Which pair of the following has maximum and minimum ionic character respectively

Options

A. `RbCl`, `BeCl_2`
B. `LiCl, RbCl`
C. RbCl, LiCl
D. RbCl, AgCl

Answer

To determine which pair of the following has maximum and minimum ionic character respectively, we need to analyze the ionic character based on the size of cations and anions.

### Step-by-Step Solution:

1. **Understanding Ionic Character**: Ionic character is influenced by the size of the cation and anion. For maximum ionic character, we need a large cation and a small anion. Conversely, for minimum ionic character, we need a small cation and a large anion.

2. **Identifying Cations**: The cations provided are:
- Rubidium (Rb)
- Beryllium (Be)
- Lithium (Li)
- Silver (Ag⁺)

3. **Analyzing Cation Sizes**:
- Rubidium (Rb) is in Group 1 and is the largest among the given cations due to its position in the periodic table (it has more electron shells).
- Beryllium (Be) is in Group 2 and is the smallest cation among the choices because it has fewer electron shells and a higher effective nuclear charge.
- Lithium (Li) is larger than Be but smaller than Rb.
- Silver (Ag⁺) is a transition metal and its size is influenced by the d-orbitals, but it is generally larger than Be and Li.

4. **Identifying Anions**: The common anion in this context is Chlorine (Cl⁻).

5. **Determining Maximum Ionic Character**:
- For maximum ionic character, we pair the largest cation (Rb) with the small anion (Cl⁻). Thus, RbCl would have maximum ionic character.

6. **Determining Minimum Ionic Character**:
- For minimum ionic character, we pair the smallest cation (Be) with a larger anion (Cl⁻). Hence, BeCl₂ would exhibit minimum ionic character.

7. **Conclusion**: Therefore, the pair with maximum ionic character is RbCl, and the pair with minimum ionic character is BeCl₂.

### Final Answer:
- Maximum Ionic Character: RbCl
- Minimum Ionic Character: BeCl₂