# Synthesis and Properties of a New Type of Terpyridine Cholesterol Derivative Gelator with Applications to Medical Treatments

Authors: Lina Qiu; Yang Liu; Yunhe Miao; Weiwei Zhang; Aijun Gong; Zhipeng Liu
Journal: International Journal of Polymer Science
 (2022)

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## Abstract

Low molecular mass gelators (LMMGs), as a new type of intelligent soft material, possess good response properties to light, electricity, heat, and ultrasound and have many potential applications in fields such as intelligent sensing, biological materials, and drug release. Additionally, steroid derivatives have been a focus in the study of LMMGs for their desirable properties as well, such as their rigid framework, multichiral center, and strong van der Waals accumulation. Furthermore, the coordination ability of terpyridine has been an emphasis in the study of supramolecular chemistry and coordination chemistry as well. Attempts have been made with terpyridine groups that have special responses, such as terpyridine with steroid derivatives, to build more specialized and functional gelators. In this study, we used 2-acetylpyridine, 2-formaldehyde, and cholesterol to synthesize 6-(2,2:6′,2″-terpyridine-4′-carboxamide group) hexanoic acid (with a yield of 64.39%, P1), glycine cholesterol ester (with a yield of 70.36%, P2), and DMTCP (with a yield of 88.92%). Infrared spectroscopy, nuclear magnetic resonance spectroscopy, mass spectrometry, elemental analysis, and gelator performance tests were then conducted to measure the gelation effect of the materials and to explore their gelation mechanisms. Compared to P1 and P2, the DMTCP synthesized by P1 and P2 was able to form gel in more kinds of solvents. In addition, when it contains both terpyridine and cholesterol functional groups, the gelation properties of DMTCP were also significantly improved, and all the gels prepared in the four solvents in which DMTCP can form gels were stimulus responsive.


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## Body

## 1. Introduction

Supramolecular chemistry is the chemistry of intermolecular forces and molecular assembly. Ever since Lehn put forward the concept of supramolecular chemistry in 1978 [1], supramolecular chemistry has become a new discipline that has come to intersect with biology, physics, materials, and other disciplines after more than 30 years of rapid development [2, 3]. In recent years, molecular gelators, as an important branch of colloid science, have attracted increasing attention due to their unique supramolecular multistage self-assembly structure and broad application prospects [4, 5]. Low molecular mass gelators (LMMGs) are organic compounds with molecular weights below 2000 that are capable of forming physical gels with solvent molecules with the help of supramolecular self-assembly at low concentrations (mostly less than 3% w/w) [6–8]. LMMGs based on the supramolecular chemistry principle are a hot topic in current chemistry research [9, 10]. At present, there have been many studies on LMMGs, but there are still great challenges in preparing LMMGs to carry out specific functions.Recent studies have found that the introduction of some special functional groups to gelators can be added to gel materials that have stimulation responses to light, electricity, heat, ultrasonography, fluorescence, pH, magnetic, and fluorine ions. Hence, these materials have great potential applications in various fields such as photosensitive devices, biological materials, drug transport, preparation of nanomaterials, and gel rocket propellants [11–19].Cholesteric derivatives are a common type of LMMG that are usually classified as cholesterol derivatives or cholic acid derivatives [20–23]. However, the most studied LMMGs are small molecular compounds with cholesterol as their basic structural unit. The main reason for this is due to the rigid structure of cholesterol itself and its strong tendency to cluster orderly in solution. These structures and clusters make cholesterol and its derivatives able to form various aggregation structures in solution easily, and they thus can form supramolecular gelators with different structures and properties. In addition, 2,2′:6′,2″-terpyridine, as one of the most widely used ligands in coordination chemistry, has a strong coordination effect and can form complexes with stable structures with most metals [24–27]. Terpyridine and its derivatives not only have exotic structures but excellent optical, electrical, magnetic, molecular carrying, and catalysis properties as well. The study of terpyridine ligands and complexes (especially the substitutions of those with 4′ positions) has become an important focus of modern coordination chemistry [28–30].Cholesteric derivatives such as cholesterol have been found to be very effective gelators, and the introduction of terpyridine for metal ion coordination aids in the construction of stimulus-responsive gels. Additionally, a long alkyl chain connection between terpyridine and cholesterol can enhance gelatination. In this paper, we synthesized 6-(2,2′:6′,2″-terpyridine-4′-formamide) hexanoic acid, glycine cholesterol ester, and DMTCP from 2-acetylpyridine, 2-furaldehyde, cholesterol, and Boc-glycine, respectively, and characterized and tested each of their gelator properties. Molecular structures were observed by measuring the infrared spectrum of the synthesized gelators and the xerogel samples prepared in response. The generation, disappearance, or transfer of characteristic peaks in the infrared spectrum indicated the generation of specific groups. Gelation effects were measured by observing the gelation behavior of the synthesized gelators in different organic reagents, and the morphology of the gelators was studied by scanning electron microscope (SEM) in order to explore the gelation mechanism.


## 2. Materials and Methods

### 2.1. Reagents

We purchased 2-furfural (AR, 99.0%), anhydrous potassium carbonate (AR, 99.0%), anhydrous magnesium sulfate (AR, 99.0%), pyridine (AR, 99.5%), hydrochloric acid (AR, 36.0-38.0%), acetone (AR, 99.5%), sodium thiosulfate pentahydrate (AR, 99.0%), sodium chloride (AR, 99.5%), anhydrous magnesium sulfate (AR, 99.0%), potassium hydroxide (AR, 85%), and potassium permanganate (AR, 99.5%) from Sinopharm Chemical Reagent Co., Ltd. and purchased Boc-glycine (AR, 98.5%), dicyclohexylcarbodiimide (DCC, AR, 99.0%), 4-dimethylaminopyridine (DMAP, AR, 99.0%), 1-benzotriazolol (HOBT, AR, 99.0%), and 1-ethyl-3-(3-dimethylam-inopropyl) carbodiimide hydrochloride (EDCI, AR, 99.0%) from Xiya Reagent Co., Ltd. Absolute ethyl alcohol (AR, 99.7%), dichloromethane (AR, 99.5%), trichloromethane (AR, 99.0%), ethyl acetate (AR, 99.5%), DMF (N,N-dimethylformamide) (AR, 99.7%), tetrahydrofuran (AR, 99.0%) (THF), concentrated sulfuric acid (GR, 95-98%), and petroleum ether (AR) were purchased from Beijing Chemical Works Co., Ltd., and 2-acetylpyridine was purchased from Shanghai Adamas Co., Ltd. Finally, we purchased methyl 6-aminohexanoate hydrochloride from Heowns and cholesterol (AR, 99%) from J&K Scientific Co., Ltd.


### 2.2. Synthesis of 6-(2,2′:6′,2″-Terpyridine-4′-formamide) Hexanoic Acid (P1)

The synthesis route of 6-(2,2′:6′,2″-terpyridine-4′-formamide) hexanoic acid is shown in Figure 1.Figure 1
Synthesis route of 6-(2,2′:6′:2″-terpyridine-4′-formamide) hexanoic acid.


#### 2.2.1. Synthesis of 4′-(2-Furyl)-2,2′:6′,2″-terpyridine

We added 9.00 mL (80 mmol) of 2-acetylpyridine, 3.34 mL (40 mmol) of 2-furaldehyde, and 200 mL of anhydrous ethanol to a three-mouth flask. After the solution was stirred evenly, 6.16 g potassium hydroxide and 120 mL ammonia (25%) were then added. Next, the reaction was refluxed overnight at 60°C, and the cooled solution was filtered to obtain the light yellow solid that is the crude product. The crude product was further purified by using silica gel column chromatography with chloroform (or dichloromethane) as the eluent. Finally, the pale yellow eluent was distilled and dried to obtain an orange-yellow, powdery product. The yield of the reaction was 49.27%, and the elemental composition of 4′-(2-furyl)-2,2′:6′,2″-terpyridine is shown in Table 1. We also characterized its molecular structure by 1H NMR. (The same method was applied to subsequent syntheses.)Table 1
Elemental composition of 4′-(2-furyl)-2,2′:6′,2″-terpyridine.
CHNOTheoretical value76.244.3814.045.34Actual value75.974.2013.585.201H NMR (400 MHz, chloroform-d) δ 6.52–6.59 (dd, J=3.5, 1.8 Hz, 1H), 7.09–7.17 (s, 1H), 7.31–7.43 (t, J=5.8Hz, 2H), 7.53–7.62 (s, 1H), 7.82–7.94 (t, J=7.7Hz, 2H), 8.59–8.69 (d, J=8.0Hz, 2H), and 8.68–8.81 (s, 4H).


#### 2.2.2. Synthesis of 2,2′:6′,2″-Terpyridine-4′-carboxylic Acid

We added 3.20 g 4′-(2-furyl)-2,2′:6′,2″-tripyridine and 120 mL pyridine to a conical flask and kept stirring until the solids were completely dissolved. Then, potassium permanganate solution (0.1 g·mL-1) was added drop by drop into the conical flask and stirred at room temperature for 20 h. After the reaction was completed, excessive sodium thiosulfate powder was added to the filtrate of the postreaction solution, and we kept fully stirring until the color turned pale yellow. The solution was left to rest for stratification, and the upper organic phase was reserved to remove solvents by rotary evaporation. After this, 1 mol·L-1 sodium hydroxide solution was added, and the remaining solids were dissolved by heating. Then, the solution was filtered to remove the insoluble solids, and concentrated hydrochloric acid was added to the filtrate slowly while fully stirring until a large number of white precipitates appeared. Finally, the white solid product was obtained by washing with deionized water and drying; yield was about 60%. The elemental composition of 2,2′:6′,2″-terpyridine-4′-carboxylic acid is shown in Table 2.Table 2
Elemental composition of 2,2′:6′,2″-terpyridine-4′-carboxylic acid.
CHNOTheoretical value69.314.0015.1511.54Actual value69.104.1115.0111.321H NMR (300 MHz, CDCl3): δ 12.74 (s, 1H), δ 9.18 (d, 2H), δ 8.55 (d, 2H), δ 8.40 (s, 2H), δ 7.74 (t, 2H), and δ 7.23 (t, 2H).


#### 2.2.3. Synthesis of 6-(2,2′:6′,2″-Terpyridine-4′-formamide) Hexanoic Acid Methyl Ester

First, we fully dissolved 5.12 g 2,2′:6′,2″-terpyridine-4′-carboxylic acid (18.46 mmol) in 300 mL anhydrous N,N-dimethylformamide (DMF), then added 3.36 g methyl 6-aminohexanoate hydrochloride (18.46 mmol). After that, 7.08 g EDCI (36.92 mmol) was added quickly while stirring at 0°C. Next, the temperature was ambiently raised to room temperature, and the solution was stirred for 12 h and heated to 50°C for 8 h to obtain the light yellow clarification solution. After filtration, the filtrate was dried until the remaining product was viscous, and the solution was then transferred to ethyl acetate/saturated sodium bicarbonate solution=1/1 (300 mL). After sufficient vibration, the solution was placed in static stratification, and the organic phase was reserved. The aqueous phase was extracted twice with 50 mL ethyl acetate solution, and the organic phase was then recombined with it. After washing the organic phase, we dried it with anhydrous MgSO4 and concentrated it in a vacuum. Then, a white precipitate was formed by adding petroleum ether to the concentrated solution, and the white solid was the product after filtration (yield, 59.32%). The elemental composition of 6-(2,2′:6′,2″-terpyridine-4′-formamide) hexanoic acid methyl ester is shown in Table 3.Table 3
Elemental composition of 6-(2,2′:6′,2″-terpyridine-4′-formamide) hexanoic acid methyl ester.
CHNOTheoretical value68.305.9813.8511.87Actual value68.105.9513.6511.321H NMR (400 MHz, DMSO-d6) δ 1.27–1.42 (d, J=7.8Hz, 2H), 1.50–1.64 (q, J=7.5Hz, 4H), 2.27–2.37 (t, J=7.4Hz, 2H), 3.51–3.63 (s, 3H), 7.48–7.58 (dd, J=7.3, 5.1 Hz, 2H), 7.98–8.09 (t, J=7.7Hz, 2H), 8.60–8.68 (d, J=8.0Hz, 2H), 8.72–8.79 (m, 2H), 8.79–8.86 (s, 2H), and 8.99–9.10 (s, 1H).


