4,6-O-Phenylethylidene Acetal Protected D-Glucosamine Carbamate-Based Gelators and Their Applications for Multi-Component Gels

The self-assembly of carbohydrate-based low molecular weight gelators has led to useful advanced soft materials. The interactions of the gelators with various cations and anions are important in creating novel molecular architectures and expanding the scope of the small molecular gelators. In this study, a series of thirteen new C-2 carbamates of the 4,6-O-phenylethylidene acetal-protected D-glucosamine derivatives has been synthesized and characterized. These compounds are rationally designed from a common sugar template. All carbamates synthesized were found to be efficient gelators and three compounds are also hydrogelators. The resulting gels were characterized using optical microscopy, atomic force microscopy, and rheology. The gelation mechanisms were further elucidated using 1H NMR spectroscopy at different temperatures. The isopropyl carbamate hydrogelator 7 formed hydrogels at 0.2 wt% and also formed gels with several tetra alkyl ammonium salts, and showed effectiveness in the creation of gel electrolytes. The formation of metallogels using earth-abundant metal ions such as copper, nickel, iron, zinc, as well as silver and lead salts was evaluated for a few gelators. Using chemiluminescence spectroscopy, the metal–organic xerogels showed enzyme-like properties and enhanced luminescence for luminol. In addition, we also studied the applications of several gels for drug immobilizations and the gels showed sustained release of naproxen from the gel matrices. This robust sugar carbamate-derived gelator system can be used as the scaffold for the design of other functional materials with various types of applications.


Introduction
Low molecular weight gelators (LMWGs) have gained much attention due to their versatile applications in the preparation of novel functional soft materials [1][2][3][4][5]. These materials have demonstrated potential in biomedical applications, pollutant removal, and optoelectronic devices, and for catalysis [4, [6][7][8][9][10][11]. Various structural features have been carefully analyzed over the years in order to rationally design effective low molecular weight gelators [11,12]. Among the many classes of organic compounds used as the template for gelators, carbohydrates have emerged as interesting molecules for the preparation of these advanced materials due to their natural abundance, biocompatibility, and intrinsic chirality, which opens avenues for their desired modification [2,3]. The driving forces governing the formation of self-assembled networks by LMWGs are non-covalent in nature, such as hydrophobic interactions, hydrogen bonding, π-π, and CH-π interactions. Previously, various urea, amide, and carbamate derivatives of N-acetyl-D-glucosamine were synthesized, and their gelation properties were analyzed [13][14][15][16]. A variety of amides and ureas derived from 4,6-O-benzylidene acetal-protected D-glucosamine-formed gels in aqueous mixtures of ethanol and DMSO [13], and several amides were able to form gels for pump oil and engine oil [14]. Carbamate derivatives of 4,6-O-benzylidene acetal-protected Besides forming gels in organic solvents or in water, the formation of multiple component gels using these gelators for ionic liquids and electrolytes allows for their use as semiconductors and capacitors for energy and battery applications [18][19][20]. Gelators that have a response towards different anions are also reported and these have potential for practical applications in enzyme mimics and catalysis [21]. Gels formed in the presence of electrolytes such as tetrabutyl ammonium salts of halides may be useful as functional materials, such as gel electrolytes and for conductive media [22]. Similarly, ionogels can be useful for lithium ion batteries and other materials [23]. The formation of gel electrolytes from a sugar derivative is especially interesting since the materials will be more biocompatible.
Multiple component gels formed in the presence of metal ions, which are also called metallogels, have drawn an increasing amount of attention from researchers recently [20,[24][25][26][27]. The introduction of metal ions to the gel matrix increases additional functions and can lead to materials that are therapeutic, conductive, and magnetic. Metallogels also showed to undergo catalytic reactions due to the redox activity of the metal ions trapped within the gel matrix [17,28,29]. For instance, a copper metal-organic hydrogel was used as a heterogeneous catalyst for the reaction of SO2 and CO2 with epoxides to produce cyclic 1,3,2-dioxathiolane-2 oxides and carbonates [30]. A recent multi-responsive silver organic gel has been prepared and showed responses towards light and chemicals [31]. Copperbased metal-organic gels (Cu-MOG) have been converted to a Cu-based metal-organic porous network (Cu-MOPN) with intrinsic oxidase and peroxidase-mimicking activities [32], and they are used as nanozymes for the colorimetry detection of dopamine [33]. A bimetallic copper(II)/cobalt(II) organic gel showed enhanced peroxidase-like activity and was applied for fluorescent detection of glucose [34].
Chemiluminescence (CL) is a unique phenomenon when light is emitted in response to a chemical reaction. Luminol-based CL is a powerful analytical method for reporting or detecting various analytes including hydrogen sulfide [35]. In a recent report, a metalorganic xerogel (MOX) was found to exhibit peroxidase activity to catalyze chemiluminescence of luminol, which was further used for dopamine detection [36,37]. A few recent reports have demonstrated the use of metal-organic gels (MOG) or metalorganic frameworks as enzyme mimics for CL systems [36,[38][39][40]. An iron-based metal- Besides forming gels in organic solvents or in water, the formation of multiple component gels using these gelators for ionic liquids and electrolytes allows for their use as semiconductors and capacitors for energy and battery applications [18][19][20]. Gelators that have a response towards different anions are also reported and these have potential for practical applications in enzyme mimics and catalysis [21]. Gels formed in the presence of electrolytes such as tetrabutyl ammonium salts of halides may be useful as functional materials, such as gel electrolytes and for conductive media [22]. Similarly, ionogels can be useful for lithium ion batteries and other materials [23]. The formation of gel electrolytes from a sugar derivative is especially interesting since the materials will be more biocompatible.
Multiple component gels formed in the presence of metal ions, which are also called metallogels, have drawn an increasing amount of attention from researchers recently [20,[24][25][26][27]. The introduction of metal ions to the gel matrix increases additional functions and can lead to materials that are therapeutic, conductive, and magnetic. Metallogels also showed to undergo catalytic reactions due to the redox activity of the metal ions trapped within the gel matrix [17,28,29]. For instance, a copper metal-organic hydrogel was used as a heterogeneous catalyst for the reaction of SO 2 and CO 2 with epoxides to produce cyclic 1,3,2dioxathiolane-2 oxides and carbonates [30]. A recent multi-responsive silver organic gel has been prepared and showed responses towards light and chemicals [31]. Copper-based metal-organic gels (Cu-MOG) have been converted to a Cu-based metal-organic porous network (Cu-MOPN) with intrinsic oxidase and peroxidase-mimicking activities [32], and they are used as nanozymes for the colorimetry detection of dopamine [33]. A bimetallic copper(II)/cobalt(II) organic gel showed enhanced peroxidase-like activity and was applied for fluorescent detection of glucose [34].
Chemiluminescence (CL) is a unique phenomenon when light is emitted in response to a chemical reaction. Luminol-based CL is a powerful analytical method for reporting or detecting various analytes including hydrogen sulfide [35]. In a recent report, a metal-organic xerogel (MOX) was found to exhibit peroxidase activity to catalyze chemiluminescence of luminol, which was further used for dopamine detection [36,37]. A few recent reports have demonstrated the use of metal-organic gels (MOG) or metal-organic frameworks as enzyme mimics for CL systems [36,[38][39][40]. An iron-based metal-organic gel showed enzyme-mimicking activities and was able to detect H 2 O 2 released from Hela cells using luminol chemiluminescence [41].
Formation of multi-component gels will expand the scope of usefulness of LMWGs and because of the importance of metallogels and conductive gels, we are interested in designing and preparing novel self-assembled gels with these desired properties. To further expand the versatile gelation properties from sugar templates, in this study, we synthesized from Hela cells using luminol chemiluminescence [41].
Formation of multi-component gels will expand the scope of usefulness of LMWGs and because of the importance of metallogels and conductive gels, we are interested in designing and preparing novel self-assembled gels with these desired properties. To further expand the versatile gelation properties from sugar templates, in this study, we synthesized a set of thirteen carbamate derivatives and analyzed their gelation properties in various solvents, and with an emphasis of finding effective gelators for metal ions and electrolytes.

