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Journal of Nanomaterials
Volume 2012 (2012), Article ID 387581, 8 pages
Glassy Carbon Electrode-Supported Au Nanoparticles for the Glucose Electrooxidation: On the Role of Crystallographic Orientation
1Centro de Investigación y Desarrollo Tecnológico en electroquímica (CIDETEQ), Parque Tecnológico Querétaro-Sanfandila, 76703 Pedro Escobedo, QRO, Mexico
2División de Investigación y Posgrado, Facultad de Ingeniería, Universidad Autónoma de Querétaro, 76010 Cerro de las Campanas, QRO, Mexico
Received 23 February 2012; Accepted 14 June 2012
Academic Editor: Sergio J. Mejía-Rosales
Copyright © 2012 M. Guerra-Balcázar et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.
Glucose electrooxidation in alkaline solution was examined using glassy carbon electrodes modified with Au nanoparticles. Au nanoparticles were prepared following the two-phase protocol and characterized by transmission electron microscopy (TEM), UV-Vis spectroscopy, X-ray diffraction spectroscopy (XRD), and cyclic voltammetry (CV). It was found that, under the study conditions, it is possible to obtain nanoparticles between 1 and 5 nm; also it was found that the crystallographic orientation is strongly influenced by the ratio metal/thiol and to a lesser extent by the synthesis temperature. The voltammetric response for the electrocatalytic oxidation of glucose at carbon Au nanoparticle-modified electrode shows an increasing activity with nanoparticles size. Electroactivity and possibly selectivity are found to be nanoparticles' crystallographic orientation dependent. Classical electrochemical analysis shows that glucose electrooxidation is a diffusion-controlled process followed by a homogenous reaction.
Glucose electrooxidation has been extensively studied for glucose fuel cells, glucose sensor for medical applications, and food industry [1–11]. A variety of metals as Cu, Ni, Fe, Pt, and Au have been investigated for glucose electrocatalytic activity, and different results have been found: formic acid is the main product for glucose electrooxidation on Cu, Ni, and Fe [12–17], while glycolic acid is obtained when Pt electrodes are employed . In the case of Au electrodes the products are, depending on media pH, gluconolactone, gluconic acid, or gluconate [8–10]. Au single-crystal electrode modified with Ag under potential deposition (Ag-UPD) has been tested and showed good results for glucose electrooxidation [6, 7]. Coming to the nanoparticles, Au shows high catalytic activities at nanoscale level [18–20]. It has been shown that the catalytic activity was improved using carbon electrodes modified with Au nanoparticles [8, 9]. Furthermore carbon electrode bearing bimetallic Au-Ag nanoparticles containing not less than 73% Au is composed of atomically mixed Au and Ag atoms which give improvements on electrocatalytic activity for glucose oxidation . Similar behavior has been found for Au-Cu nanoparticles . This paper reports preliminary experimental findings suggesting that nanoparticle size and crystallographic orientation are important in achieving high electroactivity and selectivity for the electrocatalytic oxidation of glucose.
2. Experimental Section
2.1. Preparation of Gold Nanoparticles
Gold nanoparticles were prepared according to a previously published procedure . 0.184 mM HAuCl4·3H2O (J. T. Baker) aqueous solution, which was added to 10 mL of toluene (Aldrich) containing 0.34 mM tetraoctylammonium bromide (TOAB 98%, Fluka) as a phase-transfer agent. Dodecanethiol (Aldrich) was incorporated to this solution as a stabilizing agent; two Au/thiol ratios were used, 3 : 1 and 1 : 1/16 followed by the addition of an excess of NaBH4 as an aqueous reducing agent. NaBH4 was added to the solution at two different addition times, 10 and 60 sec. The reaction was allowed to proceed under constant stirring at different controlled temperatures for 3 h. Finally, a colored dispersion was obtained and purified several times with ethanol (J. T. Baker). The resulting gold nanoparticles were characterized by transmission electron microscopy (TEM), UV-Visible spectroscopy (UV-Vis), X-ray diffraction spectroscopy (XRD), and cyclic voltammetry (CV).
