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Chemical compound From Wikipedia, the free encyclopedia
Trifluoramine oxide or Nitrogen trifluoride oxide (F3NO) is an inorganic molecule with strong fluorinating powers.
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Properties | |||
F3NO | |||
Molar mass | 87.001 g·mol−1 | ||
Appearance | Colourless gas | ||
Melting point | −161 °C (−258 °F; 112 K) | ||
Boiling point | −87.5 °C (−125.5 °F; 185.7 K) | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Trifluoramine oxide was first discovered in 1966 independently by two different groups. One way to produce it was by an electric discharge in a mixture of oxygen on nitrogen trifluoride. Another even less yielding method is by reacting noble metal fluorides (IrF6 or PtF6) with nitric oxide.[1] It is separated by distillation, and can be purified by treating it with potassium hydroxide solution which reacts with the other fluorine containing molecules produced.[1]
An alternate way to produce it is by burning nitric acid in fluorine, followed by rapid cooling.[2] Yet another way is the photochemical reaction of fluorine and nitrosyl fluoride: F2 + FNO → F3NO. This reaction can also happen with heat, but hot fluorine is hard to contain without a reaction with the container.[3] yet another production route is to thermally decompose nitrosyl hexafluoronickelate (NO)2NiF6 → ONF + ONF3 + NiF2.[4]
F3NO is a colourless gas at standard conditions. It has a critical temperature of 29.5 °C where the density is 0.593 g/cm3. Critical pressure is about 64 atmospheres.[5]
Trifluoramine oxide has a Trouton's constant of 20.7.[5] Heat of vapourisation at the boiling point is 3.85 kcal/mol.[5]
The F3NO molecule has C3V symmetry, with all the N-F bonds being equivalent. The shape is almost a tetrahedron as N-O bond is similar to the N-F bonds in nature.[1] The nuclear magnetic resonance (NMR) spectrum of 19F has a triplet line around −363 ppm. JNF is 136 Hz.[1] The infra red spectrum N-O stretch at 1687 cm−1, N-F stretch at 743 cm−1, unsymmetrical N-F stretch 887 cm−1 ∠ONF bend 528 cm−1, wither other bands at 558, 528, 801, 929, 1055, 1410, 1622, 1772, 2435, and 3345 cm−1.[1] The dipole moment is 0.0390 D.[6]
The N-O bond has 75% double bond character. This differs from the amine oxides where the amine is much more basic and with a positive charge.[5] The N-O bond-length is 1.158 Å; the N–F bond-length is 1.431 Å ; the bond angles ∠FNF is 101°; and the three bond angles ∠ONF = 117.[7]
Trifluoramine oxide is toxic, killing rats at a concentration between 200 and 500 ppm.[5]
On fluorinating other compounds nitrosyl fluoride (NOF) is formed.[8] Trifluoramine oxide does not react with water, glass or nickel, making it easier to handle.[1] The "adducts" formed with the pentafluorides, are actually hexafluoride salts containing the F2NO+ ion.[1]
Trifluoramine oxide reacts slowly with mercury, producing mercury fluorides, and nitrogen oxides.[5] Trifluoramine oxide is fairly stable when heated to 300 °C but slowly breaks up to fluorine and NO2F, NOF, NO2 and NO. The oxygen remains attached to the nitrogen during decomposition.[5]
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