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Question

(A) The number of angular nodes for an orbital is given by the azimuthal quantum number $l$.For the third shell $(n=3)$,the possible subshells are $3s

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$3$

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(A) The number of angular nodes for an orbital is given by the azimuthal quantum number $l$.For the third shell $(n=3)$,the possible subshells are $3s$,$3p$,and $3d$.For $3s$ orbital,$l=0$,so the number of angular nodes is $0$.For $3p$ orbital,$l=1$,so the number of angular nodes is $1$.For $3d$ orbital,$l=2$,so the number of angular nodes is $2$.Therefore,the total number of angular nodes for all orbitals in the third shell is $0 + 1 + 2 = 3$.

Total number of angular nodes of orbitals associated with third shell $(n=3)$ of an atom is

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