Noble gases have compleately filled valance shall i.e. `m^(2)sp^(2)` exceps He (i.e) .Noble gases are monoomic under normal conductions .Law bolding point of the ligher noble gases are due to weak van dor wads forces between the atoms and abance of any interature imaractions `Xe` reacts with `F_(2)` so give a sourceof fouoxide mently `XeF_(2),XeF_(4),XeF_(4),XeF_(3)` on complete hydrolyes gives `XeFe_(3)`,
`XeF_(4)` and `XeF_(4)` are expected to be

Options

A. Reducting
B. Oxidising
C. Inert
D. Basic

Explanation

To solve the question regarding the nature of the compounds XeF4 and XeF6, we will follow a step-by-step approach:

### Step 1: Understand the Oxidation States
- Xenon (Xe) is a noble gas and typically has a stable oxidation state of 0. However, when it forms compounds with highly electronegative elements like fluorine, it can exhibit positive oxidation states.
- In XeF4, xenon has an oxidation state of +4.
- In XeF6, xenon has an oxidation state of +6.

### Step 2: Analyze the Stability of Oxidation States
- Noble gases are generally stable due to their completely filled valence shells.
- When xenon is in a higher oxidation state (like +4 or +6), it is less stable compared to its zero oxidation state.
- Therefore, xenon will tend to reduce its oxidation state to achieve a more stable configuration.

### Step 3: Determine the Nature of the Compounds
- Compounds with xenon in higher oxidation states (like XeF4 and XeF6) can act as oxidizing agents. This is because they can accept electrons and reduce their oxidation state.
- Since xenon in these compounds is trying to reduce its oxidation state, it exhibits oxidizing behavior.

### Step 4: Conclusion
- Based on the analysis, we conclude that XeF4 and XeF6 are expected to exhibit oxidizing nature.

### Final Answer
- The nature of XeF4 and XeF6 is oxidizing.

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