JEE Main 2022 — Structure of Atom Question with Solution

Number of Radial nodes $=\mathrm{n}-\mathrm{l}-1$

Number of angular nodes $=\mathrm{l}$

Where,

$$\begin{gathered} \mathrm{l}=\mathrm{Azimuthal} \mathrm{quantum} \mathrm{number} \\ \mathrm{n}=\mathrm{principal} \mathrm{quantum} \mathrm{number} \end{gathered}$$

For $4\mathrm{d}$ orbital, $\mathrm{n}=4$ and $\mathrm{l}=2$

In $4\mathrm{d}$ orbital the number of Radial nodes=$4-2-1$=1

In $4\mathrm{d}$ orbital the number of Angular nodes $=\mathrm{l}=2$.

Thus, the number of radial and angular nodes in $4\mathrm{d}$ orbital are $1$ and $2$ respectively.