The electronic configuration of the phosphide | vedclass

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(D) The atomic number of phosphorus $(P)$ is $15$. The phosphide ion $(P^{3-})$ is formed by gaining $3$ electrons,so it has $15 + 3 = 18$ electrons.I

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Chloride ion $(Cl^-)$

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(D) The atomic number of phosphorus $(P)$ is $15$. The phosphide ion $(P^{3-})$ is formed by gaining $3$ electrons,so it has $15 + 3 = 18$ electrons.Its electronic configuration is $1s^2 2s^2 2p^6 3s^2 3p^6$,which is the same as that of the noble gas Argon $(Ar)$.Among the given options,the chloride ion $(Cl^-)$ has an atomic number of $17$ and gains $1$ electron to have $17 + 1 = 18$ electrons.Thus,the electronic configuration of $P^{3-}$ ($18$ electrons) is similar to that of $Cl^-$ ($18$ electrons).

The electronic configuration of the phosphide ion $(P^{3-})$ is similar to which of the following?

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