# Discotic Liquid Crystals Based on Cu(I) Complexes with Benzoylthiourea Derivatives Containing a Perfluoroalkyl Chain

Authors: Monica Iliş; Viorel Cîrcu
Journal: Journal of Chemistry
 (2018)

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## Abstract

Mesomorphic three-coordinate copper(I) complexes ([Cu(BTU)2X], where X = Cl or Br) based on a new N-benzoylthiourea (BTU) ligand with two decyloxy and one perfluorooctyl groups at its periphery were designed and prepared. The BTU ligand coordinates via the S atom in a neutral monodentate fashion as confirmed by IR and NMR spectroscopy data. The liquid crystalline behavior of these copper(I) complexes was investigated by a combination of polarized optical microscopy (POM), differential scanning calorimetry (DSC), and X-ray diffraction analysis (XRD), while their thermal stability was studied by thermogravimetric analysis (TGA). These new copper(I) complexes have mesomorphic properties and exhibit a hexagonal columnar mesophase over a large temperature range, more than 100°C.


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## Body

## 1. Introduction

Liquid crystalline compounds (LC) based on metal complexes (metallomesogens) represent a special class of liquid crystals with interesting properties related to metal ions employed, such as luminescence, magnetism, redox properties, and so on [1, 2]. The unique properties of thermotropic liquid crystals, in particular their electrooptical properties [3–7], have led to various applications (LCD, molecular sensors and detectors, optical switches, spatial light modulator, etc.) [8–10]. Metallomesogens based on copper(I) complexes are quite rare, even if the copper(I) can form complexes with low coordination number suitable for the stabilization of LC phases. The copper(I) complexes with liquid crystalline properties reported so far are restricted to few classes of ligands related to alkylthiolates [11], isocyanides [12–16], phenantroline [17], azamacrocycles [18], or Schiff bases derived from 2-iminopyridines [19, 20], giving rise to either mono- or binuclear two- or tetracoordinate complexes. Ionic columnar metallomesogens formed by three-coordinate copper(I) complexes with bis(1-pyrazolyl)ethyl ether ligands were reported by Lin and Lai [21]. In this study, we report a new class of copper(I) metallomesogens based on neutral copper(I) three-coordinate complexes with benzoylthiourea (BTU) ligands. These benzoylthiourea derivatives (BTU) proved to have excellent properties to bind to various metal ions due to the very strong donor groups (carbonyl and thioamide) that yield various transition metal complexes. The BTU ligands can give neutral homoleptic or heteroleptic complexes either with S- and O-coordination, when the ligand is coordinated in monoanionic bidentate form by deprotonation or with only S-coordination if the ligand is bound in neutral form to the metal center [22–32]. The reaction between copper(II) salts and, more generally, the versatile acylthiourea compounds leads to a variety of copper(I) complexes, including tetra- and three-coordinate mononuclear complexes, halide-bridged dinuclear complexes, or cluster-type polynuclear complexes, depending on the halide type and reaction conditions [33–39]. The complexity of the redox reaction between the copper(II) salts and thiourea compounds results from the combination between the versatility of the acylthiourea ligands and the coordination flexibility of the copper(I) ion. The three-coordinate copper(I) complexes, which possess two molecules of the BTU ligand linked via the sulfur atom and one halide ion, have approximately an overall planar shape [37–39]. The molecular shape arguments indicate that such complexes could be potential candidates for new liquid crystalline materials after careful functionalization of BTU derivatives with suitable mesogenic groups. The BTU compounds having terminal alkoxy groups at the both ends of the molecule show interesting mesogenic behavior, displaying nematic, smectic A, and smectic C phases, depending on the position and length of the alkyl chains [40]. On the contrary, partially fluorinated BTU compounds show comparable mesogenic properties, with an increased stability of lamellar phases and higher transition temperatures [41]. It is well known that the alkyl chains substitution with semi- or perfluoroalkylated chains leads to a serious increasing of both the transition temperatures and mesophases thermal ranges [42, 43]. Moreover, the stability of layered phases for such compounds with perfluoroalkyl groups is significantly increased due to the incompatibility between the aliphatic and perfluoroalkylated chains as well as the rigidity of the latter [44–50].This paper reports the preparation and mesogenic behavior of a new class of copper(I) metallomesogens based on copper(I) halide complexes (chloride or bromide) with a novel benzoylthiourea ligand that have at one side two decyloxy chains and, at the other side, a perfluorooctyl group. The liquid crystalline properties of the new three-coordinate copper(I) complexes were studied by a combination of differential scanning calorimetry (DSC) and polarizing optical microscopy (POM). Moreover, these new complexes have mesomorphic properties and exhibit a columnar mesophase over a large temperature range, more than 100°C, as shown by DSC.


