# Synthesis and Characterization of Optically Active Fractal Seed Mediated Silver Nickel Bimetallic Nanoparticles

Authors: Joseph Adeyemi Adekoya; Enock Olugbenga Dare; Michael Adediran Mesubi; Neerish Revaprasadu
Journal: Journal of Materials
 (2014)

---

## Abstract

The synthesis of new seed mediated AgNi allied bimetallic nanocomposites was successfully carried out by the successive reduction of the metal ions in diethylene glycol, ethylene glycol, glycerol, and pentaerythritol solutions, with concomitant precipitation of Ag/Ni bimetal sols. The optical measurement revealed the existence of distinct band edge with surface plasmon resonance (SPR) in the region of 400–425 nm and excitonic emission with maximum peak at 382 nm which were reminiscent of cluster-in-cluster surface enriched bimetallic silver-nickel sols. The morphological characterization by transmission electron microscopy, high resolution transmission electron microscopy, and X-ray diffraction analyses complimented by surface scan using X-ray photoelectron spectroscopy strongly supported the formation of intimately alloyed face-centered silver/nickel nanoclusters.


---

## Body

## 1. Introduction

The synthesis of new materials and the investigation of their characteristic properties is a noble aspect of nanochemistry due to the fact that various applications have been found for these materials in electronics, sensor, optical devices, waveguide, and fibre optics to mention a few. As a result, immense effort directed at synthesizing and manipulating the size, size distribution, and shape of these nanoparticles is inexhaustive. In particular, silver nanoparticles have been largely prepared and evaluated for sensor, optical, and antimicrobial properties. However, the nanocomposite silver nickel is being considered due to its synergistic effect which offers a wide range of applications that include catalysis. Monodispersed allied silver/nickel nanoparticles have been prepared using various chemical routes based on hydrolytic reduction of the metal ions followed by polycondensation of the reduced nuclei. The reactions are largely thermodynamically driven with respect to temperature and time to produce uniformly distributed nanosized particles.There are a number of literature reports on AgNi nanoparticles; Xiao and coworkers presented an approach in which laser ablation was used in the deposition silver/nickel bimetallic nanoparticles; the laser was a pulsed Nd:YAG laser source [1, 2]. The effective nonlinear absorption of Ni/Ag nanoparticles was found to be higher than that of pristine Ag nanoparticles. The nanoparticles were synthesized via wet chemical reduction in C19H42BrN (CTAB) matrix, hydrazine hydrate being the reducing agent, and it was found to be a very potent material for optical limiting and photonic applications in the work of Kishore et al., 2012 [3].Likewise, one-step facile synthetic route was also devised for the preparation of well-dispersed Ag/Ni core-shell nanoparticles with uniform and intact shells. The process was performed by the reduction of silver nitrate and nickel nitrate with sodium borohydride in water-in-oil (W/O) microemulsions of water/polyoxyethylene, nonylphenol, and polyoxyethylene nonylphenol/n-heptane. The Ag/Ni core-shell nanoparticles showed a high catalytic activity for degradation reaction of eosin Y [4].So, also, Lee and Chen have successfully prepared NiAg core-shell nanoparticles by successive hydrazine reduction of metal salts in ethylene glycol without the addition of protective agents. To prohibit the particles from coalescing, the appropriate nickel concentration for the coating of Ag nanoshells was less than 1.0 mm. The TEM and XPS surface composition studies indicated that Ni cores were fully covered by Ag nanoshells. The shell thickness was controlled by the silver nitrate concentration. The EDX and XRD analyses reveal that both Ni cores and Ag shells have a face-centered cubic structure.Later on, a synthetic method was developed in which polyethyleneimine (PEI) was used as a protective agent to fabricate Ni-core/Ag-shell (NiAg) nanoparticles. The produced NiAg nanoparticles were monodispersed, and the core was about 6.2 nm in diameter, and the shell thickness was about 0.85 nm. In the nickel concentration of 0.25–25 mM; the size of the NiAg nanoparticles showed no significant change for different thickness of Ag coating. X-ray photoelectron spectroscopy indicated that both Ni cores and Ag shells had face-centered-cubic structure, and the Ni cores were fully covered by Ag shells. Moreover, a peak was observed at 430 nm in the absorption band of the NiAg nanoparticles, which is consistent with the characteristic spectra of Ag nanoparticles. The sample was nearly superparamagnetic. The coating of Ag shells led to a decrease of supersaturation magnetization, which indicated that the Ni/Ag interface quenched the magnetic moment. The thermal and XRD analyses also indicated that the Ag shells provided a better protection for Ni/Ag nanoparticles as an antioxidant compared to pure Ni nanoparticles [5].In this work, we have extended earlier approaches to preparing silver/nickel nanoparticles which could be stable over a period of six months by coprecipitating the allied nanoparticles from organic and aqueous phases. The use of chelating organic groups is usually intended to thermodynamically control anisotropic nucleation and particle growth processes. Thus, the choice of polyols was made primarily considering their nontoxicity and the ability to furnish the base hydrolysis required for the reduction and nucleation process.


