Which statement is not correct for n = 5,m = | vedclass

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Question

(B) For a given principal quantum number $n$,the azimuthal quantum number $l$ can take values from $0$ to $n-1$. For $n = 5$,$l$ can be $0, 1, 2, 3, 4

Vedclass · Accepted Answer

$l = 0, 1, 3; s = + \frac{1}{2}$

Vedclass · Answer

(B) For a given principal quantum number $n$,the azimuthal quantum number $l$ can take values from $0$ to $n-1$. For $n = 5$,$l$ can be $0, 1, 2, 3, 4$. The magnetic quantum number $m$ ranges from $-l$ to $+l$. If $m = +3$,then $l$ must be at least $3$ (i.e.,$l = 3$ or $l = 4$). Option $A$ $(l = 4)$ is possible because $m = +3$ is allowed for $l = 4$. Option $C$ $(l = 3)$ is possible because $m = +3$ is allowed for $l = 3$. Option $B$ suggests $l = 0, 1, 3$. While $l = 3$ is valid for $m = +3$,$l = 0$ and $l = 1$ are not valid for $m = +3$ because for $l=0, m=0$ and for $l=1, m=-1, 0, +1$. Therefore,the statement in option $B$ is incorrect.

Quantum Number	Information
$(1)$ Principal quantum number	$(A)$ Spatial orientation of the orbital
$(2)$ Azimuthal quantum number	$(B)$ Energy and size of the orbital
$(3)$ Magnetic quantum number	$(C)$ Electron spin
$(4)$ Spin quantum number	$(D)$ Shape of the orbital

Which statement is not correct for $n = 5$,$m = +3$?

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