Given,(A) n=5, m_l=-1(B) n=3, l=2, m_l=-1, m_ | vedclass

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(D) For $n=5$:For each subshell $l$, the number of orbitals with $m_l=-1$ is $1$ (if $l \ge 1$).Subshells present in $n=5$ are $l=0, 1, 2, 3, 4$.$m_l=

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$8$ and $1$

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(D) For $n=5$:For each subshell $l$, the number of orbitals with $m_l=-1$ is $1$ (if $l \ge 1$).Subshells present in $n=5$ are $l=0, 1, 2, 3, 4$.$m_l=-1$ is possible for $l=1, 2, 3, 4$.Each orbital can hold $2$ electrons.Total electrons $= 4 	ext{ orbitals} 	imes 2 	ext{ electrons/orbital} = 8$ electrons.$(B)$ For $n=3, l=2, m_l=-1, m_s=+\frac{1}{2}$:This set of quantum numbers defines a specific orbital and a specific spin.Only $1$ electron can have these exact quantum numbers.

Given,
$(A)$ $n=5, m_l=-1$
$(B)$ $n=3, l=2, m_l=-1, m_s=+\frac{1}{2}$
The maximum number of electron$(s)$ in an atom that can have the quantum numbers as given in $(A)$ and $(B)$ respectively are:

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Given,$(A)$ $n=5, m_l=-1$$(B)$ $n=3, l=2, m_l=-1, m_s=+\frac{1}{2}$The maximum number of electron$(s)$ in an atom that can have the quantum numbers as given in $(A)$ and $(B)$ respectively are: