Sulfur monofluoride

D. Disuleur Difluoride ( Sulfur Monofluoride ) and Sulfur Difluoride... 

Leclanche or dry cell Alkaline Cell Silver-Zinc Reuben Cell Zinc-Air Fuel Cell Lithium Iodine Lithium-Sulfur Dioxide Lithium-Thionyl Chloride Lithium-Manganese Dioxide Lithium-Carbon Monofluoride... 

C03-0008. Write chemical formulas for the following compounds chlorine monofluoride, xenon trioxide, hydrogen bromide, silicon tetrachloride, sulfur dioxide, and hydrogen peroxide. 

Chlorine monofluoride is capable of oxidizing a sulfur atom bonded to one or two perfluoroalkyl groups through the addition of two or four fluorine atoms to the sulfur atom, depending on the ratio of the reagents and the reaction temperature. 

Oxidation of bis(trifluoromethyl) sulfide with commercially obtainable chlorine monofluoride in the absence of solvent yields bis(trifluoromethyl)sulfur difluoride in >90% yield.2,3 Pure bis-(trifluoromethyl)sulfur difluoride is resistant to hydrolysis and is stable in Pyrex glass at 25°C. for extended periods of time. Reaction of bis(trifluoromethyl)sulfur difluoride with anhydrous... 

Whereas the difference in the reactivity of RfCH=CHR/ and CF2=C(CF3)2 is marginal, the double bond in PFIB is significantly less reactive towards E+ compared to F-propylene. Most electrophilic reactions of this olefin proceed in a temperature range of 100-200°C. Among known reactions are those with HF, HgF2/HF, sulfur/SbF5, and iodine monofluoride [46] ... 

A good method for the chlorofluorination of halogenated alkenes is the use of hexachloro-melaminc and anhydrous hydrogen fluoride. Chlorofluoroalkanes can be prepared in yields of 25 to 70 % (see Table 18). Other reagents for chlorofluorinations are chlorine monofluoride, chlorine Irifluoride or the sulfur tetrafluoride/hydrogen fluoride/chlorinc system (see Table 18). 

The first reported preparations of sulfur chloride penta-fluoride involved the fluorination of sulfur(II) chloride, the chlorination of disulfur decafluoride, and the electrolysis of sulfur(II) chloride-hydrogen fluoride mixtures. Newer methods utilize the reaction between chlorine monofluoride and sulfur(IV) fluoride or the reaction between chlorine, cesium fluoride, and sulfur(IV) fluoride. The directions described here for the reaction between chlorine monofluoride and sulfur(IV) fluoride are for the preparation of substantial quantities if only a 1- or 2-g. sample is required, the modifications described in the last paragraph of the Procedure section may be employed or a batch pro-... 

TIN or TIN POWDER (7440-31-5) Sn Finely divided material is combustible and forms explosive mixture with air [autoignition temp (dust cloud) 1166°F/630°C]. Contact with moisture in 911 forms tin dioxide. A reducing agent the powder is very reactive. 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 + water, chlorine, chlorine monofluoride, chlorine nitrate, chlorine pentafluoride, chlorites, copper(II) nitrate, dimethylarsinic acid, fluorine, hydriodic acid, iodine heptafluoride, nitrosyl fluoride, oxygen difluoride, perchlorates, perchloroethylene, potassium dioxide, phosphorus pentoxide, sulfur, sulfur dichloride, turpentine (fire or explosion). 

Lithium batteries use nonaqueous solvents for the electrolyte because of the reactivity of lithium in aqueous solutions. Organic solvents such as acetonitrile, propylene carbonate, and dimethoxyethane and inorganic solvents such as thionyl chloride are typically employed. A compatible solute is added to provide the necessary electrolyte conductivity. (Solid-state and molten-salt electrolytes are also used in some other primary and reserve lithium cells see Chaps. 15, 20, and 21.) Many different materials were considered for the active cathode material sulfur dioxide, manganese dioxide, iron disulfide, and carbon monofluoride are now in common use. The term lithium battery, therefore, applies to many different types of chemistries, each using lithium as the anode but differing in cathode material, electrolyte, and chemistry as well as in design and other physical and mechanical features. 

These researches opened the door to the fabrication and commercialization of varieties of primary hthium batteries since the late l%0s nonaqueous hthium cells, especially the 3-V primary systems, have been developed. These systems include lithium-sulfur dioxide (Li//S02) cehs, lithium-polycarbon monofluoride (Li//(CF t) ) cells introduced by Matsuschita in 1973, lithium-manganese oxide (Li//Mn02) cells commercialized by Sanyo in 1975, lithium-copper oxide (Li//CuO) cells, lithium-iodine (Li//(P2VP)1J cells. During the same period, molten salt systems (LiCl-KCl eutecticum) using a Li-Al alloy anode and a FeS cathode were introduced [1]. The lithium-iodine battery has been used to power more than four million cardiac pacemakers since its introduction in 1972. During this time the lithium-iodine system has established a record of reliability and performance unsurpassed by any other electrochemical power source [18]. 

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