Hui Feng‡
ab,
Yuqi Du‡a,
Fan Tanga,
Ning Jia,
Xuefeng Zhao*a,
Hang Zhao*a and
Qianming Chena
aState Key Laboratory of Oral Diseases, West China Hospital of Stomatology, Sichuan University, Chengdu, Sichuan 610065610041, P. R. China. E-mail: zhao.zxf@gmail.com; zhaohangahy@scu.edu.cn
bXiangYa Stomatological Hospital, Central South University, Changsha, Hunan 410000, P. R. China
First published on 27th April 2018
In this work, the detailed crystallization process of 2′-deoxy-2′-fluoroguanosine (FGd) hydrogel has been studied using single crystal X-ray diffraction, variable-temperature nuclear magnetic resonance (VT-NMR), and scanning electron microscopy (SEM). Both solid and solution results indicated that the K+-mediated G-quartet structures were unstable and easily resulted in the breakdown of the hydrogel to form linear ribbon structures by forming mimic reverse Watson–Crick base pairs between the two faces with an intermolecular hydrogen-bond (N10H–O11). Accordingly, Ag+ was introduced to block the crystallization of FGd to form long lifetime stable supramolecular hydrogel (>6 months) and possible silver-ions-mediated base pair motifs were suggested via NMR, UV, and mass spectroscopy (MS) in combination with powder X-ray diffraction (PXRD) and circular dichroism spectroscopy (CD). Furthermore, FGdAg hydrogel exhibited low toxicity for normal oral keratinocyte cells (NOK-SI) and good antibacterial activities for Fusobacterium nucleatum in vitro.
However, to the best of our knowledge, the crystallization process of guanosine-based hydrogels has not been explored yet. Thus, determining their delicate structural balance between gelation and crystallization is critical, not only to gain more insight into the reasons for crystallization and further understand how to design new guanosine-based gelators but also to tune their lifetime stability and mechanical properties to develop multifunction supramolecular materials in the future. Inspired by this, the crystallization process of 2′-deoxy-2′-fluoroguanosine (FGd) hydrogel has been studied in this work. FGd has the same base and similar sugar moiety as guanosine. It was first synthesized by J. Imura in 1981 and thereafter, it was observed to exhibit significant anti-virus activities for influenza A and B, herpes simplex virus (HSV), and H7N1.35–39 Furthermore, Christopher J. L. suggested that FGd is a powerful anti-favoring tool to manipulate G-quadruplex polymorphism and folding topology.40 Recently, the gel properties of FGd have been investigated by our group and the results indicated that FGd forms a transparent hydrogel only in the presence of K+.41 In this work, the detailed crystallization process of FGd hydrogel was first studied using single crystal X-ray diffraction, VT NMR, SEM, PXRD, and CD. Based on the above information, we observed that silver ions could not only block the crystallization of FGd but also induce FGd to form a long-term stable supramolecular hydrogel with favorable antimicrobial activities (Fig. 1).
Furthermore, to get more detail information about the crystal from the hydrogel in molecular level, the single crystal structure of FGd has been analyzed carefully from three levels: monomer molecular, base pair motif and three-dimension structure. Firstly, the monomer molecular structure with systematic numbering and the single crystal structure of FGd were shown in Fig. 3. The anti/syn conformation of the glycosyl bond was paramount to the canonical purine or pyrimidine nucleosides, which could be defined by the torsion angle χ (O4′–C1′–N9–C4). The torsion angles χ of FGd were measured to be −93.15(33)°, indicating that it adopted a normal anti conformation. Sugar puckering is another significant conformational parameter defined by the pseudorotation phase angle (P) and maximum puckering amplitude (τm). Two ranges of pseudorotation phase angle were initially observed in natural and synthetic nucleosides: C3′-endo with 0° ≤ P ≤ 36° (North) or C2′-endo with 144° ≤ P ≤ 180° (South). FGd adopted a typical N-type conformation with a twist of C3′-endo (3T2, N, P = 15.6(4)°, τm = 33.6(7)°). Moreover, it was also a crucial structural parameter for the orientation of the 5′-hydroxyl group defined by the torsion angle γ (O5′–C5′–C4′–O4′) relative to the sugar ring. For FGd, it was in the ap (gauche, trans) range with the O5B′–OH at the axial position and pointing outside the sugar ring (γ = 61.98(33)°). Secondly, as FGd has the same base moiety as guanosine, which has three faces with hydrogen bonding donors and acceptors, it can self-assemble into complex and unique supramolecular structures, such as dimers, ribbons, and tetramers. In this case, the aforementioned structures were not obtained as the hydrogels broke down and it was only found that FGd could form mimic reverse Watson–Crick base pairs between two faces with an intermolecular hydrogen-bond (N10H–O11), which extended to form a linear ribbon structure with sugar residues located on both sides.