Results and Discussion
The synthesis of the carbamates is shown in Scheme 1. The glucosamine derivative 1 was synthesized in a few steps from N-acetyl-D-glucosamine according to literature procedures [14]. This intermediate was reacted with a series of commercially available chloroformates to afford N-linked carbamate derivatives 2-14. We selected short-chain alkyl substituents (2)(3)(4)(5)(6) and branched derivatives (7)(8)(9), as well as aromatic derivatives (10)(11)(12)(13)(14). Compound 14 contains the F-MOC functional group, which often leads to good gelation performance. These carbamates were tested in a panel of solvents ranging from non-polar organic solvents such as hexane to polar solvents such as alcohols and aqueous mixtures of ethanol and dimethyl sulfoxide. Additionally, the compounds were also tested for their ability to form hydrogels as well as gelling pump oil. As shown in Table 1, compounds 2-14 displayed impressive gelation ability. The best performing solvent is glycerol and all compounds formed stable gels. Many compounds also formed gels in ethylene glycol, vacuum pump oil, and aqueous mixtures of organic solvents. These compounds did not form gels in ethanol and isopropanol. Scheme 1. Synthesis of carbamate derivatives with general structure IV. Table 1, compounds with linear aliphatic chains such as 5 and 6 formed gels in hexanes at 5.0 mg/mL and they also formed gels in six and seven other selected solvents. The branched alkyl derivatives 7 and 8 formed hydrogels at 2.0 and 10.0 mg/mL, respectively. Interestingly, the trichloro derivative compound 9 and the phenyl carbamate 10 were not able to gelate many solvents and they only formed gels in two solvents. However, benzyl and substituted benzyl derivatives 11 and 12 performed much better, forming gels in eight and seven solvents, respectively. The benzyl derivative 11 also formed a hydrogel at 0.4 wt% and the nitrobenzyl carbamate 12 showed great gelation ability by forming gels in aqueous mixtures of DMSO and ethanol at low concentrations. It formed a gel at 1.8 mg/mL in DMSO:H2O (1:2) and 2.8 mg/mL in EtOH:H2O (1:2). A similar reduction trend was observed with the chloro-phenyl derivative 13; it became a Scheme 1. Synthesis of carbamate derivatives with general structure IV. Table 1, compounds with linear aliphatic chains such as 5 and 6 formed gels in hexanes at 5.0 mg/mL and they also formed gels in six and seven other selected solvents. The branched alkyl derivatives 7 and 8 formed hydrogels at 2.0 and 10.0 mg/mL, respectively. Interestingly, the trichloro derivative compound 9 and the phenyl carbamate 10 were not able to gelate many solvents and they only formed gels in two solvents. However, benzyl and substituted benzyl derivatives 11 and 12 performed much better, forming gels in eight and seven solvents, respectively. The benzyl derivative 11 also formed a hydrogel at 0.4 wt% and the nitrobenzyl carbamate 12 showed great gelation ability by forming gels in aqueous mixtures of DMSO and ethanol at low concentrations. It formed a gel at 1.8 mg/mL in DMSO:H 2 O (1:2) and 2.8 mg/mL in EtOH:H 2 O (1:2). A similar reduction trend was observed with the chloro-phenyl derivative 13; it became a less effective gelator and only formed gels in three solvents. The F-MOC derivative, on the other hand, was able to gelate several solvents. A majority of the gels appeared opaque and some were translucent. The representative gel photos are shown in Figure 2. less effective gelator and only formed gels in three solvents. The F-MOC derivative, on the other hand, was able to gelate several solvents. A majority of the gels appeared opaque and some were translucent. The representative gel photos are shown in Figure 2. less effective gelator and only formed gels in three solvents. The F-MOC derivative, on the other hand, was able to gelate several solvents. A majority of the gels appeared opaque and some were translucent. The representative gel photos are shown in Figure 2. To compare the gelation performance of derivatives IV from this study with the general structures I reported before [14], a few examples in the same solvents are shown in Table 2. Compound IV-a formed more effective gels in EtOH:H2O (v/v 1:2) and DMSO:H2O (v/v 1:2) at concentrations of 6.7 and 4.0 mg/mL in comparison to compound less effective gelator and only formed gels in three solvents. The F-MOC derivative, on the other hand, was able to gelate several solvents. A majority of the gels appeared opaque and some were translucent. The representative gel photos are shown in Figure 2. To compare the gelation performance of derivatives IV from this study with the general structures I reported before [14], a few examples in the same solvents are shown in Table 2. Compound IV-a formed more effective gels in EtOH:H2O (v/v 1:2) and DMSO:H2O (v/v 1:2) at concentrations of 6.7 and 4.0 mg/mL in comparison to compound less effective gelator and only formed gels in three solvents. The F-MOC derivative, on the other hand, was able to gelate several solvents. A majority of the gels appeared opaque and some were translucent. The representative gel photos are shown in Figure 2.  To compare the gelation performance of derivatives IV from this study with the general structures I reported before [14], a few examples in the same solvents are shown in Table 2. Compound IV-a formed more effective gels in EtOH:H2O (v/v 1:2) and DMSO:H2O (v/v 1:2) at concentrations of 6.7 and 4.0 mg/mL in comparison to compound less effective gelator and only formed gels in three solvents. The F-MOC derivative, on the other hand, was able to gelate several solvents. A majority of the gels appeared opaque and some were translucent. The representative gel photos are shown in Figure 2.  To compare the gelation performance of derivatives IV from this study with the general structures I reported before [14], a few examples in the same solvents are shown in Table 2. Compound IV-a formed more effective gels in EtOH:H2O (v/v 1:2) and DMSO:H2O (v/v 1:2) at concentrations of 6.7 and 4.0 mg/mL in comparison to compound less effective gelator and only formed gels in three solvents. The F-MOC derivative, on the other hand, was able to gelate several solvents. A majority of the gels appeared opaque and some were translucent. The representative gel photos are shown in Figure 2.

