Mimoza
Gjikaj
*a,
Wolfgang
Brockner
a,
Jan
Namyslo
b and
Arnold
Adam
a
aInstitute of Inorganic and Analytical Chemistry, Clausthal University of Technology, Clausthal-Zellerfeld, Germany. E-mail: mimoza.gjikaj@tu-clausthal.de; Fax: +49 5323 722995; Tel: +49 5323 722887
bInstitute of Organic Chemistry, Clausthal University of Technology, Clausthal-Zellerfeld, Germany
First published on 17th September 2007
Bis(1,3-dimethylimidazolium methylsulfate) [18-crown-6] (1), ([DMIm]2[CH3SO4]2[18-crown-6], bis(1-butyl-3-methylimidazolium methylsulfate) [18-crown-6] (2), ([BMIm]2[CH3SO4]2[18-crown-6]), bis(1-ethyl-3-methylimidazolium methanesulfonate) [18-crown-6] (3), ([EMIm]2 [CH3SO3]2[18-crown-6]) and bis(1-ethyl-3-methylimidazolium trifluoromethanesulfonate) [18-crown-6] (4), ([EMIm]2[CF3SO3]2[18-crown-6]) were prepared and characterized by single-crystal X-ray diffraction, NMR and Raman spectroscopy. Coulomb interactions between the ionic (liquid) components as well as hydrogen bonding are important. No significant close contacts are observed between the ionic components and the 18-crown-6 molecules. Crystal structures of all compounds consist of alternated layers of crown-ether molecules and respective ionic units compounds. Within the layers of the ionic components (compounds 1, 3 and 4), two cations are linked to each other by C–H⋯π interactions between one methyl carbon and the imidazolium ring of another cation.
In this work, we report the co-crystallisation of imidazolium based salts with 18-crown-6. Comparable (inclusion) compounds have been synthesized very recently by Bates, Gale and coworkers16–18 out of imidazolium salts and calixarene derivatives. These compounds show interesting structural architectures as well as the capacity to act as (selective) ion-pair receptors. Different kinds of interactions can also be studied thereby. Generally the complex formation of organic molecules via weak non-covalent interactions such as hydrogen bonds, π-stacking, charge-transfer interaction and electrostatic interaction is of great importance.19 These interactions and charge transfers have received increasing attention recently.20 The investigated compounds were characterised by X-ray analysis, Raman spectroscopy and NMR.
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Scheme 1 Molecular structure of 1-alkyl-3-methylimidazolium cation (DMIm: R = methyl, BMIm: R = n-butyl and EMIm: R = ethyl). |
Four low melting alkylimidazolium salts, bis(1,3-dimethyl-imidazolium methylsulfate) [18-crown-6] (1), bis(1-butyl-3-methylimidazolium methylsulfate) [18-crown-6] (2), bis(1-ethyl-3-methylimidazolium methanesulfonate) [18-crown-6] (3), and bis(1-ethyl-3-methylimidazolium trifluoromethane-sulfonate)[18-crown-6] (4) have been prepared and their single-crystal structures determined.
All compounds consist of alternating layers of crown-ether molecules and the respective ionic components [DMIm]+, [CH3SO4]– for 1, [BMIm]+, [CH3SO4]– for 2, [EMIm]+, [CH3SO3]– for 3 and [EMIm]+, [CF3SO3]– for 4. The layers of crown ether are surrounded above and below from methyl groups of imidazolium with a distance of 1.976 Å for 1, 2.001 Å for 2, 2.011 Å for 3 and 2.090 Å for 4. The crystallographic data and details of the single crystal structure determinations are given in Table 1. Selected interatomic distances and angles for compounds 1–4 are collected in Table 2.
