Ammonia reacts with boron trifluoride to form a stable compound, as we saw in Section 8.7. (a) Draw the Lewis structure of the ammonia–boron trifluoride reaction product.

Video transcript

Hi everyone here we have a question telling us that sulfur trioxide and water reacts to form sulfuric acid. And our goal is to provide the lewis structure of sulfuric acid. So we have two hydrogen. So two times 1 valence electron, we have sulfur With six valence electrons. We have four oxygen. So four times 6 valence electrons. For a total of 32 valence electrons, Which is 16 electron pairs. Now let's bond everything. We'll have our softer in the middle Bonded to four oxygen's and then two of the oxygen's will be bonded to a hydrogen. So so far we have 123, 456 electron pairs. So now let's focus on filling everything's octet. So this oxygen needs two lone pairs. This oxygen needs to be double bonded to sulfur and have two lone pairs. The next oxygen also needs to be double bonded to sulfur with two lone pairs and our last oxygen needs to lump pairs. So now let's count how many electron pairs we have. We have six, eight, 9, 10, 11, 12, 13, 14, 15 and 16. Which is the amount of electron pairs we needed. So this is our final louis structure. Thank you for watching. Bye.