As shown in
0T I All compounds were tested starting from 20.0 mg/mL. UG, unstable gel at room temperature and the numbers are concentrations in mg/mL; G, stable gel at room temperature and the numbers are MGC in mg/mL; P, precipitation; S, soluble; and I, insoluble. Gel appearance: C for clear or transparent; T, translucent; and O, opaque. Compounds 5 and 6 formed opaque gels in hexane at 5.0 mg/mL, while 4 and 8 formed precipitate, and all others were insoluble in hexane. The ratios for all mixed solvents are volume ratios. To compare the gelation performance of derivatives IV from this study with the general structures I reported before [14], a few examples in the same solvents are shown in Table 2. Compound IV-a formed more effective gels in EtOH:H2O (v/v 1:2) and DMSO:H2O (v/v 1:2) at concentrations of 6.7 and 4.0 mg/mL in comparison to compound P UG 6.7 T G10.0 C S P P P P I less effective gelator and only formed gels in three solvents. The F-MOC derivative, on the other hand, was able to gelate several solvents. A majority of the gels appeared opaque and some were translucent. The representative gel photos are shown in Figure 2.
0T I All compounds were tested starting from 20.0 mg/mL. UG, unstable gel at room temperature and the numbers are concentrations in mg/mL; G, stable gel at room temperature and the numbers are MGC in mg/mL; P, precipitation; S, soluble; and I, insoluble. Gel appearance: C for clear or transparent; T, translucent; and O, opaque. Compounds 5 and 6 formed opaque gels in hexane at 5.0 mg/mL, while 4 and 8 formed precipitate, and all others were insoluble in hexane. The ratios for all mixed solvents are volume ratios. To compare the gelation performance of derivatives IV from this study with the general structures I reported before [14], a few examples in the same solvents are shown in Table 2. Compound IV-a formed more effective gels in EtOH:H2O (v/v 1:2) and DMSO:H2O (v/v 1:2) at concentrations of 6.7 and 4.0 mg/mL in comparison to compound less effective gelator and only formed gels in three solvents. The F-MOC derivative, on the other hand, was able to gelate several solvents. A majority of the gels appeared opaque and some were translucent. The representative gel photos are shown in Figure 2.
0T I All compounds were tested starting from 20.0 mg/mL. UG, unstable gel at room temperature and the numbers are concentrations in mg/mL; G, stable gel at room temperature and the numbers are MGC in mg/mL; P, precipitation; S, soluble; and I, insoluble. Gel appearance: C for clear or transparent; T, translucent; and O, opaque. Compounds 5 and 6 formed opaque gels in hexane at 5.0 mg/mL, while 4 and 8 formed precipitate, and all others were insoluble in hexane. The ratios for all mixed solvents are volume ratios. To compare the gelation performance of derivatives IV from this study with the general structures I reported before [14], a few examples in the same solvents are shown in Table 2. Compound IV-a formed more effective gels in EtOH:H2O (v/v 1:2) and DMSO:H2O (v/v 1:2) at concentrations of 6.7 and 4.0 mg/mL in comparison to compound less effective gelator and only formed gels in three solvents. The F-MOC derivative, on the other hand, was able to gelate several solvents. A majority of the gels appeared opaque and some were translucent. The representative gel photos are shown in Figure 2.
0T I All compounds were tested starting from 20.0 mg/mL. UG, unstable gel at room temperature and the numbers are concentrations in mg/mL; G, stable gel at room temperature and the numbers are MGC in mg/mL; P, precipitation; S, soluble; and I, insoluble. Gel appearance: C for clear or transparent; T, translucent; and O, opaque. Compounds 5 and 6 formed opaque gels in hexane at 5.0 mg/mL, while 4 and 8 formed precipitate, and all others were insoluble in hexane. The ratios for all mixed solvents are volume ratios. To compare the gelation performance of derivatives IV from this study with the general structures I reported before [14], a few examples in the same solvents are shown in Table 2. Compound IV-a formed more effective gels in EtOH:H2O (v/v 1:2) and DMSO:H2O (v/v 1:2) at concentrations of 6.7 and 4.0 mg/mL in comparison to compound less effective gelator and only formed gels in three solvents. The F-MOC derivative, on the other hand, was able to gelate several solvents. A majority of the gels appeared opaque and some were translucent. The representative gel photos are shown in Figure 2.
0T I All compounds were tested starting from 20.0 mg/mL. UG, unstable gel at room temperature and the numbers are concentrations in mg/mL; G, stable gel at room temperature and the numbers are MGC in mg/mL; P, precipitation; S, soluble; and I, insoluble. Gel appearance: C for clear or transparent; T, translucent; and O, opaque. Compounds 5 and 6 formed opaque gels in hexane at 5.0 mg/mL, while 4 and 8 formed precipitate, and all others were insoluble in hexane. The ratios for all mixed solvents are volume ratios. To compare the gelation performance of derivatives IV from this study with the general structures I reported before [14], a few examples in the same solvents are shown in Table 2. Compound IV-a formed more effective gels in EtOH:H2O (v/v 1:2) and DMSO:H2O (v/v 1:2) at concentrations of 6.7 and 4.0 mg/mL in comparison to compound All compounds were tested starting from 20.0 mg/mL. UG, unstable gel at room tem the numbers are concentrations in mg/mL; G, stable gel at room temperature and th MGC in mg/mL; P, precipitation; S, soluble; and I, insoluble. Gel appearance: C for transparent; T, translucent; and O, opaque. Compounds 5 and 6 formed opaque gel 5.0 mg/mL, while 4 and 8 formed precipitate, and all others were insoluble in hexan for all mixed solvents are volume ratios. To compare the gelation performance of derivatives IV from this s general structures I reported before [14], a few examples in the same solve in Table 2. Compound IV-a formed more effective gels in EtOH:H2O To compare the gelation performance of derivatives IV from this study with the general structures I reported before [14], a few examples in the same solvents are shown in Table 2. Compound IV-a formed more effective gels in EtOH:H 2 O (v/v 1:2) and DMSO:H 2 O (v/v 1:2) at concentrations of 6.7 and 4.0 mg/mL in comparison to compound I-a, which formed gels at 10.0 mg/mL in these solvent systems. However, the isobutyl derivative IV-b and I-b showed similar gelation tendencies, with the benzylidene derivative performed at lower concentrations in water and DMSO:H 2 O (v/v 1:2). With the benzyl carbamates, the gelation ability improved significantly for compound IV-c; it formed gels at lower concentrations at 3.3 mg/mL in EtOH:H 2 O (v/v 1:2) and 6.7 mg/mL in DMSO:H 2 O (v/v 1:2), and even formed a hydrogel at 4.0 mg/mL as compared to I-c, which did not form a hydrogel. The gelation properties of these carbamate derivatives showed overall enhancement possibly due to the increased hydrophobic methylene group "insertion" in the 4,6-protecting group. The calculated CLogP values for the butyl derivative I-a is 1.66 and 2.03 for compound 5, which reflects the increased hydrophobicity of the benzyl derivative. I-a, which formed gels at 10.0 mg/mL in these solvent systems. However, the isobutyl derivative IV-b and I-b showed similar gelation tendencies, with the benzylidene derivative performed at lower concentrations in water and DMSO:H2O (v/v 1:2). With the benzyl carbamates, the gelation ability improved significantly for compound IV-c; it formed gels at lower concentrations at 3.3 mg/mL in EtOH:H2O (v/v 1:2) and 6.7 mg/mL in DMSO:H2O (v/v 1:2), and even formed a hydrogel at 4.0 mg/mL as compared to I-c, which did not form a hydrogel. The gelation properties of these carbamate derivatives showed overall enhancement possibly due to the increased hydrophobic methylene group "insertion" in the 4,6-protecting group. The calculated CLogP values for the butyl derivative I-a is 1.66 and 2.03 for compound 5, which reflects the increased hydrophobicity of the benzyl derivative.