1 | 2 | 3 | 4 | |
---|---|---|---|---|
a R = Σ| |Fo| – |Fc| |/Σ||Fo|. wR2 = {Σ[w(|Fo|2 – |Fc|2)2]/Σ[w(|Fo|2)2]}1/2. | ||||
Empirical formula | C24H48N4O14S2 | C30H60N4O14S2 | C26H52N4O12S2 | C26H46F6N4O12S2 |
Formula weight/g mol–1 | 680.78 | 764.94 | 676.84 | 784.79 |
Temperature/K | 223 | 223 | 223 | 223 |
Wavelength/Å | 0.71073 | 0.71073 | 0.71073 | 0.71073 |
Crystal system | Triclinic | Monoclinic | Triclinic | Triclinic |
Space group |
P![]() |
P21/n (no. 14) |
P![]() |
P![]() |
a/Å | 8.551(2) | 9.123(11) | 8.751(5) | 8.946(2) |
b/Å | 9.298(2) | 16.188(1) | 9.126(4) | 9.165(2) |
c/Å | 10.774(3) | 13.939(2) | 11.357(6) | 11.469(3) |
α/° | 86.93(2) | 97.26(4) | 92.60(2) | |
β /° | 80.09(2) | 98.03(1) | 97.99(4) | 98.72(2) |
γ/° | 82.06(2) | 97.76(4) | 97.86(2) | |
Volume/Å3 | 835.3(3) | 2038.2(4) | 880.1(7) | 918.6(4) |
Z | 1 | 2 | 1 | 1 |
Density (calc.)/g cm–3 | 1.353 | 1.246 | 1.277 | 1.419 |
Abs. coefficient/mm–1 | 0.228 | 0.194 | 0.212 | 0.236 |
F(000) | 364 | 824 | 364 | 412 |
θ min, max/° | 2.21, 25.02 | 1.94, 25.02 | 2.25, 25.03 | 2.25, 25.02 |
Index ranges | –9 ≤ h ≤ 10 | –10 ≤ h ≤ 10 | –10 ≤ h ≤ 9 | –10 ≤ h ≤ 9 |
–11 ≤ k ≤ 11 | –19 ≤ k ≤ 18 | –10 ≤ k ≤ 10 | –10 ≤ k ≤ 10 | |
–12 ≤ l ≤ 12 | –16 ≤ l ≤ 15 | –13 ≤ l ≤ 13 | –13 ≤ l ≤ 13 | |
Unique reflections | 2903 | 3598 | 3085 | 3202 |
Data/restrains/parameters | 2903/0/293 | 3598/0/336 | 3085/0/303 | 3202/0/319 |
Goodness-of-fit on F2 | 1.030 | 1.090 | 1.038 | 1.080 |
R indexes [I > 2σI] | R1 = 0.0621 | R1 = 0.0612 | R1 = 0.0725 | R1 = 0.0612 |
wR2 = 0.1542 | wR2 = 0.1484 | wR2 = 0.1454 | wR2 = 0.1080 | |
R indexes (all data) | R1 = 0.0845 | R1 = 0.0779 | R1 = 0.1172 | R1 = 0.1016 |
wR2 = 0.1682 | wR2 = 0.1591 | wR2 = 0.1638 | wR2 = 0.1217 | |
Largest diff. peak and hole/e Å3 | 0.576 and –0.295 | 0.418 and –0.289 | 0.365 and –0.261 | 0.261 and –0.232 |
Compound 1 | |||
---|---|---|---|
S–O(1) | 1.397(4) | O(1)–S–O(2) | 116.2(3) |
S–O(2) | 1.406(4) | O(1)–S–O(3) | 111.3(3) |
S–O(3) | 1.436(4) | O(1)–S–O(4) | 107.3(3) |
S–O(4) | 1.573(3) | O(2)–S–O(3) | 110.0(3) |
O(4)–C(8) | 1.470(7) | C(8)–O(4)–S | 114.0(4) |
Compound 2 | |||
S–O(1) | 1.400(3) | O(1)–S–O(2) | 113.3(2) |
S–O(2) | 1.400(3) | O(1)–S–O(3) | 113.4(2) |
S–O(3) | 1.434(3) | O(1)–S–O(4) | 107.0(2) |
S–O(4) | 1.565(3) | O(2)–S–O(3) | 112.7(2) |
O(4)–C(11) | 1.466(9) | C(11)–O(4)–S | 114.2(5) |
Compound 3 | |||
S–O(1) | 1.429(4) | O(1)–S–O(2) | 112.6(3) |
S–O(2) | 1.432(4) | O(1)–S–O(3) | 110.3(3) |
S–O(3) | 1.440(4) | O(2)–S–O(3) | 113.9(3) |
S–C(9) | 1.749(6) | O(1)–S–C(9) | 106.9(3) |
O(2)–S–C(9) | 106.8(3) | ||
