Bonding, Structure, and Resonance
How To Find The Best Resonance Structure By Applying Electronegativity
Last updated: November 26th, 2019 |
Finding The Best (And Second-Best) Resonance Structures By Applying Electronegativity
The last time I talked about evaluating resonance structures the molecules were, to be honest – pretty simple. Evaluating the resonance structures of ethene, the allyl carbocation, and the allyl carbanion are a pretty far cry from some of the more complicated structures you’ll see in a typical course.
So today let’s get started with how to evaluate non-equivalent resonance structures from pi bonds.
Table of Contents
- Always Break A Pi Bond So As To Put The Electrons On The More Electronegative Atom
- Evaluating The Resonance Structures Of Acetone (Propanone)
- Evaluating The Resonance Structures Of An Imine
- Evaluating The Resonance Structures Of The Acetate Ion
- Apply The Rule Of Electronegativity To Determine The “Second-Best” Resonance Structures For These Molecules
So today I thought I’d start to talk about the (much more common) situation when you have a π bond between two dissimilar atoms. How do you evaluate the resonance forms in these cases?
We’re going to have to go back to using our old friendly measuring stick, electronegativity for this task. Here’s the bottom line lesson for the resonance structures we’ll evaluate today.
Hopefully this makes some sense! Charged resonance forms are less stable than neutral resonance forms. So if we absolutely must form a charged resonance form, it makes sense to put the negative charge on the atom best able to stabilize it. How do we know which atoms stabilize negative charge the best? Well, a pKa table will give you a really good idea. But beyond that, if you look at the five key factors that influence acidity, one of the most important factors is the electronegativity of an atom. After all, electronegativity is ultimately a measure of to what extent an atom is able to stabilize negative charge.
So hopefully it should come as no surprise as we walk through these three examples that the second-best resonance forms are the ones where negative charge ends up on the more electronegative atom.
Let’s start by looking at a simple carbonyl compound, acetone (2-propanone).
If we look at the possible curved-arrow “moves” for drawing the resonance forms of this molecule, there’s two possibilities. In the first possibility, we draw an arrow from the π bond to the oxygen atom, putting a negative charge on the oxygen and leaving behind a positive charge on the carbon.
In the second, we’re making the carbon negative and leaving behind a positive charge on the oxygen. Not only is there a positive charge on the oxygen, it has less than a full octet. This is an extremely unstable situation.
So hopefully it’s clear that the resonance form where there is a negative charge on oxygen is the second-best resonance form next to the neutral one, and the resonance form where there is a negative charge on carbon is insignificant. Experiment bears this out. Calculations of the charge density on acetone reveal that the carbon is electropositive and the oxygen is electronegative, as per what we’d expect from electronegativity differences. So the molecule can be thought of as a hybrid of the best and second-best resonance forms.
Likewise, the resonance forms for the imine below similar behavior. As expected, calculations of electron density for this imine show that there is considerable positive charge density on the carbon and a high density of negative charge on the nitrogen. As you’d expect, the resonance form where there’s negative charge on carbon gets very little weight.
Finally we come to the acetate ion, which we discussed previously. Again, the second-best resonance form is that where there’s a positive charge on the carbon (and the worst is the one where it bears a negative charge).
5. Apply The Rule Of Electronegativity To Determine The “Second-Best” Resonance Structures For These Molecules
With these examples in mind, can you apply the rule to determine the “second-best” resonance forms for each of these molecules?
Next time I’ll go into a few more details on evaluating resonance forms based on lessons we learn from acidity and basicity.