3= |Section7= |Section8= }} Sulfuryl fluoride (also spelled ''sulphuryl fluoride'') is the inorganic compound with the formula SO2F2. This easily condensed gas has properties more similar to sulfur hexafluoride than sulfuryl chloride, being resistant to hydrolysis even up to 150 °C.〔 ==Structure, preparation, reactions== The molecule is tetrahedral with C2v symmetry. The S-O distance is 140.5 pm, S-F is 153.0 pm. As predicted by VSEPR, the O-S-O angle is more open than the F-S-F angle, 124° and 97°, respectively.〔 One synthesis begins with the preparation of potassium fluorosulfite:〔Seel, F. "Potassium Fluorosulfite" Inorganic Syntheses 1967, IX, pages 113-115. .〕 :SO2 + KF → KSO2F This salt is then chlorinated to give sulfuryl chloride fluoride: :KSO2F + Cl2 → SO2ClF + KCl Further heating at 180 °C of potassium fluorosulfite with the sulfuryl chloride fluoride gives the desired product:〔Seel, F. "Sulfuryl Chloride Fluoride and Sulfuryl Fluoride" Inorganic Syntheses 1967, vol. IX, pages 111-113. 〕 :SO2ClF + KSO2F → SO2F2 + KCl + SO2 Heating metal fluorosulfonate salts also gives this molecule:〔 :Ba(OSO2F)2 → BaSO4 + SO2F2 It can be prepared by direct reaction of fluorine with sulfur dioxide: :SO2 + F2 → SO2F2 Sulfuryl fluoride is unreactive toward molten sodium metal.〔Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.〕 Similarly it is slow to hydrolyze, but eventually converts to sulfur trioxide.〔〔Cady, G.H., and S. Misra, Hydrolysis of Sulfuryl Fluoride, Inorganic Chemistry, 13 (4), 837-841, 1974. 〕 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「Sulfuryl fluoride」の詳細全文を読む スポンサード リンク
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