Statement-1: Fluorine has less electron affinity than chlorine.
Statement-2 : Due to small size, more electron-electron repulsions are observed in F.

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 need to break down the concepts of electron affinity and the factors influencing it, particularly in the context of fluorine and chlorine.

### Step-by-Step Solution:

1. **Understanding Electron Affinity**:
- Electron affinity refers to the amount of energy released when a neutral gaseous atom gains an electron. It is often measured in kilojoules per mole (kJ/mol). A higher electron affinity indicates that an atom releases more energy upon gaining an electron.

**Hint**: Remember that electron affinity is about the energy change when an atom gains an electron.

2. **Comparison of Fluorine and Chlorine**:
- Fluorine (F) and chlorine (Cl) are both in Group 17 of the periodic table (the halogens). Generally, as we move down a group in the periodic table, electron affinity tends to decrease. This is due to the increasing atomic size and the corresponding increase in distance between the nucleus and the added electron.

**Hint**: Consider the position of the elements in the periodic table and the general trend of electron affinity in groups.

3. **Analyzing Statement 1**:
- Statement 1 claims that fluorine has less electron affinity than chlorine. This is indeed true; chlorine has a higher electron affinity than fluorine. This is an exception to the general trend due to the unique properties of fluorine.

**Hint**: Think about why exceptions occur in periodic trends, especially for small atoms like fluorine.

4. **Analyzing Statement 2**:
- Statement 2 states that due to its small size, fluorine experiences more electron-electron repulsions. This is also true. The small size of fluorine means that when it gains an electron, the added electron is very close to the nucleus and to the other electrons, leading to significant repulsion among them. This repulsion makes it energetically less favorable for fluorine to gain an electron compared to chlorine.

**Hint**: Reflect on how atomic size influences the interactions between electrons in an atom.

5. **Conclusion**:
- Both statements are true. Statement 1 is correct because fluorine does have less electron affinity than chlorine. Statement 2 correctly explains why this is the case, attributing it to the increased electron-electron repulsion in the smaller fluorine atom.

**Final Answer**: Both statements are true, and Statement 2 is the correct explanation of Statement 1.

### Summary of the Solution:
- **Statement 1**: True (Fluorine has less electron affinity than chlorine).
- **Statement 2**: True (Due to small size, more electron-electron repulsions are observed in F).
- **Conclusion**: Both statements are true, and Statement 2 explains Statement 1.