# Comparative Study of Ag Nanostructures: Molecular Simulations, Electrochemical Behavior, and Antibacterial Effect

Authors: Álvaro de Jesús Ruíz-Baltazar; Simón Yobanny Reyes-López; D. Larrañaga; R. Pérez
Journal: Journal of Nanomaterials
 (2016)

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## Abstract

Nanoparticles of Ag with different sizes and structures were obtained and studied. Two methods for reductions of Ag ions were employed, chemical reduction by sodium borohydride and ethylene glycol. Cuboctahedral and icosahedral structures were obtained. Molecular simulations were carried out in order to evaluate the reactivity of both structures. On the other hand, the electrochemical activity and antibacterial effect (E. coli) of the cuboctahedral and icosahedral structures were measured experimentally. The results obtained by molecular simulation, cyclic voltammetry, and antibacterial effect were compared and discussed in this work.


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## Body

## 1. Introduction

Recently, the study of metallic nanoparticles has acquired particular interest due to the great number of potential applications on diverse science fields [1–3]. Specifically, silver nanoparticles have been widely studied due their particular physicochemical properties, including the notable electrical and thermal conductivity, a high catalytic activity, and surface-enhanced Raman scattering [4–6]. Consequently, AgNPs offer potential applications in chemistry, physics, biomedicine, catalysis, electronics, optics, environment engineering, and materials science [7–10]. Specifically, in biomedicine, AgNPs exhibit broad spectrum bactericidal and fungicidal activity [9]. The AgNPs have been synthesized by a great variety of chemical and physical methods. However, some reports indicate that the chemical reduction method provides well control under the structure and morphology of the AgNPs [11–15]. Specifically, reducing agents as sodium borohydride (NaBH4) and ethylene glycol (EG) offer an excellent alternative to obtain silver nanoparticles sizes and morphologies controlled [16–22].In this work, a comparative study regarding the nanostructure obtained as a function of the synthesis method is presented. On the other hand it has been reported that the structure observed for the Ag nanoparticles determines the properties and consequently their potential applications [23–26]. In this study, we focused on the behavior of the AgNPs obtained by the two synthesis methods proposed. Theoretical simulation using Density Functional Theory (DFT) was performed in order to calculate the values of the energy gap and binding energies associated with the AgNPs obtained. These values can be a great reference to determine the reactivity of the AgNPs. Additionally, cyclic voltammetry analysis and bactericidal tests were conducted. The theoretical and experimental data were compared and discussed widely.


## 2. Experimental Details

### 2.1. Synthesis of Ag Nanoparticles

#### 2.1.1. Polyol Method

Chemical synthesis of Ag nanoparticles was performed using ethylene glycol (EG, C2H6O2). Briefly, 3 vials with 9 mL of ethylene glycol (EG) were placed in an oil-bath of silicone. A polyvinylpirrolidone 1 M (PVP, C
6
H
9
N
O
n) solution in EG was added. The mixture underwent magnetic stirring (150 rpm) and was heated at 150°C. Then three solutions of AgNO3 concentrations 0.2 M, 0.1 M and 0.05 M were adhered to the solution of PVP and EG.


#### 2.1.2. Chemical Reduction by Sodium Borohydride NaBH4

To reduce the Ag ions, aqueous solutions of NaBH4 (0.2 M) were added dropwise to the PVP containing metal ion mixtures. The chemical reduction process was carried out at room temperature. Ag concentrations of 0.05, 0.1, and 0.2 M were prepared.


### 2.2. Structural Characterization

The structural and morphological characteristics of the dispersed metallic nanoparticles have been studied using a Philips Tecnai F20 transmission electron microscope with a field emission gun attachment and dot-to-dot direct maximum resolution of 0.23 nm. TEM specimens were prepared by dispersing and subsequent drying of a drop of colloidal solution on a copper grid (3 mm in diameter) covered with an amorphous carbon film. Analysis of Fourier transform infrared (FT-IR) and Raman (RMN) spectroscopy were conducted. Additionally we employed the technique of UV-Vis spectroscopy as a rapid and reliable technique for characterization of silver nanoparticles, through a fiber optic spectrometer Ocean Optics model USB4F01962, in a range of 200 from 900 nm wavelength, with an integration time of 17 milliseconds and 10 scans.