2.2. Preparation of Carbon Electrodes Modified with Nanoparticles
Au nanoparticle-modified electrodes were prepared as follows: 1 μL aliquot of thiol-Au nanoparticles in hexane was mixed with Vulcan XC-72 and Nafion 5% ELECTROCHEM (1 : 10 ratio) and cast onto a carbon disk (CD) followed by natural evaporation at room temperature. To remove the thiol stabilizing agent layer from nanoparticles, CD-modified electrodes were heated at 300°C for 2 h under air atmosphere, the temperature was controlled to within ±2°C.
2.3. Characterization of Nanoparticles
Synthesized Au nanoparticles were characterized using TEM, UV-Vis, XRD, and CV. TEM characterizations were performed on a Philips CM-200 microscope. Images and statistical treatment were performed using the SIMM software developed by one of us. Nanoparticle samples dissolved in hexane were cast onto a carbon-coated copper grid sample holder followed by natural evaporation at room temperature.
UV-Vis measurements were carried out on a HP spectrophotometer model 8453.
XRD measurements were obtained using a Bruker model D8 Advance diffractometer. Spectra were collected from 10 to 50° at a speed of 0.0025°seg−1.
Cyclic voltammetric measurements were performed using a BAS Epsilon potentiostat/galvanostat (Bioanalytical Systems), with a conventional three electrode cell. An Hg/HgO was used as reference electrode and a Pt wire as the counter electrode. All potentials were referred to this electrode. The electrolyte solution was purged for twenty minutes with high-purity nitrogen before taking measurements. Glucose was used at various concentrations ranging from 0.00625 to 0.1 M in 0.1 M NaOH.
3. Results and Discussion
3.1. Characterization of Au Nanoparticles
3.1.1. TEM Characterization
Figures 1(a)–1(g) show TEM micrographs of the synthesized Au nanoparticles (labeled as M1 to M8), their population core size, and their average size. The synthesis conditions are summarized in Table 1. Synthesis of Au nanoparticles can be easily controlled to obtain nanoparticles with a suitable size and low dispersion.
3.1.2. Influence of Reducing Agent Addition Rate and Temperature
It is known that the addition rate of reducing agent affects the nanoparticles size . We have synthesized the Au nanoparticles using two different addition times.
For the 10-second reducing agent addition, it was found that the greater the Au/thiol ratio, the smallest core size is obtained regardless of synthesis temperature; at least temperature seems to have less influence than Au/thiol ratio on nanoparticles size. Increasing temperature tends to reduce nanoparticles size. Core size for the highest Au/thiol ratio is about three times smaller than the lowest Au/thiol ratio (Table 1 and Figure 2).
It is well known that Au nanoparticles have surface plasmon (SP) resonance absorption bands in the visible region. SP resonance bands are strongly dependent on the size, shape, composition, and dielectric properties of nanoparticles and their local environment. Figure 3 shows UV-Visible spectra from Au nanoparticles in hexane. Results are in agreement with the literature ; only nanoparticles having a size greater than 1.5 nm present the Plasmon band.
3.1.4. XRD Characterization
Figure 4 shows the diffractograms for the different Au nanoparticles synthesized. One can see the presence of two signals corresponding to (111) and (200) crystallographic plane orientation. The intensity of signals means the proportion of each orientation present in that particular nanoparticle. As for nanoparticles size, the main factor influencing the orientation plane is the Au : thiol ratio (Table 1, Figure 4(b)). We can see that the higher the Au-to-thiol ratio, the more intense the (111) signal is (Figures 4(a) and 4(b)). Results suggest that we can, by controlling the synthesis conditions, obtain the desired size and suitable crystallographic plane orientation in the Au nanoparticles.
3.1.5. Electrochemical Characterization
We have used cyclic voltammetry for the Au nanoparticles electrochemical characterization. Figure 5(a) shows the response of both electrodes Au polycrystalline and a carbon electrode modified with Au nanoparticle in 0.1 M NaOH. We can see the typical Au response with the formation and reduction of Au oxides. Figure 5(b) shows the electrocatalytic activity of a carbon-modified electrode with Au nanoparticles in presence of glucose and gluconate in 0.1 M NaOH.
Figure 6 shows the typical Au nanoparticle responses in the presence of glucose in 0.1 M NaOH. All the nanoparticles capped onto carbon electrodes gave similar electrocatalytic activity. Nevertheless some differences arise from Figures 6 and 7. As can be seen, the current peak is a function of Au nanoparticle size with an apparent maxima around 6-7 nm. Moreover, peak current is also a function of crystallographic orientation meaning at least that the electrocatalytic activity of carbon modified with au nanoparticles depend on the plane orientation of Au nanoparticles (Figures 6 and 7). Results suggest that selectivity could also be plane orientation dependent.
