Limitations of Bohr’s Atomic Model-
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Although Bohr’s theory could successfully explain the spectrum of hydrogen atom, yet it had the following shortcomings-
Limitation-01:
Bohr’s theory is applicable only to hydrogen-like single electron atoms and fails in the case of atoms with two or more electrons.
Limitation-02:
It does not explain why only circular orbits should be chosen when elliptical orbits are also possible.
Limitation-03:
An electron exhibit wave properties also, so orbits of electrons cannot be exactly defined as in Bohr’s theory.
Limitation-04:
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.
Limitation-05:
It does not explain the further splitting of spectral lines in a magnetic field (Zeeman effect) or in an electric field (stark effect).
Limitation-06:
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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