The electronic configuration of nitrogen is `1s^2,2s^(2)2p_x^(1)2p_y^(1)2p_z^(1)` and not `1s^(2),2s^(2)2p_x^(2)2p_(y)^(1)2p_(z)^(0)` . This is explained by

Options

A. Uncertainty principle
B. Aufbau's principle
C. Pauli's exclusion principle
D. Hund's rule

Answer

To solve the question regarding the electronic configuration of nitrogen, we need to analyze the given configurations and apply the relevant principles of electron configuration.

### Step-by-Step Solution:

1. **Understand the Electronic Configuration of Nitrogen**:
- The atomic number of nitrogen (N) is 7, which means it has 7 electrons.
- The correct electronic configuration is `1s² 2s² 2p_x¹ 2p_y¹ 2p_z¹`.

2. **Identify the Incorrect Configuration**:
- The incorrect configuration provided is `1s² 2s² 2p_x² 2p_y¹ 2p_z⁰`.
- In this configuration, two electrons are placed in the `2p_x` orbital, while the other two `2p` orbitals (`2p_y` and `2p_z`) are not fully utilized.

3. **Apply Hund's Rule**:
- Hund's rule states that electrons will fill degenerate orbitals (orbitals of the same energy) singly before pairing up. This maximizes the number of unpaired electrons.
- In the correct configuration (`2p_x¹ 2p_y¹ 2p_z¹`), nitrogen has three unpaired electrons (one in each of the three `2p` orbitals), which is more favorable than having two electrons in one orbital and one in another (as in the incorrect configuration).

4. **Conclusion**:
- The correct electronic configuration of nitrogen is `1s² 2s² 2p_x¹ 2p_y¹ 2p_z¹`, as it adheres to Hund's rule by maximizing the number of unpaired electrons.
- Therefore, the explanation for the electronic configuration of nitrogen is based on **Hund's rule**.

### Final Answer:
The electronic configuration of nitrogen is explained by **Hund's rule**.