From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding

Chemistry
 

Summary

A protocol for the synthesis of a new type of mesogens, based on the halogen-bonded supramolecular anion [CnF2n+1-I···I···I-CnF2n+1], is reported.

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Cavallo, G., Bruce, D. W., Terraneo, G., Resnati, G., Metrangolo, P. From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding. J. Vis. Exp. (133), e55636, doi:10.3791/55636 (2018).

Abstract

Herein, we demonstrate that a bottom-up approach, based on halogen bonding (XB), can be successfully applied for the design of a new type of ionic liquid crystals (ILCs). Taking advantages of the high specificity of XB for haloperfluorocarbons and the ability of anions to act as XB-acceptors, we obtained supramolecular complexes based on 1-alkyl-3-methylimidazolium iodides and iodoperfluorocarbons, overcoming the well-known immiscibility between hydrocarbons (HCs) and perfluorocarbons (PFCs). The high directionality of the XB combined with the fluorophobic effect, allowed us to obtain enantiotropic liquid crystals where a rigid, non-aromatic, XB supramolecular anion acts as mesogenic core.

X-ray structure analysis of the complex between 1-ethyl-3-methylimidazolium iodide and iodoperfluorooctane showed the presence of a layered structure, which is a manifestation of the well-known tendency to segregation of perfluoroalkyl chains. This is consistent with the observation of smectic mesophases. Moreover, all the reported complexes melt below 100 °C, and most are mesomorphic even at room temperature, despite that the starting materials were non-mesomorphic in nature.

The supramolecular strategy reported here provides new design principles for mesogen design allowing a totally new class of functional materials.

Introduction

Intermolecular interactions play a very important role in determining physical and chemical properties of bulk materials. When a new interaction becomes available, new structures, namely, new functions, become available. Therefore, exploring novel, specific non-covalent interactions underlying an intermolecular recognition process may open new perspectives in different fields such as materials sciences, catalysis, drug design, supramolecular chemistry, and crystal engineering. This was the case for the XB that recently became a routine tool for controlling aggregation and self-assembly phenomena1,2,3,4,5.

According to the IUPAC definition6: "A halogen bond occurs when there is evidence of a net attractive interaction between an electrophilic region associated with a halogen atom in a molecular entity and a nucleophilic region in another, or the same, molecular entity." A schematic representation of the XB is given in Figure 1, where X is the electrophilic halogen atom (Lewis acid, XB donor) and Y is a donor of electron density (Lewis base, XB acceptor).

Figure 1
Figure 1: Schematic representation of the halogen bond.
The electrophilic halogen atoms (XB-donors) are covalently linked to a wide variety of molecular scaffolds (R), while the XB-acceptors (Y) can be neutral or anionic species. This figure has been reprinted from reference2. Please click here to view a larger version of this figure.

At first sight, it may seem that this definition tackles somewhat puzzling aspects, since halogen atoms, because of their high electronegativity, are typically considered as sites of high electron density. However, the behavior of halogen atoms as electrophiles is quite general and has been elegantly rationalized by Politzer et al. with the introduction of the "σ-hole" concept7.

When a halogen atom is involved in a covalent bond, an electron redistribution occurs and the electronic density becomes anisotropic8,9,10,11. The shape of the atom becomes oblate and a region of positive electrostatic potential (the so-called σ-hole) develops along the extension of the covalent bond, on the outermost surface of the halogen atom (Figure 2A). This positive region is surrounded by a belt of negative electrostatic potential, orthogonal to the covalent bond. This model seems to solve the "enigma" of the XB since it explains the non-covalent interaction pattern of covalently-bonded halogen atoms, and the associated directional preferences, i.e., linear interactions with nucleophiles and lateral interactions with electrophiles.

Figure 2
Figure 2: Anisotropic distribution of electron density around halogen atoms. (A) Schematic representation of the anisotropic distribution of the electron density around covalently bound halogen atoms and the pattern of the resulting interactions. (B) Molecular electrostatic potential maps at the isodensity surface with 0.001 au for CF4, CF3Cl, CF3Br, and CF3I. Color ranges: red, greater than 27 kcal/mol; yellow, between 20 and 14 kcal/mol; green, between 12 and 6 kcal/mol; blue, negative. This figure has been modified from reference2. Please click here to view a larger version of this figure.

