Which of the following configuration is incorrect ?

Options

A. `1s^(2)2s^(2)2p_(x)^(2)2p_(y)^(2)2p_(z)^(0)`
B. `1s^(2)2s^(2)2p_(x)^(1)2p_(y)^(1)`
C. `1s^(2)2s^(2)2p_(x)^(1)2p_(y)^(1)2p_(z)^(1)`
D. `1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)4s^(1)``

Explanation

To determine which electron configuration is incorrect, we will analyze each provided configuration based on the principles of electron distribution, particularly Hund's Rule and the Pauli Exclusion Principle.

### Step-by-step Solution:

1. **Understanding Electron Configurations**:
- Electron configurations describe how electrons are distributed among the various atomic orbitals. Each orbital can hold a maximum of two electrons, and they must have opposite spins.

2. **Applying Hund's Rule**:
- According to Hund's Rule, electrons will fill degenerate orbitals (orbitals of the same energy) singly first, with parallel spins, before pairing up.

3. **Analyzing Each Configuration**:
- **Configuration A: 1s² 2s² 2p² (2px², 2py², 2pz)**
- Here, the 2p subshell has 2 electrons distributed across the three orbitals (2px, 2py, 2pz).
- According to Hund's Rule, the correct filling should be: 2px¹, 2py¹, and 2pz⁰ (one electron in each of the 2p orbitals before pairing).
- Thus, this configuration is incorrect as it violates Hund's Rule.

- **Configuration B: 1s² 2s² 2p¹ (2px¹, 2py⁰, 2pz⁰)**
- This configuration is correct as it places one electron in the 2px orbital, which follows Hund's Rule.

- **Configuration C: 1s² 2s² 2p³ (2px¹, 2py¹, 2pz¹)**
- This configuration is also correct as it fills each of the 2p orbitals with one electron before pairing.

- **Configuration D: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹**
- This configuration is correct as it fills the orbitals in the proper order according to the Aufbau principle.

4. **Conclusion**:
- The incorrect configuration is **Option A: 1s² 2s² 2p² (2px², 2py², 2pz)**.

### Final Answer:
The incorrect electron configuration is **Option A: 1s² 2s² 2p² (2px², 2py², 2pz)**.