Question

what are the shortcoming of bohr's theory

Answer 1

Hi my name is PAVANKALYAN

Ans:

1. Bohr treated electrons as particles where according to de Broglie's hypothesis, having a very low mass, electron also exhibits wave nature.

2. Bohr's model was adequate only for nucleus having only one electron e.g. Hydrogen, He+1, Li+2 etc. Bohr's model could not explain the spectra of multi-electronic atoms.

3. Bohr's model was two-dimensional where an atom is three-dimensional.

4. Using a better spectrometer, the spectra showed very fine lines. Bohr's model could not explain the origin of those fine lines. (Solved by Arthur Sommerfield who imagined electrons orbiting in different planes and having elliptical orbits.)

5. Bohr's model could not explain the effect electric field and magnetic field on spectra. (Stark effect and Zeeman effect)

6. In Bohr's equation, the momentum and position of electron, revolving around the nucleus were well defined. But, according, Heisenberg's Uncertainty principle, it is impossible to measure the position and momentum of electrons precisely. If the position is measure with maximum precision, there will be uncertainty in the value of momentum and vice versa.

Answer 2

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1. Bohr unable to give the following information, the spectrum lines of hydrogen should be sharp and single, but with spectroscopy of high resolution capacity, On seeing, it is found that no spectrum line is a single line But there are a number of lines near very close to the desired line. him . The fine structure of the spectrum line is called.

For example, the first line of the Baller Range $(H _{ \alpha })$is the group of five very fine lines. Bore theory is unsuccessful to explain the subtle structure.


2 . The bore theory interprets only the wavelengths of the spectrum lines, does not explain the variation of their intensities, that is, does not give any information regarding the wave nature of the electron.


3. The bore theory can only explain the spectrum of hydrogen and hydrogen-like atoms. It is unsuccessful to explain the spectrum of complex atoms.


4. This principle does not define the rate of electron infection and the selection of infections - restrictions or selection rules.


5. This principle does not provide any information about the electron orientation of the atom.


6. This principle is unable to explain the effect of the magnetic field on the spectrum lines and the effect of the effects of the effects of the effects of the effects of the spin-back effects and the effects of the field.


7. The most serious drawback of the model is that it is based on two conflicting concepts. According to this model, the state of equilibrium is determined by absolute rules while emission is interpreted on the basis of quantum theory.