Final answer:
According to classical physics, electrons in Rutherford's nuclear model should theoretically spiral into the nucleus as they lose energy, leading to the collapse of the atom, which conflicts with the stability observed in atoms.
Step-by-step explanation:
According to classical physics, as described by Maxwell's theory of electromagnetic radiation, any charged particle that changes its speed or direction of motion, such as an electron in orbit around a nucleus, must emit energy. This continuous change in direction of an electron circling the nucleus in Rutherford's nuclear model of the atom should result in a steady emission of energy. Consequently, as electrons lose energy, they should theoretically spiral into the nucleus, leading to the collapse of the atom in an extremely short period. This contradicts the observed stability of atoms, indicating that classical physics cannot fully explain the behavior of electrons in an atom.
Rutherford's model was initially successful in describing his experimental findings with alpha particles and gold foil, suggesting most of the atom is empty space. However, the model could not account for the stability of atoms nor the discrete spectral lines observed in atomic emissions. The later development of the Bohr model and quantum mechanics provided a more complete understanding of atomic structure, incorporating quantized orbits for electrons and explaining the stability and emission spectra of atoms.