## 2. Experimental

### 2.1. Characterization Methods

All the chemicals were used as supplied. C, H, and N analyses were carried out with an EuroEA 3300 instrument. IR spectra were recorded on a Bruker spectrophotometer using KBr discs.1H and 13C NMR spectra were recorded on a Bruker spectrometer operating at 500 MHz, using CDCl3 as solvent. 1H chemical shifts were referenced to the solvent peak position, δ 7.26 ppm. The phase assignments for the BTU ligand and its copper(I) complexes were evaluated by polarizing optical light microscopy (POM), placed on untreated glass slides, using a Nikon 50iPol microscope equipped with a Linkam THMS600 hot stage and TMS94 control processor. Temperatures and enthalpies of transitions were recorded by using the differential scanning calorimetry (DSC) technique employing a Diamond DSC PerkinElmer instrument. The BTU ligand and its copper(I) complexes were studied at 10°/min of scanning rate after being encapsulated in aluminium pans. Three heating/cooling cycles were performed on each sample. Thermogravimetric analysis for all samples was performed on a TA Q50 TGA instrument using alumina crucibles and nitrogen as purging gas. The heating rate employed was 10°C·min−1 from room temperature to 550°C. The powder XRD measurements were made on a D8 Advance diffractometer (Bruker AXS GmbH, Germany), in parallel beam setting, with monochromatized Cu-Kα1 radiation (λ = 1.5406 Å), scintillation detector, and horizontal sample stage. The measurements were performed in symmetric (θ–θ) geometry in the 2θ range from 1.5° to 30° in steps of 0.02°, with measuring times per step in the 5–40 s range. The temperature control of the samples during measurements was achieved by adapting a home-made heating stage to the sample stage of the diffractometer.


### 2.2. Preparation ofN-(4-Perfluorooctylphenylcarbamothioyl)-3,4-didecyloxybenzamide (1)

The synthesis of the BTU ligand1 followed the procedure described elsewhere [40, 41]. In the first step, the acid chlorides were prepared by reacting the 3,4-didecyloxybenzoic acid (5 mmol) with an excess of thionyl chloride (20 mmol) in freshly distilled dichloromethane (25 ml) for 3 hours and heating under reflux. Then, the excess of thionyl chloride and the solvent were removed under reduced pressure. The resulting acid chloride was taken to the next step without further purification. The acid chloride was dissolved in dry acetone (20 ml), and a solution of NH4SCN (5 mmol) in acetone (15 mL) was added dropwise for a period of 15 min under nitrogen. The mixture was heated under reflux for a period of 30 min. During the addition of the ammonium thiocyanate solution, the formation of a cloudy white precipitate was observed. The mixture was cooled down to room temperature, and a solution of p-perfluorooctylaniline (4.6 mmol) in acetone (10 mL) was added dropwise for a period of 30 min. The mixture was further stirred for 2 hours at room temperature, and then it was poured in 100 ml of deionized water. The resulting precipitate was filtered off and washed several times with water and ethanol followed by two times of recrystallization from a mixture of dichloromethane/ethanol to yield a white solid.


#### 2.2.1. Compound1

White crystalline solid. Yield: 77%. Anal. Calcd. For C42H51F17N2O3S (%): C, 51.11; H, 5.21; and N, 2.84; Found: C, 51.59; H, 5.35; and N, 2.65. 1H NMR (500 MHz, CDCl3) δ 12.99 (s, 1H), 9.05 (s, 1H), 7.98 (d, J = 8.6 Hz, 2H), 7.74 (d, J = 8.6 Hz, 2H), 7.60–7.30 (m, 2H), 6.93 (d, J = 8.2 Hz, 1H), 4.24–3.71 (m, 4H), 1.93–1.80 (m, 4H), and 1.55–1.20 (m, 28H), 0.88 (m, 6H). 13C NMR (126 MHz, CDCl3, ppm) δ: 178.5, 166.4, 154.2, 149.6, 141.1, 127.7, 127.6, 126.5, 123.3, 123.0, 121.1, 119.6, 112.4, 112.1, 69.6, 69.3, 31.8, 29.6, 29.4, 29.3, 29.1, 29.0, 26.1, 25.9, 22.7, and 14.1. IR (KBr, cm−1): 3266 (νNH), 2924, 2853 (νCH2), 1665 (νC=O), 1503 (νC-N), 1350 (νC=S), and 1144 (νC-N).


### 2.3. Preparation of Copper(I) Complexes (2a and 2b)

The synthesis of copper(I) complexes with benzoylthiourea ligand1 is similar to the preparation of such copper(I) complexes described elsewhere [36, 38, 39]. A solution of the corresponding halide copper(II) salt (CuX2, where X = Cl or Br; 0.5 mmol) dissolved in ethanol (5 ml) was added dropwise over a period of 5 min to a hot solution of the ligand (1 mmol) in ethanol (10 ml). A bright-yellow precipitate was formed during the addition of the solution of copper(II) salt. The mixture was further stirred and heated under reflux for 2 hours. After this period of time, the hot mixture was filtered and the resulting precipitate was washed several times with ethanol and dried in vacuum to yield a yellow solid. The yields were calculated based on copper salts. The 1H NMR spectroscopy and the elemental analysis confirmed the formation and purity of these copper(I) complexes.


#### 2.3.1. Compound2a

Yellow solid. Yield: 74%. Anal. Calcd. For C84H102ClCuF34N4O6S2(%): C, 48.67; H, 4.96; and N, 2.70; Found: C, 49.23; H, 4.84; and N, 2.74. 1H NMR (500 MHz, CDCl3, ppm) δ 13.35 (s, 2H), 11.06 (s, 2H), 8.16–7.92 (m, 2H), 7.70–7.62 (m, 10H), 6.89 (d, J = 8.6 Hz, 2H), 4.09 (t, J = 6.5 Hz, 4H), 4.03 (t, J = 6.5 Hz, 4H), 2.05–1.69 (m, 8H), 1.51–1.20 (m, 56H), and 0.88 (m, 12H).13C NMR (126 MHz, CDCl3) δ 179.1, 169.0, 154.6, 148.9, 139.9, 127.8, 125.4, 123.9, 122.2, 113.4, 111.7, 69.5, 69.1, 31.9, 30.9, 29.6, 29.5, 29.3, 29.2, 29.1, 26.0, 22.7, 22.3, and 14.1.IR (KBr, cm−1): 3274 (νNH), 2927, 2856 (νCH2), 1664 (νC=O), 1512 (νC-N), and 1152 (νC-N).


