The electronic configuration with the highest ionization enthalpy is :

Options

A. `[Ar]3d^(10)4s^(2)4p^3`
B. `[Ne]3s^(2)3p^1`
C. `[Ne]3s^(2)3p^3`
D. `[Ne]3s^(2)3p^2`

Answer

To determine which electronic configuration has the highest ionization enthalpy, we need to analyze the stability of the electronic configurations given in the options. Ionization enthalpy is the energy required to remove an electron from an atom, and it is influenced by the stability of the electron configuration.

### Step-by-Step Solution:

1. **Understand Ionization Enthalpy**: Ionization enthalpy increases with the stability of the electronic configuration. Full and half-filled subshells are more stable than other configurations.

2. **Identify the Electronic Configurations**: Let's analyze the provided configurations:
- A: 3D10 4S2 4P3
- B: 3P2
- C: 3S2 3P3
- D: 3P1

3. **Eliminate Less Stable Configurations**:
- Configurations B (3P2) and D (3P1) are less stable as they do not have full or half-filled subshells. These configurations will have lower ionization enthalpy as they can easily lose electrons.

4. **Focus on Configurations with Full or Half-Filled Subshells**:
- Configuration A (3D10 4S2 4P3) has a full 3D subshell and a half-filled 4P subshell.
- Configuration C (3S2 3P3) has a half-filled 3P subshell.

5. **Consider the Distance from the Nucleus**:
- Electrons in the 3P subshell (Configuration C) are closer to the nucleus than those in the 4P subshell (Configuration A).
- The closer the electrons are to the nucleus, the more energy is required to remove them.

6. **Compare the Stability and Distance**:
- While both configurations A and C have stable arrangements, Configuration C (3S2 3P3) has electrons that are closer to the nucleus, making it harder to remove them compared to Configuration A (3D10 4S2 4P3).

7. **Conclusion**:
- Therefore, the configuration with the highest ionization enthalpy is **C: 3S2 3P3**.

### Final Answer:
The electronic configuration with the highest ionization enthalpy is **C: 3S2 3P3**.