Trichlorofluoromethane, decomposition

Carbon tetrachloride (5) and trichlorofluoromethane (6) react with xenon difluoride more slowly, but small amounts of hydrogen fluoride lead to fast decomposition of the reagent within one hour at room temperature. 

The formation of a solid, isolated by bubbling fluorine diluted with nitrogen into a solution of pyridine in trichlorofluoromethane at — 80 °C followed by filtering at low temperature, has been noted.30 The solid is considered to be a pyridine/fluorine compound with polar character however, spectral or other data on the structure of the pyridine/fluorine compound are presently not available, probably due to its explosive nature. This compound has been used for the fluorination of uracil and some chloroalkenes,30,31 but the adduct is of little use because of its violent decomposition above — 2CC. 

TRICHLOROFLUOROMETHANE (75-69-4) Reaets violently with barium, alkali amides, alkali metals, metal powders, sodium, and potassium, molten aluminum or magnesium. Undergoes thermal decomposition when exposed to red-hot surfaces or fire, forming chlorine, hydrogen fluoride or chloride, phosgene, and carbonyl fluoride. Contact with water causes slow decomposition. Attacks some plastics, rubber, and coatings. Attacks aluminum, copper, magnesium, tin, zinc. 

Reaction Q). Formation of water was apparent when filtered homogeneous trichlorofluoromethane solutions were warmed. Solids initially precipitated from these solutions appeared to be either hydrogen peroxide or a mixture of all other products aggregated with hydrogen peroxide. The acetone precursor was in fact shown to be more polar than acetone, as measured by distribution coeflScient between trichlorofluoromethane and 80% methanol. Its decomposition rate, 2.3 X 10 sec." at 0°C., is comparable with that of di-ferf-butyltrioxide (I) slow decomposition even at —78°C. is catalyzed by triethylamine. There is every reason for accepting the obvious formula (IV) ... 

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