Finally, based on the base pair motif, a multilayered structure was formed at the 3D supramolecular level with complicated hydrogen bond networks including additional contributions from sugar residues (Fig. 4). To clearly display the hydrogen bond networks, the 3D supramolecular network was divided into three aspects: base–base, sugar–sugar, and base–sugar interactions of different layers. The interaction between base moieties is shown in Fig. 4b. O11 held three molecules from three neighboring layers together as a bridge with two hydrogen bonds, and it was connected to C8H of one molecule and N10H of another molecule. The sugar–sugar interactions are displayed in Fig. 4c. The C2′–H of one molecule was directly connected to the O5′ of another molecule. 5′-OH linked together three molecules from three adjacent layers with two hydrogen bonds (2′F–5′OH–3′O). The interactions of base–sugar are shown in Fig. 4d. There were four hydrogen bonds between four molecules at three neighboring layers (5′O–N1H, N7–3′OH, 3′O–N10H, O11–C2′H). In general, a complicated hydrogen bond network formed with nine hydrogen bonds was repeated infinitely throughout the assembly process of the 3D multilayered supramolecular structure in the single-crystal state.
In order to explore their self-assembling properties in solution state, VT NMR spectrometry was used to investigate the formation of hydrogen bonds of FGd. As shown in Fig. S2,† the chemical shift of N10H atom of the amino group moved from δ 6.60 (298 K) to δ 6.46 ppm (338 K) with Δδ = 0.14 ppm, the chemical shift of 3′-OH atom of the hydroxyl group moved from δ 5.69 (298 K) to δ 5.53 ppm (338 K) with Δδ = 0.16 ppm, and the chemical shift of 5′-OH atom of the hydroxyl group moved from δ 5.15 (298 K) to δ 4.97 ppm (338 K) with Δδ = 0.18 ppm. These results indicated that these hydrogen atoms participated in the formation of intermolecular hydrogen bonds. Another hydrogen atom (N1H) from the imino group at δ 10.73 ppm was assigned as the intramolecular hydrogen bond as its chemical shift remained unchanged upon the increase in the temperature. To this end, 1H–1H nuclear overhauser effect (NOE) experiments was performed and they demonstrated that the C8–H⋯NH2 and NH NOE signals (illustrated by the empty boxes, see ESI, Fig. S3†) were not observed, which was consistent with the solid state.
Both solid and solution results indicated that the K+-introduced G-quartet structure was not stable and easily broke down in hydrogel and subsequently formed a linear ribbon structure with mimic reverse Watson–Crick base pairs between the two faces with an intermolecular hydrogen-bond (N10H–O11), which may be the reason for the propensity of guanosine-based hydrogel to crystallize over time. To block the crystallization of FGd hydrogel getting a long lifetime stable supramolecular hydrogel, introducing stronger metal bonds would be a good choice. Previously, researchers determined that metal ions such as Pt2+, Hg2+, and Ag+ tended to alter hydrogen bonding patterns between guanosine molecules by the coordination of the electron-rich nitrogen and oxygen groups around the purine ring to produce a range of metal ion-linked H-bonded architectures.34,46,47 For example, Kraatz et al. reported that an Ag+ induced G gel was exploited for the light triggered in situ fabrication of uniform AgNPs within a gel to make a nano–bio hybrid material; Mann et al. found that supramolecular hydrogels produced by spontaneous self association of disodium guanosine 5′-monophosphate (Na25′GMP) in the presence of Ag+ ions. Inspired by this, Ag+ was introduced in this work and the results showed that FGd can not only form hydrogel in the presence of silver ions but also demonstrate long lifetime stability (>6 months). Furthermore, FGd hydrogelation experiments were carried out at different concentrations of AgNO3 and FGd (0.0125 M to 0.2 M AgNO3 and 0.175 mg to 2.8 mg of FGd per 100 μL of solution). The phase diagram in Fig. 5 revealed that the formative qualification of the hydrogel. The concentration control between AgNO3 and FGd was observed to play a critical role in the formation process of FGd hydrogel. Interestingly, FGd tended to form a hydrogel at low silver ion concentration, which suggested that the hydrogel had significant potential for biological or medical applications.
