# A Simple Approach to the Synthesis of Hexagonal-Shaped Silver Nanoplates

Authors: G. Cynthia Jemima Swarnavalli; V. Joseph; V. Kannappan; D. Roopsingh
Journal: Journal of Nanomaterials
 (2011)

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## Abstract

This paper deals with the synthesis of hexagonal-shaped silver nanoplates with diameters ranging from 15 to 20 nm along with a smooth nanobulk of 120 nm. These nanoplates were prepared by a kinetically controlled solution growth method using mild reducing agent dextrose, polyvinylpyrrolidone (PVPMw 40 k Da) as the capping agent and urea as a habit modifier and at a moderate temperature of 50°C. The crystal structure of the highly faceted particles consists mostly of (111) surfaces as revealed by both X-ray diffraction (XRD) studies and transmission electron microscopy (TEM).


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## Body

## 1. Introduction

Silver (Ag) nanoparticles of different shapes possess unique and tunable optical properties. Their surface Plasmon resonance (SPR) and surface-enhanced Raman spectroscopy (SERS) can be used for optical labels, contrast enhancement agents, near-field optical probes, and chemical and biological sensors [1–6]. They can be treated as fluorescent analogue tracer in biological assay [7]. These properties and applications of silver nanoparticles relate to their morphology and size. Hence, controlled synthesis of silver nanoparticles with well-defined shapes and sizes is pursued for investigating their size and morphology-dependent properties and their practical applications. A number of solution-phase methodologies have been developed to synthesize the nanoparticles successfully with a wide range of well-defined shapes [8, 9] such as cubes and octahedrons [10, 11], tetrahedrons [12], icosahedrons and decahedrons [13], wires/rods [14, 15], plates with varying profiles such as triangular plates [16], and nanodiscs [17]. Among these particles, two-dimensional nanoplates have particularly attracted attention due to their ability to control optical properties. They exhibit intense in-plane dipole surface Plasmon resonance peak which is tunable in Visible and NIR regions by simply controlling its edge length to thickness ratio and/or truncation degree of tips which is not possible with spherical Ag particles. Strong absorption coefficient of Ag nanoplates over the broad UV-NIR spectral regions and the scattering of light by these nanoplates make them an ideal class of light trapping material which enhances charge carrier generation in organic photovoltaic films [18]. Nanoplates are generally synthesized by transformation of spherical nanoparticles into plates by photo-induced methods. Mirkin’s [19] group pioneered this strategy by using fluorescent light and laser with controlled wavelength. Visible light [20], UV light [21], microwaves [22] were also used to induce the conversion of spheres to nanoplates. Later on, kinetically controlled reduction of Ag+ ions provided a simple cost effective method to synthesize plate like morphologies [23]. Seed-mediated growth method [24, 25] is another method used for the synthesis of nanoplates.  Xionghui and Aixia [26] have used sulphuric acid as a modifier to prepare hexagonal silver nanoplates. All of these methods require high temperature and long duration of reaction time. In the present work, Ag nanoplates were prepared by heterogeneous nucleation method using preformed silver seeds of size 3–10 nm.  The growth solution contained reagents according to a method proposed by Lu and Chou [27]. The reaction conditions and the molecular weight of the capping agent are altered to follow a kinetically controlled route to synthesize hexagonal plates. Moderate temperature of 50°C was used to synthesize hexagonal plates with a reaction time of 3 hrs. Urea was added to the growth solution as a habit modifier. Urea is known to change crystal habits in bulk crystals [28]. PVP (Mw 40 k Da) was used as a capping agent. Silver nanoparticles, 3–10 nm in diameter, were used as seeds to grow hexagonal silver nanoplates of 15–20 nm size.


## 2. Materials and Methods

### 2.1. Materials

Qualigen samples of silver nitrate AgNO3 and polyvinylpyrrolidone (PVP, Mw 40 k Da) and Merck samples of dextrose, urea, and trisodium citrate were used as such. All solutions were prepared in deionized water.


