Classical physics made Rutherford's atom collapse, so Bohr declared that only certain orbits were allowed.
Year
1913
People
Niels Bohr, Ernest Rutherford, Johann Balmer, Max Planck
Ideas at stake
Bohr model, energy level, atomic spectrum, quantum transition
Rutherford’s atom could not survive
An electron orbiting a positive nucleus should radiate energy, spiral inward, and destroy the atom. Real atoms remain stable and emit only specific spectral frequencies.
The young Niels Bohr put Planck’s quantum directly into Rutherford’s atom. He allowed electrons to occupy only selected stationary states, even though classical physics could not explain the rule.
The fixed differences explained hydrogen’s fixed spectral lines. Bohr could not explain why only these states existed or why stationary electrons did not radiate. The model also struggled with larger atoms.
It was scaffolding, not a finished building. Its achievement was to admit that nature might skip the intermediate states demanded by classical imagination.
