Oxygen fluoride

[5] A common preparative method involves fluorination of sodium hydroxide: OF2 is a colorless gas at room temperature and a yellow liquid below 128 K. Oxygen difluoride has an irritating odor and is poisonous.

[9] The general method of preparation of many oxygen fluorides is a gas-phase electric discharge in cold containers including O2F2.

[10] It is typically an orange-yellow solid which rapidly decomposes to O2 and F2 close to its normal boiling point of about 216 K.[3] O2F2 reacts violently with red phosphorus, even at −196 °C.

However, the oxygen monofluoride radicals are assumed to not play as big a role in the ozone depletion because free fluorine atoms in the atmosphere are believed to react with methane to produce hydrofluoric acid which precipitates in rain.

The mechanism involves the boiling off oxygen from the solution containing O3F2, making it more reactive to have a spontaneous reaction with the rocket fuel.