Heinrich Oswald- Reflection
- 2025-01-14
### 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.