Gelation Mechanism by 1 H NMR Studies
In order to probe the inter/intramolecular interactions, we carried out the 1 H NMR experiment at different temperatures with compound 8 in DMSO-d6 ( Figure 3). The full range 1 H NMR overlaid spectra are shown in ESI Figure S1. As shown in previous studies for a similar system [14], typically both the -NH and O-H functional groups potentially participate in H-bonding. The carbamate NH signal of compound 8 showed a significant upfield shift from δ 6.88 to 6.68 ppm, corresponding to 30 °C and 60 °C, respectively. Similarly, the 3-hydroxyl group showed an upfield shift of 0.16 ppm from 5.05 to 4.89 ppm. These indicated the importance of hydrogen bonding from the carbamate NH and 3-OH groups intermolecularly. Interestingly, we also observed a slight downfield shift in the anomeric proton from δ 4.61 to 4. 63 ppm. Although the gelation mechanism varies with solvents, it is obvious that both the 2-NH and 3-OH functional groups play important roles in the gelation process. In comparison to the urea derivative 21 reported previously [14], the 3-OH also had a 0. 16  I-a, which formed gels at 10.0 mg/mL in these solvent systems. However, the isobutyl derivative IV-b and I-b showed similar gelation tendencies, with the benzylidene derivative performed at lower concentrations in water and DMSO:H2O (v/v 1:2). With the benzyl carbamates, the gelation ability improved significantly for compound IV-c; it formed gels at lower concentrations at 3.3 mg/mL in EtOH:H2O (v/v 1:2) and 6.7 mg/mL in DMSO:H2O (v/v 1:2), and even formed a hydrogel at 4.0 mg/mL as compared to I-c, which did not form a hydrogel. The gelation properties of these carbamate derivatives showed overall enhancement possibly due to the increased hydrophobic methylene group "insertion" in the 4,6-protecting group. The calculated CLogP values for the butyl derivative I-a is 1.66 and 2.03 for compound 5, which reflects the increased hydrophobicity of the benzyl derivative.

Gelation Mechanism by 1 H NMR Studies
In order to probe the inter/intramolecular interactions, we carried out the 1 H NMR experiment at different temperatures with compound 8 in DMSO-d6 ( Figure 3). The full range 1 H NMR overlaid spectra are shown in ESI Figure S1. As shown in previous studies for a similar system [14], typically both the -NH and O-H functional groups potentially participate in H-bonding. The carbamate NH signal of compound 8 showed a significant upfield shift from δ 6.88 to 6.68 ppm, corresponding to 30 °C and 60 °C, respectively. Similarly, the 3-hydroxyl group showed an upfield shift of 0.16 ppm from 5.05 to 4.89 ppm. These indicated the importance of hydrogen bonding from the carbamate NH and 3-OH groups intermolecularly. Interestingly, we also observed a slight downfield shift in the anomeric proton from δ 4.61 to 4. 63 ppm. Although the gelation mechanism varies with solvents, it is obvious that both the 2-NH and 3-OH functional groups play important roles in the gelation process. In comparison to the urea derivative 21 reported previously [14], the 3-OH also had a 0.16 ppm shift from δ 5.09 (30 °C ) to 4.93 (60 °C ) ppm. The urea's 2-NH signal, however, showed a smaller chemical shift change of 0.07 ppm from 30 °C to 60 °C. This indicates that that the carbamate functional group played more important role during the gelation process since it offers both hydrogen bonding donating and accepting properties. I-a, which formed gels at 10.0 mg/mL in these solvent systems. However, the isobutyl derivative IV-b and I-b showed similar gelation tendencies, with the benzylidene derivative performed at lower concentrations in water and DMSO:H2O (v/v 1:2). With the benzyl carbamates, the gelation ability improved significantly for compound IV-c; it formed gels at lower concentrations at 3.3 mg/mL in EtOH:H2O (v/v 1:2) and 6.7 mg/mL in DMSO:H2O (v/v 1:2), and even formed a hydrogel at 4.0 mg/mL as compared to I-c, which did not form a hydrogel. The gelation properties of these carbamate derivatives showed overall enhancement possibly due to the increased hydrophobic methylene group "insertion" in the 4,6-protecting group. The calculated CLogP values for the butyl derivative I-a is 1.66 and 2.03 for compound 5, which reflects the increased hydrophobicity of the benzyl derivative.

Gelation Mechanism by 1 H NMR Studies
In order to probe the inter/intramolecular interactions, we carried out the 1 H NMR experiment at different temperatures with compound 8 in DMSO-d6 ( Figure 3). The full range 1 H NMR overlaid spectra are shown in ESI Figure S1. As shown in previous studies for a similar system [14], typically both the -NH and O-H functional groups potentially participate in H-bonding. The carbamate NH signal of compound 8 showed a significant upfield shift from δ 6.88 to 6.68 ppm, corresponding to 30 °C and 60 °C, respectively. Similarly, the 3-hydroxyl group showed an upfield shift of 0.16 ppm from 5.05 to 4.89 ppm. These indicated the importance of hydrogen bonding from the carbamate NH and 3-OH groups intermolecularly. Interestingly, we also observed a slight downfield shift in the anomeric proton from δ 4.61 to 4. 63 ppm. Although the gelation mechanism varies with solvents, it is obvious that both the 2-NH and 3-OH functional groups play important roles in the gelation process. In comparison to the urea derivative 21 reported previously [14], the 3-OH also had a 0.16 ppm shift from δ 5.09 (30 °C ) to 4.93 (60 °C ) ppm. The urea's 2-NH signal, however, showed a smaller chemical shift change of 0.07 ppm from 30 °C to 60 °C. This indicates that that the carbamate functional group played more important role during the gelation process since it offers both hydrogen bonding donating and accepting properties. I-a, which formed gels at 10.0 mg/mL in these solvent systems. However, the isobutyl derivative IV-b and I-b showed similar gelation tendencies, with the benzylidene derivative performed at lower concentrations in water and DMSO:H2O (v/v 1:2). With the benzyl carbamates, the gelation ability improved significantly for compound IV-c; it formed gels at lower concentrations at 3.3 mg/mL in EtOH:H2O (v/v 1:2) and 6.7 mg/mL in DMSO:H2O (v/v 1:2), and even formed a hydrogel at 4.0 mg/mL as compared to I-c, which did not form a hydrogel. The gelation properties of these carbamate derivatives showed overall enhancement possibly due to the increased hydrophobic methylene group "insertion" in the 4,6-protecting group. The calculated CLogP values for the butyl derivative I-a is 1.66 and 2.03 for compound 5, which reflects the increased hydrophobicity of the benzyl derivative.

