Simon
Ristig
,
Diana
Kozlova
,
Wolfgang
Meyer-Zaika
and
Matthias
Epple
*
Inorganic Chemistry and Centre for Nanointegration Duisburg-Essen (CeNIDE), University of Duisburg-Essen, Universitaetsstr. 5-7, 45117 Essen, Germany. E-mail: matthias.epple@uni-due.de
First published on 18th September 2014
A one-pot synthesis of fluorescent bimetallic silver–gold nanoparticles in aqueous medium is presented. Carboxylic acid-functionalized nanoparticles were prepared with different metal compositions from 90:10 to 10:90 (n:n) for silver:gold with a diameter of 1.8 ± 0.4 nm. Pure silver and gold nanoparticles were prepared for comparison. Spectroscopic analyses showed that the ligand, i.e. 11-mercaptoundecanoic acid, binds to the particle surface by the thiol group, leaving the carboxylic acid accessible for further functionalization, e.g. by suitable coupling reactions. Nanoparticles with a silver content up to 60:40 showed autofluorescence with a large Stokes shift of about 250–300 nm (maximum wavelength of the emission between 608 nm and 645 nm). The intracellular localization of bimetallic silver–gold nanoparticles was studied in HeLa cells by confocal laser scanning microscopy (CLSM). The alloyed silver–gold nanoparticles showed no significant cytotoxicity at a metal concentration of 5 μg mL−1 for 24 h, but were cytotoxic to some degree at 50 μg mL−1 at higher silver content.
Bimetallic nanoparticles of silver and gold are readily available in different sizes and compositions due to their similar lattice constants that make mixed crystals over the whole concentration range possible.37–39 The generation of bimetallic clusters of silver and gold is a promising way to bypass the generally weak fluorescence intensity of gold clusters in comparison with other common fluorophores because the bimetallic clusters show a distinctly increased fluorescence quantum yield.40,41 However, only a very few syntheses for ultra-small bimetallic silver–gold nanoparticles have been reported so far. Ganguly et al. synthesized fluorescent silver clusters on a micrometer-sized gold core and observed a synergetic effect between the two noble metals.42 Udayabhaskararao et al. prepared fluorescent alloyed silver–gold clusters by core etching of silver nanoparticles with mercaptosuccinic acid, followed by a galvanic exchange reaction with gold.43 Le Guével et al. synthesized fluorescent bimetallic silver–gold nanoparticles by co-reduction of silver and gold salts in the presence of glutathione.40 Grade et al. prepared bimetallic silver–gold nanoparticles with a diameter of about 4 nm by laser ablation.44
Here we present the synthesis of ultra-small silver–gold nanoparticles with variable composition over the whole concentration range (from silver:gold 90:10 to 10:90) and the investigation of their fluorescent properties. The particles were prepared by co-reduction of silver and gold ions with sodium borohydride in water and simultaneous capping with 11-MUA. As the composition will influence the biological properties, we also studied the effect on HeLa cells.
Silver nitrate was obtained from Roth (p.a.), and HAuCl4 was prepared by dissolution of gold in aqua regia according to standard procedures. Ultrapure water (Purelab ultra instrument from ELGA) was used for all preparation processes.
Differential centrifugal sedimentation (DCS) was performed with a CPS Instruments Disc Centrifuge DC 24000 (24000 rpm, 28978 g). As a density gradient, two sucrose solutions (8 wt% and 24 wt%) were used and capped with 0.5 mL dodecane as the stabilizing agent. The calibration standard was a poly(vinyl chloride) (PVC) latex in water with a particle size of 476 nm provided by CPS instruments. Calibration was carried out prior to each run. A sample volume of 100 μL was used.
Fourier transform infrared spectroscopy (FTIR) was carried out with a Bruker Alpha-Platinum FTIR with an attenuated total reflection (ATR) sampler. Prior to the measurements the samples were lyophilized with a Christ Alpha 2-4 LSC instrument.
Ultraviolet-visible spectroscopy (UV-vis) was performed with a Varian Cary 300 instrument. Suprasil® microcuvettes with a sample volume of 700 μL were used.
1H-NMR-spectroscopy was carried out with a Bruker DPX 300 instrument. The spectra were recorded with 128 scans in CDCl3 or D2O with NaOD.
