This also states that these shells have different energies and are spherical in shape. But Bohr model is more advanced than the Rutherford model because it says that, the electrons are always traveling in specific shells or orbits around the nucleus. Side by Side Comparison – Bohr vs Quantum Model in Tabular FormĪs mentioned above, the Bohr model is a modification of the Rutherford model since the Bohr model explains the structure of the atom as composed of a nucleus surrounded by electrons. The key difference between Bohr and quantum model is that Bohr model states that electrons behave as particles whereas quantum model explains that the electron has both particle and wave behavior. Quantum model is the modern model of an atom. Bohr model was proposed by Niels Bohr in 1915. ![]() Bohr model is also called Rutherford-Bohr model because it is a modification of the Rutherford model. Bohr's model and postulates do not explain this phenomenon.The Bohr model and quantum model are models that explain the structure of an atom. Spectral lines undergo splitting when a sample of gas is affected by an electric field (Stark effect) and magnetic field (Zeeman effect).These are referred to as hyperfine spectral lines. Bohr's model does not explain the presence of hyperfine lines. Each spectral line, when examined at higher magnification, actually consists of a number of smaller fine lines.The accuracy decreases as the effective nuclear charge of an atom or ion increases (due to greater number of protons). Predictions made by Bohr’s model is only accurate for the hydrogen atom.Bohr's model cannot predict the relative intensity (brightness) of the spectral lines.In other words, his model does not explain why electrons can remain in their orbits without spiralling into the nucleus due to electrostatic attraction. Bohr does not provide an explanation to 'stationary states' of electrons.Circular motion of electrons is from classical physics while the quantisation of its momentum and energy of orbits is from quantum physics. Bohr's model combines principles from both classical and quantum physics.$$\Delta E_ J$$ Limitations of Bohr's Atomic Modelīohr's model of the atom has several limitations. An electron can transition between orbits by absorbing or releasing energy that is exactly equal to the difference in energy of orbits, consistent with the law of conservation of energy.Įlectron excitation occurs when an electron absorbs energy to move to an orbit of higher energy.Įlectron relaxation occurs when an electron moves to a lower orbit, releasing energy in the form of electromagnetic radiation (photon). In these orbits, electrons exist in 'stationary states' and do not emit energy.īohr’s model of the atom describes electrons orbiting in stable energy levels as opposed to Rutherford's model in which electrons' motion was not described.Ģ. ![]() Electrons revolve around the nucleus in circular orbits with discrete radii and quantised energies. ![]() Niels Bohr proposed three postulates in his atomic model:ġ. ![]() – Rydberg's equation Bohr's Model of the Atom
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