### 2.3. Cyclic Voltammetry

The cyclic voltammetry of the AgNPs was carried out in acid medium employing a solution of H2SO4 (0.5 M), with scan rate 50 mVs−1 at 25°C in the presence of N2. The AgNPs were supported on Vulcan carbon in order to measure the electrochemical activity.


### 2.4. Experimental Details of Antibacterial Effect

The antibacterial activity againstEscherichia coli (E. coli) of silver nanoparticles synthesized with EG and NaBH4 as reducing agents was evaluated using the disk diffusion method. Three filter paper discs of 5 mm diameter were impregnated with 5 mL of AgNPs solutions at concentrations of 5, 10, and 15 mM. Subsequently, the discs were placed in the vial containing theE. coli. To evaluate the antibacterial activity of nanoparticles, a control disk was assessed too. The system was incubated at 36°C for 24 h. Finally, the inhibition zone was measured.


## 2.1. Synthesis of Ag Nanoparticles

### 2.1.1. Polyol Method

Chemical synthesis of Ag nanoparticles was performed using ethylene glycol (EG, C2H6O2). Briefly, 3 vials with 9 mL of ethylene glycol (EG) were placed in an oil-bath of silicone. A polyvinylpirrolidone 1 M (PVP, C
6
H
9
N
O
n) solution in EG was added. The mixture underwent magnetic stirring (150 rpm) and was heated at 150°C. Then three solutions of AgNO3 concentrations 0.2 M, 0.1 M and 0.05 M were adhered to the solution of PVP and EG.


### 2.1.2. Chemical Reduction by Sodium Borohydride NaBH4

To reduce the Ag ions, aqueous solutions of NaBH4 (0.2 M) were added dropwise to the PVP containing metal ion mixtures. The chemical reduction process was carried out at room temperature. Ag concentrations of 0.05, 0.1, and 0.2 M were prepared.


## 2.1.1. Polyol Method

Chemical synthesis of Ag nanoparticles was performed using ethylene glycol (EG, C2H6O2). Briefly, 3 vials with 9 mL of ethylene glycol (EG) were placed in an oil-bath of silicone. A polyvinylpirrolidone 1 M (PVP, C
6
H
9
N
O
n) solution in EG was added. The mixture underwent magnetic stirring (150 rpm) and was heated at 150°C. Then three solutions of AgNO3 concentrations 0.2 M, 0.1 M and 0.05 M were adhered to the solution of PVP and EG.


## 2.1.2. Chemical Reduction by Sodium Borohydride NaBH4

To reduce the Ag ions, aqueous solutions of NaBH4 (0.2 M) were added dropwise to the PVP containing metal ion mixtures. The chemical reduction process was carried out at room temperature. Ag concentrations of 0.05, 0.1, and 0.2 M were prepared.


## 2.2. Structural Characterization

The structural and morphological characteristics of the dispersed metallic nanoparticles have been studied using a Philips Tecnai F20 transmission electron microscope with a field emission gun attachment and dot-to-dot direct maximum resolution of 0.23 nm. TEM specimens were prepared by dispersing and subsequent drying of a drop of colloidal solution on a copper grid (3 mm in diameter) covered with an amorphous carbon film. Analysis of Fourier transform infrared (FT-IR) and Raman (RMN) spectroscopy were conducted. Additionally we employed the technique of UV-Vis spectroscopy as a rapid and reliable technique for characterization of silver nanoparticles, through a fiber optic spectrometer Ocean Optics model USB4F01962, in a range of 200 from 900 nm wavelength, with an integration time of 17 milliseconds and 10 scans.


## 2.3. Cyclic Voltammetry

The cyclic voltammetry of the AgNPs was carried out in acid medium employing a solution of H2SO4 (0.5 M), with scan rate 50 mVs−1 at 25°C in the presence of N2. The AgNPs were supported on Vulcan carbon in order to measure the electrochemical activity.


## 2.4. Experimental Details of Antibacterial Effect

The antibacterial activity againstEscherichia coli (E. coli) of silver nanoparticles synthesized with EG and NaBH4 as reducing agents was evaluated using the disk diffusion method. Three filter paper discs of 5 mm diameter were impregnated with 5 mL of AgNPs solutions at concentrations of 5, 10, and 15 mM. Subsequently, the discs were placed in the vial containing theE. coli. To evaluate the antibacterial activity of nanoparticles, a control disk was assessed too. The system was incubated at 36°C for 24 h. Finally, the inhibition zone was measured.


