1. Electron Configuration Mapping the electrons

2. Electron Configuration The way electrons are arranged around the nucleus.

3. Quantum Mechanical Model 1920’s Werner Heisenberg (Uncertainty Principle) Louis de Broglie (electron has wave properties) Erwin Schrodinger (mathematical equations using probability, quantum numbers)

4. Heisenberg uncertainty principle it is impossible to determine simultaneously both the position and velocity of an electron or any other particle with any great degree of accuracy or certainty.

5. Erwin Schrodinger  Formulated equation that describes behavior and energies of subatomic particles.  Incorporates both particle and wave behavior in terms of wave function: is proportional to the probability of finding an electron.  Leads to Quantum Mechanics: we cannot pinpoint an electron in an atom but we can define the region where electrons can be in a particular time……… called a Probability map….a 3-dimensional area in space called an ORBITAL

6. Principal Quantum Number, n Indicates main energy levels n = 1, 2, 3, 4… Each main energy level has sub-levels

7. Energy Sublevels s p d fg

8. The principle quantum number, n, determines the number of sublevels within the principle energy level.

9. Orbital Quantum Number, ℓ (Angular Momentum Quantum Number) Indicates shape of orbital sublevels ℓ = n-1 ℓsublevel 0 s 1 p 2 d 3 f 4 g

10. Orbital The space where there is a high probability that it is occupied by a pair of electrons. Orbitals are solutions of Schrodinger’s equations.

11. Orbitals

12. Visualizing the orbitals

13. Orbitals in Sublevels Sublevel # Orbitals # electrons s12 p36 d510 f714 g918

14. Three rules are used to build the electron configuration: Aufbau principle Pauli Exclusion Principle Hund’s Rule

15. Aufbau Principle Electrons occupy orbitals of lower energy first.

16. Orbital Diagram

17. Filling Order diagram

18. -Pauli Exclusion Principle (Wolfgang Pauli, Austria, 1900-1958) -Electron Spin Quantum Number An orbital can hold only two electrons and they must have opposite spin. Electron Spin Quantum Number (m s ): +1/2, -1/2

19. Hund’s Rule In a set of orbitals, the electrons will fill the orbitals in a way that would give the maximum number of parallel spins (maximum number of unpaired electrons). Analogy: Students could fill each seat of a school bus, one person at a time, before doubling up.

20. Orbital Diagram for Hydrogen

21. Orbital Diagram for Helium

22. Orbital Diagram for Lithium

23. Orbital Diagram for Beryllium

24. Orbital Diagram for Boron

25. Orbital Diagram for Carbon

26. Orbital Diagram for Nitrogen

27. Orbital Diagram

28. Notations of Electron Configurations Standard Shorthand

29. Orbital Diagram for Fluorine

30. Standard Notation of Fluorine Main Energy Level Numbers 1, 2, 2 Sublevels Number of electrons in the sub level 2,2,5 1s 2 2s 2 2p 5

31. Shorthand Notation Use the last noble gas that is located in the periodic table right before the element. Write the symbol of the noble gas in brackets. Write the remaining configuration after the brackets. Ex: Fluorine: [He] 2s 2 2p 5

32. Blocks in the Periodic Table