A mongst the elements with following electronic configurations, which one of them may have the highest ionization energy?

Options

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

Answer

To determine which element has the highest ionization energy among those with the given electronic configurations, we need to analyze the configurations and apply our understanding of periodic trends.

### Step-by-Step Solution:

1. **Identify the Electronic Configurations**:
- The electronic configurations given are:
1. Neon: \(1s^2 2s^2 2p^6\)
2. Argon: \(1s^2 2s^2 2p^6 3s^2 3p^2\)
3. Another element: \(1s^2 2s^2 2p^6 3s^2 3p^1\)
4. Another element: \(1s^2 2s^2 2p^6 3s^2 3p^3\)

2. **Determine the Period and Group**:
- All the elements listed belong to the third period of the periodic table, as they have the highest principal quantum number \(n = 3\).
- The elements are likely to be from the p-block, as indicated by the presence of p electrons.

3. **Understand Ionization Energy Trends**:
- Ionization energy generally increases across a period from left to right due to increasing nuclear charge, which holds the electrons more tightly.
- Ionization energy decreases down a group due to increased atomic size and shielding effect.

4. **Evaluate the Stability of Electron Configurations**:
- The stability of half-filled and fully filled subshells leads to higher ionization energy.
- The configuration with \(3p^3\) (which corresponds to the fourth option) is half-filled and thus more stable compared to configurations with \(3p^1\) and \(3p^2\).

5. **Conclusion**:
- Among the configurations provided, the element with the configuration \(3p^3\) will have the highest ionization energy due to its half-filled stability.

### Final Answer:
The element with the configuration \(3s^2 3p^3\) has the highest ionization energy.

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