Limitations of Bohr Model:

Bohr's atomic model is an effective model for understanding the structure of an atom, but it has certain limitations.

1. Only applicable to Hydrogen-like atoms:
Bohr's atomic model is only applicable to hydrogen-like atoms, i.e., atoms containing only one electron. It does not apply to atoms with more than one electron, such as helium.

2. The model is limited in its ability to explain the chemical properties of elements:
The model does not explain the chemical properties of elements, such as how they interact with other elements to form compounds.

3. The model is limited in its ability to explain the spectra of atoms:
The model fails to explain the fine structure of the spectral lines of atoms, which is caused by the interaction between the electron spins and the magnetic field.

4. The model violates the Heisenberg uncertainty principle:
The Bohr model violates the Heisenberg uncertainty principle, which states that it is impossible to simultaneously determine both the position and momentum of an electron.

5. The model does not account for the relativistic effects:
The Bohr model does not account for the relativistic effects that arise when an electron moves at a high speed, which is the case for electrons in atoms with a large atomic number.

6. The model does not account for the electron-electron repulsion:
The Bohr model does not account for the electron-electron repulsion, which becomes significant in atoms with more than one electron.

7. The model does not explain the Zeeman effect:
The Bohr model does not explain the Zeeman effect, which is the splitting of spectral lines in a magnetic field.

Conclusion:

In conclusion, although the Bohr model was a significant step forward in understanding the structure of an atom, it has certain limitations that make it an incomplete model. The development of quantum mechanics in the 1920s and 1930s provided a more complete and accurate description of the structure of an atom.