Which of the following compounds has the longest bond length?

(A) $\ce{H3C-CF3}$
(B) $\ce{FCH2-CH2F}$
(C) $\ce{F2CH-CHF2}$
(D) $\ce{F3C-CF3}$

My logic was based on the relative electronegativities of the two carbons. The more fluorines there are on one carbon, the more polarised the C-C bond will be, and the longer the C-C bond length will be (since the bond is weakened). Thus, I think that the answer is A.

Is this right?


2 Answers 2


Actually, the more the polarization of a bond, the stronger it is, since both the atoms are drawn close together due to electrostatic attraction, decreasing the bond length and increasing the bond stability (think about ionic bonds. Your reasoning would dictate them to be very weak, while we know how strong they are!). Actually, I would predict $\ce{CH3-CF3}$ to have a really small bond length (the bond is probably the strongest, would someone confirm this please?), since the fluorinated carbon has quite a positive charge, while the other one is relatively negatively charged (not negative in the absolute, just relative to the other carbon).

All the remaining options have equal number of fluorines on either carbon, differing only in their number. These three are tricky. Consider $\ce{CF3-CF3}$. Both of its carbons are severely deficient in electrons. Each badly needs electrons, and since it can't argue with fluorine (fluorine is an unreasonable bully), so both carbons try to drag the shared pair of electrons towards itself. This ultimately results in them both coming closer to each other. As we reduce the number of fluorines on each carbon, their desparation is reduced, thus increasing the bond length. Thus the answer is (B).

Edit: If @pentavalentcarbon's calculations of bond lengths are correct, then my reasoning was too simplistic, and indeed it seems so now. So if we dig deeper, $\ce{CH2F-CH2F}$ could have the second smallest bond length and $\ce{CF3-CF3}$. Why? Well, it is because of hyperconjugation, similar to the gauche effect (read it up to get better understanding of the gauche effect, although I explain it in short here also).

So, what happens is that in the case of $\ce{CH2F-CH2F}$, the bonding C-H molecular orbital (MO) overlaps with the antibonding C-F MO, transferring some of its electron density to the C-F MO (see diagram). This interaction is stabilizing (since delocalization of electrons stabilizes the molecule), and also introduces slight double bond character in the C-C sigma bond, thus serving to shorten it.

Now in $\ce{CH2F-CH2F}$, there will be two such interactions, but then there are also two such interactions in $\ce{CHF2-CHF2}$! There is a difference though. In the latter case, there are two fluorines on each carbon, which heavily draw electron density away from the carbon through the sigma bonds. This decreases the sigma bond density in the C-H bond, which being poor in electrons, gives relatively low stabilization when overlapping with the antibonding C-F MO. So $\ce{CHF2-CHF2}$ has a slightly higher bond length than $\ce{CH2F-CH2F}$.

Using this same reasoning, we can see why $\ce{CH3-CF3}$ has the smallest bond length (three favourable hyperconjugational interactions!) and $\ce{CF3-CF3}$ has the longest bond length (no hyperconjugation).

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    $\begingroup$ I calculated the bond lengths to be (in angstrom) A: 1.511 B: 1.526 C: 1.544 D: 1.573. $\endgroup$ Commented Sep 28, 2016 at 20:10
  • $\begingroup$ @pentavalentcarbon Your comment suggests that my answer and the textbook's answer is wrong. Either I am missing something or there is quantum mechanics involved. I am also curious, so could you add an answer of your own too, please? I would love to understand the reasons behind it! $\endgroup$ Commented Sep 29, 2016 at 6:27
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    $\begingroup$ I agree with the newer edit. Penta's calculations make a lot of sense too. I expect the gauche effect to shorten the bond length, in accordance with the resonance form that Jan drew here involving a C=C double bond. Ah, you mentioned the slight double bond character too! Very good. I would, however, say that the gauche effect is a specific example of hyperconjugation (which is a very general term). +1 anyway. $\endgroup$ Commented Sep 29, 2016 at 8:00
  • $\begingroup$ So to summarise things as I understand it so far: hyperconjugation (shortens bond) competes with electron withdrawal by F atoms (repulsion lengthens). The effect is best seen compared to ethane which has a bond length 153.5. Therefore structures (A) and (B) are shorter, just, due to hyperconjugation being dominant, (C) the two effects just about balance and (D) repulsion of C-C nuclei make bond stronger due to electron withdrawal by F atoms. Do the experimental bond lengths support this? $\endgroup$
    – porphyrin
    Commented Sep 29, 2016 at 8:25
  • $\begingroup$ @porphyrin You could say so, but instead of treating it as C-C nucleic repulsion, I feel that it should be treated as which molecule shows more hyperconjugation effect! I didn't find any good sources for experimental bond lengths for these molecules. $\endgroup$ Commented Sep 29, 2016 at 10:15

Many of these cases hinge on some weird effect. Evidently the gauche form of 1,2-Difluoroethane is more stable than the anti form which is sort of weird.

This wikipedia article on the Gauche Effect list CC bond of gauche 1,2-Difluoroethane as 150 pm and anti form as 151.4 pm.

This reference says 151.2 pm for C-C bond in 1,1,2,2-tetrafluoroethane. (High-Resolution Microwave and Infrared Molecular-Beam Studies of the Conformers of 1,1,2,2-Tetrafluoroethane, Stephen C. Stone et al., Journal of Molecular Spectroscopy 192, 75–85 (1998).)

This reference says the C-C bond length is shorter for hexafluoroethane than then the corresponding hydrocarbon. (Fluorocarbon and Related Chemistry By R. E. Banks, M. G. Barlow, ISBN-13: 978-0851865140, page 10.)

This answer on this website says ethane C-C bond is 153.51 pm.

So to summarize: $$ \small \begin{array}{lcc} \hline \text{Compound} & \text{Bond Length (pm)}\\ \hline \text{gauche 1,2-difluoroethane} & 150 \\ \text{anti 1,2-difluoroethane} & 151.4 \\ \text{1,1,2,2-tetrafluoroethane} & 151.2 \\ \text{Hexafluoroethane} & \text{<ethane C-C} \\ \text{Ethane} & 153.51 \\ \hline \end{array} $$


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