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 compounds has maximum and minimum ionic character, we need to analyze the factors that influence ionic character in compounds. Ionic character is influenced by the sizes of the cation and anion involved in the ionic bond.

### Step-by-Step Solution:

1. **Understanding Ionic Character**:
- Ionic character is the degree to which a bond between two atoms has ionic characteristics. It is influenced by the size of the cation (positive ion) and the anion (negative ion).
- Generally, a large cation and a small anion will lead to a higher ionic character, while a small cation and a large anion will lead to a lower ionic character.

2. **Identifying Cations and Anions**:
- From the given options, identify the cations and anions present in each compound. For example, if we have compounds like RbCl and BeCl2, Rb (Rubidium) is a cation and Cl (Chlorine) is an anion in both cases.

3. **Comparing Sizes of Cations**:
- Among alkali metals, Rubidium (Rb) is the largest cation. Therefore, Rb will have a higher ionic character when paired with a small anion like Cl.
- For the minimum ionic character, we look for the smallest cation, which is Beryllium (Be) in the second group.

4. **Comparing Sizes of Anions**:
- Chlorine (Cl) is a relatively small anion, while larger anions would decrease ionic character. In the case of BeCl2, Be is small and Cl is larger compared to other anions, leading to lower ionic character.

5. **Conclusion**:
- The pair with maximum ionic character is RbCl (Rubidium Chloride) due to the large size of Rb and the small size of Cl.
- The pair with minimum ionic character is BeCl2 (Beryllium Chloride) due to the small size of Be and the relatively larger size of Cl.

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