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The Bohr model of atoms :-
A
Uses Einstein's photo electric equation
B
Predicts continuous emission spectra for atoms
C
Predicts the same emission spectra for all types of atoms
D
Assumes that the angular momentum of electrons is quantized
Detailed Solution
Bohr's postulates: (i) electrons revolve in certain stable orbits without radiating energy; (ii) only those orbits are allowed for which the angular momentum is an integral multiple of $\dfrac{h}{2\pi}$, i.e. $mvr = \dfrac{nh}{2\pi}$; (iii) radiation is emitted or absorbed only when an electron jumps between orbits, $h\nu = E_i - E_f$.
Since only discrete energy levels exist, the model predicts a line spectrum, not a continuous spectrum.
The energy levels depend on the atomic number Z, so different atoms have different spectra.
The model does not use Einstein's photoelectric equation.
So the Bohr model assumes that the angular momentum of electrons is quantized.
Since only discrete energy levels exist, the model predicts a line spectrum, not a continuous spectrum.
The energy levels depend on the atomic number Z, so different atoms have different spectra.
The model does not use Einstein's photoelectric equation.
So the Bohr model assumes that the angular momentum of electrons is quantized.