XB has rapidly grown from a scientific curiosity to one of the most interesting noncovalent interactions in designing functional supramolecular materials12,13,14,15,16, thanks to its unique features, i.e., high directionality, tunable interaction strength, hydrophobicity, and donor atom dimensions1. The high directionality of XB can be easily understood by considering the focused nature of the σ-hole, while the interaction strength frequently correlates to the magnitude of the σ-hole. Both the size (the spatial range) and the magnitude (the value of the maximum electrostatic potential VS,max) of the σ-hole are affected by the polarizability and electronegativity of the halogen atom and the electron-withdrawing ability of the substituents in the neighborhood of the halogen17 (Figure 2B). As a general trend, as the halogen atom becomes more polarizable and the substituents on the molecule become more electron-withdrawing, the halogen σ-hole becomes more positive. Therefore, for a given R, VS,max increases in the order F < Cl < Br < I, namely it increases with the halogen atom polarizability and decreases with its electronegativity. For a given halogen, VS,max becomes more positive when the electron-withdrawing ability of R is increased. Therefore, haloperfluorocarbons, specifically iodo-perfluoroalkanes and arenes, can act as powerful XB-donors forming particularly strong interactions18,19,20 and particularly hydrophobic adducts.

A case of PFC-HC self-assembly to give cocrystals has been reported in the late 1990s21. Upon mixing equimolar amounts of 1,2-diiodotetrafluoroethane and N,N,N',N'-tetramethyl-ethylenediamine in chloroform, a supramolecular complex was isolated as white crystals stable in air at room temperature. Single crystal X-ray analysis revealed that the two components alternate in a 1-dimentional (1D) infinite chain and the interaction between the nitrogen and iodine atoms is largely responsible for keeping the perfluorinated bis-iodide in place. This proved that the nitrogen-iodine XB interaction is strong enough to overcome the low affinity existing between PFC and HC compounds and suggested that XB can be successfully exploited as an easy route to introduce fluorinated moieties into any new supramolecular materials22,23,24, including liquid crystalline materials.

Fluorinated substituents, in fact, have been successfully incorporated into liquid crystalline molecules because of the excellent stability that is offered by the C-F bond as well as the small size and the low polarizability of the fluorine atom, which gives rise to very low intermolecular dispersion interactions25,26,27. Moreover the segregation occurring between PFC and HC chains allowed control over supramolecular liquid-crystalline phases, enhancing the smectic character of a mesomorphic material28,29,30. It is generally understood that both the physical/chemical properties and the mesomorphism are strongly affected by the molecular architecture29,31. Thus, an appropriate molecular design is essential to generate new supramolecular liquid crystals with tailored properties. The basic motif of these soft materials lies in a fairly rigid, rod-like moiety linked to one or two flexible aliphatic chains32,33,34. The conventional design of mesomorphic compounds was mainly performed with neutral species but studies have shown that also ionic pairs can exhibit a mesomorphic behavior, yielding materials with properties at the interface between ionic liquids and liquid crystals35,36,37.

Taking into account recent results on XB liquid crystals24,38,39, and the specific ability of anions to act as XB-acceptors, it seemed particularly interesting to exploit this non-covalent interaction in designing new types of ILCs.

1-Alkyl-3-methylimidazolium iodides (1-m) of various chain-length, which are known as ionic liquids40, were used for the synthesis of the complexes (Figure 3)41,42. Note that only 1-12, bearing a C12 alkyl chain, exhibits liquid crystallinity with smectic A (Sm A) phase (crystal (Cr) to SmA transition temperature = 27 °C; Sm A to isotropic liquid (ISO) transition temperature = 80 °C; Cr • 27 • SmA • 80 • Iso)43. Imidazolium salts were reacted with iodoperfluorooctane (2-8) and iodoperfluorodecane (2-10), which are well-known XB-donors44,45.

Figure 3
Figure 3: Synthetic scheme. Chemical formulae of starting ionic liquids (1-m), iodoperfluoroalkanes (2-n), and related XB-complexes 1-m•2-n. Please click here to view a larger version of this figure.

The iodide anions are expected to participate readily as XB-acceptor in the formation of supramolecular structures with haloperfluoroalkanes44. However, it remains challenging to anticipate the number and topology of the coordinated XB-donor species. In fact, halide anions typically are involved in two or three XBs46,47,48, but higher coordination numbers were also observed49,50.

Herein, we describe a procedure for obtaining highly fluorinated XB ILCs and a detailed procedure for the identification and characterization of the occurrence of XB. The sequence of analysis reported here and utilized to identify the XB can be considered as a general procedure and can be applied to the characterization of any type of XB system.

