In the `sp^(3)d` hybridisation of the central atom having two lone pairs, the lone pairs are placed along the equator and not along the axis while in the `sp^(3)d` hybridisation of the central atom with three lone pairs, the lone pairs are again placed along the equator and not along the two axis because :

Options

A. In order to minimize lone pair-lone pair repulsion in both the cases
B. In order to minimize lone pair-bond pair repulsion in both the cases
C. In order to minimize bond pair-bond pair repulsion in the former and lone pair-lone pair repulsion in the latter
D. In order to minimize bond pair-bond pair repulsion in the former and lone-pair-lone pair repulsion in the latter

Explanation

To answer the question regarding the placement of lone pairs in `sp^3d` hybridization, we need to analyze the geometry and repulsion effects associated with lone pairs and bond pairs.

### Step-by-Step Solution:

1. **Understanding `sp^3d` Hybridization**:
- The `sp^3d` hybridization corresponds to a trigonal bipyramidal geometry. In this geometry, there are five positions: three equatorial and two axial.

2. **Lone Pairs in `sp^3d` Hybridization**:
- When a central atom has lone pairs, these lone pairs will occupy positions that minimize repulsion with bond pairs.

3. **Case 1: Two Lone Pairs**:
- If the central atom has two lone pairs, the preferred arrangement is to place both lone pairs in the equatorial positions. This is because:
- The equatorial positions are 120 degrees apart, which reduces the repulsion between the lone pairs.
- If the lone pairs were placed in the axial positions, they would be 90 degrees apart from the equatorial bond pairs, leading to greater repulsion.

4. **Case 2: Three Lone Pairs**:
- Similarly, if the central atom has three lone pairs, these lone pairs will also occupy the equatorial positions. This is due to:
- The arrangement allows the lone pairs to be 120 degrees apart, minimizing the repulsion among them.
- Placing them in axial positions would increase the repulsion with the bond pairs due to the 90-degree angles.

5. **Conclusion**:
- In both cases, the placement of lone pairs in the equatorial positions minimizes the repulsion between lone pairs and bond pairs, leading to a more stable molecular geometry.

### Final Answer:
In `sp^3d` hybridization, lone pairs are placed along the equator (equatorial positions) rather than along the axis (axial positions) to minimize the repulsion between lone pairs and bond pairs, which stabilizes the molecular structure.