Question

Dissolution of $Xe{{F}_{6}}$ in anhydrous $HF$ to give a good conducting solution which contains:
A. ${{H}^{+}}$ and $Xe{{F}_{7}}^{-}$ ions
B. $H{{F}_{2}}^{-}$ and $Xe{{F}_{5}}^{+}$ ions
C. $HXe{{F}_{6}}^{+}$ and ${{F}^{-}}$ ions
D. none of these

Answer 1

Hint $Xe{{F}_{6}}$ is a noble gas compound known by the name xenon hexafluoride. These compounds generally exist in three forms other than xenon hexafluoride it exists as $Xe{{F}_{2}}$and $Xe{{F}_{4}}$. It is very stable at normal room temperature.

Complete Step by step solution:
$Xe{{F}_{6}}$ is strongest fluorinating agent and exist as a colourless solid which readily sublimes into intense yellow vapours and according to VSEPR theory the structure of $Xe{{F}_{6}}$ is of octahedral geometry due to 6 chlorine atoms and one lone pair. This molecule is termed as fluxional molecule where the fluxional term refers for that molecule which undergoes dynamics where some atoms or all atoms interchange their symmetry equivalent positions.
$HF$ is known by the name hydrofluoric acid which is generally a solution of hydrogen fluoride in water. It is colourless, acidic and highly corrosive in nature. When this acid comes in contact with the skin then it causes deep burns. This is basically used to organofluorine compounds.
$Xe{{F}_{6}}$ dissolves in anhydrous $HF$to give a good conducting solution which is generally yellow in colour and shows conductivity due to the formation of $H{{F}_{2}}^{-}$ and $Xe{{F}_{5}}^{+}$ ions. Conducting solution is that solution which allows the electricity to pass through it.

Hence we can conclude that option B is the correct answer.

Note: Xenon hexafluoride is prepared by heating $Xe{{F}_{2}}$ at $300{}^\circ$C under 60-atmosphere pressure of fluorine with the help of catalyst while hydrogen fluoride also known as hydrofluoric acid is prepared by treatment of the mineral fluorite with concentrated sulfuric acid at $265{}^\circ$C.