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|Section2= |Section5= |Section8= }} }} Dioxygen difluoride is a compound of fluorine and oxygen with the molecular formula . It exists as an orange solid that melts into a red liquid at . It is an extremely strong oxidant and decomposes into oxygen and fluorine even at at a rate of 4% per day: its lifetime at room temperature is thus extremely short.〔 〕 Dioxygen difluoride reacts with nearly every chemical it encounters – even ordinary ice – leading to its onomatopoeic nickname "FOOF" (a play on its chemical structure). The material has no practical applications, but has been of theoretical interest. One laboratory's use of it was the synthesis of plutonium hexafluoride at unprecedentedly low temperatures, which was significant because previous methods for its preparation needed temperatures so high that the plutonium hexafluoride created would rapidly decompose. ==Preparation== Dioxygen difluoride can be obtained by subjecting a 1:1 mixture of gaseous fluorine and oxygen at low pressure (7–17 mmHg is optimal) to an electric discharge of 25–30 mA at 2.1–2.4 kV. A similar method was used for the first synthesis by Otto Ruff in 1933.〔 〕 Another synthesis involves mixing and in a stainless steel vessel cooled to , followed by exposing the elements to bremsstrahlung for several hours. A third method requires heating a mix of fluorine and oxygen to , and then rapidly cooling it using liquid oxygen. All of these methods involve synthesis according to the equation: : + → It also arises from the thermal decomposition of ozone difluoride:〔 〕 : → + ½ or :2 → 2 + 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「Dioxygen difluoride」の詳細全文を読む スポンサード リンク
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