Drawbacks of Rutherford's Theory

The video discusses the application of Newton's laws in classical mechanics, which works well for large systems like the solar system but fails for small systems like atoms. It highlights the limitations of Rutherford's atomic model, which couldn't explain atomic stability or spectra. The video explains that electrons lose energy in a discontinuous manner, leading to line spectra, contrary to continuous spectra predicted by classical theories.

Discuss the discrepancy between the expected continuous spectra and the actual line spectra observed in atoms.

What conclusions can be drawn about the energy transitions of electrons in atoms based on the observed spectra?