Dioxygen difluoride

Dioxygen difluoride
Stick model of dioxygen difluoride
Stick model of dioxygen difluoride
Spacefill model of dioxygen difluoride
Spacefill model of dioxygen difluoride
Names
Preferred IUPAC name
Dioxygen difluoride
Systematic IUPAC name
Fluorooxygen hypofluorite
Other names
  • Monofluorooxygenyl hypofluorite
  • Peroxydifluoride
  • Oxygen perfluoride
  • Oxyfluoryl hypofluorite
  • Fluorine peroxide
  • FOOF
Identifiers
3D model (JSmol)
Abbreviations FOOF
ChEBI
ChemSpider
1570
UNII
  • InChI=1S/F2O2/c1-3-4-2 checkY
    Key: REAOZOPEJGPVCB-UHFFFAOYSA-N checkY
  • InChI=1/F2O2/c1-3-4-2
    Key: REAOZOPEJGPVCB-UHFFFAOYAK
  • FOOF
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
62.1 J/(mol·K)
277.2 J/(mol·K)
19.2 kJ/mol
58.2 kJ/mol
Related compounds
Related compounds
Hazards
GHS labelling:
GHS03: OxidizingGHS05: CorrosiveGHS06: ToxicGHS09: Environmental hazard
Danger
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 4: Very short exposure could cause death or major residual injury. E.g. VX gasFlammability 0: Will not burn. E.g. waterInstability 4: Readily capable of detonation or explosive decomposition at normal temperatures and pressures. E.g. nitroglycerinSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
4
0
4
OX
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)

Dioxygen difluoride is a compound of fluorine and oxygen with the molecular formula O2F2. It can exist as an orange-red 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]

  1. ^ Holleman, A. F.; Wiberg, E. (2001). Inorganic Chemistry. Academic Press. ISBN 978-0-12-352651-9.
  2. ^ Lowe, Derek (2010-02-23). "Things I Won't Work With: Dioxygen Difluoride". www.science.org. Retrieved 2022-05-26.