Bohr’s Atomic Model

L = \[\frac {nh​}{2π}\]

1. An electron in an atom revolves round the nucleus in a fixed circular orbit (stationary orbit) with constant speed without emitting radiant energy. Thus each atom has definite states and each possible state has definite total energy.
2. The electron revolves around the nucleus only in those orbits for which the angular momentum is an integral multiple of h2π2πh​, where hh is Planck's constant (6.6 × 10^-34 J·s). Thus the angular momentum is quantised:
   L = \[\frac{nh}{2π}\]
3. An electron can make a transition from a higher unstable orbit to a lower stable orbit. When it does so, a photon is emitted having energy equal to the energy difference between the initial and final states. The frequency of the emitted photon is:
   v = \[\frac {E_i−E_f}{h}\]
   where E_i and E_f are the energies of the initial and final states and E_i > E_f.
4. Failures of Bohr's Model: It is unable to explain the fine structure of spectral lines and is valid only for single-electron atoms.