Gelation Mechanism by 1 H NMR Studies
In order to probe the inter/intramolecular interactions, we carried out the 1 H NMR experiment at different temperatures with compound 8 in DMSO-d6 ( Figure 3). The full range 1 H NMR overlaid spectra are shown in ESI Figure S1. As shown in previous studies for a similar system [14], typically both the -NH and O-H functional groups potentially participate in H-bonding. The carbamate NH signal of compound 8 showed a significant upfield shift from δ 6.88 to 6.68 ppm, corresponding to 30 °C and 60 °C, respectively. Similarly, the 3-hydroxyl group showed an upfield shift of 0.16 ppm from 5.05 to 4.89 ppm. These indicated the importance of hydrogen bonding from the carbamate NH and 3-OH groups intermolecularly. Interestingly, we also observed a slight downfield shift in the anomeric proton from δ 4.61 to 4. 63 ppm. Although the gelation mechanism varies with solvents, it is obvious that both the 2-NH and 3-OH functional groups play important roles in the gelation process. In comparison to the urea derivative 21 reported previously [14], the 3-OH also had a 0.16 ppm shift from δ 5.09 (30 °C ) to 4.93 (60 °C ) ppm. The urea's 2-NH signal, however, showed a smaller chemical shift change of 0.07 ppm from 30 °C to 60 °C. This indicates that that the carbamate functional group played more important role during the gelation process since it offers both hydrogen bonding donating and accepting properties.

Gelation Mechanism by 1 H NMR Studies
In order to probe the inter/intramolecular interactions, we carried out the 1 H NMR experiment at different temperatures with compound 8 in DMSO-d 6 ( Figure 3). The full range 1 H NMR overlaid spectra are shown in ESI Figure S1. As shown in previous studies for a similar system [14], typically both the -NH and O-H functional groups potentially participate in H-bonding. The carbamate NH signal of compound 8 showed a significant upfield shift from δ 6.88 to 6.68 ppm, corresponding to 30 • C and 60 • C, respectively. Similarly, the 3-hydroxyl group showed an upfield shift of 0.16 ppm from 5.05 to 4.89 ppm. These indicated the importance of hydrogen bonding from the carbamate NH and 3-OH groups intermolecularly. Interestingly, we also observed a slight downfield shift in the anomeric proton from δ 4.61 to 4. 63 ppm. Although the gelation mechanism varies with solvents, it is obvious that both the 2-NH and 3-OH functional groups play important roles in the gelation process. In comparison to the urea derivative 21 reported previously [14], the 3-OH also had a 0.16 ppm shift from δ 5.09 (30 • C) to 4.93 (60 • C) ppm. The urea's 2-NH signal, however, showed a smaller chemical shift change of 0.07 ppm from 30 • C to 60 • C. This indicates that that the carbamate functional group played more important role during the gelation process since it offers both hydrogen bonding donating and accepting properties.

Metallogels Preparation and Analysis
The versatility of these gelators was further demonstrated by their ability to form gels in the presence of various metal salts. Several earth-abundant metal salts including Cu(OAc)2⋅H2O, CuBr2, CuSO4⋅5H2O, Zn(OAc)2⋅2H2O, Hg(OAc)2, Pb(OAc)4, NiCl2⋅6H2O, FeCl3⋅6H2O, FeCl2, and AgNO3 were used for the formation of metallogels. Compound 8 formed stable gels in the DMSO:H2O (v/v 1:5) solvent at 5.0 mg/mL concentration. This solvent was used for the metallogel formation for gelator 8. The detailed gelation results are included in the ESI Figure S2 and Table S1. Besides compound 8, we also tested the gelation performance of compound 11 with a few metal ions; it formed metallogels in the presence of the 1.0 equivalent (eq.) metal salt including Cu(OAc)2⋅H2O, ZnCl2, NiCl2⋅6H2O, and CoBr2 in the DMSO:H2O (1:5) mixture at 3.0 mg/mL concentration (Table S2). The photographs of the metallogels for compounds 8 and 11 are shown in ESI Figures S3a and S3b, respectively.
The summarized gelation results for compound 8 are shown in Table 3. Except for Hg (II), in the presence of the 1.5 equivalent of the metal ions to the gelator, opaque gels were obtained for all other metal salts with gelation concentrations ranging from 2.5 to 3.8 mg/mL. However, the compound showed an interesting sensing ability to detect Hg (II) ions as it did not form gels, in contrast to other metal ions. FTIR spectroscopy was used to analyze several gels with or without the metal ions. As shown in Figure 4, the binding of compound 8 with salts such as zinc acetate and copper acetate showed some changes in the peaks corresponding to functional groups such as C=O, C-O, N-H, and -OH. The full range FTIR spectra are available in ESI Figure S3c. These metallogels were characterized using an optical microscope, which revealed the presence of a three-dimensional network of long fibers as shown in Figure 5h.

Metallogels Preparation and Analysis
The versatility of these gelators was further demonstrated by their ability to form gels in the presence of various metal salts. Several earth-abundant metal salts including Cu(OAc) 2 ·H 2 O, CuBr 2 , CuSO 4 ·5H 2 O, Zn(OAc) 2 ·2H 2 O, Hg(OAc) 2 , Pb(OAc) 4 , NiCl 2 ·6H 2 O, FeCl 3 ·6H 2 O, FeCl 2 , and AgNO 3 were used for the formation of metallogels. Compound 8 formed stable gels in the DMSO:H 2 O (v/v 1:5) solvent at 5.0 mg/mL concentration. This solvent was used for the metallogel formation for gelator 8. The detailed gelation results are included in the ESI Figure S2 and Table S1. Besides compound 8, we also tested the gelation performance of compound 11 with a few metal ions; it formed metallogels in the presence of the 1.0 equivalent (eq.) metal salt including Cu(OAc) 2 ·H 2 O, ZnCl 2 , NiCl 2 ·6H 2 O, and CoBr 2 in the DMSO:H 2 O (1:5) mixture at 3.0 mg/mL concentration (Table S2). The photographs of the metallogels for compounds 8 and 11 are shown in ESI Figure S3a,b, respectively.
The summarized gelation results for compound 8 are shown in Table 3. Except for Hg (II), in the presence of the 1.5 equivalent of the metal ions to the gelator, opaque gels were obtained for all other metal salts with gelation concentrations ranging from 2.5 to 3.8 mg/mL. However, the compound showed an interesting sensing ability to detect Hg (II) ions as it did not form gels, in contrast to other metal ions. FTIR spectroscopy was used to analyze several gels with or without the metal ions. As shown in Figure 4, the binding of compound 8 with salts such as zinc acetate and copper acetate showed some changes in the peaks corresponding to functional groups such as C=O, C-O, N-H, and -OH. The full range FTIR spectra are available in ESI Figure S3c. These metallogels were characterized using an optical microscope, which revealed the presence of a three-dimensional network of long fibers as shown in Figure 5h.

