Xenon tetrachloride

Xenon dichloride [13780-38-6], XeCl, and xenon(II) chloroduoride [73378-52-6], XeClE, have been prepared by photochemical and electric discharge methods and have been examined at low temperatures by matrix-isolation techniques (39,40). The dichloride has a linear stmcture like that of XeE2. Evidence for the existence of XeCl2, XeBr2, and xenon tetrachloride [14989-42-5], XeCl, has been obtained from Mn ssbauer studies (41,42). Owing to thermal chemical instabiUties, no dihaUde other than the binary duorides has been prepared in macroscopic amounts. 

Xenon tetrachloride and xenon dibromide have been detected by (see Mossbauer Spectroscopy) as products of the -decay of their relatives (equation 13). 

The fluorides are essentially the only stable halides of xenon. XeCl2 has been obtained by condensing the products after a microwave discharge has been passed through a mixture of chlorine and an excess of xenon. Xenon tetrachloride and xenon dibromide have also been detected. 

C03-0008. Write chemical formulas for the following compounds chlorine monofluoride, xenon trioxide, hydrogen bromide, silicon tetrachloride, sulfur dioxide, and hydrogen peroxide. 

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. 

Xenon Orthotellurate. (Xenon bis (pentafluor-oorthotellurate)). Xe (OTeFj) 2 mw 369.89 colorl cryst mp 35 —7°. Sol in acetonitrile and C tetrachloride. Prepn in 97% yield is by treating Xe difluoride with 2 moles of /anhydr HOTeFs. The compd reacts explosively with acet, benz and ethanol... 

Using Lewis structures and VSEPR theory, predict the shape of each of the following species (a) sulfur tetrachloride (b) iodine trichloride (c) IF4 (d) xenon trioxide. Give the VSEPR AX Em designation for each. 

Xenon difluoride reacts also with some halosubstituted alkanes18,19 at room temperature in chloroform, carbon tetrachloride, dichloromethane or bromoform, and depending on the nature of the solvent used chloro or bromo derivatives are isolated with imidazo-(l,2-fr)-pyridazine18. Carbon tetrachloride reacts with xenon difluoride at 180°C, while room-temperature transformations are achieved when various catalysts [antimony trifluoride, tantalum(V) fluoride or silica dioxide] are used, whose structure also influences the product distribution20. Tris(fluorosulfonyl)methane gives a fluoro-substi-tuted product in its reaction with xenon difluoride in difluorodichloromethane21. 

To extract TMB from TMB-methanol mixtures it is necessary to find a solvent that is relatively immiscible in methanol yet is miscible with TMB at the same conditions. TMB is very soluble in benzene, hexane, heptane, nonane, and carbon tetrachloride indicating that it exhibits very lipophilic characteristics (Plank and Christopher, 1976 Niswonger, Plank, and Laukhuaf, 1985 Schmidt, Plank, and Laukhuf, 1985 Munster et al., 1984). Hence, TMB should be soluble in the more common supercritical fluid solvents such as ethane and carbon dioxide. Methanol is moderately miscible with xenon, ethane, ethylene, and carbon dioxide since a single phase is obtained at pressures of less than —200 bar at temperatures between the respective critical temperatures of the binary components (Brunner, 1985). To obtain quickly an estimate of the distribution coefficient for TMB in carbon dioxide, ethane, and ethylene, rapid screening experiments were performed with a dynamic flow apparatus at temperatures ranging from 0 to 55°C at a number of pressures. From this preliminary study it was found that carbon dioxide does not... 

FOLLOW-UP PROBLEM 11.1 Use partial orbital diagrams to show how the atomic orbitals of the central atoms mix to form hybrid orbitals in (a) beiyllium fluoride, BeF2 (b) silicon tetrachloride, SiCU (c) xenon tetrafluoride, XeF4. 

Fig. 3. Variation with temperature of the diffusion coefficients for various simulated fluids and actual laboratory fluids. Sources of data are, from left to right LJ argon, simulated Refs. 7 (DC) and 12 (C) laboratory. Ref. 41 bard spheres (for which temperature axis corresponds to pV/NkT X.50), Ref. 82 soft spheres. Ref. 20 xenon. Ref. 41 toluene. Ref. 42 methyl cyclohexane. Ref. 43 carbon tetrachloride. Ref. 44 o-terphenyl. Ref. 45 molten KQ, simulated using Tosi-Fumi (TF) potential parameters. Ref. S repellent Gaussian core particles. Ref. 21 (F. H. Stillinger kindly deduced the values his simulation results would infer for argonlike particles in familiar units) Na ions diffusing in molten 6KN03-4Ca(N0j)2 solvent medium. Ref. 46. The dashed extension of lower temperature in the case of xenon is based on the Arrhenius parameters quoted for the data. ...

Xenon tetrafluoride and hexafluoride are very powerful oxidizing agents also. They are particularly dangerous because they react with water, giving explosive xenon trioxide. [See Cautions under the syntheses of XeF and XeO solution. The best way to dispose of xenon tetrafluoride or hexafluoride is to rinse the vessel [e.g., a protective trap) first with carbon tetrachloride and then with plenty of water, otherwise explosions may occur.)... 

Like xenon hexafluoride or xenon tetrafluoride, krypton difluoride reacts with water, giving highly explosive hydrolysis products. The best way for disposing of krypton difluoride is to allow it to react with carbon tetrachloride (see caution note under xenon tetrafluoride procedure). 

Phosphorus pentafluoride Polarine oil Selenium mustard Silicon tetrafluoride Strontium chlorate Strontium permanganate Sulfur chloropentafluoride Sulfur dichloride Sulfur hexafluoride Sulfur monochloride Titanium tetrachloride Thiocarhonyl dichloride Thionyl fluoride Thioptiosgene Triethyl aluminum Trifluoromethyl iodide Triisohutylaluminum Trimethylaluminum Vanadium tetrachloride Vincennite Vinyl bromide Vinylmagnesium bromide Xenon difluoride Zinc arsenide... 

Write a formula for each molecular compoimd. (a) carbon monoxide (b) disulfur tetrafluoride (c) dichlorine monoxide (d) phosphorus pentafluoride (e) boron tribromide (f) diphosphorus pentasulfide 74. Write a formula for each molecular compound. (a) chlorine monoxide (b) xenon tetroxide (c) xenon hexafluoride (d) carbon tetrabromide (e) diboron tetrachloride (f) tetraphosphorus triselenide... 

Other xenon halides include the dichloride, the tetrachloride, and the dibromide, but these are not particularly stable. Solutions of xenon trioxide, called xenic acid, are excellent oxidizing agents, as is the octahedral perxenate anion, XeOg. Krypton difluoride, a few nitrogen compounds of both xenon and krypton, and radon difluoride have also been prepared but are not well-characterized. 

For the fission process, natural uranium foils and solid U02(N03)2.6H20 were used as targets. The isomer was separated with carrier from irradiated uranium foils in the following manner. The uranium was dissolved in concentrated hydrochloric acid which contained a little concentrated nitric acid. Iodide carrier was added and oxidized to periodate by means of sodium hypochlorite after the solution had been made basic with sodium carbonate. Then the usual redox steps were carried out reduction of 10 to I2 with NH2OH.HCI extraction of I2 into carbon tetrachloride back-extraction Into aqueous sodium bisulfite repetition of l2"I cycles until the y spectrum showed the presence only of iodine products or their xenon decay products. 

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