Question

4. How Bohr's atomic model was explained by De-Broglie? Explain.
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Answer 1

Answer:

hope it's helpful to you

Explanation:

According to Bohr's atomic model, the angular momentum of electron orbiting around the nucleus is quantized. ... This postulate regarding the quantisation of angular momentum of an electron was later explained by Louis de Broglie. According to him, a moving electron in its circular orbit behaves like a particle wave.

Answer 2

Explanation:

Bohr's atomic model proposed that the electrons could only revolve in fixed orbits called bohr's orbits. In these orbits the angular momentum of electron would be an integer multiple of (h/2π) where 'h' is the Planck's constant.

i.e

$l = n\frac{h}{2\pi}$

Where 'n' is an integer and L the angular momentum of electron .

Even though bohr proposed this idea there was no proper explanation as to why the electron should revolve only in fixed orbits, this was then explained by De-broglie.

De-broglie proposed the idea of wave particle duality, according to which, electrons and all other particles also show wave properties, with wavelength of such waves given by

$\gamma = \frac{h}{p} = \frac{h}{mv}$

Where , p=mv is the linear momentum.

Now, assuming this theory, electrons would thus exist only when complete waves could be formed or the circumference of the orbit would be an integer multiple of the wavelength, i.e

$2\pi r = n \gamma = n \frac{h}{mv}$

Manipulating the above expression,

$mvr = n \frac{h}{2\pi} = l$

as, mvr=L=angular momentum,

This is exactly what was proposed by bohr's theory.

So bohr's atomic model was explained by De-broglie by assuming wave particle duality and that electrons could only exist in orbits in which complete waves could lie.