Limitations of Bhor's Model
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Limitations of Bohr's model of the atom
Bohr's biggest contribution in his model was to introduce quantum principles to classical physics, but his model had a few limitations:
Spectra of Large atoms:
The Bohr model could only successfully explain the hydrogen spectrum.
It could NOT accurately calculate the spectral lines of larger atoms.
The model only worked for hydrogen-like atoms
That is, if the atom had only one electron.
Relative Spectra Intensity
Bohr's model could not explain why the intensity of the spectra lines were NOT all equal.
This suggests that some transitions are favoured more than others.
Hyperfine spectral lines
With better equipment and careful observation, it was found that there were previously undiscovered spectral lines
These were named Hyperfine lines and they accompanied the other more visible lines.
Bohr's model could not explain why this was the case due to the lack of equipment and development in quantum physics.
The reason for these lines is actually because of a hyperfine structure of atoms.
Solved through developments into Matrix Mechanics
The Zeeman effect
It was found that, when hydrogen gas was excited in a magnetic field, the produced emission spectrum was split.
Bohr's model could not account for this
Solved by accounting for the existence of a tiny magnetic moment of each electron.
Stationary states
Although Bohr stated that electrons were in stationary states, he could not explain why.
The reason is covered later
Mixture of Sciences
The Bohr model was a mixture of quantum and classical physics
This is an issue because it was thought that quantum physics was completely irrelevant and different to classical physics.
Bohr's biggest contribution in his model was to introduce quantum principles to classical physics, but his model had a few limitations:
Spectra of Large atoms:
The Bohr model could only successfully explain the hydrogen spectrum.
It could NOT accurately calculate the spectral lines of larger atoms.
The model only worked for hydrogen-like atoms
That is, if the atom had only one electron.
Relative Spectra Intensity
Bohr's model could not explain why the intensity of the spectra lines were NOT all equal.
This suggests that some transitions are favoured more than others.
Hyperfine spectral lines
With better equipment and careful observation, it was found that there were previously undiscovered spectral lines
These were named Hyperfine lines and they accompanied the other more visible lines.
Bohr's model could not explain why this was the case due to the lack of equipment and development in quantum physics.
The reason for these lines is actually because of a hyperfine structure of atoms.
Solved through developments into Matrix Mechanics
The Zeeman effect
It was found that, when hydrogen gas was excited in a magnetic field, the produced emission spectrum was split.
Bohr's model could not account for this
Solved by accounting for the existence of a tiny magnetic moment of each electron.
Stationary states
Although Bohr stated that electrons were in stationary states, he could not explain why.
The reason is covered later
Mixture of Sciences
The Bohr model was a mixture of quantum and classical physics
This is an issue because it was thought that quantum physics was completely irrelevant and different to classical physics.
sourishdgreat1:
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→ Bohr explained the Hydrogen atom model... But fails for higher elements even for Helium which has 2 electrons.
→ He failed to explain two closely spaced lines.
→ He also failed to explain splitting of spectral lines.
In presence of Electric and Magnetic field.
Spectrum in Electric field = Stark effect.
Spectrum in Magnetic Field = Zeeman effect.
→ He could not explain the formation of molecules from atoms by chemical bonding.
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