Module 5 : MODERN PHYSICS
Lecture 26 : Wave Nature of Particle - the de Broglie Hypothesis
 
Exercise 6
  Bohr Model :
  Bohr's model of an atom, which was very successful in explaining the spectra of hydrogen like atoms is based on the following postulates :
Electrons move in stationary orbits around the nucleus. As long as an electron is in such an orbit, it does not y
  radiate. However, it emits ( absorbs) radiation when it makes a discontinuous transition form an orbit with energy $ E$ to an orbit of lower (higher) energy $ E^\prime$. The frequency of emitted (absorbed) radiation is given b
 
$\displaystyle \nu = (-) \frac{E-E^\prime}{h}$
The angular momentum of an electron in a stationary orbit is an integral multiple of $ h/2\pi$ :
 
$\displaystyle mvr = n\frac{h}{2\pi}$
  where $ n$ is an integer.
  Using Bohr model, one can show that the wavelength of the radiation emitted when an electron makes a transition from an orbit with quantum number $ n_i$ to an orbit with $ n_f$, is given by
   
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