Chlorine xenon compounds

Chlorine. Xenon trioxide reacts with RbCl and CsCl to give compounds with the composition M9(Xe03Cl2)4Cl, which consist of M+ cations, Cl" anions, and infinite chain anions in which each Xe atom is surrounded by a very distorted octahedron of three oxygen atoms (Xe—O 1.77 A) and three Cl atoms (Xe—Cl = 2.96 A). These are the only examples of compounds stable at room temperature that contain Xe—Cl bonds. 

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

Chlorine, the next most electronegative element, reacts with xenon to form transient species that decompose at room temperature. Krypton forms KtF2 and a few other compounds, but the chemishy of krypton is much more restricted than that of xenon. 

Safety precautions applicable to direct liquid phase fluorination of aromatic compounds are discussed [1]. Attention is drawn to the hazards attached to the use of many newer fluorinating agents [2], In a study of fluorination reactions of hafnium and zirconium oxides by the fluoroxidisers xenon difluoride, chlorine trifluoride and bromine trifluoride, reactivity decreased in the order given [3],... 

Chlorine gas is noncombustible but, like oxygen, it supports combustion. It combines with practically all elements except nitrogen and the inert gases, helium, neon, argon, crypton, and radon. A few compounds with the inert gas xenon are also known. The diatomic CI2 molecule can dissociate into Cl atoms upon heating or irradiation with UV. 

Frohn and coworkers have obtained the unique chloronium cation 374,1120 which is the first unambiguously characterized xenon(II) chlorine compound [Eq. (4.261)]. There is no strong contact between cation 374 and the anion in the solid state. The two C—Xe—Cl contacts are linear (bond angles = 176.0 and 178.8°) with shorter C—Xe (2.111 and 2.116 A) and longer Xe—Cl (2.784 and 2.847 A) bond lengths. The Xe—Cl—Xe bond angle is 116.96°. 

L. V. Gurvich, I. V. Veyts, and C. B. Alcock, Thermodynamic Properties of Individual Substances, Vol. 1 Elements Oxygen, Hydrogen (Deuterium, Tritium), Fluorine, Chlorine, Bromine, Iodine, Helium, Neon, Argon, Krypton, Xenon, Radon, Sulfur, Nitrogen, Phosphorus, and Their Compounds, Pt. 1 Methods and Computation, Hemisphere, New York, 1989. 

Transformations of phosphines to difluorophosphoranes proceed with xenon difluoride under mild conditions and in high yields, and the phosphorus-hydrogen bond is stable chlorine atoms are replaced by fluorine in chlorine-phosphorus molecules, while triphenyl and trimethyldifluorophosphorane are isolated in 90-100% yield130-132. Reactions of compounds containing P—N, P—O and P—S bonds with xenon difluoride proceed by fragmentation or dimerization133 (Scheme 55). 

Replacements of one or two chlorine atoms and hydrogen by fluorine were observed in various organosilicon compounds in reactions with xenon difluoride99,135, while aryl-silicon bond cleavage was observed in the presence of potassium fluoride136,137 (Scheme 57). 

A gas is defined as any material that boils within the general ranges of STP standard temperature (25°C) and Pressure (l atmosphere). Although there are many compounds that satisfy these conditions, only ll elements do, and these are argon, chlorine, fluorine, helium, hydrogen, krypton, oxygen, neon, nitrogen, radon, and xenon. 

Fluorination with elemental fluorine diluted 1 20 with nitrogen was used to prepare pentafluorophenyl tellurium trifluoride from bis[pentafluorophenyl] ditellurium at — 60° with fluorotrichloromethane as the reaction medium. The yield in this reaction was 80% 4-Methoxyphenyl tellurium trifluoride was obtained by electrochemical oxidation of the diaryl ditellurium in 0.5 M hydrofluoric acid at platinum electrodes2. Bisfpentafluoroethyl] ditellurium and chlorine fluoride (1 6) reacted at — 78° to give pentafluoroethyl tellurium trifluoride, a white solid melting at 95°3. The same compound was obtained with xenon difluoride as the fluorinating agent and melted at 143°4. 

The elements neon, argon, krypton, and xenon, the gases which are now used so much in electrical signs, all have no chemical properties. They do not form compounds with other elements. Their atomic numbers are 10, 18, 36, and 54, which are greater by unity than the numbers of flourine, chlorine, bromine, and iodine. 

Nevertheless the analogy with clathrate compounds (p. 179) does not go further since it is just the xenon hydrate (1 at. press, at — 3.40 G) which is very much more stable than the argon hydrate (1 at. at —42.8°) likewise the bromine hydrate is more stable than the chlorine hydrate. 

Xenon forms stable compounds only with the most electronegative elements fluorine (x = 4.0) and oxygen (x = 3.5), or with groups such as OSeF and OTeFj that contain these elements. Reasonably stable, though uncommon, bonds are known between xenon and both chlorine (x = 3.0) and nitrogen (x = 3.0). Bis(tri-fluoromethyOxenon, XeiCFj), = 3.3), is known but decomposes in a matter of minutes. 

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