### 2.2. Synthesis of Silver Seeds

20 mL aqueous solution of silver nitrate (0.156 M) was heated to boiling, 2 mL of sodium citrate (0.025 M) solution was added to it, and the solution was stirred for 3 minutes and was allowed to react for 5 minutes. The solution turned yellow indicating the formation of silver nanoparticles of size 3–10 nm.


### 2.3. Preparation of Growth Solution

A growth solution containing 20 mL of aqueous solution of AgNO3 (0.156 M) and 20 mL of urea solution (0.63 M) was prepared in a 100 mL conical flask. To this flask was added 20 mL alkaline solution of PVP (1 g/1 g of AgNO3). This solution was used as the growth solution.


### 2.4. Kinetically Controlled Synthesis of Silver Nanoplates

Silver nanoplates with hexagonal shape were prepared by adding 20 mL of seed solution to the growth solution in a flask and mixed well by stirring. 20 mL of an ice cold aqueous solution of dextrose (0.313 M) was added to the flask drop-wise with continuous stirring at room temperature. The solution turned jet black and was heated in a thermostat for 3 hrs at 50°C. The silver nanoparticles were centrifuged at 4000 rpm to produce the precipitate and analyzed by UV-Visible absorption spectra, XRD, and TEM.


### 2.5. Characterization

UV-Visible spectrum of the silver nanoparticles was recorded using a Cary 5 E UV-VIS-NIR spectrophotometer. Powder X-ray diffraction (XRD) patterns were measured using (RICHSEIFER) powder diffractometer, using nickel filtered copperK-alpha radiations (λ=1.5461 Å) with a scanning rate of 0.02°. The diffraction pattern was recorded in the range of 5–70°. The HRTEM images of the silver nanoparticles were recorded using a JEOL JEM 3010 instrument with a UHR pole piece electron microscope operating at 200 kV.


## 2.1. Materials

Qualigen samples of silver nitrate AgNO3 and polyvinylpyrrolidone (PVP, Mw 40 k Da) and Merck samples of dextrose, urea, and trisodium citrate were used as such. All solutions were prepared in deionized water.


## 2.2. Synthesis of Silver Seeds

20 mL aqueous solution of silver nitrate (0.156 M) was heated to boiling, 2 mL of sodium citrate (0.025 M) solution was added to it, and the solution was stirred for 3 minutes and was allowed to react for 5 minutes. The solution turned yellow indicating the formation of silver nanoparticles of size 3–10 nm.


## 2.3. Preparation of Growth Solution

A growth solution containing 20 mL of aqueous solution of AgNO3 (0.156 M) and 20 mL of urea solution (0.63 M) was prepared in a 100 mL conical flask. To this flask was added 20 mL alkaline solution of PVP (1 g/1 g of AgNO3). This solution was used as the growth solution.


## 2.4. Kinetically Controlled Synthesis of Silver Nanoplates

Silver nanoplates with hexagonal shape were prepared by adding 20 mL of seed solution to the growth solution in a flask and mixed well by stirring. 20 mL of an ice cold aqueous solution of dextrose (0.313 M) was added to the flask drop-wise with continuous stirring at room temperature. The solution turned jet black and was heated in a thermostat for 3 hrs at 50°C. The silver nanoparticles were centrifuged at 4000 rpm to produce the precipitate and analyzed by UV-Visible absorption spectra, XRD, and TEM.


## 2.5. Characterization

UV-Visible spectrum of the silver nanoparticles was recorded using a Cary 5 E UV-VIS-NIR spectrophotometer. Powder X-ray diffraction (XRD) patterns were measured using (RICHSEIFER) powder diffractometer, using nickel filtered copperK-alpha radiations (λ=1.5461 Å) with a scanning rate of 0.02°. The diffraction pattern was recorded in the range of 5–70°. The HRTEM images of the silver nanoparticles were recorded using a JEOL JEM 3010 instrument with a UHR pole piece electron microscope operating at 200 kV.


