Andrew J.
Valentine
a,
Ana M.
Geer
b,
Laurence J.
Taylor
a,
Andrew M.
Teale
a,
Katherine E.
Wood
a,
Huw E. L.
Williams
c,
William
Lewis
d,
Stephen P.
Argent
a,
Jonathan
McMaster
*a and
Deborah L.
Kays
*a
aSchool of Chemistry, University of Nottingham, University Park, Nottingham, NG7 2RD, UK. E-mail: Deborah.Kays@nottingham.ac.uk; Jonathan.McMaster@nottingham.ac.uk
bDepartamento de Química Inorgánica, Instituto de Síntesis Química y Catálisis Homogénea (ISQCH), CSIC, Universidad de Zaragoza, Pedro Cerbuna 12, 50009 Zaragoza, Spain
cCentre for Biomolecular Sciences, University of Nottingham, University Park, Nottingham, NG7 2RD, UK
dSchool of Chemistry, The University of Sydney, F11, Eastern Ave, Sydney, NSW 2006, Australia
First published on 8th December 2020
The effect of para-substitution upon the structural and electronic properties of a series of m-terphenyl lithium complexes [R–Ar#–Li]2 (R = t-Bu 1, SiMe32, H 3, Cl 4, CF35; where R–Ar# = 2,6-{2,6-Xyl}2-4-R-C6H2 and 2,6-Xyl = 2,6-Me2C6H3) has been investigated. X-ray crystallography reveals the complexes to be structurally similar, with little variation in C–M–C bond lengths and angles across the series. However, in-depth NMR spectroscopic studies reveal notable electronic differences, showing a linear correlation between the 7Li{1H} NMR chemical shifts of the para-substituted complexes and their Hammett constants. The flanking methyl protons exhibit a similar electronic shift in the 1H NMR spectra, which has been rationalised by the presence of through-space Li⋯H interactions, as evidenced by two-dimensional 7Li–1H heteronuclear Overhauser spectroscopy (HOESY). In both cases, electron-withdrawing substituents are found to cause an upfield peak shift. A computational analysis is employed to account for these trends.
For instance, the solid state structures observed for a series of m-terphenyl lithium complexes vary depending on the steric demands of the flanking ortho-aryl substituents.19,20 Increasing the steric bulk of 2,6-Ar2C6H3Li alters its aggregation state from a dimer,19 to a more crowded dimer featuring η6-arene coordination of the flanking aryl groups,20 to a monomer stabilised by a coordinated molecule of benzene,20 for Ar = Mes (2,4,6-Me3C6H2), Dipp (2,6-i-Pr2C6H3) and Tripp (2,4,6-i-Pr3C6H2) respectively.5,6
However, less work has been reported on varying the electronic effects of these m-terphenyl systems, with studies limited mainly to a handful of main group complexes21–25 and the quintuply-bonded Cr–Cr dimer [(2,6-Dipp2-4-R-C6H2)Cr]2 (R = H, SiMe3, OMe, F).26 Even their lithium precursors, while structurally characterised, have not been studied from an electronic viewpoint. Therefore, it is the objective of this research to develop a toolbox of m-terphenyl ligands featuring a range of para-substituents (R) to investigate the electronic effects of substitution upon their metal complexes.
To this end, a series of para-substituted m-terphenyl lithium complexes [R–Ar#–Li]2 (R–Ar# = 2,6-{2,6-Xyl}2-4-R-C6H2; R = t-Bu, SiMe3, Cl, CF3; 2,6-Xyl = 2,6-Me2C6H3) are reported, and discussed alongside the previously published unsubstituted analogue [H–Ar#–Li]2.27 The geometric and electronic structures of these compounds are elucidated through X-ray crystallographic and NMR spectroscopic studies, respectively. Specifically, 7Li NMR spectroscopy is employed to assess the electronic effects directly at the metal centre, with two-dimensional 7Li–1H heteronuclear Overhauser spectroscopy (HOESY) measurements demonstrating the presence of through-space 7Li⋯1H interactions. Computational modelling with density functional theory (DFT) is also employed to help rationalise the observed trends in NMR parameters across the series.
