Jakub S. Cyniak and
Artur Kasprzak
*
Faculty of Chemistry, Warsaw University of Technology, Noakowskiego Str. 3, 00-664 Warsaw, Poland. E-mail: artur.kasprzak@pw.edu.pl
First published on 23rd April 2024
A mechanochemical synthesis of novel polyaromatic amide consisting of 1,3,5-triphenylbenzene and 1,1′,2,2′-tetraphenylethylene skeletons has been established. The designed mechanochemical approach using readily available and low-cost equipment allowed a twofold increase in reaction yield, a 350-fold reduction in reaction time and a significant reduction in the use of harmful reactants in comparison to the solution synthesis method. The parameters of Green Chemistry were used to highlight the advantages of the developed synthesis method over the solution-based approach. The title compound was found to exhibit attractive optical properties related to the Aggregation-induced emission (AIE) behaviour. Taking the advantage of AIE-active properties of the synthesized polyaromatic amide, its application as effective and versatile molecular receptor towards detection of monovalent anions, as well as bio-relevant anions – nucleotides, has been demonstrated. The values of the binding constants were at the satisfactory level of 104, the detection limit values were low and ranged from 0.2 μM to 19.9 μM.
Mechanochemistry, although known since ancient times,38 is considered a modern and attractive synthetic tool in organic chemistry. The reduction in the use of harmful organic reactants and solvents, and thus the reduction in waste generation and notable reduction in reaction times are one of the most important advantages of mechanochemistry. Furthermore, despite the usage of simple and readily available instruments, mechanochemistry often allow synthesis of compounds, which are hard or even impossible to obtain by traditional solution-based methods.39,40 All these benefits make mechanochemistry one of the flagship methods of Green Chemistry, fulfilling many of its paradigms. Despite mechanochemical synthesis and design of AIE-active compounds are emerging fields of chemistry, the reports dealing with merging these concepts are extremely sparse.41 To the best of our knowledge, the reports mostly include very recent (2021–2023) studies on the grinding-induced synthesis of AIE-active benzothiazole-azine42–44 or benzothiazole derivatives45 (Fig. 1a). Despite 1,1′,2,2′-tetraphenylethylene skeleton is commonly used as first- or best-choice AIE-active unit,8,24,25,46 only one phthalimide derivative bearing this motif was recently synthesized under mechanochemical conditions47 (Fig. 1a). Neither other conjugates of 1,1′,2,2′-tetraphenylethylene nor the AIE-active 1,3,5-triphenylbenzene derivatives were obtained using mechanochemistry. Also, 1,1′,2,2′-tetraphenylethylene derivatives monosubstituted with 1,3,5-triphenylbenzene have not been studied extensively. To the best of our knowledge, only one such carbon–carbon linked conjugate, bearing the naphthalene linker, has been described in the patent (2005).48
In this work (Fig. 1b), the application of a mechanochemical method to synthesise a polyaromatic amide 3 consisting of 1,3,5-triphenylbenene and 1,1′,2,2′-tetraphenylethylene units is described for the first time. We demonstrated that the developed mechanochemical synthesis method provided excellent yields with shorter reaction times while significantly reducing usage of toxic reactants and solvents compared to the current state of the art. The parameters of Green Chemistry were used to highlight the advantages of the developed synthesis method over the conventional approach. The synthesized polyaromatic amide has been comprehensively characterised by multiple spectroscopic methods in terms of properties derived from the AIE effect, and then was applied as an innovative, versatile receptor for the detection of both monovalent and bio-relevant anions, that is nucleotides. Taking into account that the synthesis of 3 was performed with readily available and low-cost equipment, herein, we were able to show the power of using simple mechanochemical approaches for creation of attractive AIE-active compound toward the design of innovative organic molecular receptors.
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Scheme 1 General synthesis path to obtain compound 3 together with the graphical presentation of key-results. |
Initial trials were focused on reactions carried out in various organic solvents in the presence of EDC·HCl (1-(3-dimethylaminopropyl)-3-ethylcarbodiimide hydrochloride) as a coupling agent (all starting materials as well as the product had good solubility in the solvents tested). These were intended to provide a reference point for further syntheses by mechanochemical and sonochemical methods, as well as to provide a benchmark for comparing reaction yields. To our surprise, these experiments provided unsatisfactory to moderate yields (9–48%), even for very long reaction times (up to 170 h). The usage of thionyl chloride also did not provide satisfactory yield (9%).