## 3. Results and Discussion

### 3.1. Transmission Electron Microscopy (TEM)

Figures1(a) and 1(b) show low magnification TEM images of Ag nanoparticles produced by NaBH4 and EG, respectively. In both cases, the morphology of the particles is semispherical and the formation of agglomerates is not appreciated. The histograms corresponding to the samples synthesized by NaBH4 and EG are insert in Figures 1(a) and 1(b), which indicates that the average particle sizes were 15 nm and 42 nm, respectively. This fact can be attributed to the synthesis methodology and consequently to reduction rate of the reagent involved. The NaBH4 presents more capacity to reduce the Ag ions, because the reaction is carried out in 2 minutes, while in the case of the poliol method the reaction time is 2 hours. The Ag ions reduction by NaBH4 is carried out at room temperature. Figures 1(c) and 1(d) correspond to the high resolution transmission electron microscopy (HRTEM) images associated withAgNPs-NaBH
4 and AgNPs-EG, respectively. Specifically, in the case of AgNPs-NaBH4, the d-spacing measured was 0.23 nm and 0.2 nm which corresponds, respectively, to the (111) and (200) planes of the FCC of the Ag structure. These values were obtained from the Fast Fourier Transform (FFT) and the HRTEM filtered images showed in the Figures 1(e) and 1(f). Regarding sample AgNPs-EG (Figure 1(d)), particles with multiple-twinned structures type [MTP] are observed. MTP particles were more commonly observed in the case of the samples produced by EG reducing agent. The particles obtained with ethylene glycol require the incorporation of heat for a period of 2 hr, which is carried out by nucleation of crystals of Ag. During this period formation of these crystalline defects is possible due to coalescence of nucleated fine particles. Therefore a decrease in reaction time can reduce particle sizes, crystalline defects, and well-defined morphologies. It is important to mention that the interplanar distances measured in this sample (AgNPs-EG) were 0.23 nm and 0.2 which belong to the (111) and (200) planes previously mentioned in figures (Figures 1(g) and 1(h)). In order to discuss these results, it is important to note that the structure in both cases is different. The structure associated with AgNPs-NaBH4 sample can be considered as a cubooctahedral (CO) structure, while the AgNPs-EG sample exhibits an icosahedral (Ih) structure. In this sense, the reactivity and, consequently, the electrochemical and antibacterial activity can be evaluated from the point of view of the structure observed.Figure 1
((a) and (b)) Bright field TEM images corresponding to the AgNPs-NaBH4 and AgNPs-EG samples. ((c) and (d)) HRTEM images of the AgNPs obtained by NaBH4 and EG. ((e) and (f)) Fast Fourier Transform (FFT) and HRTEM filtered image of AgNPs-NaBH4. ((g) and (h)) Fast Fourier Transform and HRTEM filtered image of AgNPs-EG.


### 3.2. Spectroscopy Characterization

#### 3.2.1. Raman Spectroscopy

Figures2(a) and 2(b) show the Raman spectroscopy of AgNPs-EG and AgNPs-NaBH4 samples, respectively. Regarding AgNPs-EG spectra, the bands located at 884, 1050, and 1090 cm−1 are attributed to the pure EG [27]. The intensity observed at 1276 cm−1 corresponds to the symmetric stretching mode of C-O-C present in the EG. The band at 1458 cm−1 can be associated with the vibrations of the C-H group [10, 28, 29].Figure 2
((a) and (b)) Raman spectra of Ih and CO AgNPs. FT-IR spectra of AgNPs-EG (c) and AgNPs-NaBH4 (d) samples. ((e) and (f)) UV-Vis analysis of Ih and CO Ag nanostructures, respectively.
(a)
(b)
(c)
(d)
(e)
(f)In the AgNPs-NaBH4 spectra, the band situated at 158 cm−1 shows clearly the presence of the Ag lattice vibrations models [30]. In these spectra can be appreciated the presence of the nitrate (NO−) functional group, which was dissociated in the aqueous medium employed during AgNPs-NaBH4 synthesis. The intensities observed at 698, 717, and 791 cm−1 correspond to vibration of the doubly generated N-O in plane bending [31, 32]. Complementarily, the presence of the Ag nanoparticles is demonstrated by the bands situated at 1319 and 1643 cm−1 [33, 34].