#### 2.3.2. Compound2b

Yellow solid. Yield: 78%. Anal. Calcd. For C84H102BrCuF34N4O6S2(%): C, 47.65; H, 4.86; and N, 2.65; Found: C, 48.51; H, 4.64; and N, 2.66. 1H NMR (500 MHz, CDCl3, ppm) δ 13.27 (s, 2H), 10.66 (s, 2H), 7.98 (d, 7.8 Hz, 2H), 7.68 (m, 4H), 7.59 (m, 6H), 6.88 (d, J = 8.6 Hz, 2H), 4.09 (t, J = 6.5 Hz, 4H), 4.01 (t, J = 6.5 Hz, 4H), 1.97–1.65 (m, 8H), 1.50–1.11 (m, 56H), and 0.88 (m, 12H).13C NMR (126 MHz, CDCl3) δ 178.4, 168.6, 154.7, 149.0, 139.9, 127.8, 125.1, 123.8, 122.1, 113.3, 111.7, 69.6, 69.1, 31.9, 29.6, 29.5, 29.4, 29.3, 29.2, 29.0, 26.0, 22.7, and 14.1.IR (KBr, cm−1): 3275 (νNH), 2927, 2856 (νCH2), 1665 (νC=O), 1510 (νC-N), and 1152 (νC-N).


## 2.1. Characterization Methods

All the chemicals were used as supplied. C, H, and N analyses were carried out with an EuroEA 3300 instrument. IR spectra were recorded on a Bruker spectrophotometer using KBr discs.1H and 13C NMR spectra were recorded on a Bruker spectrometer operating at 500 MHz, using CDCl3 as solvent. 1H chemical shifts were referenced to the solvent peak position, δ 7.26 ppm. The phase assignments for the BTU ligand and its copper(I) complexes were evaluated by polarizing optical light microscopy (POM), placed on untreated glass slides, using a Nikon 50iPol microscope equipped with a Linkam THMS600 hot stage and TMS94 control processor. Temperatures and enthalpies of transitions were recorded by using the differential scanning calorimetry (DSC) technique employing a Diamond DSC PerkinElmer instrument. The BTU ligand and its copper(I) complexes were studied at 10°/min of scanning rate after being encapsulated in aluminium pans. Three heating/cooling cycles were performed on each sample. Thermogravimetric analysis for all samples was performed on a TA Q50 TGA instrument using alumina crucibles and nitrogen as purging gas. The heating rate employed was 10°C·min−1 from room temperature to 550°C. The powder XRD measurements were made on a D8 Advance diffractometer (Bruker AXS GmbH, Germany), in parallel beam setting, with monochromatized Cu-Kα1 radiation (λ = 1.5406 Å), scintillation detector, and horizontal sample stage. The measurements were performed in symmetric (θ–θ) geometry in the 2θ range from 1.5° to 30° in steps of 0.02°, with measuring times per step in the 5–40 s range. The temperature control of the samples during measurements was achieved by adapting a home-made heating stage to the sample stage of the diffractometer.


## 2.2. Preparation ofN-(4-Perfluorooctylphenylcarbamothioyl)-3,4-didecyloxybenzamide (1)

The synthesis of the BTU ligand1 followed the procedure described elsewhere [40, 41]. In the first step, the acid chlorides were prepared by reacting the 3,4-didecyloxybenzoic acid (5 mmol) with an excess of thionyl chloride (20 mmol) in freshly distilled dichloromethane (25 ml) for 3 hours and heating under reflux. Then, the excess of thionyl chloride and the solvent were removed under reduced pressure. The resulting acid chloride was taken to the next step without further purification. The acid chloride was dissolved in dry acetone (20 ml), and a solution of NH4SCN (5 mmol) in acetone (15 mL) was added dropwise for a period of 15 min under nitrogen. The mixture was heated under reflux for a period of 30 min. During the addition of the ammonium thiocyanate solution, the formation of a cloudy white precipitate was observed. The mixture was cooled down to room temperature, and a solution of p-perfluorooctylaniline (4.6 mmol) in acetone (10 mL) was added dropwise for a period of 30 min. The mixture was further stirred for 2 hours at room temperature, and then it was poured in 100 ml of deionized water. The resulting precipitate was filtered off and washed several times with water and ethanol followed by two times of recrystallization from a mixture of dichloromethane/ethanol to yield a white solid.


### 2.2.1. Compound1

White crystalline solid. Yield: 77%. Anal. Calcd. For C42H51F17N2O3S (%): C, 51.11; H, 5.21; and N, 2.84; Found: C, 51.59; H, 5.35; and N, 2.65. 1H NMR (500 MHz, CDCl3) δ 12.99 (s, 1H), 9.05 (s, 1H), 7.98 (d, J = 8.6 Hz, 2H), 7.74 (d, J = 8.6 Hz, 2H), 7.60–7.30 (m, 2H), 6.93 (d, J = 8.2 Hz, 1H), 4.24–3.71 (m, 4H), 1.93–1.80 (m, 4H), and 1.55–1.20 (m, 28H), 0.88 (m, 6H). 13C NMR (126 MHz, CDCl3, ppm) δ: 178.5, 166.4, 154.2, 149.6, 141.1, 127.7, 127.6, 126.5, 123.3, 123.0, 121.1, 119.6, 112.4, 112.1, 69.6, 69.3, 31.8, 29.6, 29.4, 29.3, 29.1, 29.0, 26.1, 25.9, 22.7, and 14.1. IR (KBr, cm−1): 3266 (νNH), 2924, 2853 (νCH2), 1665 (νC=O), 1503 (νC-N), 1350 (νC=S), and 1144 (νC-N).