## 2. Experimental

The seed mediated or successive addition method was modified from the literature method and used to prepare monodispersed bimetallic AgNi nanoparticles in different polyols at optimum concentration of metal precursors and controlled temperature [6, 7]. The reactions for the formation of the bimetallic nanoparticles via anisotropic nucleation and growth are shown in Scheme 1.Scheme 1
Scheme of reaction for the formation of Ag/Ni nanocluster prior to anisotropic nucleation and particle growth.


### 2.1. Materials

All inorganic salts, solvents, and chemical reagents used were analytical grade and were purchased from Sigma-Aldrich Corporation, UK. They are as follow: silver nitrate, nickel (II) acetate, glycerol, ethylene glycol (EG) and diethylene glycol (DEG), pentaerythritol (PET), poly(vinyl pyrrolidone) (PVP), methanol (99.5% w/w), and ethanol (99.5% w/w).


### 2.2. Synthesis of Ag/Ni Nanoparticles

The bimetallic nanosized particles of AgNi were prepared by the seed growth or successive addition method [8] as follows: 15 mL glycerol (99.5% w/w) was measured into a round bottom flask containing a magnetic stirrer, and (0.03–0.08 mmol) PVP was added. Then, the mixture was stirred and gradually heated at the rate of 1.7°C/minute to 150°C. Afterward (0.41–2.01 mmol) Ni(CH3CO2)2
·4H2O was injected into the hot solution; the colour rapidly changed to Prussian green. After allowing the growth of Ni nanoparticles which sometimes acted as a seed, (0.35–1.24 mmol) AgNO3 was injected into the colloidal mixture and the reaction was continued for 4 hours with continuous stirring. After the hot injection of silver nitrate, pale brown coloured Ag/Ni sol was obtained. While hot, the AgNi sol was copiously washed with methanol several times and centrifuged at 4400 rpm for 10–15 min. to remove excess unreacted stabilizer. The AgNi sol was later redispersed in ethanol.Similarly, the aqueous coprecipitation of Ag/Ni sol was carried out by using 0.02–0.13 mmol PVP, 24.01–37.25 mmol PET (capping agent), 0.12–0.82 mmol AgNO3, and 0.66–1.48 mmol Ni(CO2CH3)2
·4H2O in 100 mL Milliken deionized H2O at 90°C. The procedure was repeated at 160°C, 2 hours, and 175°C, 2 hours; and then for ethylene glycol at 160°C, 3 hours, and 175°C, 2 hours; diethylene glycol at 190°C, 2 hours, and at 200°C, 2 hours. The difference in colour indicated the formation of different AgNi nanoparticles.


### 2.3. Isolation of Ag/Ni Nanoparticles

The centrifuged sols obtained after decantation were redispersed in double distilled ethanol and cleaned in ultrasonic bath at 50°C for 60 minutes before further characterization.


### 2.4. Characterization

#### 2.4.1. Optical Characterization

A Varian Cary 50 Conc UV-Vis spectrophotometer was used to carry out the optical measurements and the samples were placed in silica cuvettes (1 cm path length), using ethanol as a reference solvent. A PerkinElmer LS 55 Luminescence spectrometer was used to measure the photoluminescence of the particles. The samples were placed in a quartz cuvette (1 cm path length).


#### 2.4.2. Structural Characterization

The crystalline phase was identified by XRD, employing a scanning rate of 0.05° min−1 in a 2
θ range from 20 to 80°, using a Bruker AXS D8 diffractometer equipped with nickel filtered Cu Kα radiation (λ
=
1.5406 Å) at 40 kV, 40 mA, and at room temperature. The morphology and particle sizes of the samples were characterized by a JEOL 1010 TEM with an accelerating voltage of 100 kV, Megaview III camera, and Soft Imaging Systems iTEM software. The detail morphological and structural features were investigated using HRTEM images with a JEOL 2010 TEM operated at an accelerating voltage of 200 kV.The survey of surface property and high resolution spectra of nanoparticles were collected using XPS PHI 5000 Versaprobe-Scanning ESCA Microprobe, with 100μm 25 W 15 kV Al monochromatic X-ray beams.


## 2.1. Materials

All inorganic salts, solvents, and chemical reagents used were analytical grade and were purchased from Sigma-Aldrich Corporation, UK. They are as follow: silver nitrate, nickel (II) acetate, glycerol, ethylene glycol (EG) and diethylene glycol (DEG), pentaerythritol (PET), poly(vinyl pyrrolidone) (PVP), methanol (99.5% w/w), and ethanol (99.5% w/w).


