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Ionization Energy - Ionization Energy The ionization energy...

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Ionization Energy The ionization energy of an atom measures how strongly an atom holds its electrons The ionization energy is the minimum energy required to remove an electron from the ground state of the isolated gaseous atom Note that this does not mean the energy required to remove an electron from the n =1 shell (i.e the ground state orbital), the ground state here refers to the lowest energy electron configuration for the element in question The first ionization energy, I 1 , is the energy needed to remove the first electron from the atom: Na( g ) -> Na + ( g ) + 1e - The second ionization energy, I 2 , is the energy needed to remove the next (i.e. the second) electron from the atom Na + ( g ) -> Na 2+ ( g ) + 1e - The higher the value of the ionization energy, the more difficult it is to remove the electron As electrons are removed, the positive charge from the nucleus remains unchanged, however, there is less repulsion between the remaining electrons Z eff increases with removal of electrons Greater energy is needed to remove remaining electrons (i.e.
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