Statement-1 : `B_(2)O_(3)` is more acidic than BeO.
Statement-2 : Ionisation energy of B is more than Be.

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

Answer

To analyze the statements provided in the question, we will break down each statement step by step and determine their validity.

### Step 1: Analyze Statement 1
**Statement 1**: B₂O₃ is more acidic than BeO.

- **Explanation**: In the periodic table, as we move from left to right across a period, the oxides of elements tend to become more acidic. Metals typically form basic oxides, while non-metals form acidic oxides.
- Beryllium (Be) is a metal and forms BeO, which is a basic oxide. Boron (B), on the other hand, is a metalloid and forms B₂O₃, which is an acidic oxide.
- Therefore, since B₂O₃ is an acidic oxide and BeO is a basic oxide, it follows that B₂O₃ is indeed more acidic than BeO.

**Conclusion**: Statement 1 is correct.

### Step 2: Analyze Statement 2
**Statement 2**: Ionization energy of B is more than Be.

- **Explanation**: Ionization energy is the energy required to remove an electron from an atom.
- The electronic configuration of Beryllium (Be) is 1s² 2s², and for Boron (B), it is 1s² 2s² 2p¹.
- Beryllium has a completely filled outer shell (2s²), which makes it more stable and requires more energy to remove an electron compared to Boron, which has an unfilled p-orbital (2p¹).
- Thus, it is easier to remove an electron from Boron than from Beryllium, indicating that the ionization energy of Beryllium is greater than that of Boron.

**Conclusion**: Statement 2 is incorrect.

### Final Conclusion
- Statement 1 is correct: B₂O₃ is more acidic than BeO.
- Statement 2 is incorrect: The ionization energy of B is not more than that of Be; it is the other way around.

### Answer
- Statement 1 is correct, and Statement 2 is incorrect.