Furthermore, the mechanical properties of the hydrogel were analyzed in detail using rheological measurements. The storage modulus (measurement of elastic property) and loss modulus (measurement of fluidity) were expressed as G′ and G′′, respectively. As shown in Fig. 6, the typical elastic nature of FGd + Ag+ (FGdAg) hydrogel was evident from the fact that G′ > G′′ (solid-like behavior) via strain amplitudes ranging from 0.001 to 0.1% at 6.28 rad s−1. Moreover, the frequency sweep experiments of FGdAg hydrogel were performed in the angular frequency range of 0.1–100 rad s−1 under an initial strain of 0.1% and the results showed that FGdAg hydrogel had a higher storage modulus G′ than loss modulus G′′ over the entire applied frequency range, indicating that it exhibited a solid-like behavior.
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Fig. 6 Evaluation of G′ and G′′ as a function of the strain (a) and frequency sweep (b). The compound was measured at the concentration of 0.7 mg per 100 μL in 0.025 M AgNO3 solutions at 25 °C. |
To obtain microstructures of the FGdAg hydrogel, we prepared xerogels for SEM observations (Fig. 7a–f). The hydrogels were prepared in a sample tube (0.7 w/v%) containing 0.025 M AgNO3 and they were subsequently frozen. The frozen samples were lyophilized using a vacuum pump. Prior to examination, the xerogel was attached to the silica wafer and coated with a thin layer of gold. The SEM images revealed the three-dimensional uniform porous-like structures with a diameter of approximately 500 nm. Careful inspection of the images revealed that flexible fibers with a diameter of approximately 20–30 nm and several micrometers in length were formed spontaneously during the formation of hydrogel. The fibers intertangled with each other to form highly ordered film-like structures. Energy-dispersive X-ray spectroscopy analysis confirmed the presence of Ag in the fibers. AFM was carried out to further analyze and evaluate the structures of the hydrogel. Fig. 7g–i reveals the existence of an interconnected fibrous network with a diameter of approximately 20–30 nm, height of 6–8 nm, and length of several micrometers, which are consistent with the above results.
To explore more molecular-level evidences of the hydrogel, CD spectroscopy, PXRD, and NMR were carried out. Previous reports indicated that a planar quartet system show peaks at 240 nm and 260 nm in CD spectrum.28 Here, the FGdAg hydrogel showed two negative peaks at 220 and 290 nm (see ESI, Fig. S4†), which indicated that the G-quartet structures were not observed in this hydrogel. As shown in Fig. S5,† the freeze-dried sample of FGdAg hydrogel was studied using PXRD and it exhibited similar patents for FGdAg hydrogel and the crystal of FGd hydrogel in the presence of K+. All of them exhibited a significant peak at 2θ ≈ 6.0° and 26.8° (d = 14.5 Å and 3.4 Å, respectively) consistent with the monomeric length and Pi–Pi stacking distance between two layers of G rings.31 Subsequently, FGd and FGdAg were characterized using 1H NMR spectra at 298 K (see ESI, Fig. S6†). The results showed that N10H peak almost disappeared when Ag+ was introduced to FGd, indicating that the amino group may participate in the silver base pair. VT NMR experiments were carried out to further investigate the formation of hydrogen bonds of FGdAg. As shown in Fig. 8 and Table S1,† the chemical shift of N1H atom was from δ 10.84 (298 K) to δ 10.64 ppm (338 K) with Δδ = 0.20 ppm, the chemical shift of N10H atom of the amino group was from δ 6.65 (298 K) to δ 6.47 ppm (338 K) with Δδ = 0.18 ppm, and the peak began to increase in relative intensity when the temperature increased from 298 K to 338 K. The chemical shift of 3′-OH atom of the hydroxyl group moved from δ 5.69 (298 K) to δ 5.53 ppm (338 K) with Δδ = 0.16 ppm and the chemical shift of 5′-OH atom of the hydroxyl group moved from δ 5.16 (298 K) to δ 4.98 ppm (338 K) with Δδ = 0.18 ppm. These results demonstrated that these hydrogen atoms participated in the formation of intermolecular hydrogen bonds.
