1. Quantum Electron Configurations

2. Erwin Schrödinger 1887 - 1961

3. The Schrödinger Equation

4. Werner Heisenberg 1901 – 1976

5. Bohr Theory The electron is a particle that must be in orbital in the atom. Quantum Theory The electron is like a cloud of negative energy or a wave. Orbitals are areas in 3D space where the electrons most probably are. The energy of the electron is in its vibrational modes- like notes on a guitar string. Photons are produced when high energy modes change to lower energy modes

6. S orbitals Each orbital holds 2 electrons

7. S orbitals S S

8. P orbitals There are 3 suborbitals Each contains 2 electrons Total electrons = 6 Animation

9. P Orbitals

11. D orbitals There are 5 suborbitals Each contains 2 electrons Total electrons = 10

12. D orbitals

13. F orbitals There are 7 suborbitals Each contains 2 electrons Total electrons = 14

14. F orbitals

15. Quantum Periodic Table F Count the electrons in each different orbital type until you get to Fluorine. Put in order of lowest to highest energy level. 1s 2 2s 2 2p 5

16. 1.F The Electron Configuration 1s22s22p51s22s22p5 Principle Quantum Number Number of Electrons in the Orbital Orbital Type- s, p, d, or f

17. Quantum Periodic Table 2p 6 3p 6

18. Simplify to a Bohr electron configuration 1s22s22p63s23p64s21s22s22p63s23p64s2 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 2 8 8 2 2.Ca

19. Quantum Periodic Table 2p 6 3p 6 3d 9

20. 3.Cu 1s22s22p63s23p63d94s21s22s22p63s23p63d94s2 Simplify to a Bohr electron configuration 1s 2 2s 2 2p 6 3s 2 3p 6 3d 9 4s 2 2 8 17 2

21. Quantum Periodic Table Count the electrons in each different orbital type until you get to Kr. Put in order of lowest to highest energy level. 2p 6 3p 6 3d 10 4p 6

22. 4.Kr 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 Simplify to a Bohr electron configuration 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 2 8 18 8

23. Quantum Periodic Table 2p 6 3p 6 3d 10 4p 6 4d 4

24. 4.Mo 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 4 5s 2

25. Quantum Periodic Table 2p 6 3p 6 3d 10 4p 6 4d 10 5p 5

26. 5.I 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 5s 2 5p 5 Simplify to a Bohr electron configuration 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 5s 2 5p 5 2 8 18 18 7

27. Why does the 4s fill before the 3d? 3s 3d 3p 4s 4p 5s

29. Quantum Periodic Table 2p 6 3p 6 3d 10 4p 6 4d 10 5p 6

30. 6.Ba 2+ 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 5s 2 5p 6 7.Xe 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 5s 2 5p 6 8.I - 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 5s 2 5p 6 The above chemical species are isoelectronic- same electron configuration

32. Ishihara Test for Colour Blindness – if you can read all of the numbers you have good colour vision Atomic Theory Song