TiCl has structure similar as CsCl, the co-ordination number of `Ti^(+)` will be:

Options

A. 4
B. 6
C. 10
D. 8

Answer

To determine the coordination number of \( \text{Ti}^+ \) in \( \text{TiCl} \), which has a structure similar to \( \text{CsCl} \), we can follow these steps:

### Step-by-Step Solution:

1. **Understand the Structure of CsCl**:
- CsCl crystallizes in a body-centered cubic (BCC) structure. In this structure, there are 8 atoms located at the corners of the cube and 1 atom at the center of the cube.

2. **Identify the Position of Atoms**:
- In the case of CsCl, the cesium ion (\( \text{Cs}^+ \)) is located at the body center, while the chloride ions (\( \text{Cl}^- \)) occupy the corners of the cube.

3. **Apply the Same Structure to TiCl**:
- Since \( \text{TiCl} \) has a similar structure to \( \text{CsCl} \), we can infer that \( \text{Ti}^+ \) will occupy the body center of the cube and the \( \text{Cl}^- \) ions will be at the corners.

4. **Determine the Coordination Number**:
- The coordination number is defined as the number of nearest neighboring atoms surrounding a central atom. In this case, the \( \text{Ti}^+ \) ion is surrounded by the 8 \( \text{Cl}^- \) ions located at the corners of the cube.

5. **Conclusion**:
- Therefore, the coordination number of \( \text{Ti}^+ \) in \( \text{TiCl} \) is 8.

### Final Answer:
The coordination number of \( \text{Ti}^+ \) in \( \text{TiCl} \) is **8**.

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