Question

Calculate the maximum and minimum number of electrons which may have magnetic quantum number $m=-1$ and spin quantum number $s=-\frac{1}{2}$ in Manganese $\left(Mn\right)$

• A. $3,2$
• B. $6,4$
• C. $4,2$
• D. $2,1$

Answer 1

The correct option is A $3,2$

The atomic number of $Mn$ is $25$.
$\therefore$ Electronic configuration of $Mn$ is $\left[Ar\right]4s^{2}3d^5$


Out of $6$ electrons in $2p$ and $3p$, there must have one electron with $m=-1$ and $s=-\frac{1}{2}$ in each.But in $3d$ subshell an orbital having $m=-1$ may have spin quantum number of $-\frac{1}{2}$ or $+\frac{1}{2}$.
Therefore, maximum possible value is $=3$
and minimum possible value is $=2$