1 / 35

Chapter 29

Chapter 29. 0. Atoms and Molecules. 29 Atoms and Molecules. Slide 29-2. Slide 29-3. Slide 29-4. Slide 29-5. Spectroscopy. Slide 29-10. Continuous Spectra and Blackbody Radiation. Slide 29-11. Discrete Spectra of the Elements. Slide 29-12. The Hydrogen Spectrum.

helmut
Download Presentation

Chapter 29

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chapter 29 0 Atoms and Molecules

  2. 29Atoms and Molecules Slide 29-2

  3. Slide 29-3

  4. Slide 29-4

  5. Slide 29-5

  6. Spectroscopy Slide 29-10

  7. Continuous Spectra and Blackbody Radiation Slide 29-11

  8. Discrete Spectra of the Elements Slide 29-12

  9. The Hydrogen Spectrum Wavelengths of visible lines in the hydrogen spectrum Balmer’s formula Slide 29-13

  10. Rutherford’s Experiment Slide 29-14

  11. Using the Nuclear Model Ionization The nucleus Isotopes Slide 29-15

  12. Bohr’s Model of Atomic Quantization Slide 29-16

  13. Bohr’s Model of Atomic Quantization (cont’d) Slide 29-17

  14. Frequencies of Photons Emitted in Electron Transitions Slide 29-18

  15. Representing Atomic States Energy-level diagram Slide 29-19

  16. The Bohr Hydrogen Atom Slide 29-20

  17. Energy-Level Diagram of the Hydrogen Atom Slide 29-21

  18. The Quantum-Mechanical Hydrogen Atom Schrödinger found that the energy of the hydrogen atom is given by the same expression found by Bohr, or The integer n is called the principal quantum number. The angular momentum L of the electron’s orbit must be one of the values The integerl is called the orbital quantum number. Slide 29-22

  19. The Quantum-Mechanical Hydrogen Atom (cont’d) The plane of the electron’s orbit can be tilted, but only at certain discrete angles. Each allowed angle is characterized by a quantum number m, which must be one of the values The integer m is called the magnetic quantum number because it becomes important when the atom is placed in a magnetic field. The electron’s spin can point only up or down. These two orientations are described by the spin quantum numberms, which must be one of the values Slide 29-23

  20. Energy and Angular Momentum of the Hydrogen Atom Slide 29-24

  21. Energy Levels in Multielectron Atoms Hydrogen atom Multielectron atom Slide 29-25

  22. Excited States and the Pauli Exclusion Principle Helium atom Lithium atom Slide 29-26

  23. The Periodic Table Slide 29-27

  24. Building Up the Periodic Table Slide 29-28

  25. Excitation by Absorption and Collision Slide 29-29

  26. Emission Spectra Slide 29-30

  27. Checking Understanding • Suppose that an atomic excited state decays to the ground state by emission of two photons, with energies E1 and E2. Is it possible for that excited state to decay to the ground state by emission of a single photon with energy E1 + E2? • It is always possible, for every atom. • It is never possible, for any atom. • It is always possible for hydrogen atoms, but is unlikely for other atoms. Slide 29-31

  28. Answer • Suppose that an atomic excited state decays to the ground state by emission of two photons, with energies E1 and E2. Is it possible for that excited state to decay to the ground state by emission of a single photon with energy E1 + E2? • It is always possible, for every atom. • It is never possible, for any atom. • It is always possible for hydrogen atoms, but is unlikely for other atoms. Slide 29-32

  29. Molecules Slide 29-33

  30. Fluorescence Slide 29-34

  31. Checking Understanding • Which of the following is not a possible fluorescence process? • Absorption of red light and emission of green light • Absorption of ultraviolet light and emission of infrared light • Absorption of ultraviolet light and emission of green light • Absorption of blue light and emission of red light Slide 29-35

  32. Answer • Which of the following is not a possible fluorescence process? • Absorption of red light and emission of green light • Absorption of ultraviolet light and emission of infrared light • Absorption of ultraviolet light and emission of green light • Absorption of blue light and emission of red light Slide 29-36

  33. Stimulated Emission and Lasers Slide 29-37

  34. Photon Amplification Slide 29-38

  35. A Helium-Neon Laser Slide 29-39

More Related