## 2.2. Synthesis of Ag/Ni Nanoparticles

The bimetallic nanosized particles of AgNi were prepared by the seed growth or successive addition method [8] as follows: 15 mL glycerol (99.5% w/w) was measured into a round bottom flask containing a magnetic stirrer, and (0.03–0.08 mmol) PVP was added. Then, the mixture was stirred and gradually heated at the rate of 1.7°C/minute to 150°C. Afterward (0.41–2.01 mmol) Ni(CH3CO2)2
·4H2O was injected into the hot solution; the colour rapidly changed to Prussian green. After allowing the growth of Ni nanoparticles which sometimes acted as a seed, (0.35–1.24 mmol) AgNO3 was injected into the colloidal mixture and the reaction was continued for 4 hours with continuous stirring. After the hot injection of silver nitrate, pale brown coloured Ag/Ni sol was obtained. While hot, the AgNi sol was copiously washed with methanol several times and centrifuged at 4400 rpm for 10–15 min. to remove excess unreacted stabilizer. The AgNi sol was later redispersed in ethanol.Similarly, the aqueous coprecipitation of Ag/Ni sol was carried out by using 0.02–0.13 mmol PVP, 24.01–37.25 mmol PET (capping agent), 0.12–0.82 mmol AgNO3, and 0.66–1.48 mmol Ni(CO2CH3)2
·4H2O in 100 mL Milliken deionized H2O at 90°C. The procedure was repeated at 160°C, 2 hours, and 175°C, 2 hours; and then for ethylene glycol at 160°C, 3 hours, and 175°C, 2 hours; diethylene glycol at 190°C, 2 hours, and at 200°C, 2 hours. The difference in colour indicated the formation of different AgNi nanoparticles.


## 2.3. Isolation of Ag/Ni Nanoparticles

The centrifuged sols obtained after decantation were redispersed in double distilled ethanol and cleaned in ultrasonic bath at 50°C for 60 minutes before further characterization.


## 2.4. Characterization

### 2.4.1. Optical Characterization

A Varian Cary 50 Conc UV-Vis spectrophotometer was used to carry out the optical measurements and the samples were placed in silica cuvettes (1 cm path length), using ethanol as a reference solvent. A PerkinElmer LS 55 Luminescence spectrometer was used to measure the photoluminescence of the particles. The samples were placed in a quartz cuvette (1 cm path length).


### 2.4.2. Structural Characterization

The crystalline phase was identified by XRD, employing a scanning rate of 0.05° min−1 in a 2
θ range from 20 to 80°, using a Bruker AXS D8 diffractometer equipped with nickel filtered Cu Kα radiation (λ
=
1.5406 Å) at 40 kV, 40 mA, and at room temperature. The morphology and particle sizes of the samples were characterized by a JEOL 1010 TEM with an accelerating voltage of 100 kV, Megaview III camera, and Soft Imaging Systems iTEM software. The detail morphological and structural features were investigated using HRTEM images with a JEOL 2010 TEM operated at an accelerating voltage of 200 kV.The survey of surface property and high resolution spectra of nanoparticles were collected using XPS PHI 5000 Versaprobe-Scanning ESCA Microprobe, with 100μm 25 W 15 kV Al monochromatic X-ray beams.


## 2.4.1. Optical Characterization

A Varian Cary 50 Conc UV-Vis spectrophotometer was used to carry out the optical measurements and the samples were placed in silica cuvettes (1 cm path length), using ethanol as a reference solvent. A PerkinElmer LS 55 Luminescence spectrometer was used to measure the photoluminescence of the particles. The samples were placed in a quartz cuvette (1 cm path length).


## 2.4.2. Structural Characterization

The crystalline phase was identified by XRD, employing a scanning rate of 0.05° min−1 in a 2
θ range from 20 to 80°, using a Bruker AXS D8 diffractometer equipped with nickel filtered Cu Kα radiation (λ
=
1.5406 Å) at 40 kV, 40 mA, and at room temperature. The morphology and particle sizes of the samples were characterized by a JEOL 1010 TEM with an accelerating voltage of 100 kV, Megaview III camera, and Soft Imaging Systems iTEM software. The detail morphological and structural features were investigated using HRTEM images with a JEOL 2010 TEM operated at an accelerating voltage of 200 kV.The survey of surface property and high resolution spectra of nanoparticles were collected using XPS PHI 5000 Versaprobe-Scanning ESCA Microprobe, with 100μm 25 W 15 kV Al monochromatic X-ray beams.


## 3. Results and Discussion

The polyol stabilized nanoparticles were very stable both in the liquid and solid phases. The stability was checked by following the absorbance spectra over extended periods of six months and reproducible absorption maxima were obtained typical of Ag/Ni sol property. The oxo groups present in the vinylpyrrolidone stabilized by the bimetallic nanoparticles as proposed by Veronese, 2001 [9]. The use of sodium borohydride resulted in fast reduction of metal ions when pentaerythritol was used as a capping agent in the aqueous phase synthesis of Ag/Ni sols.