Fluorescence spectroscopy was performed with an Agilent Cary Eclipse spectrophotometer. Suprasil® cuvettes with a sample volume of 3.5 mL were used.
Atomic absorption spectroscopy was carried out with a Thermo Electron M-Series spectrometer with a graphite tube furnace after dissolving the particles in aqua regia.
Confocal laser scanning microscopy was performed with Leica TCS SP5 instrument using a 63×/NA 1.2 water objective. Alloyed silver–gold nanoparticle fluorescence was excited at 405 nm; the emission was recorded through a 635 nm long-pass filter. The immunofluorescence of actin staining was excited at 488 nm.
For uptake studies, HeLa cells were cultured in DMEM medium, supplemented with 10% fetal bovine serum (FBS), 100 U mL−1 penicillin, and 100 U mL−1 streptomycin at 37 °C in a humidified atmosphere with 5% CO2. 12 h prior to the uptake experiments, the cells were trypsinized and seeded in cell culture dishes with 1 × 105 cells per well in 0.5 mL cell culture medium. For the uptake studies, the cells were incubated with 50 μg mL−1 Ag:Au 30:70 or Ag:Au 50:50 nanoparticles in serum-free medium for 5 h or in medium with 10% FBS for 5 h and 24 h. After selected times, cells were washed five times with PBS to remove adhering nanoparticles, fixed with 4% aqueous formalin for 20 min at room temperature. For immunofluorescence staining, the cells were incubated with Alexa-488-conjugated phalloidin (Invitrogen, Germany). Finally, the cells were studied by confocal laser scanning microscopy (Leica TCS SP5) using a 63×/NA 1.2 water objective.
Fig. 1 Transmission electron micrograph of Ag:Au 30:70 nanoparticles (A) and Ag:Au 20:80 nanoparticles (B). |
Disc centrifugal sedimentation (DCS) supported these findings, giving average particle diameters between 1.7 nm and 2.1 nm. It is noteworthy that the sizes derived from DCS were slightly smaller than those derived from TEM. As the density of the nanoparticles is a fixed parameter in DCS runs (which we had set to the weighed density of silver and gold, using the nanoparticle composition), the smaller size is a result of the shell of the organic ligand which lowers the effective density of the whole particle and slows down the sedimentation. DCS data were collected from 150 nm to 1 nm. We obtained narrow size distributions, indicating that the nanoparticles were monodisperse and stable against agglomeration (Table 1). No larger particles were observed by DCS. Fig. 2 shows a representative DCS size distribution of particles with the composition of Ag:Au 10:90. Dynamic light scattering was not possible due to the small particle size.
Theoretical composition Ag:Au in mol% | 0:100 | 10:90 | 20:80 | 30:70 | 40:60 | 50:50 | 60:40 | 70:30 | 80:20 | 90:10 | 100:0 |
Experimental composition Ag:Au in mol% | 0:100 | 12:88 | 20:80 | 28:72 | 40:60 | 50:50 | 63:37 | 68:32 | 79:21 | 93:7 | 100:0 |
Diameter (DCS) in nm | 1.5 | 1.7 | 1.8 | 1.8 | 1.8 | 1.8 | 2.1 | 2.0 | 2.1 | 2.1 | 2.2 |
The composition of the nanoparticles was determined by atomic absorption spectroscopy (AAS). The experimental data are shown in Table 1. The experimental molar ratios of silver and gold agree well with the expected values.
The stability against agglomeration depends on the pH of the dispersion and the protonation equilibrium of the terminal carboxylic acid groups of the ligand. We used a borate/hydrochloric acid buffer to keep the pH at 9. Borate was chosen because it is also generated during the reduction with sodium borohydride, thus avoiding additional chemical components in the system. The deprotonated carboxylic acid led to high electrostatic stability, even in the presence of a high electrolyte concentration (a final buffer concentration of 20 mM tetraborate).
Although the nanoparticles were too small to conduct reliable dynamic light scattering measurements, it can be safely assumed that the nanoparticles possess a negative zeta potential and a point of zero charge similar to the pKa of 11-MUA. This was reported to be 5.4 for a monolayer of 11-MUA on a gold surface.45 We can conclude that at a pH below 5, the carboxylic group will be mostly protonated, and agglomeration will occur.
