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Understanding Quantum Mechanics: Particles, Waves, and the Nature of Light

Dive into the intricate world of quantum mechanics as we explore the dual nature of particles and waves in Chapter 37. This segment focuses on the concept of quantization, highlighting how matter is composed of atoms with tightly packed protons and neutrons, and electrons that orbit with quantized energy levels. We discuss the revolutionary idea that light behaves as particles known as photons, governed by Planck’s constant. Key experiments like the Davison-Germer experiment illustrate wave behavior in electrons, helping us understand emission and absorption spectra.

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Understanding Quantum Mechanics: Particles, Waves, and the Nature of Light

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  1. quantization part 2 –particles as waves ch 37

  2. The world – a) matter - atoms nucleus of tightly packed protons and neutrons. Protons-positive charge electrons orbiting negative charge charges come in bits e=1.602 x 10-19C “quantized”

  3. The World: LightWe have a crazy new idea • LIGHT IS A PARTICLE …. • These things are called photons h a constant – Plank’s constant h=6.625 x 10-34 J-s 1eV=1.602 x 10-19J

  4. How is light made?absorbed?idea!

  5. Trouble: Why discreet?? Emission spectrum Absorption spectrum Like a Merry go round that can only go 1mph, 3mph, 5mph and NOTHING IN BETWEEN

  6. Why do we exist at all????

  7. Crazy possibility #2 – Bohr: electrons are waves here is what the book says (It doesn’t help me much) Think of a bugle now take this in a circle

  8. Bohr 1 electron as wave in a circle 2πr=nλelectron

  9. So only certain orbitals are OK, and NOTHING in between. We require 2πr=nλelectron (whatever λelectron is…) States are stationary For orbitals in between, the electron goes around and interferes destructively with itself. Quantization of orbitals 2πr=nλelectron

  10. Starting Stuff Relativity Einstein E=hf Waves c=fλ Mechanics F=ma circular motion _ E&M Now lets see if we can figure out the energies of these orbitals 2πr=nλelectron

  11. But what is λelectron??? • back to light as particle • Relativity • mass of light?? mass of photon?? =0 • E=pc=hf=hc/λ SO p=h/λ or λ=h/p • Now to electron as wave • λelectron=h/pelectron

  12. Now lets see if we can figure out the energies of these orbitals (Hydrogen) here we get • F=ma • 2πr=nλe from here we get L=mvr=nh/2π the quantization of angular momentum

  13. quantization of the energy levels • We get

  14. The Rydberg constant and Bohr radius aB~ size of atom ~10-10m

  15. quantized energy, radius, velocity

  16. What about the spectral lines? Emission spectrum Absorption spectrum Balmer forumla

  17. Only photons with certain energies allowed! bohr photons

  18. Energy of the photonsthe Balmer formula

  19. Some names for hydrogen m

  20. Binding energy, ionization energy 13.6/n2 eV 13.6 eV

  21. The Davison Germer Experiment • If electrons are really waves, they should diffract. • The Davison Germer Experiment

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