## 3. Results and Discussion

### 3.1. Absorption Spectra

The UV-Vis absorption spectra of freshly prepared samples are given in Figure1. The seed solution shows an intense band centered at 416 nm, and the particle size is around 3–10 nm. For small nanoparticles, the peaks in the absorption spectra are due to light absorption only. The product solution containing the hexagonal nanoplates shows two bands and a strong SPR absorption  peak at about 418 nm and a shoulder at about 586 nm are contrary to a single SPR band in the range of 390 and 430 nm for spherical Ag nanoparticles. Additional peak at 586 nm is attributed to reduction in symmetry, and the number of peaks correlates with the number of ways the electron density can be polarized [29]. The peak at 416–418 nm is attributed to the transverse oscillation of electrons and has contributions from the light scattering as well. The new SPR band at 586 nm has originated from the hexagonal-shaped plates. This peak is attributed to longitudinal oscillation of electrons which can be shifted even up to 1000 nm in the near-IR region when the aspect ratio of the nanoplates increases [30]. The UV-Visible SPR information is an evidence for the generation of the Ag nanoplates with hexagonal shape.Figure 1
UV-Visible spectra of (a) silver seeds and (b) product solution containing hexagonal silver nanoplates.


### 3.2. X-Ray Diffraction Studies

The crystalline character of the silver nanoplates is supported by XRD technique. Appearance of the XRD peaks (Figures2(a) and 2(b)) corresponding to seed and product particles demonstrates typical nature of pure FCC crystalline silver (JCPDS Card no. 89-3722).Figure 2
Typical X-ray diffraction patterns of (a) Ag nanoseeds and (b) product solution containing hexagonal silver nanoplates.A comparison among (111), (200), and (220) diffraction intensities reveals that the ratio between the (111) and (200) peaks is much lower than that of the conventional bulk silver. This fact indicates that the obtained silver nanoplates are dominantly ruled by (111) planes. The diffraction peak for the (220) lattice planes is also present, but its intensity is very weak. Interestingly, there is an obvious increase in the diffraction intensity of the (111) peak relative to that of the (200) peak in going from particles in seed solution to product solution (Figure2(b)). This is a strong evidence of the preferential growth of the particles along (111) directions. The formation of nanoplates with essentially (111) facets may be the result of the lower free energy of the (111) planes and the effective adsorption of urea and PVP to the (100) plane.


### 3.3. Transmission Electron Microscopy

The particle structure and size distribution can be determined by transmission electron microscopy (TEM). The electron micrographs of PVP-stabilized silver nanoparticles in the seed solution and product solution are given in Figures3(a) and 3(b). It may be seen that in the seed solution (Figure 3(a)) the particles are spherical and moderately monodispersed. In the product solution (Figure 3(b)), however, the images reveal well-defined hexagonal facets present in many of the nanoparticles. A twin boundary in the middle of the particles can be seen when viewing these nanoparticles at different angles (e.g., Figure 3(b) particles 1, 2, 3). We can also see a nanobulk with a smooth surface of about 120 nm in size with a highly faceted hexagonal shape (Figure 3(c)). (The diameter of the hexagonal particles is determined as the mean of the three distances between opposite corners.) The longest side has a length of around 100 nm and the shortest side 60 nm. It may be the twinning boundary that allows the Ag nanoplates to grow into microplates. The bulk may also be a single crystal according to the “surface-wrapping” mechanism proposed by Feng and Zeng [31]. To further understand the crystal habit of the hexagonal silver nanoplates prepared in this study, a high-resolution TEM characterization was performed on the hexagonal silver nanoplates. HRTEM image of a hexagonal-shaped silver nanoplate (Figure 3(d)) shows the lattice planes of the crystal. The plate seems to contain twin boundaries, which is typical for many of the nanoparticles obtained in this study. The lattice planes have a d-spacing of 2.36 Å for adjacent lattice planes that corresponds to the (111) planes of face-centered cubic silver. In addition to the presence of twin boundaries, the particle contains (111) and (200) lattice planes with the (111) planes covering a much larger fraction of the particle  surface.(a) TEM image showing  the spherical Ag nanoparticles of the seed solution (3–10 nm scale bar 20 nm), (b) faceted hexagonal Ag nanoparticles of 15–20 nm with twin boundaries (scale bar 20 nm), (c) highly faceted hexagonal Ag nanobulk with 120 nm size (100 nm), (d) highly faceted hexagonal Ag nanoplates with twin boundary showing a (111) plane with a (d) spacing of 2.36 Å.
(a)(b)(c)(d)


