Which of the following sets of quantum number | vedclass

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Question

(A) For a $4f$ orbital,the principal quantum number $n = 4$.For an $f$ subshell,the azimuthal quantum number $l = 3$.The magnetic quantum number $m$ c

Vedclass · Accepted Answer

$n = 4, l = 3, m = +1, s = +\frac{1}{2}$

Vedclass · Answer

(A) For a $4f$ orbital,the principal quantum number $n = 4$.For an $f$ subshell,the azimuthal quantum number $l = 3$.The magnetic quantum number $m$ can take values from $-l$ to $+l$,i.e.,$-3, -2, -1, 0, +1, +2, +3$.The spin quantum number $s$ can be either $+\frac{1}{2}$ or $-\frac{1}{2}$.Checking the options:Option $A$: $n = 4, l = 3, m = +1, s = +\frac{1}{2}$ is valid because $m = +1$ lies within the range $[-3, +3]$.Option $B$: $l = 4$ is not possible for $n = 4$ (since $l Option $C$: $m = +4$ is not possible for $l = 3$ (since $|m| \leq l$).Option $D$: $n = 3$ corresponds to the $3d$ orbital,not $4f$.

Which of the following sets of quantum numbers is correct for an electron in a $4f$ orbital?

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