Protocol

Note: Reactions were carried out in oven-dried glassware under nitrogen atmosphere. Please follow the safety measures described in the MSDS of each chemical.

1. Synthesis of 1-Alkyl-3-methylimidazolium Iodide Salts (1-m, Figure 3)

  1. In a three-necked, round-bottomed flask equipped with a reflux condenser fitted with a nitrogen inlet, a thermometer, a magnetic stirring bar, and a heating oil bath, dissolve 1.5 g (0.018 mol, 1 equiv) of freshly distilled 1-methyl-imidazole and 1.3 equiv of the 1-iodoalkane (chain length from C2 to C12) in 10 mL of acetonitrile.
  2. Heat the reaction mixture to reflux (75 - 80 °C internal temperature) overnight under nitrogen atmosphere and then cool the mixture down to room temperature.
  3. Remove the volatile materials from the resulting mixture under reduced pressure at 50 °C, using a rotatory evaporator.
    NOTE: Imidazolium salts are highly hygroscopic and they quickly absorb water from the air. Thus, it is recommended to store them in a desiccator until use.

2. Synthesis of 1-m • 2-n XB Complexes

  1. Procedure 1: From solution (only for 1-2 • 2-8 in Figure 1)
    1. Prepare a solution of the 1-ethyl-3-methylimidazolium iodide (1-2, MW = 238.07 g/mol) by dissolving 50 mg (0.21 mmol, 1 equiv) of 1-2 in 0.5 mL of acetonitrile.
    2. Prepare a solution of the perfluorooctyl iodide (2-8, MW = 545.96 g/mol) by dissolving 229 mg (0.42 mmol, 2 equiv) of 2-8 in 0.5 mL of acetonitrile.
    3. Mix the two solutions in a vial and keep the vial in a jar filled with paraffin oil.
    4. Let the solvent diffuse slowly in the paraffin oil at room temperature. After a period ranging from 3 to 7 days, good-quality single crystals suitable for X-ray diffraction analysis were obtained.
  2. Procedure 2: Melt methodology
    NOTE: This methodology requires an air-sealed system to mitigate against the volatility of the iodoperfluoroalkanes.
    1. Mix each 1-alkyl-3-methylimidazolium iodide (1-m) with the appropriate iodoperfluoroalkanes (2-n) in a 1:2 molar ratio in a clear borosilicate glass vial equipped with a magnetic stirring bar.
    2. Close the vial and put it into an oil bath under vigorous stirring.
    3. Heat at 70 °C using a hot plate for 15 min then cool the mixture down to room temperature.

3. 1H and 19F NMR Experiments

NOTE: 1H NMR and 19F NMR spectra were recorded at 25 °C on a NMR spectrometer operating at 499.78 MHz for 1H and 470.21 MHz for 19F, and using CDCl3 as the solvent. TMS and CFCl3 were used as internal standards for calibrating the chemical shifts in 1H NMR and 19F NMR, respectively. Bis-(2,2,2-trifluoroethyl) ether that contains both hydrogen and fluorine nuclei, was used as internal standard for establishing the ratio between 1-m and 2-n in the cocrystals.

  1. Preparation of the sample for NMR analysis and spectra calibration
    1. Dissolve about 10 mg of each complex 1-m • 2-n in 0.5 mL of CDCl3.
    2. Add 1 µL of 2,2,2-trifluoroethyl ether using a micropipette.
    3. Lock the sample, set the acquisition parameters as reported in Table 1, and record 1H and 19F NMR consecutive spectra, without removing the NMR tube from the magnet, in order to operate under the same operating conditions.
    4. Calibrate the integration parameters so that in the 1H NMR spectra the CH2O quartet of bis(2,2,2-trifluoroethyl) ether (δ = 4.3 ppm) corresponds to four, and in the 19F NMR spectra the CF3 triplet (δ = −74.5 ppm) of 2,2,2-trifluoroethyl ether corresponds to six.
    5. Calculate the ratio of the -CF2-I signal area deriving from 2-n (δ = −61.2 ppm in the 19F NMR spectra) and the -CH3 signal area deriving from 1-m (δ ≈ 4.0 ppm in the 1H NMR spectra), in order to evaluate the ratio between 2-n and 1-m in each complex.

