Krypton difluoride
chemical compound
Krypton difluoride, KrF2 is a chemical compound of krypton and fluorine. It was the first compound of krypton discovered. It is a volatile, colourless solid at room temperature. The structure of the KrF2 molecule is linear, with Kr−F distances of 188.9 pm. It reacts with strong Lewis acids to form salts of the KrF+ and Kr2F3+ cations.
The atomization energy of KrF2 (KrF2(g) → Kr(g) + 2 F(g)) is 92 kJ/mol (21.9 kcal/mol), giving an average Kr–F bond energy of only 46 kJ/mol (11 kcal/mol), the weakest of any isolable fluoride. In comparison, the dissociation of difluorine to atomic fluorine requires cleaving a F–F bond with a bond dissociation energy of 150 kJ/mol (36 kcal/mol). Consequently, KrF2 is a good source of the extremely reactive and oxidizing atomic fluorine. It is thermally unstable, with a decomposition rate of 10 % per hour at room temperature. The formation of krypton difluoride is endothermic, with a heat of formation (gas) of 57–64 kJ/mol (13.6–15.2 kcal/mol) measured at 93 °C.
Synthesis
Krypton difluoride can be synthesized using many different methods including electrical discharge, photoionization, hot wire, and proton bombardment.
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