#### 3.2.2. FT-IR Spectroscopy

Figure2(c) shows the FT-IR spectra of the EG pure and the samples of AgNPs-EG at 5 and 10 mM. The bands observed at 1046 and 1424 cm−1 can be attributed to the vibrations bonds of the C-O and C-O-H, respectively [6, 35]. The presence of the N
O
3
- ion is confirmed by the band located at 1383 cm−1 [36]. The stretching vibrations of the hydroxyl functional (OH) group can be associated with the bands located in the interval from 1600 to 2700 cm−1 [37]. However, the adsorption band situated at 2356 cm−1 confirms the presence of AgNPs [38]. In this case, this band is generated due to the interaction of the hydroxyl group of the EG and the partial charges of AgNPs [6, 38]. It is important to note that the peaks observed in the range of 1662 to 1587 cm−1 describe a maximum hydrogen bonding association, typical in the in the alcohol-water system [39]. Finally, the intensities at 2873 and 2930 cm−1 correspond to the stretching vibrations of the C-H bonds [36].Figure2(d) shows the infrared spectra of deionized water and the samples synthetized by NaBH4 (5 mM and 10 mM). It is worth noting that the intensity at 2357 cm−1 is also observed in these FT-IR spectra. This fact confirms the AgNPs formation [6, 14, 36, 40]. In this case, this band also is generated by the interaction of the hydroxyl group (1646 cm−1) of the deionized water and the partial charges of the AgNPs [40]. This result supports the TEM analysis.


#### 3.2.3. UV-Vis Spectroscopy

In order to provide the full evidence with respect to the AgNPs presence, Figures2(e) and 2(f) show the UV-Vis analysis corresponding to the CO and Ih samples, respectively. In these spectra, typical bands around 400 nm are observed in both cases [12, 41]. Specifically, for AgNPs-NaBH4 and AgNPs-EG samples, bands located at 419 and 388 nm were observed, respectively. This result supports the particle size observed by TEM.


### 3.3. DFT Molecular Simulation

In order to describe the differences between the AgNP’s configurations observed (cubooctahedral and icosahedral), DFT simulation of AgNP’s models was carried out. Table1 describes the HOMO and LUMO values calculated from the cubooctahedral, decahedral, and icosahedral configurations. These configurations were modeled with 55 atoms of Ag. Complementarily, the values of the energy gap and binding energies from the different AgNP’s configurations were calculated. From the energy gap values, we can observe that the cubooctahedral structure (Ag CO55) exhibits the lowest energy HOMO-LUMO gap (0.0144 Ha), which is due to the higher density of electrons on its surface. With respect to the decahedral configurations, the energy gap is 0.0297 Ha. In this regard, it can expect theoretically a higher reactivity of the cubooctahedral configurations. Figure 3 shows an illustration of the electrophilic fields of the Ag CO55 and Ag Dh55 models obtained at 0.0025 eV isovalue distributions.Table 1
Calculation of HOMO and LUMO energy levels of AgNPs.
Structure
HOMO (Ha)
LUMO (Ha)
Gap (Ha)
Binding energy (eV)
Binding energy/atom (eV)
Ag CO55
−0.134055
−0.119645
0.0144
−98.38302
−1.7888
Ag Dh55
−0.142562
−0.11284
0.0297
−99.03232
−1.8006
Ag Ih55
−0.129181
−0.096796
0.0324
−100.82873
−1.8332Figure 3
Electrophilic fields of the Ag CO55 and Ag Dh55 models obtained at 0.0025 eV isovalue distributions.It is clear that the electrophilic field of the cubooctahedron configuration is localized on the vortices, and for the icosahedral configuration the electrophilic field is localized on the face with fivefold symmetry. However, it is important to note that the size of the AgNPs model was the same in both cases. In this sense, it has been reported that the reactivity of the AgNPs can vary with respect to particle size; for example, only small decahedral structures exhibit superior catalytic activity compared with cubooctahedral structures [39, 40, 42–44]. In this case, the experimental results observed by TEM images indicate that, in AgNPs-NaBH4 sample, the cubooctahedral structures appear with major frequency and with a significant minor particle size (17 nm) with respect to the AgNPs-EG sample (40 nm). For this reason a higher catalytic activity of AgNPs-NaBH4 sample would be expected. In this sense, the catalytic activity of the AgNPs-NaBH4 and AgNPs-EG structures can be evaluated by cyclic voltammetry.


