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(D) The number of radial nodes for an orbital is given by the formula: $	ext{Number of radial nodes} = n - \ell - 1$.For the $3s$ orbital, the princi

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$(D)$

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(D) The number of radial nodes for an orbital is given by the formula: $	ext{Number of radial nodes} = n - \ell - 1$.For the $3s$ orbital, the principal quantum number $n = 3$ and the azimuthal quantum number $\ell = 0$.Substituting these values: $	ext{Number of radial nodes} = 3 - 0 - 1 = 2$.$A$ radial distribution function plot for an orbital with $2$ radial nodes must show $2$ points where the probability density touches the $r$-axis (excluding $r=0$ and $r=\infty$).Looking at the provided plots:- Plot $(A)$ has $0$ radial nodes.- Plot $(B)$ has $1$ radial node.- Plot $(C)$ has $0$ radial nodes.- Plot $(D)$ has $2$ radial nodes.Therefore, the correct plot for the $3s$ orbital is $(D)$.

The plots of radial distribution functions for various orbitals of a hydrogen atom against $r$ are given below. The correct plot for the $3s$ orbital is

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