Question

The electron configuration of the oxide ion is much most similar to the electron configuration of the

• A. sulphide ion
• B. nitride ion
• C. oxygen atom
• D. nitrogen atom

Answer 1

Answer: (B)

Species having the same number of electrons as in oxide ion, has the same electronic configuration as oxide ion.

In oxide ion $\left(O^{2-}\right)$, number of electrons $=8+2=10$

In sulphide ion $\left(S^{2-}\right)$, number of electrons $=16+2=18$

In nitride ion $\left(N^{3-}\right)$, number of electrons $=7+3=10$

In oxygen atom and nitrogen atom, number of electrons $=8,7$ respectively.

Hence, electronic configuration of

$O^{2-}$ or $N^{3-}(10)=\sigma 1s^2,\stackrel{\ast }{\sigma }1s^2,\sigma 2s^2,\stackrel{\ast }{\sigma }2s^2,\pi 2p_x^1\approx \pi 2p_y^1$