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Ionization Energy

Ionization Energy. Kyle Albro , Nathaniel Cho, Jeremy Ha. General. Ionization Energy is the energy required to remove the electron from the outermost shell of the atom. Units are KJ/ mol What Goes into Ionization Energy ? The overall charge of the atom the effect of shielding

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Ionization Energy

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  1. Ionization Energy Kyle Albro, Nathaniel Cho, Jeremy Ha

  2. General • Ionization Energy is the energy required to remove the electron from the outermost shell of the atom. • Units are KJ/mol What Goes into Ionization Energy? • The overall charge of the atom • the effect of shielding • the distance between electrons and the nucleus.

  3. General Trend • Going across the periodic table, there should be an increase in ionization energy because of the increasing nuclear charge. • As you go down a column the energy levels increase, placing the electron further away from the nucleus so they are not so strongly attracted to the nucleus. • the effect of increased nuclear charge is balanced by the effect of increased shielding

  4. Exceptions H- Hydrogen’s ionization energy is so much greater than any other alkali metals because Hydrogen does not experience any shielding from other electrons Transition metals- As a general trend, the transition metals energies are greater as they go down the family. Oxygen family- The oxygen family’s energies are less, because the p orbital.

  5. Going Further • Generally the (n+1)th ionization energy is larger than the nth ionization energy. Cause: • the next ionization energy involves removing an electron from an orbital closer to the nucleus. • Electrons in the closer orbitals experience greater forces of electrostatic attraction; thus, their removal requires increasingly more energy. • When removing the second electron from sodium (Na) you must remove an electron from the much closer p-orbital, which is why the second energy level is relatively much larger than the first.

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