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Names | |||
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Preferred IUPAC name
Dioxygen difluoride | |||
Systematic IUPAC name
Fluorooxygen hypofluorite | |||
Other names
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Identifiers | |||
3D model (JSmol)
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Abbreviations | FOOF | ||
ChEBI | |||
ChemSpider | |||
1570 | |||
PubChem CID
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UNII | |||
CompTox Dashboard (EPA)
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Properties | |||
O 2F 2 | |||
Molar mass | 69.996 g·mol−1 | ||
Appearance | orange as a solid red as a liquid | ||
Density | 1.45 g/cm3 (at b.p.) | ||
Melting point | −154 °C (−245 °F; 119 K) | ||
Boiling point | −57 °C (−71 °F; 216 K) extrapolated | ||
Solubility in other solvents | decomposes | ||
Thermochemistry | |||
Heat capacity (C)
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62.1 J/(mol·K) | ||
Std molar
entropy (S⦵298) |
277.2 J/(mol·K) | ||
Std enthalpy of
formation (ΔfH⦵298) |
19.2 kJ/mol | ||
Gibbs free energy (ΔfG⦵)
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58.2 kJ/mol | ||
Related compounds | |||
Related compounds
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Hazards | |||
GHS labelling: | |||
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Danger | |||
NFPA 704 (fire diamond) | |||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Dioxygen difluoride is a compound of fluorine and oxygen with the molecular formula O2F2. It can exist as an orange-colored solid which melts into a red liquid at −163 °C (110 K). It is an extremely strong oxidant and decomposes into oxygen and fluorine even at −160 °C (113 K) at a rate of 4% per day — its lifetime at room temperature is thus extremely short.[1] Dioxygen difluoride reacts vigorously with nearly every chemical it encounters (including ordinary ice) leading to its onomatopoeic nickname FOOF (a play on its chemical structure and its explosive tendencies).[2]