Stoichiometric titration experiments were performed to verify the formation of silver-mediated pairs and determine the amount of silver ions bound to the nucleoside FGd. As shown in Fig. 9, the changes in UV wavelengths were plotted versus the ratio of silver equivalents/FGd, suggesting that two silver ions were captured by one FGd (Fig. 9a and b). Accordingly, positive mode electrospray ionization-mass spectroscopy analysis was carried out and the corresponding silver complexes of 1:
1 and 1
:
2 peaks at 475.1 and 624.1, respectively, were observed (see ESI, Fig. S7†), which provided powerful evidence further indicating that the two silver ions were captured by one FGd. Based on the above results, the possible silver-mediated base pair motifs are shown in Fig. 9c. To validate the assumption, 1H–1H NOE experiments were carried out and the results suggested that C8–H produced a strong NOE at NH2a, NH2b, and NH simultaneously (Fig. 9c), which provided an unambiguous interpretation of the G-ribbon structures.
Fusobacterium nucleatum and Porphyromonas gingivalis, two Gram-negative anaerobes, are the most abundant microorganisms present in the oral cavity during periodontal disease.48,49 In this study, the antibacterial activities of FGd and FGdAg hydrogels in vitro were preliminarily evaluated. Initially, we assessed the biocompatibility of FGd (FGd dissolved in PBS) and FGdAg hydrogels in vitro, the cell viability of the immortalized normal oral keratinocyte cells (NOK-SI) was assessed using CCK8 assay. As shown in Fig. 10, when the concentration of FGd and FGdAg increased to 2.0 mg mL−1, the viability of the NOK-SI cell line was higher than 97%. As the concentration of FGd and FGdAg increased to 8.0 mg mL−1, the viability of NOK-SI cell line was higher than 86%. As expected, these results indicated that the FGd and FGdAg hydrogels had only slight toxicity in vitro to be used as a safe biomaterial. Furthermore, the preliminary in vitro antimicrobial activities of FGd and FGdAg hydrogels on Fusobacterium nucleatum and Porphyromonas gingivalis were evaluated by measuring the inhibition growth diameter and minimal bactericidal concentrations (MBCs). The results presented FGd and FGdAg hydrogels had no obvious inhibition effect on Porphyromonas gingivalis. However, FGdAg hydrogel exhibited excellent antibacterial activities for Fusobacterium nucleatum (MBC: 31.25 μg mL−1), compared to the control group, FGd hydrogel, which exhibited no antibacterial activities, silver ions as positive control (see ESI, Fig. S8†). In Fig. 10c and d, the diameters of Fusobacterium nucleatum inhibiting loops were approximately 0.57, 1.3, 1.9, 2.67 mm for FGdAg hydrogel 31.5, 62.5, 125, and 250 μg mL−1, respectively. Therefore, these findings suggested that FGdAg might be a possible biomaterial for antimicrobial medical applications.
Footnotes |
† Electronic supplementary information (ESI) available: Experimental section and additional figures. CCDC 1588934. For ESI and crystallographic data in CIF or other electronic format see DOI: 10.1039/c8ra02500b |
‡ These authors contributed equally to this work. |
This journal is © The Royal Society of Chemistry 2018 |