Preparation of silver colloids with improved uniformity and stable surface-enhanced Raman scattering
© Meng et al. ; licensee Springer. 2015
Received: 17 October 2014
Accepted: 10 January 2015
Published: 5 February 2015
Silver colloids of uniform shape and size are prepared by a two-step reduction. Small silver particles form initially by the rapid reduction of silver nitrate with sodium citrate at 100°C and then grow at 92°C. The reaction processes and resulting silver colloids are characterized by transmission electron microscopy, ultraviolet–visible absorption spectrophotometry, zeta-potential measurements, and Ag+ concentration analysis. The surface-enhanced Raman scattering (SERS) activity of the silver colloids is then investigated, using crystal violet (CV) as a SERS probe. The silver colloids exhibit uniform shape and size and stable SERS activity. The average size of the silver particles is 47 nm (14% relative standard deviation), while the average sizes of the silver colloids prepared at 100°C and 92°C are 41 (30%) and 71 nm (33%), respectively.
Surface-enhanced Raman scattering (SERS) was first observed from pyridine adsorbed on a roughened silver electrode by Fleischmann et al. . SERS has since attracted much attention because of its high sensitivity to low analyte concentrations. The sensitivity enhancement factor is on the order of 105 to 106 but can reach 1014 to 1015 . Previous SERS studies of bulk samples have elucidated the SERS mechanisms and shown that electromagnetic and chemical enhancements operate simultaneously. The former is due to surface plasmon resonance (SPR) confined to the near-surface region, while the latter is due to surface active sites or charge transfer between the adsorbate and substrate [3,4]. Regardless of electromagnetic or chemical enhancement, active substrates and adsorbed analytes (mono- or multi-layers) are both necessary for producing high-quality SERS spectra. Substrate activity depends on the scale of its features (10 to 100 nm) and its morphology [5-7].
Many SERS-compatible active substrates have been investigated. Ag and Au are the most widely studied, because of their high enhancement factors, but transition metals, semiconductors, and other materials have also been studied [8-10]. The morphologies of SERS substrates can include roughened electrodes, colloids, island films, and nanoarrays. Silver and gold colloids, especially citrate-reduced colloids, are the most commonly used SERS substrates because they are easily prepared and can be well characterized. The shape and size of their particles can also be controlled by inexpensive, versatile approaches.
Stable gold colloids with narrow size distributions were recently synthesized by a reduction with citrate . Improved shape/size control of silver particles - along with the preparation of uniform, stable silver colloids - has become an active research area. Citrate-reduced silver colloids can be prepared by reducing silver nitrate with sodium citrate at its boiling point, according to Lee and Meisel , wherein citrate also stabilizes the dispersion. In contrast to gold colloids, silver colloids can exist as prisms, rods, and disks of varying size, though spherical particles are the most common. Methods for controlling particle morphologies include adding stabilizers, adjusting heating and stirring rates, changing the citrate/silver nitrate ratio, and adjusting the pH [13,14]. Stable, monodisperse sols can be obtained by such methods. However, some added substances decrease the SERS activity of silver particles in substrates used for diagnosing and characterizing analytes. This is attributable to competitive adsorption of the analyte and added substance. Thus, understanding the nucleation mechanism of silver colloidal particles is important for improving size control.
Probe molecules are used to investigate the SERS activity of substrates and usually contain azo, carboxyl, or thiol groups. These analytes strongly adsorb to a substrate’s surface, which maximizes SERS enhancement. Crystal violet (CV) exhibits SERS activity on silver surfaces [15,16].
In the current study, silver colloids are prepared by a two-step reduction of silver nitrate at high (100°C) and low (92°C) temperatures in the presence of sodium citrate. These uniformly sized silver particles have an average size of 47 nm and a relative standard deviation of 14%. CV is used as a SERS probe, and the silver particles exhibit high SERS activity compared with the colloids prepared at 100°C or 92°C.
