Why 2p-subhsell has the capacity to accommodate more electrons than 2s-subshell?
(2) Arrange the followinng sets of electrons in order of decreasingg energy.
(a) n=4, l=0, m=0, s=`+(1)/(2)`
(b) `n=3, l=1,m=1,s=-(1)/(2)`
(c) `n=3,l=2,m=0,s=+(1)/(2)`
(d) n=3,l=0, m=0, `s=-(1)/(2)`.
(3) Which is the lowest principal energy level that permits the existence of 'g' sub-shell?

Explanation

(1) For s-sub-shell, l=0. so, the number of orbitals in this subshell=2l+1=2`xx`0+1=1.
An orbital can accommodate maximum 2 electrons.
so, maximum number of electrons that can be accommodated in 2s-subshell=2. again for p-subshell, l=1. So, the number of orbitals in this subshell=2l+1=`2xx1+1=3`.
(2) The relative order of energies of various subshells can be predicted by the following rules: (i) A subshell with lower lower value of (n+l) has lower energy. (ii) if two subshell have equal value of (n+l), the sub-shell with lower value of n has lower energy.

So, we have the following sequence of energies of the electrons: (c)`gt(a)gt(b)gt(d)`
(3) For'g' subshell, the azimuthal quantum number l=4. thus the lowest principal energy level that permits the existence of g-subshell is given by, n=l+1=4+1=5.