Bromine trifluoride reactivity

Safety precautions applicable to direct liquid phase fluorination of aromatic compounds are discussed [1]. Attention is drawn to the hazards attached to the use of many newer fluorinating agents [2], In a study of fluorination reactions of hafnium and zirconium oxides by the fluoroxidisers xenon difluoride, chlorine trifluoride and bromine trifluoride, reactivity decreased in the order given [3],... 

Bromine trifluoride, though it reacts explosively with water and hydrocarbon tap greases, is somewhat less violent and vigorous a fluorinat-ing agent than is CIF3. The sequence of reactivity usually quoted for the halogen fluorides is ... 

The physical properties of the interhalogens are intermediate between those of their parent halogens. Trends in the chemistry of the interhalogen fluorides can be related to the decrease in bond dissociation energy as the central halogen atom becomes heavier. The fluorides of the heavier halogens are all very reactive bromine trifluoride gas is so reactive that even asbestos burns in it. 

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. 

Bromine trifluoride is a highly reactive compound. It ignites or explodes in contact with a wide array of substances including water, finely divided metals, metal oxides and salts and organics. See Bromine Pentafluoride. 

The reactivity of bromine trifluoride is significantly enhanced by Lewis acids, such as tin(IV) chloride, antimony(V) chloride, titanium(IV) chloride, which are exchanged to the corresponding fluorides and give complexes with bromine trifluoride. Thus, the reaction of 2,2,2-tri-fluoroethyl or 2,2,3,3-tetrafluoropropyl 2,3-dibromopropanoate with bromine trifluoride in the presence of 1 mol% tin(IV) chloride affords the corresponding 2,3-difluoropropanoates in 85-87% yield.110... 

The third group of solvents consists of those that are highly polar and autoioniz-ing. They are usually highly reactive and are difficult to keep pure because they react with traces of moisture and other contaminants. Some even react slowly with silica containers or dissolve electrodes of gold and platinum. An example of one of the more reactive of these solvents is bromine trifluoride. Nonfluoride salts, such as oxides, carbonates, nitrates, iodates, and other halides, are fluorinated ... 

Alkyl bromides are effectively transformed into alkyl fluorides by both chlorine monofluoride [47] (Figure 3.4) and the less reactive bromine trifluoride [48-50]. Since tertiary... 

For production of micro-mechanic devices etching paths parallel to the wafer substrate surface are often required. Bromine trifluoride (BrF3) is used for this special kind of anisotropic etching. Because of the extreme reactivity of this compound, electrical excitation and plasma formation is not necessary. 

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). 

VANADIUM (7440-62-2) V The finely divided material reacts with air, water, acids, alcohols may release flammable hydrogen gas and chemically basic materials. A reducing agent. Violent reaction with strong oxidizers, bromine trifluoride, chlorine, lithium, nitryl fluoride nitric, hydrofluoric, or concentrated sulfuric acids. May react with halogenated hydrocarbons, forming other reactive and possibly explosive materials. It reacts with chlorine at 356°F/180°C, forming vanadium tetrachloride. Forms water-soluble vanadates in alkalis. 

AMCHLOR (12125-02-9) Can be self-reactive explosion may occur when closed containers are opened after long storage. Contact with water can cause a violent reaction with heat and formation of hydrogen chloride. Violent reaction with boron trifluoiide, boron penta-fluoride, bromine trifluoride, iodine heptafluoride, potassium chlorate. Mixture with hydrogen cyanide may form explosive nitrogen trichloride. Incompatible with alkalis, alkali carbonates, acids, salts of lead or silver. At fire temperature conditions, fumes corrode metals. 

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