I learnt about Heisenberg's Uncertainty principle which states that it is not possible to determine the position and momentum of a small particle at the same time.
I was told that it is because in order to be able to see the atoms, we need to make use of radiations, and when we do that, the electrons get excited by those radiations and their position changes. No matter how sophisticated our instruments get, there will be some error. If we use radiation of wavelength "D" to measure the position of electron, then minimum error in position will be "D"
I didn't really get how would we use radiations to make the atoms visible. Can you please explain that?
This principle clearly states that we cannot be certain about the position and velocity of an electron in an atom, and this must also be true for hydrogen like species. But we still use the formulae given by Bohr's model of atom to find out velocity of electron in nth orbit and its position for hydrogen like species. My teacher says that these formulae give satisfactory results for hydrogen like species. How could that be? Is it because the error is minimum in the case of hydrogen like species?
I am not able to intuitively arrive to an explanation to both these above question.