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 compounds is more stable, okay? So, here we've got negative charge right in between three carbons, right? And here we've got one, two, three, four carbons, so these both have four carbons; but guys, which one of these is going to be more stable? It's actually a lot simpler than you might think to figure this out, right? These are both just carbon compounds, right? And one of these has a negative charge at the end, so you might be thinking "Oh, that's probably more unstable than this one", but no, actually an SP hybridized carbon, this triple bond carbon here, it's going to be much more acidic, right? Which means that it has a more stable conjugate base, right? We know that the conjuga-, that the pKa of this alkane here is going to be about 50, which means that its conjugate base is not very stable, and guys, this is its conjugate base, right? Or if this would just be the conjugate acid, right? This would be the acidic version, even though it's not very acidic at all and this is the conjugate base, right? With a negative charge. Guys, this has a pKa and is certain form of 25 which means that if this conjugate base here is very stable, relative to the other one, right? So guys, this one is going to be our more stable molecule, alright? Let's move on.