Limitations of Bohr’s Atomic Model

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Limitations of Bohr’s Atomic Model-


Before you go through this article, make sure that you have gone through the previous article on Bohr’s Atomic Model.


Although Bohr’s theory could successfully explain the spectrum of hydrogen atom, yet it had the following shortcomings-




Bohr’s theory is applicable only to hydrogen-like single electron atoms and fails in the case of atoms with two or more electrons.




It does not explain why only circular orbits should be chosen when elliptical orbits are also possible.




An electron exhibit wave properties also, so orbits of electrons cannot be exactly defined as in Bohr’s theory.




Bohr’s theory does not tell anything about the relative intensities of the various spectral lines. Bohr’s theory predicts only the frequency of these lines.




It does not explain the further splitting of spectral lines in a magnetic field (Zeeman effect) or in an electric field (stark effect).




Bohr’s theory determines the position and momentum of the electron simultaneously with no uncertainty, thus violates the Heisenberg’s uncertainty principle.


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