Assertion `MgCl_(2)` is more soluble as comared to `BeCl_(2)`
Reasoning `BeCl_(2)` is covalent and `MgCl_(2)` is ionic compound .

Options

A. If both `(A)` and `(R )` are correct and `(R )` is the correct
explanation of `(A)`
B. If both `(A)` and `(R )` are correct and `(R )` is the correct
explanation of `(A)`
C. If `(A)` is correct but `(R )` is incorrect
D. If `(A)` is incorrect but `(R )` is correct

Answer

To solve the assertion and reasoning question regarding the solubility of MgCl₂ compared to BeCl₂, we can break down the solution into the following steps:

### Step 1: Identify the Compounds
We are comparing two compounds: magnesium chloride (MgCl₂) and beryllium chloride (BeCl₂).

### Step 2: Determine the Nature of the Compounds
- **MgCl₂**: Magnesium has a +2 oxidation state, and it forms an ionic compound with chloride ions (Cl⁻).
- **BeCl₂**: Beryllium also has a +2 oxidation state, but it forms a covalent compound with chloride ions.

### Step 3: Analyze the Solubility
- Ionic compounds tend to be more soluble in polar solvents (like water) compared to covalent compounds.
- Since MgCl₂ is ionic, it is expected to be more soluble in water than BeCl₂, which is covalent.

### Step 4: Consider the Size of the Cations
- Beryllium (Be) has a smaller ionic radius compared to magnesium (Mg). According to Fajans' rules, smaller cations tend to have a higher covalent character because they polarize the electron cloud of the anion more effectively.
- Therefore, BeCl₂ has more covalent character than MgCl₂.

### Step 5: Conclusion
- Since MgCl₂ is more ionic and BeCl₂ is more covalent, MgCl₂ is indeed more soluble in water than BeCl₂.

### Final Answer
Both the assertion and reasoning are correct. The reasoning correctly explains why MgCl₂ is more soluble than BeCl₂.

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