#### 2.2.4. Synthesis of 6-(2,2′:6′,2″-Terpyridine-4′-formamide) Hexanoic Acid (P1)

Here, we suspended 0.80 g 6-(2,2′:6′,2″-terpyridine-4′-formamide) methyl hexanoate (1.978 mmol) in 150 mL and 1 mol·L-1 sodium hydroxide solution and stirred it at room temperature for 14 h to obtain a transparent solution from the reaction. After filtration, the filtrate was reserved, and concentrated hydrochloric acid was added to form a large number of white precipitates. The white solid was then filtered, washed, and dried to obtain the product (yield, 64.39%). The elemental composition of 6-(2,2′:6′,2″-terpyridine-4′-formamide) hexanoic acid is shown in Table 4.Table 4
Elemental composition of 6-(2,2′:6′,2″-terpyridine-4′-formamide) hexanoic acid.
CHNOTheoretical value67.685.6814.3512.29Actual value67.305.2013.9912.321H NMR (400 MHz, DMSO-d6) δ 1.25–1.43 (m, 2H), 1.46–1.69 (dq, J=14.5, 7.1 Hz, 4H), 2.14–2.30 (t, J=7.3Hz, 2H), 7.48–7.58 (dd, J=7.5, 4.9 Hz, 2H), 7.98–8.09 (dt, J=7.9, 4.0 Hz, 2H), 8.61–8.67 (d, J=8.0Hz, 2H), 8.73–8.79 (d, J=4.7Hz, 2H), 8.79–8.84 (s, 2H), 9.00–9.11 (s, 1H), and 11.77–12.09 (s, 1H).


### 2.3. Synthesis of Glycine Cholesterol Ester

The synthesis route of glycine cholesterol ester is shown in Figure2.Figure 2
Synthesis route of glycine cholesterol ester.


#### 2.3.1. Synthesis of Boc-Glycine Cholesterol Ester

We dissolved 7.74 g cholesterol (20 mmol) and 3.50 g Boc-glycine (20 mmol) in 350 mL dichloromethane and added 4.12 g dicyclohexylcarbodiimide (DCC) (20 mmol) and 0.24 g 4-dimethylaminopyridine (DMAP) (2 mmol) at 0-2°C. Then, the temperature was ambiently raised to room temperature, and the solution was stirred for 24 h. After the reaction, the postreaction solution was filtered, and the filtrate was washed with hydrochloric acid (0.01 mol·L-1), sodium hydroxide solution (0.01 mol·L-1), and distilled water (50 mL each time) for three times each in turn. After this, we separated the organic phase and dried it with anhydrous MgSO4. Next, a white solid was obtained after the solvent was dried. This crude product was further purified using 200- to 300-mesh silica gel column chromatography with a mixed solvent (VEthylacetate:VPetroleumether=1:6) as the eluent to afford the first product, which was the target product (yield, 53.34%). The elemental composition of Boc-glycine cholesterol ester is shown in Table 5.Table 5
Elemental composition of Boc-glycine cholesterol ester.
CHNOTheoretical value75.0910.572.5811.77Actual value74.5611.342.3312.561H NMR (400 MHz, chloroform-d) δ 0.58–0.73 (s, 4H), 0.77–1.67 (m, 56H), 1.90–2.06 (t, J=15.3Hz, 3H), 2.24–2.37 (d, J=8.3Hz, 3H), 3.81–3.91 (d, J=5.4Hz, 2H), 4.60–4.72 (d, J=9.9Hz, 1H), and 5.32–5.40 (d, J=4.9Hz, 1H).


#### 2.3.2. Synthesis of Glycine Cholesterol Ester Hydrochloride

To make the glycine cholesterol ester hydrochloride, we first added 5.44 g Boc-glycine cholesterol ester (10 mmol) to 200 mL dichloromethane. Dry hydrogen chloride gas was slowly injected while stirring until there was no longer any white precipitate being generated. The solution turned into a gel after 30 minutes of rest, and the gel was then stirred to transform it into a solution. After that, a white solid was obtained by filtering, which was the target product (yield, 75.36%). The elemental composition of glycine cholesterol ester hydrochloride is shown in Table6.Table 6
Elemental composition of glycine cholesterol ester hydrochloride.
CHClNOTheoretical value72.5410.507.382.926.66Actual value72.4412.456.582.858.211H NMR (400 MHz, DMSO-d6) δ 0.62–0.67 (s, 2H), 0.80–0.92 (m, 8H), 0.95–1.00 (s, 3H), 0.98–1.08 (d, J=18.5Hz, 1H), 1.05–1.15 (t, J=10.1Hz, 4H), 1.27–1.34 (d, J=8.4Hz, 2H), 1.32–1.50 (m, 2H), 1.46–1.57 (dd, J=15.6, 8.5 Hz, 2H), 1.74–1.86 (d, J=13.0Hz, 2H), 1.84–2.00 (m, 2H), 2.28–2.34 (d, J=7.2Hz, 2H), 3.73–3.80 (d, J=5.7Hz, 2H), 4.53–4.62 (m, 1H), 5.19–5.52 (s, 1H), and 8.32–8.37 (s, 2H).


#### 2.3.3. Synthesis of Glycine Cholesterol Ester (P2)

For the glycine cholesterol ester (P2), we dissolved 8.52 g glycine cholesterol ester hydrochloride (17.8 mmol) in 300 mL THF and added 2.50 mL triethylamine (17.8 mmol) while stirring. Then, the system was heated to 80°C and refluxed for 5 h. After filtration, the filter residue was removed, and the target product was obtained by distillation under pressure (yield, 70.36%). The elemental composition of glycine cholesterol ester is shown in Table7.Table 7
Elemental composition of glycine cholesterol ester.
CHNOTheoretical value78.5011.133.167.21Actual value78.3212.353.018.321H NMR (400 MHz, chloroform-d) δ 0.58–0.72 (s, 3H), 0.75–1.66 (m, 34H), 1.66–1.90 (s, 5H), 1.90–2.06 (m, 2H), 2.13–2.50 (d, J=8.2Hz, 2H), 3.25–3.53 (s, 2H), 4.53–4.72 (q, J=11.2, 10.2 Hz, 1H), and 5.27–5.46 (m, 1H).


### 2.4. Synthesis of DMTCP

The synthesis of DMTCP is shown in Figure3.Figure 3
Synthesis route of DMTCP.To synthesize the DMTCP, we dissolved 0.3900 g 6-(2,2′:6′,2″-terpyridine-4′-formamide) caproic acid (1 mmol) and 0.1351 g HOBT (1 mmol) in 15 mL DMF and dissolved 0.5320 g cholesterol glycine ester (1.2 mmol) and 0.3834 g EDCI (2 mmol) in 60 mL DCM at the same time. Next, the two solutions were mixed and stirred at 30°C for 24 h. After the reaction, we obtained the reaction product by rotatory evaporation and then added 30 mL DCM to dissolve it. The product was washed with 100 mL deionized water three times, and the organic phase was retained. After rotatory evaporation, the product was then purified on a silica gel column (methanol:DCM=2:5). Finally, we obtained pure DMTCP (yield, 88.92%). The elemental composition of DMTCP is shown in Table 8.Table 8
Elemental composition of DMTCP.
CHNOTheoretical value75.068.528.587.84Actual value74.887.988.457.901H NMR (400 MHz, chloroform-d) δ 0.54–2.04 (m, 43H), 2.15–2.36 (m, 4H), 3.40–3.58 (m, 4H), 3.92–4.03 (d, J=5.3Hz, 2H), 4.49–4.61 (m, 1H), 5.23–5.34 (d, J=19.6Hz, 1H), 6.18–6.32 (m, 1H), 6.93–7.01 (s, 1H), 7.30–7.39 (m, 2H), 7.80–7.90 (td, J=7.8, 1.8 Hz, 2H), 8.54–8.62 (d, J=8.0Hz, 2H), 8.65–8.72 (q, J=1.6Hz, 2H), and 8.72–8.80 (s, 2H).


### 2.5. Methods

After the above chemical syntheses, FT-IR P1, P2, DMTCP, and the gels formed by them were pressed together with KBr and tested with the FT-IR 8400 SHIMADZU Fourier transform infrared spectrometer. However, because P1 failed to form a gel in the experimental organic solvent, the correlation spectrum of gel formed by P1 could not be created.


#### 2.5.1. Preparation of Xerogel

The gels formed by P2 or DMTCP were placed on an ultraclean platform, and the ventilation hood was opened until all the organic solvents in the gel were removed so that the resulting xerogel could be used for SEM analysis. Since the boiling point of bromododecane is 276°C, the gel prepared with bromododecane was put into the drying oven overnight at 100°C to the xerogel.


#### 2.5.2. SEM

The sample used for SEM analysis was sprayed with gold for 200 s prior to being observed. The acceleration voltage of the SEM test was set to 5 kV, and the emission current was set to 100μA.


