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Polarizability increases w atomic radius aka down a group bc their electron clouds can easily be distorted where as small highly charged cations have high polarizing power (decreases across a period)
Polarizability goes inverse along with the electron affinity of elements. If an atom can be easily polarized, it can easily lose an electron, meaning it has a low electron affinity.
Did he say that polarizability will be covered on the midterm?
if it can easily lose an electron then there is a lower electron affinity
Polarizability essentially has to do with how much charge is there and how much space does the atom have to spread the charge out. For example, a large anion like Iodide is large and can spread the charge over its volume and become polarized. Polarizing ability increase with decreasing radius and increasing charge. So, a highly charged, small cation will have a highly localized charge which will affect negatively charged species strongly.
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