For the electronic configuration $1s^2 2s^2 2p^3$,what is the number of electrons having $n = 2, l = 1$,and $s = +1/2$?

In the following pairs,which orbital experiences greater nuclear attraction?
$(i)$ $4f$ and $5d$ $(ii)$ $4d$ and $5s$ $(iii)$ $7s$ and $5f$ $(iv)$ $7p$ and $5p$
$(v)$ $3d$ and $3f$

Consider the following sets of quantum numbers:

$Set$	$(n)-(l)-(m)-(s)$
$(i)$	$(3)-(2)-(1)-(+1/2)$
$(ii)$	$(2)-(2)-(1)-(+1/2)$
$(iii)$	$(4)-(3)-(-2)-(-1/2)$
$(iv)$	$(1)-(0)-(-1)-(-1/2)$
$(v)$	$(3)-(2)-(3)-(+1/2)$

Which of the following sets of quantum numbers is not possible?

The valence shell electronic configuration is $(n - 1)s^2 (n - 1)p^6 (n - 1)d^x ns^2$. If $n = 4$ and $x = 5$,what is the number of protons in the element?

The two electrons occupying the same orbital are distinguished by:

What is the maximum number of electrons which can be accommodated in an atom in which the highest principal quantum number value is $4$?