Bohr's atomic model differed from Rutherford's because it explained that

Bohr's model explained that there were electrons that orbited the nucleus quantised orbits

Bohr's atomic model differed from Rutherford's because it explained that electrons exist in specified energy levels surrounding the nucleus (option A)

Explanation:

Rutherford's atomic model was based on a central nucleus surrounded by electrons, as in the solar system. But this model had a contradiction corresponding to the fundamental laws of electrodynamics: considering that negatively charged electrons revolve around the nucleus they should emit electromagnetic radiation, with the consequent loss of energy. This radiation would consume energy that would cause electrons to collapse with the nucleus. Therefore, this model could not explain the stability of the atom.

Therefore, Bohr proposed that the electrons were at a certain distance from the nucleus, rotating in circles. Each circle or orbit was provided with a predetermined amount of energy. If an electron jumped into an orbit of lower energy, it would emit electromagnetic radiation. In short, Bohr's model solved the problem of the Rutherford model by indicating that electrons orbit around the nucleus but in certain orbits allowed with a specific energy. These defined orbits were referred to as layers of energy or energy levels. In other words, the energy of an electron within an atom is not continuous, but "quantified." Electrons can only gain or lose energy by jumping from one permitted orbit to another and, when this happens, it would absorb or emit electromagnetic radiation in the process.

Then, Bohr's atomic model differed from Rutherford's because it explained that electrons exist in specified energy levels surrounding the nucleus (option A)