Select the correct alternate about ionisation energy(IE)

Options

A. `(IE_1) of Be^+gt(IE) of B`
B. `(IE_1) of Ogt(IE)_1of N`
C. both(1)(2)
D. none of the above

Answer

### Step-by-Step Solution:

1. **Understanding Ionization Energy (IE)**:
- Ionization energy is defined as the minimum amount of energy required to remove an electron from the valence shell of an isolated atom.

2. **Factors Affecting Ionization Energy**:
- The distance of the electron from the nucleus affects ionization energy. Electrons that are farther away from the nucleus experience less electrostatic attraction, making them easier to remove, thus requiring less energy.

3. **Comparison of Elements**:
- To determine which element has a higher ionization energy, we can compare the electronic configurations of the elements in question.
- For example, consider Beryllium (Be) and Boron (B):
- Beryllium: 1s² 2s²
- Boron: 1s² 2s² 2p¹
- In Boron, the removal of the 2p electron leads to a stable configuration (fully filled 2s orbital), making it easier to lose that electron compared to Beryllium.

4. **Analyzing Specific Cases**:
- When comparing Nitrogen (N) and Oxygen (O):
- Nitrogen: 1s² 2s² 2p³ (half-filled p orbital, stable)
- Oxygen: 1s² 2s² 2p⁴
- It is more difficult to remove an electron from Nitrogen due to its stable half-filled p orbital, which results in a higher ionization energy than that of Oxygen.

5. **Conclusion**:
- Based on the comparisons, we can conclude that:
- The ionization energy of Boron is less than that of Beryllium.
- The ionization energy of Nitrogen is greater than that of Oxygen.

### Correct Alternatives:
- The correct statement about ionization energy is that the first ionization energy of Nitrogen is greater than that of Oxygen, while the first ionization energy of Boron is less than that of Beryllium.