## 2.2.1. Compound1

White crystalline solid. Yield: 77%. Anal. Calcd. For C42H51F17N2O3S (%): C, 51.11; H, 5.21; and N, 2.84; Found: C, 51.59; H, 5.35; and N, 2.65. 1H NMR (500 MHz, CDCl3) δ 12.99 (s, 1H), 9.05 (s, 1H), 7.98 (d, J = 8.6 Hz, 2H), 7.74 (d, J = 8.6 Hz, 2H), 7.60–7.30 (m, 2H), 6.93 (d, J = 8.2 Hz, 1H), 4.24–3.71 (m, 4H), 1.93–1.80 (m, 4H), and 1.55–1.20 (m, 28H), 0.88 (m, 6H). 13C NMR (126 MHz, CDCl3, ppm) δ: 178.5, 166.4, 154.2, 149.6, 141.1, 127.7, 127.6, 126.5, 123.3, 123.0, 121.1, 119.6, 112.4, 112.1, 69.6, 69.3, 31.8, 29.6, 29.4, 29.3, 29.1, 29.0, 26.1, 25.9, 22.7, and 14.1. IR (KBr, cm−1): 3266 (νNH), 2924, 2853 (νCH2), 1665 (νC=O), 1503 (νC-N), 1350 (νC=S), and 1144 (νC-N).


## 2.3. Preparation of Copper(I) Complexes (2a and 2b)

The synthesis of copper(I) complexes with benzoylthiourea ligand1 is similar to the preparation of such copper(I) complexes described elsewhere [36, 38, 39]. A solution of the corresponding halide copper(II) salt (CuX2, where X = Cl or Br; 0.5 mmol) dissolved in ethanol (5 ml) was added dropwise over a period of 5 min to a hot solution of the ligand (1 mmol) in ethanol (10 ml). A bright-yellow precipitate was formed during the addition of the solution of copper(II) salt. The mixture was further stirred and heated under reflux for 2 hours. After this period of time, the hot mixture was filtered and the resulting precipitate was washed several times with ethanol and dried in vacuum to yield a yellow solid. The yields were calculated based on copper salts. The 1H NMR spectroscopy and the elemental analysis confirmed the formation and purity of these copper(I) complexes.


### 2.3.1. Compound2a

Yellow solid. Yield: 74%. Anal. Calcd. For C84H102ClCuF34N4O6S2(%): C, 48.67; H, 4.96; and N, 2.70; Found: C, 49.23; H, 4.84; and N, 2.74. 1H NMR (500 MHz, CDCl3, ppm) δ 13.35 (s, 2H), 11.06 (s, 2H), 8.16–7.92 (m, 2H), 7.70–7.62 (m, 10H), 6.89 (d, J = 8.6 Hz, 2H), 4.09 (t, J = 6.5 Hz, 4H), 4.03 (t, J = 6.5 Hz, 4H), 2.05–1.69 (m, 8H), 1.51–1.20 (m, 56H), and 0.88 (m, 12H).13C NMR (126 MHz, CDCl3) δ 179.1, 169.0, 154.6, 148.9, 139.9, 127.8, 125.4, 123.9, 122.2, 113.4, 111.7, 69.5, 69.1, 31.9, 30.9, 29.6, 29.5, 29.3, 29.2, 29.1, 26.0, 22.7, 22.3, and 14.1.IR (KBr, cm−1): 3274 (νNH), 2927, 2856 (νCH2), 1664 (νC=O), 1512 (νC-N), and 1152 (νC-N).


### 2.3.2. Compound2b

Yellow solid. Yield: 78%. Anal. Calcd. For C84H102BrCuF34N4O6S2(%): C, 47.65; H, 4.86; and N, 2.65; Found: C, 48.51; H, 4.64; and N, 2.66. 1H NMR (500 MHz, CDCl3, ppm) δ 13.27 (s, 2H), 10.66 (s, 2H), 7.98 (d, 7.8 Hz, 2H), 7.68 (m, 4H), 7.59 (m, 6H), 6.88 (d, J = 8.6 Hz, 2H), 4.09 (t, J = 6.5 Hz, 4H), 4.01 (t, J = 6.5 Hz, 4H), 1.97–1.65 (m, 8H), 1.50–1.11 (m, 56H), and 0.88 (m, 12H).13C NMR (126 MHz, CDCl3) δ 178.4, 168.6, 154.7, 149.0, 139.9, 127.8, 125.1, 123.8, 122.1, 113.3, 111.7, 69.6, 69.1, 31.9, 29.6, 29.5, 29.4, 29.3, 29.2, 29.0, 26.0, 22.7, and 14.1.IR (KBr, cm−1): 3275 (νNH), 2927, 2856 (νCH2), 1665 (νC=O), 1510 (νC-N), and 1152 (νC-N).