### 3.4. Cyclic Voltammetry

In order to demonstrate experimentally the result obtained by DFT simulations, Figure4 shows the cyclic voltammogram corresponding to the AgNPs with cubooctahedral (CO) and icosahedral (Ih) configuration. It can be seen that in the case of CO nanoparticles there is an increase in the current value of the redox processes involved in comparison with the Ih nanoparticles. Also, the cyclic voltammogram of both configurations is similar; no displacements are observed in the voltage values and they differ only in the associated current intensity reduction capability. This fact supports the theoretical analysis (DFT) presented previously.Figure 4
Cyclic voltammogram of the icosahedral and cuboctahedral structures of Ag nanoparticles in acid medium evaluated with a solution of H2SO4 (0.5 M). Scan rate 50 mVs−1 at 25°C in the presence of N2.


### 3.5. Antibacterial Effect

The antibacterial activity of the AgNPs is showed in Figure5. Figure 5(a) shows the antimicrobial property of AgNPs-EG associated with the decahedral structure. In this image can be appreciated the inhibition zone corresponding to AgNPs solution at concentrations of 5, 10, and 15 mM; the values measured in this case were 6.5, 7.5, and 10 mm, respectively (Figure 5(c)). Regarding the AgNPs-NaBH4 sample with cubooctahedral structure, Figure 5(b) illustrates in qualitative way the antibacterial effect with respect to theE. coli. Inhibitions zones of 7.5, 9 and 15 mm were observed in this case (Figure 5(c)). In this work, it was found that the growth inhibition effect inS. coli depends on the Ag concentration promoting good antimicrobial effect on lower Ag concentration (15 mM). These results confirmed the antibacterial properties of silver nanoparticles; however, the most significant one of these results is to compare the antibacterial effect as a function of the AgNPs structures. According to the theoretical (DFT analysis) and experimental (cyclic voltammetry) results obtained, the cubooctahedral structure (AgNPs-NaBH4) exhibits the highest catalytic and antibacterial activity.Figure 5
(a)
(b)
(c)


## 3.1. Transmission Electron Microscopy (TEM)

Figures1(a) and 1(b) show low magnification TEM images of Ag nanoparticles produced by NaBH4 and EG, respectively. In both cases, the morphology of the particles is semispherical and the formation of agglomerates is not appreciated. The histograms corresponding to the samples synthesized by NaBH4 and EG are insert in Figures 1(a) and 1(b), which indicates that the average particle sizes were 15 nm and 42 nm, respectively. This fact can be attributed to the synthesis methodology and consequently to reduction rate of the reagent involved. The NaBH4 presents more capacity to reduce the Ag ions, because the reaction is carried out in 2 minutes, while in the case of the poliol method the reaction time is 2 hours. The Ag ions reduction by NaBH4 is carried out at room temperature. Figures 1(c) and 1(d) correspond to the high resolution transmission electron microscopy (HRTEM) images associated withAgNPs-NaBH
4 and AgNPs-EG, respectively. Specifically, in the case of AgNPs-NaBH4, the d-spacing measured was 0.23 nm and 0.2 nm which corresponds, respectively, to the (111) and (200) planes of the FCC of the Ag structure. These values were obtained from the Fast Fourier Transform (FFT) and the HRTEM filtered images showed in the Figures 1(e) and 1(f). Regarding sample AgNPs-EG (Figure 1(d)), particles with multiple-twinned structures type [MTP] are observed. MTP particles were more commonly observed in the case of the samples produced by EG reducing agent. The particles obtained with ethylene glycol require the incorporation of heat for a period of 2 hr, which is carried out by nucleation of crystals of Ag. During this period formation of these crystalline defects is possible due to coalescence of nucleated fine particles. Therefore a decrease in reaction time can reduce particle sizes, crystalline defects, and well-defined morphologies. It is important to mention that the interplanar distances measured in this sample (AgNPs-EG) were 0.23 nm and 0.2 which belong to the (111) and (200) planes previously mentioned in figures (Figures 1(g) and 1(h)). In order to discuss these results, it is important to note that the structure in both cases is different. The structure associated with AgNPs-NaBH4 sample can be considered as a cubooctahedral (CO) structure, while the AgNPs-EG sample exhibits an icosahedral (Ih) structure. In this sense, the reactivity and, consequently, the electrochemical and antibacterial activity can be evaluated from the point of view of the structure observed.Figure 1
((a) and (b)) Bright field TEM images corresponding to the AgNPs-NaBH4 and AgNPs-EG samples. ((c) and (d)) HRTEM images of the AgNPs obtained by NaBH4 and EG. ((e) and (f)) Fast Fourier Transform (FFT) and HRTEM filtered image of AgNPs-NaBH4. ((g) and (h)) Fast Fourier Transform and HRTEM filtered image of AgNPs-EG.


