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CLF3 DIPOLE MOMENT FREE
Pure ClF 3 is stable to 180 ☌ (356 ☏) in quartz vessels above this temperature, it decomposes by a free radical mechanism to its constituent elements. The elongated Cl-F axial bonds are consistent with hypervalent bonding. 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 molecular geometry of ClF 3 is approximately T-shaped, with one short bond (1.598 Å) and two long bonds (1.698 Å). It was first reported in 1930 by Ruff and Krug who prepared it by fluorination of chlorine this also produced Chlorine monofluoride (ClF) and the mixture was separated by distillation. The compound is primarily of interest in plasmaless cleaning and etching operations in the semiconductor industry, in nuclear reactor fuel processing, historically as a component in rocket fuels, and various other industrial operations owing to its corrosive nature. Despite being famous for its extreme oxidation properties and igniting many things, chlorine trifluoride is not combustible itself. This colorless, 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).
Chlorine trifluoride is an interhalogen compound with the formula ClF 3.
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