My question is from the concept of finding the probability of electron
as if we draw probability distribution curve maximum probability of finding the electron is maximum just near or on the nucleaus but this can t be possible so we intro duce the concept of radial probabiliy in which near the nucleaus probabiity of finding the electron in shelll is zero but we say both concepts are right plz explain expert

To find out what extent will quantum mechanics permit us to pinpoint the position of an electron when it is bound to an atom? We can obtain an order of magnitude answer to this question by applying the uncertainty principle

to estimateDx. The value ofDxwill represent the minimum uncertainty in our knowledge of the position of the electron. The momentum of an electron in an atom is of the order of magnitude of 9´10^-19g cm/sec. Theuncertaintyin the momentumDpmust necessarily be of the same order of magnitude. Thus

The uncertainty in the position of the electron is of the same order of magnitude as the diameter of the atom itself. As long as the electron is bound to the atom, we will not be able to say much more about its position than that it is in the atom. Certainly all models of the atom which describe the electron as a particle following a definite trajectory or orbit must be discarded. This way of estimation is based on the magnitude of energy of the electron.

whereas the radial distribution curve gives an idea about the electron density at a radial distance from the nucleus. The value of 4πr²ψ²(radial probability density function) becomes zero at a nodal point, also known as radial node.

Hence both the things are correct on their own.

Regards

Sumit