Question

How Many Radial Nodes And Angular Nodes Are Present In $4d$ Orbital ?

Answer 1

The above question can be solved as:

Step 1:

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

Number of angular nodes $=\mathrm{l}$

where, $\mathrm{n}=$Principal Quantum No. $\mathrm{l}=$Azimuthal Quantum No.

Step 2:

For $4\mathrm{d}$ orbital, $$\begin{gathered} \mathrm{n}=4 \\ \mathrm{l}=2 \end{gathered}$$

Step 3:

Hence, for $4\mathrm{d}$ orbital, the number of radial nodes $$\begin{gathered} =\mathrm{n}-\mathrm{l}-1 \\ =4-2-1 \\ =1 \end{gathered}$$

Hence for $4\mathrm{d}$ orbital, the number of angular nodes $$\begin{gathered} =\mathrm{l} \\ =2 \end{gathered}$$

Therefore, $4d$ orbital have $2$ Angular Nodes and $1$ Radial Nodes.