O(3)–S–C(9) | 105.6(3) | ||
Compound 4 | |||
S–O(1) | 1.406(3) | O(1)–S–O(2) | 115.9(3) |
S–O(2) | 1.428(3) | O(1)–S–O(3) | 115.0(3) |
S–O(3) | 1.430(3) | O(2)–S–O(3) | 113.1(2) |
S–C(9) | 1.807(4) | O(1)–S–C(9) | 104.0(2) |
F(1)–C(9) | 1.314(5) | O(2)–S–C(9) | 103.4(2) |
F(2)–C(9) | 1.308(5) | O(3)–S–C(9) | 103.3(2) |
F(3)–C(9) | 1.297(5) | F(1)–C(9)–S | 112.0(3) |
F(2)–C(9)–S | 111.3(3) | ||
F(3)–C(9)–S | 116.6(3) |
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Fig. 1 Perspective view of the unit cell of compound 1 along the c-axis and H atoms of crown ethers have been omitted for clarity. |
Within the layer of the ionic components, two cations are linked to each other by C–H⋯π interactions between one methyl carbon C(7) and the imidazolium ring of another cation (Fig. 2). The distance between the methyl carbon and the center of the imidazolium ring is estimated to be 3.682 Å, which is in excellent agreement with the values expected for the lowest benzene⋯methane interactions.21 The only significant hydrogen bonding are contacts between the two (acidic) ring-hydrogens C(2) and C(5), and the two terminal oxygen atoms of the sulfate anion. Each imidazolium cation participates in two hydrogen bonds, forming a chain with C–H⋯O distances 2.351 and 2.730 Å and C–H⋯O angles 150.0 and 175.8° (Table 3). The hydrogen bonding and the C–H⋯π stacking contacts help stabilize the extended crystal lattice and allow a close packing in the crystal structure.
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Fig. 2 Interionic contacts between [DMIm]+ cation and [CH3SO4]– anion in compound 1; hydrogen bonding and C–H⋯π interactions are shown by dotted lines. |
Donor–H⋯Acceptor | D–H/Å | H⋯A/Å | D⋯A/Å | D–H⋯A/° |
---|---|---|---|---|
a x, y – 1, z. b x–1/2, –y + 1/2, z + 1/2. c x – 1, y, z. d –x + 1, –y + 1, –z + 2. e –x + 1, –y, –z + 2. f x, y + 1, z. | ||||
Compound 1 | ||||
C(2)–H(2)⋯O(2) | 0.824 | 2.738 | 3.476 | 150.0 |
C(5)–H(5)⋯O(1)a | 0.808 | 2.351 | 3.157 | 175.8 |
Compound 2 | ||||
C(2)–H(2)⋯O(4) | 0.918 | 2.771 | 3.620 | 154.4 |
C(4)–H(4)⋯O(1)b | 0.902 | 2.448 | 3.290 | 155.4 |
C(5)–H(5)⋯O(2)c | 0.906 | 2.521 | 3.352 | 152.8 |
Compound 3 | ||||
C(2)–H(2)⋯O(3)e | 0.925 | 2.410 | 3.283 | 157.4 |
C(5)–H(5)⋯O(2)d | 0.911 | 2.286 | 3.169 | 163.1 |
Compound 4 | ||||
C(2)–H(2)⋯O(2) | 0.918 | 2.533 | 3.292 | 140.4 |
C(5)–H(5)⋯O(1)f | 0.830 | 2.373 | 3.180 | 164.2 |
S–O bond distances in [CH3SO4]– range from 1.396 to 1.572 Å, the O–S–O bond angles from 100.2 to 116.2° and C–O bond length in the [CH3SO4]– amounts to 1.473 Å (Table 2).
