Xenon tetrafluoride

Survey and account for the group characteristics and trends in the elements of Group O (He-Rn). Outline the preparation and stereochemistry of xenon tetrafluoride. 

Xenon tetrafluoride is a much weaker fluoride ion donor and only forms stable complex salts with the strongest fluoride ion acceptors, eg,... 

Stable noble-gas compounds have no industrial uses as of this writing but are frequently utilized in laboratories as fluorinating and oxidizing agents. Xenon difluoride and xenon tetrafluoride are relatively mild oxidative fluorinating agents and have been used for the preparation of phosphoms, sulfur, tellurium. 

In many expanded-octet molecules, one or more of the electron pairs around the central atom are unshared. Recall, for example, the Lewis structure of xenon tetrafluoride, XeF4 (Example 7.4). 

X. See Mole fraction X-ray diffraction, 248 Xanthoprotein, 571 Xenon tetrafluoride, 100,180... 

I Self-Test 2.10B Write the lewis structure for the l ion and give the number of 25 Xenon tetrafluoride, XeF4 I electrons in the expanded valence shell. 

Self-Test 3.4B Predict the shape of a xenon tetrafluoride molecule, XeF4. 

FIGURE 15.27 Crystals of xenon tetrafluoride, XeF4. This compound was first prepared in 1062 by the reaction of xenon and fluorine at 6 atm and 4(J(J C. 

The starting point for the synthesis of xenon compounds is the preparation of xenon difluoride, XeF2, and xenon tetrafluoride, XeF4, by heating a mixture of the elements to 400°C at 6 atm. At higher pressures, fluorination proceeds as far as xenon hexafluoride, XeFfi. All three fluorides are crystalline solids (Fig. 15.27). In the gas phase, all are molecular compounds. Solid xenon hexafluoride, however, is ionic, with a complex structure consisting of XeF< + cations bridged by F anions. 

The xenon fluorides are used to prepare the xenon oxides and oxoacids and, in a series of disproportionations, to bring the oxidation number of xenon up to +8. First, xenon tetrafluoride is hydrolyzed to xenon trioxide, Xe03 in a disproportionation reaction ... 

Xenon tetrafluoride is a powerful oxidizing agent. In an acidic solution, it is reduced to xenon. Write the corresponding half-reaction. 

Xenon tetrafluoride forms intercalates with graphite at room temperature (S19). Powder and Grafoil have both been used, and products have been isolated having stoichiometries C2sXeF4 and C4oXeF4 that apparently correspond to the second- and third-stage compounds, re-... 

Describe the geometry and draw a ball-and-stick sketch of xenon tetrafluoride. 

Chlorine pentafluoride and xenon tetrafluoride appear in Figure 9-26. Each has an inner atom with a steric number of 6, but their electron group arrangements include lone pairs. As a result, CIF5 has a square pyramidal shape, whereas XeF4 has a square planar shape. Pictures can help us determine whether or not the bond polarities cancel ... 

Describe the bonding of chlorine trifluoride and xenon tetrafluoride. 

See Xenon hexafluoride Caesium nitrate Xenon tetrafluoride... 

See Xenon tetrafluoride Caesium nitrate See other METAL NITRATES... 

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

Xenon difluoride (or the tetrafluoride, or their mixtures) could not be caused to detonate by impact. Xenon difluoride and xenon tetrafluoride both may cause explosion in contact with acetone, aluminium, pentacarbonyliron, styrene, polyethylene, lubricants, paper, sawdust, wool or other combustible materials. Their vigorous reactions with ethanol, potassium iodate or potassium permanganate are not explosive, however. 

In the preparation of xenon difluoride dioxide from caesium nitrate and xenon tetrafluoride oxide, the latter must always be used in excess to prevent formation of explosive xenon trioxide. 

The graphite-xenon tetrafluoride oxide intercalation compound exploded in contact... 

Interaction of the yellow hexafluoride with silica to give xenon tetrafluoride oxide must be interrupted before completion (disappearance of colour) to avoid the possibility of formation and detonation of xenon trioxide [1]. An attempt to collect the hexafluoride in fused silica traps at — 20°C after separation by preparative gas chromatography failed because of reaction with the silica and subsequent explosion of the oxygen compounds of xenon so produced [2],... 

In the reaction of the pentaoxide with xenon tetrafluoride oxide to give xenon difluoride dioxide and nitryl fluoride, the xenon tetrafluoride oxide must be used in excess to avoid formation of xenon trioxide, which forms a sensitive explosive mixture with xenon difluoride dioxide. 

It is a powerful explosive [1] produced when xenon tetrafluoride or xenon hexafluoride are exposed to moist air and hydrolysed. Some tetrafluoride is usually present in xenon difluoride, so the latter is potentially dangerous. Although safe to handle in small amounts in aqueous solution, great care must be taken to avoid solutions drying out, e.g. around ground stoppers [2], Full safety precautions have been discussed [2,3,4], Precautions necessary for use of aqueous solutions of the trioxide as an epoxidation reagent are detailed [5,6], A safe method of preparation,... 

Xenon tetrafluoride reacts rapidly with water by undergoing disproportionation,... 

Xenon tetrafluoride undergoes reactions that are similar to those of the interhalogens. For example, the XeF3+ cation is generated when XeF4 reacts with a very strong Lewis acid, such as BiF5. 

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