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Posted: Mon Nov 14, 2016 4:44 pm
How we would solve this problem?
Based on their valence shell electron configurations which of the following species would you expect to have the lowest ionization energy:
C2+, C2, C2- ?
Posted: Mon Nov 14, 2016 5:05 pm
You would calculate the bond orders for each one and so the one would the highest bond order would have the highest ionization energy because the bond is stronger. Then you would compare if the electrons are higher or lower in energy. Electrons in the higher energy orbitals mean that they are easier to ionize than ones with electrons in lower electron orbitals.
Posted: Mon Nov 14, 2016 6:06 pm
A low ionization energy means higher energy electrons. Writing out the valence electron configurations of these molecules reveals that C2- has an electron in the sigma 2p orbital, whereas the others do not. Therefore, C2- has the lowest ionization energy.