Between $2s$ and $2p$ electrons,which one experiences a greater shielding effect from inner shells?

For the valence shell of $Na$,screening is provided by:

Among the following pairs of orbitals,which orbital will experience the larger effective nuclear charge?
$(i)$ $2s$ and $3s$
$(ii)$ $4d$ and $4f$
$(iii)$ $3d$ and $3p$

In $Lithium$,the $2s$ electron experiences a force of attraction exerted by the nucleus that is:

Which of the following statements is correct about the "shielding effect"?
$1$. It is effective when the orbitals in the inner shells are completely filled.
$2$. Inner shells do not show any effect.
$3$. With an increase of shielding down the group,ionization energy increases.
$4$. With increasing nuclear charge,the shielding effect increases.

Among the following,the energy of $2s$ orbital is lowest in