Polyvinyl alcohol (PVA), CV (C25H30ClN3), silver nitrate (AgNO3), sodium citrate (Na3C6H5O7 · 2H2O), 2,4,5,7-tetrabromofluorescein (TBF), and 1,10-phenanthroline (PHEN) were all of analytical grade and were obtained from Sinopharm Chemical Reagent Co., Ltd. Ultraviolet–visible (UV–vis) absorption spectra were recorded on a TU-1810 spectrophotometer (Beijing Purkinje General Instrument, Beijing, China), using 2 mm-path-length quartz cells. Aliquots of the reaction solutions were removed at different times and cooled immediately in ice water to prevent further reaction. Measurements were taken from undiluted samples. Zeta potentials were measured using a Malvern Zetasizer 90 instrument. Samples for Raman spectroscopy measurements were prepared by adding 1 × 10−4 mol L−1 CV solution to the silver colloids. Samples were incubated for 30 min, and Raman spectra were recorded on a Renishaw Micro-Raman spectroscopy system and averaged over seven measurements. Excitation was provided by an Ar ion laser (514 nm). A 50×, 0.50 NA Leica objective lens with a long working distance was used to focus the laser on the surface of the silver colloid samples. Excitation power was 20 mW, integration time was 10 s, and the calculated spot size was about 1.25 μm. A droplet of silver colloid suspension was allowed to dry on a copper grid for transmission electron microscopy (TEM) observations. TEM images were collected using a Tecnai 12 (Philips) microscope, operated at 120 kV.
Preparation of samples
Sample A was prepared as follows: 194 mL of distilled water in a three-neck flask was heated to 100°C under reflux with vigorous stirring. Upon boiling, 2 mL of 0.1 mol L−1 AgNO3 and 4 mL of 1% sodium citrate were added successively to start the reaction. The solution was refluxed for 40 min then allowed to cool to room temperature. Sample B was prepared similarly, except the temperature was 92°C and the solution was refluxed for 100 min. Sample C was prepared by a two-step reduction: 2 mL of 0.1 mol L−1AgNO3 and 4 mL of 1% sodium citrate were added to 170 mL of boiling distilled water under reflux, and the reaction was allowed to continue for 4 min at 100°C. The reaction vessel was then transferred to a water bath at 92°C and allowed to remain there for 80 min to continue the reduction of silver nitrate. Upon transfer, the temperature of the reaction mixture was quickly reduced to 92°C by adding cold water. The three silver colloid samples were all adjusted to a final volume of 200 mL. All solutions were continuously stirred during preparation. All glassware was cleaned with dilute nitric acid and thoroughly rinsed with distilled water before use.
Determination of Ag+
The modified spectrophotometric determination of Ag+ was based on a method developed by Mohamed and Roland . A stock solution was prepared by adding 25 mL of 5 × 10−4 mol L−1 PHEN, 0.6 mL of 2 × 10−3 mol L−1 TBF, and 40 mL of 0.1% PVA into a 100 mL flask and diluting with water to produce a volume of 100 mL. Then, 10 to 35 μL of 1 × 10−3 mol L−1 silver nitrate was added to 5 mL of this stock solution. The characteristic absorbance of the ternary [PHEN-Ag-PHEN]2TBF complex at 548 nm was recorded in the UV–vis absorption spectrum, using 1 cm-path-length quartz cells. PVA is a stabilizer for the ternary [PHEN-Ag-PHEN]2TBF complex and can improve its solubility and analytical sensitivity. The results from several samples showed that the maximum absorbance at 548 nm increased linearly with increasing Ag+ concentration in the range of 2 × 10−6 to 7 × 10−6 mol L−1. A regression equation of A = 50, 310c (mol L−1) was obtained, where A indicates maximum absorbance and c the Ag+ concentration. A 10 to 30 μL aliquot of reaction solution was added to 5 mL of stock solution to determine Ag+ concentration. The silver-particle absorbance at 548 nm was <0.01 for each sample, so centrifugation was not necessary.
Results and discussion
The widely used method of preparing silver colloids by reduction with sodium citrate was first proposed by Lee and Meisel . Different theories for the silver-particle-formation mechanism have excited much debate, a comprehensive study on which was performed by Munro et al. . Spectroscopic results for UV–vis absorption and photon correlation suggest that the initial reduction of Ag+ occurs within 2 min of adding citrate, (forming the initial 60- to 80-nm-diameter particles). Subsequent heating disperses the large particles, yielding a semi-monodisperse silver colloid with a mean particle diameter of 27 nm. The maximum absorption wavelength (λ max) blueshifts, while the maximum absorbance increases during dispersion. Alternative colloid-formation mechanisms have also been proposed: Pillai and Kamat  suggested that only a few silver seed crystals form during the initial citrate-reduction procedure. In this framework, the seeds strongly complex with citrate anions and then grow into larger particles until electrostatic repulsion prevents further aggregation. Larger particles continue to grow at the expense of smaller ones, via Ostwald ripening.