### 3.1. Optical Properties of Ag/Ni Sols

The UV-Visible characterization of the prepared bimetallic AgNi cluster was carried out in absolute ethanol and the spectra recorded for various mole ratios of metal precursors and stabilizer are presented in Figure1.Figure 1
Absorbance Spectra of AgNi sols with different stabilizer/capping agents: PVP/DEG at 190°C, 2 h; PVP/EG at 175°C, 2 h; PVP/GLY at 175°C, 2 h; PVP/PET at 90°C, 2 h.In all, there was a clear evidence of surface plasmon band (SPB) occurring at 416.04 nm, 438.96 nm, 452.00 nm, and 436.97 nm for PVP/DEG, PVP/GLY, PVP/EG, and PVP/PET stabilized/capped sols, respectively (Figure1), which was similar to the maximum wavelength of absorption of monometallic Ag nanoparticles. This suggests that the surface of the bimetallic nanoparticles is enriched with Ag, and there is a possible existence of a core-shell structure as reported in previous studies [3, 4].Furthermore, change in temperature and time of reaction as expected caused a shift in the maximum wavelength of AgNi PVP/EG synthesized at 175°C, 2 h, and at 160°C, 3 h (Figure2).Figure 2
Effect of change in temperature and time of reaction on the absorbance property of Ag/Ni sols passivated with PVP/EG at 160°C, 3 h and 175°C, 2 h.There was a corresponding blue shift in absorbance wavelength from 452.0 to 430.0 nm. Similarly, Ag/Ni PVP/PET synthesized at 90°C, 4 h and 2 h (Figure3), exhibited a shift in maximum wavelength from 437 to 436 nm, respectively. The latter on each occasion exhibits a narrow peak with a higher intensity, which often results to particles with a lower aspect ratio.Figure 3
Effect of change in temperature and time of reaction on the absorbance property of Ag/Ni sols capped with PVP/PET at 90°C, 4 h, and 90°C, 2 h.Photoluminescence (PL) measurements were done for the prepared AgNi sols at a very dilute concentration. The PL spectra, Figures4 and 5, show that there is an emission of appropriate quantum yield indicated by high fluorophores intensity.Figure 4
PL emission Spectra of AgNi NPs stabilized with PVP/EG at 175°C, 2 h (blue), and 160°C, 3 h (red).Figure 5
PL emission Spectra of AgNi NPs stabilized with PVP/GLY at 160°C, 2 h (red), and 150°C, 4 h (blue).In all, the emission wavelength was independent of excitation wavelength, indicating a fluorescence property. For an excitation at 320 nm, the AgNi PVP/EG synthesized at 175°C, 2 h, and 160°C, 3 h (Figure4), and exhibited an emission at 382 and 379 nm, respectively. Whereas a slight increase in emission wavelength was observed for AgNi NPs stabilized with PVP/GLY at 160°C, 2 h, and 150°C, 4 h (Figure 5). AgNi NPs were found to emit at 345 and 350 nm, respectively. The emission band edges were close to the absorption band edges in all the optical spectra considered; thus further indicating the fluorescence property of the prepared Ag/Ni nanoparticles. However, the fluorescence emission of PVP/PET functionalized AgNi sols (Figure 6) excited at 340 nm occurred at 392 nm which was relatively close to the emission peak of Ag sols. It was observed that fluorophore emission occurred in Ag/Ni just before the corresponding absorbance at 440 nm due to spin orbit coupling [10].Figure 6
Combined UV-Vis/PL emission spectra of AgNi NPs stabilized with PVP/PET at 90°C, 4 h, showing relative position of electronic transition (blue) and emission due to S1-S0 transition (red).The optimum mole ratios for the coprecipitation reactions that produced AgNi sols from different metal precursors/stabilizer media occurred at the stoichiometry ratio of 12 : 14 : 1, 13 : 17 : 1, and 11 : 17 : 1 for AgNi/PVP/
EG, AgNi/PVPGLY, and AgNi/PVPDEG, respectively. At this mole ratio the nanoparticles formed colloidal dispersion which was easily redispersed in ethanol for the optical absorbance of Ag/Ni sols to be determined.The absorption band gaps of the Ag/Ni sols were also estimated by the direct band gap method [11] and were found to be 2.83 eV (438.96 nm, t
=
2 h), 2.98 eV (416.04 nm, t
=
2 h), 2.74 eV (452.00 nm, t
=
2 h), and 2.84 eV (436.97 nm, t
=
2 h) for PVP/GLY, PVP/DEG, PVP/EG, and PVP/PET functionalized Ag/Ni nanoparticles, respectively. The absorption edges were red-shifted from that of Ag and Ni bulk crystals given as 3.99 eV [12, 13] and 5.2 eV [14], respectively.