The colour of the purified and concentrated dispersions ranged from colourless (high Au content) to light brown (high Ag content) under visible light. Pure gold nanoparticles and samples with a molar Ag:Au composition between 10:90 and 60:40 exhibited good visible fluorescence under a 254/365 nm fluorescence lamp. Nanoparticles with a higher silver content than 60 mol% and pure silver nanoparticles did not show autofluorescence. This can most likely be attributed to the slightly larger particle size, as silver clusters were reported to show autofluorescence only at diameters of 1.3 nm and below.29,30 The colour of the emitted fluorescence ranged from bright orange (high Au content) to red (high Ag content). To investigate the optical properties of the samples further, we used fluorescence spectroscopy. The absorption spectra of the nanoparticles were almost symmetric and had absorption maxima at wavelengths between 250 nm and 330 nm, although no clear trend was visible (Fig. 3). The symmetric emission spectra showed a large Stokes shift of up to 360 nm (Ag:Au 20:80), consistent with previous reports.25,41 The large shifts which are similar to those in luminescent Au(I) complexes can be attributed to electronic d–sp electronic transitions.46,47 The maximum emission wavelength showed a redshift with a clear trend from 608 nm (Ag:Au 10:90) to 645 nm (Ag:Au 60:40). Interestingly, this red shift of the maximum absorption wavelength was increasing with increasing silver content, consistent with the results reported for other silver–gold nanoparticles.40 For pure gold nanoparticles (1.5 nm), we measured an absorption maximum at 320 nm and an emission maximum at 607 nm.
The fluorescence of the nanoparticles remained visible when the particles were precipitated and freeze-dried, indicating a high stability of the noble metal–sulphur bond. The emission spectra of the nanoparticles only changed slightly in intensity when the dispersions were irradiated at different wavelengths (Fig. 4). Neither the maximum excitation wavelength nor the maximum emission wavelength shifted significantly, proving that the detected signal is indeed fluorescence and not just scattered light.
The photostability of the nanoparticles was studied for the Ag:Au 10:90 samples in a permanent irradiation experiment. The nanoparticle dispersion was continuously irradiated inside a fluorescence spectrometer with a Xenon flash lamp at 300 nm for 180 min. Every 8 min, an emission spectrum was recorded. The fluorescence intensity at 610 nm showed only a slow decay over time from an intensity of 555 units at the first measurement to 507 units after 180 min (Fig. 4). This decrease in intensity of just about 9% demonstrates the excellent stability of the nanoparticles towards photobleaching. The experiment was only carried out for the Ag:Au 10:90 samples, but we do not expect a significant difference for the samples with another composition due to their structural similarity (alloyed metallic nanoparticles).
IR-spectroscopy and 1H-NMR spectroscopy can be used to further assess the properties of nanoparticles, e.g. ligand orientation.34,48–50 The orientation is an important factor if a bifunctional ligand is attached because the accessibility of specific functional groups is critical for a subsequent chemical modification of the particle surface. In IR-spectroscopy, the disappearance of a characteristic group, in this case the S–H and COOH bands, can be interpreted as evidence for a bond from the ligand to the particle surface through this specific functionality.
Three representative FTIR-spectra are shown in Fig. 5. The free ligand shows distinctive bands at 2915/2848 cm−1 (symmetric and asymmetric –CH2– stretching), 2550 cm−1 (S–H stretching), 1690 cm−1 (CO stretching), 1290–1188 cm−1 (–CH2– progression bands) and 933 cm−1 (out-of-plane OH bend), an indication of hydrogen bridging from the formation of carboxylic acid dimers. Purified, buffered (pH 9) and freeze-dried Au:Ag 50:50 nanoparticles show sharp –CH2– bands at 2916/2847 cm−1 and weak progression bands at 1297–1209 cm−1 which indicate an ordered all-trans structure of the aliphatic chain of the ligand.51,52 The absence of the S–H band (∼2550 cm−1) indicates that the mercaptoundecanoic acid is bound to the metal by the thiol group. A shift of the CO absorption to 1564 cm−1 indicates a deprotonated carboxylate group, consistent with the precipitation of the sample at pH 9.
