The energy change for this process is called the ionization energy of the oxygen molecule. Relative to most molecules, this ionization energy is very high at 1175 kJ/mol. As a result, the scope of the chemistry of is quite limited, acting mainly as a 1-electron oxidiser.
The compound can also be prepared from a mixture of fluorine and oxygen gases in the presence of a platinum sponge at 450 °C, and from oxygen difluoride above 400 °C:
6 + 2 Pt -> 2 +
At lower temperatures (around 350 °C), platinum tetrafluoride is produced instead of dioxygenyl hexafluoroplatinate. Dioxygenyl hexafluoroplatinate played a pivotal role in the discovery of noble gas compounds. The observation that PtF6 is a powerful enough oxidising agent to oxidise O2 (which has a first ionization potential of 12.2 eV) led Bartlett to reason that it should also be able to oxidise xenon (first ionization potential 12.13 eV). His subsequent investigation yielded the first compound of a noble gas, xenon hexafluoroplatinate.
These compounds rapidly decompose at room temperature:
2 O2BF4 -> 2 O2 + F2 + 2 BF3
2 O2PF6 -> 2 O2 + F2 + 2 PF5
Some compounds including O2Sn2F9, O2Sn2F9·0.9HF, O2GeF5·HF, and O2[Hg(HF)]4(SbF6)9 can be made by ultraviolet irradiation of oxygen and fluorine dissolved in anhydrous hydrogen fluoride with a metal oxide.
The reaction of O2BF4 with xenon at 173 K (-100 °C) produces a white solid believed to be F-Xe-BF2, containing an unusual xenon-boron bond:
^Goetschel, C. T.; Loos, K. R. (1972). "Reaction of xenon with dioxygenyl tetrafluoroborate. Preparation of FXe-BF2". Journal of the American Chemical Society. 94 (9): 3018-3021. doi:10.1021/ja00764a022.
^Pernice, H.; Willner, H.; Eujen, R. (2001). "The reaction of dioxygenyl salts with 13 CO Formation of F13 C(O)13 C(O)F". Journal of Fluorine Chemistry. 112 (2): 277-590. doi:10.1016/S0022-1139(01)00512-7.