### 3.2. Morphology of AgNi Sols

The TEM images of the prepared AgNi sols as shown in the images in Figures7 and 8 revealed the existence of a well dispersed, nearly uniform sized spherical, and cube shaped AgNi nanoparticles. The HRTEM images confirmed the shape, size, and morphology of the AgNi NPs. The average size measured for AgNi NPs stabilized with PVP/GLY at 160°C, 2 h (Figures 7(a) and 7(b)), was 44.79
±
14.7 nm, while the mean size of those stabilized with PVP/DEG at 200°C, 2 h (Figure 8(a)), was 35.16
±
14.20 nm. But the average size of PVP/EG passivated AgNi NPs at 160°C, 3 h (Figure 8(b)), measured 65.34
±
14.0 nm.Figure 7
(a and b) TEM images of AgNi NPs stabilized with PVP/GLY at 160°C, 2 h; (c and d) corresponding HRTEM images of (a and b).Figure 8
TEM images of AgNi NPs stabilized with (a) PVP/DEG at 200°C, 2 h; (b) PVP/EG at 160°C, 3 h; (c and d) corresponding HRTEM images of (a and b).The HRTEM images (Figures7(c) and 7(d)) confirmed the existence of composite nanoparticles of AgNi. There was an overlap between the lattice planes of Ag and Co, resulting in the alloy formation observed. As for PVP/DEG stabilized AgNi NPs (Figure 8(c)) the HRTEM image showed the existence of well crystalline structure with lattice spacing measuring about 2.4 Å. However, the HRTEM of the PVP/EG passivated NPs (Figure 8(d)) showed a darkened edge. The thickness was about 14.46 nm, which is typical of a core-shell structure, and is in agreement with UV-Visible absorbance measurement.This also confirmed that the surface area of nickel atoms was covered by Ag atoms in the nanocomposites. The anisotropy of particles growth was largely determined by the formation of a critical nucleus which occurred at the reduction potential of the individual metals. Furthermore, according to Wu and Lai, 2004 [15], core-shell structure occurs when a large difference exists in reduction potentials of the composite metal ions. Hence, the mechanism of growth for the AgNi nanoparticles under this condition is reaction limited.The bimetallic nanoparticles were monodispersed and highly crystalline in PVP/PET polymeric network. The TEM micrograph of AgNi sols (Figure9(a)) further revealed nanoparticles which were monodispersed with a mean particle size of 32.41
±
4.20 nm. There was a clue from the HRTEM image (Figure 9(b)) of the core-shell nature of the Ag/Ni nanoparticles in the sense that the core of each quasispherical nanoparticle was occupied by a trigonal structure of about 18.57 nm.Figure 9
(a) TEM image of AgNi NPs; (b) HRTEM image of AgNi NPs functionalized with PVP/PET at 90°C, 4 h.No doubt a silver core was inside a nickel shell. The image also revealed the existence of two particles within a nickel shell which was in agreement with earlier work done to synthesise and characterize AgNi core-shell bimetallic nanoparticles [16]. The mole ratio of metal precursors has been shown previously to contribute to the formation of the core-shell structure [4].The p-XRD measurements were performed on a Bruker AXS D8 powder diffractometer over a 2-thetar angle of 20–90° at an angular resolution of 0.02°. The XRD patterns are shown in Figure10.Figure 10
XRD patterns of AgNi nanoparticles stabilized with PVP/DEG at 190°C, 2 h; PVP/EG at 160°C, 3 h; PVP/GLY at 160°C, 2 h.Four distinct reflections of PVP/DEG stabilized AgNi NPs were observed at2
θ values of 38.45°, 64.60°, 77.66°, and 81.76° corresponding to {
111
}, {
220
}, {
311
}, and {
222
} crystal planes, respectively. These peaks can be indexed to the cubic structure of metallic Ag, JCPDS, 1974 [17]. In addition, the XRD analysis also revealed two main characteristic peaks for the {
111
} and {
220
} crystal planes of metallic Ni at 2
θ = 44.62° and 76.40° [18].The characteristic peak of Ni at2
θ = 44.62° corresponding to {
111
} planes possibly overlapped with that for the {
200
} planes of Ag at 2
θ = 44.54°. Therefore, both Ni cores and Ag shells have a fcc structure. Although, it is known that nickel is easily oxidized to the oxides or hydroxide by water, no oxides or hydroxide such as NiO, Ni2O3, and Ni(OH)2 were observed from the phase analysis by XRD, indicating the formation of pure nickel of high crystalline quality. Similar phase characteristic was observed for the XRD pattern of AgNi stabilized with PVP/EG at 160°C, 3 h, and PVP/GLY at 160°C, 2 h (Figure 10). The sizes of these nanocomposites based on XRD measurement at {
100
} plain were 31.64, 14.55, and 18.5 nm for PVP/DEG, PVP/EG, and PVP/GLY stabilized AgNi nanoparticles, respectively. These values fell within the range of the estimates obtained from TEM measurements.


