1. The Interaction of Light and Matter
Spectral Lines
Photons
Rutherford-Bohr Model of the Atom
Quantum Mechanics and Wave-Particle Duality

2. How can we know about the stars…?
French Philosopher Auguste Comte ( ) stated that it would not be possible to know the chemical or mineralogical nature of the stars…
Knowledge of the stars and other astrophysical objects relies on the information that is provided to us through electromagnetic radiation….
To do astronomy one must know physics…Need to understand light and how it interacts with matter. Fortunately we understand a lot…

3. Fraunhofer Spectral Lines
Josef von Fraunhofer( ) had catalogued 475 dark spectral lines in the solar spectrum.
Fraunhofer showed that we can learn the chemical composition of the stars. Identified a spectral line of sodium in the spectrum of the Sun

4. Spectral Lines Kirchoff’s Laws of Spectra
Robert Bunsen ( ) created a burner that produced a “colorless” flame ideally suited for studying the spectra of heated substances.
Gustav Kirchoff ( ) and Bunsen designed a spectroscope that could analyze the emitted light.
Kirchoff determined that 70 of the dark lines in the solar spectrum corresponded to the 70 bright lines emitted by iron vapor.
Chemical Analysis by Spectral Observations “Spectral Fingerprint”.
A hot dense gas or hot solid object produces a continuous spectrum with no dark spectal lines
A hot, diffuse gas produces bright spectral lines (emission lines)
A cool, diffuse gas in fron of a sources of a continuous spectrum produces dark spectral lines (absorption lines) in the continuous spectrum.

5. Spectral Lines (1868) New element discovered in Sun!!
Helium discovered in solar spectrum by Pierre Janssen in 1868

6. Spectral Lines Application of Spectral Measurements
Stellar Doppler Shift
Galactic Doppler Shifts
Quasar Doppler Shifts

7. Radial Velocities

8. Spectral Lines Spectrographs
Spectroscopy
Diffraction grating equation
(n=0,1,2,…)
Resolving Power

9. Photons Photoelectric Effect
Kinetic energy of ejected electrons does not depend on intensity of light!
Increasing intensity will produce more ejected electrons.
Maximum kinetic energy of ejected electrons depends on frequency of light.
Frequency must exceed cutoff frequency before any electrons are ejected
Einstein took Planck’s assumption of quantized energy of EM waves seriously. Light consisted of massless photons whose energy was:
Einstein was awarded the Nobel Prize in 1921 for his work on the photo-electric effect

10. Photo-electric Effect

11. Photons Compton Scattering
Wikipedia entry
Arthur Holly Compton ( ) provided convincing evidence that light manifests particle-like properties in its interaction with matter by considering how (x-ray) photons can “collide” with a free electron at rest.
Conservation of energy and momentum leads to the following:
Showed that photons are massless yet carry momentum!!!
Compton Wavelength:
is the characteristic change in wavelength in the scattered photon.

12. What is matter?
Let’s Shoot stuff at it to find out…

13. Rutherford-Bohr Model of the Atom
Ernest Rutherford ( )
Rutherford Scattering
Observation consistent with scattering from a very small (10,000 times smaller radius than the atom) dense object… The nucleus

14. Models of the Atom
Models of the Atom

15. Wavelengths of Hydrogen

16. Bohr’s Semi-classical Model of the Atom
Bohr assumed for the electron proton system
to be subject to Coulomb’s Law for electric charges
Quantization of angular momentum for the electron orbit. L=nh/2
Quantization condition prevents electron from continuosly radiating away energy
Discrete energy levels for electron orbit

17. Bohr’s Semi-classical Model of the Atom

18. Bohr’s Semi-classical Model of the Atom

19. Bohr’s Semi-classical Model of the Atom

20. Bohr’s Semi-classical Model of the Atom

21. Bohr’s Semi-classical Model of the Atom

22. Bohr Hydrogen atom and spectral lines

23. Quantum Mechanics and Wave-Particle Duality
QM Tunneling
DeBroglie Matter Wave
Heisenberg Uncertainty Principle
Schroedinger Equation and QM atom
Spin and Pauli Exclusion Principle

24. DeBroglie Matter Wave

25. Quantum Mechanics and Wave-Particle Duality
Uncertainty Principle
Fourier
Wave Packets

26. Uncertainty Principle

27. Schrodinger Wave Equation and Hydrogen Atom

28. Additional Quantum Numbers and splitting of spectral lines
Normal Zeeman Effect
Can measure magnetic fields by examining spectra!!!!

29. Spin and the Pauli Exclusion Principle
No two electrons can share the same set of four quantum numbers
Chemistry….The periodic table….

30. Electron Degeneracy Pressure and White Dwarfs
Exclusion Principle for Fermions (spin-1/2 particles) and uncertainty principle provide electron degeneracy pressure that is the mechanism that prevents the further collapse of white dwarves….

31. The Complex Spectra of Atoms
Number of possible energy levels increases with number of electrons. n,l,m,…
Interactions with external magnetic fields, etc…
Complicated Spectra!!!!