#### 2.5.3. Gelation Test

The gelation properties of P1, P2, and DMTCP in different solvents were tested by the method of “tube inversion.” That is, after the heating and cooling treatment of the solvent were inverted, would the solvent flow to form a gel? A total of 27 common solvents in the laboratory were selected for the gelation tests, and 0.0250 g P1, P2, or DMTCP and 1 mL solvent were added into a 5 mL sample tube (sample concentration was 2.5% (W/V)).When a gel system formed after being dissolved completely and being placed at room temperature, it was denoted by “GT” and a gel system formed by heating and cooling as “G.” A system in which the solute could not be dissolved even at the boiling point was called an insoluble system, “I,” and one in which it partially dissolved was denoted as “PS.” Finally, a system that completely dissolved was denoted as “S.” The experimental results are shown in Tables9, 10, and 11.Table 9
Solvent gelation behavior of P1 in different organic solvents.
Solvent (polarity)P1Indoor temperature70°CFinal state of solutionWater (10.2)IIIBenzene (2.7)IIIMethylbenzene (2.4)IIIXylene (2.5)IIIN-Hexane (0.0)IIINormal octaneIIIDodecaneIIIBromododecaneIIIDichloromethane (3.4)IIITrichloromethane (4.4)IIIMethyl alcohol (5.1)IIIEthyl alcohol (4.3)III1-OctanolIIIIsopropanol (4.3)IIIN-Propyl alcoholIIIDiethyl ether (2.9)IIIPetroleum ether (0.01)IIIEthyl acetate (4.3)IIIAcetone (5.4)IIIAcetonitrile (6.2)IIITetrachloromethane (1.6)IIITriethylamine (5.0)III1,4-Dioxane (4.8)IIITetrahydrofuran (4.2)ISIPyridine (5.3)SSSDMF (6.4)SSSDMSO (7.2)SSSTable 10
Solvent gelation behavior of P2 in different organic solvents.
Solvent (polarity)P2Indoor temperature70°CFinal state of solutionAcetonitrile (6.2)IIIBenzene (2.7)IIIMethylbenzene (2.4)IIITetrachloromethane (1.6)IIIN-Hexane (0.0)IIIN-OctaneIIIDodecaneIIIBromododecaneIIITriethylamine (5.0)IIITrichloromethane (4.4)IIIMethyl alcohol (5.1)IIIEthyl alcohol (4.3)III1-OctanolIIIIsopropanol (4.3)IIIN-Propyl alcohol (4.0)IIIDiethyl ether (2.9)III1,4-Dioxane (4.8)IIIEthyl acetate (4.3)IIIAcetone (5.4)IIIWater (10.2)IPSPSXylene (2.5)SSSDichloromethane (3.1)SSSPetroleum ether (0.01)PSPSPSTetrahydrofuran (4.0)G(T)SG(T)Pyridine (5.3)SSSDMF (6.4)SSSDMSO (7.2)ISITable 11
Gelation behavior of DMTCP in different organic solvents.
SolventDMTCPIndoor temperature70°CFinal state of solutionBenzeneIIIMethylbenzeneIIIN-HexaneIIIN-OctaneIIIDodecaneIIITriethylamineIIITrichloromethaneIIIMethyl alcoholIIIEthyl alcoholIII1-OctanolIIIIsopropanolIIIN-Propyl alcoholIIIEthyl acetateIIIPetroleum etherIIIWaterIIITetrachloromethane (1.6)ISG (transparency)BromododecaneISG (transparency)Diethyl ether (2.9)IIG (turbidity)Xylene (2.5)ISG (transparency)Acetone (5.4)ISIAcetonitrile (6.2)ISI1,4-Dioxane (4.8)SSSDichloromethane (4.4)SSSTetrahydrofuran (4.2)SSSPyridine (5.3)SSSDMF (6.4)SSSDMSO (7.2)SSS


#### 2.5.4. Critical Gel Concentration (CGC) Test

The critical gel concentration was measured by the control variate method. Here, 1 mL solvent was added into a 5 mL sample tube, and the amount of gelator was then increased successively from 1 mg in 1 mg increments until a gel was formed. After heating, cooling, and standing, the minimum amount of gelator required to form a gel was recorded.


#### 2.5.5. Thermal Stability Analysis of Gels

To analyze the thermal stability of the gels, we first performed a gel-sol phase transition temperature (Tgel) test. The gel was placed in a sealed 5 mL sample bottle and immersed upside down in a water bath that was heated at 1°C·min-1 from 25°C. Then, the bottle was tilted and the temperature (Tgel) was noted as the state of the gel began to change. Each gelation concentration was tested three times in parallel to reduce error. Additionally, Tgel was tested in different concentrations of gelators and solvents to analyze the thermal stability more comprehensively.


## 2.1. Reagents

We purchased 2-furfural (AR, 99.0%), anhydrous potassium carbonate (AR, 99.0%), anhydrous magnesium sulfate (AR, 99.0%), pyridine (AR, 99.5%), hydrochloric acid (AR, 36.0-38.0%), acetone (AR, 99.5%), sodium thiosulfate pentahydrate (AR, 99.0%), sodium chloride (AR, 99.5%), anhydrous magnesium sulfate (AR, 99.0%), potassium hydroxide (AR, 85%), and potassium permanganate (AR, 99.5%) from Sinopharm Chemical Reagent Co., Ltd. and purchased Boc-glycine (AR, 98.5%), dicyclohexylcarbodiimide (DCC, AR, 99.0%), 4-dimethylaminopyridine (DMAP, AR, 99.0%), 1-benzotriazolol (HOBT, AR, 99.0%), and 1-ethyl-3-(3-dimethylam-inopropyl) carbodiimide hydrochloride (EDCI, AR, 99.0%) from Xiya Reagent Co., Ltd. Absolute ethyl alcohol (AR, 99.7%), dichloromethane (AR, 99.5%), trichloromethane (AR, 99.0%), ethyl acetate (AR, 99.5%), DMF (N,N-dimethylformamide) (AR, 99.7%), tetrahydrofuran (AR, 99.0%) (THF), concentrated sulfuric acid (GR, 95-98%), and petroleum ether (AR) were purchased from Beijing Chemical Works Co., Ltd., and 2-acetylpyridine was purchased from Shanghai Adamas Co., Ltd. Finally, we purchased methyl 6-aminohexanoate hydrochloride from Heowns and cholesterol (AR, 99%) from J&K Scientific Co., Ltd.


## 2.2. Synthesis of 6-(2,2′:6′,2″-Terpyridine-4′-formamide) Hexanoic Acid (P1)

The synthesis route of 6-(2,2′:6′,2″-terpyridine-4′-formamide) hexanoic acid is shown in Figure 1.Figure 1
Synthesis route of 6-(2,2′:6′:2″-terpyridine-4′-formamide) hexanoic acid.


### 2.2.1. Synthesis of 4′-(2-Furyl)-2,2′:6′,2″-terpyridine

We added 9.00 mL (80 mmol) of 2-acetylpyridine, 3.34 mL (40 mmol) of 2-furaldehyde, and 200 mL of anhydrous ethanol to a three-mouth flask. After the solution was stirred evenly, 6.16 g potassium hydroxide and 120 mL ammonia (25%) were then added. Next, the reaction was refluxed overnight at 60°C, and the cooled solution was filtered to obtain the light yellow solid that is the crude product. The crude product was further purified by using silica gel column chromatography with chloroform (or dichloromethane) as the eluent. Finally, the pale yellow eluent was distilled and dried to obtain an orange-yellow, powdery product. The yield of the reaction was 49.27%, and the elemental composition of 4′-(2-furyl)-2,2′:6′,2″-terpyridine is shown in Table 1. We also characterized its molecular structure by 1H NMR. (The same method was applied to subsequent syntheses.)Table 1
Elemental composition of 4′-(2-furyl)-2,2′:6′,2″-terpyridine.
CHNOTheoretical value76.244.3814.045.34Actual value75.974.2013.585.201H NMR (400 MHz, chloroform-d) δ 6.52–6.59 (dd, J=3.5, 1.8 Hz, 1H), 7.09–7.17 (s, 1H), 7.31–7.43 (t, J=5.8Hz, 2H), 7.53–7.62 (s, 1H), 7.82–7.94 (t, J=7.7Hz, 2H), 8.59–8.69 (d, J=8.0Hz, 2H), and 8.68–8.81 (s, 4H).


### 2.2.2. Synthesis of 2,2′:6′,2″-Terpyridine-4′-carboxylic Acid

We added 3.20 g 4′-(2-furyl)-2,2′:6′,2″-tripyridine and 120 mL pyridine to a conical flask and kept stirring until the solids were completely dissolved. Then, potassium permanganate solution (0.1 g·mL-1) was added drop by drop into the conical flask and stirred at room temperature for 20 h. After the reaction was completed, excessive sodium thiosulfate powder was added to the filtrate of the postreaction solution, and we kept fully stirring until the color turned pale yellow. The solution was left to rest for stratification, and the upper organic phase was reserved to remove solvents by rotary evaporation. After this, 1 mol·L-1 sodium hydroxide solution was added, and the remaining solids were dissolved by heating. Then, the solution was filtered to remove the insoluble solids, and concentrated hydrochloric acid was added to the filtrate slowly while fully stirring until a large number of white precipitates appeared. Finally, the white solid product was obtained by washing with deionized water and drying; yield was about 60%. The elemental composition of 2,2′:6′,2″-terpyridine-4′-carboxylic acid is shown in Table 2.Table 2
Elemental composition of 2,2′:6′,2″-terpyridine-4′-carboxylic acid.
CHNOTheoretical value69.314.0015.1511.54Actual value69.104.1115.0111.321H NMR (300 MHz, CDCl3): δ 12.74 (s, 1H), δ 9.18 (d, 2H), δ 8.55 (d, 2H), δ 8.40 (s, 2H), δ 7.74 (t, 2H), and δ 7.23 (t, 2H).


### 2.2.3. Synthesis of 6-(2,2′:6′,2″-Terpyridine-4′-formamide) Hexanoic Acid Methyl Ester

First, we fully dissolved 5.12 g 2,2′:6′,2″-terpyridine-4′-carboxylic acid (18.46 mmol) in 300 mL anhydrous N,N-dimethylformamide (DMF), then added 3.36 g methyl 6-aminohexanoate hydrochloride (18.46 mmol). After that, 7.08 g EDCI (36.92 mmol) was added quickly while stirring at 0°C. Next, the temperature was ambiently raised to room temperature, and the solution was stirred for 12 h and heated to 50°C for 8 h to obtain the light yellow clarification solution. After filtration, the filtrate was dried until the remaining product was viscous, and the solution was then transferred to ethyl acetate/saturated sodium bicarbonate solution=1/1 (300 mL). After sufficient vibration, the solution was placed in static stratification, and the organic phase was reserved. The aqueous phase was extracted twice with 50 mL ethyl acetate solution, and the organic phase was then recombined with it. After washing the organic phase, we dried it with anhydrous MgSO4 and concentrated it in a vacuum. Then, a white precipitate was formed by adding petroleum ether to the concentrated solution, and the white solid was the product after filtration (yield, 59.32%). The elemental composition of 6-(2,2′:6′,2″-terpyridine-4′-formamide) hexanoic acid methyl ester is shown in Table 3.Table 3
Elemental composition of 6-(2,2′:6′,2″-terpyridine-4′-formamide) hexanoic acid methyl ester.
CHNOTheoretical value68.305.9813.8511.87Actual value68.105.9513.6511.321H NMR (400 MHz, DMSO-d6) δ 1.27–1.42 (d, J=7.8Hz, 2H), 1.50–1.64 (q, J=7.5Hz, 4H), 2.27–2.37 (t, J=7.4Hz, 2H), 3.51–3.63 (s, 3H), 7.48–7.58 (dd, J=7.3, 5.1 Hz, 2H), 7.98–8.09 (t, J=7.7Hz, 2H), 8.60–8.68 (d, J=8.0Hz, 2H), 8.72–8.79 (m, 2H), 8.79–8.86 (s, 2H), and 8.99–9.10 (s, 1H).


