The Ionic radius of `Br^(-1)` is `1.96A^@` and the Ionic radius of `I^(-1)` will be 

Options

A. `2.20 A^@`
B. `1.96 A^@`
C. `1.84 A^@`
D. `1.33 A^@`

Answer

To find the ionic radius of \( I^{-1} \) given that the ionic radius of \( Br^{-1} \) is \( 1.96 \, \text{Å} \), we can follow these steps:

### Step 1: Understand the trend in ionic radii
The ionic radius generally increases down a group in the periodic table. Since bromine (Br) is above iodine (I) in Group 17 (the halogens), we can conclude that the ionic radius of iodine will be larger than that of bromine.

**Hint:** Remember that as you move down a group in the periodic table, the size of the atoms and their corresponding ions increases due to the addition of electron shells.

### Step 2: Compare the ionic radii of \( Br^{-1} \) and \( I^{-1} \)
Given that the ionic radius of \( Br^{-1} \) is \( 1.96 \, \text{Å} \), we need to find a value for \( I^{-1} \) that is larger than \( 1.96 \, \text{Å} \).

**Hint:** Look for a value that is commonly accepted in literature for the ionic radius of \( I^{-1} \) based on periodic trends.

### Step 3: Identify the ionic radius of \( I^{-1} \)
The ionic radius of \( I^{-1} \) is typically cited as approximately \( 2.20 \, \text{Å} \). This value is larger than that of \( Br^{-1} \), which is consistent with the trend we identified.

**Hint:** Use reliable sources or periodic tables to verify the ionic radius values of halides.

### Step 4: Conclusion
Therefore, the ionic radius of \( I^{-1} \) is \( 2.20 \, \text{Å} \).

**Final Answer:** The ionic radius of \( I^{-1} \) is \( 2.20 \, \text{Å} \).

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