## 2.3.1. Compound2a

Yellow solid. Yield: 74%. Anal. Calcd. For C84H102ClCuF34N4O6S2(%): C, 48.67; H, 4.96; and N, 2.70; Found: C, 49.23; H, 4.84; and N, 2.74. 1H NMR (500 MHz, CDCl3, ppm) δ 13.35 (s, 2H), 11.06 (s, 2H), 8.16–7.92 (m, 2H), 7.70–7.62 (m, 10H), 6.89 (d, J = 8.6 Hz, 2H), 4.09 (t, J = 6.5 Hz, 4H), 4.03 (t, J = 6.5 Hz, 4H), 2.05–1.69 (m, 8H), 1.51–1.20 (m, 56H), and 0.88 (m, 12H).13C NMR (126 MHz, CDCl3) δ 179.1, 169.0, 154.6, 148.9, 139.9, 127.8, 125.4, 123.9, 122.2, 113.4, 111.7, 69.5, 69.1, 31.9, 30.9, 29.6, 29.5, 29.3, 29.2, 29.1, 26.0, 22.7, 22.3, and 14.1.IR (KBr, cm−1): 3274 (νNH), 2927, 2856 (νCH2), 1664 (νC=O), 1512 (νC-N), and 1152 (νC-N).


## 2.3.2. Compound2b

Yellow solid. Yield: 78%. Anal. Calcd. For C84H102BrCuF34N4O6S2(%): C, 47.65; H, 4.86; and N, 2.65; Found: C, 48.51; H, 4.64; and N, 2.66. 1H NMR (500 MHz, CDCl3, ppm) δ 13.27 (s, 2H), 10.66 (s, 2H), 7.98 (d, 7.8 Hz, 2H), 7.68 (m, 4H), 7.59 (m, 6H), 6.88 (d, J = 8.6 Hz, 2H), 4.09 (t, J = 6.5 Hz, 4H), 4.01 (t, J = 6.5 Hz, 4H), 1.97–1.65 (m, 8H), 1.50–1.11 (m, 56H), and 0.88 (m, 12H).13C NMR (126 MHz, CDCl3) δ 178.4, 168.6, 154.7, 149.0, 139.9, 127.8, 125.1, 123.8, 122.1, 113.3, 111.7, 69.6, 69.1, 31.9, 29.6, 29.5, 29.4, 29.3, 29.2, 29.0, 26.0, 22.7, and 14.1.IR (KBr, cm−1): 3275 (νNH), 2927, 2856 (νCH2), 1665 (νC=O), 1510 (νC-N), and 1152 (νC-N).


## 3. Results and Discussions

### 3.1. Synthesis

The novel BTU ligand having two terminal decyloxy chains on the benzoyl unit and a perfluorooctyl group on the aniline fragment was prepared through the reaction of 3,4-didecyloxybenzoyl isothiocyanate with 4-perfluorooctylaniline in high yield (77%) (Scheme1) [40, 41, 51]. The copper(I) complexes were obtained by reaction of the BTU ligand with copper(II) halide salts in hot ethanol in a 2 : 1 molar ratio to give yellow solids. The reaction can be also performed by employing copper(I) salts giving identical products. The new BTU derivative and the copper(I) complexes were fully characterized by 1H NMR and 13C NMR and IR spectroscopies as well as by elemental analyses. The 1H NMR spectrum of BTU ligand 1 contains two singlets, one at 9.05 ppm and a second one at 12.99 ppm, which can be assigned to the two NH groups. The first singlet can be assigned to the NH proton located between the carbonyl and thiocarbonyl groups, while the second singlet was assigned to the NH proton between the thiocarbonyl group and the benzene ring. On the contrary, the chemical shift values for the carbonyl and thiocarbonyl carbons were found at about 166.5 ppm and around 178.5 ppm, respectively, as reported for some other fluorinated BTU compounds [52, 53].Scheme 1
Synthesis ofN-benzoyl-N′-arylthiourea perfluoroalkyl terminated BTU and of copper(I) complexes.The1H NMR spectra of copper(I) complexes recorded in CDCl3 solvent show the expected signals assigned to ligand with several significant shifts resulted from its coordination to the copper(I) center (Figure 1). The most significant changes were seen for the two NH singlets. Both signals were downfield shifted with a more pronounced shift for the signal assigned to the NH group located between the carbonyl and thiocarbonyl groups of the BTU ligand.Figure 1
The low field region of the1H NMR spectra of the benzoylthiourea derivative 1 and its copper(I) complexes 2a and 2b.While the first singlet at 12.99 ppm in the1H NMR spectrum of uncoordinated ligand downfield shifts to 13.35 ppm for 2a and to 13.27 ppm for 2b, the second NH signal at 8.99 ppm for 1 is downfield shifted to 11.06 ppm for 2a and to 10.66 ppm for 2b as a consequence of the intramolecular hydrogen bonding between the halide ion and the second NH group. These chemical shift changes are attributed to the copper(I) complexes formation, and similar results were found for related three-coordinate copper(I) complexes [33–35]. Intramolecular hydrogen-bonding between the coordinated halide ions and NH group was evidenced by X-ray structural analysis for several related complexes [37–39].Several regions of the FTIR spectra, recorded in KBr discs, are of interest for supporting the coordination via the sulfur atom: 3200–3400 cm−1 for νN-H frequencies, 1500–1700 cm−1 for strong νC=O and νC-N frequencies, and finally, 1100–1250 cm−1 where strong absorption bands assigned to a combination of νC-N and νphenyl stretching frequencies can be found [54–58]. For example, the intensity and the position of the carbonyl stretching νC=O at ∼1665 cm−1 are essentially the same in the IR spectra of 2a and 2b as in the free ligand 1. The medium intense band at 1350 cm−1 in the IR of ligand 1, assigned to νC=S, is absent in the IR spectra of copper(I) complexes [34]. Additionally, the very strong band at 1144 cm−1 for 1, corresponding to νC-N of the thioamide group, shifts to higher wavenumber at 1152 cm−1 for 2a and 2b.


