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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
Question:I know that the electronic configuration of Cr only is [Ar] 3d5 4s1. But how about Cr2+? Answers:[Ar]3d4 4s0 elimination of electron starts from the outermost shell. Question:Write the electron configuration for the sodium atom and for the simple ion it most commonly forms. Indicate which noble gas has the same electron configuration as the ion. I've got about 20 more of these problems and I haven't a clue how to answer them. I'm hoping somebody can explain this to me so I can figure out the rest on my own.