Explain the differences between the 1s and 2s | vedclass

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Question

(A) The $1s$ orbital corresponds to the principal quantum number $n=1$ and azimuthal quantum number $l=0$. The number of radial nodes is given by the

Vedclass · Accepted Answer

The $1s$ orbital has no radial nodes,while the $2s$ orbital has one radial node.

Vedclass · Answer

(A) The $1s$ orbital corresponds to the principal quantum number $n=1$ and azimuthal quantum number $l=0$. The number of radial nodes is given by the formula $(n-l-1)$. For $1s$,nodes = $1-0-1 = 0$. For the $2s$ orbital,$n=2$ and $l=0$. The number of radial nodes = $2-0-1 = 1$. Therefore,the $1s$ orbital has no radial nodes,whereas the $2s$ orbital has one radial node where the probability density drops to zero.

Explain the differences between the $1s$ and $2s$ orbitals based on their probability density plots and radial distribution.

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