Gel Morphology Characterization
The gels obtained by several compounds were characterized using an optical microscope and atomic force microscope. Some of the representative images can be seen in Figure 5. Clearly, the presence of densely packed long fibers, a typical characteristic for supramolecular gels, was observed. The gels formed by compound 2 in DMSO:H 2 O (1:2) displayed tubular or cylindrical-shaped fibers (Figure 5a,b). The gel formed by compound 5 in hexanes at 5.0 mg/mL showed densely packed straight fibers and some flat ribbons (Figure 5c). The hydrogel formed by compound 7 showed a somewhat different morphology, which contains a much more flexible curly fibrous network with smaller diameters (Figure 5d). The gels formed by compound 6 in DMSO:H 2 O (1:1) showed the presence of a ribbon-like morphology similar to what was seen in Figure 6a (Figure 5g), and, after forming metallogels, the gel exhibited similar but more densely packed fibers or planar ribbon-like morphologies (Figure 5h).

Gel Morphology Characterization
The gels obtained by several compounds were characterized using an optical microscope and atomic force microscope. Some of the representative images can be seen in Figure 5. Clearly, the presence of densely packed long fibers, a typical characteristic for  (Figure 5g), and, after forming metallogels, the gel exhibited similar but more densely packed fibers or planar ribbon-like morphologies (Figure 5h).
The AFM phase images of the gels by compounds 6 and 7 are shown in Figure 6. The gel formed by compound 6 in DMSO:H2O (1:1) at 2.8 mg/mL showed some individual long rods/tubule-types of assemblies (Figure 6a), while the hydrogel of compound 7 showed a uniform intertwined fibrous network (Figures 6b,c).

Rheological Analysis
The viscoelastic strength of several gels was analyzed using rheology experiments. The gels for this study were aged 15-18 h followed by analyzing the linear viscoelastic region with the help of amplitude sweep experiments. For all gels, a 0.2% strain was identified in the linear range and was thus used for frequency sweep analysis. In general, the G′s for all gels studied were found to be higher than the loss moduli G″s. The average G′/G″ ratio was highest for the gel formed by compound 12 in DMSO:H2O (v/v 1:2) and lowest for the gel formed by compound 11 in ethylene glycol. The hydrogel of compound 7 at 2.0 mg/mL showed the highest values for G′, indicating high strength. The stacked rheological data graphs for these gels are shown in Figure 7. The results for the amplitude sweep and the tables for the rheology data can be found in SI Figure S4a-c and Table S3.

Rheological Analysis
The viscoelastic strength of several gels was analyzed using rheology experiments. The gels for this study were aged 15-18 h followed by analyzing the linear viscoelastic region with the help of amplitude sweep experiments. For all gels, a 0.2% strain was identified in the linear range and was thus used for frequency sweep analysis. In general, the G s for all gels studied were found to be higher than the loss moduli G s. The average G /G ratio was highest for the gel formed by compound 12 in DMSO:H 2 O (v/v 1:2) and lowest for the gel formed by compound 11 in ethylene glycol. The hydrogel of compound 7 at 2.0 mg/mL showed the highest values for G , indicating high strength. The stacked rheological data graphs for these gels are shown in Figure 7. The results for the amplitude sweep and the tables for the rheology data can be found in SI Figure S4a-c and Table S3. The rheological properties of the metallogels were also analyzed using a similar procedure. The results for these gels are shown in Figure 8. In general, all gels were found to be stable under the tested angular frequency range. The mechanical strength of the metallogel formed by compound 8 with the 1.5 equivalents of zinc acetate salt at 2.5 mg/mL was found to be comparable with the control gel formed at 6.0 mg/mL in the DMSO:H2O (1:5) mixture in terms of their average G′/G″ values. The copper acetate and  The rheological properties of the metallogels were also analyzed using a similar procedure. The results for these gels are shown in Figure 8. In general, all gels were found to be stable under the tested angular frequency range. The mechanical strength of the metallogel formed by compound 8 with the 1.5 equivalents of zinc acetate salt at 2.5 mg/mL was found to be comparable with the control gel formed at 6.0 mg/mL in the DMSO:H 2 O (1:5) mixture in terms of their average G /G" values. The copper acetate and nickel chloride gels also displayed good mechanical strengths. The results for the amplitude sweep and the tables for the rheology data can be found in SI Figure S4d-g and Table S4. Figure 7. The rheological data for the gels formed by compound 7 in H2O at 2.0 mg/mL, 11 in glycerol at 1.3 mg/mL, and 12 in DMSO:H2O (1:2) at 1.8 mg/mL. The strain was 0.2% for all samples.
The rheological properties of the metallogels were also analyzed using a similar procedure. The results for these gels are shown in Figure 8. In general, all gels were found to be stable under the tested angular frequency range. The mechanical strength of the metallogel formed by compound 8 with the 1.5 equivalents of zinc acetate salt at 2.5 mg/mL was found to be comparable with the control gel formed at 6.0 mg/mL in the DMSO:H2O (1:5) mixture in terms of their average G′/G″ values. The copper acetate and nickel chloride gels also displayed good mechanical strengths. The results for the amplitude sweep and the tables for the rheology data can be found in SI Figure S4d-g and Table S4.