Figure 8(a) shows a classical electrochemical analysis (voltammograms not shown). The peak current versus glucose concentration plot gives a linear correlation with the highest slope for carbon-modified electrode with nanoparticles suggesting a lower poisoning of electrode surface than massive Au electrodes. In Figures 8(b) and 8(c), the analysis shows an irreversible process and the possibility of coupled chemical reactions.
It was found that Au nanoparticles supported on glassy carbon presented a catalytic activity and selectivity towards glucose oxidation, depending on the particle size and on the crystallographic orientation.
Results also suggest that oxidation process in these conditions is taking place with lower poisoning of the surface in the case of the Au nanoparticles than for massive gold, and that this process is irreversible, with perhaps some chemical reactions involved in the overall oxidation process.
Nafion is a trade mark, and the authors do not have any financial relation. The SIMM software was developed by Dr. Ivan Terol-Villalobos in behalf of CIDETEQ (Centro de Investigación y Desarrollo Tecnológico en Electroquímica S. C.), owner of the registered mark. The authors thank the Mexican Council for Science and Technology (CONACYT) for financial support through Fomix-Guanajuato, Grant GTO-2006-C01-23776. M. Guerra-Balcázar thanks the Mexican Council for Science and Technology (CONACYT) for graduate fellowship.
- Y. B. Vassilyev, O. A. Khazova, and N. N. Nikolaeva, “Kinetics and mechanism of glucose electrooxidation on different electrode-catalysts. Part II. Effect of the nature of the electrode and the electrooxidation mechanism,” Journal of Electroanalytical Chemistry, vol. 196, no. 1, pp. 127–144, 1985.
- L. A. Larew and D. C. Johnson, “Concentration dependence of the mechanism of glucose oxidation at gold electrodes in alkaline media,” Journal of Electroanalytical Chemistry, vol. 262, no. 1-2, pp. 167–182, 1989.
- R. R. Adzic, M. W. Hsiao, and E. B. Yeager, “Electrochemical oxidation of glucose on single crystal gold surfaces,” Journal of Electroanalytical Chemistry, vol. 260, no. 2, pp. 475–485, 1989.
- K. B. Kokoh, J. M. Léger, B. Beden, H. Huser, and C. Lamy, “"On line" chromatographic analysis of the products resulting from the electrocatalytic oxidation of d-glucose on pure and adatoms modified Pt and Au electrodes-Part II. Alkaline medium,” Electrochimica Acta, vol. 37, no. 11, pp. 1909–1918, 1992.
- M. W. Hsiao, R. R. Adzic, and E. B. Yeager, “Electrochemical oxidation of glucose on single crystal and polycrystalline gold surfaces in phosphate buffer,” Journal of The Electrochemical Society, vol. 143, no. 3, pp. 759–767, 1996.
- S. B. Aoun, Z. Dursun, T. Koga, G. S. Bang, T. Sotomura, and I. Taniguchi, “Effect of metal ad-layers on Au(1 1 1) electrodes on electrocatalytic oxidation of glucose in an alkaline solution,” Journal of Electroanalytical Chemistry, vol. 567, no. 2, pp. 175–183, 2004.
- S. Ben Aoun, G. S. Bang, T. Koga, Y. Nonaka, T. Sotomura, and I. Taniguchi, “Electrocatalytic oxidation of sugars on silver-UPD single crystal gold electrodes in alkaline solutions,” Electrochemistry Communications, vol. 5, no. 4, pp. 317–320, 2003.
- M. Tominaga, T. Shimazoe, M. Nagashima, and I. Taniguchi, “Electrocatalytic oxidation of glucose at gold nanoparticle-modified carbon electrodes in alkaline and neutral solutions,” Electrochemistry Communications, vol. 7, no. 2, pp. 189–193, 2005.
- M. Tominaga, T. Shimazoe, M. Nagashima et al., “Electrocatalytic oxidation of glucose at gold-silver alloy, silver and gold nanoparticles in an alkaline solution,” Journal of Electroanalytical Chemistry, vol. 590, no. 1, pp. 37–46, 2006.
