Statement-1:Beryllium resembles aluminium.
Statement-2: Charge/radius ratio of `Be^(2+)` ion is nearly the same as that of the `Al^(3+)` ion.

Options

A. Statement-1 is True, Statement-2 is True, Statement-2 is a correct explanation for Statement-1
B. Statement-1 is True, Statement-2 is True, Statement-2 is NOT a
correct explanation for Statement-1
C. Statement-1 is True, Statement-2 is False.
D. Statement-1 is False, Statement-2 is True.

Explanation

To solve the given question, we will analyze both statements and determine their validity based on chemical principles.

### Step-by-Step Solution:

1. **Understanding Statement 1**:
- Statement 1 claims that "Beryllium resembles Aluminium."
- Beryllium (Be) and Aluminium (Al) are both elements in the periodic table. Beryllium is in Group 2 (alkaline earth metals), while Aluminium is in Group 13 (p-block).
- They exhibit a diagonal relationship, which means that despite being in different groups, they share similar properties due to their position in the periodic table.

**Hint**: Look for the periodic trends and relationships between elements in different groups.

2. **Understanding Statement 2**:
- Statement 2 states that "the charge/radius ratio of Be²⁺ ion is nearly the same as that of the Al³⁺ ion."
- To analyze this, we need to calculate the charge-to-radius ratio for both ions.
- The charge/radius ratio is calculated as follows:
- For Be²⁺: Charge = +2, Radius ≈ 31 pm (picometers)
\[ \text{Charge/Radius ratio for Be}^{2+} = \frac{2}{31} \approx 0.0645 \]
- For Al³⁺: Charge = +3, Radius ≈ 50 pm
\[ \text{Charge/Radius ratio for Al}^{3+} = \frac{3}{50} \approx 0.060 \]

**Hint**: Remember to use the correct ionic radii for the calculations and ensure the units are consistent.

3. **Comparing the Ratios**:
- The calculated ratios show that both ions have similar charge-to-radius ratios (0.0645 for Be²⁺ and 0.060 for Al³⁺), indicating that they have comparable polarizing powers.
- This similarity in charge/radius ratio supports the idea that Beryllium and Aluminium can exhibit similar chemical behavior.

**Hint**: Compare the numerical values obtained from the calculations to evaluate the similarity.

4. **Conclusion**:
- Since both statements are correct and the second statement provides a valid explanation for the first statement, we conclude that:
- Statement 1 is true.
- Statement 2 is true.
- Statement 2 is a correct explanation for Statement 1.

### Final Answer:
Both statements are true, and Statement 2 is a correct explanation for Statement 1.

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