Posts Tagged ‘chemical shifts’

(another) WATOC 2017 report.

Tuesday, August 29th, 2017

Another selection (based on my interests, I have to repeat) from WATOC 2017 in Munich.

  1. Odile Eisenstein gave a talk about predicted 13C chemical shifts in transition metal (and often transient) complexes, with the focus on metallacyclobutanes. These calculations include full spin-orbit/relativistic corrections, essential when the carbon is attached to an even slightly relativistic element. She noted that the 13C shifts of the carbons attached to the metal fall into two camps, those with δ ~+80 ppm and those with values around -8 ppm. These clusters are associated with quite different reactivities, and also seem to cluster according to the planarity or non-planarity of the 4-membered ring. There followed some very nice orbital explanations which I cannot reproduce here because my note taking was incomplete, including discussion of the anisotropy of the solid state spectra. A fascinating story, which I add to here in a minor aspect. Here is a plot of the geometries of the 52 metallacyclobutanes found in the Cambridge structure database. The 4-ring can be twisted by up to 60° around either of the C-C bonds in the ring, and rather less about the M-C bonds. There is a clear cluster (red spot) for entirely flat rings, and perhaps another at around 20° for bent ones, but of interest is that it does form something of a continuum. What is needed is to correlate these geometries with the observed 13C chemical shifts to see if the two sets of clusters match. I include this here because in part such a search can be done in “real-time” whilst the speaker is presenting, and can then be offered as part of the discussion afterwards. It did not happen here because I was chairing the meeting, and hence concentrating entirely on proceedings!

  2. Stefan Grimme introduced his tight binding DFT method, an ultra fast procedure for computing large molecules and in passing noted the arrival of his D4 procedure (almost everyone currently uses D3 methods for this, including many of the results reported on this blog) for correcting for dispersion energies in molecules based on computed charge dependencies using the TBDFT methods. Thus we see dispersion as a property which is based on the wavefunction of the molecule, but still fast enough to accurately correct dispersion energies. He followed this with his automated procedures based on the TBDFT methods for computing full spin-spin coupled 1H NMR spectra of organic molecules. The core of this method is to recognise conformational and rotational freedoms and to compute the NMR properties for all identified isomers. These parameters are then Boltzmann averaged prior to computation of the final spin-coupled simulated frequency domain spectrum (rather than inverting this procedure by computing spin-coupled spectra of all rotamers and conformations and then averaging the spectral envelopes). This should widely revolutionise the interpretation of 1H NMR spectra by synthetic chemists.
  3. Another automated tool for synthetic chemists was presented by Jan Jenson, and can be seen here. It used MOPAC PM3 semi-empirical theory to compute relative proton affinities for a series of regioisomers as a prelude to predicting the position of aromatic electrophilic substitutions in heteroaromatic molecules. Try it out by putting a SMILES string into the box provided (e.g. COC1=CC=CC=C1) waiting a bit and seeing what the prediction is (it should be p- for the preceding example). During Q&A, a question was asked about the canonical “purity” of the SMILES (the one used in this tool comes from the Chemdraw program, which might not be identical to a SMILES for the same molecule produced by a different program), and whether an InChI descriptor might be better (also produced by Chemdraw, but perhaps a bit more canonical). Also asked was whether the prediction for an electrophile rather larger than a proton might not give good predictions? This one perhaps could be tested by readers, who could report back here?
  4. Walter Thiel completes the semi-empirical theme when he reported the new ODM2 method, the D now including dispersion. This is a powerful program, which includes e.g. full CI (configuration interaction + gradients) capability and is especially good for excited states, for dynamic simulations, and for combining these into dynamic photochemical simulations. This was applied to the chromophore in the famous “nanocar” in studying the dynamics of the photochemical rotation of the motor of the car (the thermally induced rotation was not studied). At the time that the nanocar caught my attention, I wondered about how the four independent molecular motors synchronised their rotations to allow the car to drive in a straight line. No doubt the answer is known, and if anyone reading this knows, please tell! It is probably a dynamics problem on four rotors (Walter reported just on one!).

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Dispersion “bonds”: a new example with an ultra-short H…H distance.

Monday, June 26th, 2017

About 18 months ago, there was much discussion on this blog about a system reported by Bob Pascal and co-workers containing a short H…H contact of ~1.5Å[1]. In this system, the hydrogens were both attached to Si as Si-H…H-Si and compressed together by rings. Now a new report[2] and commented upon by Steve Bachrach, claims a similar distance for hydrogens attached to carbon, i.e. C-H…H-C, but without the ring compression.

This new example is the structure of an C3-symmetric all-meta tBu-triphenylmethane R-H…H-R dimer determined by neutron diffraction (DOI: 10.5517/ccdc.csd.cc1nc1bd) and the close interaction is achieved purely by attractions due to dispersion forces accumulating in the remainder of the molecules. This study also reports a diverse set of computed properties for this new system, but one property reported as part of the previous discussion was not presented, the 1JH-H coupling constant. I have computed it here in the hope that it might be possible to measure by some means, perhaps in the solid state?

The chemical shift of the R3CH proton is measured as a singlet‡ at ~7.35 ppm (in deuterated benzene, Figure S6, SI).† 

The value calculated using B3LYP/Def2-TZVPP (gas phase) is 7.39 and 7.69 ppm (averaged to 7.54 for a rapidly exchanging environment). The 1J coupling is calculated as 4.3 Hz at the B3LYP/Def2-TZVPP level, DOI: 10.14469/hpc/2699. The designation 1J is normally taken as a 1-bond pathway for the coupling. In this example, the designation of the H-H region as a “bond” is the interesting discussion point!

