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Total number of nodes for \( 3 \mathrm{~s} \) orbital is three
The total number of nodes of an orbital is the sum of angular and radial nodes and is given in terms of the $\mathrm{n}$ and $\mathrm{I}$
quantum number by the following equation. Number of nodes $=n-l-1$
for 3 s-orbital, $\mathrm{n}=3$
$\mathrm{I}=0$
Nodes $=3-0-1=2$
Because for s-orbitals, $\mathrm{l}=0$, therefore, there is no angular nodes only radial nodes are present, that is, 2 radial nodes.
quantum number by the following equation. Number of nodes $=n-l-1$
for 3 s-orbital, $\mathrm{n}=3$
$\mathrm{I}=0$
Nodes $=3-0-1=2$
Because for s-orbitals, $\mathrm{l}=0$, therefore, there is no angular nodes only radial nodes are present, that is, 2 radial nodes.
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