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Exploring the Bohr Model of Hydrogen Atom: An Introduction to Quantum Energy Levels

Understand the Bohr Model's postulates, spectrum transitions, and deBroglie Equation. Delve into absorption/emission spectra and energy quantization in hydrogen atoms. Learn how matter waves manifest in electron behavior within atoms.

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Exploring the Bohr Model of Hydrogen Atom: An Introduction to Quantum Energy Levels

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  1. October 23, 2009 THE BOHR MODEL OF THE ATOM

  2. The Bohr Model of Hydrogen Atom • Light absorbed or emitted is from electrons moving between energy levels • Only certain energies are observed • Therefore, only certain energy levels exist • Energy levels are Quantized

  3. Energy Adsorption/Emission

  4. Absorption and Emission Spectra

  5. Hydrogen Energy Levels Constant = Rhc = 2.18 x 10-18 J R = Rydberg constant = 1.0974 x 107 m-1 h = Planck’s constant = 6.626 x 10-34 Js c= velocity of light in vacuum = 3.0 x 108 m/s

  6. Each line corresponds to a transition: Example: n=3  n = 2

  7. Explanation of line spectra Balmer series

  8. The emission line with the shortest wavelength is: • 1 • 2 • 3 • 4 • 5

  9. The emission line with the longest wavelength is: • 1 • 2 • 3 • 4 • 5

  10. The emission line with the highest energy is: • 1 • 2 • 3 • 4 • 5

  11. The absorption line with the shortest wavelength is: • 1 • 2 • 3 • 4 • 5

  12. The absorption line with the lowest energy is: • 1 • 2 • 3 • 4 • 5

  13. A Revolutionary Idea: Matter Waves • All matter acts as particles and as waves. • Macroscopic objects have tiny waves- not observed. • Wave nature only becomes apparent when object is VERY light • For electrons in atoms, wave properties are important. • deBroglie Equation:

  14. Matter waves- Examples Macroscopic object: 200 g rock travelling at 20 m/s has a wavelength: Electron inside an atom, moving at 40% of the speed of light (0.4 x 3x108m/s):

  15. Can see matter waves in experiments

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