I end by noting here my observation that although the neutron diffraction study of ammonium tetraphenylborate shows the  N-H protons as pointing directly towards the centroid of phenyl groups, the original observation[3] was made that “even at 20 K the ammonium ion performs large amplitude motions which allow the N-H vectors to sample the entire face of the aromatic system”.  The equivalent thermal motion for the triphenylmethane system here would have the  C-H vectors orbiting around each other in a manner that increases the H-H separation, but which averages out to them pointing directly towards one another?  The calculated normal coordinate analysis of this system is not available from the article SI, so the ease of  C-C-H bending to achieve such motion is difficult to ascertain. Perhaps trying to detect the 1J coupling might illuminate whether this happens?

Postscript. †Prof Schreiner has indicated that that the methine assignment is 5.79 ppm (b below) and not 7.35 as marked with a diamond in the S6 figure caption (a below). This is of course measured in d6-benzene solution and applies to the monomer, not presumably the dimer. The calculated value of 7.54 ppm as reported above applies specifically to the dimer, which suggests a significant shift of ~2ppm upon dimer formation. It would be interesting to verify this prediction via a solid-state measurement.

‡Measuring coupling would require an asymmetric environment to differentiate the two chemical shifts of the interacting hydrogens. Although the C3 symmetry of the crystal structure could provide such an environment, it is observed to be fluxional in solution,  which equalises the two chemical shifts on the NMR time scale. Two non-equivalent protons exhibiting only mutual couplings manifest as an AB-type double doublet of peaks in the NMR spectrum. As the difference in chemical shift between the two nuclei (in units of Hz) approaches in magnitude the value of the coupling constant between them (also in Hz), the AB quartet becomes increasingly second-order in appearance. This means that the intensities of the two outer peaks starts to decrease and the two inner peak intensities increase. When the chemical shift difference between them reaches zero, the intensity of the two outer peaks also becomes zero and the two inner peaks superimpose to become a single peak. This means that the coupling constant cannot be measured from the splitting of the peaks (which has vanished). It does not mean of course that the coupling itself has vanished; it merely no longer manifests in the spectrum.

References

  1. J. Zong, J.T. Mague, and R.A. Pascal, "Exceptional Steric Congestion in an <i>in</i>,<i>in</i>-Bis(hydrosilane)", Journal of the American Chemical Society, vol. 135, pp. 13235-13237, 2013. https://doi.org/10.1021/ja407398w
  2. S. Rösel, H. Quanz, C. Logemann, J. Becker, E. Mossou, L. Cañadillas-Delgado, E. Caldeweyher, S. Grimme, and P.R. Schreiner, "London Dispersion Enables the Shortest Intermolecular Hydrocarbon H···H Contact", Journal of the American Chemical Society, vol. 139, pp. 7428-7431, 2017. https://doi.org/10.1021/jacs.7b01879
  3. T. Steiner, and S.A. Mason, "Short N<sup>+</sup>—H...Ph hydrogen bonds in ammonium tetraphenylborate characterized by neutron diffraction", Acta Crystallographica Section B Structural Science, vol. 56, pp. 254-260, 2000. https://doi.org/10.1107/s0108768199012318

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Posted in Interesting chemistry | 3 Comments »

Dispersion "bonds": a new example with an ultra-short H…H distance.

Monday, June 26th, 2017

About 18 months ago, there was much discussion on this blog about a system reported by Bob Pascal and co-workers containing a short H…H contact of ~1.5Å[1]. In this system, the hydrogens were both attached to Si as Si-H…H-Si and compressed together by rings. Now a new report[2] and commented upon by Steve Bachrach, claims a similar distance for hydrogens attached to carbon, i.e. C-H…H-C, but without the ring compression.

This new example is the structure of an C3-symmetric all-meta tBu-triphenylmethane R-H…H-R dimer determined by neutron diffraction (DOI: 10.5517/ccdc.csd.cc1nc1bd) and the close interaction is achieved purely by attractions due to dispersion forces accumulating in the remainder of the molecules. This study also reports a diverse set of computed properties for this new system, but one property reported as part of the previous discussion was not presented, the 1JH-H coupling constant. I have computed it here in the hope that it might be possible to measure by some means, perhaps in the solid state?

The chemical shift of the R3CH proton is measured as a singlet‡ at ~7.35 ppm (in deuterated benzene, Figure S6, SI).† 

The value calculated using B3LYP/Def2-TZVPP (gas phase) is 7.39 and 7.69 ppm (averaged to 7.54 for a rapidly exchanging environment). The 1J coupling is calculated as 4.3 Hz at the B3LYP/Def2-TZVPP level, DOI: 10.14469/hpc/2699. The designation 1J is normally taken as a 1-bond pathway for the coupling. In this example, the designation of the H-H region as a “bond” is the interesting discussion point!

I end by noting here my observation that although the neutron diffraction study of ammonium tetraphenylborate shows the  N-H protons as pointing directly towards the centroid of phenyl groups, the original observation[3] was made that “even at 20 K the ammonium ion performs large amplitude motions which allow the N-H vectors to sample the entire face of the aromatic system”.  The equivalent thermal motion for the triphenylmethane system here would have the  C-H vectors orbiting around each other in a manner that increases the H-H separation, but which averages out to them pointing directly towards one another?  The calculated normal coordinate analysis of this system is not available from the article SI, so the ease of  C-C-H bending to achieve such motion is difficult to ascertain. Perhaps trying to detect the 1J coupling might illuminate whether this happens?

Postscript. †Prof Schreiner has indicated that that the methine assignment is 5.79 ppm (b below) and not 7.35 as marked with a diamond in the S6 figure caption (a below). This is of course measured in d6-benzene solution and applies to the monomer, not presumably the dimer. The calculated value of 7.54 ppm as reported above applies specifically to the dimer, which suggests a significant shift of ~2ppm upon dimer formation. It would be interesting to verify this prediction via a solid-state measurement.