### 2.2.4. Synthesis of 6-(2,2′:6′,2″-Terpyridine-4′-formamide) Hexanoic Acid (P1)

Here, we suspended 0.80 g 6-(2,2′:6′,2″-terpyridine-4′-formamide) methyl hexanoate (1.978 mmol) in 150 mL and 1 mol·L-1 sodium hydroxide solution and stirred it at room temperature for 14 h to obtain a transparent solution from the reaction. After filtration, the filtrate was reserved, and concentrated hydrochloric acid was added to form a large number of white precipitates. The white solid was then filtered, washed, and dried to obtain the product (yield, 64.39%). The elemental composition of 6-(2,2′:6′,2″-terpyridine-4′-formamide) hexanoic acid is shown in Table 4.Table 4
Elemental composition of 6-(2,2′:6′,2″-terpyridine-4′-formamide) hexanoic acid.
CHNOTheoretical value67.685.6814.3512.29Actual value67.305.2013.9912.321H NMR (400 MHz, DMSO-d6) δ 1.25–1.43 (m, 2H), 1.46–1.69 (dq, J=14.5, 7.1 Hz, 4H), 2.14–2.30 (t, J=7.3Hz, 2H), 7.48–7.58 (dd, J=7.5, 4.9 Hz, 2H), 7.98–8.09 (dt, J=7.9, 4.0 Hz, 2H), 8.61–8.67 (d, J=8.0Hz, 2H), 8.73–8.79 (d, J=4.7Hz, 2H), 8.79–8.84 (s, 2H), 9.00–9.11 (s, 1H), and 11.77–12.09 (s, 1H).


## 2.2.1. Synthesis of 4′-(2-Furyl)-2,2′:6′,2″-terpyridine

We added 9.00 mL (80 mmol) of 2-acetylpyridine, 3.34 mL (40 mmol) of 2-furaldehyde, and 200 mL of anhydrous ethanol to a three-mouth flask. After the solution was stirred evenly, 6.16 g potassium hydroxide and 120 mL ammonia (25%) were then added. Next, the reaction was refluxed overnight at 60°C, and the cooled solution was filtered to obtain the light yellow solid that is the crude product. The crude product was further purified by using silica gel column chromatography with chloroform (or dichloromethane) as the eluent. Finally, the pale yellow eluent was distilled and dried to obtain an orange-yellow, powdery product. The yield of the reaction was 49.27%, and the elemental composition of 4′-(2-furyl)-2,2′:6′,2″-terpyridine is shown in Table 1. We also characterized its molecular structure by 1H NMR. (The same method was applied to subsequent syntheses.)Table 1
Elemental composition of 4′-(2-furyl)-2,2′:6′,2″-terpyridine.
CHNOTheoretical value76.244.3814.045.34Actual value75.974.2013.585.201H NMR (400 MHz, chloroform-d) δ 6.52–6.59 (dd, J=3.5, 1.8 Hz, 1H), 7.09–7.17 (s, 1H), 7.31–7.43 (t, J=5.8Hz, 2H), 7.53–7.62 (s, 1H), 7.82–7.94 (t, J=7.7Hz, 2H), 8.59–8.69 (d, J=8.0Hz, 2H), and 8.68–8.81 (s, 4H).


## 2.2.2. Synthesis of 2,2′:6′,2″-Terpyridine-4′-carboxylic Acid

We added 3.20 g 4′-(2-furyl)-2,2′:6′,2″-tripyridine and 120 mL pyridine to a conical flask and kept stirring until the solids were completely dissolved. Then, potassium permanganate solution (0.1 g·mL-1) was added drop by drop into the conical flask and stirred at room temperature for 20 h. After the reaction was completed, excessive sodium thiosulfate powder was added to the filtrate of the postreaction solution, and we kept fully stirring until the color turned pale yellow. The solution was left to rest for stratification, and the upper organic phase was reserved to remove solvents by rotary evaporation. After this, 1 mol·L-1 sodium hydroxide solution was added, and the remaining solids were dissolved by heating. Then, the solution was filtered to remove the insoluble solids, and concentrated hydrochloric acid was added to the filtrate slowly while fully stirring until a large number of white precipitates appeared. Finally, the white solid product was obtained by washing with deionized water and drying; yield was about 60%. The elemental composition of 2,2′:6′,2″-terpyridine-4′-carboxylic acid is shown in Table 2.Table 2
Elemental composition of 2,2′:6′,2″-terpyridine-4′-carboxylic acid.
CHNOTheoretical value69.314.0015.1511.54Actual value69.104.1115.0111.321H NMR (300 MHz, CDCl3): δ 12.74 (s, 1H), δ 9.18 (d, 2H), δ 8.55 (d, 2H), δ 8.40 (s, 2H), δ 7.74 (t, 2H), and δ 7.23 (t, 2H).


## 2.2.3. Synthesis of 6-(2,2′:6′,2″-Terpyridine-4′-formamide) Hexanoic Acid Methyl Ester

First, we fully dissolved 5.12 g 2,2′:6′,2″-terpyridine-4′-carboxylic acid (18.46 mmol) in 300 mL anhydrous N,N-dimethylformamide (DMF), then added 3.36 g methyl 6-aminohexanoate hydrochloride (18.46 mmol). After that, 7.08 g EDCI (36.92 mmol) was added quickly while stirring at 0°C. Next, the temperature was ambiently raised to room temperature, and the solution was stirred for 12 h and heated to 50°C for 8 h to obtain the light yellow clarification solution. After filtration, the filtrate was dried until the remaining product was viscous, and the solution was then transferred to ethyl acetate/saturated sodium bicarbonate solution=1/1 (300 mL). After sufficient vibration, the solution was placed in static stratification, and the organic phase was reserved. The aqueous phase was extracted twice with 50 mL ethyl acetate solution, and the organic phase was then recombined with it. After washing the organic phase, we dried it with anhydrous MgSO4 and concentrated it in a vacuum. Then, a white precipitate was formed by adding petroleum ether to the concentrated solution, and the white solid was the product after filtration (yield, 59.32%). The elemental composition of 6-(2,2′:6′,2″-terpyridine-4′-formamide) hexanoic acid methyl ester is shown in Table 3.Table 3
Elemental composition of 6-(2,2′:6′,2″-terpyridine-4′-formamide) hexanoic acid methyl ester.
CHNOTheoretical value68.305.9813.8511.87Actual value68.105.9513.6511.321H NMR (400 MHz, DMSO-d6) δ 1.27–1.42 (d, J=7.8Hz, 2H), 1.50–1.64 (q, J=7.5Hz, 4H), 2.27–2.37 (t, J=7.4Hz, 2H), 3.51–3.63 (s, 3H), 7.48–7.58 (dd, J=7.3, 5.1 Hz, 2H), 7.98–8.09 (t, J=7.7Hz, 2H), 8.60–8.68 (d, J=8.0Hz, 2H), 8.72–8.79 (m, 2H), 8.79–8.86 (s, 2H), and 8.99–9.10 (s, 1H).


## 2.2.4. Synthesis of 6-(2,2′:6′,2″-Terpyridine-4′-formamide) Hexanoic Acid (P1)

Here, we suspended 0.80 g 6-(2,2′:6′,2″-terpyridine-4′-formamide) methyl hexanoate (1.978 mmol) in 150 mL and 1 mol·L-1 sodium hydroxide solution and stirred it at room temperature for 14 h to obtain a transparent solution from the reaction. After filtration, the filtrate was reserved, and concentrated hydrochloric acid was added to form a large number of white precipitates. The white solid was then filtered, washed, and dried to obtain the product (yield, 64.39%). The elemental composition of 6-(2,2′:6′,2″-terpyridine-4′-formamide) hexanoic acid is shown in Table 4.Table 4
Elemental composition of 6-(2,2′:6′,2″-terpyridine-4′-formamide) hexanoic acid.
CHNOTheoretical value67.685.6814.3512.29Actual value67.305.2013.9912.321H NMR (400 MHz, DMSO-d6) δ 1.25–1.43 (m, 2H), 1.46–1.69 (dq, J=14.5, 7.1 Hz, 4H), 2.14–2.30 (t, J=7.3Hz, 2H), 7.48–7.58 (dd, J=7.5, 4.9 Hz, 2H), 7.98–8.09 (dt, J=7.9, 4.0 Hz, 2H), 8.61–8.67 (d, J=8.0Hz, 2H), 8.73–8.79 (d, J=4.7Hz, 2H), 8.79–8.84 (s, 2H), 9.00–9.11 (s, 1H), and 11.77–12.09 (s, 1H).


## 2.3. Synthesis of Glycine Cholesterol Ester

The synthesis route of glycine cholesterol ester is shown in Figure2.Figure 2
Synthesis route of glycine cholesterol ester.


### 2.3.1. Synthesis of Boc-Glycine Cholesterol Ester

We dissolved 7.74 g cholesterol (20 mmol) and 3.50 g Boc-glycine (20 mmol) in 350 mL dichloromethane and added 4.12 g dicyclohexylcarbodiimide (DCC) (20 mmol) and 0.24 g 4-dimethylaminopyridine (DMAP) (2 mmol) at 0-2°C. Then, the temperature was ambiently raised to room temperature, and the solution was stirred for 24 h. After the reaction, the postreaction solution was filtered, and the filtrate was washed with hydrochloric acid (0.01 mol·L-1), sodium hydroxide solution (0.01 mol·L-1), and distilled water (50 mL each time) for three times each in turn. After this, we separated the organic phase and dried it with anhydrous MgSO4. Next, a white solid was obtained after the solvent was dried. This crude product was further purified using 200- to 300-mesh silica gel column chromatography with a mixed solvent (VEthylacetate:VPetroleumether=1:6) as the eluent to afford the first product, which was the target product (yield, 53.34%). The elemental composition of Boc-glycine cholesterol ester is shown in Table 5.Table 5
Elemental composition of Boc-glycine cholesterol ester.
CHNOTheoretical value75.0910.572.5811.77Actual value74.5611.342.3312.561H NMR (400 MHz, chloroform-d) δ 0.58–0.73 (s, 4H), 0.77–1.67 (m, 56H), 1.90–2.06 (t, J=15.3Hz, 3H), 2.24–2.37 (d, J=8.3Hz, 3H), 3.81–3.91 (d, J=5.4Hz, 2H), 4.60–4.72 (d, J=9.9Hz, 1H), and 5.32–5.40 (d, J=4.9Hz, 1H).


### 2.3.2. Synthesis of Glycine Cholesterol Ester Hydrochloride

To make the glycine cholesterol ester hydrochloride, we first added 5.44 g Boc-glycine cholesterol ester (10 mmol) to 200 mL dichloromethane. Dry hydrogen chloride gas was slowly injected while stirring until there was no longer any white precipitate being generated. The solution turned into a gel after 30 minutes of rest, and the gel was then stirred to transform it into a solution. After that, a white solid was obtained by filtering, which was the target product (yield, 75.36%). The elemental composition of glycine cholesterol ester hydrochloride is shown in Table6.Table 6
Elemental composition of glycine cholesterol ester hydrochloride.
CHClNOTheoretical value72.5410.507.382.926.66Actual value72.4412.456.582.858.211H NMR (400 MHz, DMSO-d6) δ 0.62–0.67 (s, 2H), 0.80–0.92 (m, 8H), 0.95–1.00 (s, 3H), 0.98–1.08 (d, J=18.5Hz, 1H), 1.05–1.15 (t, J=10.1Hz, 4H), 1.27–1.34 (d, J=8.4Hz, 2H), 1.32–1.50 (m, 2H), 1.46–1.57 (dd, J=15.6, 8.5 Hz, 2H), 1.74–1.86 (d, J=13.0Hz, 2H), 1.84–2.00 (m, 2H), 2.28–2.34 (d, J=7.2Hz, 2H), 3.73–3.80 (d, J=5.7Hz, 2H), 4.53–4.62 (m, 1H), 5.19–5.52 (s, 1H), and 8.32–8.37 (s, 2H).


