Hexaoxygen difluoride
Identifiers
InChI=1S/F2O6/c1-3-5-7-8-6-4-2
Key: PHJAHINOOJESQK-UHFFFAOYSA-N
Properties
F 2 O 6
Molar mass
133.991 g·mol−1
Appearance
dark-brown solid at 60 K
Except where otherwise noted, data are given for materials in their
standard state (at 25 °C [77 °F], 100 kPa).
Chemical compound
Hexaoxygen difluoride is a binary inorganic compound of fluorine and oxygen with the chemical formula O6 F2 .[1] [2] The compound is one of many known oxygen fluorides .[3]
Synthesis
The compound can be prepared by electric discharges through the F2 —O2 mixture of the certain molar ratio at 60 to 77 K. The ratio is predicted to be 6:2.[4]
Physical properties
Hexaoxygen difluoride is an oxidizing agent . At 60 K, the compound looks like a dark-brown crystalline solid. If slowly warmed, it decomposes to lower oxygen fluorides and ozone . If quickly warmed to 90 K, it explodes, creating O2 and F2 .[4]
References
^ Streng, A. G.; Grosse, A. V. (January 1966). "Two New Fluorides of Oxygen, O5 F2 and O6 F2 1,2" . Journal of the American Chemical Society . 88 (1): 169–170. doi :10.1021/ja00953a035 . Retrieved 19 May 2023 .
^ Bailar, John Christian; Trotman-Dickenson, A. F. (1973). Comprehensive Inorganic Chemistry: Ge, Sn, Pb, Group VB, Group VIB, Group VIIB . Pergamon Press . p. 764. ISBN 978-0-08-017275-0 . Retrieved 19 May 2023 .
^ Bretherick, L. (27 October 2016). Bretherick's Handbook of Reactive Chemical Hazards . Elsevier . p. 1622. ISBN 978-1-4831-6250-8 . Retrieved 19 May 2023 .
^ a b F Fluorine: Compounds with Oxygen and Nitrogen . Springer Science & Business Media . 29 June 2013. p. 134. ISBN 978-3-662-06339-2 . Retrieved 19 May 2023 .
PF6 − , AsF6 − , SbF6 − compounds AlF6 − compounds chlorides, bromides, iodides and pseudohalogenides SiF6 2- , GeF6 2- compounds Oxyfluorides Organofluorides with transition metal, lanthanide, actinide, ammonium nitric acids bifluorides thionyl, phosphoryl, and iodosyl