The number of angular nodes and radial nodes | vedclass

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Question

(B) For any orbital,the number of angular nodes is given by the azimuthal quantum number $l$. For an $s$-orbital,$l = 0$,so the number of angular node

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$0$ and $2,$ respectively

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(B) For any orbital,the number of angular nodes is given by the azimuthal quantum number $l$. For an $s$-orbital,$l = 0$,so the number of angular nodes is $0$. The number of radial nodes is given by the formula $n - l - 1$. For the $3s$ orbital,the principal quantum number $n = 3$ and $l = 0$. Therefore,the number of radial nodes $= 3 - 0 - 1 = 2$. Thus,the $3s$ orbital has $0$ angular nodes and $2$ radial nodes.

The number of angular nodes and radial nodes in $3s$ orbital are

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