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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
Solution: The number of electrons filling the lowest-energy orbitals are: 1 s: 2 electrons, 2 s: 2 electrons; 2 p: 6 electrons, 3 s: 2 electrons. This adds up to 12 electrons. The remaining three electrons go into the 3 p orbital, so the complete electron configuration of P is 1 s 2 2 s 2 2 p 6 3 s 2 3 p 3.