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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
Permalink Submitted by spock on Wed, 2009-03-25 22:31. The rule for Oxygen is that it is almost alway -2 in a compound. The sum of the oxidation states in an ion must add up to the charge on the ion, Therefore each Cr atom must have a +6 oxidation state: 2(+6) + 7 (-2) = -2.