### 2.3.3. Synthesis of Glycine Cholesterol Ester (P2)

For the glycine cholesterol ester (P2), we dissolved 8.52 g glycine cholesterol ester hydrochloride (17.8 mmol) in 300 mL THF and added 2.50 mL triethylamine (17.8 mmol) while stirring. Then, the system was heated to 80°C and refluxed for 5 h. After filtration, the filter residue was removed, and the target product was obtained by distillation under pressure (yield, 70.36%). The elemental composition of glycine cholesterol ester is shown in Table7.Table 7
Elemental composition of glycine cholesterol ester.
CHNOTheoretical value78.5011.133.167.21Actual value78.3212.353.018.321H NMR (400 MHz, chloroform-d) δ 0.58–0.72 (s, 3H), 0.75–1.66 (m, 34H), 1.66–1.90 (s, 5H), 1.90–2.06 (m, 2H), 2.13–2.50 (d, J=8.2Hz, 2H), 3.25–3.53 (s, 2H), 4.53–4.72 (q, J=11.2, 10.2 Hz, 1H), and 5.27–5.46 (m, 1H).


## 2.3.1. Synthesis of Boc-Glycine Cholesterol Ester

We dissolved 7.74 g cholesterol (20 mmol) and 3.50 g Boc-glycine (20 mmol) in 350 mL dichloromethane and added 4.12 g dicyclohexylcarbodiimide (DCC) (20 mmol) and 0.24 g 4-dimethylaminopyridine (DMAP) (2 mmol) at 0-2°C. Then, the temperature was ambiently raised to room temperature, and the solution was stirred for 24 h. After the reaction, the postreaction solution was filtered, and the filtrate was washed with hydrochloric acid (0.01 mol·L-1), sodium hydroxide solution (0.01 mol·L-1), and distilled water (50 mL each time) for three times each in turn. After this, we separated the organic phase and dried it with anhydrous MgSO4. Next, a white solid was obtained after the solvent was dried. This crude product was further purified using 200- to 300-mesh silica gel column chromatography with a mixed solvent (VEthylacetate:VPetroleumether=1:6) as the eluent to afford the first product, which was the target product (yield, 53.34%). The elemental composition of Boc-glycine cholesterol ester is shown in Table 5.Table 5
Elemental composition of Boc-glycine cholesterol ester.
CHNOTheoretical value75.0910.572.5811.77Actual value74.5611.342.3312.561H NMR (400 MHz, chloroform-d) δ 0.58–0.73 (s, 4H), 0.77–1.67 (m, 56H), 1.90–2.06 (t, J=15.3Hz, 3H), 2.24–2.37 (d, J=8.3Hz, 3H), 3.81–3.91 (d, J=5.4Hz, 2H), 4.60–4.72 (d, J=9.9Hz, 1H), and 5.32–5.40 (d, J=4.9Hz, 1H).


## 2.3.2. Synthesis of Glycine Cholesterol Ester Hydrochloride

To make the glycine cholesterol ester hydrochloride, we first added 5.44 g Boc-glycine cholesterol ester (10 mmol) to 200 mL dichloromethane. Dry hydrogen chloride gas was slowly injected while stirring until there was no longer any white precipitate being generated. The solution turned into a gel after 30 minutes of rest, and the gel was then stirred to transform it into a solution. After that, a white solid was obtained by filtering, which was the target product (yield, 75.36%). The elemental composition of glycine cholesterol ester hydrochloride is shown in Table6.Table 6
Elemental composition of glycine cholesterol ester hydrochloride.
CHClNOTheoretical value72.5410.507.382.926.66Actual value72.4412.456.582.858.211H NMR (400 MHz, DMSO-d6) δ 0.62–0.67 (s, 2H), 0.80–0.92 (m, 8H), 0.95–1.00 (s, 3H), 0.98–1.08 (d, J=18.5Hz, 1H), 1.05–1.15 (t, J=10.1Hz, 4H), 1.27–1.34 (d, J=8.4Hz, 2H), 1.32–1.50 (m, 2H), 1.46–1.57 (dd, J=15.6, 8.5 Hz, 2H), 1.74–1.86 (d, J=13.0Hz, 2H), 1.84–2.00 (m, 2H), 2.28–2.34 (d, J=7.2Hz, 2H), 3.73–3.80 (d, J=5.7Hz, 2H), 4.53–4.62 (m, 1H), 5.19–5.52 (s, 1H), and 8.32–8.37 (s, 2H).


## 2.3.3. Synthesis of Glycine Cholesterol Ester (P2)

For the glycine cholesterol ester (P2), we dissolved 8.52 g glycine cholesterol ester hydrochloride (17.8 mmol) in 300 mL THF and added 2.50 mL triethylamine (17.8 mmol) while stirring. Then, the system was heated to 80°C and refluxed for 5 h. After filtration, the filter residue was removed, and the target product was obtained by distillation under pressure (yield, 70.36%). The elemental composition of glycine cholesterol ester is shown in Table7.Table 7
Elemental composition of glycine cholesterol ester.
CHNOTheoretical value78.5011.133.167.21Actual value78.3212.353.018.321H NMR (400 MHz, chloroform-d) δ 0.58–0.72 (s, 3H), 0.75–1.66 (m, 34H), 1.66–1.90 (s, 5H), 1.90–2.06 (m, 2H), 2.13–2.50 (d, J=8.2Hz, 2H), 3.25–3.53 (s, 2H), 4.53–4.72 (q, J=11.2, 10.2 Hz, 1H), and 5.27–5.46 (m, 1H).


## 2.4. Synthesis of DMTCP

The synthesis of DMTCP is shown in Figure3.Figure 3
Synthesis route of DMTCP.To synthesize the DMTCP, we dissolved 0.3900 g 6-(2,2′:6′,2″-terpyridine-4′-formamide) caproic acid (1 mmol) and 0.1351 g HOBT (1 mmol) in 15 mL DMF and dissolved 0.5320 g cholesterol glycine ester (1.2 mmol) and 0.3834 g EDCI (2 mmol) in 60 mL DCM at the same time. Next, the two solutions were mixed and stirred at 30°C for 24 h. After the reaction, we obtained the reaction product by rotatory evaporation and then added 30 mL DCM to dissolve it. The product was washed with 100 mL deionized water three times, and the organic phase was retained. After rotatory evaporation, the product was then purified on a silica gel column (methanol:DCM=2:5). Finally, we obtained pure DMTCP (yield, 88.92%). The elemental composition of DMTCP is shown in Table 8.Table 8
Elemental composition of DMTCP.
CHNOTheoretical value75.068.528.587.84Actual value74.887.988.457.901H NMR (400 MHz, chloroform-d) δ 0.54–2.04 (m, 43H), 2.15–2.36 (m, 4H), 3.40–3.58 (m, 4H), 3.92–4.03 (d, J=5.3Hz, 2H), 4.49–4.61 (m, 1H), 5.23–5.34 (d, J=19.6Hz, 1H), 6.18–6.32 (m, 1H), 6.93–7.01 (s, 1H), 7.30–7.39 (m, 2H), 7.80–7.90 (td, J=7.8, 1.8 Hz, 2H), 8.54–8.62 (d, J=8.0Hz, 2H), 8.65–8.72 (q, J=1.6Hz, 2H), and 8.72–8.80 (s, 2H).


## 2.5. Methods

After the above chemical syntheses, FT-IR P1, P2, DMTCP, and the gels formed by them were pressed together with KBr and tested with the FT-IR 8400 SHIMADZU Fourier transform infrared spectrometer. However, because P1 failed to form a gel in the experimental organic solvent, the correlation spectrum of gel formed by P1 could not be created.


### 2.5.1. Preparation of Xerogel

The gels formed by P2 or DMTCP were placed on an ultraclean platform, and the ventilation hood was opened until all the organic solvents in the gel were removed so that the resulting xerogel could be used for SEM analysis. Since the boiling point of bromododecane is 276°C, the gel prepared with bromododecane was put into the drying oven overnight at 100°C to the xerogel.


### 2.5.2. SEM

The sample used for SEM analysis was sprayed with gold for 200 s prior to being observed. The acceleration voltage of the SEM test was set to 5 kV, and the emission current was set to 100μA.


### 2.5.3. Gelation Test

The gelation properties of P1, P2, and DMTCP in different solvents were tested by the method of “tube inversion.” That is, after the heating and cooling treatment of the solvent were inverted, would the solvent flow to form a gel? A total of 27 common solvents in the laboratory were selected for the gelation tests, and 0.0250 g P1, P2, or DMTCP and 1 mL solvent were added into a 5 mL sample tube (sample concentration was 2.5% (W/V)).When a gel system formed after being dissolved completely and being placed at room temperature, it was denoted by “GT” and a gel system formed by heating and cooling as “G.” A system in which the solute could not be dissolved even at the boiling point was called an insoluble system, “I,” and one in which it partially dissolved was denoted as “PS.” Finally, a system that completely dissolved was denoted as “S.” The experimental results are shown in Tables9, 10, and 11.Table 9
Solvent gelation behavior of P1 in different organic solvents.
Solvent (polarity)P1Indoor temperature70°CFinal state of solutionWater (10.2)IIIBenzene (2.7)IIIMethylbenzene (2.4)IIIXylene (2.5)IIIN-Hexane (0.0)IIINormal octaneIIIDodecaneIIIBromododecaneIIIDichloromethane (3.4)IIITrichloromethane (4.4)IIIMethyl alcohol (5.1)IIIEthyl alcohol (4.3)III1-OctanolIIIIsopropanol (4.3)IIIN-Propyl alcoholIIIDiethyl ether (2.9)IIIPetroleum ether (0.01)IIIEthyl acetate (4.3)IIIAcetone (5.4)IIIAcetonitrile (6.2)IIITetrachloromethane (1.6)IIITriethylamine (5.0)III1,4-Dioxane (4.8)IIITetrahydrofuran (4.2)ISIPyridine (5.3)SSSDMF (6.4)SSSDMSO (7.2)SSSTable 10
Solvent gelation behavior of P2 in different organic solvents.
Solvent (polarity)P2Indoor temperature70°CFinal state of solutionAcetonitrile (6.2)IIIBenzene (2.7)IIIMethylbenzene (2.4)IIITetrachloromethane (1.6)IIIN-Hexane (0.0)IIIN-OctaneIIIDodecaneIIIBromododecaneIIITriethylamine (5.0)IIITrichloromethane (4.4)IIIMethyl alcohol (5.1)IIIEthyl alcohol (4.3)III1-OctanolIIIIsopropanol (4.3)IIIN-Propyl alcohol (4.0)IIIDiethyl ether (2.9)III1,4-Dioxane (4.8)IIIEthyl acetate (4.3)IIIAcetone (5.4)IIIWater (10.2)IPSPSXylene (2.5)SSSDichloromethane (3.1)SSSPetroleum ether (0.01)PSPSPSTetrahydrofuran (4.0)G(T)SG(T)Pyridine (5.3)SSSDMF (6.4)SSSDMSO (7.2)ISITable 11
Gelation behavior of DMTCP in different organic solvents.
SolventDMTCPIndoor temperature70°CFinal state of solutionBenzeneIIIMethylbenzeneIIIN-HexaneIIIN-OctaneIIIDodecaneIIITriethylamineIIITrichloromethaneIIIMethyl alcoholIIIEthyl alcoholIII1-OctanolIIIIsopropanolIIIN-Propyl alcoholIIIEthyl acetateIIIPetroleum etherIIIWaterIIITetrachloromethane (1.6)ISG (transparency)BromododecaneISG (transparency)Diethyl ether (2.9)IIG (turbidity)Xylene (2.5)ISG (transparency)Acetone (5.4)ISIAcetonitrile (6.2)ISI1,4-Dioxane (4.8)SSSDichloromethane (4.4)SSSTetrahydrofuran (4.2)SSSPyridine (5.3)SSSDMF (6.4)SSSDMSO (7.2)SSS


### 2.5.4. Critical Gel Concentration (CGC) Test

The critical gel concentration was measured by the control variate method. Here, 1 mL solvent was added into a 5 mL sample tube, and the amount of gelator was then increased successively from 1 mg in 1 mg increments until a gel was formed. After heating, cooling, and standing, the minimum amount of gelator required to form a gel was recorded.


