Limitations of Bohr's Model

Chemistry

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Limitations of Bohr's model

  • It could not explain the line spectrum of multi electron atoms.
  • This model failed to explain the effect of magnetic field on the spectra of atoms (Zeeman effect).
  • The effect of electric field on the spectra could not be explained by Bohr's model (Stark effect).
  • The shapes of molecules arising out of directional bonding could not be explained.
  • The dual nature of electrons (both as wave and particle) and the path of motion of the electron in well defined orbits were not correct.

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Failure of Bohr's model

According to Bohr's model, the electrons are moving in fixed circular paths. The path can be defined only if the velocity and position of the electron are known exactly at the same time which is contradicted by Heisenberg uncertainty principle.

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