Radius ratio of an ionic compound is 0.93. The structure of the above ionic compound is of

Options

A. NaCl type
B. CsCl type
C. ZnS type
D. None of these

Explanation

To determine the structure of an ionic compound based on its radius ratio, we can follow these steps:

### Step 1: Understand the Radius Ratio
The radius ratio (r+/r-) is the ratio of the radius of the cation (r+) to the radius of the anion (r-). This ratio helps in predicting the type of structure an ionic compound will adopt.

### Step 2: Identify the Range of Radius Ratios
Different ranges of radius ratios correspond to different types of voids in ionic compounds:
- **Tetrahedral voids**: Radius ratio between 0.225 and 0.414
- **Octahedral voids**: Radius ratio between 0.414 and 0.732
- **Cubic voids**: Radius ratio between 0.732 and 1

### Step 3: Analyze the Given Radius Ratio
In this case, the radius ratio given is **0.93**.

### Step 4: Compare with the Ranges
- Since **0.93** is greater than **0.732** and less than or equal to **1**, it falls within the range for **cubic voids**.

### Step 5: Identify the Structure
The structure corresponding to a radius ratio of **0.93** is a **cubic structure**. An example of an ionic compound that exhibits a cubic structure is **CSCN** (thallium(I) thiocyanate).

### Conclusion
Thus, the structure of the ionic compound with a radius ratio of **0.93** is that of a **cubic void**.

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