### 3.4. Mechanism of Formation

The mechanism of kinetically controlled synthesis of the hexagonal Ag nanoplates can be discussed as follows. In order to get plate like structure, the precursor reduction rate must be greatly reduced, forcing the Ag atoms to form seeds through random hexagonal close packing with the inclusion of stacking faults. This is achieved by using wider growth conditions. Firstly a mild reducing agent dextrose was used which promotes the formation of twinned seeds in addition to making the synthesis a kinetically controlled one. Xiong and Xia have [32] demonstrated that the use of a mild reducing agent such as citric acid or ascorbic acid can promote the formation of twined seeds. Murphy and Jana [33] have shown that the addition of preformed seeds to a metal precursor in the presence of a weak reducing agent effectively isolates the nucleation and growth events allowing control over the size and shape of the resulting nanoparticles. Secondary nucleation during the growth stage was inhibited. Secondly, urea a habit modifier PVP as capping agent, helps in the formation of two-dimensional plate-like structures. Use of PVP in anisotropic synthesis of silver nanoplates and preferential adsorption of PVP to the (100) plane has been reported in literature [9, 34]. Thus (100) plane is retained, and preferential addition of silver atoms to the (111) planes was facilitated. In addition to being a habit modifier by getting adsorbed to specific crystal planes, urea was reported [27] to change the reaction path significantly by being a source of cyanate and carbonate ions and thus forming the composite intermediates AgOCN and Ag2CO3.Decomposition of urea in solution occurs as follows [27](1)NH2CONH2⟶NH4++OCN-In an alkaline solution, cyanate ions react with hydroxide ions to form carbonate ions and ammonium ion according to(2)OCN--+OH-+H2O⟶CO32-+NH4+
The intermediates were then reduced by dextrose to silver at a relatively slow rate. The kinetically controlled reaction pathway provided sufficient time for the PVP molecules and urea to adsorb onto the silver surfaces. As a result, we need not add many PVP molecules to obtain a uniform dispersion of nanosilver.  Some of the urea might have chelated with silver, further slowing down the reduction reaction of the silver ion, and significantly altered the reduction kinetics. The shape of silver nanoparticles is determined by the nature of reducing agent, capping agent, molar concentration ratio of capping agent to silver nitrate, temperature, and reaction time. In the case of mild reducing agent like dextrose, the rate of reduction of Ag+ is moderate, and, when PVP/AgNO3 ratio is 1 : 1, PVP can act mostly as capping agent and may not be a reducing agent in the present study. Yang et al. [35] have reported the solvothermal synthesis of hexagonal Ag nanoplates in DMF assisted by PVP at 140°C. The reaction time was 6 hrs. He has proposed that as PVP/AgNO3 ratio decreases, anisotropy increases, but, in the absence of PVP only spherical particles were obtained. In the present study, the temperature is considerably less (50°C), and the duration of reaction is 3 hrs. These conditions favour anisotropy, and the PVP gets adsorbed preferentially to (100) facets of   the FCC silver, and this increases the growth rate along (111). All these factors favored the formation of hexagonal nanoplates of size 15–20 nm.


