Which of the following sets of quantum number | vedclass

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(D) The rules for quantum numbers are as follows:$1$. $n$ is the principal quantum number $(n = 1, 2, 3, ...)$.$2$. $l$ is the azimuthal quantum numbe

Vedclass · Accepted Answer

$4, 3, -4, -1/2$

Vedclass · Answer

(D) The rules for quantum numbers are as follows:$1$. $n$ is the principal quantum number $(n = 1, 2, 3, ...)$.$2$. $l$ is the azimuthal quantum number ($l = 0$ to $n-1$).$3$. $m$ is the magnetic quantum number ($m = -l$ to $+l$ including $0$).$4$. $s$ is the spin quantum number ($s = +1/2$ or $-1/2$).Evaluating the options:- Option $A$: $n=4, l=0, m=0, s=-1/2$. This is valid ($l - Option $B$: $n=3, l=2, m=-2, s=+1/2$. This is valid ($l - Option $C$: $n=5, l=4, m=0, s=-1/2$. This is valid ($l - Option $D$: $n=4, l=3, m=-4, s=-1/2$. Here,$m$ must be in the range $-3$ to $+3$. Since $m = -4$ is outside this range,this set is incorrect.

Which of the following sets of quantum numbers $(n, l, m, s)$ is incorrect?

Similar Questions

Two electrons $A$ and $B$ in an atom have the following set of quantum numbers:
$A: n=3, l=2, m_l=-2, m_s=+1/2$
$B: n=3, l=0, m_l=0, m_s=+1/2$
What is true for $A$ and $B$?

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The state of an electron in a $3d_{z^2}$ orbital is described by which quantum numbers?

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Which one of the following sets of quantum numbers represents an impossible arrangement?

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