De-Broglie explained the Bohr's postulate of quantization by particle nature of electron. (True /False)

The de-Broglie equation treats an electron to be

(a) Using Bohr's second postulate of quantization of orbital angular momentum show that the circumference of the electron in the n^(th) orbital state in hydrogen atom is n times the de-Broglie wavelength associated with it. (b) The electron in hydrogen atom is initially in the third excited state. What is the maximum number of spectral lines which can be emitted which it finally moves to the ground state ?

The de-Broglie equation suggests that an electron has

The de-Broglie wavelength of electron in gound state of an hydrogen atom is

Assertion Second orbit circumference of hydrogen atom is two times the de-Broglie wavelength of electrons in that orbit Reason de-Broglie wavelength of electron in ground state is minimum.

Using Bohr's postulates of the atomic model. Derive the expression for radius of nth electron orbit, thus obtaining the expression for Bohr's radius.

(i) State Bohr's quantization condition for defining stationary orbits . How does de- Broglie hypothesis explain the stationary orbits ? (ii) find the relation beween the three wavelengths lambda_(1), lambda _(2) " and " lambda_(3) from the energy level diagram shown :

A particle is moving 5 times as fast as an electron. The ratio of the de-Broglie wavelength of the particle to that of the electron is 1.878 xx10^(-4) . The mass of the particle is close to :

The de-broglie wavelength of a photon is twice the de-broglie wavelength of an electron. The speed of the electron is v_(e)=c/100 . Then