Magnetic and spin quantum number of an electr | vedclass

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(A) For a given azimuthal quantum number $l$,the magnetic quantum number $m$ ranges from $-l$ to $+l$.For $s$ orbital,$l = 0$,so $m$ can only be $0$.F

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$s$ orbital

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(A) For a given azimuthal quantum number $l$,the magnetic quantum number $m$ ranges 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 given magnetic quantum number is $m = -1$,it is impossible for the electron to be in an $s$ orbital because $m$ must be $0$ for $l = 0$.

Magnetic and spin quantum number of an electron are $-1$ and $+1/2$ respectively. This electron cannot be in

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