The main flaws of Bohr's atomic model include its inability to explain the fine structure of spectral lines, the inability to explain the Zeeman effect, and the failure to predict the relative intensities of spectral lines. Additionally, the model does not account for the wave-like behavior of electrons.
Bohr's atomic model was the first to successfully explain the stability of atoms and the discrete nature of atomic spectra. It also introduced the concept of quantized energy levels, which paved the way for the development of quantum mechanics.
The discovery of subatomic particles, such as the electron, proton, and neutron, provided evidence that the atom is not a simple structure as proposed by Bohr. The wave-particle duality of electrons and the Heisenberg uncertainty principle also contradicted the rigid orbits of electrons in Bohr's model.
Quantum mechanics, through the Schrödinger equation, provides a more accurate description of the behavior of electrons in atoms. It considers the wave-like nature of electrons and allows for the calculation of the probability of finding an electron in a particular location around the nucleus. This addresses the limitations of Bohr's model in explaining the distribution of electrons in atoms.
Yes, some aspects of Bohr's model are still applicable today. For example, the concept of quantized energy levels is still used to explain the stability of atoms. The model also serves as a simplified representation of the atom, which is still useful in introductory chemistry courses. However, it has been replaced by more accurate models, such as the quantum mechanical model, in advanced science fields.