We are introduced to the Bohr model of atom one time or the other in the course of physics. This model has its place in the history of quantum mechanics and particularly in explaining the structure of an atom. It has become a milestone since Bohr introduced the revolutionary idea of definite energy orbits for the electrons, contrary to the classical picture requiring an accelerating particle to radiate. Bohr also introduced the idea of quantisation of angular momentum of electrons moving in definite orbits. Thus, it was a semi-classical picture of the structure of atom.

Now with the development of quantum mechanics, we have a better understanding of the structure of atom. Solutions of the Schrodinger wave equation assign a wave-like description to the electrons bound in an atom due to attractive forces of the protons.

An orbit of the electron in the Bohr model is the circular path of motion of an electron around the nucleus.

Bohr model is valid only for one-electron atoms/ions; an energy value, assigned to each orbit, depends on the principal quantum number $n$ in this model. We know that energy associated with a stationary state of an electron depends on $n$ only. For one electron atoms/ions. For a multi-electron atom/ion, this is not true.

In the Hydrogen Spectrum provided by Bohr's model, spectral series falls in ultra-violet region of E.M. wave is:

Lyman series

Transition from the first shell to any other shell lies in ultraviolet region– Lyman series