### 3.3. XPS Result

The wide area spectrum and the high resolution scans of the core levels of AgNi nanocluster are presented in Figures11–14.Figure 11
XPS spectrum of AgNi nanoparticles stabilized with PVP/DEG at 200°C, 2 h.Figure 12
High resolution scan of Ag core levels.Figure 13
High resolution scan of Ni2p core levels.Figure 14
High resolution scan of O1s core levels.In order to confirm the existence of the composite nature of AgNi nanoparticles, XPS measurements were carried out with (XPS) PHI 5000 Versaprobe-Scanning ESCA Microprobe, with 100μm 25 W 15 kV Al monochromatic X-ray beams. The wide area scan (Figure 11), indicated the presence of Ag, Ni, O, N, and C according to their binding energies, but the characteristic XPS peaks of Ag (3d5/2) (Figure 12) and Ni(2p3/2) peaks (Figure 13) appeared at 368.45 eV and 852.87 eV, respectively [19, 20]. The surface atomic ratio of Ag to Ni in AgNi was 0.5 : 1.6 which rather confirmed an alloy structure for PVP/DEG stabilized AgNi nanobimetallic particles.Considering the core levels of Ag (Figure12) two strong peaks were identified at (3d5/2) 367.60 eV and (3d3/2) 375.60 eV assigned to Ag2O, which was in agreement with XRD analysis. Similarly, deconvoluted Ni2p band (Figure 13) was resolved to give another peak at 872.96 which was assigned to Ni–M (BE).The O1s peak at 530 eV (Figure14) may have resulted from adsorbed oxygen [21]. There were no XPS peaks for NiO, Ni2O3, and Ni(OH)2, showing that Ni was not oxidized to the oxides or hydroxide. A Comparison of the relative areas of integrated intensity showed that Ni0 was a predominant component of the outer surface of the synthesized core-shell nanoparticles.


## 3.1. Optical Properties of Ag/Ni Sols

The UV-Visible characterization of the prepared bimetallic AgNi cluster was carried out in absolute ethanol and the spectra recorded for various mole ratios of metal precursors and stabilizer are presented in Figure1.Figure 1
Absorbance Spectra of AgNi sols with different stabilizer/capping agents: PVP/DEG at 190°C, 2 h; PVP/EG at 175°C, 2 h; PVP/GLY at 175°C, 2 h; PVP/PET at 90°C, 2 h.In all, there was a clear evidence of surface plasmon band (SPB) occurring at 416.04 nm, 438.96 nm, 452.00 nm, and 436.97 nm for PVP/DEG, PVP/GLY, PVP/EG, and PVP/PET stabilized/capped sols, respectively (Figure1), which was similar to the maximum wavelength of absorption of monometallic Ag nanoparticles. This suggests that the surface of the bimetallic nanoparticles is enriched with Ag, and there is a possible existence of a core-shell structure as reported in previous studies [3, 4].Furthermore, change in temperature and time of reaction as expected caused a shift in the maximum wavelength of AgNi PVP/EG synthesized at 175°C, 2 h, and at 160°C, 3 h (Figure2).Figure 2
Effect of change in temperature and time of reaction on the absorbance property of Ag/Ni sols passivated with PVP/EG at 160°C, 3 h and 175°C, 2 h.There was a corresponding blue shift in absorbance wavelength from 452.0 to 430.0 nm. Similarly, Ag/Ni PVP/PET synthesized at 90°C, 4 h and 2 h (Figure3), exhibited a shift in maximum wavelength from 437 to 436 nm, respectively. The latter on each occasion exhibits a narrow peak with a higher intensity, which often results to particles with a lower aspect ratio.Figure 3
Effect of change in temperature and time of reaction on the absorbance property of Ag/Ni sols capped with PVP/PET at 90°C, 4 h, and 90°C, 2 h.Photoluminescence (PL) measurements were done for the prepared AgNi sols at a very dilute concentration. The PL spectra, Figures4 and 5, show that there is an emission of appropriate quantum yield indicated by high fluorophores intensity.Figure 4
PL emission Spectra of AgNi NPs stabilized with PVP/EG at 175°C, 2 h (blue), and 160°C, 3 h (red).Figure 5
PL emission Spectra of AgNi NPs stabilized with PVP/GLY at 160°C, 2 h (red), and 150°C, 4 h (blue).In all, the emission wavelength was independent of excitation wavelength, indicating a fluorescence property. For an excitation at 320 nm, the AgNi PVP/EG synthesized at 175°C, 2 h, and 160°C, 3 h (Figure4), and exhibited an emission at 382 and 379 nm, respectively. Whereas a slight increase in emission wavelength was observed for AgNi NPs stabilized with PVP/GLY at 160°C, 2 h, and 150°C, 4 h (Figure 5). AgNi NPs were found to emit at 345 and 350 nm, respectively. The emission band edges were close to the absorption band edges in all the optical spectra considered; thus further indicating the fluorescence property of the prepared Ag/Ni nanoparticles. However, the fluorescence emission of PVP/PET functionalized AgNi sols (Figure 6) excited at 340 nm occurred at 392 nm which was relatively close to the emission peak of Ag sols. It was observed that fluorophore emission occurred in Ag/Ni just before the corresponding absorbance at 440 nm due to spin orbit coupling [10].Figure 6
Combined UV-Vis/PL emission spectra of AgNi NPs stabilized with PVP/PET at 90°C, 4 h, showing relative position of electronic transition (blue) and emission due to S1-S0 transition (red).The optimum mole ratios for the coprecipitation reactions that produced AgNi sols from different metal precursors/stabilizer media occurred at the stoichiometry ratio of 12 : 14 : 1, 13 : 17 : 1, and 11 : 17 : 1 for AgNi/PVP/
EG, AgNi/PVPGLY, and AgNi/PVPDEG, respectively. At this mole ratio the nanoparticles formed colloidal dispersion which was easily redispersed in ethanol for the optical absorbance of Ag/Ni sols to be determined.The absorption band gaps of the Ag/Ni sols were also estimated by the direct band gap method [11] and were found to be 2.83 eV (438.96 nm, t
=
2 h), 2.98 eV (416.04 nm, t
=
2 h), 2.74 eV (452.00 nm, t
=
2 h), and 2.84 eV (436.97 nm, t
=
2 h) for PVP/GLY, PVP/DEG, PVP/EG, and PVP/PET functionalized Ag/Ni nanoparticles, respectively. The absorption edges were red-shifted from that of Ag and Ni bulk crystals given as 3.99 eV [12, 13] and 5.2 eV [14], respectively.


