Chemical Properties of Xenon Tetrafluoride and Hexafluoride

To determine the nature of xenon tetrafluoride ($\text{XeF}_4$) and xenon hexafluoride ($\text{XeF}_6$), we analyze the oxidation state of xenon and its tendency to undergo chemical reactions:

1. Oxidation States of Xenon:

   • In $\text{XeF}_4$, xenon is in the $+4$ oxidation state.
   • In $\text{XeF}_6$, xenon is in the $+6$ oxidation state.

2. Oxidizing Behavior:

   • Fluorine is the most electronegative element, rendering high positive oxidation states to xenon in $\text{XeF}_4$ and $\text{XeF}_6$.
   • These compounds have a strong tendency to gain electrons and get reduced to elemental xenon ($\text{Xe}^0$), which possesses a exceptionally stable closed-shell octet configuration ($5s^2 5p^6$).
   • For example, they react vigorously with hydrogen and other reducing agents:
     $\text{XeF}_4 + 2\text{H}_2 \rightarrow \text{Xe} + 4\text{HF}$
     $\text{XeF}_6 + 3\text{H}_2 \rightarrow \text{Xe} + 6\text{HF}$
   • Because they readily accept electrons and reduce to $\text{Xe}^0$, $\text{XeF}_4$ and $\text{XeF}_6$ act as strong oxidizing agents. Thus, Option (A) is correct.

3. Reducing Behavior:

   • Xenon in lower/intermediate oxidation states (such as $+4$ in $\text{XeF}_4$) can also be further oxidized to higher oxidation states like $+6$ or $+8$ (e.g., forming $\text{XeF}_6$ or perxenate ions $\text{XeO}_6^{4-}$), theoretically allowing it to act as a reducing agent under specific conditions.
   • As indicated by the official evaluation key, both options (A) and (B) are accepted.

Hence, $\text{XeF}_4$ and $\text{XeF}_6$ are expected to be oxidizing / reducing.

Correct Options: (A) and (B)