Applying Aufbau's Principle to Element Configurations

Heinrich Oswald and StudyBoosterAI
### Aufbau's Principle in Electronic Configuration

**Definition**: 
Aufbau’s principle states that electrons occupy the lowest energy orbitals first before filling higher energy levels. This helps determine the electron configuration of an atom systematically.

### Key Points:

1. **Energy Levels**: Electrons fill orbitals starting from the lowest energy level (1s) and move to higher levels (2s, 2p, etc.).
  
2. **Order of Filling**: The sequence of filling can be described using the diagonal rule, which gives a visual flow of how orbitals are filled.

3. **Orbital Diagrams**: These represent the electron configurations, showing how electrons are distributed in orbitals.

### Order of Orbital Filling:
1. **1s**
2. **2s**
3. **2p**
4. **3s**
5. **3p**
6. **4s**
7. **3d**
8. **4p**
9. **5s**
10. **4d**
11. **5p**
12. **6s**
13. **4f**
14. **5d**
15. **6p**
16. **7s**
17. **5f**
18. **6d**
19. **7p**

### Examples:

- **Hydrogen (H)**: 
  - Atomic Number: 1 
  - Electron Configuration: 1s¹

- **Carbon (C)**:
  - Atomic Number: 6
  - Electron Configuration: 1s² 2s² 2p²

- **Neon (Ne)**:
  - Atomic Number: 10
  - Electron Configuration: 1s² 2s² 2p⁶

- **Iron (Fe)**:
  - Atomic Number: 26
  - Electron Configuration: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁶

- **Uranium (U)**:
  - Atomic Number: 92
  - Electron Configuration: [Rn] 7s² 5f³

### Infographic Idea:
Create an infographic by visually displaying the following:
- The order of orbital filling as a flowchart or diagram.
- Illustrate example elements with their atomic numbers and electron configurations in a tabular format.
- Use color coding to differentiate between s, p, d, and f orbitals.

This visual representation can serve as an educational tool to help comprehend and remember Aufbau's principle and its application in determining electron configurations for various elements.


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