Due to stable electronic configurations
I. noble gases exhibit very high ionisation enthalpy.
II. These have no tendency to accept the electron.
III. these have large positive values of electron gain enthalpy.
The correct set of statements is

Options

A. I and III
B. II and III
C. I and II
D. None of these

Answer

To determine the correct set of statements regarding noble gases and their electronic configurations, we will analyze each statement step by step.

### Step 1: Analyze Statement I
**Statement I:** Noble gases exhibit very high ionization enthalpy due to stable electronic configurations.

- Noble gases (e.g., helium, neon, argon, krypton, xenon) have complete outer electron shells, which makes them very stable.
- The ionization enthalpy is the energy required to remove an electron from an atom. Since noble gases are already stable, removing an electron would disrupt this stability, requiring a significant amount of energy.
- Therefore, this statement is **correct**.

### Step 2: Analyze Statement II
**Statement II:** Noble gases have no tendency to accept an electron.

- Noble gases have full outer electron shells, meaning they do not need to gain electrons to achieve stability.
- As a result, they have a very low tendency to accept additional electrons.
- This statement is also **correct**.

### Step 3: Analyze Statement III
**Statement III:** Noble gases have large positive values of electron gain enthalpy.

- Electron gain enthalpy is the energy change when an electron is added to an atom. For noble gases, since they already have full outer shells, they do not readily accept electrons.
- In fact, the electron gain enthalpy for noble gases is typically zero or even negative, indicating that they do not favor the addition of electrons.
- Therefore, this statement is **incorrect**.

### Conclusion
Based on the analysis:
- Statement I is correct.
- Statement II is correct.
- Statement III is incorrect.

Thus, the correct set of statements is **I and II only**.