Which of the following ions is more stable? Use resonance to explain your answer.

enter image description here

When we have to compare stability of resonance structures we generally check for the following features in the resonance forms (in sequence):

  1. Neutral molecule;
  2. More covalent bonds;
  3. Complete octet of all the atoms;
  4. Less separation of opposite charges;
  5. Positive charge (if any) on more electro positive atom and negative charge (if any) on more electronegative atom.

In the above problem:

  1. Both the molecules are charged;
  2. Both have same nuber of covalent bonds;
  3. Both have the octet of one carbon atom incomplete (the positively charged one);
  4. Both have positive charges on carbon atoms.

From all of these considerations the molecules should be equally stable. But the answer given in my book is (A).

What is that I can't figure out?

  • 2
    $\begingroup$ For the ions to be equally stable, they would have to be identical. Here, you have a primary allyl carbocation vs. a secondary allyl carbocation. I also didn't get how (A) is more stable though... $\endgroup$ Dec 11 '17 at 16:03
  • 1
    $\begingroup$ One way of reasoning that would lead to determining A as more stable is to ignore the charge and take the cue from the double bond, which is more substituted in A. I also seem to recall that an endo double bond (as in ring system) is more stable than an exo double bond. However, these lines of reasoning are flawed since the two structures are in resonance anyway and, as pointed out by Eashaan Godbole, the primary allyl carbocation of A is less stable than B. $\endgroup$
    – TAR86
    Dec 12 '17 at 6:39
  • 1
    $\begingroup$ "Use resonance "in the question does not make sense $\endgroup$
    – Alchimista
    Dec 12 '17 at 9:46
  • 1
    $\begingroup$ Throw away the book, if it doesn't get this right, there are more distorted and wrong views about chemistry in it. $\endgroup$ Dec 13 '17 at 14:58
  • 1
    $\begingroup$ Throw away the book, if it doesn't get this right, there are more distorted and wrong views about chemistry in it. $\endgroup$ Dec 13 '17 at 14:58

It has been noted in the comments and I shall repeat that the premise of the question is already bogus. The question does not consider two different ions but two mesomeric depiction of the same ion. This is also evident by the mesomeric arrow between the two forms. Since mesomery strictly means that no geometrical change takes place, both depictions are identical in all aspects and have the same (resonance-influenced) energy. Thus, any book claiming that either of the two have a lower energy is wrong.

However, what is commonly done is to determine a more likely resonance structure. This is, for example, commonly used to explain the strongly stabilised nature of certain aromatic systems, e.g. when DMAP (4-N,N′-dimethylaminopyridine) is used as a carboxylic activating agent. We can attempt to do that for your structure, too. If we compare the two we see — of course — that a lot of features are identical. The principal differences are:

  • A has a trisubstituted double bond while B only as a disubstituted (and terminal) double bond
  • B has a secondary carbocation while A has a primary one (both, however, are allylic).

Since allylic stabilisation for cations is much stronger than hyperconjugation, we can discard the second bullet point as being essentially equal for both resonance structures. Thus, we should argue with the location of the double bond. Both double bonds can benefit from hyperconjugation twice (the primary cation of A cannot hyperconjugate due to geometry), but in A the two hyperconjugations stabilise different carbons. Along with the general double bond stability given as:

$$\text{monosubstituted} < \text{terminal disubstituted} < \textit{cis} < \textit{trans} < \text{trisubstituted} < \text{tetrasubstituted}$$

we can identify A as being slightly better than B and therefore contributing slightly more towards the overall structure.

You mentioned in the comments that your book states:

structure B is not planar and hence conjugation is not possible in it

Your book probably wants you to assume that the following depiction in figure 1 is adequate for the two resonance forms:

The book’s intended way of drawing the structures with geometry difference
Figure 1: structures B and A under the assumption of a chair-configured cyclohexyl structure for B.

Under the underlying assumption of a different geometry for both structures, this may be valid. However, there is no way that cation B will adopt a chair cyclohexane configuration. Instead, as I mentioned above, the following structures in figure 2 are much more likely and even show that we are dealing with resonance:

A better depiction of the two ions not required a change in geometry
Figure 2: depiction of the mesomeric forms without geometry change.

You can easily see that the argument of non-conjugation is bogus, since there very well is a way to optimise geometry so that the orbitals may form an allyl system.


The question got mangled when it was copied and posted on the internet. It should read (I recreated the missing image):

Which structure, I or II, is more stable? Use resonance in your answer. enter image description here

And of course it is the allylic carbocation, I, as explained in the answer key that is available on the internet (see e.g. Comparing stability of two canonical structures).

Here is an image of the original question (part d): enter image description here

And here another one: enter image description here

  • $\begingroup$ Makes more sense now! Where did you find them? $\endgroup$
    – user55119
    2 days ago
  • $\begingroup$ Google “for the following pair of ions which one is more stable”. @user55119 $\endgroup$ 2 days ago
  • $\begingroup$ Or “Which of the following ions is more stable? Use resonance to explain your answer.” $\endgroup$ 2 days ago

Your Answer

By clicking “Post Your Answer”, you agree to our terms of service, privacy policy and cookie policy

Not the answer you're looking for? Browse other questions tagged or ask your own question.