‡Measuring coupling would require an asymmetric environment to differentiate the two chemical shifts of the interacting hydrogens. Although the C3 symmetry of the crystal structure could provide such an environment, it is observed to be fluxional in solution,  which equalises the two chemical shifts on the NMR time scale. Two non-equivalent protons exhibiting only mutual couplings manifest as an AB-type double doublet of peaks in the NMR spectrum. As the difference in chemical shift between the two nuclei (in units of Hz) approaches in magnitude the value of the coupling constant between them (also in Hz), the AB quartet becomes increasingly second-order in appearance. This means that the intensities of the two outer peaks starts to decrease and the two inner peak intensities increase. When the chemical shift difference between them reaches zero, the intensity of the two outer peaks also becomes zero and the two inner peaks superimpose to become a single peak. This means that the coupling constant cannot be measured from the splitting of the peaks (which has vanished). It does not mean of course that the coupling itself has vanished; it merely no longer manifests in the spectrum.

References

  1. J. Zong, J.T. Mague, and R.A. Pascal, "Exceptional Steric Congestion in an <i>in</i>,<i>in</i>-Bis(hydrosilane)", Journal of the American Chemical Society, vol. 135, pp. 13235-13237, 2013. https://doi.org/10.1021/ja407398w
  2. S. Rösel, H. Quanz, C. Logemann, J. Becker, E. Mossou, L. Cañadillas-Delgado, E. Caldeweyher, S. Grimme, and P.R. Schreiner, "London Dispersion Enables the Shortest Intermolecular Hydrocarbon H···H Contact", Journal of the American Chemical Society, vol. 139, pp. 7428-7431, 2017. https://doi.org/10.1021/jacs.7b01879
  3. T. Steiner, and S.A. Mason, "Short N<sup>+</sup>—H...Ph hydrogen bonds in ammonium tetraphenylborate characterized by neutron diffraction", Acta Crystallographica Section B Structural Science, vol. 56, pp. 254-260, 2000. https://doi.org/10.1107/s0108768199012318

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Posted in Interesting chemistry | 3 Comments »

Molecule of the year? “CrN123”, a molecule with three different types of Cr-N bond.

Friday, December 16th, 2016

Here is a third candidate for the C&EN “molecule of the year” vote. This one was shortlisted because it is the first example of a metal-nitrogen complex exhibiting single, double and triple bonds from different nitrogens to the same metal[1] (XUZLUB has a 3D display available at DOI: 10.5517/CC1JYY6M). Since no calculation of its molecular properties was reported, I annotate some here.

Firstly, the 14N spectra were recorded, and so it is of interest to see if the chemical shifts reported can be replicated using calculation (ωB97XD/Def2-TZVPP/SCRF=thf). The method selected is not in the least “optimised” for this nucleus; it is often the case that various permutations of functional and basis set must be probed for the best combination for any particular nucleus. Another limitation of the calculation is that it has been done without the (rather large) counterion in place; a full model should certainly include this. The shifts below are referenced with respect to the internal N≡N signal reported at 310 ppm. The calculations have DOI: 10.14469/hpc/1980 (N2) and 10.14469/hpc/1983 (CrN123).

Nucleus N-Cr N=Cr N≡Cr
N(obs,thf), ppm 214 560 963
N(calc,thf), ppm 213;223 558 1093

The match is reasonable for three nitrogens; less so for the Cr≡N variety (DOI: 10.14469/hpc/1982) but no doubt could be improved by playing with the method as noted above and probably also correcting for spin-orbit coupling perturbations of the N nucleus by the Cr nucleus. The 14N shifts of quite a number of other intermediates in the synthesis of this molecule are reported and having a method to hand which can be used to check if the structural assignment matches that calculated for it is always useful. 

Next, I have a look at the nature of the Cr-N bonds themselves. The observed lengths are Cr-N: 1.863 (1.862) 1.881 (1.873); Cr=N 1.736 (1.714); Cr≡N 1.556 (1.518)Å. Calculated values in parentheses. To put this into context, I show CSD (Cambridge structure database) searches (search query DOI:10.14469/hpc/1981) for the three types of CrN bond. Firstly the triple bond (65 examples) which reveals the most probable value of ~1.54Å. This matches fairly well with the above values.

Next, Cr=N (50 examples) with a most probable value of 1.65Å. The value reported for CrN123 (1.736Å) is quite a bit longer for this bond. Again a caveat; the searches specified the bond type exactly, and this does then depend very much on how each entry in the CSD was indexed, by humans perceiving the structure and assigning the bond type on the basis of their expert chemical knowledge. It is quite likely that these integer assignments are at best informed estimates and at worst poor guesses. 

Finally, Cr-N (1398 examples) with the most probable value of 2.07Å which is a fair bit longer than the two values for CrN123. There are relatively few examples in the region of 1.87Å, which is where the CrN123 values come.

If one repeats this search, but limiting the N atom to carrying two carbons as well as a bond to Cr (as in NPri2) one gets the surprise of a bimodal (perhaps even trimodal) distribution, with an additional cluster at lengths of 1.82Å, in closer agreement with CrN123. Again I remind of the caveat that “single” bonds are often assigned by human curators on the basis of perceived chemistry. It would nevertheless be interesting to tunnel down to the possible explanation of this bimodal feature.

These comparisons suggest that in CrN123, the three types of bond are not isolated but may be interacting electronically in a complex manner to increase the bond order of the nominal Cr-NR2 “single” bonds (Cr=N(+)R2) whilst decreasing that of the nominal Cr=N “double” bond. 

