From what I know Shielding effect is the ability of inner electrons to repel outer electrons and reduce the Nuclear charge felt by the outer electrons and this is caused by electron-electron repulsion.
When I read the explanation from a site it said that
Shielding refers to the core electrons repelling the outer rings and thus lowering the 1:1 ratio. Hence, the nucleus has "less grip" on the outer electrons and are shielded from them. Electrons that have greater penetration can get closer to the nucleus and effectively block out the charge from electrons that have less proximity. Because the order of electron penetration from greatest to least is s, p, d, f; the order of the amount of shielding done is also in the order s, p, d, f.
But I don't understand the fact that inner orbitals would have greater shielding effect than the outer orbitals as the closer the electrons are the more the repulsion they will have as it follows the inverse squared law. So, as the outer electrons are closer to other electrons hence they will show more repulsive force than the inner electrons as the outer electrons are closer.
One explanation which I thought was that as the electrons are not stationary and moving at great speeds, the charge could be considered as symmetrically distributed over the volume and as the charge density would be low for outer orbitals they would have less shielding effect.
Is this explanation correct or am I going wrong somewhere?