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|Section2= |Section3= |Section4= |Section5= |Section6= }} Chlorine trifluoride is an interhalogen compound with the formula ClF3. This colourless, poisonous, corrosive, and extremely reactive gas condenses to a pale-greenish yellow liquid, the form in which it is most often sold (pressurized at room temperature). The compound is primarily of interest as a component in rocket fuels, in plasmaless cleaning and etching operations in the semiconductor industry,〔(United States Patent 5849092 "Process for chlorine trifluoride chamber cleaning" )〕 in nuclear reactor fuel processing, and other industrial operations.〔(United States Patent 6034016 "Method for regenerating halogenated Lewis acid catalysts" )〕 ==Preparation, structure, and properties== It was first reported in 1930 by Ruff and Krug who prepared it by fluorination of chlorine; this also produced ClF and the mixture was separated by distillation.〔 〕 :3 F2 + Cl2 → 2 ClF3 ClF3 is approximately T-shaped, with one short bond (1.598 Å) and two long bonds (1.698 Å). This structure agrees with the prediction of VSEPR theory, which predicts lone pairs of electrons as occupying two equatorial positions of a hypothetic trigonal bipyramid. The elongated Cl-F axial bonds are consistent with hypervalent bonding. Pure ClF3 is stable to 180 °C in quartz vessels; above this temperature it decomposes by a free radical mechanism to the elements. 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「chlorine trifluoride」の詳細全文を読む スポンサード リンク
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