Try try to quantify the bond properties a bit more, I tried the ELF basin population technique. ELF (electron localization function) is one method of partitioning the electron density in the molecule into well defined regions or basins (which we call bonds). The results (DOI: 10.14469/hpc/1984) came out Cr-N 4.05 and 4.01e, each comprising two basins which is often typical of a bond with significant π character. The integration for a single bond is of course 2.0. The Cr=N bond was 5.07e in two basins and that for the Cr≡N 3.26e (far removed from ~6.0 in a triple bond). The valence shell total is 16.4e. These values could be said to be “challenging”, perhaps hinting that the bonding and electron density distribution in this molecule is not quite what it seems. Certainly worth a more detailed look with other methods of bond partitioning.

Well, with M123 synthesized, are there any prospects of a M1234 complex being discovered? (quadruple bonds to N HAVE been suggested!).

References

  1. E.P. Beaumier, B.S. Billow, A.K. Singh, S.M. Biros, and A.L. Odom, "A complex with nitrogen single, double, and triple bonds to the same chromium atom: synthesis, structure, and reactivity", Chemical Science, vol. 7, pp. 2532-2536, 2016. https://doi.org/10.1039/c5sc04608d

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Posted in crystal_structure_mining, Interesting chemistry | 10 Comments »

Molecule of the year? "CrN123", a molecule with three different types of Cr-N bond.

Friday, December 16th, 2016

Here is a third candidate for the C&EN “molecule of the year” vote. This one was shortlisted because it is the first example of a metal-nitrogen complex exhibiting single, double and triple bonds from different nitrogens to the same metal[1] (XUZLUB has a 3D display available at DOI: 10.5517/CC1JYY6M). Since no calculation of its molecular properties was reported, I annotate some here.

Firstly, the 14N spectra were recorded, and so it is of interest to see if the chemical shifts reported can be replicated using calculation (ωB97XD/Def2-TZVPP/SCRF=thf). The method selected is not in the least “optimised” for this nucleus; it is often the case that various permutations of functional and basis set must be probed for the best combination for any particular nucleus. Another limitation of the calculation is that it has been done without the (rather large) counterion in place; a full model should certainly include this. The shifts below are referenced with respect to the internal N≡N signal reported at 310 ppm. The calculations have DOI: 10.14469/hpc/1980 (N2) and 10.14469/hpc/1983 (CrN123).

Nucleus N-Cr N=Cr N≡Cr
N(obs,thf), ppm 214 560 963
N(calc,thf), ppm 213;223 558 1093

The match is reasonable for three nitrogens; less so for the Cr≡N variety (DOI: 10.14469/hpc/1982) but no doubt could be improved by playing with the method as noted above and probably also correcting for spin-orbit coupling perturbations of the N nucleus by the Cr nucleus. The 14N shifts of quite a number of other intermediates in the synthesis of this molecule are reported and having a method to hand which can be used to check if the structural assignment matches that calculated for it is always useful. 

Next, I have a look at the nature of the Cr-N bonds themselves. The observed lengths are Cr-N: 1.863 (1.862) 1.881 (1.873); Cr=N 1.736 (1.714); Cr≡N 1.556 (1.518)Å. Calculated values in parentheses. To put this into context, I show CSD (Cambridge structure database) searches (search query DOI:10.14469/hpc/1981) for the three types of CrN bond. Firstly the triple bond (65 examples) which reveals the most probable value of ~1.54Å. This matches fairly well with the above values.

Next, Cr=N (50 examples) with a most probable value of 1.65Å. The value reported for CrN123 (1.736Å) is quite a bit longer for this bond. Again a caveat; the searches specified the bond type exactly, and this does then depend very much on how each entry in the CSD was indexed, by humans perceiving the structure and assigning the bond type on the basis of their expert chemical knowledge. It is quite likely that these integer assignments are at best informed estimates and at worst poor guesses. 

Finally, Cr-N (1398 examples) with the most probable value of 2.07Å which is a fair bit longer than the two values for CrN123. There are relatively few examples in the region of 1.87Å, which is where the CrN123 values come.

If one repeats this search, but limiting the N atom to carrying two carbons as well as a bond to Cr (as in NPri2) one gets the surprise of a bimodal (perhaps even trimodal) distribution, with an additional cluster at lengths of 1.82Å, in closer agreement with CrN123. Again I remind of the caveat that “single” bonds are often assigned by human curators on the basis of perceived chemistry. It would nevertheless be interesting to tunnel down to the possible explanation of this bimodal feature.

These comparisons suggest that in CrN123, the three types of bond are not isolated but may be interacting electronically in a complex manner to increase the bond order of the nominal Cr-NR2 “single” bonds (Cr=N(+)R2) whilst decreasing that of the nominal Cr=N “double” bond. 

Try try to quantify the bond properties a bit more, I tried the ELF basin population technique. ELF (electron localization function) is one method of partitioning the electron density in the molecule into well defined regions or basins (which we call bonds). The results (DOI: 10.14469/hpc/1984) came out Cr-N 4.05 and 4.01e, each comprising two basins which is often typical of a bond with significant π character. The integration for a single bond is of course 2.0. The Cr=N bond was 5.07e in two basins and that for the Cr≡N 3.26e (far removed from ~6.0 in a triple bond). The valence shell total is 16.4e. These values could be said to be “challenging”, perhaps hinting that the bonding and electron density distribution in this molecule is not quite what it seems. Certainly worth a more detailed look with other methods of bond partitioning.

Well, with M123 synthesized, are there any prospects of a M1234 complex being discovered? (quadruple bonds to N HAVE been suggested!).

References

  1. E.P. Beaumier, B.S. Billow, A.K. Singh, S.M. Biros, and A.L. Odom, "A complex with nitrogen single, double, and triple bonds to the same chromium atom: synthesis, structure, and reactivity", Chemical Science, vol. 7, pp. 2532-2536, 2016. https://doi.org/10.1039/c5sc04608d

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Posted in crystal_structure_mining, Interesting chemistry | 10 Comments »

Hydrogen bonding to chloroform.

