Benefits And Limitations Of Niels Bohr's Model
Niels Bohr was a Danish physician interested in quantum mechanics at the start of the 20th century.
Bohrs model states that electrons orbit around the nucleus in specific shells.
Electrons change energy levels by absorbing and emitting photons.
His model only works when one electron is present
Bohrs model followed after JJ Thompson discovered the electron and ernest Rutherford discovered the nucleus.
The Planetary model stated that a positively charged nucleus sits at the middle and electrons revolve around this is rings.
Erwin Schrödinger proved that electrons can behave like waves and behaving as particles. Schrödingers model goes against what Bohr was saying by stating that electrons do not travel in specific orbit.
The Quantum Mechanical Model is known as
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Benefit and Limitations of the Bohr Model
Limitations – Could only explain the spectrum of Hydrogen. Only worked when atom has 1 electron.
Hyperfine Spectral lines- Some spectral lines were only recently discovered. These lines were with the more visible lines. His model could not explain this.
The Zeeman effect showed that Bohrs model would split if the hydrogen was excited in a magnetic field. His model couldn’t account for this.
Bohr said that the electrons were stationary in state, he couldn’t explain why.
His model combines quantum and classical physics, this is a problem as quantum physics is thought of being completely irrelevant when compared to classical physics.
Benefits - The quantum model is quite confusing and the Bohr model allows people to understand the basic principle of atomic structure.
His model shows the stability of the atom. He proved that radiation is not present due to the electrons staying in their energy levels, therefore they do not omit or take in energy.
It could foresee the energy values of an electron in revolution of the nucleus of the hydrogen
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