These data correspond well to those previously reported for the methylsulfate anion in [DMIm] [CH3SO4]22 and [NH4]6[calix][4] [arenesulfonate] [MeOSO3]·(H2O)2.23
Bis(1-butyl-3-methylimidazolium methylsulfate) [18-crown-6] (2) crystallizes in the monoclinic P21/n space group. Similar to compound 1 the structure consists of alternate layers of 18-crown-6 and the ionic units ([BMIm]+ and [CH3SO4]–). In the 1-butyl-3-methylimidazolium cation all C–C bonds of the alkyl chain are in a trans–trans conformation which projects the chain away from the imidazolium ring, with a torsion angle around C(7)–C(8) of 177.3° (Fig. 3).
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Fig. 3 Trans–trans conformation of [BMIm]+ cation in compound 2. |
Distinguished by a trans–trans conformation of the butyl chain, each cation in the lattice has three neighbouring counter ions in contact at the van der Waals distance. The shortest hydrogen bonds are between C(4) and C(5) of the imidazolium ring and two oxygen atoms of the sulfate anion O(1) and O(2), with C–H⋯O distances of 2.448 and 2.521 Å, and C–H⋯O angles of 152.8 and 155.4° (Table 3). The next interaction is between C(2) and O(4) with C–H⋯O bond distance of 2.771 Å and C–H⋯O angle of 154.4° (Fig. 4). In compound 2, the orientation of the butyl chain away from the imidazolium ring allows no other significant van der Waals contacts or C–H⋯π interactions.24
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Fig. 4 Interionic contacts between [BMIm]+ cation and [CH3SO4]– anion in compound 2; hydrogen bondings are shown by dotted lines. |
S–O bond distances in the [CH3SO4]– range from 1.400 to 1.564 Å, the O–S–O bond angles from 99.8 to 113.3° and C–O bond length is 1.469 Å. These data correspond well with those found in 1 (Table 2).
Both imidazolium salts 3 and 4 crystallized in the triclinic space groupP. The crystal structures contain one crystallographically independent [EMIm]+ cation, [CH3SO3]– and crown ether for 3 and one crystallographically independent [EMIm]+ cation, [CF3SO3]– and crown ether for 4. The crystallographic data for 3 and 4 are given in Table 1. The ions are packed in the crystal lattice of compounds 3 and 4via weak interionic C–H⋯O hydrogen bonds as well as significant C–H⋯π interactions.
Comparable to compound 1, two [EMIm]+ cations in both compounds 3 and 4 are linked to each other by C–H⋯π interactions between one methyl carbon (C(6) for 3 and C(6) for 4) and the imidazolium ring of another cation (Fig. 5 and 6). The distance between the methyl carbon and the center of the imidazolium ring is estimated to be 3.717 Å for 3 and 3.990 Å for 4, which agrees very well with the value expected for the lowest benzene⋯methane interactions.
