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Mössbauer Spectroscopy and X-ray Diffraction Study of 57Fe-Labeled Tetrachloroferrate(III)-Based Magnetic Ionic Liquids

Int. J. Mol. Sci. 2012, 13(2), 1612-1619; doi:10.3390/ijms13021612

Tetrachloridocuprates(II)—Synthesis and Electron Paramagnetic Resonance (EPR) Spectroscopy
Alette Winter, André Zabel and Peter Strauch *
Institute of Chemistry, University of Potsdam, Karl-Liebknecht-Str. 24-25, D-14476 Potsdam/Golm, Germany
Author to whom correspondence should be addressed; Tel.: +49-331-977-5190; Fax: +49-331-977-5268.
Received: 4 January 2012; in revised form: 23 January 2012 / Accepted: 29 January 2012 / Published: 2 February 2012


: Ionic liquids (ILs) on the basis of metal containing anions and/or cations are of interest for a variety of technical applications e.g., synthesis of particles, magnetic or thermochromic materials. We present the synthesis and the results of electron paramagnetic resonance (EPR) spectroscopic analyses of a series of some new potential ionic liquids based on tetrachloridocuprates(II), [CuCl4]2−, with different sterically demanding cations: hexadecyltrimethylammonium 1, tetradecyltrimethylammonium 2, tetrabutylammonium 3 and benzyltriethylammonium 4. The cations in the new compounds were used to achieve a reasonable separation of the paramagnetic Cu(II) ions for EPR spectroscopy. The EPR hyperfine structure was not resolved. This is due to the exchange broadening, resulting from still incomplete separation of the paramagnetic Cu(II) centers. Nevertheless, the principal values of the electron Zeemann tensor (g and g) of the complexes could be determined. Even though the solid substances show slightly different colors, the UV/Vis spectra are nearly identical, indicating structural changes of the tetrachloridocuprate moieties between solid state and solution. The complexes have a promising potential e.g., as high temperature ionic liquids, as precursors for the formation of copper chloride particles or as catalytic paramagnetic ionic liquids.
tetrachloridocuprate(II); electron paramagnetic resonance; copper(II); ionic liquid

1. Introduction

Ionic liquids (ILs) or ionic liquid crystals (ILCs) on the basis of metal containing anions and/or cations are of interest for a variety of technical applications e.g., as precursors for synthesis of (nano)particles, magnetic or thermochromic materials [13] or for usage as extraction agents [4] or catalysts [58]. Tetrahalidometalate complexes can combine many of these desired properties: Liquid-crystalline ionic liquids based on tetrahalidometalates (M = Co, Ni) have been reported first in 1996 by C.J. Bowlas, D.W. Bruce and K.R. Seddon [9]. In 2001 F. Neve et al. [1013] showed that tetrahalidocuprate(II) complexes with alkylpyridinium cations including an alkyl chain length of n ≥ 12 are thermotropic liquid crystals. With shorter alkyl chains, they are ionic liquids. Additionally, alkylpyridinium tetrahalidocuprate ILs and ILCs have also been used as precursors for inorganic materials [2,14,15]. For the purpose of a deeper understanding of the thermotropic behavior of these N-alkylpyridinium salts, they were further investigated starting from the chain length of n = 9–18 [10,11]. R.D. Willett et al. already reported in 1974 one of the most striking examples of the copper(II) chloride complexes characterized by the phenomena of thermochromism which is interpreted in the same work as a phase transition leading to the change in the coordination geometry [16]. The compound forms bright green crystals at room temperature. When heated above 43 °C, the compound suddenly turns yellow and the color change is reversible. The compounds of our series do not show any thermochromic behavior in the investigated temperature range (up to 120 °C).

