Neil Bohr proposed a theory to explain the emission spectrum of hydrogen. His theory states that the electron in hydrogen atom circle the nucleus in certain FIXED PATH.
1) How does this theory explains that the emission spectrum of hydrogen consist of a set number of discrete lines?
2) State 1 way understand of electron structure of atom differ from that proposed by Bohr for hydrogen atom.
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1) When the electrons in an atom absorb energy they move up into higher energy levels. The electrons are said to be in their excited state, but this state is unstable. The electrons will quickly return to their home positions (or ground states), and when they do, they must give back the energy they absorbed. This usually happens in the form of electromagnetic radiation, which takes the form of visible light for many of these transitions.
If energy were continuous, we would expect all the possible wavelengths of light to be given off as the electron slid downward toward the nucleus, but that isn't what happens. We only get specific wavelengths, because only certain energy levels are allowed. This shows us that energy can only be absorbed or released by electrons in discrete bundles called quanta.
2) According to the Bohr's atomic theory, the electrons revolve in particular orbits of precised values of radii.
And according to this theory position and momentum of the electron can be known.
But according to the quantum theory, there are wide ranges of possible radii for each electron and it gives only the probability of finding the electron at a particular radius.
And the uncertainty principle says that both position and momentum of an electron can be known at a time.