4. Preparation of the Sample for Hot Stage Polarized Optical Microscopy (POM)

  1. Prepare a thin layer of the sample by placing a spatula tip amount of the supramolecular complex 1-m• 2-n between two micro cover glasses (18 mm x 18 mm).
  2. Place the sample in the hot stage between two crossed polarizers, and heat the sample to melt.
  3. Submit the sample to repeated heating/cooling cycles in order to promote phase transitions. Crystalline and liquid crystalline phases will interact with polarized light leading to brightness and color gradient, while the isotropic phase will appear dark.

Representative Results

Differential scanning calorimetry (DSC), POM, and thermogravimetric analysis (TGA), as well as 1H and 19F NMR were used to characterize the obtained complexes. Good-quality single crystals of 1-2•2-8 were obtained from a 1:2 solution of the starting components in acetonitrile by slow evaporation of the solvent at room temperature.

DSC analyses on mixtures of 1-2 and 2-8 with different stoichiometric ratios, allowed us to derive that the right coordination stoichiometry between the imidazolium salt and the iodoperfluoroalkane is 1:2. In fact, the DSC thermogram of the 1:1 complex in Figure 4A shows the presence of the uncomplexed imidazolium salt 1-2 (peak at 57 °C), while in the 1:3 complex there is an excess pure 2-8 (melting point 24 °C). On the other hand, the thermogram of the 1:2 complex shows a single peak distinct from those of the starting compounds, demonstrating that a new pure crystalline species was formed.

TGA analyses confirmed this result. In fact, only upon mixing 1-12 and 2-10 in 1:2 ratio, a homogenous sample was obtained, which released quantitatively the fluorinated building block at a temperature higher than the uncomplexed iodoperfluorodecane (Figure 5A and 5B).

19F NMR has been applied as a simple, effective, and sensitive tool to detect the formation of XB adducts. The XB between the electron deficient iodine of the iodoperfluoroalkanes and the I- anion strongly influences the signals of the -CF2-I group (δ = −60,0 ppm) and gives rise to detectable upfield shifts of the 19F NMR resonances. A Δδ value of 1.2 ppm was measured for complex 1-2•2-8, confirming the occurrence of attractive noncovalent interactions involving halogen atoms as electrophilic species (Figure 6). Moreover, by recording consecutive 1H and 19F NMR analyses in the presence of 2,2,2-trifluoroethyl ether as the internal standard for signal integration, the 1:2 stoichiometry between the XB-acceptor and donor modules has been further confirmed.

Single crystal X-ray analysis of 1-2•2-8 confirmed that the XB drives the formation of a trimeric supramolecular complex where the iodide anion acts as a bidentate XB-acceptor, binding two fluorinated chains. The I···I- distances are almost the same [3.4582(9) Å and 3.4625(10) Å] and roughly correspond to 27% shortening with respect to the sum of the vdW and Pauling radii of the iodine atom and iodide anion, respectively51. The high directionality of XB is confirmed by the C-I···I- angles of 174.1(1)° and 175.4(2)°, respectively (Figure 7A). Two equally-populated conformations are observed for the imidazolium cations, which lie approximately on the same plane and are related by a non-crystallographic twofold axis. Figure 7B shows the separation between the ionic and neutral parts, as well as between the HC and PFC chains, within the crystal (disorder removed).

DSC and POM studies revealed that all complexes melted at temperatures lower than 100 °C (Figure 8A), as typical for ionic liquids. Furthermore, they all show an enantiotropic liquid crystalline behavior, some at room temperature, with SmB and SmA phases (Figure 8A). On cooling, the SmA-SmB transition was identified by the characteristic striations across the back of the fans (Figure 8B,left). The striations disappeared on cooling further below the transition.

Figure 4
Figure 4: Differential Scanning Calorimetry. DSC thermograms of samples prepared by mixing 1-2 and 2-8 in different stoichiometric ratios: 1:3 sample (top), 1:2 sample (mid), and 1:1 sample (bottom). Please click here to view a larger version of this figure.

Figure 5
Figure 5:Thermal Analysis. DSC heating/cooling cycles (A) and TGA analysis (B) on a sample prepared by mixing 1-12 and 2-10 in a 1:2 molar ratio. This figure has been modified from reference37. Please click here to view a larger version of this figure.

Figure 6
Figure 6:19F NMR Analysis. 19F NMR spectra in CDCl3 of 2-8 (top) and related halogen-bonded complex 1-2•2-8 (bottom). Please click here to view a larger version of this figure.