Monday, November 14th, 2016

Chloroform, often in the deuterated form CDCl3, is a very common solvent for NMR and other types of spectroscopy. Quantum mechanics is increasingly used to calculate such spectra to aid assignment and the solvent is here normally simulated as a continuum rather than by explicit inclusion of one or more chloroform molecules. But what are the features of the hydrogen bonds that form from chloroform to other acceptors? Here I do a quick search for the common characteristics of such interactions.

  1. This first search (R < 0.05, no errors, no disorder) is for interactions from the CH… O, and is a plot of that distance against the angle subtended at the oxygen.

    clcho-rt

    Note that there are not that many crystalline examples. The “hotspot” is at a distance of ~2.3Å, but real examples down to 1.9Å exist. The angle subtended at the oxygen is close to 120° (the angle subtended at the hydrogen is always close to 180°). The plot below constrains the search to data collected below 140K to reduce the thermal noise in the measurements, with the hotspot shortening slightly to 2.2Å. clcho-140

  2. The next search is for interactions to N rather than O (T < 140K). There are rather fewer hits, but again with similar features.clchn-140
  3. Finally, an attempt to see if there is a correlation between the C-H length and the H…O length. ch-vs-co

    This has odd characteristics, which suggests that in most cases the C-H distance is not measured from the diffraction data but simply “idealised” (and which therefore renders this plot meaningless). Unless its been added recently, it is not possible to specify in the search how the hydrogen positions have been refined, if at all and hence to restrict the search only to those structures where the C-H distance is meaningful.

In the last ten years or so, great progress has been made in assigning experimental spectra with the help of quantum calculations. This is true of chemical shifts in NMR, but especially so for chiroptical measurements such as ORP, ECD and VCD. Given that explicit hydrogen bonds can introduce anisotropy into the otherwise isotropic solvent continuum, it might be worth including perhaps one chloroform molecule into these calculations, especially if the  CH…O distance is <2Å (which suggests it is fairly strong). If nothing else, chloroform is rather big and might exert effects based on dispersion attractions or steric repulsions as well as the H-bonding.

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The NMR spectra of methano[10]annulene and its dianion. The diatropic/paratropic inversion.

Saturday, October 26th, 2013

The 1H NMR spectrum of an aromatic molecule such as benzene is iconic; one learns that the unusual chemical shift of the protons (~δ 7-8 ppm) is due to their deshielding by a diatropic ring current resulting from the circulation of six aromatic π-electrons following the Hückel 4n+2 rule. But rather less well-known is the spectacular inversion of these effects as induced by the paratropic circulation of 4n electrons. A 4n+2 rule can be converted to a 4n one by the addition of two electrons, and chemically this can be done by reduction with lithium metal to form a dianion. Fortunately, this experiment has been done for a molecule known as methano[10]annulene. This is a 4n+2 aromatic molecule with ten π-electrons (n=2) that can be reduced with lithium metal to form an ion-pair comprising lithium cations and the twelve π-electron (4n, n=3) methano[10]annulene dianion.[1]

Here I ask whether these magnetic effects can be modelled using quantum mechanics. The point of interest here is the ion-pair. Can one get away with simply modelling the di-anion in say a continuum solvent (thf), or is the nearby presence of lithium cations (variously solvated) essential? dianion

 I used the model ωB97XD/TZVP/SCRF=THF (this DFT functional was shown to give good results for Rebek’s encapsulated methane, itself manifesting lots of diamagnetic effects from the benzo groups of the capsule). Several models 3-6 for the di-anion were explored:

  1. A negatively charged species, stabilised by continuum solvation (thf).
  2. A neutral species, with two naked Li cations bound to the under face of the annulene
  3. Same as 4, but with one water molecule in the remaining coordination sphere of the Li.
  4. Same as 4, but with two MeOMe molecules in the remaining coordination sphere of the Li.
  5. Models 4-6 relate to what is called an intimate ion-pair (also a contact ion pair). We are not exploring the solvent-separated variety here.

I should also note that whereas the methane[10]annulene itself has C2v symmetry, the di-anion has the lower C2 symmetry, since the bond lengths are no longer approximately equal, a well known consequence of anti-aromaticity and associated paratropicity. Model 6 is shown below. It corresponds to two allyl anion.lithium cation ion pairs, separated by two localized double bonds.

Click for 3D

Click for 3D

The NMR is shown below. The shifts computed for the dianion are the average of two equilibrating forms, the barrier to which is fast on the NMR time scale. It would be fair to say that overall, the chemical shifts computed for the ion-pair model are a better fit to the recorded spectra than the purely anionic model. The most realistic ion-pair model, in which the lithium is also coordinated to two (dimethyl) ether oxygens, is a fair, if not perfect fit. Realistically in solution a number of dynamically equilibrating arrangements of the ion pair, possibly solvated by more ethers, or even to the extent of creating a solvent separated ion-pair, probably contribute to the overall Boltzmann populations.