Having established that carrying out the reaction using solution method yielded poor or average results, we proceeded to attempt a mechanochemical synthesis of 3. Our ultimate goal was to perform the reaction using readily available and low-cost equipment, available in every organic chemistry laboratory. To our delight, just 15 minute grinding of compounds 1 and 2 in a hand-held mortar in the presence of EDC·HCl and small amount of DCM (50 μL) (LAG – Liquid Assisted Grinding) provided 3 with similar reaction yield (52%) as for the process in the solvent conducted for 170 hours, i.e., in the 350-fold less time. In the next steps, we evaluated whether other coupling agents or additives (grinding auxiliaries) would enable a further increase in reaction yield. For this purpose, reactions were carried out by grinding starting materials in hand-held mortar with different coupling agents or additives. The highest yields were obtained for carbodiimides (Fig. 2a). During grinding procedure, the mixture was a pale-yellow powder and did not change throughout the grinding process. Additives we used (Fig. 2b) differed in their acid-base nature. Experiments showed only a slight increase in reaction yield for compounds of neutral character (NaCl and SiO2). Alkaline and acidic additives generally caused a decrease in reaction yield. We also noted that the additives caused the form of the mixture to change to a dark yellow viscous paste, which made grinding more difficult. An important parameter for mechanochemical reactions is the presence of a small amount of solvent (LAG). To our delight, we found that it was possible to replace dichloromethane with ethyl acetate without any significant decrease in the reaction yield. The effect of grinding time on reaction yield was also investigated. The reaction mixture was ground in a hand-held mortar for 5 to 30 minutes. Increasing the grinding time did not significantly change the reaction yield.
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Fig. 2 Effect of reaction parameters on the relative yield of mechanochemical synthesis (grinding in mortar); (a) coupling agent, (b) additives. |
Mechanochemical reactions can be carried out not only in mortars or specialised mills, but also using systems as simple as a glass rod and a narrow glass vial. There are reported examples of reactions for which such a simple set-up has allowed high yields to be obtained.49 To our delight, just a 15 minute grinding of the reactants with glass rod in glass vial provided target product with 84% yield. Further extension of the reaction time to 30 minutes provided an excellent 96% yield (for the optimised reaction protocol, see experimental section). During grinding, after about 3 minutes the mixture became a dark yellow viscous paste, which then solidified. The reaction carried out in ethyl acetate provided a slightly lower yield (80%), confirming the possibility of using this biodegradable solvent50,51 for the synthesis. This allows for a more sustainable synthesis with a slightly lower yield. We hypothesise that the differences in the yields obtained in the grinding reactions in the mortar and in the glass vial can be attributed to the method of the grinding. This might be due to the larger ratio of the surface area of the glass rod to that of the vial than the ratio of the surface area of the pestle to that of the mortar.
It is also worth noting that carrying out the reaction under sonochemical conditions did not provide higher yields (80%).
Finally, to check the repeatability of the designed grinding-induced protocol, we performed the mechanochemical synthesis of the target compound 3 under optimized mechanochemical conditions three times, at the similar scales and on different days (independent runs; grinding in glass vial with glass rod, reaction time: 30 minutes, 1.0 equiv. of EDCl). The synthesis outcomes were highly consistent what demonstrated that the designed grinding-induced synthesis is highly reproducible; the obtained isolated yields were consistent and equalled 93 ± 3%. 1H NMR analyses also supported the isolation of pure 3 in each synthesis run. Refer to ESI, subsection S1.3† for the full data regarding the reproducibility of the experiments.
