Nitrogen pentafluoride explained

Nitrogen pentafluoride is a theoretical compound of nitrogen and fluorine with the chemical formula . It is hypothesized to exist based on the existence of the pentafluorides of the atoms below nitrogen in the periodic table, such as phosphorus pentafluoride. Theoretical models of the nitrogen pentafluoride molecule are either a trigonal bipyramidal covalently bound molecule with symmetry group D3h, or (tetrafluoroammonium fluoride), which would be an ionic solid.

Ionic solid

A variety of other tetrafluoroammonium salts are known, as are fluoride salts of other ammonium cations .

In 1966, W. E. Tolberg first synthesized a five-valent nitrogen compound of nitrogen and fluorine when tetrafluoroammonium compounds, tetrafluoroammonium hexafluoroantimonate(V) and tetrafluoroammonium hexafluoroarsenate(V) were made.[1] In 1971 C. T. Goetschel announced the preparation of and also produced a white solid assumed to be tetrafluoroammonium fluoride . This was made by treating nitrogen trifluoride and fluorine with 3 MeV electron radiation at 77 K. It decomposed above 143 K back into those ingredients.[1] Theoretical studies also show the ionic compound is very likely to decompose to nitrogen trifluoride and fluorine gas.[2]

Karl O. Christe synthesised bis(tetrafluoroammonium) hexafluoronickelate(IV) .[3] He also prepared compounds with manganese, a fluorouranate, tetrafluoroammonium perchlorate, tetrafluoroammonium fluorosulfate and (trifluorodiazenium) salts.[4] Christe attempted to make by metathesis of with CsF in HF solvent at 20 °C. However, a variant, tetrafluoroammonium bifluoride hydrofluorates, was produced. At room temperature it was a milky liquid, but when cooled, turned pasty. At −45 °C it had the form of a white solid. When reheated it frothed, giving off , HF and as gases.[4] This has CAS number 71485-49-9.[5]

I. J. Solomon believed that nitrogen pentafluoride was produced by the thermal decomposition of, but experimental results were not reproduced.[6]

Dominik Kurzydłowski and Patryk Zaleski-Ejgierd predict that a mixture of fluorine and nitrogen trifluoride under pressure between 10 and 33 GPa forms with space group R3m. This is a high-pressure oxidation. Over 33 GPa it will form a stable ionic compound with formula (bis(tetrafluoroammonium) hexafluoronitrate(V) fluoride) with space group I4/m. Over 151 GPa this is predicted to transform to (tetrafluoroammonium hexafluoronitrate(V)) with space group P4/n.[7] A molecular compound is not stable under any pressure conditions.

Covalent molecule

For a molecule to form, five fluorine atoms have to be arranged around a nitrogen atom. There is insufficient space to do this at typical nitrogen–fluorine covalent-bond lengths, so at least some bonds are forced to be longer. Calculations show that fragmentation to form and F radicals would have a transition state barrier of around NaNorder=flipNaNorder=flip and that this process is thermodynamically favourable (exothermic) by 9order=flipNaNorder=flip.[8] Nitrogen pentafluoride also violates the octet rule in which compounds with eight outer shell electrons are particularly stable.[9]

Notes and References

  1. Goetschel . C. T. . V. A. Campanile . R. M. Curtis . K. R. Loos . C. D. Wagner . J. N. Wilson . 3. Preparation and properties of perfluoroammonium tetrafluoroborate, [NF<sub>4</sub>]+[BF<sub>4</sub>], and possible synthesis of nitrogen pentafluoride . July 1972 . Inorganic Chemistry . 11 . 7 . 1696–1701 . 10.1021/ic50113a051.
  2. Christe . Karl O. . William W. Wilson . December 1992 . Nitrogen pentafluoride: covalent NF5 versus ionic NF4+F and studies on the instability of the latter . Journal of the American Chemical Society . 114 . 25 . 9934–9936 . 10.1021/ja00051a027.
  3. Christe . Karl O. . September 1977 . Synthesis and characterization of bis(tetrafluoroammonium) hexafluoronickelate . Inorganic Chemistry . 16 . 9 . 2238–2241 . 10.1021/ic50175a017.
  4. Web site: Research Studies in NF4+ Salts . https://web.archive.org/web/20151227005623/http://www.dtic.mil/dtic/tr/fulltext/u2/a086981.pdf . live . December 27, 2015 . Christe . Karl O. . 23 May 1980 . Rockwell . 23 February 2012.
  5. Tetrafluoroammonium bifluoride
  6. Christe . Karl O.. William W. Wilson . Gary J. Schrobilgen . Raman V. Chirakal . George A. Olah . 3. March 1998 . On the existence of pentacoordinated nitrogen . Inorganic Chemistry . 27 . 5 . 789–790 . 10.1021/ic00278a009.
  7. Kurzydłowski . Dominik . Zaleski-Ejgierd . Patryk . Hexacoordinated nitrogen(V) stabilized by high pressure . Scientific Reports . 3 November 2016 . 6 . 36049 . 10.1038/srep36049 . 27808104 . 5093683 . 2016NatSR...636049K.
  8. Holger F. Bettinger . Paul v. R. Schleyer . Henry F. Schaefer III . NF5 — Viable or Not?. Journal of the American Chemical Society. 27 October 1998. 120. 44. 11439–11448. 10.1021/ja9813921.
  9. Book: Lewars, Errol G. . Modeling marvels: computational anticipation of novel molecules. https://books.google.com/books?id=IoFzgBSSCwEC. 3 November 2008. Springer. 53–67. Nitrogen Pentafluoride and Related Compounds. 978-1-4020-6972-7. 10.1007/978-1-4020-6973-4_4.