## 3.1. Absorption Spectra

The UV-Vis absorption spectra of freshly prepared samples are given in Figure1. The seed solution shows an intense band centered at 416 nm, and the particle size is around 3–10 nm. For small nanoparticles, the peaks in the absorption spectra are due to light absorption only. The product solution containing the hexagonal nanoplates shows two bands and a strong SPR absorption  peak at about 418 nm and a shoulder at about 586 nm are contrary to a single SPR band in the range of 390 and 430 nm for spherical Ag nanoparticles. Additional peak at 586 nm is attributed to reduction in symmetry, and the number of peaks correlates with the number of ways the electron density can be polarized [29]. The peak at 416–418 nm is attributed to the transverse oscillation of electrons and has contributions from the light scattering as well. The new SPR band at 586 nm has originated from the hexagonal-shaped plates. This peak is attributed to longitudinal oscillation of electrons which can be shifted even up to 1000 nm in the near-IR region when the aspect ratio of the nanoplates increases [30]. The UV-Visible SPR information is an evidence for the generation of the Ag nanoplates with hexagonal shape.Figure 1
UV-Visible spectra of (a) silver seeds and (b) product solution containing hexagonal silver nanoplates.


## 3.2. X-Ray Diffraction Studies

The crystalline character of the silver nanoplates is supported by XRD technique. Appearance of the XRD peaks (Figures2(a) and 2(b)) corresponding to seed and product particles demonstrates typical nature of pure FCC crystalline silver (JCPDS Card no. 89-3722).Figure 2
Typical X-ray diffraction patterns of (a) Ag nanoseeds and (b) product solution containing hexagonal silver nanoplates.A comparison among (111), (200), and (220) diffraction intensities reveals that the ratio between the (111) and (200) peaks is much lower than that of the conventional bulk silver. This fact indicates that the obtained silver nanoplates are dominantly ruled by (111) planes. The diffraction peak for the (220) lattice planes is also present, but its intensity is very weak. Interestingly, there is an obvious increase in the diffraction intensity of the (111) peak relative to that of the (200) peak in going from particles in seed solution to product solution (Figure2(b)). This is a strong evidence of the preferential growth of the particles along (111) directions. The formation of nanoplates with essentially (111) facets may be the result of the lower free energy of the (111) planes and the effective adsorption of urea and PVP to the (100) plane.


## 3.3. Transmission Electron Microscopy

The particle structure and size distribution can be determined by transmission electron microscopy (TEM). The electron micrographs of PVP-stabilized silver nanoparticles in the seed solution and product solution are given in Figures3(a) and 3(b). It may be seen that in the seed solution (Figure 3(a)) the particles are spherical and moderately monodispersed. In the product solution (Figure 3(b)), however, the images reveal well-defined hexagonal facets present in many of the nanoparticles. A twin boundary in the middle of the particles can be seen when viewing these nanoparticles at different angles (e.g., Figure 3(b) particles 1, 2, 3). We can also see a nanobulk with a smooth surface of about 120 nm in size with a highly faceted hexagonal shape (Figure 3(c)). (The diameter of the hexagonal particles is determined as the mean of the three distances between opposite corners.) The longest side has a length of around 100 nm and the shortest side 60 nm. It may be the twinning boundary that allows the Ag nanoplates to grow into microplates. The bulk may also be a single crystal according to the “surface-wrapping” mechanism proposed by Feng and Zeng [31]. To further understand the crystal habit of the hexagonal silver nanoplates prepared in this study, a high-resolution TEM characterization was performed on the hexagonal silver nanoplates. HRTEM image of a hexagonal-shaped silver nanoplate (Figure 3(d)) shows the lattice planes of the crystal. The plate seems to contain twin boundaries, which is typical for many of the nanoparticles obtained in this study. The lattice planes have a d-spacing of 2.36 Å for adjacent lattice planes that corresponds to the (111) planes of face-centered cubic silver. In addition to the presence of twin boundaries, the particle contains (111) and (200) lattice planes with the (111) planes covering a much larger fraction of the particle  surface.(a) TEM image showing  the spherical Ag nanoparticles of the seed solution (3–10 nm scale bar 20 nm), (b) faceted hexagonal Ag nanoparticles of 15–20 nm with twin boundaries (scale bar 20 nm), (c) highly faceted hexagonal Ag nanobulk with 120 nm size (100 nm), (d) highly faceted hexagonal Ag nanoplates with twin boundary showing a (111) plane with a (d) spacing of 2.36 Å.
(a)(b)(c)(d)


