Which of the following is correct for `XeO_(2)F_(2)` and `PCl_(5)` ?

Options

A. Both have same hybridisation and shape
B. Both have same hybridisation but different geometry
C. Both have different hybridisation but same shape
D. both have same hybridisation but different shape

Answer

To solve the question regarding the correct statements for `XeO_(2)F_(2)` and `PCl_(5)`, we will analyze their hybridization, geometry, and shape step by step.

### Step 1: Determine the Hybridization of `XeO_(2)F_(2)`

1. **Identify the central atom**: The central atom in `XeO_(2)F_(2)` is xenon (Xe).
2. **Count the valence electrons**: Xenon has 8 valence electrons.
3. **Count the number of monovalent atoms**: There are 2 fluorine (F) atoms and 2 oxygen (O) atoms contributing to the bonding.
4. **Calculate the total number of electron pairs**:
- Total = Valence electrons + Monovalent atoms = 8 + 2 = 10 electrons.
- Number of electron pairs = Total electrons / 2 = 10 / 2 = 5 pairs.
5. **Determine hybridization**: Since there are 5 pairs, the hybridization is **sp³d**.

### Step 2: Determine the Geometry and Shape of `XeO_(2)F_(2)`

1. **Count bond pairs and lone pairs**:
- Bond pairs: There are 4 bond pairs (2 from O and 2 from F).
- Lone pairs: There is 1 lone pair on xenon.
2. **Determine molecular geometry**: With 5 regions of electron density (4 bond pairs + 1 lone pair), the geometry is **trigonal bipyramidal**.
3. **Determine the shape**: The presence of the lone pair distorts the shape to **seesaw**.

### Step 3: Determine the Hybridization of `PCl_(5)`

1. **Identify the central atom**: The central atom in `PCl_(5)` is phosphorus (P).
2. **Count the valence electrons**: Phosphorus has 5 valence electrons.
3. **Count the number of monovalent atoms**: There are 5 chlorine (Cl) atoms.
4. **Calculate the total number of electron pairs**:
- Total = Valence electrons + Monovalent atoms = 5 + 5 = 10 electrons.
- Number of electron pairs = Total electrons / 2 = 10 / 2 = 5 pairs.
5. **Determine hybridization**: Since there are 5 pairs, the hybridization is also **sp³d**.

### Step 4: Determine the Geometry and Shape of `PCl_(5)`

1. **Count bond pairs and lone pairs**:
- Bond pairs: There are 5 bond pairs (one for each Cl).
- Lone pairs: There are 0 lone pairs.
2. **Determine molecular geometry**: With 5 regions of electron density (5 bond pairs), the geometry is **trigonal bipyramidal**.
3. **Determine the shape**: The shape is also **trigonal bipyramidal**.

### Step 5: Compare `XeO_(2)F_(2)` and `PCl_(5)`

1. **Hybridization**: Both `XeO_(2)F_(2)` and `PCl_(5)` have the same hybridization of **sp³d**.
2. **Geometry**: Both have the same geometry of **trigonal bipyramidal**.
3. **Shape**: The shape of `XeO_(2)F_(2)` is **seesaw**, while the shape of `PCl_(5)` is **trigonal bipyramidal**.

### Conclusion

Based on the analysis:
- Both have the same hybridization (sp³d).
- Both have the same geometry (trigonal bipyramidal).
- They have different shapes (seesaw for `XeO_(2)F_(2)` and trigonal bipyramidal for `PCl_(5)`).

Thus, the correct statement is: **Same hybridization but different shape**.