Which of the following sets of quantum number | vedclass

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(B) The energy of an orbital is determined by the $(n + l)$ rule. For option $A$: $(n + l) = 3 + 1 = 4$. For option $B$: $(n + l) = 7 + 0 = 7$. For op

Vedclass · Accepted Answer

$n = 7, l = 0, m = 0, s = +\frac{1}{2}$

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(B) The energy of an orbital is determined by the $(n + l)$ rule. For option $A$: $(n + l) = 3 + 1 = 4$. For option $B$: $(n + l) = 7 + 0 = 7$. For option $C$: $(n + l) = 3 + 2 = 5$. For option $D$: $(n + l) = 3 + 0 = 3$. Comparing the $(n + l)$ values,$7 > 5 > 4 > 3$. Therefore,the orbital with the highest energy is represented by the set of quantum numbers in option $B$.

Which of the following sets of quantum numbers represents the orbital with the highest energy?

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