Which of the following set of quantum numbers | vedclass

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(C) The energy of an orbital is determined by the $(n + l)$ rule.For $A$: $n = 3, l = 0$,so $(n + l) = 3 + 0 = 3$ ($3s$ orbital).For $B$: $n = 3, l =

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$n = 3, l = 2, m = 1, s = +1/2$

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(C) The energy of an orbital is determined by the $(n + l)$ rule.For $A$: $n = 3, l = 0$,so $(n + l) = 3 + 0 = 3$ ($3s$ orbital).For $B$: $n = 3, l = 1$,so $(n + l) = 3 + 1 = 4$ ($3p$ orbital).For $C$: $n = 3, l = 2$,so $(n + l) = 3 + 2 = 5$ ($3d$ orbital).For $D$: $n = 4, l = 0$,so $(n + l) = 4 + 0 = 4$ ($4s$ orbital).Comparing the $(n + l)$ values,$5$ is the highest value.Therefore,the set of quantum numbers $n = 3, l = 2, m = 1, s = +1/2$ represents the highest energy.

Which of the following set of quantum numbers represents the highest energy of an atom?

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