The number of radial nodes and angular nodes | vedclass

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Question

(A) For any orbital,the number of angular nodes is equal to the azimuthal quantum number $(l)$.For a $4f$-orbital,the principal quantum number $n = 4$

Vedclass · Accepted Answer

$0, 3$

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(A) For any orbital,the number of angular nodes is equal to the azimuthal quantum number $(l)$.For a $4f$-orbital,the principal quantum number $n = 4$ and the azimuthal quantum number $l = 3$.Angular nodes $= l = 3$.The number of radial nodes is given by the formula: $	ext{Radial nodes} = n - l - 1$.Substituting the values: $	ext{Radial nodes} = 4 - 3 - 1 = 0$.Therefore,the number of radial nodes is $0$ and the number of angular nodes is $3$.

The number of radial nodes and angular nodes of a $4f$-orbital are respectively:

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