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Calculate the total number of angular nodes and radial nodes present in $3p$ orbital.
(A) For $3p$ orbital,the principal quantum number $n = 3$ and the azimuthal quantum number $l = 1$.
The number of angular nodes is given by $l = 1$.
The number of radial nodes is given by $n - l - 1 = 3 - 1 - 1 = 1$.
Therefore,the $3p$ orbital has $1$ angular node and $1$ radial node.
The number of angular nodes is given by $l = 1$.
The number of radial nodes is given by $n - l - 1 = 3 - 1 - 1 = 1$.
Therefore,the $3p$ orbital has $1$ angular node and $1$ radial node.
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