Question

How Many Radial Nodes Are Present In $3\mathrm{s}$ Orbital ?

Answer 1

The number of radial nodes in $3\mathrm{s}$ orbital is explained below:

No. of radial nodes $=\mathrm{n}-\mathrm{l}-1$

where, $\mathrm{n}=$principal quantum number

$\mathrm{l}=$azimuthal quantum number

1. For, $3\mathrm{s}$ orbital, $$\begin{gathered} \mathrm{n}=3 \\ \mathrm{l}=0 \end{gathered}$$
2. Hence number of radial nodes in $3\mathrm{s}$ orbital $$\begin{gathered} =3-0-1 \\ =2 \end{gathered}$$

Therefore, the number of radial nodes in $3\mathrm{s}$ orbital is $2$.