Atomic Radius and Ionization Energy
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- So, what is Atomic Radius?
- Well, Atomic Radius is the distance between an atom's nucleus and its outermost electron shell. The smaller the Atomic Radius, the higher the Coulombic Attraction.
- See, while moving across a period on the periodic table, the atomic radius decreases due to an increase in protons, causing an increase in Coulombic Attraction. For example, the atomic radius of Lithium is 182 pm. But further across the period, with Oxygen, there is an atomic radius of 48 pm.
- Wow! What about while moving down a group? What is the trend there?
- Ah, for when moving down a group, the Atomic Radius increases. This is due to an increase in electron energy levels. For example, in Sodium, near the top of group 1, the Atomic Radius is only 186 pm, while in a Cesium atom, which is much closer to the bottom of the same group, the Atomic Radius is 343 pm.
- And how does this placement affect the Coulombic Attraction?
- Great question! As the Atomic Radius decreases, the Coulombic Attraction also decreases, since the electrons are moving further away from the protons.
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