If nitrogen atoms had electronic configuration `1s^(7)` It would have energy lower than that of the normal ground state configuration `1s^(2) 2s^(2) 2p^(3)` because the electrons would be closer to the nucleus yet `1s^(7)` is not observed because it violates ?

Options

A. Heisenberg's uncertainty principal
B. Hand,'s rule
C. Pauill's exclusion principle
D. Bohr's postatate of stationary orbit

Explanation

To solve the question regarding why the electronic configuration `1s^(7)` is not observed for nitrogen atoms, we need to analyze the principles governing electron configurations.

### Step-by-Step Solution:

1. **Understanding the Ground State Configuration**:
- The normal ground state electronic configuration of nitrogen is `1s^(2) 2s^(2) 2p^(3)`. This configuration has a total of 7 electrons, which is consistent with nitrogen's atomic number of 7.

2. **Proposed Configuration**:
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