Both Rutherford's and Bohr's models have electrons orbiting the nucleus. Why did Rutherford's model fail to explain atomic stability, while Bohr's model succeeded?

Rutherford's model stated that electrons revolve around the nucleus like planets revolve around the Sun. However, according to this model, a moving electron should continuously lose energy while revolving around the nucleus. As a result, the electron would gradually spiral inward and finally fall into the nucleus, making the atom unstable. Rutherford's model could not explain why atoms remain stable.

Bohr overcame this problem by proposing that electrons revolve around the nucleus only in certain fixed orbits or energy levels having definite energy. In these fixed orbits, electrons do not lose energy while moving around the nucleus. Therefore, they neither fall into the nucleus nor fly away from the atom. In this way, Bohr's model successfully explained the stability of atoms.