How did the Bohr model differ from the Rutherford model?

The Rutherford model and the Bohr atomic model both describe an atom with a dense, positively charged nucleus surrounded by electrons. However, they differ fundamentally in their treatment of electron motion and atomic stability.123

• Stability and Classical Physics: In the Rutherford model, electrons revolve in orbits of arbitrary radii, similar to planets orbiting the Sun. According to classical electromagnetic theory, such electrons should continuously emit radiation, lose energy, and spiral into the nucleus, rendering the atom unstable.1423
• Quantization: Niels Bohr addressed this by incorporating quantum theory. He postulated that electrons can only occupy specific, "allowed" orbits of fixed size and energy.453
• Energy Transitions: Unlike the Rutherford model, where orbits are arbitrary, the Bohr model dictates that electrons do not radiate energy while in these stationary states. Radiation (light) is emitted or absorbed only when an electron makes a "quantum leap" between these discrete energy levels.435

By restricting electrons to quantized orbits, Bohr successfully explained the stability of atoms and the discrete spectral lines observed in hydrogen.243