Statement-1 : First electron gain enthalpy is alway -ve for an element.
Statement-2 : Magnitude of electron gain enthalpy irregularly increases from left to right in a period.

Options

A. Statement-1 is true, statement-2 is true and statement-2 is correct explanation for statement-1.
B. Staterment-1 is true, statement-2 is true and statement-2 is NOT the 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 given in the question, we will break down each statement and evaluate its validity.

### Step 1: Evaluate Statement-1
**Statement-1**: First electron gain enthalpy is always negative for an element.

**Analysis**:
- The electron gain enthalpy refers to the energy change when an electron is added to a neutral atom in the gas phase.
- For most elements, this process releases energy, resulting in a negative value for electron gain enthalpy. However, noble gases (like Helium, Neon, Argon, etc.) have a complete valence shell and do not favorably accept additional electrons.
- Therefore, the first electron gain enthalpy for noble gases is positive, indicating that energy must be supplied to add an electron.

**Conclusion**: Statement-1 is **false**.

### Step 2: Evaluate Statement-2
**Statement-2**: Magnitude of electron gain enthalpy irregularly increases from left to right in a period.

**Analysis**:
- As we move from left to right across a period in the periodic table, the atomic size decreases due to increasing nuclear charge, which pulls the electrons closer to the nucleus.
- This decrease in size generally leads to an increase in the attraction between the nucleus and the added electron, which means that the energy released (magnitude of electron gain enthalpy) tends to increase.
- However, the increase is not uniform due to the presence of different subshells and the stability of half-filled and fully filled orbitals, which can cause irregularities in the trend.

**Conclusion**: Statement-2 is **true**.

### Final Conclusion
- **Statement-1** is false.
- **Statement-2** is true.

Thus, the correct answer is that Statement-1 is false and Statement-2 is true.