In `CsCl` structure, each 'Cs^+' ion is surrounded by

Options

A. `4Cl^(-)` ions
B. `6Cl^(-)` ions
C. `8Cl^(-)` ions
D. `12Cl^(-)` ions

Answer

To determine how many chloride ions (Cl^-) surround each cesium ion (Cs^+) in the cesium chloride (CsCl) structure, we can follow these steps:

### Step-by-Step Solution:

1. **Understand the Structure of CsCl**:
- Cesium chloride crystallizes in a cubic structure. It is often described as having a body-centered cubic (BCC) arrangement.

2. **Identify the Positions of Ions**:
- In the CsCl structure, the Cs^+ ions are located at the center of the cube (the body center), while the Cl^- ions occupy the corners of the cube.

3. **Count the Chloride Ions Surrounding Cesium**:
- Each corner of the cube is occupied by a Cl^- ion. In a cubic unit cell, there are 8 corners.
- Each Cl^- ion at the corner is shared among 8 adjacent unit cells, meaning that each contributes 1/8 of an ion to the unit cell.

4. **Calculate the Total Contribution of Cl^- Ions**:
- Since there are 8 corners, the total contribution of Cl^- ions in one unit cell is:
\[ 8 \text{ corners} \times \frac{1}{8} = 1 \text{ Cl}^- \text{ ion} \]
- However, since we are looking at the coordination of the Cs^+ ion, we need to consider how many Cl^- ions surround it directly.

5. **Determine the Coordination Number**:
- In the CsCl structure, each Cs^+ ion is surrounded by 8 Cl^- ions located at the corners of the cube. Therefore, the coordination number of Cs^+ in CsCl is 8.

6. **Conclusion**:
- The correct answer to the question is that each Cs^+ ion is surrounded by **8 Cl^- ions**.

### Final Answer:
Each Cs^+ ion in CsCl is surrounded by **8 Cl^- ions**.