The third spectrum was recorded from Au:Ag 50:50 particles that were precipitated from dispersion with hydrochloric acid, i.e. at low pH. Here we see characteristic bands of –CH2– at 2916/2847 cm−1, weak progression bands at 1294–1195 cm−1, and again a missing S–H band. The CO stretching at 1699 cm−1 indicates the presence of the protonated terminal carboxylic acid.
1H-NMR spectroscopy was used to obtain further information about the ligand orientation on the particle surface because the interaction of a ligand with a nanoparticle surface leads to distinct changes in the resulting spectrum compared to the dissolved ligand molecules. Adsorbed (chemisorbed) molecules show peak broadening and a different chemical shift. The broadening is a result of fast spin relaxation from dipolar interactions with the metallic core and increases with proximity of the methylene groups to the nanoparticle surface. Furthermore, a change in magnetic susceptibility at ligand–metal boundary and spin–spin relaxation broadening which depends on the velocity of the nanoparticles in solution may contribute to a significant difference between the free ligand and adsorbed species, up to a complete disappearance of the peaks of the methylene groups that are closest to the nanoparticle. This allows the identification of terminal and particle-facing groups and thus permits the assessment of the ligand orientation.34,49,53–55
In Fig. 6, the 1H-NMR spectra of pure 11-MUA (300 MHz, D2O, 25 μL NaOD, δ = 1.28 (m, 12H, CH2), δ = 1.53 (m, 4H, CH2), δ = 2.16 (t, 2H, CH2–COO−), δ = 2.49 ppm (t, 2H, CH2–S−)), and of purified Ag:Au 70:30 nanoparticles (300 MHz, D2O, 25 μL NaOD, δ = 1.0–1.48 (br m, 12H, CH2), δ = 1.48–1.85 (br m, 4H, CH2), δ = 2.10–2.42 (br m, t, 2H, CH2–COO−)) are shown. In comparison with dissolved 11-MUA, the peaks of the functionalized nanoparticles are strongly broadened and no free ligand is present. Obviously, the α-methylene protons next to the thiol group (4) have disappeared. This indicates that the ligand is bound to the particle surface with the thiol group, leaving the terminal carboxylic acid exposed for stability manipulation through pH-changes and possible modification of the particles via coupling reactions. In the ligand spectrum, a small triplet at 2.76 ppm (*) is visible which originates from the α-methylene group of the disulphide-form of the ligand.49 In the spectrum of the nanoparticles, this triplet is found at 2.90 ppm. The triplet in the spectrum of the nanoparticles, visible overlapping with a broad peak at 2.16 ppm, can be attributed to the methylene group next to the carboxylate (3). The signal is the least broadened, because of its maximum distance to the metal surface. The overlapping broadened peak, however, indicates that the ligand shell is not completely oriented with the thiol-groups towards the gold but with some carboxylate groups located in proximity to the nanoparticle surface as well.
Fig. 6 Representative 1H-NMR of 11-MUA (top) and purified Ag:Au 70:30 nanoparticles, functionalized with 11-MUA (bottom). |
The cytotoxicity of the alloyed silver–gold nanoparticles was analysed by the MTT assay (Fig. 7). For a better comparison between the samples, the total metal concentrations of 5 μg mL−1 (5 ppm) and 50 μg mL−1 (50 ppm) were used. The calculated nanoparticle concentrations for the different particle samples, based on the average diameter in DCS and the AAS values for silver and gold, are given in Table 2. Previously, we had reported that tris(3-sulfonatophenyl)phosphine- or poly(N-vinylpyrrolidone)-stabilized gold nanoparticles with a diameter of 5 nm were not toxic for hMSCs after 24 h at 5–20 μg mL−1.38 Here we found a decrease of the cell viability after 24 h incubation with 50 μg mL−1 of 11-MUA-stabilized small gold nanoparticles (Fig. 7A). Small gold nanoparticles (diameter 1.4 nm) were shown previously to be more cytotoxic than smaller or larger ones.56,57
Fig. 7 MTT assays of HeLa cells after incubation with different concentrations of alloyed silver–gold nanoparticles for 24 h (A) and 72 h (B). |
Theoretical composition Ag:Au in mol% | 0:100 | 10:90 | 20:80 | 30:70 | 40:60 | 50:50 | 60:40 | 70:30 | 80:20 | 90:10 | 100:0 |