Metal containing ionic liquids provide also the interesting feature of being electrochromic and/or magnetic [17,18]. With their already known properties such as tunable acidity, polarity, amphiphilic character, coordinating ability, and miscibility with various compounds and properties due to the metal ion, these ILs could be the best candidates as catalysts for many chemical reactions as well as alternative solvents and morphology templates for inorganic materials at the same time. However, reports on tetrahalidometalate-based ILs/ILCs and their applications as well as their characterization are relatively rare [2,1013,1932]. This is somewhat surprising because metal containing ILs and ILCs may open the door towards a new valuable branch of IL research, due to its additional properties such as color, geometry, and magnetism, proffered by the metal ion composition.

We present the syntheses and the results of electron paramagnetic resonance (EPR) spectroscopic analyses including temperature dependent measurements of some new tetrachloridocuprate(II) compounds with the following sterically demanding cations: hexadecyltrimethylammonium (C16H33Me3N+), tetradecyltrimethylammonium (C14H29Me3N+), tetrabutylammonium (Bu4N+) and benzyltriethylammonium (BzlEt3N+) ions (see Figure 1). They were used to achieve a reasonable separation of the paramagnetic Cu(II) ions for EPR spectroscopy.

2. Results and Discussion

EPR spectroscopy offers a good method for the investigation of Cu(II) compounds because of its high sensitivity towards diamagnetic systems and the accessibility to measure the samples in various physical states, i.e., liquids and solids (powder, crystal and frozen solution); moreover the investigation of flexible systems like ILs on the basis of tetrachloridocuprate(II). For EPR investigations of pure ionic liquids or crystalline powder samples one problem arises. The paramagnetic interactions usually exceed the limits of the individual complex. Therefore, we use sterically rather demanding ammonium cations to separate the paramagnetic tetrachloridocuprate(II) moieties to achieve a minimum of magnetic interactions between the Cu(II) centers. Nevertheless, due to line broadening because of an incomplete separation of the paramagnetic centers, no hyperfine structure was observed (63Cu, 65Cu; nuclear spin I = 3/2 each). In addition, the four chlorido ligands lead to a further splitting of the signals (35Cl, 37Cl; nuclear spin I = 3/2 each) which is also not resolved and contributes to the line broadening in the EPR spectra. Finally, we succeeded in recording EPR spectra of our series which allowed us to determine the g-tensor parameters (g and g).

Figure 2 shows two characteristic spectra of powdered samples of this series (C16H33Me3N)2[CuCl4] (1) and (BzlEt3N)2[CuCl4] (4). The spectra are all of axial symmetry and g as well as g can be determined (see Table 1). In Table 1 the averaged g-values gav calculated from the following simple expression for axial symmetry are also listed:

g av = g | | + 2 · g 3

The gav-value corresponds to the isotropic giso-value of liquid systems (e.g., solutions or ionic liquids). The table also contains an example of a diamagnetically diluted ionic liquid bis(n-butylpyridinium)tetrachloridocuprate/zincate(II), (BuPy)2[Cu/ZnCl4]. In this spectrum the parallel part of the copper hyperfine structure is reasonably resolved [33]. The variation of the parameters reflects the degree of structural flexibility of the tetrachloridocuprate(II) moiety. With a series of known X-ray structures combined with EPR parameters of tetrachloridocuprates(II), it was possible to classify the degree of distortion between square planar and tetrahedral geometries, as it was recently shown for tetrabromidocuprates(II) [34].

A sample of (C14H29Me3N)2[CuCl4] (2), was investigated by EPR at various temperatures. Figure 3 summarizes the results of the X-band EPR measurements of a powdered sample of 2, measured in a temperature range from 150 to 390 K in 10 K steps. The spectrum at 150 K is comparable to the spectra shown in Figure 2. Interestingly, the signal continuously decreases with rising temperatures and disappears fully above ~350 K. The significant decrease in intensity of the spectra might be attributed to saturation effects depending on the energy gap between the ground state and the first excited state in the [CuCl4]2− unit. This effect is completely reversible in the investigated temperature range, indicating that the compound is also stable at higher temperatures without any signs of decomposition (at least at 390 K).