### 3.2. Liquid Crystalline Properties

The new copper(I) complexes and the benzoylthiourea ligand were investigated for their liquid crystalline properties by a combination of hot-stage polarizing optical microscopy (POM) and differential scanning calorimetry (DSC). The thermal parameters for all compounds are presented in Table1.Table 1
Transition temperatures (in °C) and enthalpies (kJ·mol−1) for ligand 1 and its copper(I) complexes.
Compound
Transitions, T/°C (ΔH/kJ·mol−1)a
1
Cr 110 (58.7) Iso 99 (−35.0) Cr1 87 (−7.1) Cr2 17 (−7.7) Cr3
2a
g 50b Colh 162 (13.7) Iso 162 (−13.0) Colh 50b g
2b
g 52 Colh 173 (18.2) Iso 170 (−16.3) Colh 47 g
aCr1, Cr2, and Cr3 = crystalline phases; Iso = isotropic phase; Colh = hexagonal columnar phase; g = glassy state. bTransition detected by POM.The heating run of the DSC curve recorded for ligand1 shows only one transition assigned to a crystal-to-isotropic state transition (Table 1). On cooling from the isotropic state down to 0°C, three transitions were observed, an isotropic to a crystalline phase (Cr1) transition followed by other two transitions between crystalline states (Cr2 and Cr3). No LC phase was evidenced for the BTU ligand. On the contrary, it was found that both copper(I) complexes show mesogenic properties.Two transitions were detected in the DSC traces both during the heating and cooling runs for the two copper(I) complexes: a first transition from the isotropic state to a columnar phase followed by a second transition assigned to a glass transition around 50°C (Figures2 and 3). All these transitions were detected by POM as well, and an example of textural changes for compound 2a is presented in Figure 4. These results are consistent with the POM studies, where typical optical textures of a hexagonal columnar (Colh) phase were observed for both copper(I) complexes (Figures 4 and 5). The clearing temperatures of the two copper(I) complexes (Table 1, measured during the first heating run) depend significantly on the size of the halide ion.Figure 2
DSC traces for2a: first (a) and second heating-cooling cycles (b).
(a)
(b)Figure 3
DSC traces for2b: first (a) and second heating-cooling cycles (b).
(a)
(b)Figure 4
Pictures taken at the polarizing optical microscope showing the optical textures of2a at 170°C (a), 160°C (b), 85°C (c), and 35°C (d).
(a)
(b)
(c)
(d)Figure 5
Pictures taken at the polarizing optical microscope showing the optical textures of2b at 175°C (a) and 35°C (b).
(a)
(b)The lowest clearing temperature was recorded for chlorocomplex2a (162°C), while a higher clearing temperature was measured for the bromocomplex 2b (173°C). Interestingly, these two copper(I) compounds are stable in the glassy state at room temperature as no crystalline phases were seen during the first and subsequent heating-cooling cycles.The mesophase assignment for the two Cu(I) complexes was confirmed further by powder X-ray diffraction (XRD) measurements (Table2). The samples were heated up to 125°C in the mesomorphic domain, and typical patterns that are characteristic of a hexagonal packing were obtained in each case.Table 2
Temperature dependent X-ray powder diffraction for Cu(I) compounds.
Compound
Mesophase
T (°C)
Indexation
d-spacing observed (Å)
d-spacing calculated (Å)
Lattice parameters (Å)a
2a
Colh
125
100
26.91
26.91
a = 31.07
110
15.49
15.54
200
13.42
13.46
210
10.04
10.17
400
6.66
6.73
Broadb
4.6
—
2b
Colh
125
100
26.51
26.51
a = 30.61
110
15.17
15.30
200
13.18
13.26
210
10.00
10.02
300
8.80
8.84
Broadb
4.6
—
aThe Colh lattice parameter a = 2<d100>/√3. bBroad peak assigned to molten alkyl chains.The diffractograms of2a and 2b show a strong maximum from the (100) reflection followed by a series of four weaker sharp peaks with a d-spacing ratio of d/√3, d/2, d/√7, and d/4 from the (110), (200), (210), and (400) reflections for 2a or d/√3, d/2, d/√7, and d/3 from the (110), (200), (210), and (300) reflections for 2b, respectively (Figure 6).Figure 6
X-ray powder diffractograms for Cu(I) compounds:2a at 125°C (a) and 2b at 125°C (b).
(a)
(b)It is important to mention that the transition temperatures recorded both during the heating and cooling runs by DSC were slightly shifted towards lower values on subsequent heating-cooling cycles for complexes2a and 2b. These observations indicate a possible slight decomposition of the copper(I) complexes on heating above the clearing points. Therefore, a study regarding the thermal stability of these compounds was performed in the next step.