- M. Tominaga, M. Nagashima, K. Nishiyama, and I. Taniguchi, “Surface poisoning during electrocatalytic monosaccharide oxidation reactions at gold electrodes in alkaline medium,” Electrochemistry Communications, vol. 9, no. 8, pp. 1892–1898, 2007.
- M. Tominaga, T. Shimazoe, M. Nagashima, and I. Taniguchi, “Electrocatalytic oxidation of glucose at carbon electrodes modified with gold and gold-platinum alloy nanoparticles in an alkaline solution,” Chemistry Letters, vol. 31, no. 2, pp. 202–203, 2005.
- P. Parpot, N. Nunes, and A. P. Bettencourt, “Electrocatalytic oxidation of monosaccharides on gold electrode in alkaline medium: structure-reactivity relationship,” Journal of Electroanalytical Chemistry, vol. 596, no. 1, pp. 65–73, 2006.
- M. Z. Luo and R. P. Baldwin, “Characterization of carbohydrate oxidation at copper electrodes,” Journal of Electroanalytical Chemistry, vol. 387, no. 1-2, pp. 87–94, 1995.
- N. Torto, T. Ruzgas, and L. Gorton, “Electrochemical oxidation of mono- and disaccharides at fresh as well as oxidized copper electrodes in alkaline media,” Journal of Electroanalytical Chemistry, vol. 464, no. 2, pp. 252–258, 1999.
- K. B. Male, S. Hrapovic, Y. Liu, D. Wang, and J. H. T. Luong, “Electrochemical detection of carbohydrates using copper nanoparticles and carbon nanotubes,” Analytica Chimica Acta, vol. 516, no. 1-2, pp. 35–41, 2004.
- R. Ojani, J. B. Raoof, and P. Salmany-Afagh, “Electrocatalytic oxidation of some carbohydrates by poly(1-naphthylamine)/ nickel modified carbon paste electrode,” Journal of Electroanalytical Chemistry, vol. 571, no. 1, pp. 1–8, 2004.
- A. Salimi and M. Roushani, “Non-enzymatic glucose detection free of ascorbic acid interference using nickel powder and nafion sol-gel dispersed renewable carbon ceramic electrode,” Electrochemistry Communications, vol. 7, no. 9, pp. 879–887, 2005.
- M. Haruta, H. Kageyama, N. Kajimo, T. Kobayashi, and F. Delannay, “Fine structure of novel gold catalysts prepared by coprecipitation,” Studies in Surface Science and Catalysis, vol. 44, pp. 33–42, 1989.
- J. M. Gottfried, K. J. Schmidt, S. L. M. Schroeder, and K. Christmann, “Adsorption of carbon monoxide on Au(1 1 0)-(1 × 2),” Surface Science, vol. 536, no. 1–3, pp. 206–224, 2003.
- M. S. El-Deab, T. Sotomura, and T. Oshaka, “Oxygen reduction at electrochemically deposited crystallographically oriented Au(1 0 0)-like gold nanoparticles,” Electrochemistry Communications, vol. 7, no. 1, pp. 29–34, 2005.
- M. Tominaga, T. Shimazoe, M. Nagashima, and I. Taniguchi, “Composition-activity relationships of carbon electrode-supported bimetallic gold-silver nanoparticles in electrocatalytic oxidation of glucose,” Journal of Electroanalytical Chemistry, vol. 615, no. 1, pp. 51–61, 2008.
- M. Tominaga, Y. Taema, and I. Taniguchi, “Electrocatalytic glucose oxidation at bimetallic gold-copper nanoparticle-modified carbon electrodes in alkaline solution,” Journal of Electroanalytical Chemistry, vol. 624, no. 1-2, pp. 1–8, 2008.
- M. Guerra-Balcázar, D. Morales-Acosta, F. Castaneda, J. Ledesma-García, and L. G. Arriaga, “Synthesis of Au/C and Au/Pani for anode electrodes in glucose microfluidic fuel cell,” Electrochemistry Communications, vol. 12, no. 6, pp. 864–867, 2010.
- M. J. Hostetler, J. E. Wingate, C. J. Zhong et al., “Alkanethiolate gold cluster molecules with core diameters from 1.5 to 5.2 nm: core and monolayer properties as a function of core size,” Langmuir, vol. 14, no. 1, pp. 17–30, 1998.