Yeah, let's take a look at this acid Tate Ill. So this is a rudimentary acid Tate ion, just a c o. Negative. And what can happen is well, first, we know that this oxygen has two double bonds. This oxygen iss are two lone pairs and this auction as three loan players. So you know that this oxygen does that speak to hybridized. And we know that this carbon makes three different bonds, is also expected Hybridized this oxygen looks like it's SP three item hybridized. However, what it can do is donate these electrons two residents and we know that if those electrons can engage in residence, they exist in a P orbital, which means that it's in fact, not SB three, but SB two because SP two allows for that free P orbital. So SP two plus p orbital equals residents and that's key. And we need three of them adjacent so that it will involve in resonance. And what we get is, well, something that looks entirely similar to the first structure, where now the negative charges on the top oxygen and of course it can go backwards and go that way. Well, it either way that makes it that the all three of these Adams, the carbon theocracy gin and the other oxygen our SP two hybridized. Now, if we were to select one of these structures, let's go with this one. So we have carbon or so Let's draw the lone pairs on these or at the bonding pairs on these. So when we have a bond or a double bond specifically, well, let's start with a single blow. Single bond is a signal bond, and a Sigma bond is an overlap of SP to Orbital's. In this case, SP two Orbital's on That is a signal bond, and the same can be done with our our group. It's It's an overlap to sharing of those electrons, and the same can be done with this Carbonell carbon. So one of those bonds is a Sigma Bond, s P two. However, there is a pipe bond between this carbon and this oxygen. And what that looks like is, well, r p orbital going to be something like this, and it's not quite a direct overlap. It's more of like an attraction of distant of through distance, but like it za weak poll. But it's not a direct overlap. And that's rpai bond in R P orbital and this oxygen also has. It's lone electron here or lone pair, as a matter of fact, giving it a negative charge because charges exist in the P orbital. No matter what. If there is a charge it exists in the P orbital, there's no way can exist in a hybridized orbital and it has its normal electron pairs, which are in SP hybridize. That should be red, but but yes, so the overlap. The only overlapping orbital's are the SP two orbital's. Those were the only overlapping orbital's to form bonds. The A P orbital doesn't technically overlap to form a bond, it's more of an attraction, but the main overlap is from the SP to hybridize orbital.