CIF CHLORINE MONOFLUORIDE

CIF CHLORINE MONOFLUORIDE 22.567 4.7581E-02 -6.3572E-05 3.9963E-08 -9.4968E-12 298 1500 gas... 

Chlorine monofluoride, CIF Chlorine trifluoride, CIF3 Bromine monofluoride, BrF Bromine trifluoride, BrF3 Bromine pentafluoride, BrF5 Bromine monochloride, BrCI Iodine trifluoride, IF3 Iodine pentafluoride, IF5 Iodine heptafluoride, IF7 Iodine monobromide, IBr Iodine monochloride, ICI Iodine pentabromide, IBr5 Iodine tribromide, IBr3 Iodine trichloride, ICI3 Iodine pentachloride, ICI5... 

Chlorine monofluoride is a colorless gas that condenses to a very pale yellow liquid. It is prepared by the interaction of chlorine trifluoride and chlorine or by heating chlorine and fluorine together in a 1 1 ratio. It can be used to saturate multiply bonded systems or oxidize coordinatively unsaturated central atoms. Scheme 8 illustrates some types of CIF reactivity. 

SeFg can be prepared, stepwise directly from the elements (equation 31). A patent claims the formation of selenium haxafluoride from selenium and chlorine monofluoride, CIF, at temperatures above 200 °C under substantially anhydrous conditions. Below 200 °C, SeF4 is formed. The rotational movements of the SeFe molecules in the plastic and liquid phases have been studied by F NMR, IR, and Raman spectroscopy. 

The advantages of the TeFyClF reaction are that one-fifth as much chlorine monofluoride is necessary as when TeC is used and there is less chlorine to separate from TeClFj. The advantage of the TeCVClF reaction is that TeC is readily available commercially, whereas Tep4 is not. The purity of TeClF, in both cases depends largely upon the purity of CIF and the method of purifying the TeClFs-... 

Tellurium tetrafluoride is moisture-sensitive and should be handled in a moisture-free environment, as has been fully described. The tellurium tetrachloride [Alfa Inorganics] may be used without further purification. Chlorine monofluoride [Ozark-Mahoning] is best manipulated in a preconditioned metal vacuum line. The reaction vessel is pretreated with Fj or SF4, followed by treatment overnight with CIF. The reaction vessel is constructed by either sealing one end of a length... 

Tellurium tetrafluoride (0.72 g, 3.5 mmol) is placed in the 25-mL Teflon vessel inside the dry box. The vessel and contents are evacuated for 1 hr. Chlorine monofluoride (0.42 g, 7.9 mmol) is condensed in small aliquots (aliquots of 0.23 g of CIF have been used this mount corresponds to approximately 100 mL of CIF at a pressure of 760 torr) onto the tellurium tetrafluoride at — 196°. The reactants are warmed to room temperature and left for at least 20 min. This procedure is repeated until all of the CIF is consumed. The reactants are allowed to stand overnight at 25°. The solid TeF4 is gradually consumed, and a yellow liquid is formed. The product is separated by holding the Teflon vessel at — 78° and allowing any volatile materials to distill into another vessel held at —196° for a period of about 1 min. The more volatile fraction consists of unreacted CIF and traces of SiF4, TeClFj, and fluorocarbon impurities. Upon warming the Teflon vessel that contains the less volatile fraction to room temperature, clear liquid, TeClFj, is observed. 

Chlorine monofluoride, CIF, and iodine monofluoride, IF, are interhalogen compounds—compounds that contain bonds between different halogen elements. Which of these molecules has the larger dipole moment ... 

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. 

A compound of chlorine and fluorine, C1F , reacts at about 75°C with uranium metal to produce uranium hexafluoride, UFe, and chlorine monofluoride, ClF(g). A quantity of uranium produced 3.53 g UFs and 343 mL CIF at 75°C and 2.50 atm. What is the formula (n) of the compound Describe the bonding in the molecule, using valence bond theory. 

C,Fs-C N+ 2C1F->CjF5 CF, NC1 4.C,F,N N C,F, -1- Cl,). Pyrolysis (at 180°C) or photolysis of the CIF-adduct of theimineC,F,-N CF, ((CF,)-(C,F5)NC1, also obtainable via reaction of OF with (CF,XC,Fj)NH] yields the tetrasubstituted hydrazine (CF,XC,Fj)N N(C,FsXCF,). Reaction of chlorine monofluoride with potassium thiocyanate at — 30°C yields INW-dichlorotrifluoromethylamine, sulphur chloride pentafluoride, chlorine, potassium fluoride, and traces of sulphur hexafluoride and hexafluoroazo-methane. ... 

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