Find the number of electron pairs in P atom w | vedclass

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(B) The atomic number of Phosphorus $(P)$ is $15$. The electronic configuration of $P$ is $1s^2 2s^2 2p^6 3s^2 3p^3$. For $l = 1$,the orbitals are $2p

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$1$

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(B) The atomic number of Phosphorus $(P)$ is $15$. The electronic configuration of $P$ is $1s^2 2s^2 2p^6 3s^2 3p^3$. For $l = 1$,the orbitals are $2p$ and $3p$. In $2p^6$,all three orbitals $(m = -1, 0, +1)$ are fully filled,so there is one pair in $m = 0$. In $3p^3$,according to Hund's rule,each orbital has one electron,so there is no pair in $m = 0$. Thus,the total number of electron pairs with $l = 1$ and $m = 0$ is $1$ (from the $2p$ subshell).

Find the number of electron pairs in $P$ atom with $l = 1$ and $m = 0$.

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