These details of the silver-particle-formation mechanism suggest that heating, stirring, the time and rate of reagent addition, and reagent concentrations should affect particle formation. Different mechanisms may occur under different reaction conditions. Aggregation, dispersion, nucleation, seed formation, and crystal growth may coexist (and be balanced) in the reaction procedure. Dong and Yang  controlled the nucleation and growth of silver particles by adjusting the pH.
The formation of silver particles is often investigated using UV–vis absorption spectroscopy, which does not always provide a comprehensive understanding of the formation mechanism. Crystallization consists of nucleation, seed crystal formation, and crystal growth. Nucleation involves the clustering of molecules of a critical size, which comprise nuclei. Once these nuclei form, they quickly grow into seed crystals, which trigger the crystal-growth process. Nucleation remains difficult to observe, even with current TEM technology. Nevertheless, TEM and other methods suitable for characterizing Ag+ should be used to more clearly understand the formation of silver particles.
Many published studies have addressed Ag+ detection by means such as UV–vis absorption and fluorescence spectroscopies and electrodes with Ag+ selectivity. Other more complex spectrometric techniques involve flame and electrothermal atomic adsorption spectrometry (FAAS and ETAAS) as well as inductively coupled plasma mass spectrometry.
Detection of Ag+ in silver colloids is difficult because of its low concentration and matrix effects. Some Ag+ adsorbs on the silver particles. The adsorption of ions and subsequent disturbance of Ag atoms mean that the Ag+ concentration cannot be readily determined using selective electrodes or atomic spectroscopy, unless the Ag+ and Ag particles are separated. Thus, in this study, we employ a modified UV–vis spectrometric process to determine the aqueous Ag+ content.
Sample B is prepared by reduction at low temperature to prevent continuous seed formation. During stage 1 (0 to 20 min) the solution is colorless and does not absorb (Figure 1b). The longer duration of stage 1 compared with sample A (100°C) is attributed to the slower reaction at 92°C. During stage 2 (20 to 75 min), the λ max and maximum absorbance increase with decreasing Ag+ concentration, indicating the growth of silver seeds. In contrast to stage 2 for sample A, few silver seeds (approximately 10 nm) are observed in the TEM images of sample B during stage 2 (Figure 2e); this is attributed to the slower reaction, which hinders seed formation. Figure 2f shows that the average particle size of sample B is 71 nm, with a relative standard deviation of 33%. The lower reaction rate results in fewer seeds, which grow larger because they are subjected to the same Ag+ concentration as sample A. Continuous nucleation is avoided, but the particle size range is larger because of the larger size distribution of seeds (Figure 2d). Heterogeneous nucleation is the predominant nucleation type for a low Ag+ reduction rate and low supersaturation.
The zeta potentials of samples A, B, and C are −40.3, −41.1, and −39.8 mV, respectively. These similar potentials arise from the adsorption of citrate and its carboxylate oxidation products  on the silver-particle surface. Colloidal silver particles are negatively charged and thus attract positively charged CV. The zeta potentials of samples B and C are no greater than that of sample A, despite these samples’ larger particle sizes and lower surface areas. This implies that the adsorption of citrate is saturated in all three samples.
Samples for Raman spectrometry are prepared by mixing 5 mL of silver colloid with 50 μL of 1 × 10−4 mol L−1 CV solution (with a CV concentration of 1 × 10−6 mol L−1). No significant changes in the UV–vis absorption spectra of the silver colloids are observed in the presence of CV, indicating that CV does not induce particle aggregation. SERS spectra are recorded without the addition of active substances such as halide anions. The addition of such substances tends to aggregate the particles, causing stronger SPR, and thus chemically enhancing SERS activity . Nie suggested that aggregation also produces hot junctions, which can increase SERS intensity . This phenomenon was not observed in the present study.
where θ is the fraction of adsorbed CV at equilibrium and is estimated to be 0.09 , C is the concentration of CV in the solution (C sol 1 × 10−4 mol L−1) or in the silver colloids (C SERS 6 × 10−8 mol L−1), and I is the intensity of a band of the Raman spectrum in solution (I sol) or of the SERS spectrum (I SERS). Using this expression, we obtain an estimated EF value of approximately 9.5 × 103. Generally speaking, aggregation caused by active substances such as Cl−1, Br−1, and I−1 will further increase the enhancement factor by one to three orders of magnitude through the intense magnetic fields created at particle junctions, but SERS signals are not stable in this case. Thus, the actual overall EF can exceed 9.5 × 103.
