Consider the following sets of quantum number | vedclass

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(D) The rules for quantum numbers are as follows: $1$. The principal quantum number $n$ can be any positive integer. $2$. The azimuthal quantum number

Vedclass · Accepted Answer

$n = 3, l = 2, m = -3, s = +1/2$

Vedclass · Answer

(D) The rules for quantum numbers are as follows: $1$. The principal quantum number $n$ can be any positive integer. $2$. The azimuthal quantum number $l$ can have values from $0$ to $n-1$. $3$. The magnetic quantum number $m_l$ can have values from $-l$ to $+l$. $4$. The spin quantum number $s$ can only be $+1/2$ or $-1/2$. Evaluating the options: - In option $D$,for $n = 3$,the maximum value of $l$ is $2$. If $l = 2$,the possible values for $m_l$ are $-2, -1, 0, +1, +2$. - Therefore,$m_l = -3$ is not permissible for $l = 2$. - Additionally,the spin quantum number $s$ must be $\pm 1/2$. The original options provided $s = \pm 2$,which is physically impossible.

Consider the following sets of quantum numbers. Which of the below settings is not a permissible arrangement of electrons in an atom?

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