The following ball-and-stick molecular model is a representation of acetaminophen, the active ingredient in such over-thecounter headache remedies as Tylenol. (Red = O, gray = C, blue = N, ivory = H.) (b) Indicate the positions of the multiple bonds in acetaminophen.

Video transcript

Welcome back everyone the ball and stick molecular model of metal yellow and as a dye used for plastics is shown below. Complete the structure by identifying positions of multiple bonds present in metal yellow. So we're going to recognize that our gray colored atoms correspond to the atom carbon in models. When we have white colored atoms in our models that corresponds to hydrogen atoms. And when we have blue colored atoms in our models, this will correspond to nitrogen atoms are. Next thing that we want to make note of is bonding preference of these atoms. This is important because this speaks to whether our atoms are honoring our octet rule to be stable. So for carbon, we want to recall that it should have four bonds to have a full octet, Hydrogen We want to recognize only has one valence electron being in group one a and so it should only form one bond to be stable and to have a full octet or rather do it. Now moving on to nitrogen, we would recall that to be stable and to have a full octet. It should have three bonds And one lone pair. So going to our molecule of metal yellow and focusing on our rings here, we can see that the carbon atoms do have three bonds and they're missing 1/ bond. So we're gonna make these carbon stable by adding three sets of double bonds in our rings. And by doing so we can see that these editions of double bonds have allowed these carbon atoms to have a total of four bonds and fuller cut to be stable. We can also see that the hydrogen atoms bonded to the carbons in the ring all have one bond. And so the hydrogen atoms are stable and taken care of. Now moving on to our nitrogen atoms, we can see that these nitrogen atoms have two bonds each, however, they're missing their lone pair as well as a third bond. So we're going to draw the third bond to these nitrogen atoms between each other for a double bond here where we're going to draw their lone pair on each individual nitrogen atom. Now we didn't place it here because we can see that this carbon atom already has four bonds. And so if we were to add a double bond here, that would make that carbon unstable, it would not be able to sustain that. You can only have a maximum of four bonds. So now moving on to this half of our molecule of metal yellow. We see that we do have a nitrogen atom with three bonds and it's missing its lone pair in itself and as far as our carbon atoms outside of rings, we do see that they have four bonds. So with these additions that we've added, this would actually be our final answer for the complete structure of metal yellow with multiple bonds present in our rings here where we have double bonds in the rings as well as double bond between our two nitrogen atoms in the middle of our structure. I hope everything was clear. If you have any questions, please leave them down below and I'll see everyone in the next practice video.