  1H 13C
system δ2,5,7,10 δ3,4,8,9 δ11 δ2,5,7,10 δ3,4,8,9 δ1,6 δ11
 1[1]  7.27  6.95  -0.52  128.7  126.1  114.6  34.8
 1(calc)[2]  7.93  7.58  -0.86  137.0  133.3  121.2  37.3
 2[1]  1.59  3.07  11.64  76.5  118.0  165.0  60.0
 3(2–)[3]  2.45  2.78  10.75  90.4  105.1  155.1  64.0
 4(2–2Li+)[4]  2.02  3.59  11.69  76.8  122.6  201.8  62.2
 5(2–2Li+.H2O)[5]  2.03  3.39  11.82  78.4  120.9  197.4  62.5
 6(2–2Li+.2Me2O)[6]  2.55  3.43  10.37  86.5  113.2  182.4  63.5

The most spectacular effect can be seen on the protons on C-11. For the neutral aromatic annulene, they are strongly shielded by a diatropic ring current. For the anti-aromatic di-anion, they are very strongly deshielded by a paratropic ring current, with Δδ 11-12 ppm. Such two-electron reductions (or oxidation) can yield equally spectacular effects on the NMR of other systems as well, as for example extended porphyrins.[7]

References

  1. D. Schmalz, and H. Günther, "1,6‐Methano[10]annulene Dianion, a Paratropic 12π‐Electron Dianion with a C<sub>10</sub> Perimeter", Angewandte Chemie International Edition in English, vol. 27, pp. 1692-1693, 1988. https://doi.org/10.1002/anie.198816921
  2. H.S. Rzepa, "Gaussian Job Archive for C11H10", 2013. https://doi.org/10.6084/m9.figshare.831450
  3. H.S. Rzepa, "Gaussian Job Archive for C11H10(2-)", 2013. https://doi.org/10.6084/m9.figshare.832421
  4. H.S. Rzepa, "Gaussian Job Archive for C11H10Li2", 2013. https://doi.org/10.6084/m9.figshare.832422
  5. H.S. Rzepa, "Gaussian Job Archive for C11H14Li2O2", 2013. https://doi.org/10.6084/m9.figshare.832423
  6. H.S. Rzepa, "Gaussian Job Archive for C19H34Li2O4", 2013. https://doi.org/10.6084/m9.figshare.832448
  7. C.S.M. Allan, and H.S. Rzepa, "Chiral Aromaticities. AIM and ELF Critical Point and NICS Magnetic Analyses of Möbius-Type Aromaticity and Homoaromaticity in Lemniscular Annulenes and Hexaphyrins", The Journal of Organic Chemistry, vol. 73, pp. 6615-6622, 2008. https://doi.org/10.1021/jo801022b

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The mysterious (aromatic) structure of n-Butyl lithium.

Sunday, March 17th, 2013

n-Butyl lithium is hexameric in the solid state and in cyclohexane solutions. Why? Here I try to find out some of its secrets.

SUHBEC. CLICK FOR 3D.

SUHBEC. CLICK FOR 3D.

The crystal structure reveals the following points of interest:

  1. Six lithium atoms form a cluster with triangular faces.
  2. An off-centre carbanion caps a triangular lithium face.
  3. Four of the butyl groups are in a fully extended antiperiplanar conformation
  4. But two di-axial n-butyl exhibit a gauche conformation.

The lithium cluster has twelve electrons available for bonding; if the Li is considered as Li+, balanced by six C– carbanions, the twelve electrons come from the six carbon lone pairs pointing towards each of six triangular faces. An ELF analysis can help identify how these twelve electrons are arranged. Shown below is the environment of a single Li-face, with the ELF basin ringed. It integrates to 2.08 electrons. So each tetrahedral cluster of three lithiums and one carbanion could be considered as a two-electron-four-centre bond, perhaps a natural progression from the two-electron-three-centre bonding found in a slightly less electron deficient system such as diborane. 

ELF basins. Click for 3D

ELF basins. Click for 3D

NBOs (natural bond orbitals) reflect this character. An NBO represents a localised two-electron orbital, and analysis indeed reveals six such orbitals, each having the form shown below.

NBO. Click for 3D.

NBO. Click for 3D.

This picture in turn leads us to identify this system as spherically aromatic (doi: 10.1002/1521-3773(20010803)40:15<2834::AID-ANIE2834>3.0.CO;2-H ). The three-dimensional equivalent of the Hückel rule is that any system with 2(N+1)2 σ or π electrons (or both) in a cluster can be considered aromatic/diatropic. In this case, N=0 and hence the magic count is 2 for each of the six CLi3 tetrahedra. The diatropic ring current might be manifested in the computed 1H NMR chemical shifts of the CH2– protons (-0.8ppm). Aromaticity does not immediately spring to mind with the name n-butyl lithium, but this unprepossessing molecule has six aromatic regions!

Each lithium atom is in turn hemispherically surrounded by three of these 2.08 electron basins (below, although the ELF centroid is very much biased towards the carbon, indicating considerable ionicity). What wonderful electronic economy! Despite there being only twelve electrons to be shared amongst six lithium atoms, each lithium manages nevertheless to surround itself with 6.24 electrons. All crammed into one half sphere, leaving a nice coordination hole; n-butyl lithium is after all a highly reactive species (even as a hexamer).

n-butyl-ELF1

I want to finish by exploring the observation that two of the six n-butyl groups adopt a gauche conformation. In free n-butane itself, around 31% of the population adopts this shape, which curiously is around the same proportion as is found in the hexameric structure of n-butyl lithium. More generally, a search of the Cambridge database for compounds containing such groups reveals the following distribution; about 1 in 7.

Gauche

Well, when you deprive a molecule of electrons, as any species with lithium must invariably suffer from, it is wonderful how the system responds. In this sense, a hexameric structure seems a very natural outcome. And it has brought us the two-electron-four-centre bond and the associated spherical aromaticity, both of which are a nice bonus.

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Computers 1967-2011: a personal perspective. Part 1. 1967-1985.

Thursday, July 7th, 2011

Computers and I go back a while (44 years to be precise), and it struck me (with some horror) that I have been around them for ~62% of the modern computing era (Babbage notwithstanding, ~1940 is normally taken as the start of the modern computing era). So indulge me whilst I record this perspective from the viewpoint of the computers I have used over this 62% of the computing era.