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Fig. 5 Interionic contacts between [EMIm]+ cation and [CH3SO3]– anion in compound 3; hydrogen bonding and C–H⋯π interactions are shown by dotted lines. |
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Fig. 6 Interionic contacts between [EMIm]+ cation and [CF3SO3]– anion in compound 4. Hydrogen bonding and the C–H⋯π interactions are shown by dotted lines. |
Two significant C–H⋯O hydrogen bonds involving H(2) and H(5) connect the cations and anions forming layered structures for compounds 3 and 4. C–H⋯O bond distances of 2.286 and 2.410 Å and C–H⋯O bond angles of 157.4 and 163.1° are found for compound 3, and two [CF3SO3]– anions with C–H⋯O bond distances of 2.373 and 2.533 Å, and C–H⋯O bond angles of 140.3 and 164.2° for compound 4 (Fig. 6 and Table 3).
In 3 the methanesulfonate ion is in a staggered conformation with C3v symmetry. The sulfonate group has an average S–O bond distance of 1.434 Å, an average O–S–O bond angle of 112.3°, and a C–S bond distance of 1.750 Å (Table 2).
The arrangement of the [CF3SO3]– anion in 4 agrees very well with this in several dehydrated salts, such as LiCF3SO3 and [EMIm] [SO3CF3].25 It also has a staggered conformation with C3v symmetry. The S–C (1.808 Å), average C–F (1.306 Å), and average S–O (1.421 Å) bond lengths for compound 4 (Table 2) are in best agreement with those measured by Dehnicke et al.26 and Jansen et al.27
Raman frequencies of the respective anions of the studied compounds are, more or less, known in detail. The Raman frequencies of the crystalline compounds are summarized along with their assignments in groups in Table S1 (ESI)† along with these of 18-crown-6. For the crystalline compound 2Raman spectra at –60 and –150 °C were recorded to extend the temperature range of the temperature dependence of the equilibrium between the trans–trans and trans–gauche[BMIm]+ conformers, demonstrated hitherto only between 50 and 110 °C.28,30 Unexpectedly, no significant change in the intensity relation of the 730 cm–1 Raman mode (trans–trans conformer) to the 602 cm–1 band (trans–gauche) could be determined for all temperatures (20, –60, and –150 °C). This can be understood by the assumption that the mentioned equilibrium is frozen and the rotational formation of the different conformers is hindered.
The crystal-structure determination of 2 was carried out at –50 °C (Table S1),† resulting in the monoclinic space groupP21/n (trans–trans conformer), without any indication of a structural disorder. So, the low temperature Raman frequencies of 2 are not in complete accordance with the crystal structure (determination). An explanation could be that the X-ray radiation during the measurement overcomes the rotational hindering from the trans–gauche to the trans–trans conformers of [BMIm]+. In Fig. 7 the Raman spectra of compound 2 at 20 and –60 °C are shown.
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Fig. 7 FT-Raman spectra (λexc. = 1064 nm) of crystalline [BMIm]2[CH3SO4]2[18-crown-6] at –60 and 20 °C. The Raman intensity is given in arbitrary units. |
Considering the Raman spectra of the investigated compounds, it can be noticed that the vibrational modes of the ionic units and the 18-crown-6 molecules superimpose as mentioned; also, the “molecular groups” in the relevant species (e.g., CH3, CH2, CH, imidazole ring, –SO3) give rise to uncoupled vibrations and hence to Raman bands in typical frequency regions. In consequence, single component modes e.g. CH3 from CH3SO4–, CH3SO3– or CH3 (ring substituent) are superpositioned and not always at their original frequency value anymore. Therefore, the assignments are done to groups in Table S1 (ESI).†
The assignments of the Raman frequencies of 1–4 are first related to the ionic components (IL) and 18-crown-6 (cr). The noticeable modes of the respective anions, [CH3SO4]–, [CH3SO3]–, and [CF3SO3]–, are marked in italics in Table S1 (ESI).† Secondly, the frequency assignments are proposed to characteristic group frequencies in comparison to literature data partly based on sophisticated ab initio as well as on DFT computations. In the following, some related comments are given (c.f. Table S1, ESI).†
