Water Xenon hexafluoride

The higher fluorides are prepared using excess fluorine (Figure A). All these compounds are stable in dry air at room temperature. However, they react with water te form compounds in which one or more of the fluorine atoms has been replaced by oxygen. Thus xenon hexafluoride reacts rapidly with water to give the trioxide... 

See Xenon hexafluoride Water (reference 2) Xenon tetrafluoride oxide Caesium nitrate... 

Although uncontrolled reaction of xenon hexafluoride and moisture produces explosive xenon trioxide, controlled action by progressive addition of limited amounts of water vapour with agitation to a frozen solution of the hexafluoride in anhydrous hydrogen fluoride at —196° C to give xenon oxide tetrafluoride or xenon dioxide difluoride is safe [1], Controlled hydrolysis in solution in hydrogen fluoride is, however, described as hazardous [2],... 

Xenon hexafluoride reacts with water to produce xenon trioxide and hydrofluoric acid. Write the chemical equation for the reaction. 

Xenon hexafluoride hydrolyzes in excess dilute acid or water to produce XeOa [Xe(VI)] in solution. Hydrolysis with strong base results in the precipitation of a perxenate salt [Xe(VIlI)]. Xenon hexafluoride is a fairly strong fluorinating agent, and it forms addition compounds w ith other fluorides such as BF3, AsFs, SbFs, and alkali metal fluorides. 

Xenon hexafluoride is a better fluorinating agent than the xenon difluoride described in the previous problem, but it must be carefully isolated from any moisture. This is because xenon hexafluoride reacts with water to form hydrogen fluoride (hydrogen monofluoride) and the dangerously explosive xenon trioxide. 

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). 

What happens if xenon hexafluoride is reacted with an excess of water Write an... 

New problems on comparing/contrasting the suffixes for the names of the noble gases, making a case for the name helon or helion for the lightest gas, the relationships of thoron, actinon, and niton to radon, the thorium series, the succession of radioactive processes that produce the radon isotope, and what happens when xenon hexafluoride reacts with an excess of water... 

All the xenon fluorides react with water to form various products. For example, in aqueous solution, xenon hexafluoride is first hydrolyzed to xenon oxide tetrafluoride, XeOp4, which is further hydrolyzed to xenon trioxide. The reactions are as follows ... 

Compounds in oxidation states +2, +4, +6, and +8 are well known. The tetrafluoride and hexafluoride are readily hydrolyzed by water forming xenon trioxide, XeOs, and the xenon tetraoxide, Xe04, both of which are dangerously explosive. While the trioxide XeOs is a colorless crystalline solid, stable in solution, the tetraoxide Xe04 is a colorless unstable gas. 

Xenon difluoride dissolves in water, yielding a solution which contains undissociated XeFa molecules which have a half-life of about 7 hours at 0°. It eventually hydrolyzes to yield the expected products, xenon, hydrogen fluoride, and oxygen. The hydrolysis reactions of the tetrafluoride and hexafluoride are somewhat more complicated. The addition of the stoichiometric amount of water to the hexafluoride results in the formation of xenon oxide tetrafluoride. Hydrolysis of either fluoride with an excess of water or acid yields in solution a stable xenon(VI) species, which has been shown to be hydrated xenon trioxide. Removal of the excess water leaves xenon trioxide as a solid residue. Inasmuch as this solid is an extremely sensitive explosive, such solutions must be handled with care. 

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.)... 

In another investigation of the comparative value of lipid and hydration hypotheses (Eger et aL 1969), the minimal anaesthetic concentrations of the following agents were plotted against the relevant physical properties carbon tetrafluoride, sulphur hexafluoride, nitrous oxide, xenon, cyclopropane, fluorexene (trifluoroethyl vinyl ether), diethyl ether, enflurane (see above), halothane, chloroform, and methoxyflurane (see above). (These anaesthetics have been arranged here in order of increasing lipid/water solubility.) The results of this study showed an excellent correlation between... 

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