3. Experimental Section

3.1. Chemicals

The following chemicals were used without further purification. Copper(II) chloride (98%), copper(II) chloride dihydrate (99%), hydrochloric acid (37%), ethanol anhydrous (99%), potassium bromide (Uvasol, for IR spectroscopy), hexadecyltrimethylammonium chloride (>95%), tetrabutylammonium chloride (95%), benzyltriethylammonium chloride (>98%), tetradecyltrimethylammonium chloride (>98%), 2-propanol (99.5%), diisopropyl ether (100%).

3.2. Preparation

In general, tetrachloridocuprate(II) complexes can be achieved by different procedures [3538], three of them are mentioned here. (1) At first the internal [CuCl4]2− coordination sphere is prepared by dissolving copper(II) chloride dihydrate in hydrochloric acid (37% wt). This is followed by addition of the counter ion as chloride salt dissolved in 2-propanol. After 30 minutes heating under reflux the solvent is evaporated until the complex precipitates [36]; (2) In a second synthetic protocol the internal coordination sphere is obtained in situ by adding an ethanolic solution of a stoichiometric amount of CuCl2 to the chloride salt of the cation dissolved in a minimum volume of 2-propanol. The solution is evaporated and the remaining complex is washed with diisopropyl ether [37]; (3) For a third procedure CuCl2 is added to an ethanolic solution of the chloride salt of the appropriate cation. The reaction mixture is heated under reflux for one hour and the product is precipitated by evaporating the solvent [38].

3.3. Bis(hexadecyltrimethylammonium) Tetrachloridocuprate(II), (C16H33Me3N)2[CuCl4] (1)

According to the second synthesis approach, for complex 1 2.0 mmol (0.64 g) of C16H33Me3NCl were dissolved in 1.5 mL of 2-propanol and 1.0 mmol (0.14 g) of copper(II) chloride were dissolved in 0.3 mL of ethanol. Subsequently, both solutions were combined and cooled. An orange-red powder was obtained and separated by filtration.

Melting point: 85–86 °C. Yield: 0.74 g (95%). Elemental analysis calculated for C38H84N2CuCl4 (774.45): C 58.93, H 10.93, N 3.62 (%); found: C 58.17, H 11.27, N 3.61 (%). IR (KBr, cm−1): 2953 m, 2919 s, 2850 s, 1468 m, 963 m, 911 w, 721 w.

3.4. Bis(tetradecyltrimethylammonium) Tetrachloridocuprate(II), (C14H29Me3N)2[CuCl4] (2)

The complex 2 was prepared following the second procedure briefly mentioned above. 1.0 mmol (0.14 g) of copper(II) chloride, previously dissolved in 0.3 mL of ethanol, were added to 2.0 mmol (0.58 g) of C14H29Me3NCl dissolved in 1.5 mL of 2-propanol. The complex precipitated as orange powder.

Melting point: 83–85 °C. Yield: 0.61 g (85%). Elemental analysis calculated for C34H76N2CuCl4 (718.35): C 56.84, H 10.66, N 3.90 (%); found: C 58.11, H 11.03, N 4.15 (%). IR (KBr, cm−1): 2952 m, 2920 s, 2850 s, 1468 m, 966 w, 911 w, 722 w.

3.5. Bis(tetrabutylammonium) Tetrachloridocuprate(II), (Bu4N)2[CuCl4] (3)

This complex was synthesized via the third procedure using the following quantities: 0.5 mmol (0.07 g) of CuCl2 were added to 1.0 mmol (0.28 g) of Bu4NCl dissolved in 6 mL of ethanol and heated under reflux for one hour. Afterwards the alcoholic solution was evaporated until a dark red powder precipitated.

Melting point: 94–98 °C. Yield: 0.20 g (58%). Elemental analysis calculated for C32H72N2CuCl4 (690.29): C 55.68, H 10.51, N 4.06 (%); found: C 53.62, H 11.35, N 3.93 (%). IR (KBr, cm−1): 2962 s, 2873 ms, 1485 m, 1462 w, 1382 m, 881 m, 802 w, 739 mw.

