Nitrogen pentafluoride
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 [molecular geometry|trigonal bipyramidal] covalently bound molecule with symmetry group D3h, or, 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 and tetrafluoroammonium hexafluoroarsenate were made. 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. Theoretical studies also show the ionic compound is very likely to decompose to nitrogen trifluoride and fluorine gas.
Karl O. Christe synthesised bis hexafluoronickelate. He also prepared compounds with manganese, a fluorouranate, tetrafluoroammonium perchlorate, tetrafluoroammonium fluorosulfate and salts. 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 [Fluorine|], HF and [Nitrogen trifluoride|] as gases. This has CAS number 71485-49-9.
I. J. Solomon believed that nitrogen pentafluoride was produced by the thermal decomposition of, but experimental results were not reproduced.
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 hexafluoronitrate with space group I4/m. Over 151 GPa this is predicted to transform to with space group P4/n. A molecular compound is not stable under any pressure conditions.