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 see if we can come up with a resonance structure that's more stable for this guy up here, so we've got this CH3 that can't really resonate, right? Because it's got no lone pairs and it got those three hydrogens directly bonded to it can't, get rid of them, right? Because we know they aren in a resonance structure, we can't move atoms only electrons, right? So then we have this nitrogen over here with three bonds and a lone pair, so it's neutral, and then we've got this nitrogen that's a little bit strange, right? It's got two bonds and one lone pair versus two, which you would normally have, right? And it's got a positive charge because we've got just four electrons there, not five. So, can we do anything that would make this more stable? Well, guys actually yes we can and we know that nitrogen with a positive charge is more stable if it's got four electrons around it with in the form of two double bonds, right? or just more bonds in general, so guys what we can do here is just kick electrons onto this bond, right? And now we don't shift any of these electrons and what we get is the exact same shape, right? Because it looks like this but now we've got our nitrogen with no lone pair on top, right? We've got a triple bond now and then this nitrogen over here has, it's three bonds and one electron a one lone pair, so it's actually in a neutral state but now this one has four bonds and it's positively charged, so that, this is actually the more stable conformation, okay? If you have any questions please feel free to ask, if not, let's move on.