What is the biggest known difference between rₑ and r₀?

What is the biggest known difference between $$r_e$$ and $$r_0$$? Where $$r_0$$ is the average bond length of the lowest vibrational state, and $$r_e$$ is the location where the potential is lowest.

For a perfect harmonic oscillator, these are the same (notice that the peak probability is exactly at the minimum of the potential): What is the largest known difference between $$r_e$$ and $$r_0$$ in a real molecule?

This is important because the CRC Handbook on Chemistry and Physics almost always gives $$r_0$$ because that's what can be determined more easily from experiment, but ab initio geometry optimization almost always gives $$r_e$$, yet many publications do not even say which type of bond length they are reporting.

• I think what you are asking is, in effect, 'what is the most anharmonic bond?' as this will give the greatest ratio of lengths. Aug 24 '19 at 11:35
• @porphyrin: I thought of asking that too, but as a separate question because I don't think it is guaranteed to have the same answer. Some bonds have a double-well potential, whose solution to the Schrödinger equation (eigenfunction/wavefunction) is not so simple anymore. Likewise in polyatomics the picture is much more complicated than in this diagram. Aug 24 '19 at 11:47
• The largest anharmonic constant $\omega_e\chi_e$ in the CRC book for a diatomic is 121.34 cm$^{-1}$ (for H2). Aug 24 '19 at 23:05
• Keeping things simple, if the average bond length ($r_0$) for $n=0$ is calculated for a Morse potential then the largest deviation from $r_e$ seems to be proportional to the ratio $D_e / \omega_e$. Aug 27 '19 at 17:42
• Good question +1. @porphyrin I think that it is not the same that anharmonicity. I would separate the contributions due the potential as $\mu(V)$ (with $\mu=r(V)-r_e$) into the sum of symmetric and assymetric contributions. The expected value of the symmetric part will be 0, so only the assymetric part contributes to $r_0-r_e$ Sep 22 '19 at 21:33

Let me start by saying that this is a very difficult question to answer because it's not very hard to come up with pathological cases which I will address at the end. Also, as you point out, it is somewhat non-trivial to calculate $$r_0$$ from theory and also somewhat non-trivial to determine $$r_e$$ from experiment. That being said, I think I have a good first suggestion that I am guessing will be hard to beat. I will just answer with theory because this data is more readily available.

$$\ce{F^-(H2O)}$$:

As has been pointed out, this question is very closely related to the anharmonicity of the vibration in question. The $$\ce{O-H}$$ stretch of $$\ce{F^-(H2O)}$$ is the most anharmonic known vibration for a water molecule. This has an experimentally observed vibrational frequency shift of about $$2000~\mathrm{cm^{-1}}$$ which I'm almost sure is the largest known vibrational frequency shift in a molecular complex, where the molecule in question doesn't dissociate.

Now, that being said, this will vary based on the method used, but at the MP2/AVTZ level, $$r_e=1.0653$$ angstroms while $$r_0=1.1248$$ angstroms resulting in a difference of $$0.0595$$ angstroms.

This $$r_0$$ value is calculated from VPT2, which is probably the easiest way to calculate this quantity, but this can fail for certain pathological cases like those I'll discuss below.

$$\ce{H5O2^+Ar}$$:

Ok, now I know that 0.06 angstroms doesn't seem like that huge of a difference, but generally both of these numbers will increase together, so it's hard for them to be all that different. Now, another way you could consider finding a very large difference would be to look for a double-well system where the zero-point energy of the vibration in question is larger than the barrier height.

Now, the zundel cation is a proton shared symmetrically between two water molecules. This is a single well system, however, so $$r_e$$ and $$r_0$$ will be the same and they have a calculated $$\ce{O-H}$$ distance of $$1.202$$ angstroms at the CCSD(T)/aug-cc-pVDZ level of theory.

If, however, we disturb this system ever so slightly, we will break the symmetry and might get the desired behavior. This can be done by tagging the complex with a rare gas atom, which is often done in experiments as it reduces the noise in spectra for reasons I won't get into.

$$\ce{H5O2^+Ar}$$ has a hydronium like complex with an elongated $$\ce{O-H}$$ bond length of $$1.108$$ ansgtroms. It is very likely that the barrier to proton transfer in this case is very small because there is no barrier in the absence of an Argon atom. Therefore, it is likely that the proton will be close to symmetric after vibrational averaging, so if it were perfectly symmetric, we would get an $$r_0$$ of $$1.202$$ angstroms again. It is likely less than this, but it is possible this would lead to a difference greater than $$0.06$$ angstroms which we got from $$\ce{F^-(H2O)}$$.

I should point out that calculating $$r_0$$ for this system is pretty difficult because using VPT2 will almost certainly give nonsensical answers because the harmonic reference is a terrible one, so the perturbation theory will break down. The best option is probably to do diffusion monte carlo and extract the average from the wavefunction directly. It's possible this has been done, but a cursory search of the literature didn't turn anything up.

Also, the data for the first part comes from the SI of ref. and the data for the second part comes from ref..

References:

: Boyer, M. A., Marsalek, O., Heindel, J. P., Markland, T. E., McCoy, A. B., & Xantheas, S. S. (2019). Beyond Badger’s Rule: The Origins and Generality of the Structure–Spectra Relationship of Aqueous Hydrogen Bonds. The journal of physical chemistry letters, 10(5), 918-924.

: Park, M., Shin, I., Singh, N. J., & Kim, K. S. (2007). Eigen and Zundel forms of small protonated water clusters: structures and infrared spectra. The Journal of Physical Chemistry A, 111(42), 10692-10702.