Nitrogen trifluoride

Nitrogen trifluoride is the inorganic compound with the formula (NF
₃). It is a colorless, non-flammable, toxic gas with a slightly musty odor. In contrast with ammonia, it is nonbasic. It finds increasing use within the manufacturing of flat-panel displays, photovoltaics, LEDs and other microelectronics. NF
₃ is a greenhouse gas, with a global warming potential (GWP) 17,200 times greater than that of CO
₂ when compared over a 100-year period.

Nitrogen trifluoride can be prepared from the elements in the presence of an electric discharge. In 1903, Otto Ruff prepared nitrogen trifluoride by the electrolysis of a molten mixture of ammonium fluoride and hydrogen fluoride. It is far less reactive than the other nitrogen trihalides nitrogen trichloride, nitrogen tribromide, and nitrogen triiodide, all of which are explosive. Alone among the nitrogen trihalides it has a negative enthalpy of formation. It is prepared in modern times both by direct reaction of ammonia and fluorine and by a variation of Ruff's method. It is supplied in pressurized cylinders.

NF
₃ is slightly soluble in water without undergoing chemical reaction. It is nonbasic with a low dipole moment of 0.2340 D. By contrast, ammonia is basic and highly polar (1.47 D). This contrast reflects the differing electronegativities of H vs F.

Similar to dioxygen, NF₃ is a potent yet sluggish oxidizer. It oxidizes hydrogen chloride to chlorine:^{[citation needed]}

However, it only attacks (explosively) organic compounds at high temperatures. Consequently it is compatible under standard conditions with several plastics, as well as steel and Monel.

Above 200-300 °C, NF₃ reacts with metals, carbon, and other reagents to give tetrafluorohydrazine:

NF₃ reacts with fluorine and antimony pentafluoride to give the tetrafluoroammonium salt:

NF₃ and B₂H₆ react vigorously even at cryogenic temperatures to give nitrogen gas, boron trifluoride, and hydrofluoric acid.