Dioxygenyl
The dioxygenyl ion,, has been studied in both the gas phase and in salts with anions that cannot be oxidized. The first synthesis was . Rather than the double bond of, the bond order is considered to be. 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.
Structure and molecular properties
has a bond order of 2.5, and a bond length of 112.3 pm in solid O2. It is isoelectronic with nitric oxide and is paramagnetic. The bond energy is 625.1 kJ mol−1 and the stretching frequency is 1858 cm−1, both of which are high relative to most of the molecules.Synthesis
demonstrated that dioxygenyl hexafluoroplatinate, containing the dioxygenyl cation, can be prepared at room temperature by direct reaction of oxygen gas with platinum hexafluoride :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:
At lower temperatures, 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 led Bartlett to reason that it should also be able to oxidise xenon. His subsequent investigation yielded the first compound of a noble gas, xenon hexafluoroplatinate.
is also found in similar compounds of the form O2MF6, where M is arsenic, antimony, gold, niobium, ruthenium, rhenium, rhodium, vanadium, or phosphorus. Other forms are also attested, including O2GeF5 and 2SnF6.
The tetrafluoroborate and hexafluorophosphate salts may be prepared by the reaction of dioxygen difluoride with boron trifluoride or phosphorus pentafluoride at −126 °C:
These compounds rapidly decompose at room temperature:
Some compounds including O2Sn2F9, O2Sn2F9·0.9HF, O2GeF5·HF, and O249 can be made by ultraviolet irradiation of oxygen and fluorine dissolved in anhydrous hydrogen fluoride with a metal oxide.
All attempts to prepare with chloro anions like met with failure.
Reactions
The reaction of O2BF4 with xenon at produces a white solid believed to be F–Xe–BF2, containing an unusual xenon-boron bond:The dioxygenyl salts O2BF4 and O2AsF6 react with carbon monoxide to give oxalyl fluoride, C2O2F2, in high yield.