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Why did Bohr's model work for 1 electron systems?

  1. Oct 24, 2012 #1
    If I am not mistaken the Bohr model had 3 main problems: the assumption that the electron moves in fixed orbits, the angular momentum assumption's violation of the Heisenberg uncertainty principle, and finally the restriction of the validity of the model for only 1-electron systems ( i.e. hydrogen, He +1, ect ). Why was it that Bohr's model only worked for 1-electron systems and failed when applied to poly-electron systems? Please be as thorough as possible. Thank you for all your help.
  2. jcsd
  3. Oct 24, 2012 #2
    nothing stops multiple electrons from being in the same quantum state.
  4. Oct 25, 2012 #3


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    Nothing but Pauli exclusion principle?
  5. Oct 25, 2012 #4


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    What happens when you put two negatively charged object close to each other?
  6. Oct 25, 2012 #5
    that is not part of the Bohr theory =)
  7. Oct 25, 2012 #6
    As Borek has already alluded to, the answer is that systems with more than one electron have a much more complicated charge interaction.

    As an interesting side note, the context of Bohr's work is misrepresented when it's taught at schools. At the time he published his model (1913) there was no concept of a de Broglie wavelength. The idea of electron orbits as standing waves wasn't introduced until de Broglie published his thesis in 1924.
  8. Oct 25, 2012 #7


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    It does not even work for all one electron systems e.g. H2+.
  9. Oct 25, 2012 #8


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    Arnold Sommerfeld cured two shortcomings: the plane motion was generalized to elliptic orbits and moreover in agreement with the specially relativistic dynamics.
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