HEISENBERG’S PRINCIPLE OF UNCERTAINTY:-
The Hinesburg’s principle of uncertainty is defined as.
“Both position and momentum of electron cannot be determined at the same time with absolute exactness or certainty”
This equation shows as that an object having greater mass and greater velocity (greater momentum), it will have very short wavelength. In order to locate the position of electron, we use wave whose wavelength must be less then the size of the electron itself. It means that the wave world be having greater momentum. Thus when the position of electron is determined, its momentum changes and the position become uncertain.
In order to find out about the position and momentum of electron around nucleus, we use probability. We can only tell, the probable position and probable velocity of an electron around the nucleus.
Another scientist Schrödinger treated electrons as moving with wave like motion in three-dimensional space around the nucleus and not in fixed orbit, as Bohr had described in his atomic model. He replaced the idea of a fixed path or orbit around the nucleus. He called this area of region orbital.
The region or space around the nucleus in which electrons is most probably located is called an atomic orbital.
In short, the orbital is not a fixed path, but a region around the nucleus where the probability of finding electron is maximum.
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