2. Chapter 30 Light Emission

3. Radio waves are produced by electrons moving up and down an antenna. Visible light is produced by electrons changing energy states in an atom.

4. 1.EXCITATION

5. u Excitation - occurs when an electron in an atom is given energy causing it to jump to a higher orbit. u This can happen through collisions or photon absorption (the photon absorption must exactly match the energy jump).

6. e-e- Here comes a nucleus With possible orbits for electrons e-e- e-e- Here comes a photon Now the atom is said to be excited because the electron is in a higher than normal orbit. In this configuration the atom is not excited. Now the atom is in a non-excited state again. It emitted a photon when it changed orbits.

7. e-e- e-e- e-e- Here comes a photon In this configuration the atom is not excited.

8. e-e- e-e- Now the atom is said to be excited because the electron is in a higher than normal orbit.

9. Now the atom is in a non-excited state again. It emitted a photon when it changed orbits. e-e- e-e- e-e-

10. u The excited atom usually de-excites in about 100 millionth of a second. u The subsequent emitted radiation has an energy that matches that of the orbital change in the atom. u Video - Atomic Excitation

11. u This emitted radiation gives the characteristic colors of the element involved. u The atoms do not “wear out.” u Demo - Flame Colors

12. u Classical explanation fails - it says there should be radiation even when there has been no change in energy levels. u The electron should spiral into the nucleus - the ultraviolet catastrophe. u E = hf (h = Planck’s constant)

13. Emission Spectra Continuous Emission Spectrum Prism Photographic Film Slit White Light Source

14. Emission Spectra of Hydrogen Prism Photographic Film Film Slit Low Density Glowing Hydrogen Gas Discrete Emission Spectrum

15. u Slide - Spectra of Some Gases u Demo - Spectra of a Discharge Tube Gas

16. 2.INCANDESCENCE u Demo - Spectrum of Incandescent Bulb u Blue hot is hotter than white hot which is hotter than red hot. u White light - all colors in the visible are present. u Electron transitions occur not only in the parent atom but in adjacent atoms as well.

17. 0.0 0.1 0.2 0 Relative Energy 0.0 0.1 0.2 05001000 Wavelength (nm) Relative Energy (measured in Kelvins) u Brightness versus color curve for different temperatures Peak Frequency

18. Frequency Relative Energy (measured in Kelvins) u Brightness versus color curve for different temperatures Peak Frequency

19. Discrete Absorption Spectrum Absorption Spectra of Hydrogen Prism Photographic Film Film Slit White Light Source Discrete Emission Spectrum Hydrogen Gas

20. Absorption Spectra u Frequencies of light that represent the correct energy jumps in the atom will be absorbed. u When the atom de-excites, it emits the same kinds of frequencies it absorbed. u However, this emission can be in any direction.

21. u Close inspection of the absorption spectrum of the sun reveals missing lines known as Fraunhofer lines. u In 1868 a pattern of lines was observed in the solar spectrum that represented an element that had not been found on earth. It was Helium -named for Helios, the sun.

22. u Doppler shifts are observed in the spectra of stars. u If a star is approaching, its spectra will be blue shifted. u If a star is moving away, its spectra will be red shifted. Most spectra are red shifted indicating that on the average the universe is expanding.

23. 3.FLUORESCENCE u Some materials that are excited by UV emit visible. u These materials are referred to as fluorescent materials.

24. Fluorescent Lamps u Primary excitation - electron collisions with low pressure Hg vapor, UV given off u Secondary excitation - UV photons absorbed by phosphors. Phosphors fluoresce emitting visible light. u Remember that the visible light from the excited mercury vapor is also emitted.

25. 4.PHOSPHORESCENCE u Electrons get "stuck" in excited states in the atoms and de-excitation occurs at different times for different atoms. u A continuous glow occurs for some time. u Demo - Fluorescent & Phosphorescent Objects (including helicopter and “Starry, Starry Night”) “Starry, Starry Night”) u Bioluminescence

26. Light Amplification by Stimulated Emission of Radiation E 5.LASERS LA S R

27. Lasers produce coherent light. Coherent light is light with the same frequency and the same phase. Demo - Making Laser Beam Visible

28. u Early model - ruby crystal doped with Cr u Slide - Helium-Neon Laser u Video - Lasers u Today's models include gas (He-Ne), glass, chemical, liquid, semiconductor, and x-ray.

29. Applications: u Surveying u Surgery u Communication u Computer storage u Pollution detection u 3-d TV (holograms) u Thermonuclear fusion - heat H 2 pellets

30. Chapter 30 Review Questions

31. In fluorescence which has the higher energy, radiation absorbed or the radiation of an emitted photon? In fluorescence which has the higher energy, the radiation absorbed or the radiation of an emitted photon? (a) absorbed (b) emitted (c) they both have the same energy (a) absorbed

32. What type of spectrum would you expect to obtain if white light is shined through sodium vapor? (a) an emission spectrum of sodium (b) an absorption spectrum of sodium (c) a continuous spectrum (b) an absorption spectrum of sodium

33. What causes laser light to have all of its waves moving in the same direction? (a) the mirrors in the laser (b) the stimulated emission of the atoms to radiate in the same direction (c) atoms are lined-up in the crystal so that they emit light only in one direction (a) the mirrors in the laser

34. Each element gives off a characteristic color when it undergoes the excitation and de- excitation process. The color is due to (a) fluorescence (b) secondary emission (c) electrons moving to lower energy states (d) refraction of light through the characteristic gas (e) electrons giving off Cerenkov radiation (c) electrons moving to lower energy states

35. Which phenomenon has electrons getting "stuck" in excited states? (a) incandescence (b) fluorescence (c) phosphorescence