From the ground state, electronic configuration of the elements given below, pick up the one with highest value of second ionization energy:

Options

A. `1s^(2)2s^(2)2p^(6)3s^(2)`
B. `1s^(2)2s^(2)2p^(6)3s^(1)`
C. `1s^(2)2s^(2)2p^(6)`
D. `1s^(2)2s^(2)2p^(5)`

Answer

To determine which element has the highest second ionization energy from the given options, we need to analyze the electronic configurations of the elements and how they change upon the removal of electrons. The second ionization energy (E2) is influenced by the stability of the ion formed after the first ionization energy (E1) is applied. Here’s a step-by-step solution:

### Step 1: Understand Ionization Energy
Ionization energy is the energy required to remove an electron from an atom. The second ionization energy refers to the energy required to remove a second electron after the first has already been removed. The stability of the resulting ion after the first ionization is crucial in determining the second ionization energy.

### Step 2: Analyze Each Option
Let's analyze each option based on their electronic configurations.

1. **Option 1**:
- Assume the element has the configuration: \(1s^2 2s^2 2p^6 3s^1\).
- After the first ionization (removing \(3s^1\)): \(1s^2 2s^2 2p^6\) (Noble gas configuration).
- This is a stable configuration. However, removing another electron from a stable noble gas configuration requires a lot of energy, making \(E2\) large.

2. **Option 2**:
- Assume the element has the configuration: \(1s^2 2s^2 2p^6 3p^1\).
- After the first ionization (removing \(3p^1\)): \(1s^2 2s^2 2p^6\) (Noble gas configuration).
- Again, this is stable, and removing another electron from this stable configuration requires a significant amount of energy, indicating a high \(E2\).

3. **Option 3**:
- Assume the element has the configuration: \(1s^2 2s^2 2p^5\).
- After the first ionization (removing \(2p^5\)): \(1s^2 2s^2 2p^4\).
- This configuration is not as stable as the noble gas configuration, so \(E2\) will not be as high.

4. **Option 4**:
- Assume the element has the configuration: \(1s^2 2s^2 2p^4\).
- After the first ionization (removing \(2p^4\)): \(1s^2 2s^2 2p^3\).
- This configuration is also not very stable, and thus \(E2\) will not be high.

### Step 3: Compare the Ionization Energies
From the analysis:
- **Option 1** and **Option 2** both lead to stable noble gas configurations after the first ionization, suggesting high \(E2\).
- **Option 2** is likely to have a higher \(E2\) compared to **Option 1** because it involves removing an electron from a less stable state (p-orbital) compared to a noble gas configuration.

### Conclusion
The element with the highest second ionization energy is **Option 2**, as it involves removing an electron from a stable noble gas configuration, which requires more energy.