Drawbacks of Rutherford's Atomic Model

Rutherford proposed that electrons revolve around the nucleus in circular orbits, much like planets around the sun.

However, according to Maxwell's electromagnetic theory, any charged particle moving in a circular path undergoes acceleration. An accelerating charged particle must continuously emit (lose) energy in the form of electromagnetic radiation.

The Consequence: If an electron (a charged particle) continuously loses energy while orbiting, its orbit will keep shrinking. It will spiral inwards and eventually crash into the positive nucleus in a fraction of a second. If this were true, all matter would collapse instantly. Conclusion: Rutherford's model could not explain why atoms are stable.

1. Electronic Structure: His model did not explain anything about the arrangement or distribution of electrons around the nucleus.
2. Line Spectra: It could not explain the atomic line spectrum of elements (like Hydrogen). Since his model suggested continuous energy loss, the spectrum should have been continuous, but atoms actually produce a discrete line spectrum.

Niels Bohr solved this problem by proposing that electrons revolve only in specific, 'discrete orbits' (shells) where they do not radiate energy.