Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: zerothedestroyer on May 07, 2010, 09:41:52 PM
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Why would the electron affinity of group 15A electrons be smaller than electrons in 14A? Electron affinity is the energy released when an electron is added to an atom in its gaseous state isn't it? Does it have anything to do with the ionization energy?
I am looking at the periodic table and the electron affinity of these two atoms are vastly different. I am trying to think what reason would adding an electron release energy? Is it because the ionization of that group is so much larger since elements like nitrogen desperately want electrons?
Can someone explain to me what is going on? I would be grateful.
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How are 3, 4 and 5 electrons configured in a p-orbital? Which is most stable?