Hydrazinium fluoride

FIG. 8.5. The structure of hydrazinium fluoride N2HJF2 (after Kronberg and Marker) (a) Plan of one layer. The lower N atoms of each N2Hj ion (shaded) are slightly displaced. The open circles, full and dotted lines, represent F ions respectively above and below the plane of the paper. All lines are N-H-F bonds, (b) Elevation, showing the packing of the layers. The broken line is the trace of the plane of the paper in (a). 

Simple hydrazinium fluoride is prepared by the reaction of ammonium fluoride with hydrazine hydrate ... 

It can also be prepared by isothermal heating of hydrazinium fluoride at 160 °C ... 

The above book [1] deals, in 26 chapters in 5 sections, with theoretical and practical aspects of the use and safe handling of powerful oxidants and their complementary reactive fuels. Materials include nitrogen pentaoxide, perfluoroam-monium ion and salts, nitronium tetrafluoroborate, hydrazinium mono- and diperchlorates, nitronium perchlorate, tricyanomethyl compounds, difluoramine and its alkyl derivatives, oxygen difluoride, chlorine trifluoride, dinitrogen tetraoxide, bromine trifluoride nitrogen fluorides, and liquid ozone-fluorine system. 

ESTANO (Spanish) (7440-31-5) Finely divided material is combustible and forms explosive mixture with air. Contact with moisture in air forms tin dioxide. Violent reaction with strong acids, strong oxidizers, ammonium perchlorate, ammonium nitrate, bis-o-azido benzoyl peroxide, bromates, bromine, bromine pentafluoride, bromine trifluoride, bromine azide, cadmium, carbon tetrachloride, chlorine, chlorine monofluoride, chlorine nitrate, chlorine pentafluoride, chlorites, copper(II) nitrate, fluorine, hydriodic acid, dimethylarsinic acid, ni-trosyl fluoride, oxygen difluoride, perchlorates, perchloroethylene, potassium dioxide, phosphorus pentoxide, sulfur, sulfur dichloride. Reacts with alkalis, forming flammable hydrogen gas. Incompatible with arsenic compounds, azochloramide, benzene diazonium-4-sulfonate, benzyl chloride, chloric acid, cobalt chloride, copper oxide, 3,3 -dichloro-4,4 -diamin-odiphenylmethane, hexafluorobenzene, hydrazinium nitrate, glicidol, iodine heptafluoride, iodine monochloride, iodine pentafluoride, lead monoxide, mercuric oxide, nitryl fluoride, peroxyformic acid, phosphorus, phosphorus trichloride, tellurium, turpentine, sodium acetylide, sodium peroxide, titanium dioxide. Contact with acetaldehyde may cause polymerization. May form explosive compounds with hexachloroethane, pentachloroethane, picric acid, potassium iodate, potassium peroxide, 2,4,6-trinitrobenzene-1,3,5-triol. 

HEXAHYDRATE (10377-60-3) A powerful oxidizer. Reacts violently with dimethyl-formamide, reducing agents, combustible materials, fuels, organic substances, metal powders, potassium hexanitrocobalite(III) (C.I. pigment yellow), sodium acetylide, and easily oxidizable matter. Incompatible with aluminum, ammonium hexacyanoferrate(II), tert-butylhydroperoxide, citric acid, ethanol, ferrocyanides, hydrazinium perchlorate, isopropyl chlorocarbonate, metal phosphinates, nitrosyl perchlorate, organic azides, phosphorus, sodium thiosulfate, sulfamic acid, thiocyanates, tin(II) fluoride, and many other substances. 

SODIUM IODIDE (7681-82-5) Reacts violently with bromotrifluoride, perchloric acid, perchloryl fluoride, oxidants, chlorine trifluoride, fluorine, hydrazine. Incompatible with acrolein, isopropyl chlorocarbonate, mercuric salicylate, mercurous chloride, nitrosyl perchlorate, paraldehyde, peroxyfuroic acid, phosphorus pentoxide, silver nitrate, sodium acetylide, sodium borohydride. May sensitize organie azides, hydrazinium perchlorate. 

HAZARD RISK Powdered cobalt ignites spontaneously in air ignites on contact with bromine pentafluoride incandescent reaction with acetylene or nitryl fluoride explosive reaction with hydrazinium nitrate, ammonium nitrate plus heat, 1,3,4,7-tetramethylisoindole may produce acrid smoke and fumes when heated to decomposition NFPA code H2 FO RO (cobalt oxide and cobalt chloride). 

N2H5F), Hydrazinium Bifluoride (N2H5HF2), and Hydrazonium Fluoride (N2H6F2)... 

As mentioned in Chapter 1, the development of inorganic derivatives by complex formation with organic anions is of interest from the viewpoint of generating new precursors [7-12]. Several hydrazinium fluorometal-lates have been investigated as their decomposition offers a convenient route for the synthesis of binary fluorides [6]. 

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