Silver colloids are prepared in a two-step reduction, without capping agents. Small silver particles are generated by rapid reduction with sodium citrate at 100°C and subsequent growth at 92°C. Two other silver colloids are prepared at 100°C and 92°C for comparison. The silver colloids prepared by the two-step reduction exhibit greater uniformity in size and shape. TEM, UV–vis absorption spectroscopy, and Ag+ concentration measurements during reaction provided insight into the silver-particle-formation mechanism. The average particle size for the two-step reduction was 47 nm, with a 14% relative standard deviation, whereas the sizes (relative standard deviations) of particles prepared at 100°C and 92°C are 41 (30%) and 71 nm (33%), respectively. All silver colloids are negatively charged and have equivalent zeta potentials. CV is used as a SERS probe. The SERS signals of CV on the colloids had an improved stability and intensity, demonstrating the colloids’ viability for applications in quantitative SERS analysis.
This study was supported by the National Natural Science Foundation of China (Grant No. 50972059), Intergovernmental Cooperation Projects in Science and Technology of the Ministry of Science and Technology of PRC (No. 5), and the Department of Education of Jiangsu Province (Grant No. CXLX11_0245).
- Fleischmann M, Hendra PJ, McQuillan AJ. Raman spectra of pyridine adsorbed at a silver electrode. Chem Phys Lett. 1974;26:163–6.View ArticleGoogle Scholar
- Nie S, Emory SR. Probing single molecules and single nanoparticles by surface-enhanced Raman scattering. Science. 1997;275:1102–6.View ArticleGoogle Scholar
- Campion A, Kambhampati P. Surface-enhanced Raman scattering. Chem Soc Rev. 1998;27:241–50.View ArticleGoogle Scholar
- Meng W, Hu F, Zhang LY, Jiang XH, Lu LD, Wang X. SERS and DFT study of crystal violet. J Mol Struct. 2013;1035:326–31.View ArticleGoogle Scholar
- Chai P, Liu J, Tang J, Shi Y, Xue C, Wen H. Base effects on fluorescence and surface-enhanced Raman scattering of crystal violet adsorbed on Au nanoparticles surface. J Nanosci Nanotechnol. 2013;13:1011–6.View ArticleGoogle Scholar
- Yuan J, Lai Y, Duan J, Zhao Q, Zhan J. Synthesis of a β-cyclodextrin-modified Ag film by the galvanic displacement on copper foil for SERS detection of PCBs. J Colloid Interface Sci. 2012;365:122–6.View ArticleGoogle Scholar
- Novara C, Petracca F, Virga A, Rivolo P, Ferrero S, Chiolerio A, et al. SERS active silver nanoparticles synthesized by inkjet printing on mesoporous silicon. Nanoscale Res Lett. 2014;9:1–7.View ArticleGoogle Scholar
- Quagliano LG. Observation of molecules adsorbed on III-V semiconductor quantum dots by surface-enhanced Raman scattering. J Am Chem Soc. 2004;126:7393–8.View ArticleGoogle Scholar
- Yang Y, Matsubara S, Nogami M, Shi J. Controlling the aggregation behavior of gold nanoparticles. Mater Sci Eng B. 2007;140:172–6.View ArticleGoogle Scholar
- Chervinskii S, Matikainen A, Dergachev A, Lipovskii A, Honkanen S. Out-diffused silver island films for surface-enhanced Raman scattering protected with TiO2 films using atomic layer deposition. Nanoscale Res Lett. 2014;9:1–8.View ArticleGoogle Scholar
- Daniel MC, Astruc D. Gold nanoparticles: assembly, supramolecular chemistry, quantum-size-related properties, and applications toward biology, catalysis, and nanotechnology. Chem Rev. 2004;104:293–346.View ArticleGoogle Scholar
- Lee PC, Meisel D. Adsorption and surface-enhanced Raman of dyes on silver and gold sols. J Phys Chem. 1982;86:3391–5.View ArticleGoogle Scholar
