Which of the following options dose not represent electronic ground state of an atom ?

Options

A. `1s^2 2s^2 2p^6 3p^6 3d^8 4s^2`
B. `1s^2 2s^2 2p^6 3p^6 3d^9 4s^2`
C. `1s^2 2s^2 2p^6 3p^6 3d^10 4s^2`
D. `1s^2 2s^2 2p^6 3p^6 3d^5 4s^2`

Explanation

To determine which option does not represent the electronic ground state of an atom, we need to understand the principles of electron configuration, specifically the Aufbau principle, Pauli exclusion principle, and Hund's rule.

### Step-by-Step Solution:

1. **Understand the Aufbau Principle**: This principle states that electrons occupy the lowest energy orbitals first before moving to higher energy levels. The order of filling is generally: 1s, 2s, 2p, 3s, 3p, 4s, 3d, etc.

2. **Analyze Each Option**: We will evaluate each option to see if it follows the correct order of filling according to the Aufbau principle.

- **Option 1**: 1s² 2s² 2p⁶ 3s 0 3p 6
- In this configuration, electrons are placed in 3s before 3p. This is incorrect because 3p should be filled before 3s is left unfilled.
- **Conclusion**: This option does not represent a ground state configuration.

- **Option 2**: 1s² 2s² 2p⁶ 3p⁶
- This configuration fills 3p after 3s, which is correct.
- **Conclusion**: This option represents a ground state configuration.

- **Option 3**: (Assuming a similar pattern as above)
- Evaluate the configuration similarly to see if it follows the Aufbau principle.
- If it fills in the correct order, it represents a ground state.

- **Option 4**: (Assuming a similar pattern as above)
- Again, evaluate for proper filling order.

3. **Final Evaluation**: After analyzing all options, we conclude that the first option is the only one that does not represent the electronic ground state of an atom.

### Answer:
The option that does not represent the electronic ground state of an atom is **Option 1**.