Figure 7
Figure 7: X-ray single crystal analysis. (A) The asymmetric unit of the complex 1-2•2-8 showing the formation of a trimeric superanion where two fluorinated chains are bonded to the central I- anion (a single conformer of the disordered cation is reported); (B) The imidazolium salt 1-2 and the iodoperfluorooctane 2-8 segregate along the crystallographic b-axis; (C) Side view showing ionic and fluorocarbon areas of the structure. Color code: grey, carbon; blue, nitrogen; magenta, iodine; green, fluorine; white, hydrogen. Halogen bonds depicted as grey lines. Please click here to view a larger version of this figure.

Figure 8
Figure 8: Polarized Optical Microscopy. (A) Chart of thethermal transitions of halogen-bonded complexes 1-m•2-n measured by hot-stage POM (blue is solid, red is SmB, and orange is SmA phases). (B) Optical textures of the smectic phases observed for 1-12•2-10 on cooling from the isotropic state. Left: SmB phase at 77 °C; Right: SmA phase at 83 °C.Scale bar: 100 µm. This figure has been modified from reference37. Please click here to view a larger version of this figure.

Spectral width (KHz) Scans number Pulse delay (s)
1H 7 16 1
19F 95 16 1

Table 1: Acquisition parameters for 1H and 19F NMR experiments

Discussion

We have reported an easy and versatile protocol for the synthesis of XB fluorinated ILCs in which mesomorphicity is driven by the supramolecular anions [CnF2n+1-I∙∙∙I∙∙∙I-CnF2n+1]-.

It is well-established that ionic liquids based on 1-alkyl-3-methylimidazolium salts can exhibit liquid crystalline behavior. However, whatever the anion, no mesophases were observed for compounds with alkyl chains shorter than 12 carbon atoms. Therefore, the most striking aspect of the reported materials is that it is the anisotropy of the XB anion that determines mesophase formation. In fact, the strict geometrical constraints of XB impose that the intermolecular interaction occurs along the extension of the C-I bond, at the sigma hole, with angles close to 180°. The iodide anions act as bidentate XB acceptors, binding two perfluorinated modules that show linear arrangement around the central iodide anion. Moreover, the fact that perfluoroalkyl chains are stiffer than equivalent HC chains, and adopt a twisted helical structure due to repulsion between 1,3-disposed CF2 groups9,52, further contributes to the generation of rigid, rod-like superanions.

This perfectly agrees with the observation that complexes containing the iodoperfluorodecane (2-10) show transition temperatures higher than those containing the iodoperfluorooctane (2-8) as the former is more anisotropic. Furthermore, the known tendency45,53 of fluoroalkanes to pack into lamellar phases determines the obtainment of SmB and SmA phases.

The superfluorinated ILCs reported in this paper demonstrate for the first time the application of the XB in the construction of ILCs based on imidazolium salts. Thanks to an accurate supramolecular design based on the high directionality of the XB and the fluorophobic effect, it is possible to obtain enantiotropic liquid crystals based on a rigid, non-aromatic, XB supramolecular synthon as the mesogenic core. The liquid crystalline behavior is independent from the length of the alkyl chains.

The supramolecular approach presented here represents an attractive platform for the design of new liquid crystalline materials and can provide new opportunities for the development of sophisticated functional materials such as room temperature ionic conductors, photoresponsive ILCs, and liquid crystalline electrolytes for application in energy devices.

Disclosures

The authors have nothing to disclose.

Acknowledgements

We gratefully acknowledge support from the grant, ERC-2012-StG_20111012 FOLDHALO (Grant Agreement no. 307108).

Materials

Name Company Catalog Number Comments
1-Methyl-imidazole  Sigma-Aldrich M50834-500G liquid reagent
1-Iodoethane Sigma-Aldrich I7780-100G liquid reagent
1-Iodobutane Sigma-Aldrich 167304-100G liquid reagent
1-Iodohexane Sigma-Aldrich 238287-100G liquid reagent
1-Iodooctane Sigma-Aldrich 238295-25G liquid reagent
1-Iododecane Sigma-Aldrich 238252-100G liquid reagent
1-Iodododecane Sigma-Aldrich 238260-100G liquid reagent
Acetonitrile Sigma-Aldrich 271004-1L organic solvent
Perfluorooctyl iodide  Apollo Scientific PC6170 fluorinated reagent/halogen-bond donor 
Perfluorodecyl iodide Apollo Scientific PC5970 fluorinated reagent/halogen-bond donor 
Bis(2,2,2-trifluoroethyl) ether  Sigma-Aldrich 287571-5G Internal standard for NMR
Chloroform-d Sigma-Aldrich 151823-100G Solvent for NMR

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