### 2.5.5. Thermal Stability Analysis of Gels

To analyze the thermal stability of the gels, we first performed a gel-sol phase transition temperature (Tgel) test. The gel was placed in a sealed 5 mL sample bottle and immersed upside down in a water bath that was heated at 1°C·min-1 from 25°C. Then, the bottle was tilted and the temperature (Tgel) was noted as the state of the gel began to change. Each gelation concentration was tested three times in parallel to reduce error. Additionally, Tgel was tested in different concentrations of gelators and solvents to analyze the thermal stability more comprehensively.


## 2.5.1. Preparation of Xerogel

The gels formed by P2 or DMTCP were placed on an ultraclean platform, and the ventilation hood was opened until all the organic solvents in the gel were removed so that the resulting xerogel could be used for SEM analysis. Since the boiling point of bromododecane is 276°C, the gel prepared with bromododecane was put into the drying oven overnight at 100°C to the xerogel.


## 2.5.2. SEM

The sample used for SEM analysis was sprayed with gold for 200 s prior to being observed. The acceleration voltage of the SEM test was set to 5 kV, and the emission current was set to 100μA.


## 2.5.3. Gelation Test

The gelation properties of P1, P2, and DMTCP in different solvents were tested by the method of “tube inversion.” That is, after the heating and cooling treatment of the solvent were inverted, would the solvent flow to form a gel? A total of 27 common solvents in the laboratory were selected for the gelation tests, and 0.0250 g P1, P2, or DMTCP and 1 mL solvent were added into a 5 mL sample tube (sample concentration was 2.5% (W/V)).When a gel system formed after being dissolved completely and being placed at room temperature, it was denoted by “GT” and a gel system formed by heating and cooling as “G.” A system in which the solute could not be dissolved even at the boiling point was called an insoluble system, “I,” and one in which it partially dissolved was denoted as “PS.” Finally, a system that completely dissolved was denoted as “S.” The experimental results are shown in Tables9, 10, and 11.Table 9
Solvent gelation behavior of P1 in different organic solvents.
Solvent (polarity)P1Indoor temperature70°CFinal state of solutionWater (10.2)IIIBenzene (2.7)IIIMethylbenzene (2.4)IIIXylene (2.5)IIIN-Hexane (0.0)IIINormal octaneIIIDodecaneIIIBromododecaneIIIDichloromethane (3.4)IIITrichloromethane (4.4)IIIMethyl alcohol (5.1)IIIEthyl alcohol (4.3)III1-OctanolIIIIsopropanol (4.3)IIIN-Propyl alcoholIIIDiethyl ether (2.9)IIIPetroleum ether (0.01)IIIEthyl acetate (4.3)IIIAcetone (5.4)IIIAcetonitrile (6.2)IIITetrachloromethane (1.6)IIITriethylamine (5.0)III1,4-Dioxane (4.8)IIITetrahydrofuran (4.2)ISIPyridine (5.3)SSSDMF (6.4)SSSDMSO (7.2)SSSTable 10
Solvent gelation behavior of P2 in different organic solvents.
Solvent (polarity)P2Indoor temperature70°CFinal state of solutionAcetonitrile (6.2)IIIBenzene (2.7)IIIMethylbenzene (2.4)IIITetrachloromethane (1.6)IIIN-Hexane (0.0)IIIN-OctaneIIIDodecaneIIIBromododecaneIIITriethylamine (5.0)IIITrichloromethane (4.4)IIIMethyl alcohol (5.1)IIIEthyl alcohol (4.3)III1-OctanolIIIIsopropanol (4.3)IIIN-Propyl alcohol (4.0)IIIDiethyl ether (2.9)III1,4-Dioxane (4.8)IIIEthyl acetate (4.3)IIIAcetone (5.4)IIIWater (10.2)IPSPSXylene (2.5)SSSDichloromethane (3.1)SSSPetroleum ether (0.01)PSPSPSTetrahydrofuran (4.0)G(T)SG(T)Pyridine (5.3)SSSDMF (6.4)SSSDMSO (7.2)ISITable 11
Gelation behavior of DMTCP in different organic solvents.
SolventDMTCPIndoor temperature70°CFinal state of solutionBenzeneIIIMethylbenzeneIIIN-HexaneIIIN-OctaneIIIDodecaneIIITriethylamineIIITrichloromethaneIIIMethyl alcoholIIIEthyl alcoholIII1-OctanolIIIIsopropanolIIIN-Propyl alcoholIIIEthyl acetateIIIPetroleum etherIIIWaterIIITetrachloromethane (1.6)ISG (transparency)BromododecaneISG (transparency)Diethyl ether (2.9)IIG (turbidity)Xylene (2.5)ISG (transparency)Acetone (5.4)ISIAcetonitrile (6.2)ISI1,4-Dioxane (4.8)SSSDichloromethane (4.4)SSSTetrahydrofuran (4.2)SSSPyridine (5.3)SSSDMF (6.4)SSSDMSO (7.2)SSS


## 2.5.4. Critical Gel Concentration (CGC) Test

The critical gel concentration was measured by the control variate method. Here, 1 mL solvent was added into a 5 mL sample tube, and the amount of gelator was then increased successively from 1 mg in 1 mg increments until a gel was formed. After heating, cooling, and standing, the minimum amount of gelator required to form a gel was recorded.


## 2.5.5. Thermal Stability Analysis of Gels

To analyze the thermal stability of the gels, we first performed a gel-sol phase transition temperature (Tgel) test. The gel was placed in a sealed 5 mL sample bottle and immersed upside down in a water bath that was heated at 1°C·min-1 from 25°C. Then, the bottle was tilted and the temperature (Tgel) was noted as the state of the gel began to change. Each gelation concentration was tested three times in parallel to reduce error. Additionally, Tgel was tested in different concentrations of gelators and solvents to analyze the thermal stability more comprehensively.


## 3. Results and Discussion

### 3.1. Gelation Behaviors of the Compounds

As we can see from Table9, P1 was insoluble in all tested solvents except pyridine, DMF, and DMSO (but was soluble under heating conditions in THF), showing a poor solubility among the gel solvents we tried. Because P1 could not be dissolved in so many solvents, the spatial network structure could not be formed. Hence, P1 could not be prepared as a gel with these solvents. However, in the solvents that could dissolve P1, it was completely dissociated in the solvent and the interaction between the solute and P1 was weak. As a result, the network structures necessary for preparing gels could not be formed.The solvent gelation experiments for P2 in 27 solvents showed that P2 only formed a gel in THF (Table10). Furthermore, there were two ways it could generate a gel. The first was that a gel could be formed after ultrasonic treatment at room temperature. The other was that a gel could be formed after heating and cooling without ultrasonic treatment. In addition, the gel formed with the latter method could return to its solution state after heating and violent shaking, but this gel could be formed again after heating and cooling.By comparing the polarity between solvents, we found that P2 exhibited a medium polarity. The P2 could dissolve in the solvents with a similar polarity to THF (4.2), such as xylene (2.5), dichloromethane (3.4), pyridine (5.3), DMF (6.4), and DMSO (7.2). This can be explained on the microscopic level: when the interaction between disperse phases that is weaker than that between disperse phase and dispersant, the P2 appears as a solution. Conversely, the dispersions can also aggregate to form precipitates.The results of the gelation test (Table11) indicate that DMTCP was insoluble in ethyl ether at room temperature and under heating conditions. However, in the concentration of 10‰ (w/v), the DMTCP was able to form an opaque gel after 20 seconds of ultrasonic processing (Figure 4). In other words, DMTCP (diethyl ether) gel had a special response to ultrasound. Unfortunately, the gel did not possess the property of thermal reversibility.Figure 4
Changes of DMTCP (diethyl ether) gel-sol.In contrast, DMTCP could dissolve in carbon tetrachloride, dodecane bromide, and xylene to form a clear solution under heating conditions. After ambient cooling, it could also form a transparent gel.Furthermore, the gels we tested that formed in carbon tetrachloride, dodecane bromide, and xylene had the same properties. They could be transformed from a solution into a gel by heating and cooling; they were thermally reversible. In addition, under the action of shear stress, they could be transformed from the gel state to the solution state, but could not be automatically transformed into a gel at room temperature. However, they were able to convert to gels after being heated and cooled, and this could be repeated several times (Figure5).Figure 5
Gel-sol transition diagram of DMTCP (CCl4, bromodecane, and xylene).