## 3.2. Spectroscopy Characterization

### 3.2.1. Raman Spectroscopy

Figures2(a) and 2(b) show the Raman spectroscopy of AgNPs-EG and AgNPs-NaBH4 samples, respectively. Regarding AgNPs-EG spectra, the bands located at 884, 1050, and 1090 cm−1 are attributed to the pure EG [27]. The intensity observed at 1276 cm−1 corresponds to the symmetric stretching mode of C-O-C present in the EG. The band at 1458 cm−1 can be associated with the vibrations of the C-H group [10, 28, 29].Figure 2
((a) and (b)) Raman spectra of Ih and CO AgNPs. FT-IR spectra of AgNPs-EG (c) and AgNPs-NaBH4 (d) samples. ((e) and (f)) UV-Vis analysis of Ih and CO Ag nanostructures, respectively.
(a)
(b)
(c)
(d)
(e)
(f)In the AgNPs-NaBH4 spectra, the band situated at 158 cm−1 shows clearly the presence of the Ag lattice vibrations models [30]. In these spectra can be appreciated the presence of the nitrate (NO−) functional group, which was dissociated in the aqueous medium employed during AgNPs-NaBH4 synthesis. The intensities observed at 698, 717, and 791 cm−1 correspond to vibration of the doubly generated N-O in plane bending [31, 32]. Complementarily, the presence of the Ag nanoparticles is demonstrated by the bands situated at 1319 and 1643 cm−1 [33, 34].


### 3.2.2. FT-IR Spectroscopy

Figure2(c) shows the FT-IR spectra of the EG pure and the samples of AgNPs-EG at 5 and 10 mM. The bands observed at 1046 and 1424 cm−1 can be attributed to the vibrations bonds of the C-O and C-O-H, respectively [6, 35]. The presence of the N
O
3
- ion is confirmed by the band located at 1383 cm−1 [36]. The stretching vibrations of the hydroxyl functional (OH) group can be associated with the bands located in the interval from 1600 to 2700 cm−1 [37]. However, the adsorption band situated at 2356 cm−1 confirms the presence of AgNPs [38]. In this case, this band is generated due to the interaction of the hydroxyl group of the EG and the partial charges of AgNPs [6, 38]. It is important to note that the peaks observed in the range of 1662 to 1587 cm−1 describe a maximum hydrogen bonding association, typical in the in the alcohol-water system [39]. Finally, the intensities at 2873 and 2930 cm−1 correspond to the stretching vibrations of the C-H bonds [36].Figure2(d) shows the infrared spectra of deionized water and the samples synthetized by NaBH4 (5 mM and 10 mM). It is worth noting that the intensity at 2357 cm−1 is also observed in these FT-IR spectra. This fact confirms the AgNPs formation [6, 14, 36, 40]. In this case, this band also is generated by the interaction of the hydroxyl group (1646 cm−1) of the deionized water and the partial charges of the AgNPs [40]. This result supports the TEM analysis.


### 3.2.3. UV-Vis Spectroscopy

In order to provide the full evidence with respect to the AgNPs presence, Figures2(e) and 2(f) show the UV-Vis analysis corresponding to the CO and Ih samples, respectively. In these spectra, typical bands around 400 nm are observed in both cases [12, 41]. Specifically, for AgNPs-NaBH4 and AgNPs-EG samples, bands located at 419 and 388 nm were observed, respectively. This result supports the particle size observed by TEM.


