Name: Allotropes of Sulphur
Uploaded: 2019-07-19
Duration: 6 min 39 s
Description: Sulphur is one of the most useful non-metals which has wide applications in our industries. Watch this video to learn about the important allotropes of sulphur.

Question

Complete the following:

${XeF}_{4} + O_{2} F_{2} \to$

${XeF}_{2} + H_{2} O \to$

Accepted Answer

The complete balanced reaction is:

${XeF}_{4} + O_{2} F_{2} \to {XeF}_{6} + O_{2}$

Xenon-fluorine compounds: Xenon forms three binary fluorides, ${XeF}_{2}$ , ${XeF}_{4}$ and ${XeF}_{6}$ by the direct reaction of elements under appropriate experimental conditions.

$Xe (g) + F_{2} (g) \overset{673 K, 1 bar}{\to} {XeF}_{2} (s) (xenon in excess)$

$Xe (g) + 2 F_{2} (g) \overset{873 K, 7 bar}{\to} {XeF}_{4} (s) (1 : 5 ratio)$

$Xe (g) + 3 F_{2} (g) \overset{573 K, 60 - 70 bar}{\to} {XeF}_{6} (s) (1 : 20 ratio)$

${XeF}_{6}$ can also be prepared by the interaction of ${XeF}_{4}$ and $O_{2} F_{2}$ at 143K.

${XeF}_{4} + O_{2} F_{2} \to {XeF}_{6} + O_{2}$

The complete balanced reaction is:

$2 {XeF}_{2} + 2 H_{2} O \to 2 Xe + 4 HF + O_{2} $

Xenon-fluorine compounds: Xenon forms three binary fluorides, ${XeF}_{2}$ , ${XeF}_{4}$ and ${XeF}_{6}$ which are colourless crystalline solids and sublime readily at $298$ K. They are powerful fluorinating agents. They are readily hydrolysed even by traces of water. For example, ${XeF}_{2}$ is hydrolysed to give xenon, hydrogen fluoride and oxygen.
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$2 {XeF}_{2} (s) + 2 H_{2} O (l) \to 2 Xe (g) + 4 HF (aq) + O_{2} (g)$

Note: In general, noble gases are the least reactive. Their inertness to chemical reactivity is attributed to the following reasons:

The noble gases except helium ( $1 s^{2}$ ) have completely filled ${ns}^{2} {np}^{6}$ electronic configuration in their valence shell.

They have high ionisation enthalpy and more positive electron gain enthalpy.

The reactivity of noble gases has been investigated occasionally, ever since their discovery, but all attempts to force them to react to form the compounds were unsuccessful for quite a few years. In March $1962$ , Neil Bartlett, then at the University of British Columbia, observed the reaction of xenon noble gas. After this discovery, a number of xenon compounds mainly with the most electronegative elements like fluorine and oxygen, have been synthesised.

The compounds of krypton are fewer. Only the difluoride ( ${KrF}_{2}$ ) has been studied in detail. Compounds of radon have not been isolated but only identified (e.g., ${RnF}_{2}$ ) by radiotracer technique. No true compounds of $Ar$ , $Ne$ or $He$ are yet known.

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