Oxidizing agents chlorine monofluoride

Chlorine monofluoride (which is commercially available) acts as a powerful fluorinating and oxidizing agent (e.g. reaction 16.19) oxidative addition to SF4 was shown in Figure... [Pg.480]

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). [Pg.1008]

TIN(II) CHLORIDE (7772-99-8) SnClj A powerful reducing agent. Reacts violently with strong oxidizers, strong alkalis, bromine, bromine trifluoride (ignition), calcium carbide, chlorine, chlorine monofluoride, copper nitrate, ethylene oxide fluorine, hydrogen peroxide, nitrates, potassium, potassium dioxide, sodium, with risk of fire and explosions. Incompatible with calcium acetylide, hydrazine hydrate (forms explosive stannous dihydrazine chloride) metal nitrates. On small fires, use dry chemical powder (such as Purple-K-Powder), alcohol-resistant foam, or COj extinguishers. [Pg.1008]

Chlorine monofluoride (which is commercially available) acts as a powerful fluorinating and oxidizing agent (e.g. reaction 17.22) oxidative addition to SF4 was shown in Figure 16.13. It may behave as a fluoride donor (equation 17.23) or as a fluoride acceptor (equation 17.24). The structures of [C12F] (17.9) and [C1F2] (17.10) can be rationalized using the VSEPR model. Iodine monochloride and monobromide are less reactive than CIF, but of importance is the fact that, in polar solvents, ICl is a source of I" " and iodinates aromatic compounds. [Pg.546]