## 3.2.1. Raman Spectroscopy

Figures2(a) and 2(b) show the Raman spectroscopy of AgNPs-EG and AgNPs-NaBH4 samples, respectively. Regarding AgNPs-EG spectra, the bands located at 884, 1050, and 1090 cm−1 are attributed to the pure EG [27]. The intensity observed at 1276 cm−1 corresponds to the symmetric stretching mode of C-O-C present in the EG. The band at 1458 cm−1 can be associated with the vibrations of the C-H group [10, 28, 29].Figure 2
((a) and (b)) Raman spectra of Ih and CO AgNPs. FT-IR spectra of AgNPs-EG (c) and AgNPs-NaBH4 (d) samples. ((e) and (f)) UV-Vis analysis of Ih and CO Ag nanostructures, respectively.
(a)
(b)
(c)
(d)
(e)
(f)In the AgNPs-NaBH4 spectra, the band situated at 158 cm−1 shows clearly the presence of the Ag lattice vibrations models [30]. In these spectra can be appreciated the presence of the nitrate (NO−) functional group, which was dissociated in the aqueous medium employed during AgNPs-NaBH4 synthesis. The intensities observed at 698, 717, and 791 cm−1 correspond to vibration of the doubly generated N-O in plane bending [31, 32]. Complementarily, the presence of the Ag nanoparticles is demonstrated by the bands situated at 1319 and 1643 cm−1 [33, 34].


## 3.2.2. FT-IR Spectroscopy

Figure2(c) shows the FT-IR spectra of the EG pure and the samples of AgNPs-EG at 5 and 10 mM. The bands observed at 1046 and 1424 cm−1 can be attributed to the vibrations bonds of the C-O and C-O-H, respectively [6, 35]. The presence of the N
O
3
- ion is confirmed by the band located at 1383 cm−1 [36]. The stretching vibrations of the hydroxyl functional (OH) group can be associated with the bands located in the interval from 1600 to 2700 cm−1 [37]. However, the adsorption band situated at 2356 cm−1 confirms the presence of AgNPs [38]. In this case, this band is generated due to the interaction of the hydroxyl group of the EG and the partial charges of AgNPs [6, 38]. It is important to note that the peaks observed in the range of 1662 to 1587 cm−1 describe a maximum hydrogen bonding association, typical in the in the alcohol-water system [39]. Finally, the intensities at 2873 and 2930 cm−1 correspond to the stretching vibrations of the C-H bonds [36].Figure2(d) shows the infrared spectra of deionized water and the samples synthetized by NaBH4 (5 mM and 10 mM). It is worth noting that the intensity at 2357 cm−1 is also observed in these FT-IR spectra. This fact confirms the AgNPs formation [6, 14, 36, 40]. In this case, this band also is generated by the interaction of the hydroxyl group (1646 cm−1) of the deionized water and the partial charges of the AgNPs [40]. This result supports the TEM analysis.


## 3.2.3. UV-Vis Spectroscopy

In order to provide the full evidence with respect to the AgNPs presence, Figures2(e) and 2(f) show the UV-Vis analysis corresponding to the CO and Ih samples, respectively. In these spectra, typical bands around 400 nm are observed in both cases [12, 41]. Specifically, for AgNPs-NaBH4 and AgNPs-EG samples, bands located at 419 and 388 nm were observed, respectively. This result supports the particle size observed by TEM.


