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Photon Theory of Light: Unveiling Wave-Particle Duality

Explore the fascinating concepts of Photon Theory of Light and Wave-Particle Duality in this lecture. Delve into topics such as the Photoelectric Effect, Energy-Mass-Momentum of Photons, Wave Nature of Matter, and Early Models of the Atom. Understand key principles like de Broglie’s Hypothesis and the Atomic Spectra. Embrace the dual nature of light as both wave and particle, and discover the intriguing behavior of matter as waves. Gain insight into crucial calculations and examples related to photon energy and electron wavelengths, enhancing your understanding of this essential chapter in quantum theory.

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Photon Theory of Light: Unveiling Wave-Particle Duality

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  1. Lecture 11a Photon Theory of Light & Wave Particle Duality

  2. Chapter 37Early Quantum Theory and Models of the Atom

  3. Units of Chapter 37 • Photon Theory of Light and the Photoelectric • Effect • Energy, Mass, and Momentum of a Photon • Wave–Particle Duality • Wave Nature of Matter • Early Models of the Atom • Atomic Spectra: Key to the Structure of the Atom • de Broglie’s Hypothesis Applied to Atoms

  4. 37-2 Photon Theory of Light and the Photoelectric Effect . Einstein suggested that, given the success of Planck’s theory, light must be emitted in small energy packets: These tiny packets, or particles, are called photons.

  5. 37-2 Photon Theory of Light and the Photoelectric Effect The photoelectric effect: if light strikes a metal, electrons are emitted. The effect does not occur if the frequency of the light is too low; the kinetic energy of the electrons increases with frequency.

  6. 37-2 Photon Theory of Light and the Photoelectric Effect • If light is a wave, theory predicts: • Number of electrons and their energy should increase with intensity. • Frequency would not matter.

  7. 37-2 Photon Theory of Light and the Photoelectric Effect • If light is particles, theory predicts: • Increasing intensity increases number of electrons but not energy. • Above a minimum energy required to break atomic bond, kinetic energy will increase linearly with frequency. (Kmax = hf – Wo) • There is a cutoff frequency (fo) below which no electrons will be emitted, regardless of intensity. (hfo = Wo)

  8. 37-2 Photon Theory of Light and the Photoelectric Effect The particle theory assumes that an electron absorbs a single photon. Plotting the kinetic energy vs. frequency: This shows clear agreement with the photon theory, and not with wave theory.

  9. 37-2 Photon Theory of Light and the Photoelectric Effect Example 37-3: Photon energy. Calculate the energy of a photon of blue light, λ = 450 nm in air (or vacuum).

  10. 37-2 Photon Theory of Light and the Photoelectric Effect Example 37-5: Photoelectron speed and energy. What are the kinetic energy and the speed of an electron ejected from a sodium surface whose work function is W0 = 2.28 eV when illuminated by light of wavelength (a) 410 nm and (b) 550 nm?

  11. 37-3 Energy, Mass, and Momentum of a Photon Clearly, a photon must travel at the speed of light. Looking at the relativistic equation for momentum, it is clear that this can only happen if its rest mass is zero. We already know that the energy is hf; we can put this in the relativistic energy-momentum relation and find the momentum:

  12. 37-6 Wave-Particle Duality; the Principle of Complementarity We have phenomena such as diffraction and interference that show that light is a wave, and phenomena such as the photoelectric effect and the Compton effect that show that it is a particle. Which is it? This question has no answer; we must accept the dual wave–particle nature of light.

  13. 37-6 Wave–Particle Duality; the Principle of Complementarity The principle of complementarity states that both the wave and particle aspects of light are fundamental to its nature. Indeed, waves and particles are just our interpretations of how light behaves.

  14. 37-7 Wave Nature of Matter . Just as light sometimes behaves like a particle, matter sometimes behaves like a wave. The wavelength of a particle of matter is This wavelength is extraordinarily small.

  15. 37-7 Wave Nature of Matter Example 37-10: Wavelength of a ball. Calculate the de Broglie wavelength of a 0.20-kg ball moving with a speed of 15 m/s.

  16. 37-7 Wave Nature of Matter Example 37-11: Wavelength of an electron. Determine the wavelength of an electron that has been accelerated through a potential difference of 100 V.

  17. 37-7 Wave Nature of Matter The wave nature of matter becomes more important for very light particles such as the electron. Electron wavelengths can easily be on the order of 10-10 m; electrons can be diffracted by crystals just as X-rays can.

  18. Summary of Chapter 37 . • Light can be considered to consist of photons, each of energy • Photoelectric effect: incident photons knock electrons out of material.

  19. Summary of Chapter 37 . • Wave–particle duality – both light and matter have both wave and particle properties. • Wavelength of an object: • Principle of complementarity: both wave and particle properties are necessary for complete understanding.

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