## 3.4. Mechanism of Formation

The mechanism of kinetically controlled synthesis of the hexagonal Ag nanoplates can be discussed as follows. In order to get plate like structure, the precursor reduction rate must be greatly reduced, forcing the Ag atoms to form seeds through random hexagonal close packing with the inclusion of stacking faults. This is achieved by using wider growth conditions. Firstly a mild reducing agent dextrose was used which promotes the formation of twinned seeds in addition to making the synthesis a kinetically controlled one. Xiong and Xia have [32] demonstrated that the use of a mild reducing agent such as citric acid or ascorbic acid can promote the formation of twined seeds. Murphy and Jana [33] have shown that the addition of preformed seeds to a metal precursor in the presence of a weak reducing agent effectively isolates the nucleation and growth events allowing control over the size and shape of the resulting nanoparticles. Secondary nucleation during the growth stage was inhibited. Secondly, urea a habit modifier PVP as capping agent, helps in the formation of two-dimensional plate-like structures. Use of PVP in anisotropic synthesis of silver nanoplates and preferential adsorption of PVP to the (100) plane has been reported in literature [9, 34]. Thus (100) plane is retained, and preferential addition of silver atoms to the (111) planes was facilitated. In addition to being a habit modifier by getting adsorbed to specific crystal planes, urea was reported [27] to change the reaction path significantly by being a source of cyanate and carbonate ions and thus forming the composite intermediates AgOCN and Ag2CO3.Decomposition of urea in solution occurs as follows [27](1)NH2CONH2⟶NH4++OCN-In an alkaline solution, cyanate ions react with hydroxide ions to form carbonate ions and ammonium ion according to(2)OCN--+OH-+H2O⟶CO32-+NH4+
The intermediates were then reduced by dextrose to silver at a relatively slow rate. The kinetically controlled reaction pathway provided sufficient time for the PVP molecules and urea to adsorb onto the silver surfaces. As a result, we need not add many PVP molecules to obtain a uniform dispersion of nanosilver.  Some of the urea might have chelated with silver, further slowing down the reduction reaction of the silver ion, and significantly altered the reduction kinetics. The shape of silver nanoparticles is determined by the nature of reducing agent, capping agent, molar concentration ratio of capping agent to silver nitrate, temperature, and reaction time. In the case of mild reducing agent like dextrose, the rate of reduction of Ag+ is moderate, and, when PVP/AgNO3 ratio is 1 : 1, PVP can act mostly as capping agent and may not be a reducing agent in the present study. Yang et al. [35] have reported the solvothermal synthesis of hexagonal Ag nanoplates in DMF assisted by PVP at 140°C. The reaction time was 6 hrs. He has proposed that as PVP/AgNO3 ratio decreases, anisotropy increases, but, in the absence of PVP only spherical particles were obtained. In the present study, the temperature is considerably less (50°C), and the duration of reaction is 3 hrs. These conditions favour anisotropy, and the PVP gets adsorbed preferentially to (100) facets of   the FCC silver, and this increases the growth rate along (111). All these factors favored the formation of hexagonal nanoplates of size 15–20 nm.


## 4. Conclusion

The use of a mild reducing agent like dextrose, higher concentration of AgNO3, polyvinylpyrrolidone (PVP), and urea as a modifier maneuvered the reduction of AgNO3 in a kinetically controlled pathway to produce hexagonal silver nanoplates at a moderate temperature of 50°C. The reaction time is also considerably less when compared to other existing methods. Moderately monodispersed hexagonal plates of size 15–20 nm were achieved by the combined use of urea and PVP by adsorption of both to specific crystal planes.  The crystal structure was confirmed by XRD data and was determined to possess mostly (111) facets and smaller regions of (100) facets as particle size increases. The formation of these hexagonal nanoplates is attributed to the possible intermediate formation to slow down the synthesis and adsorption of urea and PVP to specific crystal planes.  The present work may help to modify optical properties of Ag nanoplates in the visible and near infrared (NIR) region by controlling their edge length to thickness ratio. These properties and applications of silver nanoparticles relate to their morphology and size.



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*Source: 825637-2011-08-04.xml*