## 3.3. DFT Molecular Simulation

In order to describe the differences between the AgNP’s configurations observed (cubooctahedral and icosahedral), DFT simulation of AgNP’s models was carried out. Table1 describes the HOMO and LUMO values calculated from the cubooctahedral, decahedral, and icosahedral configurations. These configurations were modeled with 55 atoms of Ag. Complementarily, the values of the energy gap and binding energies from the different AgNP’s configurations were calculated. From the energy gap values, we can observe that the cubooctahedral structure (Ag CO55) exhibits the lowest energy HOMO-LUMO gap (0.0144 Ha), which is due to the higher density of electrons on its surface. With respect to the decahedral configurations, the energy gap is 0.0297 Ha. In this regard, it can expect theoretically a higher reactivity of the cubooctahedral configurations. Figure 3 shows an illustration of the electrophilic fields of the Ag CO55 and Ag Dh55 models obtained at 0.0025 eV isovalue distributions.Table 1
Calculation of HOMO and LUMO energy levels of AgNPs.
Structure
HOMO (Ha)
LUMO (Ha)
Gap (Ha)
Binding energy (eV)
Binding energy/atom (eV)
Ag CO55
−0.134055
−0.119645
0.0144
−98.38302
−1.7888
Ag Dh55
−0.142562
−0.11284
0.0297
−99.03232
−1.8006
Ag Ih55
−0.129181
−0.096796
0.0324
−100.82873
−1.8332Figure 3
Electrophilic fields of the Ag CO55 and Ag Dh55 models obtained at 0.0025 eV isovalue distributions.It is clear that the electrophilic field of the cubooctahedron configuration is localized on the vortices, and for the icosahedral configuration the electrophilic field is localized on the face with fivefold symmetry. However, it is important to note that the size of the AgNPs model was the same in both cases. In this sense, it has been reported that the reactivity of the AgNPs can vary with respect to particle size; for example, only small decahedral structures exhibit superior catalytic activity compared with cubooctahedral structures [39, 40, 42–44]. In this case, the experimental results observed by TEM images indicate that, in AgNPs-NaBH4 sample, the cubooctahedral structures appear with major frequency and with a significant minor particle size (17 nm) with respect to the AgNPs-EG sample (40 nm). For this reason a higher catalytic activity of AgNPs-NaBH4 sample would be expected. In this sense, the catalytic activity of the AgNPs-NaBH4 and AgNPs-EG structures can be evaluated by cyclic voltammetry.


## 3.4. Cyclic Voltammetry

In order to demonstrate experimentally the result obtained by DFT simulations, Figure4 shows the cyclic voltammogram corresponding to the AgNPs with cubooctahedral (CO) and icosahedral (Ih) configuration. It can be seen that in the case of CO nanoparticles there is an increase in the current value of the redox processes involved in comparison with the Ih nanoparticles. Also, the cyclic voltammogram of both configurations is similar; no displacements are observed in the voltage values and they differ only in the associated current intensity reduction capability. This fact supports the theoretical analysis (DFT) presented previously.Figure 4
Cyclic voltammogram of the icosahedral and cuboctahedral structures of Ag nanoparticles in acid medium evaluated with a solution of H2SO4 (0.5 M). Scan rate 50 mVs−1 at 25°C in the presence of N2.


## 3.5. Antibacterial Effect

The antibacterial activity of the AgNPs is showed in Figure5. Figure 5(a) shows the antimicrobial property of AgNPs-EG associated with the decahedral structure. In this image can be appreciated the inhibition zone corresponding to AgNPs solution at concentrations of 5, 10, and 15 mM; the values measured in this case were 6.5, 7.5, and 10 mm, respectively (Figure 5(c)). Regarding the AgNPs-NaBH4 sample with cubooctahedral structure, Figure 5(b) illustrates in qualitative way the antibacterial effect with respect to theE. coli. Inhibitions zones of 7.5, 9 and 15 mm were observed in this case (Figure 5(c)). In this work, it was found that the growth inhibition effect inS. coli depends on the Ag concentration promoting good antimicrobial effect on lower Ag concentration (15 mM). These results confirmed the antibacterial properties of silver nanoparticles; however, the most significant one of these results is to compare the antibacterial effect as a function of the AgNPs structures. According to the theoretical (DFT analysis) and experimental (cyclic voltammetry) results obtained, the cubooctahedral structure (AgNPs-NaBH4) exhibits the highest catalytic and antibacterial activity.Figure 5
(a)
(b)
(c)


## 4. Conclusions

The AgNPs synthesis route determines the structure obtained. Factors such as the reducing agent, the reduction rate, and temperature determine the formation of crystal defects in the Ag nanoparticles. The structure associated with the AgNPs-NaBH4 sample can be considered as a cubooctahedral structure, while the AgNPs-EG sample exhibits an icosahedral structure. Theoretical analyses (DFT) have made it possible to evaluate the reactivity of each structure and theoretically predict the reactivity of the AgNPs obtained. These results were proven experimentally by cyclic voltammetry and through a test of antibacterial effect. Due to their small size, the cubooctahedral structures obtained by NaBH4 were the most reactive and these AgNPs exhibit a major electrochemical and antibacterial activity.



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*Source: 9372056-2016-11-30.xml*