The total maximum number of electrons possibl | vedclass

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(A) The magnetic quantum number $m_l$ ranges from $-l$ to $+l$. An orbital can contain a maximum of $2$ electrons (with opposite spins).$1$. For $3d$

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$6$

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(A) The magnetic quantum number $m_l$ ranges from $-l$ to $+l$. An orbital can contain a maximum of $2$ electrons (with opposite spins).$1$. For $3d$ orbital $(l=2)$: $m_l$ values are $-2, -1, 0, +1, +2$. The value $m_l = -2$ is possible. Max electrons = $2$.$2$. For $6d$ orbital $(l=2)$: $m_l$ values are $-2, -1, 0, +1, +2$. The value $m_l = -2$ is possible. Max electrons = $2$.$3$. For $5s$ orbital $(l=0)$: $m_l$ value is $0$. The value $m_l = -2$ is not possible. Max electrons = $0$.$4$. For $4f$ orbital $(l=3)$: $m_l$ values are $-3, -2, -1, 0, +1, +2, +3$. The value $m_l = -2$ is possible. Max electrons = $2$.Total electrons = $2 + 2 + 0 + 2 = 6$.

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

The total maximum number of electrons possible in $3d$,$6d$,$5s$,and $4f$ orbitals with $m_l$ (magnetic quantum number) value $-2$ is

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