3.6. Bis(benzyltriethylammonium) Tetrachloridocuprate(II), (BzlEt3N)2[CuCl4] (4)

Following the first synthesis, for complex 4 1.0 mmol (0.23 g) of BzlEt3NCl were dissolved in 5 mL of 2-propanol and mixed with 0.5 mmol (0.09 g) of copper(II) chloride dihydrate, previously dissolved in 0.6 mL of hydrochloric acid. The mixture was heated for 30 min, after that the solution was evaporated. A yellow powder was obtained and washed with diisopropyl ether.

Melting point: 107–109 °C. Yield: 0.20 g (69%). Elemental analysis calculated for C26H44N2CuCl4 (590.00): C 52.93, H 7.52, N 4.75 (%), found: C 52.61, H 7.01, N 4.74 (%). IR (KBr, cm−1): 3059 w, 2985 m, 2944 w, 1582 w, 1479 s, 1453 w, 1390 ms, 1210 m, 1153 s, 1007 s, 900 m, 792 s, 752 s, 708 s, 603 w, 537 w, 462 w.

The UV/Vis spectra of all four compounds in solution (CH3CN, λmax/nm) are nearly identical with three characteristic absorptions: 256, 311, 462 nm.

4. Conclusions

A series of four potential high temperature ionic liquids on the basis of tetrachloridocuprate(II) anions with different sterically demanding cations has been studied by EPR spectroscopy as solid samples. These large cations are necessary for a reasonable separation of the paramagnetic Cu(II) centers. The spectra are all of axial symmetry. At lower temperatures (150 K) they show no resolved hyperfine pattern, but allow the determination of the g-tensor main values g and g. From these values it is also possible to calculate the averaged g-values gav which are comparable to the isotropic g-values of liquid systems. According to possible saturation effects, the signal in the EPR spectra decreases with increasing temperature and totally disappears at temperatures higher than about 350 K. This behavior is completely reversible and proves the thermal stability of these compounds at least up to 390 K.

From the very close UV/Vis absorption bands, one can conclude that all complexes in this series exhibit related coordination geometries of the [CuCl4]2− unit. The compounds 14 do not show any thermochromic behavior up to 390 K. Even though the solid substances show slightly different colors in solid state, the UV/Vis spectra are nearly identical, indicating structural changes of the tetrachloridocuprate moieties between solid state and solution. The compounds have a promising potential e.g., as high temperature ionic liquids, as precursors for the formation of copper chloride particles or as catalytic paramagnetic ionic liquids.


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Figure 1. Cations of the CuCl4 salts 14.
Figure 1. Cations of the CuCl4 salts 14.
Ijms 13 01612f1 1024
Figure 2. X-band powder electron paramagnetic resonance (EPR) spectra of 1 and 4 measured at 150 K.
Figure 2. X-band powder electron paramagnetic resonance (EPR) spectra of 1 and 4 measured at 150 K.
Ijms 13 01612f2 1024
Figure 3. X-band EPR spectra of 2 (measured in a temperature range from 150 to 390 K in 10 K steps).
Figure 3. X-band EPR spectra of 2 (measured in a temperature range from 150 to 390 K in 10 K steps).
Ijms 13 01612f3 1024
Table 1. Experimental EPR parameters (g- and g-values) measured at 150 K.
Table 1. Experimental EPR parameters (g- and g-values) measured at 150 K.
(C16H33Me3N)2[CuCl4] (1)2.365 ± 0.0052.145 ± 0.0052.218 ± 0.005
(C14H29Me3N)2[CuCl4] (2)2.366 ± 0.0052.141 ± 0.0052.216 ± 0.005
(Bu4N)2[CuCl4] (3)2.394 ± 0.0052.081 ± 0.0052.185 ± 0.005
(BzlEt3N)2[CuCl4] (4)2.424 ± 0.0052.089 ± 0.0052.200 ± 0.005
(BuPy)2[Cu/ZnCl4] [33]2.300 ± 0.0052.070 ± 0.0052.147 ± 0.005
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