CHMA10H3 Lecture Notes - Lecture 19: Ionic Radius, Valence Electron, Electron Affinity
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CHMA10H3 Full Course Notes
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If more than one electron can be removed, atoms will have a serious of ionization energies. Each successive ionization energy is larger than the previous one i. e. second, third, etc. For lithum, the first ie is 0. 52 but the ie2 and ie3 are dramatically increased bc it"s easy to take out the first electron but not the rest. For beryllium, there"s a dramatic increase in ie3 bc there are 2 valence electrons on beryllium and it"s easy to remove them, but the rest are not valence and it"s hard to remove them. Valence electrons will feel the least attractive force to the nucleus, so they don"t need a lot of energy to take them away. For sodium, since it"s the same group as lithium, its change in ie are similar to lithium. Also, ie1 increased as you go across the periodic table bc the valence electrons start to have a strong attraction to the nucleus bc there"s more of them.
