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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
Hence the molecule has three electron pairs and is trigonal planar for electron pair geometry. The one lone electron exerts a less repulsion than normal on the two bonding oxygen atoms so they are able to spread out more to a 134obond angle from the ideal of 120o .