# What is the electron configuration of the oxide ion O^(2-)?

It is isoelectronic with $\text{neon} \ldots \ldots . .$
For oxygen, $Z = 8$, and thus ${O}^{2 -}$ has a configuration of:
$1 {s}^{2} 2 {s}^{2} 2 {p}^{6}$, i.e. 10 electrons distributed..........why?