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Scheme 1 Synthesis of lithium complexes [R–Ar#–Li]2 (R = t-Bu 1, SiMe32, H 3, Cl 4, CF35). Reaction conditions: (i) isohexane, 0 °C to room temperature, 16 h, – n-BuI. |
Weaker intramolecular interactions are also observed between the lithium ions and the xylyl flanking groups, with secondary contacts that are shorter than the sum of the van der Waals radii for lithium and hydrogen (3.02 Å) or lithium and carbon (3.52 Å).34,35 A summary of these contacts is given in Table S2 of the ESI.† For complexes 1, 2, 4 and 5, the lithium ions interact with the ipso-carbons of the flanking aryls [2.4244(15)–2.729(4) Å], and also form multiple Li⋯H–C anagostic interactions36 with the hydrogens of the flanking methyl groups [2.338(2)–2.920(3) Å].
In summary, the crystal structures of 1, 2, 4 and 5 show little structural variation as the para-substituent is changed, which suggests that the geometries of m-terphenyl organolithiums are dominated by steric rather than electronic factors.5,6,19,20 The structures do, however, show weak Li⋯H–C anagostic contacts between the lithium ions and the flanking methyl groups. These interactions have been explored further in our NMR spectroscopic investigations, as discussed below.
Compounda | Diffusion coefficient, D (10−10 m2 s−1) | Hydrodynamic radius, rH (Å) | Crystallographic diameters, dc (Å) | |
---|---|---|---|---|
Lengthb | Widthc | |||
a All samples were prepared as 24 mM solutions in d6-benzene. b Length along the compound measured between R⋯I (H–Ar#–I) and R⋯R (1–5), where R is the outermost nucleus of the para-substituent. c Width across the compound measured between C⋯C for the outermost carbon atoms of the flanking aryl rings on each m-terphenyl ligand. All widths averaged at 9.9 Å. | ||||
H–Ar#–I | 12.30 | 3.0 | 4.9 | 9.9 |
[H–Ar#–Li]2 (3) | 7.54 | 4.8 | 9.4 | 9.9 |
[Cl–Ar#–Li]2 (4) | 6.72 | 5.4 | 12.8 | 9.9 |
[F3C–Ar#–Li]2 (5) | 7.59 | 4.8 | 13.4 | 9.9 |
[t-Bu–Ar#–Li]2 (1) | 6.59 | 5.5 | 13.6 | 9.9 |
[Me3Si–Ar#–Li]2 (2) | 6.27 | 5.8 | 14.4 | 9.9 |
The key 1H, 13C{1H}, and 7Li{1H} NMR spectroscopic signals of 1–5 are summarised in Table 2, with the numbering scheme presented in Fig. 2. The 1H NMR spectra show four characteristic peaks, although in some cases the signals for the aromatic xylyl protons (H-7 and H-8) overlap. Relative to the iodides (R–Ar#–I), all resonances are shifted upfield due to the greater shielding provided by the anionic ligands. A comparison of the 1H NMR spectra across the series reveals three key features. Firstly, the meta-hydrogens on the central rings exhibit small variations in chemical shift (H-3 = 6.85, 7.04, 6.77, 6.78, 6.99 ppm for 1–5, respectively) with no overall trend, see Table 2. Secondly, the xylyl aryl protons, H-7 (6.86–7.01 ppm) and H-8 (6.94–7.01 ppm), remain essentially unshifted, suggesting that the substituent in the para-position has minimal electronic communication with the flanking aryl rings. Thirdly, the xylyl methyl protons shift upfield (H-9 = 1.83, 1.81, 1.80, 1.61, 1.55 ppm for 1–5, respectively) with increased electron-withdrawing strength of the para-substituent. A graph of these chemical shifts (δ) against the corresponding Hammett constants (σpara)40 reveals a linear correlation, see Fig. 4 (blue line; R2 = 0.92). This trend is not observed in the respective iodide compounds (H-9 = 2.06, 2.05, 2.06, 2.07 and 2.02 ppm for R–Ar#–I, where R = t-Bu, SiMe3, H, Cl and CF3, respectively) and proceeds in the opposite direction to what one might expect, with electron-withdrawing groups causing an apparent shielding effect. This suggests that the para-substituent is exerting a direct electronic influence on the environment of the H-9 methyl protons.
