1. CHAPTER FOUR – ELECTRON CONFIGURATION SOUTH LAKE HIGH SCHOOL SCIENCE DEPARTMENT MS. SANDERS Chemistry

2. Electron Configuration  3 Rules:  Aufbau Principle – electrons occupy the lowest energy level first (1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p)  Pauli Exclusion Principle – 2 electrons can occupy one orbital and they must have opposite spins  Hund’s Rule – if there is more than one orbital, each orbital has one electron before the second electron is added

3. Electron Configuration Representation:  Orbital Notation  Electron Configuration  Noble Gas Configuration

4. Electron Configuration Sublevels and Orbitals: Sublevel # Orbitals# Electrons s12 p36 d510 f714

5. Electron Configuration Four Sublevel Blocks

6. Practice Electron Configuration Practice page 113: Nitrogen  Electron Configuration: 1s ²2s²2p³  # electrons: 7  Atomic #: 7  Orbital Notation:  Unpaired electrons: 3  Electrons in highest energy level: 5

7. Practice Electron Configuration Practice page 113 Fluorine  Electron Configuration: 1s ²2s²2p⁵  Atomic #: 9  # Electrons: 9  Orbital Notation:  Filled p orbitals: 2

8. Practice Electron Configuration Practice page 113 Phosphorus  Orbital Notation:  Electron Configuration:  Noble-Gas Configuration: [Ne] 3s ²3p³

9. Orbital Shapes Shapes of s, p, and d orbitals

10. Energy Levels Relative Energies