The most Raman bands of the title compounds belong to the imidazolium cations. The quasi-aromatic imidazolium contains “aromatic” C–H units with distinctive stretching modes in the area 3070–3200 cm–1, whereas the corresponding deformations are attributed to vibrations around 1300 cm–1.24,28–30 Furthermore, the imidazolium ring itself has characteristic bands in the region 1450–1570 cm–1 and at about 1150–1370 cm–1.29,31,33 The intensities of these modes can be affected by the kind and number of the ring (alkyl) substituents. The frequencies in the region 2800–3000 cm–1 are a result of the aliphatic CH3 and CH2 stretching vibrations (superpositioned by CH3groups of the respective anions and CH2 units of 18-crown-6). Corresponding CH3 and CH2 bending modes are found at 1350–1440 and around 1100–1200 cm–1, respectively. Butyl substituent in 2 further contributes a number of vibrations in the region from about 500 to 800 cm–1 caused by alkyl chain orientations. As mentioned, two different conformers, trans–trans and trans–gauche, could be identified by Raman spectroscopy at room temperature.28–30
Recently, [BMIm][CH3SO4] was studied in relation to the formation of solutions with some n-alkanes and aromatic hydrocarbons.34 Unfortunately, IR and Raman data of methylsulfate, [CH3SO4]–, are daunting,35 nevertheless the characteristic νs(SO3) can be attributed to the strong Raman band at 1061 cm–1 for 1 and 2, and νs(SO2) is assigned to the medium bands at 1144 cm–1 (1) and 1146 cm–1 (2), respectively. The methanesulfonate ion, [CH3SO3]–, in 3 exhibits C3v symmetry. The vibrational spectrum for this anion has been published for several compounds.36 In accordance with literature data, the characteristic Raman frequencies are assigned as νs(SO3): 1042 cm–1, νas(SO3): 1203 cm–1, δs(SO3): 551 cm–1 and δas(SO3): 526 cm–1.
The triflate ion, [CF3SO3]– in 4 also exhibits C3v symmetry. All fundamental triflate vibrations are situated below 1400 cm–1 (meaning also below most of the CH3 and CH2 bending modes).37 Most of its vibrational modes can be ascribed to the SO3 and CF3 units, respectively. Very strong νs(SO3) at 1033 cm–1 dominates the Raman spectrum of 4 in the region below 1500 cm–1, and νas(SO3) comes out at 1246 cm–1 with weak–medium intensity. The deformation δs(SO3) is attributed to the weak–medium Raman band at 572 cm–1. The Raman mode at 1226 cm–1 is ascribed to the symmetric CF3 stretching, and δs(CF3) is the strong band at 756 cm–1. For further details, see Table S1 (ESI).†
Further details on the crystal structure investigations may be obtained from the Cambridge Crystallographic Data Centre (CCDC, 12 Union Road, Cambridge CB2 1EZ, fax (+44)1223-336-033, e-mail deposit@ccdc.cam.ac.uk) on quoting the depository numbers CCDC-648112 for compound 1, CCDC-648113 for compound 2, CCDC-648115 for compound 3 and CCDC-648114 for compound 4. For crystallographic data in CIF or other electronic format see DOI: 10.1039/b708724c
One reason for the enclosure of 18-crown-6 in imidazolium based salts is obviously the formation of dense packing, or alternatively a space filling. The enclosure of 18-crown-6 stabilizes the new structures according to their melting temperatures in relation to these of the corresponding pure imidazolium based salts.
From the crystal structure conclusive information can be drawn for the relevant species in the liquid state and also for possible reaction mechanisms. The use of crown ethers in molten salt systems (ILs) can result in the synthesis of new compounds by exchange reactions or equilibrium shifting as, e.g.
AB + CD + crown → [A(crown)D]↓ + C |
+ |
+ D |
– |
. |
Footnote |
† Electronic supplementary information (ESI) available![]() ![]() |
This journal is © The Royal Society of Chemistry 2008 |