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The electronic configuration for the oxygen atom is [math]1s^2 2s^2 2p^4[/math]. It must acquire 2 electrons to become an ion with a charge of -2 . Thus the electronic configuration for an [math]O^{2 -}[/math] ion is
Each oxygen atom has 6 valence electrons, for a total of 12. If we start, in typical fashion, by drawing out the Lewis structure with just a single bond between them, we then have (12 - (2*1bond)) = 10 electrons left to distribute.