## 3.2. Morphology of AgNi Sols

The TEM images of the prepared AgNi sols as shown in the images in Figures7 and 8 revealed the existence of a well dispersed, nearly uniform sized spherical, and cube shaped AgNi nanoparticles. The HRTEM images confirmed the shape, size, and morphology of the AgNi NPs. The average size measured for AgNi NPs stabilized with PVP/GLY at 160°C, 2 h (Figures 7(a) and 7(b)), was 44.79
±
14.7 nm, while the mean size of those stabilized with PVP/DEG at 200°C, 2 h (Figure 8(a)), was 35.16
±
14.20 nm. But the average size of PVP/EG passivated AgNi NPs at 160°C, 3 h (Figure 8(b)), measured 65.34
±
14.0 nm.Figure 7
(a and b) TEM images of AgNi NPs stabilized with PVP/GLY at 160°C, 2 h; (c and d) corresponding HRTEM images of (a and b).Figure 8
TEM images of AgNi NPs stabilized with (a) PVP/DEG at 200°C, 2 h; (b) PVP/EG at 160°C, 3 h; (c and d) corresponding HRTEM images of (a and b).The HRTEM images (Figures7(c) and 7(d)) confirmed the existence of composite nanoparticles of AgNi. There was an overlap between the lattice planes of Ag and Co, resulting in the alloy formation observed. As for PVP/DEG stabilized AgNi NPs (Figure 8(c)) the HRTEM image showed the existence of well crystalline structure with lattice spacing measuring about 2.4 Å. However, the HRTEM of the PVP/EG passivated NPs (Figure 8(d)) showed a darkened edge. The thickness was about 14.46 nm, which is typical of a core-shell structure, and is in agreement with UV-Visible absorbance measurement.This also confirmed that the surface area of nickel atoms was covered by Ag atoms in the nanocomposites. The anisotropy of particles growth was largely determined by the formation of a critical nucleus which occurred at the reduction potential of the individual metals. Furthermore, according to Wu and Lai, 2004 [15], core-shell structure occurs when a large difference exists in reduction potentials of the composite metal ions. Hence, the mechanism of growth for the AgNi nanoparticles under this condition is reaction limited.The bimetallic nanoparticles were monodispersed and highly crystalline in PVP/PET polymeric network. The TEM micrograph of AgNi sols (Figure9(a)) further revealed nanoparticles which were monodispersed with a mean particle size of 32.41
±
4.20 nm. There was a clue from the HRTEM image (Figure 9(b)) of the core-shell nature of the Ag/Ni nanoparticles in the sense that the core of each quasispherical nanoparticle was occupied by a trigonal structure of about 18.57 nm.Figure 9
(a) TEM image of AgNi NPs; (b) HRTEM image of AgNi NPs functionalized with PVP/PET at 90°C, 4 h.No doubt a silver core was inside a nickel shell. The image also revealed the existence of two particles within a nickel shell which was in agreement with earlier work done to synthesise and characterize AgNi core-shell bimetallic nanoparticles [16]. The mole ratio of metal precursors has been shown previously to contribute to the formation of the core-shell structure [4].The p-XRD measurements were performed on a Bruker AXS D8 powder diffractometer over a 2-thetar angle of 20–90° at an angular resolution of 0.02°. The XRD patterns are shown in Figure10.Figure 10
XRD patterns of AgNi nanoparticles stabilized with PVP/DEG at 190°C, 2 h; PVP/EG at 160°C, 3 h; PVP/GLY at 160°C, 2 h.Four distinct reflections of PVP/DEG stabilized AgNi NPs were observed at2
θ values of 38.45°, 64.60°, 77.66°, and 81.76° corresponding to {
111
}, {
220
}, {
311
}, and {
222
} crystal planes, respectively. These peaks can be indexed to the cubic structure of metallic Ag, JCPDS, 1974 [17]. In addition, the XRD analysis also revealed two main characteristic peaks for the {
111
} and {
220
} crystal planes of metallic Ni at 2
θ = 44.62° and 76.40° [18].The characteristic peak of Ni at2
θ = 44.62° corresponding to {
111
} planes possibly overlapped with that for the {
200
} planes of Ag at 2
θ = 44.54°. Therefore, both Ni cores and Ag shells have a fcc structure. Although, it is known that nickel is easily oxidized to the oxides or hydroxide by water, no oxides or hydroxide such as NiO, Ni2O3, and Ni(OH)2 were observed from the phase analysis by XRD, indicating the formation of pure nickel of high crystalline quality. Similar phase characteristic was observed for the XRD pattern of AgNi stabilized with PVP/EG at 160°C, 3 h, and PVP/GLY at 160°C, 2 h (Figure 10). The sizes of these nanocomposites based on XRD measurement at {
100
} plain were 31.64, 14.55, and 18.5 nm for PVP/DEG, PVP/EG, and PVP/GLY stabilized AgNi nanoparticles, respectively. These values fell within the range of the estimates obtained from TEM measurements.


