The electronic configuration of the phosphide | vedclass

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Question

(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.E

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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.Electronic configuration of $P^{3-}$ is $1s^2 2s^2 2p^6 3s^2 3p^6$,which corresponds to the noble gas Argon $(Ar)$.Now,let us check the number of electrons in the options:$A$) Nitride ion $(N^{3-})$: $7 + 3 = 10$ electrons.$B$) Fluoride ion $(F^-)$: $9 + 1 = 10$ electrons.$C$) Sodium ion $(Na^+)$: $11 - 1 = 10$ electrons.$D$) Chloride ion $(Cl^-)$: $17 + 1 = 18$ electrons.Since the chloride ion $(Cl^-)$ has $18$ electrons,its electronic configuration is $1s^2 2s^2 2p^6 3s^2 3p^6$,which is the same as the phosphide ion $(P^{3-})$.

The electronic configuration of the phosphide ion $(P^{3-})$ is similar to that of:

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