Drawbacks of Bohr model ?

Question

Accepted Answer

Bohr treated electrons as particles where according to de Broglie's hypothesis, having a very low mass, electron also exhibits wave nature. 2. Bohr's model was adequate only for nucleus having only one electron e.g. Hydrogen, He+1, Li+2 etc. Bohr's model could not explain the spectra of multi-electronic atoms.

Answer

The drawbacks are :-
1)Bohr's model couldn't explain the spectra of complex atoms of multi electronic systems.
2)It couldn't explain the difference in the intensities of emitted radiations.
3)It could only partially explain hydrogen atom. it doesn't explain the fine structure of spectral lines in the hydrogen atom.
4)It is silent about the wave properties of electrons.
5)Bohr's model does not explain why the orbits are circular while elliptical orbits are also possible..

Answer

Drawbacks of Bohr Model
The Bohr model of the atom, proposed by Niels Bohr in 1913, was a significant advancement in understanding atomic structure. However, it also had several drawbacks that limited its applicability in certain situations.

1. Failure to explain complex atoms:
- One of the major drawbacks of the Bohr model is its inability to explain the spectral lines of atoms with more than one electron.
- While the model was successful in explaining the hydrogen spectrum, it failed to accurately predict the spectral lines of atoms with multiple electrons.

2. Lack of explanation for electron motion:
- The Bohr model suggested that electrons moved in fixed orbits around the nucleus, similar to planets orbiting the sun.
- However, this concept of fixed orbits contradicted the principles of quantum mechanics, which describe electrons as having wave-like properties and existing in probability clouds around the nucleus.

3. Ignoring electron-electron repulsion:
- The Bohr model did not take into account the repulsion between electrons in the same orbit, known as electron-electron repulsion.
- This repulsion plays a significant role in determining the stability and energy levels of atoms, which the Bohr model failed to address.

4. Inaccurate prediction of fine structure:
- When applied to atoms with multiple electrons, the Bohr model inaccurately predicted the fine structure of spectral lines.
- This discrepancy between the model's predictions and experimental observations highlighted its limitations in describing the behavior of complex atoms.
In conclusion, while the Bohr model was a groundbreaking theory that revolutionized our understanding of atomic structure, it had several drawbacks that limited its accuracy and applicability to complex systems. Subsequent developments in quantum mechanics, such as the Schrödinger equation, have provided a more comprehensive and accurate description of atomic behavior.

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