Values of `1^(st)` four ionisation energies `(kJ//mol)` of an element are respectively 496, 4563, 6913, 9541 the electronic configuration of that element can be.

Options

A. `1s^(2), 2s^(1)`
B. `1s^(2)2s^(2)2p^(1)`
C. `1s^(2),2s^(2),2p^(6)3s^(1)`
D. (3) and (2) both

Answer

To determine the electronic configuration of the element based on the given ionization energies, we will analyze the provided values step by step.

### Step 1: Analyze the Ionization Energies
The first four ionization energies given are:
1. \(IE_1 = 496 \, \text{kJ/mol}\)
2. \(IE_2 = 4563 \, \text{kJ/mol}\)
3. \(IE_3 = 6913 \, \text{kJ/mol}\)
4. \(IE_4 = 9541 \, \text{kJ/mol}\)

The significant increase in the second ionization energy compared to the first suggests that the first electron removed is from a relatively less stable outer shell, while the second electron is removed from a more stable configuration.

### Step 2: Determine the Number of Valence Electrons
The first ionization energy (496 kJ/mol) is relatively low, indicating that the first electron can be removed easily. The large jump to the second ionization energy (4563 kJ/mol) indicates that the second electron is much harder to remove, suggesting that the element has a stable electron configuration after the first ionization.

### Step 3: Consider Possible Electronic Configurations
Given that the first ionization energy is low, and the second is significantly higher, we can infer that the element likely has one valence electron in its outermost shell.

1. **Option 1**: If the element had only three electrons, it would not be able to show four ionization energies. This option is ruled out.
2. **Option 2**: The configuration \(1s^2 2s^2 2p^1\) would result in a very high second ionization energy, which is not consistent with the given values. This option is ruled out.
3. **Option 3**: The configuration \(1s^2 2s^2 2p^6 3s^1\) suggests that after removing one electron, the configuration becomes \(1s^2 2s^2 2p^6\) (which is stable). The second ionization energy would then be much higher, consistent with the given data.

### Step 4: Confirm the Electronic Configuration
After the first ionization, the configuration becomes \(1s^2 2s^2 2p^6\). The second ionization would involve removing an electron from the \(3s\) orbital, which is indeed more stable than the previous configuration. The third and fourth ionization energies would involve removing electrons from the \(2p\) subshell, leading to configurations of \(1s^2 2s^2 2p^5\) and \(1s^2 2s^2 2p^4\), respectively.

### Conclusion
The electronic configuration of the element based on the provided ionization energies is:
**Answer**: \(1s^2 2s^2 2p^6 3s^1\)