chemistry 4_Quantum_theory_Hydrogen.pptx

chemistry

1. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 1 of 50 Philip Dutton University of Windsor, Canada Prentice-Hall © 2002 General Chemistry Principles and Modern Applications Petrucci • Harwood • Herring 8 th Edition Chapter 9: Electrons in Atoms

2. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 2 of 50 9-5 Two Ideas Leading to a New Quantum Mechanics Wave-Particle Duality. Einstein suggested particle-like properties of light could explain the photoelectric effect. But diffraction patterns suggest photons are wave-like. deBroglie, 1924 Small particles of matter may at times display wavelike properties.

3. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 3 of 50 deBroglie and Matter Waves E = mc 2 h  = mc 2 h /c = mc = p p = h/ λ λ = h/p = h/mv

4. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 4 of 50

5. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 5 of 50 The Uncertainty Principle Δ x Δ p ≥ h 4 π Werner Heisenberg

6. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 6 of 50

7. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 7 of 50 STANDING WAVES See standing waves

8. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 8 of 50 9-6 Wave Mechanics 2L n Standing waves. Nodes do not undergo displacement. L = n ( λ  2), n = 1, 2, 3… λ = , n = 1, 2, 3…

9. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 9 of 50 Schrodinger Equation: Erwin Schrodinger 1887 - 1961

10. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 10 of 50 Wave Functions ψ , psi, the wave function. Should correspond to a standing wave within the boundary of the system being described. Particle in a box.

11. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 11 of 50 Probability of Finding an Electron

12. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 12 of 50 The Energy of The Waves E n = The Energy is quantized The lowest Energy is not zero

13. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 13 of 50 Principle Shells and Subshells Principle electronic shell, n = 1, 2, 3… Angular momentum quantum number, l = 0, 1, 2…(n-1) l = 0, s l = 1, p l = 2, d l = 3, f Magnetic quantum number, m l = - l …-2, -1, 0, 1, 2…+ l

14. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 14 of 50

15. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 15 of 50

16. Prentice-Hall © 2002 General Chemistry: Chapter 2 Slide 16 of 25 S -orbital

17. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 17 of 50 s orbitals

18. Prentice-Hall © 2002 General Chemistry: Chapter 2 Slide 18 of 25 S –orbitals

19. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 19 of 50 p Orbitals

20. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 20 of 50 p Orbitals

21. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 21 of 50 P-Orbitals

22. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 22 of 50 d Orbitals

23. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 23 of 50 4f - Orbitals

24. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 24 of 50

25. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 25 of 50 Radial Probability distribution =  2 ·4  r 2 ·dr Z eff is the effective nuclear charge. Penetration and Shielding

26. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 26 of 50 9-9 Electron Spin: A Fourth Quantum Number

27. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 27 of 50

28. Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 28 of 50 Orbital Energies