### 3.3. Thermal Stability of the Ligands and Copper(I) Complexes

The two copper(I) complexes and the BTU ligand were investigated by TG analysis in nitrogen, in the 25–550°C temperature range, and the decomposition curves are presented in Figure7. These TG curves do not contain steps or other indication of mass loss in the 25–160°C region, and therefore, the complexes do not contain small molecules (water or ethanol solvent). On the contrary, the results of the thermogravimetric analyses show that the copper(I) complexes 2a and 2b have a higher thermal stability compared to the BTU ligand 1, and their decomposition started at temperatures around 180°C. For exemplification, Figure 7 gives the TG curves for the BTU ligand 1 and its copper(I) complexes 2a and 2b. The BTU ligand starts decomposing around 160°C.Figure 7
TG curves for ligand1 and its copper(I) complexes 2a and 2b.As it can be seen from Figure7, the two copper(I) complexes undergo complete decomposition up to 500°C. A small weight loss, less than 2%, was recorded on heating the copper(I) complexes 2a and 2b above the clearing points around 180°C. The slight decomposition observed at temperatures higher than the clearing point could explain the transition temperatures shifting recorded by DSC. Similar observations were found for some palladium(II) complexes with mixed ligands, Schiff bases, and BTU derivatives, reported previously [59, 60].


## 3.1. Synthesis

The novel BTU ligand having two terminal decyloxy chains on the benzoyl unit and a perfluorooctyl group on the aniline fragment was prepared through the reaction of 3,4-didecyloxybenzoyl isothiocyanate with 4-perfluorooctylaniline in high yield (77%) (Scheme1) [40, 41, 51]. The copper(I) complexes were obtained by reaction of the BTU ligand with copper(II) halide salts in hot ethanol in a 2 : 1 molar ratio to give yellow solids. The reaction can be also performed by employing copper(I) salts giving identical products. The new BTU derivative and the copper(I) complexes were fully characterized by 1H NMR and 13C NMR and IR spectroscopies as well as by elemental analyses. The 1H NMR spectrum of BTU ligand 1 contains two singlets, one at 9.05 ppm and a second one at 12.99 ppm, which can be assigned to the two NH groups. The first singlet can be assigned to the NH proton located between the carbonyl and thiocarbonyl groups, while the second singlet was assigned to the NH proton between the thiocarbonyl group and the benzene ring. On the contrary, the chemical shift values for the carbonyl and thiocarbonyl carbons were found at about 166.5 ppm and around 178.5 ppm, respectively, as reported for some other fluorinated BTU compounds [52, 53].Scheme 1
Synthesis ofN-benzoyl-N′-arylthiourea perfluoroalkyl terminated BTU and of copper(I) complexes.The1H NMR spectra of copper(I) complexes recorded in CDCl3 solvent show the expected signals assigned to ligand with several significant shifts resulted from its coordination to the copper(I) center (Figure 1). The most significant changes were seen for the two NH singlets. Both signals were downfield shifted with a more pronounced shift for the signal assigned to the NH group located between the carbonyl and thiocarbonyl groups of the BTU ligand.Figure 1
The low field region of the1H NMR spectra of the benzoylthiourea derivative 1 and its copper(I) complexes 2a and 2b.While the first singlet at 12.99 ppm in the1H NMR spectrum of uncoordinated ligand downfield shifts to 13.35 ppm for 2a and to 13.27 ppm for 2b, the second NH signal at 8.99 ppm for 1 is downfield shifted to 11.06 ppm for 2a and to 10.66 ppm for 2b as a consequence of the intramolecular hydrogen bonding between the halide ion and the second NH group. These chemical shift changes are attributed to the copper(I) complexes formation, and similar results were found for related three-coordinate copper(I) complexes [33–35]. Intramolecular hydrogen-bonding between the coordinated halide ions and NH group was evidenced by X-ray structural analysis for several related complexes [37–39].Several regions of the FTIR spectra, recorded in KBr discs, are of interest for supporting the coordination via the sulfur atom: 3200–3400 cm−1 for νN-H frequencies, 1500–1700 cm−1 for strong νC=O and νC-N frequencies, and finally, 1100–1250 cm−1 where strong absorption bands assigned to a combination of νC-N and νphenyl stretching frequencies can be found [54–58]. For example, the intensity and the position of the carbonyl stretching νC=O at ∼1665 cm−1 are essentially the same in the IR spectra of 2a and 2b as in the free ligand 1. The medium intense band at 1350 cm−1 in the IR of ligand 1, assigned to νC=S, is absent in the IR spectra of copper(I) complexes [34]. Additionally, the very strong band at 1144 cm−1 for 1, corresponding to νC-N of the thioamide group, shifts to higher wavenumber at 1152 cm−1 for 2a and 2b.