Chemiluminescence Properties of the Metal-Organic Xero Gels with Several Metal Ions
To analyze the catalytic potential of the metallogels obtained from this study, the chemiluminescence of luminol was analyzed. It is well known that some transition metal

Chemiluminescence Properties of the Metal-Organic Xero Gels with Several Metal Ions
To analyze the catalytic potential of the metallogels obtained from this study, the chemiluminescence of luminol was analyzed. It is well known that some transition metal cations can catalyze luminol CL reactions [42] and metal-organic gels have been utilized to both catalyze luminol chemiluminescence reactions and show enhanced CL intensities. The metallogels were prepared using compounds 8 and 11 with different earth metal salts including Cu(OAc) 2 ·H 2 O, CoBr 2 , NiCl 2 ·6H 2 O, and ZnCl 2 . The results are included in Figure S5 and Table S5a for compound 8, and in Figure 9 and Table S5b for compound 11.
As shown in Figure 9, the control panels include samples of metallogels of compound 11 (3.0 mg/mL in DMSO:H 2 O (1:5)) + luminol (100 µL of 2.0 mg/mL solution in 10 mM NaOH) without adding hydrogen peroxide. There was no CL observed with the control (orange). The second control (blue) included the solution of metal ions with luminol and hydrogen peroxide, and aqueous solutions of metal ions + luminol (100 µL of 2.0 mg/mL solution in 10.0 mM NaOH) + H 2 O 2 (0.15%). Without adding gelators, the CL was almost nondetected, except for the copper solution, which showed weak luminescence. However, strong chemiluminescence (green) was detected with the metallogels and luminol together with 0.15% H 2 O 2 . This can be attributed to the abundance of the active metal sites and large surface area generated by the fibrous network of the gels, making them better catalysts in comparison to their corresponding solutions [36,43]. The xerogels obtained from this system were able to detect hydrogen peroxide with high intensity at concentrations as low as 15 mM. The copper xerogels showed the strongest CL, followed by zinc, nickel, and cobalt gels.
However, strong chemiluminescence (green) was detected with the metallogels luminol together with 0.15% H2O2. This can be attributed to the abundance of the ac metal sites and large surface area generated by the fibrous network of the gels, mak them better catalysts in comparison to their corresponding solutions [36,43]. The xero obtained from this system were able to detect hydrogen peroxide with high intensit concentrations as low as 15 mM. The copper xerogels showed the strongest CL, follow by zinc, nickel, and cobalt gels.

Drug loading and Their Sustained Release Studies
Another important feature of the carbohydrate-based gels is their ability to form in the presence of drug molecules. For our system, we were able to load 0.5 mg naproxen sodium in the gel formed by 11 at 7.7 mg/mL. Figure 10 represents the ima of gels formed by compound 11 with naproxen sodium and compound 8 in the prese

Drug loading and Their Sustained Release Studies
Another important feature of the carbohydrate-based gels is their ability to form gels in the presence of drug molecules. For our system, we were able to load 0.5 mg of naproxen sodium in the gel formed by 11 at 7.7 mg/mL. Figure 10 represents the images of gels formed by compound 11 with naproxen sodium and compound 8 in the presence of vitamin B 2 . Followed by these results, we carried out a study to analyze the sustained release of naproxen sodium from the gel to solution phase. This was carried out similarly to the literature [14] by monitoring the UV-vis absorptions of naproxen in the aqueous phase and the results are shown in Figure 11 and ESI File Figure S6. At 60 h, naproxen was about 90% released to the solution phase. In contrast to the release profile using the amide derivative, the carbamate gel showed more sustained release over time. of vitamin B2. Followed by these results, we carried out a study to analyze the sustained release of naproxen sodium from the gel to solution phase. This was carried out similarly to the literature [14] by monitoring the UV-vis absorptions of naproxen in the aqueous phase and the results are shown in Figure 11 and ESI File Figure S6. At 60 h, naproxen was about 90% released to the solution phase. In contrast to the release profile using the amide derivative, the carbamate gel showed more sustained release over time.

Co-Gels with Electrolytes
Since compound 7 formed a hydrogel, it was analyzed for its ability to form co-gels in the presence of electrolytes such as tetrabutyl ammonium (TBA) salts. The compound was able to form co-gels with up to the 10.0-equivalents salts such as TBABr, TBAF, TBAI,

Co-Gels with Electrolytes
Since compound 7 formed a hydrogel, it was analyzed for its ability to form co-gels in the presence of electrolytes such as tetrabutyl ammonium (TBA) salts. The compound was able to form co-gels with up to the 10.0-equivalents salts such as TBABr, TBAF, TBAI, TBACl, TBAHSO 4 , and TMABr at 3.0 mg/mL concentration calculated with respect to the amount of gelator. Images of these co-gels are shown in Figure 12. TBACl, TBAHSO4, and TMABr at 3.0 mg/mL concentration calculated with respect to the amount of gelator. Images of these co-gels are shown in Figure 12. The formation of gel electrolytes using low molecular weight gelators has theoretical and practical applications, as reported in the literature [44,45]. Gelator 7 formed stable gels in the presence of various TBA salts and these could have electrochemical applications. Therefore, the conductivity of the co-gels with TBABr and the solutions of TBABr salt alone was measured. The calibration curve of the conductivity of TBABr in The formation of gel electrolytes using low molecular weight gelators has theoretical and practical applications, as reported in the literature [44,45]. Gelator 7 formed stable gels in the presence of various TBA salts and these could have electrochemical applications. Therefore, the conductivity of the co-gels with TBABr and the solutions of TBABr salt alone was measured. The calibration curve of the conductivity of TBABr in DMSO:H 2 O (v/v 1:9) at various concentrations and conductivity data for gels formed by compound 7 at 3.0 mg/mL with various amounts of TBABr in DMSO:H 2 O (v/v 1:9) can be found in ESI Figures S7 and S8, and Table S6. The gel electrolytes showed increased conductivity in the gel form. For instance, co-gel formed by compound 7 with a 6.2 mM solution of TBABr showed a conductivity value of 1307 µS/cm, while the corresponding solution showed 700 µS/cm. These results illustrate the potential of small-molecule gelators in the formation of multiple-component gels, in this case, with tetra-alkyl ammonium salts that result in gel matrices with enhanced conductivity.

Conclusions
Thirteen new C-2 carbamates derived from 4,6-O-phenylethylidene acetal protected D-glucosamine 1 were synthesized and characterized. These compounds were prepared in one step by reaction with the amine functional group in compound 1. These compounds were found to be effective organogelators for several solvents. Three hydrogelators were also obtained from these compounds. The carbamates with linear or branched alkyl chains between three and eight carbons are the most versatile gelators, forming gels in at least six different solvents. The aromatic carbamate derivatives with a methylene group linker are also effective gelators. The gels were characterized using optical microscopy and atomic force microscopy for the morphology of the assemblies. The hydrogelators were selected to study for a few applications. They were shown to be able to form multiple component gels with metal ions, tetra-alkyl ammonium salts, vitamin B 2 , and naproxen. The gelators 8 and 11 formed metallogels with different metal ions and both the copper and cobalt xerogels demonstrated higher catalytic properties for chemiluminescence in the presence of hydrogen peroxide and luminol as compared to the corresponding metal salt solutions. Hydrogelator 7 also formed co-gels with many tetra-alkyl ammonium ions and exhibited higher conductivity in comparison to the solution. Gelator 11 formed stable gels with naproxen sodium, which showed sustained release over time for naproxen. These gelators and their various applications are expected to be useful models for designing soft materials that can function as sensors or conductive electrolytes. The hydrogelators can also be useful for drug delivery applications of other drug compounds.