### 3.2. Spectroscopy

The infrared spectrum of compound 6-(2,2′:6′,2″-terpyridine-4′-formamide) hexanoic acid is shown in Figure 6, where we can see that the absorption peak at 3357 cm-1 is N-H stretching vibration absorption of the secondary amide. At 3064 cm-1, there is a wide peak center, which is the characteristic absorption peak of carboxylic acid, and at 1720 cm-1, the wide peak absorption indicates the existence of carboxylic acid. The absorption peaks at 2950 cm-1 and 2871 cm-1 are the stretching vibration absorption of saturated alkanes, and the peak at 1654 cm-1 is the stretching vibration absorption of the carbonyl group C=O, which also reflects the association absorption peak of the compound’s amide bond. The four peaks at 1583 cm-1, 1552 cm-1, 1533 cm-1, and 1469 cm-1 are the characteristic absorption of pyridine ring skeleton vibration. Hence, when we combined this analysis with our 1H NMR analysis, we determined the product to indeed be target product P1.Figure 6
Infrared spectra of 6-(2,2′:6′:2″-terpyridine-4′-formamide) hexanoic acid.From the structural analysis we conducted, we found that one end of P1 was terpyridine, which itself forms a large conjugated system but has poor solubility. The long chain of hexanoic acid at the other end and the long chain of carbon can reduce the polarity of the material, but the overall polarity of the material was higher. Thin layer chromatography also showed that only by increasing the amount of methanol in the developing agent can it be developed.As we can see from the comparison between P2 and P2-Gel in Figure7, after P2 formed the gel, two absorption peaks formed by the stretching vibration of the primary amine at 3485 cm-1 and 3413 cm-1 appear at 3398 cm-1 and 3338 cm-1, respectively. In addition, the peak became wider. Additionally, the stretching vibration absorption peaks of the carbonyl group in the ester group at 1745 cm-1 appear at 1735 cm-1. Under the influence of hydrogen bonds, these peaks move to the direction of the small wave numbers, which directly indicates the existence of hydrogen bonds in the formed gel. We conclude that the position of the hydrogen bonds in P2 should be between the primary amine group and the ester carbonyl group.Figure 7
Infrared contrast spectra of P2 and P2-Gel.Figure8 shows that the N-H stretching vibration absorption peak in the amide bond located at 3292 cm-1 moved 2 units to the direction of the low wave numbers after the formation of the gel and that the C=O stretching vibration absorption peak of the amide bond at 1652 cm-1 moved to 1650 cm-1 in the xerogel. The bending vibration peak of N-H in the amide bond at 1539 cm-1 stayed the same. Moreover, the C=O stretching vibration peak of the ester group at 1741 cm-1 moved to 1743 cm-1, which is an abnormal move to the direction of higher wave numbers. According to the above data, DMTCP may form a weak hydrogen bond in diethyl ether.Figure 8
Infrared comparison between DMTCP (ether) xerogel and DMTCP.In Figure9, we see that after gel formation in CCl4, the N-H stretching vibration absorption peak of the amide bond at 3292 cm-1 moved toward the low wave numbers, at 3291 cm-1, with a slight red shift, and that the C=O stretching vibration absorption peak at 1652 cm-1 in the amide bond moved to 1647 cm-1 in the xerogel. That is, it moved 5 units towards the lower wave numbers. The N-H bending vibration peak in the amide bond at 1539 cm-1 moved to the higher wave numbers and reached 1543 cm-1. This shows that hydrogen bonds were formed between the amide bonds.Figure 9
Infrared comparison between DMTCP(CCl4) xerogel and DMTCP.Figure10 shows that the N-H stretching vibration absorption peak of the amide bond at 3292 cm-1 moved to the lower wave numbers to the point at 3282 cm-1 after the gel was formed in xylene (red shift). The C=O stretching vibration absorption peak at 1652 cm-1 in the amide bond moved to 1644 cm-1 in the xerogel. In other words, it moved 8 units towards the lower wave numbers. Additionally, the N-H bending vibration peak in the amide bond at 1539 cm-1 moved toward the higher wave numbers and reached 1544 cm-1. This shows that hydrogen bonds were formed between the amide bonds, as in Figure 9.Figure 10
Infrared comparison between DMTCP (xylene) xerogel and DMTCP.


### 3.3. Morphology

The macroscopic characteristics of the gel formed by P2 are shown in Figure11. As can be seen from the figure, it was an opaque gel in the THF solvent, with an obvious solvent gelation effect. There also were no free solvent flows after inversion.Figure 11
Macroscopic view of P2 forming a gel in THF.The microcosmic characteristics of the gel are shown in Figure12. From the scanning electron microscopy (SEM) images of the P2-Gel at 400 times (Figure 12(a)) and 1000 times (Figure 12(b)) magnification, we can see that P2 formed a fibrous gelatinous structure in the THF solvent. Based on the hydrogen bond formation mechanism of the P2-Gel mentioned above, we can further infer that the hydrogen bond between primary amines formed the ester carbonyl group. The promoted fibers between P2 molecules formed a three-dimensional network structure and bound with the THF solvent to form a gel.Figure 12
SEM image of P2 xerogel (THF) at 400 times (a) and 1000 times (b) magnification.
(a)(b)The macroscopic characteristic diagram of the gel formed by DMTCP in different organic solvents is shown in Figure13.Figure 13
Macroscopic morphology of DMTCP gel formed in four solvents: (a) diethyl ether, (b) carbon tetrachloride, (c) bromododecane, and (d) xylene.
(a)(b)(c)(d)As we can see from Figures14(a) and 14(b), DMTCP formed a densely interlaced and extremely fine fibrous structure in diethyl ether that was also very disorderly. This is consistent with the appearance of the opaque gel that DMTCP formed under ultrasonic in diethyl ether as well, and we speculate that DMTCP molecules stack themselves through hydrogen bonding under intense ultrasonic vibration. In addition, the intermolecular interactions between ether and DMTCP are balanced. That is, the intermolecular interactions between solute and solvent are balanced, and these balanced intermolecular interactions prevent DMTCP from forming its own excessive agglomeration to form precipitation and from sufficient dispersion in ether to establish a spatial network. Therefore, DMTCP has ultrasonic response characteristics in ethyl ether and forms an opaque gel, which is the macroscopic representation of the balanced intermolecular interactions between the dispersed substance and the dispersant.Figure 14
(a) 600-fold SEM diagram of DMTCP (ethyl ether), (b) 1.5K SEM diagram of DMTCP (ethyl ether), (c) DMTCP (CCl4) 500 times SEM, (d) DMTCP (CCl4) 7K times SEM, (e) DMTCP(CH3(CH2)11Br) 300 times SEM, and (f) DMTCP (DMB) 100 times SEM.
(a)(b)(c)(d)(e)(f)Figures14(c) and 14(d) show the SEM images of DMTCP (carbon tetrachloride) xerogel at 500 and 7K magnification, respectively. At lower magnification, we can see that the surface of the gel is tight but wrinkled. At 7K magnification, however, we can see that DMTCP forms flat banded fiber bundles in carbon tetrachloride, and the amide bond structure in the molecular structure is one of the factors that promote the process of solvent gelation.Figures14(e) and 14(f) show the SEM images of gels formed by DMTCP in bromododecane and xylene, but the clear microstructure of xerogel cannot be seen. Reasons for this may include the following. First, it may be that because of the high boiling point of bromododecane and xylene, it is difficult to volatilize the solvent at room temperature. Hence, the method of solvent evaporation by high temperature heating was used. The high temperature makes the solvent outside the gel evaporate rapidly, however, which may lead to the rapid collapse and contraction of the gel structure. The xerogel therefore may have appeared to form a denser structure so that the microstructure could not be observed. Second, macroscopically, the transparent gels formed by them is relatively tight, and this may be because the structures themselves are closely connected. As a result, the microstructure could not be observed after drying and agglomeration.


### 3.4. Properties of Gelation

#### 3.4.1. Critical Gel Concentration (CGC) Test

The CGC test results show that the CGC of P2 in THF was 6‰ (w/v). Since DMTCP had good gelation behavior in diethyl ether, carbon tetrachloride, bromododecane, and xylene, the CGCs of these four kinds of gels were each tested. The final experiment showed that the CGCs of DMTCP in the four solvents were CGCether=10‰W/V, CGCcarbontetrachloride=6‰W/V, CGCbromododecane=2.5‰W/V, and CGCxylene=12‰W/V, and from this, we see that DMTCP had the lowest critical gel concentration in bromododecane.


#### 3.4.2. Thermal Stability Analysis of Gels

In our thermal stability analysis, we testedTgel in different concentrations of P2 in THF. Figure 15 shows that Tgel increased with the concentration of P2, and this indicates that the higher the gelator concentration, the tighter the gel accumulation and the better the thermal stability.Figure 15
P2 (THF) gel-sol phase transition temperature diagram.Due to the thermally reversible properties of the gels formed by DMTCP in the three organic solvents we tested, we tested the gel-sol phase transition temperature (Tgel) as well in different concentrations of DMTCP in carbon tetrachloride, bromododecane, and xylene, and the results are shown in Figure 16. Here, we see that Tgel increased with the concentration of DMTCP in all three organic solvents, and this also indicates that the higher the gel factor concentration, the closer the gel accumulation and the better the thermal stability.Figure 16
Gel-sol phase transition temperature diagram of DMTCP.


## 3.1. Gelation Behaviors of the Compounds

As we can see from Table9, P1 was insoluble in all tested solvents except pyridine, DMF, and DMSO (but was soluble under heating conditions in THF), showing a poor solubility among the gel solvents we tried. Because P1 could not be dissolved in so many solvents, the spatial network structure could not be formed. Hence, P1 could not be prepared as a gel with these solvents. However, in the solvents that could dissolve P1, it was completely dissociated in the solvent and the interaction between the solute and P1 was weak. As a result, the network structures necessary for preparing gels could not be formed.The solvent gelation experiments for P2 in 27 solvents showed that P2 only formed a gel in THF (Table10). Furthermore, there were two ways it could generate a gel. The first was that a gel could be formed after ultrasonic treatment at room temperature. The other was that a gel could be formed after heating and cooling without ultrasonic treatment. In addition, the gel formed with the latter method could return to its solution state after heating and violent shaking, but this gel could be formed again after heating and cooling.By comparing the polarity between solvents, we found that P2 exhibited a medium polarity. The P2 could dissolve in the solvents with a similar polarity to THF (4.2), such as xylene (2.5), dichloromethane (3.4), pyridine (5.3), DMF (6.4), and DMSO (7.2). This can be explained on the microscopic level: when the interaction between disperse phases that is weaker than that between disperse phase and dispersant, the P2 appears as a solution. Conversely, the dispersions can also aggregate to form precipitates.The results of the gelation test (Table11) indicate that DMTCP was insoluble in ethyl ether at room temperature and under heating conditions. However, in the concentration of 10‰ (w/v), the DMTCP was able to form an opaque gel after 20 seconds of ultrasonic processing (Figure 4). In other words, DMTCP (diethyl ether) gel had a special response to ultrasound. Unfortunately, the gel did not possess the property of thermal reversibility.Figure 4
Changes of DMTCP (diethyl ether) gel-sol.In contrast, DMTCP could dissolve in carbon tetrachloride, dodecane bromide, and xylene to form a clear solution under heating conditions. After ambient cooling, it could also form a transparent gel.Furthermore, the gels we tested that formed in carbon tetrachloride, dodecane bromide, and xylene had the same properties. They could be transformed from a solution into a gel by heating and cooling; they were thermally reversible. In addition, under the action of shear stress, they could be transformed from the gel state to the solution state, but could not be automatically transformed into a gel at room temperature. However, they were able to convert to gels after being heated and cooled, and this could be repeated several times (Figure5).Figure 5
Gel-sol transition diagram of DMTCP (CCl4, bromodecane, and xylene).


