1. Chapter 8: Electronic Structure and Periodic Properties

2. Orbital Energies For Single Electron Systems

3. Penetration and Shielding

4. Orbital Energies

5. Electron Configurations The Aufbau process (building up): Electrons will always populate the lowest energy state available. We will use several “rules”, plus our knowledge of electron orbitals to identify the electronic configuration of any atom

6. The Pauli exclusion principle No two electrons can have all four quantum numbers alike. Hund’s rule Populate all degenerate orbitals (orbitals of the same energy) with a single electron before putting a second electron in any orbital. There are several exceptions to this rule. Electron Configurations

7. Orbital Filling Because of electron shielding, orbital energies are usually ordered as shown above

8. The Electronic Configuration of Carbon

9. The Electronic Configuration of N – Ne

10. Filling the d Orbitals

12. Classifying the Elements When the elements are arranged in order of increasing atomic mass, certain sets of properties recur periodically.

13. Alkali MetalsAlkaline EarthsTransition MetalsHalogensNoble Gases Lanthanides and Actinides Main Group

14. Electron Configurations and the Periodic Table

15. The Sizes of Atoms and Ions

16. Radii of Cations

17. Radii of Anions

18. Atomic and Ionic Radii

20. Electron Affinity

21. Periodic Properties of the Elements

22. Trends in Physical Properties

23. 332 266 Trends in Physical Properties