`XeO_4` molecule is tetrahedral having 'n' number of `p pi - d pi` bonds. The value of 'n' is

Options

A. 1
B. 2
C. 3
D. 4

Answer

To determine the value of 'n' for the molecule \( XeO_4 \), we need to analyze the bonding in the molecule.

### Step-by-Step Solution:

1. **Identify the Central Atom and Its Hybridization**:
- The central atom in \( XeO_4 \) is xenon (Xe).
- Xenon has the electronic configuration of \( [Kr] 5s^2 5p^6 \). In \( XeO_4 \), xenon uses its \( 5s \) and \( 5p \) orbitals for bonding.

2. **Determine the Geometry of the Molecule**:
- The molecular geometry of \( XeO_4 \) is tetrahedral. This is due to the four oxygen atoms surrounding the xenon atom.

3. **Count the Number of Bonds**:
- Each oxygen atom forms a double bond with xenon. In \( XeO_4 \), there are four oxygen atoms, and each forms a double bond with xenon.

4. **Identify the Type of Bonds Formed**:
- The double bond between xenon and oxygen consists of one sigma bond and one pi bond. The pi bond in this case is formed by the overlap of the filled p-orbitals of oxygen with the empty d-orbitals of xenon.

5. **Count the pπ-dπ Bonds**:
- Since there are four oxygen atoms, and each forms a pπ-dπ bond with xenon, we can conclude that there are four such bonds in total.

6. **Final Calculation**:
- Thus, the value of 'n', which represents the number of pπ-dπ bonds in \( XeO_4 \), is 4.

### Conclusion:
The value of 'n' is 4.