[R–Ar#–Li]2 | R group | 1H, 13C{1H} and 7Li{1H} NMR Chemical Shifts, δ (ppm) | Li | ||||||
---|---|---|---|---|---|---|---|---|---|
H-3 | H-9 | C-1 | C-2 | C-3 | C-4 | C-9 | |||
a Peak C-4 for 5 not observed (obscured by d6-benzene solvent peak). | |||||||||
1 | t-Bu | 6.85 | 1.83 | 168.1 | 152.0 | 120.4 | 148.7 | 21.8 | 1.60 |
2 | SiMe3 | 7.04 | 1.81 | 174.2 | 151.6 | 128.1 | 136.5 | 21.9 | 1.47 |
3 | H | 6.77 | 1.80 | 172.7 | 152.0 | 123.6 | 126.3 | 21.8 | 1.46 |
4 | Cl | 6.78 | 1.61 | 170.7 | 153.6 | 123.6 | 132.9 | 21.5 | 1.10 |
5 | CF3 | 6.99 | 1.55 | 180.2 | 152.4 | 119.5 | —a | 21.5 | 0.93 |
The 13C{1H} NMR spectra of 1–5 show nine peaks for the carbons of the ligand framework, with additional peaks for the t-Bu, SiMe3 and CF3 groups in 1, 2 and 5, respectively. Compared to the iodides (R–Ar#–I), the largest change is seen in the ipso-carbons, which are shifted downfield (C-1 = 106.9 vs. 172.7 ppm for H–Ar#–I and 3, respectively) owing to a large deshielding effect in the plane perpendicular to the C–Li bond.19,41–44 In all cases, the NMR resonances for the ipso-carbons of 1–5 were of low intensity and therefore assigned from 1H–13C HMBC spectra. For 3, a longer 13C{1H} NMR experiment with d1 of 10 s was performed to achieve better resolution of the ipso-carbon peak (Fig. 3). This revealed a seven-line splitting pattern (blue) centred at 172.7 ppm with a 1:
2
:
3
:
4
:
3
:
2
:
1 intensity ratio (1J13C7Li = 23.3 Hz) characteristic of quadrupolar coupling to two 7Li nuclei (I = 3/2, natural abundance: 92.41%), providing further evidence that the lithium complexes are dimeric in d6-benzene solution.45–48 The experimental spectrum was well simulated (red, see ESI, section S1†). Multiplets arising from 6Li (I = 1, natural abundance = 7.59%) were too low intensity to resolve experimentally.
![]() | ||
Fig. 3 Seven-line splitting pattern of the ipso-carbons in the experimental (blue) and simulated (red) 13C{1H} NMR spectra of [H–Ar#–Li]2 (3). |
A comparison of the 13C{1H} NMR spectra of 1–5 reveals that all 13C signals of the xylyl flanking groups remain essentially unshifted across the series. The shift observed for the xylyl methyl groups in the 1H NMR spectrum (H-9) is not replicated in the 13C{1H} NMR spectrum (C-9). The peaks for the central ring carbons vary considerably across the series (except for C-2, see Table 2): larger variations are noted for C-4 (126.3–148.7 ppm) than for C-1 (168.1–180.2 ppm) and C-3 (119.5–128.1 ppm). Though no reliable trends can be identified, a general downfield shift is observed for C-1 with increasing σpara.
The 7Li{1H} NMR spectra of 1–5 also provided valuable information on the complexes. Although 7Li NMR spectroscopy is typically sensitive to the analyte concentration, aggregation, and solvent effects, these factors appear to be negligible here.49–51 This was demonstrated by the spectra for the more soluble t-Bu complex (1) whose 7Li{1H} NMR resonance remains unshifted over a wide concentration range (1.60 ppm at 24, 48 and 72 mM, respectively). This may be due to the steric bulk of the ligands shielding the metal centre from the surrounding solvent. For complexes 2–5, saturated samples were used for NMR measurements due to their poor solubilities in d6-benzene. The steric influence of the xylyl flanking groups on the lithium ions is assumed to remain consistent throughout the series and, therefore, not to contribute to changes in the 7Li{1H} NMR chemical shifts. This is in contrast to previous work on m-terphenyl lithium complexes, where changing the steric bulk of the flanking groups varies the 7Li{1H} NMR signal.15
In all cases, the 7Li{1H} NMR spectra show a single environment for the two lithium ions of the dimer. The position of these peaks shifts upfield (1.60, 1.47, 1.46, 1.10 and 0.93 ppm for 1–5, respectively) as the electron-withdrawing strength of the para-substituent is increased (Table 2). Once again, plotting a graph of these chemical shifts (δ) against the Hammett constants (σpara) reveals a linear correlation, see Fig. 4 (red line; R2 = 0.96),40 indicating a direct influence on the electronic properties of the lithium ions by the para-substituent. As with the H-9 protons, the trend is counterintuitive, since one might expect electron-withdrawing groups to deshield the nuclei and cause a downfield shift. However, a similar observation has been reported for the series of para-substituted aryllithium complexes [4-R-C6H4]2Li (R = OMe, Me, H, F, Cl, CF3).52–54
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Fig. 4 Plot of the 1H (for flanking methyl protons, H-9) and 7Li{1H} NMR chemical shifts (δ) for the para-substituted lithium complexes [R–Ar#–Li]2 (1–5) versus their corresponding literature Hammett constants (σpara).40 |
These 7Li{1H} NMR spectroscopic results help to rationalise the trend observed for the flanking methyl protons (H-9) (Fig. 4). Since all other atoms on the xylyl rings remain unshifted, this suggests that electronic communication occurs via a through-space interaction between the methyl protons and lithium atoms. Some evidence of this is seen in the crystal structures, with weak Li⋯H–C anagostic interactions observed in the solid state (Fig. S31 and S32†). In solution, this is further corroborated by two-dimensional 7Li–1H HOESY experiments,55,56 which reveal short 7Li⋯1H contacts in 1–5 as evidenced by the intense cross-peak between the lithium signals and the H-9 protons (Fig. 5 and ESI, section 3†).
