1. An Electron Trapped in A Potential Well Probability densities for an infinite well Solve Schrödinger equation outside the well

2. inside the well An Electron Trapped in A Potential Well The general solution is By the boundary conditions

3. An Electron Trapped in A Potential Well Normalization For odd wave function For even wave function probability

4. inside the well An Electron Trapped in A Potential Well energy distribution

5. Barrier Tunneling Dividing the space into three parts: I) to the left of the barrier II) within the barrier; and III) to the right of the barrier The conditions for wave functions at the boundary are continuity.

6. Barrier Tunneling Tunneling current

8. Si(111) Surface

9. Tetracene/Ag(110) [001] 0.04 nm

10. Wave (matter wave) Uncertainty Principle Wave Function Schrödinger’s Equation probability Free Electrons Hydrogen atom de Broglie relation, de Broglie wavelength. Potential Well Particle The Nature of Matter Energy quantization Probability Barrier Tunneling STM

11. Chapter 48 Atomic Structure

12. Schrödinger’s Equation =0.529ÅBohr radius ground state (n=1) n=2

13. ground state Energy quantization Principle quantum number Schrödinger’s Equation

14. The Uncertainty Principle The angular momentum-angle Uncertainty Relationship

15. Schrödinger’s Equation Angular Momentum of Electrons in Atoms Angular momentum quantum number Angular momentum quantization

16. l 0 1 2 3 4 5 code s p d f g h Using this labeling, we can express 1s for ground state (n=1, l=0). The first excited state has two designations: 2s (n=2, l=0) and 2p (n=2, l=1). Angular momentum quantum number l=0, 1, 2, …, n-1. Ex. n=1, l=0 for s state n=2, l=0, 1. for l=0, s state and l=1, p state

17. Space quantization m l =-l, -(l-1), …-1, 0, 1, …,(l-1), l magnetic quantum number

18. n Principle quantum number l Angular momentum quantum number m l =-l, -(l-1), …-1, 0, 1, …,(l-1), l m l magnetic quantum number

19. (n=1, l=0) The Ground State ground state (n=1) m l =0, is spherically symmetric.

20. The 2s State (n=2, l=0) m l =0, is spherically symmetric.

21. An Excited State Of The Hydrogen Atom The 2p State (n=2, l=1) m l =-1, 0, +1 is not spherically symmetric.

22. Electron Spin Pauli pointed out the need for a 4 th quantum number in 1924—Spin quantum number and l Angular momentum quantum number Spin magnetic quantum number s Spin momentum quantum number

23. The States of Atomic Hydrogen The assembly of all hydrogen-atom states with the same principal quantum number n are said to form a shell. The collection of all states with the same value of the orbital angular momentum quantum number l is called a subshell. For a certain angular momentum l, there are 2l+1 states, and consider spin there are 2(2l+1) states. m l =-l, -(l-1), …-1, 0, 1, …,(l-1), l

24. states Example m l =-l, -(l-1), …-1, 0, 1, …,(l-1), l states

25. The X-Ray Spectrum of Atoms The Characteristic X-ray Spectrum

26. Atomic Magnetism How to study the angular momentum properties of the atom ? L is the orbital angular momentum vector of the electron. The component of z direction L z =m l ħ, m l =-l, -(l-1),...-1, 0, +1,..., +l

27. Atomic Magnetism L z =m l ħ, m l =-l, -(l-1),...-1, 0, +1,..., +l It can be expressed by Bohr magnetron µ B We can express the magnetic dipole moment in terms of the Bohr magnetron

28. The energy of electron

29. If we were to place an atom having a magnetic dipole moment in a magnetic field, which we assume is in the z direction, the energy associated with the interaction between the atom and the magnetic field is That is, atoms with different values of m l have different energies in the field, which provides a way to determine their orbital angular momentum. Atomic Magnetism

30. The Stern-Gerlach Experiment

31. there is no semiclassical corresponding. The full quantum mechanics gives Atomic Magnetism spin angular momentum angular momentum Sodium atom (Z=11) The Zeeman effect

32. Inverted population Lasers and Laser Light Stimulated emission Emission

33. Lasers and Laser Light Four properties 1) Laser light is highly monochromatic. 2) Laser light is highly coherent 3) Laser light is highly directional 4) Laser light can be sharply focused.

34. Exercises P1099 15, 16, 17 P1100 28, 30