- Qin Y, Ji X, Jing J, Liu H, Wu H, Yang W. Size control over spherical silver nanoparticles by ascorbic acid reduction. Colloids Surf A: Physicochem Eng Aspects. 2010;372:172–6.View ArticleGoogle Scholar
- Dong X, Ji X, Wu H, Zhao L, Li J, Yang W. Shape control of silver nanoparticles by stepwise citrate reduction. J Phys Chem C. 2009;113:6573–6.View ArticleGoogle Scholar
- Liu RM, Kang YP, Zi XF, Feng MJ, Cheng M, Si MZ. The ultratrace detection of crystal violet using surface enhanced Raman scattering on colloidal Ag nanoparticles prepared by electrolysis. Chin Chem Lett. 2009;20:711–5.View ArticleGoogle Scholar
- Andrzej K. Raman studies of rhodamine 6G and crystal violet sub-monolayers on electrochemically roughened silver substrates: Do dye molecules adsorb preferentially on highly SERS-active sites? Chem Phys Lett. 2005;414:271–5.View ArticleGoogle Scholar
- El-Ghamry MT, Frei RW. Spectrophotometric determination of trace amounts of silver (I). Anal Chem. 1968;40:1986–90.View ArticleGoogle Scholar
- Munro CH, Smith WE, Garner M, Clarkson J, White PC. Characterization of the surface of a citrate-reduced colloid optimized for use as a substrate for surface-enhanced resonance Raman scattering. Langmuir. 1995;11:3712–20.View ArticleGoogle Scholar
- Pillai ZS, Kamat PV. What factors control the size and shape of silver nanoparticles in the citrate ion reduction method? J Phys Chem B. 2004;108:945–51.View ArticleGoogle Scholar
- Maillard M, Huang P, Brus L. Silver nanodisk growth by surface plasmon enhanced photoreduction of adsorbed [Ag+]. Nano Lett. 2003;3:1611–5.View ArticleGoogle Scholar
- McFarland AD, Van Duyne RP. Single silver nanoparticles as real-time optical sensors with zeptomole sensitivity. Nano Lett. 2003;3:1057–62.View ArticleGoogle Scholar
- LaMer VK, Dinegar RH. Theory, production and mechanism of formation of monodispersed hydrosols. J Am Chem Soc. 1950;72:4847–54.View ArticleGoogle Scholar
- Hu F, Meng W. Study on homogeneous nucleation of silver colloids. J Huazhong Norm Univ Nat Sci. 2012;46:71–4.Google Scholar
- Henglein A, Giersig M. Formation of colloidal silver nanoparticles: capping action of citrate. J Phys Chem B. 1999;103:9533–9.View ArticleGoogle Scholar
- Link S, El-Sayed MA. Spectral properties and relaxation dynamics of surface plasmon electronic oscillations in gold and silver nanodots and nanorods. J Phys Chem B. 1999;103:8410–26.View ArticleGoogle Scholar
- Otto A, Bruckbauer A, Chen YX. On the chloride activation in SERS and single molecule SERS. J Mol Struct. 2003;661–662:501–14.View ArticleGoogle Scholar
- Doering WE, Nie S. Single-molecule and single-nanoparticle SERS: examining the roles of surface active sites and chemical enhancement. J Phys Chem B. 2001;106:311–7.View ArticleGoogle Scholar
- Cañamares MV, Chenal C, Birke RL, Lombardi JR. DFT, SERS, and single-molecule SERS of crystal violet. J Phys Chem C. 2008;112:20295–300.View ArticleGoogle Scholar
- Upender G, Sathyavathi R, Raju B, Bansal C, Narayana RD. SERS study of molecules on Ag nanocluster films deposited on glass and silicon substrates by cluster deposition method. J Mol Struct. 2012;1012:56–61.View ArticleGoogle Scholar
- Meng W, Jiang XH, Lu LD, Wang X. Adsorption of crystal violet onto the surface of silver colloids. Chin J Spectro Lab. 2013;30:117–21.Google Scholar
This is an Open Access article distributed under the terms of the Creative Commons Attribution License (http://creativecommons.org/licenses/by/4.0), which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly credited.