Nanoparticle concentration at 5 μg mL−1 metal in nmol mL−1 | 0.24 | 0.17 | 0.15 | 0.15 | 0.16 | 0.17 | 0.11 | 0.14 | 0.13 | 0.14 | 0.14 |
Nanoparticle concentration at 50 μg mL−1 metal in nmol mL−1 | 2.43 | 1.72 | 1.49 | 1.54 | 1.61 | 1.68 | 1.11 | 1.38 | 1.29 | 1.43 | 1.42 |
Pure silver nanoparticles displayed no toxic effect for HeLa cells after 24 h and 72 h at a metal concentration of 5 μg mL−1. With increasing concentration of silver nanoparticles (50 μg mL−1), the cell viability rapidly decreased, as expected for the cytotoxic silver ion.58 Biological studies on ligand-free gold–silver nanoalloys were reported by Barcikowski et al. They found an increasing cytotoxicity with increasing silver content and ascribed this effect to released silver ions, possibly enhanced by the presence of the noble metal gold, forming a local electrochemical element with silver.39,44
Interestingly, the increase of the dose of silver in alloyed silver–gold nanoparticles did not lead to a monotonous decrease of cell viability. In particular, the Ag:Au 90:10 nanoparticles were more toxic than pure silver nanoparticles (100:0). This is an unexpected result that cannot be explained so far and deserves further attention. However, we have found that this discontinuity was reproducible. Barcikowski et al. reported similar observations with alloyed silver–gold nanoparticles from laser ablation in mammalian gametes.39
Uptake studies were performed on HeLa cells with two types of silver–gold nanoparticles, i.e. Ag:Au 30:70 and Ag:Au 50:50 nanoparticles in serum-free medium for 5 h. To avoid the interaction of the nanoparticles with serum proteins that may act as a protective layer, shielding the nanoparticle surface from interactions with the cells,29,59–61 the cellular uptake studies were performed in the absence of proteins. In Fig. 8, it is clearly visible that the bimetallic nanoparticles are mostly localized on the cell membrane. Due to the very small size of investigated nanoparticles, a diffuse nature of fluorescence was observed. To shed further light on the effect of protein adsorption on the nanoparticle surface, the cellular uptake of silver–gold nanoparticles was investigated in serum-supplemented medium.
The uptake studies in serum-supplemented medium showed a less pronounced localization of the nanoparticles around the cell membrane compared with the cellular uptake in serum-free medium after 5 h (Fig. 9). Shang et al. showed a reduced amount of internalized silver nanoparticles in the presence of proteins.29 This observation can be explained by the better stability of the nanoparticles in protein-containing medium.62 In general, the uptake and the cytotoxicity of small metallic nanoparticles depend on their size44 and their surface functionalization.47 In this case, the uptake mechanism is not known, but it is likely that cellular uptake occurs by endocytosis as observed for nanoparticles in general63–65 and small gold nanoparticles in HeLa cells in particular.66 Recent studies have also demonstrated a size-dependent toxicity of gold nanoparticles.67,68 The ligand chemistry may also affect the cytotoxicity of gold nanoclusters.57 Polavarapu et al. demonstrated a rather low toxicity of glutathione-capped gold clusters towards human neuroblastoma cells even at very high concentrations (400 μg mL−1).69
The incubation of HeLa cells with Ag:Au 30:70 nanoparticles and Ag:Au 50:50 nanoparticles for 24 h in serum-supplemented medium clearly showed the red fluorescing particles in the cytoplasm (Fig. 10) around the nucleus, indicating the successful internalization of bimetallic nanoparticles in the cells. The red fluorescent dots within the cells are not individual nanoparticles but a number of accumulated nanoparticles in endosomal vesicles.66,70
Note that these results were obtained with one cell line (HeLa) and cannot be quantitatively transposed to other cell lines. This is due to the variability of cell lines towards particles, as it was summarized for silver.58 However, the general trends should hold for other cell lines as well.
This journal is © The Royal Society of Chemistry 2014 |