What is the primary reason Rutherford’s model could not explain the line spectra of atoms?
**Rutherford's nuclear model** atom has small massive positively charged nucleus with electrons orbiting, size ratio atomic to nuclear ~10⁵, nucleus ~10⁻¹⁵ m atom ~10⁻¹⁰ m, most alpha particles with large impact parameter pass undeflected, small fraction >90° scatter from close approach, centripetal force provided by Coulomb attraction k Z e²/r², fails to explain stability because accelerating charge should radiate and collapse. Rutherford’s model lacks quantized energy levels, predicting continuous radiation as electrons accelerate, not discrete spectral lines. Using E_n = -13.6/n² eV, r_n =
Ref: NCERT > Physics Book > Atoms and Nuclei > Atomic Models - Rutherford, Thomson and Bohr