De Broglie & Bohr: Electron Kinetic Energy Formula

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SUMMARY

The discussion centers on the relationship between the electron's kinetic energy and its wavelength in the context of the Bohr model of the hydrogen atom. The formula presented, 2πr = n(λ), connects the radius of the electron's orbit to its wavelength. Substituting the wavelength with h/p (where h is Planck's constant and p is momentum) allows for the derivation of the electron's kinetic energy, aligning with Bohr's energy formula. The conversation highlights the historical significance of Bohr's model while acknowledging its limitations compared to Schrödinger's quantum mechanics.

PREREQUISITES
  • Understanding of the Bohr model of the hydrogen atom
  • Familiarity with the concepts of wavelength and momentum in quantum mechanics
  • Knowledge of Planck's constant and its role in quantum physics
  • Basic grasp of Schrödinger's wave mechanics
NEXT STEPS
  • Study the derivation of kinetic energy from the de Broglie wavelength
  • Explore the differences between the Bohr model and Schrödinger's quantum mechanics
  • Investigate the implications of the wave-particle duality of electrons
  • Learn about the limitations of the Bohr model in explaining atomic structure
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Students of physics, educators teaching quantum mechanics, and researchers interested in atomic theory and its historical development.

matsorz
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An electron around a hydrogen-atom, with radius r and length of circle a whole number, n, times wavelength. This implies that
2*3,14*r=n*(wavelength)

I have read someplace that if you substitute the wavelength with h/p, you can find the kinetic energy of an electron, which is the same as Bohrs formula for energy.

Anyone here that can help?:)
 
Physics news on Phys.org
Bohr's discussion of the atom was a predecessor of Schrödinger quantum mechanics. It happened to give the right energy levels for hydrogen, but is wrong in other details, for example the multiplicity of the levels. Unfortunate that it is still taught.
 

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