Sulfuryl difluoride

Synonyms Sulfuric oxyfluoride sulfuryl difluoride Vikane... 

Sulfuryl difluoride is also called sulfonyl difluoride or sulfonyl fluoride. 

Nitric oxide and OF2 inflame on contact emission and absorption spectra of the flame have been studied (24). Oxygen difluoride oxidizes SO2 to SO, but under the influence of uv kradiation it forms sulfuryl fluoride [2699-79-8] SO2F2, and pyrosulfuryl fluoride [37240-33-8] S20 F2 (25). Photolysis of SO —OF2 mixtures yields the peroxy compound FSO2OOF [13997-94-9] (25,26). 

Xenon difluoride labelled with positron-emitting F has been prepared by reaction of cyclotron produced [ F]p2 with xenon [88]. This low-yielding method requires high pressure. [ F]Xep2 was also obtained by treating sulfuryl chloride fluoride solutions of Xep2 in fluorinated ethylene propylene vessels with Bronst-... 

Thiadiazole oxides and reduced forms are readily prepared via [4 -h 1] cyclizations (Table 4). The reagents employed for this purpose are thionyl chloride, sulfuryl chloride, sulfur tetrafluoride, N,N -bis(p-toluenesulfonyl)sulfur diimide, cyclic diimides, pentafluoroethyliminosulfur difluoride and sulfamide. 

At ambient temperature xenon difluoride is very soluble in hydrogen fluoride, bromine trifluoride, iodine pentafluoride, sulfur dioxide, sulfuryl chloride fluoride, acetonitrile it is... 

Ethylene dithioacetals of benzophenone and its 4-fluoro-, 4-bromo-, 4,4 -difluoro-, 4,4 -dichlo-ro-, and 3,5-dimethyl-substituted analogs react with sulfuryl chloride or sttlfuryl chloride fluoride in hydrogen fluoride/ pyridine at — 78 C to room temperature to give the corresponding geminal difluorides in 85-90% yield. The reaction is, however, not applicable to dialkyl or alkyl aryl ketones as they undergo chlorination under these conditions.73... 

The yield is reduced by small amounts of water (formation of sulfuryl fluoride and oxygen difluoride oxygen difluoride reacts with hydrogen sulfide to form water and sulfur). Explosions have been observed in cases involving impure hydrogen sulfide and a water-containing electrolyte. 

Bis[pentafluoroethyl] ditellurium reacted with a slurry of xenon difluoride/sulfuryl fluoride in the temperature range — 45 to 20°. Pentafluoroethyl tellurium trifluoride was obtained as a crystalline solid in quantitative yield5. 

Bis pentafluoroethyl] tellurium difluoride (m.p. 57°) was obtained in quantitative yield from bis[pentafluoroethyl] tellurium and a mixture of xenon difluoride and sulfuryl chloride fluoride at — 45°4. 

This method is convenient because the reagents are easier to handle compared with molecular chlorine or fluorine. Trimethylbismuth dichloride is obtainable by using sulfuryl chloride at low temperatures [94AG(E)976]. However, an attempt to synthesize trimethylbismuth difluoride by using xenon difluoride has failed. 

Moissan and Lebeau (1901) produced sulfuryl fluoride by the combination of sulfur dioxide with fluorine (217). Other processes which have been used to produce the gas are (a) the thermal decomposition of barium fluorosulfonate or certain other fluorosulfonates (188, 221, 808), (b) the reaction of sulfur dioxide with chlorine and hydrogen fluoride in the presence of activated charcoal at 400° (11), (c) the reaction of sulfur dioxide and chlorine with potassium or sodium fluoride at 400° (328), (d) the disproportionation of sulfuryl chlorofluoride at 300-400° (328), (e) the reaction of sulfuryl chloride with a mixture of antimony trifluoride and antimony pentachloride at about 250° (86), (f) the reaction of sulfur dioxide with silver difluoride (86), (g) the reaction of thionyl fluoride with oxygen in an electrical discharge (314), (h) electrolysis of a solution of fluorosulfonic acid in hydrogen fluoride (264), ( ) the reaction of fluorine with sodium sulfate, sodium sulfite or sodium thiosulfate (229, 239), (j) the reaction of hydrogen fluoride with sulfuryl chloride (820). 

EXPLOSION and FIRE CONCERNS nonflammable gas NFPA rating (none) can contain variable quantities of the low-sulfur fluorides (e.g., sulfur pentafluoride) which are highly toxic very reactive chemically, and corrosive in nature materials can hydrolyze on contact with water to yield highly toxic and very corrosive hydrogen fluoride may act as a simple asphyxiant when pure and in high concentrations incompatible with disilane may be explosive hazardous decomposition products include monosulfur fluoride, tetrasulflir fluoride, sulfuryl fluoride, sulfurous fluoride, sulfuric fluoride, decasulfur difluoride and other toxic fluoride compounds if cylinders are involved in a fire, keep cool with water spray. 

F2SO2 Sulfuryl fluoride, 6 158 F2S2O6 Peroxydisulfuryl difluoride, 7 124... 

Examples of toxic compounds, including some important intermediates and starting materials in the chemical industry, are shown in Figure 3.3. Many alkali fluorides, such as alkali hexafluorosilicate, alkali hydrogen difluoride, or alkali sulfuryl fluoride, are well known toxic substances. Sulfur dioxide and ammonia (ubiquitous gases) are toxic, as are chlorine, metallic mercury vapors, many organic phenol compounds, amino aromatic compounds such as aniline, and many substituted amino-benzene derivatives. Additionally, many diisocyanates are toxic, e.g., 2,4- and 2,6-toluene diisocyanate (TDI), hexamethylene diisocyanate (HDI), chloro-, bromo-, and iodoacetic acid, methyl bromide, tribromomethane (bromoform), carbon tetrachloride, and formaldehyde. Also, many natural compounds present in many plants have toxic properties, and a selection of these are listed in Table 3.4. 

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