Statement-1 : Ionization energy of s-electrons are more than the p-electrons for the same shell.
Statement-2 : s electrons are closer to the nucleus than p-electrons, hence, more tightly attached.

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 solve the question, we need to analyze both statements regarding ionization energy and the position of s and p electrons in relation to the nucleus.

### Step-by-Step Solution:

1. **Understanding Ionization Energy**:
- Ionization energy is the energy required to remove an electron from an isolated gaseous atom. It generally increases across a period and decreases down a group in the periodic table.

2. **Comparing s and p Electrons**:
- For the same principal quantum number (n), we can compare the s and p electrons. For example, consider the 2s and 2p electrons.
- The 2s orbital is spherical in shape, while the 2p orbital has a dumbbell shape.

3. **Electron Distribution**:
- The spherical shape of the s orbital means that the electron density is distributed closer to the nucleus compared to the p orbital. This means that s electrons are generally found closer to the nucleus than p electrons.

4. **Effect on Ionization Energy**:
- Since s electrons are closer to the nucleus, they experience a stronger electrostatic attraction to the positively charged nucleus. This makes them more tightly bound compared to p electrons.
- Therefore, it requires more energy to remove an s electron than a p electron from the same shell.

5. **Evaluating the Statements**:
- **Statement 1**: "Ionization energy of s-electrons is more than the p-electrons for the same shell." This statement is true, as we have established that s electrons are more tightly bound.
- **Statement 2**: "s electrons are closer to the nucleus than p-electrons, hence, more tightly attached." This statement is also true, as it explains why s electrons have higher ionization energy.

6. **Conclusion**:
- Both statements are true, and Statement 2 correctly explains Statement 1. Therefore, the correct option is that both statements are true, and Statement 2 is the correct explanation for Statement 1.

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

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