  1. 1967: I encountered (but that term has to be qualified) my first computer, suggested to me as an alternative to running quarter marathons on Wimbledon common at school by an obviously enlightened teacher! I wrote a program (in Algol) on paper tape, put the tape in an envelope, and sent it off to Imperial College (by van) to run, on an IBM 7094. A week later, printed output showed you had made a mistake on line 1 of the program. As I recollect, after about eight weeks of this, I got the program to run (and calculated π to 5 decimal places).
  2. 1970: By now I was a student (again at Imperial College), and was introduced to Fortran, then a radical new innovation to a chemistry degree. The delightfully named pufft compiler combined with the 7094 again, but this time with punched Holerith cards as input and line printer output. I cannot remember what we were asked to program. I do remember that the punched cards were produced by a pool of punch card operators, working from code pages written by the programmer. Some students (not me!) thought it great fun to give their Fortran variables naughty names (which the punch card operators then refused to punch, thus causing the student to fail the course!).
  3. 1971: I really liked this programming lark, so when instant-turnaround was introduced that year, I decided to do a proper program. It was called NLADAD (yes, I was no good at names, even then), which stood for non-linear-analysis of donor-acceptor complexes. The idea was to take recorded NMR chemical shifts, and fit them to an equilibrium A+B ⇔ AB+B ⇔ AB2 using non-linear regression analysis. It must have been all of 200 lines of code (OK, I did not write the matrix inversion routine myself)! Instant turnaround was also great, you got to punch your own cards this time, and had the great excitement of feeding them into a card reader yourself. You then walked about 5 yards to the line printer and waited agog. No waiting one week, this was less than a minute. Or it would have been if the line printer did not paper-wreck every two minutes! (I might add that I have a dim recollection of a member of the computer centre staff standing by to recover these paper wrecks. He, by the way, is now the director of the ICT division here!).
  4. 1972: I am now doing a PhD (yes, boringly, yet again at Imperial College). I had found the one and only teletypewriter in the chemistry department. The crystallographers had secreted it away in their empire, but were very dismayed to find me occupying it constantly. Instant was now even more instant. I was now connecting to a time-sharing CDC 6400 computer, at the dazzling speed of 110 baud (or bytes per second). These were small bytes by the way, since the CDC used 6 bits per byte. The result was that one did everything in UPPER CASE, since a 6-bit byte only allows 64 characters! My (still Fortran) programs reached probably 1000 lines of code now, and I was engrossed in deriving non-linear analyses of steady state chemical kinetics (about four different kinds of rate equation as I recollect). Ah, the joys of covariance analysis, and propagation of errors (I was in a kinetics lab, and all the other students plotted graphs on graph paper, and if pressed, plotted gradients of graphs, the so-called Guggenheim plots. I thought this the dark ages, but no-one volunteered to join me in this single teletypewriter room. Not even the attractive girls in the group. I was the geek of my time, no doubt about that. My kinetic analysis did however have one upside. Its how I meet my wife to be a few years later!).
  5. 1974: PhD completed, I was now ready to go to Texas, where everything is bigger (and in terms of computers, slightly better, a CDC 6600 now and a 300 baud teletypewriter!). I had been computing now for seven years, and finally I actually got to SEE the device for the very first time. My mentor, Michael Dewar, had a sort of special relationship with the university. His students (and possibly only his students) were allowed to go into the depths of the machine room, where behind plate glass you could see the CDC 6600. I soon learnt how to get even closer. It was not particularly exciting however. I was more entranced with the CALCOMP flatbed plotter, which was located next to the 6600. Pictures at last (you probably do not want to know that to convert my kinetics in 4 above to pictures, I got quite expert in using a french curve. Look it up before you jump to conclusions). Part of the pact I negotiated was that I was only allowed into the inner sanctum at 03:00 in the morning (sic!). Still a geek then! Oddly, I was one of the few students in Dewar’s group using the CALCOMP, but at least we now had pictures of the molecules I was now calculating (using MINDO/3). To put the computing power into context, in 1975, Paul Weiner, another group member, announced that he had completed a full geometry optimisation of LSD, this having taken about 4 days to do on that over-worked 6600. The entire group went out to celebrate. Many pitchers of beer were drunk that nite.

    Computer graphics from 1976.

  6. 1977: Back to Imperial, where we might have also now had a CDC 6600. And a Tektronix terminal running at the dizzying (hardwired end-to-end) speed of 9600 baud. I learnt to Word process on this device (using a word processor, written in Fortran, although not by me) and I wrote three review articles by this means, using a fancy phototypesetter as the printer. My next program, STEK, probably ran to about 5000 lines of code, and it persuaded the Tektronix to plot all sorts of things, ball&stick diagrams, isometric potential surfaces, molecular orbitals, and the like (and jumping ahead, my experience with this program eventually led to CML, and Peter Murray-Rust, but that is indeed jumping ahead). I think I also managed to gain access to the Imperial machine room, that inner sanctum, yet again. But for reasons I will not go into, it was not as interesting as the Texan machine room.

    Chemistry Computer graphics, circa 1977-85.

  7. 1979: I encountered a Cray 1 computer, and probably also 8-bit bytes (and yes, lower case printer outputs) for the first time at the University of London Computing Centre.
  8. 1980: Remember that teletypewriter, encountered earlier. Well these were now running at 2400 baud and I started to organise the deployment of a chemistry department computer network to sprinkle several such terminals around the department. The controller was a PAD, and in that year, we introduced STN ONLINE using this network. It was the first time we could search CAS online ourselves (previously, it was a service offered by the library). Literature searching has not been the same since.
  9. 1980: I finally again encountered a real computer, which one could happily listen to without creeping into machine rooms in the middle of the night. It was the data system on a Bruker Spectrospin 250 MHz superconducting NMR spectrometer. I had many adventures on this system. It was installed, by the way, on more or less the same day as the birth of my first daughter Joana. It had a hard drive (5 Mbytes as I recollect, and cost an absolute fortune, around £10,000 if I remember correctly).

