ln which of the following electronic configuration ionisation energy will be maximum in

Options

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

Answer

To determine which electronic configuration has the maximum ionization energy, we need to analyze the electronic configurations provided and understand the factors affecting ionization energy.

### Step-by-Step Solution:

1. **Understanding Ionization Energy**:
Ionization energy is the energy required to remove an electron from an atom in its gaseous state. It is influenced by the atomic size, nuclear charge, and the electron configuration of the atom.

2. **Electron Configuration Analysis**:
- Full-filled and half-filled electron configurations are generally more stable due to symmetry and exchange energy. Therefore, they tend to have higher ionization energies.
- Half-filled configurations (like p^3) are particularly stable because of their symmetry and the exchange energy.

3. **Comparing Configurations**:
- If we have configurations like 3p^3 (which is half-filled) and 4p^3 (also half-filled), we need to consider their positions in the periodic table.
- The 3p^3 configuration corresponds to phosphorus, while the 4p^3 configuration corresponds to arsenic.

4. **Trends in Ionization Energy**:
- Ionization energy generally increases across a period and decreases down a group in the periodic table.
- Since phosphorus (3p^3) is higher up in the periodic table than arsenic (4p^3), phosphorus will have a higher ionization energy due to its smaller atomic size and greater effective nuclear charge.

5. **Conclusion**:
- Among the given electronic configurations, the one with the highest ionization energy will be the one corresponding to the half-filled configuration that is higher up in the periodic table, which is 3p^3.

### Final Answer:
The electronic configuration with maximum ionization energy is **3p^3**.