![]() | ||
Fig. 5 Superimposed 2D 7Li–1H HOESY spectra of the m-terphenyl lithium complexes [R–Ar#–Li]2 (1–5) showing strong cross-peaks between the flanking methyl protons, H-9, and the 7Li nuclei. |
Similar Li⋯H interactions have been reported for the monomeric [Mes*-Li] species, whose 6Li–1H HOESY spectrum gave a cross-peak for the ortho tert-butyl protons, but not for the para tert-butyl protons.42 Moreover, the ortho groups (1.61 ppm) occurred at lower field than the para groups (1.56 ppm), owing to the electric field produced by lithium that deshields the protons within close proximity.42 Comparable findings have been described for other aryllithium complexes [Ar–Li] (Ar = Naph, 2-{t-BuS}C6H4).57,58
From these results we suggest that the electronic influence of the para-substituents in complexes 1–5 is relayed through the central m-terphenyl ring, onto the lithium atoms, then through-space onto the nearby methyl protons. Evidence of similar through-space interactions within a m-terphenyl framework has already been reported for the m-terphenyl carboxylic acids (2,6-Ar2C6H3)COOH (Ar = 4-R-C6H4; R = OMe, Me, H, F, Cl, Br, C{O}Me) where para-substitution of the flanking aryl rings influences the pKa value, owing to through-space effects.59 In addition, the m-terphenyl silane (2,6-Ar2C6H3)SiMe2H (Ar = 2,6-F2C6H3) possesses flanking aryl fluorine atoms that couple through-space to the Si–H proton.60 To further investigate the origin of this effect we turned to computational analysis and DFT studies.
Tables summarising the calculated shifts for H-9 and Li are given in the ESI, Tables S6 and S7.† Because of the relatively narrow chemical shift range, it is difficult to accurately model the trends shown in Fig. 3. Furthermore, both the H-9 and Li shifts are composed from absolute shielding constants containing large paramagnetic components (ESI, Table S5†). It is known that when the paramagnetic components are dominant, as in these cases, then density-functional methods often fail to achieve high accuracy. It is also known that density-functionals tend to be more accurate for 1H and 13C{1H} NMR resonances than those for other nuclei.75 In line with these observations the calculated values for the 7Li{1H} NMR spectrum do not accurately capture the trend in Fig. 3. However, the trend for the 1H NMR of the flanking H-9 nuclei is more adequately reproduced, particularly for the KT2 functional in the larger pcS-2 basis. As shown in Fig. S34 of the ESI† the general trend for an upfield shift with increasing σpara is reproduced, see also Table S7.† Linear regression of the calculated 1H NMR shifts for the H-9 nuclei as a function of σpara yields a fit with R2 = 0.92, a somewhat steeper slope of −0.62 and a y-intercept of +1.82 ppm. Given the challenges associated with the relatively narrow range of chemical shifts and large paramagnetic contributions for these nuclei, these results are in reasonable agreement with the experimental observations. However, based on these results, it seems likely that the counterintuitive trends observed in both the 1H and 7Li{1H} NMR resonances is due to a large paramagnetic contribution to the shielding constant. Finally, we note that the more challenging 7Li{1H} NMR spectroscopy may provide a useful test case for the development of more refined density-functionals for NMR studies.
Footnote |
† Electronic supplementary information (ESI) available. CCDC 2045214–2045221. For ESI and crystallographic data in CIF or other electronic format see DOI: 10.1039/d0dt03972a |
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