FINISHED_Final_Notebook_Jones
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Ionization Energy<br />
Define Ionization Energy: The energy required to remove the most loosely bound electron from an electron (the valence<br />
electron).<br />
More Ionization<br />
Energy Required<br />
to Remove<br />
Electron<br />
More Ionization Energy<br />
Required to Remove Electron<br />
Explanation:<br />
As you move laterally across the chart, more ionization energy is required to remove an electron because, the<br />
greater amount of mass, the greater the gravitational pull on the electrons. As you move vertically along the periodic<br />
table, the amount of ionization energy required increases as you go up. This is because the higher the number of<br />
energy levels, the less gravity has an effect on the electrons in the outermost energy level, or the valence shell.<br />
The atom that requires the greatest amount of ionization energy is Helium, because it only has 1 energy level and<br />
has the largest mass for that period. Francium requires the least amount of ionization energy, because it is in the<br />
7th period (has 7 energy levels) and has the least amount of mass (located on the far left of the table).<br />
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