Dioxygen difluoride

Dioxygen difluoride
Stick 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
CAS Number	7783-44-0 ;
3D model (JSmol)	Interactive image;
Abbreviations	FOOF
ChEBI	CHEBI:47866 ;
ChemSpider	109870 ;
Gmelin Reference	1570
PubChem CID	123257;
UNII	XWQ158QF24 ;
CompTox Dashboard (EPA)	DTXSID70228451 ;
	InChI InChI=1S/F2O2/c1-3-4-2 Key: REAOZOPEJGPVCB-UHFFFAOYSA-N ; InChI=1/F2O2/c1-3-4-2 Key: REAOZOPEJGPVCB-UHFFFAOYAK;
	SMILES FOOF;
Properties
Chemical formula	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)	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⦵)	58.2 kJ/mol
Related compounds
Related compounds	O; 3F; 2; H; 2O; 2; OF; 2; FClO; 2; Cl; 2O; 2; S; 2Cl; 2; S; 2F; 2;
Hazards
	GHS labelling:
Pictograms
Signal word	Danger
NFPA 704 (fire diamond)	4 0 4 OX
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references

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]

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

[Holl-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.

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