## 3.2. Liquid Crystalline Properties

The new copper(I) complexes and the benzoylthiourea ligand were investigated for their liquid crystalline properties by a combination of hot-stage polarizing optical microscopy (POM) and differential scanning calorimetry (DSC). The thermal parameters for all compounds are presented in Table1.Table 1
Transition temperatures (in °C) and enthalpies (kJ·mol−1) for ligand 1 and its copper(I) complexes.
Compound
Transitions, T/°C (ΔH/kJ·mol−1)a
1
Cr 110 (58.7) Iso 99 (−35.0) Cr1 87 (−7.1) Cr2 17 (−7.7) Cr3
2a
g 50b Colh 162 (13.7) Iso 162 (−13.0) Colh 50b g
2b
g 52 Colh 173 (18.2) Iso 170 (−16.3) Colh 47 g
aCr1, Cr2, and Cr3 = crystalline phases; Iso = isotropic phase; Colh = hexagonal columnar phase; g = glassy state. bTransition detected by POM.The heating run of the DSC curve recorded for ligand1 shows only one transition assigned to a crystal-to-isotropic state transition (Table 1). On cooling from the isotropic state down to 0°C, three transitions were observed, an isotropic to a crystalline phase (Cr1) transition followed by other two transitions between crystalline states (Cr2 and Cr3). No LC phase was evidenced for the BTU ligand. On the contrary, it was found that both copper(I) complexes show mesogenic properties.Two transitions were detected in the DSC traces both during the heating and cooling runs for the two copper(I) complexes: a first transition from the isotropic state to a columnar phase followed by a second transition assigned to a glass transition around 50°C (Figures2 and 3). All these transitions were detected by POM as well, and an example of textural changes for compound 2a is presented in Figure 4. These results are consistent with the POM studies, where typical optical textures of a hexagonal columnar (Colh) phase were observed for both copper(I) complexes (Figures 4 and 5). The clearing temperatures of the two copper(I) complexes (Table 1, measured during the first heating run) depend significantly on the size of the halide ion.Figure 2
DSC traces for2a: first (a) and second heating-cooling cycles (b).
(a)
(b)Figure 3
DSC traces for2b: first (a) and second heating-cooling cycles (b).
(a)
(b)Figure 4
Pictures taken at the polarizing optical microscope showing the optical textures of2a at 170°C (a), 160°C (b), 85°C (c), and 35°C (d).
(a)
(b)
(c)
(d)Figure 5
Pictures taken at the polarizing optical microscope showing the optical textures of2b at 175°C (a) and 35°C (b).
(a)
(b)The lowest clearing temperature was recorded for chlorocomplex2a (162°C), while a higher clearing temperature was measured for the bromocomplex 2b (173°C). Interestingly, these two copper(I) compounds are stable in the glassy state at room temperature as no crystalline phases were seen during the first and subsequent heating-cooling cycles.The mesophase assignment for the two Cu(I) complexes was confirmed further by powder X-ray diffraction (XRD) measurements (Table2). The samples were heated up to 125°C in the mesomorphic domain, and typical patterns that are characteristic of a hexagonal packing were obtained in each case.Table 2
Temperature dependent X-ray powder diffraction for Cu(I) compounds.
Compound
Mesophase
T (°C)
Indexation
d-spacing observed (Å)
d-spacing calculated (Å)
Lattice parameters (Å)a
2a
Colh
125
100
26.91
26.91
a = 31.07
110
15.49
15.54
200
13.42
13.46
210
10.04
10.17
400
6.66
6.73
Broadb
4.6
—
2b
Colh
125
100
26.51
26.51
a = 30.61
110
15.17
15.30
200
13.18
13.26
210
10.00
10.02
300
8.80
8.84
Broadb
4.6
—
aThe Colh lattice parameter a = 2<d100>/√3. bBroad peak assigned to molten alkyl chains.The diffractograms of2a and 2b show a strong maximum from the (100) reflection followed by a series of four weaker sharp peaks with a d-spacing ratio of d/√3, d/2, d/√7, and d/4 from the (110), (200), (210), and (400) reflections for 2a or d/√3, d/2, d/√7, and d/3 from the (110), (200), (210), and (300) reflections for 2b, respectively (Figure 6).Figure 6
X-ray powder diffractograms for Cu(I) compounds:2a at 125°C (a) and 2b at 125°C (b).
(a)
(b)It is important to mention that the transition temperatures recorded both during the heating and cooling runs by DSC were slightly shifted towards lower values on subsequent heating-cooling cycles for complexes2a and 2b. These observations indicate a possible slight decomposition of the copper(I) complexes on heating above the clearing points. Therefore, a study regarding the thermal stability of these compounds was performed in the next step.


## 3.3. Thermal Stability of the Ligands and Copper(I) Complexes

The two copper(I) complexes and the BTU ligand were investigated by TG analysis in nitrogen, in the 25–550°C temperature range, and the decomposition curves are presented in Figure7. These TG curves do not contain steps or other indication of mass loss in the 25–160°C region, and therefore, the complexes do not contain small molecules (water or ethanol solvent). On the contrary, the results of the thermogravimetric analyses show that the copper(I) complexes 2a and 2b have a higher thermal stability compared to the BTU ligand 1, and their decomposition started at temperatures around 180°C. For exemplification, Figure 7 gives the TG curves for the BTU ligand 1 and its copper(I) complexes 2a and 2b. The BTU ligand starts decomposing around 160°C.Figure 7
TG curves for ligand1 and its copper(I) complexes 2a and 2b.As it can be seen from Figure7, the two copper(I) complexes undergo complete decomposition up to 500°C. A small weight loss, less than 2%, was recorded on heating the copper(I) complexes 2a and 2b above the clearing points around 180°C. The slight decomposition observed at temperatures higher than the clearing point could explain the transition temperatures shifting recorded by DSC. Similar observations were found for some palladium(II) complexes with mixed ligands, Schiff bases, and BTU derivatives, reported previously [59, 60].


## 4. Conclusions

Three-coordinate copper(I)-containing liquid crystalline materials with columnar mesophases were prepared by using an alkoxy-substitutedN-benzoylthiourea derivative having a perfluorooctyl group at one end. The new copper(I) complexes exhibit a hexagonal columnar phase over a large temperature range, more than 100°C, as evidenced by DSC, POM observations, and powder X-ray diffraction analysis. The thermal stability of these copper(I) metallomesogens is limited by a slight decomposition on heating above the clearing points (∼180°C).



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*Source: 7943763-2018-07-08.xml*