`XeO_(4)` molecule is tetrahedral having 'x' number of `p pi - d pi` bonds. The value of 'x' is .

Answer

To determine the number of pπ-dπ bonds in the XeO₄ molecule, we can follow these steps:

### Step 1: Identify the central atom and its valence electrons
- The central atom in the molecule XeO₄ is xenon (Xe).
- Xenon is a noble gas and has 8 valence electrons.

### Step 2: Count the number of oxygen atoms and their contributions
- There are 4 oxygen atoms in XeO₄.
- Each oxygen atom can form a double bond with xenon, which involves the sharing of electrons.

### Step 3: Determine the type of bonds formed
- In XeO₄, the bonds formed between xenon and oxygen are not just simple σ bonds; they also involve π bonding.
- The pπ-dπ bond occurs when electrons from the filled p-orbitals of oxygen are donated to the empty d-orbitals of xenon.

### Step 4: Analyze the hybridization of the molecule
- The hybridization of xenon in XeO₄ is sp³, which corresponds to a tetrahedral geometry.
- This means that there are 4 bond pairs formed between xenon and the 4 oxygen atoms.

### Step 5: Calculate the number of pπ-dπ bonds
- Since each oxygen atom forms a double bond with xenon, we can conclude that each of these bonds involves a pπ-dπ interaction.
- Therefore, with 4 oxygen atoms, there are 4 pπ-dπ bonds formed.

### Conclusion
- The value of 'x', which represents the number of pπ-dπ bonds in XeO₄, is 4.

### Final Answer
The value of 'x' is 4.

---