Which would you expect to be the stronger Lewis acid in
each of t...

Question

Which would you expect to be the stronger Lewis acid in
each of the following pairs? Explain.
(a) BF3 or BH3

Accepted Answer

Hello everyone today. We're looking at the following question, identified the strongest lewis acid. Among the following. We have boron chloride boron fluoride boron iodide in boron bromide. So these are what are known as binary acids. Binary assets simply have the formula some proton with a halo represented by X. And so within a group or the columns of the periodic table, a city is going to increase as you go down a group or a column since the size increases as well and the opposite is going to be true in the opposite direction. So if you look within a period or the horizontal rows, the acidity it's going to increase as you go left to right. And so why is this? This is because electro negativity increases as you go up and to the right. And so we can consider that the weaker the hydrogen hey light bond, this is going to result in a higher acidity with that. We can consider the following as binary acids with the common atom of B or boron. So essentially what we have to compare leftover is chloride or chlorine fluoride or floor een, iodine or iodine. And then bromide or bro mean if we were to analyze their size according to the periodic trend from the smallest to the largest is going to go from flooring chlorine bromine and iodine being the largest. If we were to look at their strength, this would follow the same trend. We would have that common adam B with our fluorine followed by the common atom b with our chloride and then with our bromide and then our iodide, and thus the strongest lewis acid. As we already discussed would be our boron iodide. And so with that we've answered the question overall, I hope this helped, and until next time.

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