Oxygen difluoride, decomposition

Oxygen Difluoride as a Source of the OF Radical. The existence of the OF radical [12061 -70-0] was first reported in 1934 (27). This work was later refuted (28). The OF radical was produced by photolysis of OF2 in a nitrogen or argon matrix at 4 K. The existence of the OF species was deduced from a study of the kinetics of decomposition of OF2 and the kinetics of the photochemical reaction (25,26) ... 

DOT CLASSIFICATION 8 Label Corrosive SAFETY PROFILE Poison by inhalation. A corrosive irritant to the eyes, skin, and mucous membranes. With the appropriate conditions it undergoes hazardous reactions with formic acid, hydrogen fluoride, inorganic bases, iodides, metals, methyl hydroperoxide, oxidants (e.g., bromine, pentafluoride, chlorine trifluoride, perchloric acid, oxygen difluoride, hydrogen peroxide), 3-propynol, water. When heated to decomposition it emits toxic fumes of POx. 

Oxygen difluoride, OF2 (15.21), is highly toxic and may be prepared by reaction 15.47. Selected properties are given in Table 15.5. Although OF2 is formally the anhydride of hypofluorous acid, HOF, only reaction 15.48 occurs with water and this is very slow at 298 K. With concentrated alkali, decomposition is much faster, and with steam, it is explosive. 

ZINC FLUORIDE or ZINC FLUORURE (French) (7783-49-5 73640-07-0) ZnFj Noncombustible solid. Reacts with water, forming an acid solution. Violent reaction with boron, bromine pentafluoride, calcium disilicide, calcium hydride, oxygen difluoride, potassium. Aqueous solution incompatible with sulfuric acid, alkalis, ammonia, aliphatic amines, alkanolamines, alkylene oxides, amides, epichlorohydrin, isocyanates, nitromethane, organic anhydrides, vinyl acetate. Corrodes metals in the presence of moisture. Thermal decomposition releases toxic hydrogen fluoride. 

FERRIC CHLORIDE HEXAHYDRATE (10025-77-1) Aqueous solution is highly acidic, precipitating hydroxide and phosphate salts, and forming corrosive fumes. Violent reaction with strong bases, allyl chloride, bromine pentafluoride, ethylene oxide, oxygen difluoride. Contact with acids, acid fumes causes decomposition with formation of chloride fumes. Shock- and friction-sensitive explosive is formed with potassium, sodium, potassium-sodium alloy, and possibly other active metals. Aqueous solution is incompatible with sulfuric acid, caustics, ammonia, aliphatic amines, alkanolamines, amides, organic anhydrides, isocyanates, vinyl acetate, alkylene oxides, epichlorohydrin Attacks metals in the presence of moisture. 

The gas-phase thermal decomposition of oxygen difluoride (F2O) in the temperature range 230 °C to 310 °C has the following time-independent stoichiometry... 

Nitriles are resistant to reaction with sulfur tetrafluoride under the conditions generally used for fluorination of oxygen functions. Acetonitrile, which is used as the solvent in the laboratory synthesis of sulfur tetrafluoride (see Section 8.1.2.), is particularly resistant and no reaction occurs up to 260"C, at which temperature extensive decomposition takes place and 1,1,2-tri-fluoroethyliminosulfur difluoride is formed in low yield,202... 

Iodine pentafluoride depletes the limonene inhibitor and then causes explosive polymerization of the monomer. Mixtures with hexafluoropropene and air form an explosive peroxide. Reacts violendy with SO3 air difluoromethylene dihypofluorite dioxygen difluoride iodine pentafluoride oxygen. When heated to decomposition it emits highly toxic fumes of F". See also FLUORIDES. 

ETHYLIDENE DIFLUORIDE (75-37-6) Flammable gas (flammability limits 3.7-18% by volume in air). Violent reaction with strong oxidizers, barium, sodium, and potassium. Incompatible with powdered aluminum, liquid oxygen, potassium, sodium. May form explosive compounds with divalent light metals and metallic azides. Attacks some metals in the presence of moisture. Undergoes thermal decomposition when exposed to flame or red-hot surfaces. Flow or agitation of substance may generate electrostatic charges due to low conductivity. 

SILVER DIFLUORIDE (7783-95-1) Contact with acetylene produces shock-sensitive material. Ammonia contact produces compounds that are explosive when dry. Hydrogen peroxide causes violent decomposition to oxygen gas. Soluble silver compounds attack some forms of plastics, rubber, and coatings. 

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). 

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