Metrics | Synthesis in solvent EDCl·HCl/DMAP | Mechanochemistry EDCl·HCl |
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a Isolated yields.b Including coupling agent and workup solvents.c Including additional reagent.d For solvents used directly in synthesis.e For additional safety data see ESI, section S1.5, Table S4.† | ||
Yielda (%) | ![]() |
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Reaction time (h) | ![]() |
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Atom economy (%) | 67% | 76% |
RME (%) | 72% | 73% |
PMI(total)b | 5834 | 5689 |
PMI(reaction)c | 154 | 9 |
PMI(solvent)d | 153 | 1.9 |
PMI(additive) | 0.037 | 0 |
Reaction solvent | ![]() |
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Health and safetye | ![]() |
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Main hazard statementse | H318, H370, H411 | H302, H315, H335 |
The closer the values of Atomic Economy (AE) and Reaction Mass Efficiency (RME) are to 100%, the more efficient is the reaction. On the other hand, the Process Mass Intensity (PMI) values should be in the lowest possible range. While the calculation of some parameters (e.g., PMI) are most direct for the reactions performed at the kilogram scale, which is not possible to conduct for every process at the design step and due to some laboratory (equipment and scale) limitations, we wanted to provide a general overview of the advantages of the designed mechanochemical approach as compared with the reaction in solution. In fact, some of the reported studies included the calculation of these parameters for the milligram scale reactions.53
The reaction yield of the mechanochemical reaction was double that of the reaction in solvent and was achieved in almost 350-fold shorter time. A higher Atom Economy (about 10%) was achieved in the mechanochemical reaction, due to the absence of an additional reactant (DMAP), which was used in the synthesis in solution. Similar values of Process Mass Intensity (PMI) and Reaction Mass Efficiency (RME) were obtained for both synthetic approaches. Differences can be seen when individual components of PMI are extracted. Mechanochemical reaction using in a lower volume of solvent (LAG) and without an additive resulted in a significant reduction in PMI(reaction) and PMI(solvent) values by approximately seventeen and eighty-one times respectively. Both methods use dichloromethane as a solvent, small amount used in mechanochemical synthesis reduces exposure to its hazardous properties (causes skin and eye irritation – H315 and H319, may cause drowsiness or dizziness – H336 and is suspected of causing cancer – H351).
Due to the presence of 1,3,5-triphenylbenzene and 1,1′,2,2′-tetraphenylethylene skeletons in the compound 3 structure we anticipated that this compound could feature AIE properties. The emission properties of compound 3 in the aggregated state were studied in the DMSO/H2O system with increasing volume of water (Fig. 3c and d). For water contents below 30 vol% emission is very weak. For 30–40 vol% water content an intensive blue emission of λmax ca. 445 nm appears, followed by a bathochromic shift of λmax to ca. 465 nm from 50 vol% water to 99 vol% of water content in the sample. A maximum emission is observed for 50 vol% water. Further increase in the amount of water slightly reduces the emission intensity and causes it to settle at a relatively constant level. Changes in emission maximum and intensity can also be observed with the naked eye (Fig. 4). The emission intensity in DMSO/H2O = 1/1 v/v system is almost double that of the solid-state (Fig. 2c). We hypothesise that the occurrence of a maximum in emission intensity for 50% water content in the sample and the subsequent slight decrease in emission intensity for higher water contents might be related to the size of the aggregates. Increasing the percentage of water content in the sample to 90% results in a more than 9-fold decrease in the mean hydrodynamic diameter of the aggregates (from 254 nm to 27 nm; see DLS data in ESI, section S6†).
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Fig. 4 Aggregates of 3 in DMSO/H2O system containing different vol% of water in the sample seen under UV light (λex = 365 nm). |
To further confirm the presence of compound 3 in the form of aggregates, DLS (Dynamic Light Scattering) analysis was performed. Importantly, no particles were detected in the DMSO solution of 3 (Fig. 5a). On the other hand, particles with a mean hydrodynamic diameter of 254 nm were found in the DMSO/H2O system, confirming the formation of aggregates (Fig. 5c). Interestingly, increasing the water content of the system from 50 vol% to 90 vol% resulted in a 27-fold reduction in the mean hydrodynamic diameter of the aggregates, to 27 nm. In order to demonstrate the differences in morphology of solid compound 3 in the aggregated form and before aggregation, SEM (Scanning Electron Microscope) images were acquired (see data on SEM in sections S1.1 and S7 in ESI†). Fig. 5b shows the SEM image of solid compound 3 obtained after purification on a chromatographic column. The image shows a smooth particle surface with a sharp boundary between grains – bright stripe on the upper left (the surface irregularities are due to the metallic gold layer applied to the sample and are not due to the surface morphology of the sample). Fig. 5d shows the SEM image of the aggregates of compound 3 obtained by filtrating them from the DMSO/H2O = 1/1 v/v solution and later drying on air at room temperature. A significant change in the morphology of the samples can be observed. Instead of a flat surface for solid compound 3, fine, spherical particles of various sizes (diameter <100 nm) are forming the entire volume of the sample of aggregated 3. The spheres are not completely merged, voids are visible between them. Three-dimensional sponge-like structure was formed. There are also areas where the spherical aggregates merge together to form elongated rod-shaped structures.
