Chlorine® fluoride

A time-of-flight mass spectrometer coupled to a shock tube was used to record the change in mass spectral peak heights as a function of reaction time [123]. Mass spectra of the gas flowing from the reflected shock zone into the ion source were taken at 25 psec intervals. 

The parent peak height of CIF declined according to a (pseudo) first-order decay. However, the appearance and influence of CI2 upon the rate led to the proposition that the mechanism for the decomposition was complex and that the first-order rate coefficients were apparent. The absence of Fj in the mass spectra eliminated the importance of the F atom abstraction reaction and subsequent decomposition of F2. The results were accounted for by the steps 

The versatility of the mass spectrometric method is demonstrated in this study with the identification and time history of Clj, an important experimental fact that could only have been inferred from a computer analysis of a spectroscopic record of absorption or emission at a particular wavelength. 

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R. L. Earrar, Jr., and E. J. Barber, Some Considerations in the Handling of Fluorine and the Chlorine Fluorides, report K/ET-252, Oak Ridge Gaseous Diffusion Plant, Oak Ridge, Term., 1979. 

R. A. Rheia and M. H. Miles, Bromine and Chlorine Fluorides A Review, Naval Weapons Center technical pubHcation 6811, NWC, China Lake, Calif., 1988. 

Bismuth pentafluoride is an active fluorinating agent. It reacts explosively with water to form ozone, oxygen difluoride, and a voluminous chocolate-brown precipitate, possibly a hydrated bismuth(V) oxyfluoride. A similar brown precipitate is observed when the white soHd compound bismuth oxytrifluoride [66172-91 -6] BiOF, is hydrolyzed. Upon standing, the chocolate-brown precipitate slowly undergoes reduction to yield a white bismuth(Ill) compound. At room temperature BiF reacts vigorously with iodine or sulfur above 50°C it converts paraffin oil to fluorocarbons at 150°C it fluorinates uranium tetrafluoride to uranium pentafluoride and at 180°C it converts Br2 to bromine trifluoride, BrF, and bromine pentafluoride, BrF, and chlorine to chlorine fluoride, GIF. It apparently does not react with dry oxygen. 

Hypochlorites- are obtained by reaction of fluorinated carbonyl compounds, such as carbonyl lluonde, with an alkali metal fluoride and chlorine fluoride f62, 720]... 

With nitriles, products from addition of one or two equivalents of halogen fluoride can be obtained [725, 726, 127, 128] (equations 25 and 26) on reaction with chlorine fluoride or bromine and an alkali metal fluoride. 

Chlorine fluoride will also oxidize perfluoroalkylsultenyl chlorides and disulfides to perfluoroalkylsullur chloride tetrafluorides [729]... 

Chlorination and bromination of perfluoroketimines take place only in the presence of alkali fluorides as catalyst [267] Chlorine fluoride adds readily across the CO or CN bond of polyfluonnated ketones and immes [268, 269]... 

Elimination reactions of fluorine compounds are not limited to the removal of simple molecules Frequently, large molecules or combination of smaller ones are formed as by-products, especially in pyrolytic reactions For example perhalo genated acid chlorides lose not only carbon monoxide but also chlorine fluoride [106, 107] (equations 74 and 75)... 

An alkyl group can also migrate from oxygen to nitrogen or phosphorus [I, 72] (Michaelis-Arbuzov rearrangement) With this methodology, tetrafluoro-pyndine phosphonates and phosphmates can be obtained [75, 74], Chlorine fluoride... 

A compound of chlorine and fluorine, CIF, reacts at about 75°C with uranium to produce uranium hexafluoride and chlorine fluoride, C1F. A certain amount of uranium produced 5.63 g of uranium hexafluoride and 457 mL of chlorine fluoride at 75°C and 3.00 atm. What is x Describe foe geometry, polarity, and bond angles of foe compound and foe hybridization of chlorine. How many sigma and pi bonds are there ... 

IBr and IC1 are also small, but that for C1F is even larger than for HC1, showing that the bond in chlorine fluoride is more ionic in character than that in hydrogen chloride. 

Of the chlorine fluorides, only the monofluoride does not intercalate in the neat state. It does, however, intercalate in the presence of HF (S15), BF3, or PFj (S16). Chlorine trifluoride intercalates into graphite with simultaneous fluorination of the graphite lattice (Si5), releasing... 

Chlorine fluoride Aluminium Iodine chloride Metals Iodine heptafluoride Metals Iodine pentafluoride Metals... 

In the preparation of trifluoromethylsulfur trifluoride, the chloride must be dissolved in a fully halogenated solvent to prevent explosion during treatment with chlorine fluoride or chlorine trifluoride. 

See Trifluoromethanesulfenyl chloride Chlorine fluorides See other ALKYLNON-METAL HALIDES... 

During preparation of the title compound from the imide and chlorine fluoride, initially at -111°C with slow warming dining 12 h to 0°C, the scale should be limited to 40 mmol or below. Forceful explosions occurred on several occasions when this scale was exceeded, but care is necessary on any scale of working. 

See Bis(trifluoromethyl) sulfide Chlorine fluorides Bis(trifluoromethyl) disulfide Chlorine fluorides... 

The compound, prepared by by co-condensation of diethyl sulfite (3.5 mmol) and chlorine fluoride (10 mmol) at —196°C, followed by slow warming to —78, then —20°, is unstable. Trap-to-trap distillation must be effected with great care, as violent explosions occurred (even on this small scale) when cryogenic cooling was removed from the traps. Scaling up is not recommended. 

Aluminium bums more readily in chlorine fluoride than in fluorine. 

Chlorine fluoride can probably ignite Teflon and Kel-F at high temperatures, or... 

Farrar, R. L. et al., Some Considerations in Handling Fluorine and Chlorine Fluorides, Oak Ridge Rept. K/ET-252, 1979, 41pp... 

Waterfeld, A. et al., J. Chem. Soc., Chem. Comm., 1982, 839 Reaction of chlorine fluoride with trifluorosulfur nitride is rather hazardous and may lead to violent explosions. A safer alternative preparation is to use chlorine and mercuric fluoride in place of chlorine fluoride. 

Acetonitrile, Chlorine fluoride Sekiya, A. et al., lnorg. Chem., 1981, 20, 1-2... 

When fluorine was condensed onto acetonitrile and chlorine fluoride frozen at — 196°C, a small explosion occurred in the reactor. 

Chlorine Non-metals Chlorine fluoride Tellurium Chlorine trifluoride Metals Fluorine Non-metals... 

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