B has a smaller first ionization enthalpy than Be. Consider the following statements
(i) it is easier to remove 2p electron than 2s electron
(ii) 2p electron of B is more shielded from the nucleus by the inner core of electrons than the 2s electrons of Be
(iii) 2s electron has more penetration power than 2p electron
(iv) atomic radius of B is more than Be (atomic number B= 5, Be = 4) The correct statements are

Options

A. (i),(ii) and (iv)
B. (i),(iii) and (iv)
C. (i),(ii) and (iii)
D. (ii),(iii) and (iv)

Answer

To solve the question regarding the first ionization enthalpy of Boron (B) and Beryllium (Be), we will analyze each statement provided in the question step by step.

### Step-by-Step Solution:

1. **Understanding the Ionization Enthalpy**:
- The first ionization enthalpy is the energy required to remove the outermost electron from an atom in its gaseous state.
- Beryllium (Be) has the electronic configuration of 1s² 2s², while Boron (B) has the configuration of 1s² 2s² 2p¹.

2. **Analyzing Statement (i)**:
- **Statement (i)**: "It is easier to remove a 2p electron than a 2s electron."
- **Analysis**: In Boron, the outermost electron is in the 2p orbital, while in Beryllium, it is in the 2s orbital. The 2s orbital is completely filled and thus more stable, making it harder to remove an electron from it compared to the 2p orbital, which has only one electron.
- **Conclusion**: This statement is **correct**.

3. **Analyzing Statement (ii)**:
- **Statement (ii)**: "The 2p electron of B is more shielded from the nucleus by the inner core of electrons than the 2s electrons of Be."
- **Analysis**: In Boron, the 2p electron is shielded by the 1s² and 2s² electrons. In Beryllium, the 2s electrons are shielded only by the 1s² electrons. Therefore, the 2p electron in Boron experiences more shielding.
- **Conclusion**: This statement is **correct**.

4. **Analyzing Statement (iii)**:
- **Statement (iii)**: "The 2s electron has more penetration power than the 2p electron."
- **Analysis**: The 2s electrons are closer to the nucleus and have a greater ability to penetrate the electron cloud, leading to a stronger attraction to the nucleus compared to the 2p electrons, which are further away.
- **Conclusion**: This statement is **correct**.

5. **Analyzing Statement (iv)**:
- **Statement (iv)**: "The atomic radius of B is more than Be."
- **Analysis**: As we move across a period from left to right in the periodic table, the atomic radius generally decreases due to the increase in nuclear charge, which pulls the electrons closer to the nucleus. Therefore, Boron has a smaller atomic radius than Beryllium.
- **Conclusion**: This statement is **incorrect**.

### Final Conclusion:
The correct statements are (i), (ii), and (iii). Thus, the answer to the question is that statements (i), (ii), and (iii) are correct.