Calculate the number of radial nodes and angular nodes for the orbital respectively. | Atomic Structure — Chem-Mantra | Chem-Mantra

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Question

Calculate the number of radial nodes and angular nodes for the $4d$ orbital respectively.

Answer: C

💡 Solution & Explanation

For a $4d$ orbital, $n=4$ and $l=2$. Radial nodes $= n - l - 1 = 4 - 2 - 1 = 1$. Angular nodes $= l = 2$. Therefore, $1$ and $2$ respectively.

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