    Combining Quantum mechanics and NMR.

    Computer graphics 1982, from NMR spectrometer.

  10. 1982: More networks, this time a curious computer known as the Corvus Concept, using a networked hard drive (possibly as big as 20 Mbytes by now), and a large screen.
  11. 1985: Enter the Mac (OK, the IBM PC came a little earlier, but it was not entrancing). Now one really had a tactile computer that made noises (not always nice), produced smoke signals occasionally, and ejected its floppy disk incessantly. Yet another revolution to cope with. As I type this, I look down on that Mac, which is still underneath my desk. Wonder if its worth anything on ebay?

Well, a second consecutive blog, with (almost) no pictures or molecules. And I have only gotten to the half way stage of my story. Better break off then.

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A molecule with an identity crisis: Aromatic or anti-aromatic?

Monday, April 13th, 2009

In 1988, Wilke (DOI: 10.1002/anie.198801851) reported molecule 1

A [24] annulene. Click on image for model.

A 24-annulene. Click for 3D.


It was a highly unexpected outcome of a nickel-catalyzed reaction and was described as a 24-annulene with an unusual 3D shape. Little attention has been paid to this molecule since its original report, but the focus has now returned! The reason is that a 24- annulene belongs formally to a class of molecule with 4n (n=6) π-electrons, and which makes it antiaromatic according to the (extended) Hückel rule. This is a select class of molecule, of which the first two members are cyclobutadiene and cyclo-octatetraene. The first of these is exceptionally reactive and unstable and is the archetypal anti-aromatic molecule. The second is not actually unstable, but it is reactive and conventional wisdom has it that it avoids the undesirable antiaromaticity by adopting a highly non-planar tub shape and hence instead adopts reactive non-aromaticity. Both these examples have localized double bonds, a great contrast with the molecule which sandwiches them, cyclo-hexatriene (i.e. benzene). The reason for the resurgent interest is that a number of crystalline, apparently stable, antiaromatic molecules have recently been discovered, and ostensibly, molecule 1 belongs to this select class!

So is 1 actually anti-aromatic? Let us look at some of the ways in which this might be estimated.

  1. One can inspect the bond lengths, measured from X-ray analysis. The longest is 1.463Å, labelled a above, and it corresponds to a single bond (value from the crystal structure).
  2. If the molecule had a bond alternating structure, the adjacent bonds would be expected to be much shorter, in the region of 1.32Å. In fact, they are rather longer, at 1.37Å. Indeed, in the cycloheptatriene part of the molecule, the alternation is much less than one might expect of an anti-aromatic molecule, oscillating between 1.37 and 1.43Å.
  3. One can also inspect aromaticity via a variety of magnetic indices. The simplest of these is the NICS probe. Placed at a ring centroid, a negative value of this index of around -10ppm indicates aromaticity (this is the value for benzene), whilst a strongly positive value (of up to +20 ppm) indicates anti-aromaticity. Molecule 1 has two potential centroids, one placed at the absolute centre of the system, and one placed at the centroid of the ~6-membered ring completed using bond b (in reality, the centroids were computed from the positions of ring critical points obtained from an AIM analysis). The NICS values at these two positions are both ~-4.4 ppm (See DOI: 10042/to-2156 for details of the calculation). These values does not indicate antiaromaticity! They could even be described as mildly aromatic. So what is going on?
  4. What about the chemical shifts of the other protons? All the hydrogens attached to sp2 carbons are predicted to resonate at around 6.7ppm (unfortunately Wilke does not report the experimental spectrum), which is typical of an aromatic system (anti-aromatic systems have high upfield shifts for such protons, at around 2ppm or even -2 ppm, see DOI: 10.1021/ol703129z for examples). The two protons of the methylene bridges are also quite different; 2.9 and 0.8 ppm. The latter is the proton endo to the cycloheptatrienyl ring, and is typical of a proton placed in the anisotropic magnetic shielding region of e.g. benzene. Thus the cycloheptatrienyl ring is itself behaving as if it were aromatic, whereas the overarching 24-annulene ring is certainly not behaving as if it were antiaromatic.

One possible explanation involves a concept known as homoaromaticity. The bond marked as b could be regarded as completing the 6π-electron local aromaticity of that ring (it would be formally considered as a 1π-electron bond, with no underlying σ-framework, see 10.1021/ct8001915 for further detail). Well characterised examples of such neutral homoaromatics are in fact very rare indeed; the phenomenon is thought to manifest mostly through cationic homoaromatics (i.e. the homotropylium cation, see 10.1021/jo801022b for discussion). So has the case been made for 1 being the first clear cut example of a neutral homoaromatic molecule, containing no less than four rings exhibiting this type of aromaticity?

There is one further concept that can be introduced. Clar (for a discussion, see DOI: 10.1021/cr0300946) proposed that benzenoid 6π-electron local aromaticity is preferred to less local or more extended cyclic conjugations, if the two compete. Many examples in a type of compound known as polybenzenoid aromatics are known where the most favourable resonance structure is that which maximises the number of Clar rings. More recently, quite a few ostensibly antiaromatic molecules have been shown to attenuate this unfavourable effect by forming instead groups of aromatic Clar islands containing delocalized benzene like rings (discussion of this point can be found at DOI: 10.1039/b810147g). In molecule 1, we could have a new phenomenon; a homoClar ring, formed to avoid antiaromaticity.

For further discussion, see the comment posted to Steve Bachrach’s blog.

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