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Fig. 5 DLS measurements: size of particles of 3 in: (a) DMSO, (c) DMSO/H2O = 1/1 v/v; SEM images of 3; (b) solid obtained after column chromatography, (d) dried aggregates. |
To confirm that the amide bond is involved in the interaction of 3 with the anions, a series of 1H NMR spectra were measured with increasing molar concentration of Br− anion (in the form of tetrabutylammonium bromide) from 0 eq to 10 eq in solution (for experimental details and spectra see ESI sections S1.7.1 and S5.1,† respectively). An upfield chemical shift of the signal coming from the proton of the amide group was observed. We have attributed this phenomenon to the anion binding, namely the process of proton transfer from the amide group of the receptor to the anion. No changes were observed neither in the chemical shift of the other signals of compound 3 nor the tetrabutylammonium cation.
Having confirmed by 1H NMR spectroscopy the occurrence of non-covalent interactions of compound 3 with anions, they were further characterised for Br− as the representative monovalent anion by spectrofluorimetry (λex = 270 nm and 340 nm) in DMSO and DMSO/H2O = 1/1 v/v system (for experimental details see ESI, section S1.7.2†). Control experiments revealed that the most significant changes (decreases) in emission intensity, were observed for the emission spectra measured in DMSO/H2O = 1/1 v/v system and applying λex of 270 nm. Therefore, this solvent system and excitation wavelength were used to further analyses. Fig. 6 shows a general comparison for the emission spectra of compound 3 in the presence or absence of Br− in different solvent systems. The addition of 0.5 eq. of Br− to compound 3 in the aggregated state (DMSO/H2O = 1/1 v/v) causes 10-fold decrease in the emission intensity (compare blue and green lines). On the other hand, for solution of 3 in DMSO (red line), only 0.06-fold increase in emission intensity was observed after the addition of 7 molar equivalents of Br− (compare pink and red lines). This observation confirms our hypothesis that compound 3 in aggregated form exhibit better receptor properties than in the molecularly solubilised state.
Based on the results obtained for Br−, interactions of 3 with other monovalent anions (I−, HSO4−, BF4−, H2PO4−, ClO4−, CN−) were characterized by emission spectra in aggregated state (2 × 10−5 M, DMSO/H2O = 1/1 v/v, λex = 270 nm; for the spectra see ESI, section S5.2†). For most of the analysed anions, decreases in emission intensity were observed, and only for ClO4− ions there was an increase in emission intensity. The values of the binding constants were determined using the Stern–Volmer method (systems for which a decrease in emission intensity was observed; Ksv was calculated) and Benesi–Hildebrant method (systems for which an increase in emission intensity was observed; Kapp was calculated) (for details see ESI, section S5†). The determined values of the binding constants were at the level of 104 M. The highest value (4.4 × 104 M) was obtained for ClO4−(Fig. 7, blue dashes). Limit of Detection (LOD) values were also determined, for anions showing an increase in emission on the basis of the Benesi–Hildebrant equation, and for anions showing a decrease in emission on the basis of the Stern–Volmer equation. The lowest value (0.17 μM) was obtained for the Br− anion (Fig. 7, green dashes).