Materials and Methods
Reagents and solvents were used as they were received from the suppliers. All purification was conducted by flash chromatography using 230-400 mesh silica gel. The solvent systems used for chromatography and for the gelation test were all in volume ratios. NMR analysis was conducted using a 400 MHz Bruker NMR spectrometer. The molecular mass was measured using LCMS on an Agilent 6120B Single Quad Mass Spectrometer and LC1260 system or Shimadzu LCMS-2020 with ESI in positive ionization mode. Melting point measurements were carried out using the Stuart automatic melting point apparatus SMP40. Fluorescence emission spectra were obtained using the Shimadzu RF-6000 Spectro Fluorophotometer with excitation and emission bandwidths set at 5.0 nm and a scan speed of 600 nm/min. The gelation tests, optical microscopy, and AFM imaging were carried out following a literature report [46]. The instruments used for optical microscopy was the Olympus BX60M optical microscope and the Olympus DP73-1-51 high-performance 17MP digital camera with pixel shifting and Peltier cooling. AFM images were acquired using the Veeco Dimension 3100 Atomic Force Microscope. The tips used were Tap300-G silicon AFM probes with a resonant frequency of 300 KHz and a force constant of 40 N/m. Chemiluminescence data were acquired using the Varioskan LUX multimode microplate reader by Thermo Scientific from a 96-well adapter for plates without lids. The data was obtained in SkanIt software.

Optical Microscopy Studies
A small amount of the gel was placed on a clean glass slide using a micro-spatula and air-dried, which was then observed under an Olympus BX60M optical microscope and with the Olympus DP73-1-51 high-performance 17MP digital camera with pixel shifting and Peltier cooling. The imaging software used for image capturing was CellSens 1.11.

Atomic Force Microscopy Studies
AFM images were acquired using the Veeco Dimension 3100 Atomic Force Microscope. The tips used were Tap300-G silicon AFM probes with a resonant frequency of 300 KHz and a force constant of 40 N/m. The samples were prepared by spreading the gel on a glass plate with the help of a micro-spatula, which were then air-dried to obtain the corresponding xerogel viewed under the microscope.

Rheological Analyses
The rheological properties of gels were investigated by Anton Parr MCR 302 with RheoCompass software. The cone geometry is a 25 mm Peltier plate for both and with a gap of 0.1 mm for the Anton Parr Rheometer. The experimental temperature was 25.0 • C and the sample was subjected to amplitude sweep for an oscillation strain from 0.1% to 10%. A frequency sweep was then performed for the sample in the range of 0.1 to 100.0 rad/s for an angular frequency at 0.2% strain. The results were expressed as the storage modules (G ) and loss modules (G") as a function of the angular frequency.

Preparation of Gels with Tetra-Alkyl Ammonium Salts and Conductivity Study
In a one-dram vial, 3.0 mg of gelator 7 and 1.0 mL of DI water were added. This mixture was heated until all solids had dissolved, which was then allowed to cool down to rt for 15 min. The formation of the gel was tested by inverting the vial. This hydrogel was used as the control (3.0 mg/mL). To prepare the gels with different anions, the desired amount of TBA salt was added. The mixture was then re-heated and cooled to test the formation of the gel.
For the conductivity studies, the gels were prepared using compound 7 (30.0 mg, 1.0 eq.) in 1.0 mL of DMSO. To this solution, warm water (9.0 mL) was added through a syringe to the solution. The resulting mixture was allowed to cool to rt until gelation was observed. To this gel, TBABr (10.0 mg, 0.5 eq.) was added for the measurement of conductivity. Similarly, gels with 1.0 eq. (20.0 mg), 1.5 eq. (30.0 mg), and 3.0 eq. (60.0 mg) of TBABr were prepared and tested for conductivity. Details of the amounts used for each gel are available in Table S7.

Metal-Organic Gels for Chemiluminescence Study
In a one-dram vial, gelator 11 (3.0 mg, 0.007 mol, 1.0 eq.) and metal salt (1.0 eq.) were added. Then, the DMSO:H 2 O (1:5) mixture (0.2 mL) was added into the vials. The mixture was heated to form a homogeneous solution and allowed to cool to room temperature to form gels. Subsequently, metal−organic gels were observed within 15 min under ambient conditions. Metal-organic Xerogels (MOX) were further acquired after removing the solvent of MOGs under air. To investigate the luminol−MOXs CL system, 100 µL of the solution of MOX (3.0 mg/mL premixed in Millipore-grade water) was added in a 96-well plate. Then, 100 µL of the luminol solution (2.0 mg/mL in 10.0 mM NaOH solution) was injected, followed by 100 µL of the H 2 O 2 solution (0.15%), and both the CL profile and intensity were measured.
Synthesis of compound 14. Compound 1 (75 mg, 0.25 mmol, 1.0 eq.), Fmoc chloroformate (52 mg, 0.20 mmol, 1.2 eq.), and DIPEA (35 µL, 0.20 mmol, 1.2 eq.). The crude product was purified by column chromatography using 0-1% MeOH in DCM to afford a yellowish solid (51.8 mg, 0.10 mmol, 59%) as the desired product. Supplementary Materials: The following supporting information can be downloaded at: https: //www.mdpi.com/article/10.3390/gels8030191/s1, Part I: Copies of NMR ( 1 H and 13 C) spectra of carbamate derivatives 2-14; and 2D spectra for compounds 3, 6, and 10 and Part II: NMR spectra of compound 8 at variable temperatures; procedures for gelation tests and water tolerance studies; details for metallogels' formation and analysis; rheological analysis data; chemiluminescence analysis, drug loading, and release studies; conductivity measurement for co-gels with TBA salts; and LCMS data. Figure S1. The 1 H NMR spectra of compound 8 from 30-60 • C at 8.0 mg/mL in DMSO-d 6 ; Figure S2. Gels of compound 8 in 0.1 mL of DMSO and incremental amounts of water; Figure S3a. Gels formed by compound 8 with 1.5 eq. of metal salt at 5.0 mg/mL; Figure S3b. Gels formed by compound 11 with 1.0 eq. of metal salt at 3.0 mg/mL; Figure S3c. Overlay of IR spectra of compound 8; Figure S4a-g, Amplitude sweep data graphs for several gels; Figure S5. Chemiluminescence intensities of luminol with Metal-Organic-Xerogels of compound 8; Figure S6. The gel images of compound 11 and naproxen in 2.0 mL of DMSO:H 2 O (v/v 1:10); Figure S7. Conductivity correspondence to concentrations of TBABr solutions; Figure S8. Conductivities of the co-gels formed by compound 7 in the presence of TBABr and the TBABr solutions. Table S1. Gelation properties of compound 8 in different amount of water; Table S2. The gelation concentrations of compound 8 after adding water to metallogels; Table S3. G /G ratios for several gels; Table S4a. G /G ratios for various gels and metallogels; Table S4b. G /G ratios for metallogels; Table S5a. Chemiluminescence data for compound 8; Table S5b. Chemiluminescence data for compound 11; Table S6. Conductivity data of multicomponent gels.

Funding:
The research study was supported by NSF grant CHE #1808609.

Informed Consent Statement: Not applicable.
Data Availability Statement: Not applicable.