What the work claims
Electrons occupy discrete, stable orbits. Transitions between orbits emit quanta of discrete energy. Atomic spectra arise from these transitions. The model applies to hydrogen-like ions.
How it was done
Bohr proposed discrete electron energy levels and stable orbital motion with quantum jumps between them. He derived the Balmer series formula from this model. He applied the same principles to ionised helium to explain the Pickering series.
What holds up
The derivation of the Balmer series formula holds. The explanation of the Pickering series as ionised helium holds. The prediction of quantised emission energies holds. The model’s empirical success against competing theories holds.
What does not
The Bohr model does not apply to multi-electron atoms. It does not explain spectral line intensities or fine structure. It contains no mechanism for why orbits are stable or how jumps occur.
Why it matters beyond the lab
It established quantisation as an inescapable feature of atomic reality—not a calculational trick—paving the way for quantum mechanics. It shifted physics from classical continuity to discrete, observable jumps.
Is it worth your time
Yes. It redefined atomic structure, generated immediate testable predictions, and forced physics to accept quantisation as physical—not just mathematical.