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Fig. 7 Values of LOD and binding constants for different anions; *determined by Benesi–Hildebrant method, for other by Stern–Volmer method. |
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Fig. 8 Structures of the nucleotides selected for the studies on interactions with compound 3; green colour denotes phosphate groups; blue colour denotes nucleobases moieties. |
The interactions of 3 with representative nucleotides, namely AMP and ADP, were investigated using 1H NMR spectroscopy (for the full spectra see ESI, section S5.1†). Measurements were made while keeping total number of moles of receptor (3) and analyte (nucleotide) in the sample on the constant level, with varying their molar fractions. Fig. 9 shows the 1H NMR titration data for representative AMP. Shift of the signal of the amide group was observed (Fig. 9a). We have attributed this feature to the anion binding phenomenon, namely the process of proton transfer from the amide group of the receptor to the anion. Shifts in the signals of the nucleobase were also observed (protons a and b, Fig. 9b). The stoichiometry of the complexes formed was estimated using Job's plot method55 (continuous variation method; see details of this methodology in section S5, ESI†), was found to be 3:
1 both for AMP and ADP, that is three molecules of amide (3) per one nucleotide. We hypothesised that, in the case of AMP, one molecule of the amide 3 binds to the phosphate group and two molecules bind to nitrogen atoms in the nucleobase (as indicated by chemical shifts on the 1H NMR spectrum) which means that this structural moiety is also involved in interaction with receptor 3. In the case of ADP, only one signal shift of the nucleobase is observed, which may indicate that two amide molecules bind to phosphate groups and one to the nucleobase.
Having confirmed by 1H NMR spectroscopy the occurrence of non-covalent interactions of compound 3 with anions, they were further characterised by emission spectra in aggregated state (2 × 10−5 M, DMSO/H2O = 1/1 v/v, λex = 270 nm; see details of this methodology in SI, section S5.2†). For all nucleotides, a decrease in emission intensity was observed as their molar concentration in the sample increased. Fig. 10 shows emission spectra of 3 in the presence of various molar equivalents of FAD as representative nucleotide. Addition of 10 equivalents of FAD caused 20-fold decrease in emission intensity. The values of the binding constants were determined using the Stern–Volmer equation (Ksv). The determined values of the binding constants were at level of 104 M. These Kapp values are in a good agreement with the values for monovalent anions. This means, that receptor 3 can not only effectively bind simple anions, but also sophisticated bio-anions, with the similar Kapp. The highest value (8.80 × 104 M) was obtained for FAD (Fig. 11, blue dashes). Limit of Detection (LOD) values were determined based on the Stern–Volmer equation. The lowest value (0.69 μM) was obtained for the FAD (Fig. 11, green dashes). When analysing the values of the binding constants obtained for each nucleotide, attention could be drawn to the value of the binding constant for FAD, which is almost 10 times higher than the binding constant for AMP. It might be explained by comparing the structure of FAD with the other nucleotides. Analyses of the interaction of amide (3) with AMP and ADP by 1H NMR show that, in addition to the interaction with the phosphate groups, there is also an interaction between amide (3) and the nitrogen atoms of the nucleobase. FAD, being a dinucleotide composed of flavin and adenine moieties, has a much higher number of nitrogen atoms in its structure that can interact with the amide.
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Fig. 10 Emission spectra of 3 in the presence of various molar equivalents of FAD (DMSO/H2O 1![]() ![]() |
1H NMR (DMSO-d6, 500 MHz, ppm), δH 10.29 (s, 1H) 7.91–7.85 (m, 11H), 7.78–7.76 (m, 2H), 7.53–7,50 (m, 4H), 7.43–7,40 (m, 2H), 7.20–7.12 (m, 11H), 7.04–7.00 (m, 6H); {1H}13C NMR (DMSO-d6, 125 MHz, ppm), 165.0, 146.7, 142.9, 142.8, 142.7, 141.6, 141.1, 140.2, 139.7, 138.9, 135.1, 132.6 × 2, 130.6, 128.9, 128.0, 127.9 × 2, 127.8, 127.7, 127.3 × 2, 127.2, 126.9, 126.7, 124.0 × 2, 120.6; HRMS (ESI) m/z [M]+ calcd for C51H37NO = 680.2948, found = 680.2942 m/z; elemental analysis: Anal. Calcd for C51H37NO: C, 90.1; H, 5.49; N. 2.06. Found: C, 89.86; H, 5.49; N, 2.08. Rf (2% hex/CH2Cl2) = 0.91.
The stoichiometry of the complexes formed was estimated using Job's plot method (based on the 1H NMR experiments), from the plot: (1 − x) × (δ − δ0) vs. x. The x stands from the mole fraction of nucleotide. The expected stoichiometry was indicated by the maximum on the plot.
Footnote |
† Electronic supplementary information (ESI) available: Full experimental section, compounds characterization data, data on AIE for title compound, data on the application of title compound as molecular receptor. See DOI: https://doi.org/10.1039/d4ra02129k |
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