An electron has a spin quantum number +1/2 an | vedclass

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(C) For a given azimuthal quantum number $l$,the magnetic quantum number $m$ can take values from $-l$ to $+l$.For $s-$ orbital,$l = 0$,so $m$ can onl

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$s-$ orbital

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(C) For a given azimuthal quantum number $l$,the magnetic quantum number $m$ can take values from $-l$ to $+l$.For $s-$ orbital,$l = 0$,so $m$ can only be $0$.For $p-$ orbital,$l = 1$,so $m$ can be $-1, 0, +1$.For $d-$ orbital,$l = 2$,so $m$ can be $-2, -1, 0, +1, +2$.For $f-$ orbital,$l = 3$,so $m$ can be $-3, -2, -1, 0, +1, +2, +3$.Since the electron has $m = -1$,it can exist in $p, d,$ or $f$ orbitals,but it cannot be present in an $s-$ orbital because the only possible value for $m$ in an $s-$ orbital is $0$.

An electron has a spin quantum number $+1/2$ and magnetic quantum number $-1.$ It cannot be present in :

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