Ibuprofen 1C13H18O22, marketed under such brand names as Advil and Motrin, is a drug sold over the counter for treatment of pain and inflammation. Complete the structure of ibuprofen by adding hydrogen atoms and lone pairs where needed.

Video transcript

welcome back everyone. Aspirin. Aceto salsa like acid C nine H 804 is used to reduce pain, fever and inflammation fill the structure of aspirin below with the missing hydrants and lone pairs. So looking at the structure given for our aspirin molecule, we can see that we only have our oxygen and carbon atoms filled in. And when we want to think of is our bonding preference of carbon as well as oxygen. When it comes to carbon, we should recall that it's bonding preferences to just have four bonds to be stable When it comes to oxygen. We're going to recall that oxygen typically forms two bonds And has two lone pairs on itself. And because we recognize that carbon and oxygen are on period two of our periodic table. These bonding preferences ensure that they honor the octet rule when in lower structures. So when we look at our atoms here, we can see that this carbon right now only has just one bond that it's sharing with this carbon here which also already has four bonds total. So this bond or this carbon rather is missing three other bonds. And we would assume that those three bonds missing are going to be bonds to hydrogen since we only see that hydrogen is the only other atom in the formula. So filling in we have these three hydrogen bonds. Looking at the next carbon atom to fill in for we have this carbon here which only has three bonds and we need one more bond to hydrogen. So that would apply to almost every carbon in this ring. It needs another bond, 1/4 bond specifically to hydrogen. So filling those in. And now let's focus on oxygen. Since we've fixed all of the carbons that were missing hydrogen bonds or 1/4 bond rather. So looking at oxygen. This one specifically here, we see that it only has one bond and we said that oxygen prefers to have two bonds and two lone pairs. So we're going to fix that by making another bond to hydrogen to this oxygen rather and filling in its two lone pairs on the oxygen itself. And so now this oxygen is stable with a total of 82468 valence electrons around it total. Looking at this oxygen, we see that it does have its two bonds but it's missing its two lone pairs. So let's fill those in. And now moving forward to this oxygen, we see that it has two bonds and is also missing two lone pairs. So we can fill those in accordingly. Yet again, we have this oxygen over here which we can fill in its two lone pairs. It already has its two bonds to carbon here. And after making these fixes, we have completely filled in the corresponding missing hydrogen and lone pairs in our structure of aspirin. So our final answer is going to be our entire structure that we have filled in with our missing hydrogen and lone pairs. I hope that everything I reviewed was clear. If you have any questions, please leave them down below and I'll see everyone in the next practice video.