## 3.2. Spectroscopy

The infrared spectrum of compound 6-(2,2′:6′,2″-terpyridine-4′-formamide) hexanoic acid is shown in Figure 6, where we can see that the absorption peak at 3357 cm-1 is N-H stretching vibration absorption of the secondary amide. At 3064 cm-1, there is a wide peak center, which is the characteristic absorption peak of carboxylic acid, and at 1720 cm-1, the wide peak absorption indicates the existence of carboxylic acid. The absorption peaks at 2950 cm-1 and 2871 cm-1 are the stretching vibration absorption of saturated alkanes, and the peak at 1654 cm-1 is the stretching vibration absorption of the carbonyl group C=O, which also reflects the association absorption peak of the compound’s amide bond. The four peaks at 1583 cm-1, 1552 cm-1, 1533 cm-1, and 1469 cm-1 are the characteristic absorption of pyridine ring skeleton vibration. Hence, when we combined this analysis with our 1H NMR analysis, we determined the product to indeed be target product P1.Figure 6
Infrared spectra of 6-(2,2′:6′:2″-terpyridine-4′-formamide) hexanoic acid.From the structural analysis we conducted, we found that one end of P1 was terpyridine, which itself forms a large conjugated system but has poor solubility. The long chain of hexanoic acid at the other end and the long chain of carbon can reduce the polarity of the material, but the overall polarity of the material was higher. Thin layer chromatography also showed that only by increasing the amount of methanol in the developing agent can it be developed.As we can see from the comparison between P2 and P2-Gel in Figure7, after P2 formed the gel, two absorption peaks formed by the stretching vibration of the primary amine at 3485 cm-1 and 3413 cm-1 appear at 3398 cm-1 and 3338 cm-1, respectively. In addition, the peak became wider. Additionally, the stretching vibration absorption peaks of the carbonyl group in the ester group at 1745 cm-1 appear at 1735 cm-1. Under the influence of hydrogen bonds, these peaks move to the direction of the small wave numbers, which directly indicates the existence of hydrogen bonds in the formed gel. We conclude that the position of the hydrogen bonds in P2 should be between the primary amine group and the ester carbonyl group.Figure 7
Infrared contrast spectra of P2 and P2-Gel.Figure8 shows that the N-H stretching vibration absorption peak in the amide bond located at 3292 cm-1 moved 2 units to the direction of the low wave numbers after the formation of the gel and that the C=O stretching vibration absorption peak of the amide bond at 1652 cm-1 moved to 1650 cm-1 in the xerogel. The bending vibration peak of N-H in the amide bond at 1539 cm-1 stayed the same. Moreover, the C=O stretching vibration peak of the ester group at 1741 cm-1 moved to 1743 cm-1, which is an abnormal move to the direction of higher wave numbers. According to the above data, DMTCP may form a weak hydrogen bond in diethyl ether.Figure 8
Infrared comparison between DMTCP (ether) xerogel and DMTCP.In Figure9, we see that after gel formation in CCl4, the N-H stretching vibration absorption peak of the amide bond at 3292 cm-1 moved toward the low wave numbers, at 3291 cm-1, with a slight red shift, and that the C=O stretching vibration absorption peak at 1652 cm-1 in the amide bond moved to 1647 cm-1 in the xerogel. That is, it moved 5 units towards the lower wave numbers. The N-H bending vibration peak in the amide bond at 1539 cm-1 moved to the higher wave numbers and reached 1543 cm-1. This shows that hydrogen bonds were formed between the amide bonds.Figure 9
Infrared comparison between DMTCP(CCl4) xerogel and DMTCP.Figure10 shows that the N-H stretching vibration absorption peak of the amide bond at 3292 cm-1 moved to the lower wave numbers to the point at 3282 cm-1 after the gel was formed in xylene (red shift). The C=O stretching vibration absorption peak at 1652 cm-1 in the amide bond moved to 1644 cm-1 in the xerogel. In other words, it moved 8 units towards the lower wave numbers. Additionally, the N-H bending vibration peak in the amide bond at 1539 cm-1 moved toward the higher wave numbers and reached 1544 cm-1. This shows that hydrogen bonds were formed between the amide bonds, as in Figure 9.Figure 10
Infrared comparison between DMTCP (xylene) xerogel and DMTCP.


## 3.3. Morphology

The macroscopic characteristics of the gel formed by P2 are shown in Figure11. As can be seen from the figure, it was an opaque gel in the THF solvent, with an obvious solvent gelation effect. There also were no free solvent flows after inversion.Figure 11
Macroscopic view of P2 forming a gel in THF.The microcosmic characteristics of the gel are shown in Figure12. From the scanning electron microscopy (SEM) images of the P2-Gel at 400 times (Figure 12(a)) and 1000 times (Figure 12(b)) magnification, we can see that P2 formed a fibrous gelatinous structure in the THF solvent. Based on the hydrogen bond formation mechanism of the P2-Gel mentioned above, we can further infer that the hydrogen bond between primary amines formed the ester carbonyl group. The promoted fibers between P2 molecules formed a three-dimensional network structure and bound with the THF solvent to form a gel.Figure 12
SEM image of P2 xerogel (THF) at 400 times (a) and 1000 times (b) magnification.
(a)(b)The macroscopic characteristic diagram of the gel formed by DMTCP in different organic solvents is shown in Figure13.Figure 13
Macroscopic morphology of DMTCP gel formed in four solvents: (a) diethyl ether, (b) carbon tetrachloride, (c) bromododecane, and (d) xylene.
(a)(b)(c)(d)As we can see from Figures14(a) and 14(b), DMTCP formed a densely interlaced and extremely fine fibrous structure in diethyl ether that was also very disorderly. This is consistent with the appearance of the opaque gel that DMTCP formed under ultrasonic in diethyl ether as well, and we speculate that DMTCP molecules stack themselves through hydrogen bonding under intense ultrasonic vibration. In addition, the intermolecular interactions between ether and DMTCP are balanced. That is, the intermolecular interactions between solute and solvent are balanced, and these balanced intermolecular interactions prevent DMTCP from forming its own excessive agglomeration to form precipitation and from sufficient dispersion in ether to establish a spatial network. Therefore, DMTCP has ultrasonic response characteristics in ethyl ether and forms an opaque gel, which is the macroscopic representation of the balanced intermolecular interactions between the dispersed substance and the dispersant.Figure 14
(a) 600-fold SEM diagram of DMTCP (ethyl ether), (b) 1.5K SEM diagram of DMTCP (ethyl ether), (c) DMTCP (CCl4) 500 times SEM, (d) DMTCP (CCl4) 7K times SEM, (e) DMTCP(CH3(CH2)11Br) 300 times SEM, and (f) DMTCP (DMB) 100 times SEM.
(a)(b)(c)(d)(e)(f)Figures14(c) and 14(d) show the SEM images of DMTCP (carbon tetrachloride) xerogel at 500 and 7K magnification, respectively. At lower magnification, we can see that the surface of the gel is tight but wrinkled. At 7K magnification, however, we can see that DMTCP forms flat banded fiber bundles in carbon tetrachloride, and the amide bond structure in the molecular structure is one of the factors that promote the process of solvent gelation.Figures14(e) and 14(f) show the SEM images of gels formed by DMTCP in bromododecane and xylene, but the clear microstructure of xerogel cannot be seen. Reasons for this may include the following. First, it may be that because of the high boiling point of bromododecane and xylene, it is difficult to volatilize the solvent at room temperature. Hence, the method of solvent evaporation by high temperature heating was used. The high temperature makes the solvent outside the gel evaporate rapidly, however, which may lead to the rapid collapse and contraction of the gel structure. The xerogel therefore may have appeared to form a denser structure so that the microstructure could not be observed. Second, macroscopically, the transparent gels formed by them is relatively tight, and this may be because the structures themselves are closely connected. As a result, the microstructure could not be observed after drying and agglomeration.


## 3.4. Properties of Gelation

### 3.4.1. Critical Gel Concentration (CGC) Test

The CGC test results show that the CGC of P2 in THF was 6‰ (w/v). Since DMTCP had good gelation behavior in diethyl ether, carbon tetrachloride, bromododecane, and xylene, the CGCs of these four kinds of gels were each tested. The final experiment showed that the CGCs of DMTCP in the four solvents were CGCether=10‰W/V, CGCcarbontetrachloride=6‰W/V, CGCbromododecane=2.5‰W/V, and CGCxylene=12‰W/V, and from this, we see that DMTCP had the lowest critical gel concentration in bromododecane.


### 3.4.2. Thermal Stability Analysis of Gels

In our thermal stability analysis, we testedTgel in different concentrations of P2 in THF. Figure 15 shows that Tgel increased with the concentration of P2, and this indicates that the higher the gelator concentration, the tighter the gel accumulation and the better the thermal stability.Figure 15
P2 (THF) gel-sol phase transition temperature diagram.Due to the thermally reversible properties of the gels formed by DMTCP in the three organic solvents we tested, we tested the gel-sol phase transition temperature (Tgel) as well in different concentrations of DMTCP in carbon tetrachloride, bromododecane, and xylene, and the results are shown in Figure 16. Here, we see that Tgel increased with the concentration of DMTCP in all three organic solvents, and this also indicates that the higher the gel factor concentration, the closer the gel accumulation and the better the thermal stability.Figure 16
Gel-sol phase transition temperature diagram of DMTCP.


## 3.4.1. Critical Gel Concentration (CGC) Test

The CGC test results show that the CGC of P2 in THF was 6‰ (w/v). Since DMTCP had good gelation behavior in diethyl ether, carbon tetrachloride, bromododecane, and xylene, the CGCs of these four kinds of gels were each tested. The final experiment showed that the CGCs of DMTCP in the four solvents were CGCether=10‰W/V, CGCcarbontetrachloride=6‰W/V, CGCbromododecane=2.5‰W/V, and CGCxylene=12‰W/V, and from this, we see that DMTCP had the lowest critical gel concentration in bromododecane.


## 3.4.2. Thermal Stability Analysis of Gels

In our thermal stability analysis, we testedTgel in different concentrations of P2 in THF. Figure 15 shows that Tgel increased with the concentration of P2, and this indicates that the higher the gelator concentration, the tighter the gel accumulation and the better the thermal stability.Figure 15
P2 (THF) gel-sol phase transition temperature diagram.Due to the thermally reversible properties of the gels formed by DMTCP in the three organic solvents we tested, we tested the gel-sol phase transition temperature (Tgel) as well in different concentrations of DMTCP in carbon tetrachloride, bromododecane, and xylene, and the results are shown in Figure 16. Here, we see that Tgel increased with the concentration of DMTCP in all three organic solvents, and this also indicates that the higher the gel factor concentration, the closer the gel accumulation and the better the thermal stability.Figure 16
Gel-sol phase transition temperature diagram of DMTCP.


## 4. Conclusions

We designed and synthesized three LMMGs, named 6-(2,2′:6′,2″,-terpyridine-4′-formylamino) hexanoic acid (P1), glycine cholesterol ester (P2), and DMTCP, for this paper and conducted infrared spectroscopy, nuclear magnetic resonance spectroscopy, mass spectrometry, elemental analysis, and gelation performance tests on each of them. Our conclusions are as follows. First, glycine cholesterol ester (P2) was able to form opaque gels in the THF solution that could be transformed into a solution under the action of heat and shear stress. The P2 also had thermal reversibility and could form gels repeatedly. Additionally, based on infrared spectrum and SEM image analysis, hydrogen bonds are the main driving force for the formation of gelator clusters. Pang et al. [31] have also mentioned that directional hydrogen bonding is helpful to the formation of aggregates.Second, DMTCP, synthesized from P1 and P2, could gelate the solvents diethyl ether, carbon tetrachloride, xylene, and bromododecane. Compared to P2 and P1, DMTCP not only introduced the terpyridine functional group into the cholesterol group but also significantly improved gelation. The gelators in the four solvents were stimulus responsive and achieved the desired effects as well. Third, the infrared spectrum analysis of each xerogel formed by DMTCP showed that the hydrogen bonds were still the main driving force of gelator formation, and the SEM image analysis of gelators formed by the four solvents showed that the micromorphology of each of the gelators formed by the same gelata in different solvents was also different.The gel formed by DMTCP not only provided a very stable structure for binding metal ions but also contained cholesterol groups with good biofilm compatibility. Currently, ruthenium complexes of terpyridine have been used in gene therapy [32], and the gel formed by the complexation of the terpyridine group and other metal ions may well advance the study of drug release. In addition, the biofilm compatibility provided by cholesterol gives DMTCP potential research significance in the directional supply of metal ions.



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*Source: 3695462-2022-06-16.xml*