Write a more stable contributing structure for each of the following. Use curved arrows to show how to transform the original Lewis formula to the new one. Be sure to specify formal charges, if any.
So let's go ahead and come up with a resonance structure for this molecule that would make a little bit more sense stability wise, right? We know that our oxygen would rather have the negative charge than our carbon because oxygen is more electronegative, right? So what we're going to do is we're going to kick this lone pair up to here onto this bond but now this carbon has too many bonds, so we need keep these electrons onto this O, right? And originally we had two lone pairs on our O and now we should have three, so we have H2C double bond. Now, we have our carbon here, our hydrogen stays then we have our O, 1, 2, 3 lone pairs, 1, 2, 3 lone pairs and our negative charge, right? So let's go ahead and close this bracket and we're done, okay? So let's move on.