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Hi,
In answering the question #40 of the BR General Chem Atomic Theory chapter, it asks which element is oxidized most easily between sulfur, magnesium, boron, and argon. I'm confused because I was debating b/w Mg and S--I know the electronic configuration of Mg is 1s^2 2s^2 2p^6 3s^2, and the electronic config of S is 1s^2 2s^2 2p^6 3s^2 3p^4; the answer was Mg, but I thought it was S, since if it lost an electron it would have its p orbitals half filled, which is more favorable than if Mg lost an electron, where it would have an s orbital half filled--does the half-filling of p orbitals take precedence over the half filling of the s orbitals? On the other hand, I know that Zeff for S is +4, whereas its only +2 for Mg, meaning that Mg would be the answer..
Thanks for any help!
In answering the question #40 of the BR General Chem Atomic Theory chapter, it asks which element is oxidized most easily between sulfur, magnesium, boron, and argon. I'm confused because I was debating b/w Mg and S--I know the electronic configuration of Mg is 1s^2 2s^2 2p^6 3s^2, and the electronic config of S is 1s^2 2s^2 2p^6 3s^2 3p^4; the answer was Mg, but I thought it was S, since if it lost an electron it would have its p orbitals half filled, which is more favorable than if Mg lost an electron, where it would have an s orbital half filled--does the half-filling of p orbitals take precedence over the half filling of the s orbitals? On the other hand, I know that Zeff for S is +4, whereas its only +2 for Mg, meaning that Mg would be the answer..
Thanks for any help!