Ionization Energy
Storyboard Text
- Could you explain to me what Ionization Energy is?
- Sure I can! Ionization Energy is the amount of energy required in order to remove an electron from an atom. Regarding the Shielding Effect, the higher the amount of electrons, the higher the Shielding Effect, and therefore the lower the Ionization Energy since the outer electrons are being shielded from the protons in the nucleus.
- Well, what is the trend in Ionization Energy as you go down a group?
- Nice question! As you go down a group, the Ionization Energy decreases, due to the electrons being further away from the protons and the Coulombic Attraction lessening. An example of this is with Sodium, whose electrons are super close to the nucleus, and has an Ionization Energy of 496 KJ/mol; and with Cesium, whose electrons are much further away from the nucleus and only has an Ionization Energy of 376 KJ/mol.
- And what about when going across a period?
- While going across a period, the Ionization Energy will increase. This is due to an increase in nuclear charge, making the electrons more strongly attracted to the protons within the nucleus. This increased nuclear charge also means that there is a higher Coulombic Attraction. For example, in Lithium, on the very left side of the periodic table, the IE is 520.2 KJ/mol. In Fluorine, which is much closer to the right of the periodic table, yet still within the same period as Lithium, the IE is 1681 KJ/mol.
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