Disulfur tetrafluoride

Sulfur difluoride is difficult to make and is known only as a dilute gas. It dimerizes to form disulfur tetrafluoride (S2F4), which has a curious structure (12-XIX). One sulfur atom (S1) can be considered to occupy an incomplete trigonal bipyramid with two axial F atoms and with a lone pair, an F atom and an S—F group in the equatorial plane. 

Explain the difference between sulfur hexafluoride and disulfur tetrafluoride. 

Write a formula for each molecular compoimd. (a) carbon monoxide (b) disulfur tetrafluoride (c) dichlorine monoxide (d) phosphorus pentafluoride (e) boron tribromide (f) diphosphorus pentasulfide 74. Write a formula for each molecular compound. (a) chlorine monoxide (b) xenon tetroxide (c) xenon hexafluoride (d) carbon tetrabromide (e) diboron tetrachloride (f) tetraphosphorus triselenide... 

Nonmeta.ls, Sulfur reacts with fluorine to yield the remarkably stable sulfur hexafluoride, SF. Operating conditions must be controlled because a mixture of the lower fluorides such as disulfur difluoride [13709-35-8] 2 2 disulfur decafluoride [5714-22-7] 2 10 sulfur tetrafluoride [7783-60-0] SF4, may also be formed. When this reaction is carried out between 310 and 340°C, SF is primarily obtained and essentially no SF and only trace amounts of lower fluorides. Below 300°C, and preferably at ca 275°C, SF is the primary product. At 450—500°C, a mixture comprising ca 50% SF and the lower sulfur fluorides is formed (see Fluorine compounds, inorganic-sulfur). 

Disulfur decafluoride does not react rapidly with water, mercury, copper, or platinum at ambient temperatures. There is evidence that it slowly decomposes on various surfaces in the presence of water when stored in the vapor state (118). It is decomposed by molten KOH to give a mixture of potassium compounds of sulfur and fluorine. The gas reacts vigorously with many other metals and siUca at red heat (114). At ca 156°C it combines with CI2 or Br2 to form SF Cl or SF Br (119,120). At ca 200°C, S2F2Q is almost completely thermally decomposed into the hexa- and tetrafluoride (121). 

Bis(2-chloroethyl) ether (4) reacts with sulfur tetrafluoride, hydrogen fluoride and ca. 3 % disulfur dichloride (in relation to the ether) to give, depending on the reaction temperature, dichlorotrifluoro ether 5, chlorotetrafluoro ether 6, or pentafluoro ether 2.238... 

The reaction of acetone with sulfur tetrafluoride, hydrogen fluoride and a catalytic amount of disulfur dichloride gives, instead of 2,2-difluoropropane, polyfluorodipropyl sulfides 8, 9, or disulfide 10 in which the number of fluorine atoms depends on the reaction temperature. The same products are obtained when 2,2-difiuoropropane, a product of the replacement of the carbonyl group of acetone by fluorines, is treated with the same reagent (SF4/HF/S2C12).239... 

Similarly, butan-2-one, pentan-3-one, 2,2-difluorobutane and 3,3-difluoropentane can be converted by the sulfur tetrafluoride/hydrogen fluoride/disulfur dichloride system into fluoro sulfides and fluoro disulfides.240... 

Disulfides are also formed in reactions of alkenes or secondary alcohols with the sulfur tetrafluoride/hydrogen fluoride/disulfur dichloride system under mild conditions. At elevated... 

Upon addition of catalytic amounts of disulfur dichloride, aliphatic ketones react with sulfur tetrafluoride to yield polyfluoro sulfides and disulfides. - In the case of acetone, different products can be isolated depending on the reaction temperature. 

Applications Disulfur dichloride is utilized in the manufacture of sulfur dichloride, thionyl chloride and sulfur tetrafluoride and with polyols for the production of additives for high pressure lubricating oils and cutting oils. In addition it is used as a catalyst in the chlorination of acetic acid. Solutions of sulfur in disulfur dichloride is utilized in the room temperature vulcanization of rubbers. 

ACETATO MERCURIOSO (Spanish) (21908-53-2) A strong oxidizer. Violent reaction with reducing agents, acetyl nitrate, diboron tetrafluoride, disulfur dichloride, combustible materials, fuels, hydrazine hydrate, hydrogen peroxide, hydrogen trisulfide, hypophospho-rous acid, methanethiol, phospham. sodium-potassium alloy, sulfur, sulfur trioxide. Incompatible with alcohols, alkali metals, ammonium nitrate, diboron tetrafluoride, hydrazinium nitrate, hydrogen sulfide, nitroalkanes, rubidium acetylide, selenium oxychloride. Forms heat-, friction-, or shock-sensitive explosives with anilinium perchlorate, chlorine, phosphorus,. sulfur, magnesium, potassium, sodium-potassium alloy. May increase the explosive or thermal sensitivity of nitromethane, nitroethane, 1-nitropropane and other lower nitroalkanes, silver azide, hydrazinium perchlorate. Slowly decomposes on exposure to air. 

YELLOW OXIDE of MERCURY (21908-53-2) A strong oxidizer. Violent reaction with reducing agents, acetyl nitrate, diboron tetrafluoride, disulfur dichloride, combustible materials, fuels, hydrazine hydrate, hydrogen peroxide, hydrogen trisulfide, hypophosphorous acid, methanethiol, phospham, sodium-potassium alloy, sulfur, sulfur trioxide. Incompatible with... 

A mixture of gaseous disulfur difluoride, dinitrogen tetra-fluoride, and sulfur tetrafluoride is placed in an effusion apparatus, (a) Rank the gases in order of increasing effusion rate, (b) Find the ratio of effusion rates of disulfur difluoride and dinitrogen tetrafluoride. (c) If gas X is added, and it effuses at 0.935 times the rate of sulfur tetrafluoride, find the molar mass of X. 

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