Only two lone pairs of electrons on this oxygen now. We have our ring here and we have now a double bond between the oxygen and the carbon. We take the electrons in red and we push them off onto this carbon. That would mean too manyīonds to this carbon. The one in red and so, we can go ahead and draw a resonance structure and we take these electrons in magenta and move then into here. We know one of our patterns is a lone pair next to a pi bond and The resonance structures for the phenoxide anion by doing the other resonance structure just like we did for benzene like that but I'm gonna save that for the end and so, let's think about The benzene ring up above and I could start off for These electrons in here, red and let's make these right here, green and then let's make these blue. Here is the phenoxide anion down here and I'm gonna try toĬolor code the electrons. On a sheet of paper, you could use one or the other but remember that it's actually the hybrid because our dot structuresĪre just not perfect ways to represent molecules or ions. I showed them moving over to here and remember that theĪctual benzene molecule is a hybrid of these two The electrons in green move down to here and then finally, we'll use blue. I'm showing them move to over here and let's make theseĮlectrons over here green. The electrons move over to here, to here and then finally, to here. We draw our resonance brackets and go ahead and draw our other resonance structure for benzene. Many bonds to this carbon and so finally, we take these pi electrons and move them over to here. We have to take these electrons and push them to here, which would mean too We could take these electrons right here. Voiceover: Here is the dot structure for benzene C6H6 and we can draw a resonance structure for this.
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