## 3.3. XPS Result

The wide area spectrum and the high resolution scans of the core levels of AgNi nanocluster are presented in Figures11–14.Figure 11
XPS spectrum of AgNi nanoparticles stabilized with PVP/DEG at 200°C, 2 h.Figure 12
High resolution scan of Ag core levels.Figure 13
High resolution scan of Ni2p core levels.Figure 14
High resolution scan of O1s core levels.In order to confirm the existence of the composite nature of AgNi nanoparticles, XPS measurements were carried out with (XPS) PHI 5000 Versaprobe-Scanning ESCA Microprobe, with 100μm 25 W 15 kV Al monochromatic X-ray beams. The wide area scan (Figure 11), indicated the presence of Ag, Ni, O, N, and C according to their binding energies, but the characteristic XPS peaks of Ag (3d5/2) (Figure 12) and Ni(2p3/2) peaks (Figure 13) appeared at 368.45 eV and 852.87 eV, respectively [19, 20]. The surface atomic ratio of Ag to Ni in AgNi was 0.5 : 1.6 which rather confirmed an alloy structure for PVP/DEG stabilized AgNi nanobimetallic particles.Considering the core levels of Ag (Figure12) two strong peaks were identified at (3d5/2) 367.60 eV and (3d3/2) 375.60 eV assigned to Ag2O, which was in agreement with XRD analysis. Similarly, deconvoluted Ni2p band (Figure 13) was resolved to give another peak at 872.96 which was assigned to Ni–M (BE).The O1s peak at 530 eV (Figure14) may have resulted from adsorbed oxygen [21]. There were no XPS peaks for NiO, Ni2O3, and Ni(OH)2, showing that Ni was not oxidized to the oxides or hydroxide. A Comparison of the relative areas of integrated intensity showed that Ni0 was a predominant component of the outer surface of the synthesized core-shell nanoparticles.


## 4. Conclusion

The synthesis of silver nickel nanobimetallic particles by coprecipitation from nonaqueous and aqueous solutions with inorganic source precursors and polymer matrix was successfully accomplished. Subsequently, characterization of the prepared nanocomposites was done using optical spectroscopy, electron microscopy, X-ray diffraction (XRD), and x-photoelectron spectroscopy. The deconvolution of XPS high resolution and detailed surface elucidation of Ag/Ni bimetallic particles in polymer and polyol ligands revealed that their surfaces consisted of both metals which resulted into alloy or core-shell formation. Their binding energies were established showing that M–Ni and Ag–O bonds were formed at the corresponding energy intervals of 872.96 and 375.60 eV. The kinetic of anisotropic particle growth shows that, for alloy formation, the diffusion coefficients need to be many orders of magnitude larger than those of the bulk materials [22].The2
θ reflections for AgNi diffraction pattern showed a relative shift to higher 2
θ values corresponding to {
111
} planes possibly overlapped with that for the {
200
} planes of Ag at 2
θ = 44.54°. Meanwhile, for alloy formation as in the case of Ag/Ni, the addition of Ag causes clear shifts of the Ni {
111
} peaks towards the Ag peaks, following the effect that the higher the Ag content, the more shift, which indicated that the alloying of bimetallic Ag/Ni occurred.



---

*Source: 184216-2014-03-11.xml*