Page 1 of 1
Posted: Sun Dec 08, 2019 1:21 am
Would we ever have to calculate anything with the formula he gave us in class? also, would it be correct to say the higher the charge, the more polarizable the anion
Posted: Sun Dec 08, 2019 1:38 am
I don't believe we need to do any calculations with the formula he gave us. Just know that because of the r6 in the denominator, the attraction decreases exponentially as distance decreases. Thus, the formula is very distant dependent. The higher the charge and smaller the cation, the more polarizing, not polarizing, it is. The bigger and more electron rich the anion, the more polarizable it is.
Posted: Sun Dec 08, 2019 1:49 am
I would just know the general trends, we likely won't have to do calculations based off this quation. Polarizability refers to an atom's ability to form instantaneous dipoles, and is based on how large an atom's electron cloud is. Know that the bigger an atom is, the more polarizable it is.
Posted: Sun Dec 08, 2019 5:22 pm
We never had to use the formula to do any calculations. if anything this would be a conceptual question,