Oxygen fluoride

Oxygen fluorides are compounds of elements oxygen and fluorine with the general formula OnF2, where n = 1 to 6. Many different oxygen fluorides are known: Oxygen fluorides are compounds of elements oxygen and fluorine with the general formula OnF2, where n = 1 to 6. Many different oxygen fluorides are known: Oxygen fluorides are strong oxidizing agents with high energy and can release their energy either instantaneously or at a controlled rate. Thus, these compounds attracted a lot of attention as potential fuels in jet propulsion systems. Here are some synthesis methods and reactions of the three most common oxygen fluorides – oxygen difluoride (OF2), dioxygen difluoride (O2F2) and ozone difluoride (O3F2). 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. It reacts quantitatively with aqueous haloacids to give free halogens: It can also displace halogens from their salts. It is both an effective fluorinating agent and a strong oxidizing agent. When reacted with unsaturated nitrogen fluorides with electrical discharge, it results in the formation of nitrogen trifluoride, oxide fluorides and other oxides. O2F2 precipitates as a brown solid upon the UV irradiation of a mixture of liquid O2 and F2 at -196 °C. It also only appears to be stable below -160 °C. The general method of preparation of a lot of oxygen fluorides is a gas-phase electric discharge in cold containers including O2F2. It is typically an orange-yellow solid which rapidly decomposes to O2 and F2 close to its normal boiling point of about 216 K. O2F2 reacts violently with red phosphorus, even at -196 °C. Explosions can also occur if Freon-13 is used to moderate the reaction.