In each case, identify the more stable anion. Explain why it is more stable.
Alright guys. Let's go ahead and figure out which one of these molecules is more stable, okay? it you notice they both have a negative charge, right? they both have a negative charge right here in this center carbon but one of them not only has another carbon, but it's got a double bond next to this negative charge, right? this one doesn't, so which one you think is going to be more stable, the one that can resonate or the one that can't? probably the one that can resonate, right? Let's go ahead and draw the resonance structures for this molecule. so, over here we know, I can actually just go ahead and block this off in our brackets, right? we know that this negative charge, we know that it's actually a lone pair, right? So, we can go ahead and imagine that, we can push that this way and then kick electrons this way, right? So, what we end up getting is something that looks like this, right? We have the same basic structure because we don't move the atoms, but now instead of having our double bond here we have our double bond here and we have our lone pair over here, right? which means we have our negative charge there, okay? So guys, this one can only really exist in one form, right? But this one exist in a combination of these two forms making it more stable. So guys, this one is definitely more stable because it;s allylic and it can resonate, allylic just means next to a double bond, alright? Let's move on.