# Spectroscopic Analysis of Au-Cu Alloy Nanoparticles of Various Compositions Synthesized by a Chemical Reduction Method

Authors: Latif-ur-Rahman; Afzal Shah; Rumana Qureshi; Sher Bahadar Khan; Abdullah M. Asiri; Anwar-ul-Haq Ali Shah; Muhammad Ishaq; Mohammad Saleem Khan; Suzanne Kay Lunsford; Muhammad Abid Zia
Journal: Advances in Materials Science and Engineering
 (2015)

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## Abstract

Au-Cu alloy nanoparticles were synthesized by a chemical reduction method. Five samples having different compositions of Au and Cu (Au-Cu 3 : 1, Au-Cu 2 : 1, Au-Cu 1 : 1, Au-Cu 1 : 2, and Au-Cu 1 : 3) were prepared. The newly synthesized nanoparticles were characterized by electronic absorption, fluorescence, and X-ray diffraction spectroscopy (XRD). These alloy nanoparticles were also analyzed by SEM and TEM. The particle size was determined by SEM and TEM and calculated by Debye Scherrer’s equation as well. The results revealed that the average diameter of nanoparticles gets lowered from 80 to 65 nm as the amount of Cu is increased in alloy nanoparticles. Some physical properties were found to change with change in molar composition of Au and Cu. Most of the properties showed optimum values for Au-Cu alloy nanoparticles of 1 : 3. Cu in Au-Cu alloy caused decrease in the intensity of the emission peak and acted as a quencher. The fluorescence data was utilized for the evaluation of number of binding sites, total number of atoms in alloy nanoparticle, binding constant, and free energy of binding while morphology was deduced from SEM and TEM.


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## Body

## 1. Introduction

The fascinating properties and small dimensions of bimetallic nanoparticles have sparked an intense research activity and nowadays “nanoscience” is one of the rapidly developing multidisciplinary fields. Nanoparticles find interesting research applications in the field of chemical engineering [1, 2]. This is due to their unique catalytic, electrocatalytic, magnetic, optical, thermal, and electrical properties. Such properties of nanomaterials differ substantially from the typical properties of compact materials as quantum size effects come into play in particles of small dimensions. As particles size and shape play an important role in modifying the physical and chemical properties [3], so many efforts in nanostructural preparations have been focused to gain a control over the size and the shape of various types of nanoparticles [3]. Complete information about the size, shape, and structure of nanoparticles is essential prior to their applications in biomedical and other advanced fields [4].With decrease in the size of nanoparticles, changes occur in geometrical, quantum, and statistical effects. Electronic properties are also related to quantum size effect. No such effect can be observed if the size particles are decreased from macro- to microlevels. However, quantum effects become dominant when size is further decreased to nanorange [4]. In such nanoparticles, nearly all the physical properties of one of the metals are changed when its alloy is made with its partner metal. Bimetallic alloy nanoparticles may have random, core shell, cluster-in-cluster, and alloy structures. Random structures have no specific arrangement. In cluster-in-cluster structures, heavy metals mostly make nanoclusters and the other light metals act as binders. However, such structures have no specific order [5]. The alloy structures of bimetallic alloy nanoparticles are more common. There are various types of alloy structures that depend on the size of the combining metals. The most common alloy structures are intermetallic alloy and random alloy. Ag-Au and Au-Cu bimetallic alloy nanoparticles mostly form intermetallic alloy structures due to the differences in the size and binding abilities of Ag, Au, and Cu.Copper is the second metal having highest electrical conductivity [6]. However, a slight decrease in its electrical properties occurs when it captures oxygen because copper oxide is relatively lower in conductance than pure copper. Hence, copper cannot be found in metallic form due its higher tendency towards oxidation. During oxidation of copper, oxygen forms a coat around it, causing a decrease in its electrical conductivity. However, its bimetallic alloy nanoparticles can be prepared with Au which overcomes this problem. Although Au is expensive, only a small amount is the requirement of the developed method for the synthesis of Au-Cu alloy nanoparticles. Au enhances the conductivity of copper to a greater extent and its bimetallic alloy nanoparticles can be used for the developing of an electrochemical sensor for the detection of polycyclic aromatic hydrocarbons.Electrical performance of each of the Au and Cu metals can be improved by making their alloy [7]. This can be further improved by bringing their size on nanorange. Hence, Au-Cu alloy nanoparticles have vast applications in the development of electrochemical and biosensors. Oxidation of Au and Cu can be prevented by making their alloy nanoparticles [7, 8]. Loading nanoparticles at the surface region of polymer are of great interest due to their higher optical and potential applications [9, 10]. Such nanoparticles embedded in silica glasses also improve optical properties [11]. All of these properties are related to the frequencies of surface plasmon resonance. The frequencies depend upon the ratios and composition of metallic nanoparticles. Hence, Au-Cu bimetallic alloy nanoparticles with various compositions are manufactured.Bimetallic alloy nanoparticles can be prepared by various methods. The most prominent methods are coprecipitation method and colloidal dispersion method using conducting polymer as capping agent. Many chemists have prepared the nanoparticles by chemical reduction methods [12, 13]. But most of the researchers have applied such methods for the preparation of colloidal mixture [14]. No doubt, these methods have synthetic applications but, for making nanoparticles of very small dimensions, these face serious difficulties. Hence, for the preparation of Au-Cu alloy nanoparticles, chemical reduction is the simplest and least time consuming approach.


## 2. Experimental

### 2.1. Reagents and Apparatus

Copper chloride CuCl2 (98%), hydrogen gold chloride HAuCl4 (99%), ethylene glycol C2H6O2 (98%), and polyethyleneimine (2%) were purchased from Thermo Fisher Scientific Inc. (USA). Polyethyleneimine was obtained from Acros Organics. For characterization centrifuge (6000 rmp/s) (model: PRO 300, Ginotech, China), UV spectrophotometer, steady-state fluorescence spectrophotometer, Perkin Elmer LS 55 (Cary 100, Varian, Shimadzu, Tokyo, Japan), XRD (Bruker, SMART APEX diffractometer), scanning electron microscopy (SEM) (Tecnai G2 F2O X-Twin MAT), and TEM (Philips, Holand, Technai 20 model operating at 200 kV) were used.


### 2.2. Synthesis of Au and Cu Nanoparticles Using Chemical Reduction Method

10 mL of polyethyleneimine (2%) was poured to 20 mL of hydrogen gold chloride (1 mM) solution and heated at 100°C for 15 minutes. The appearance of yellowish black color evidenced the formation of Au nanoparticles that were confirmed by UV-Visible spectrophotometry. For preparation of Cu nanoparticles, 10 mL of polyethyleneimine (2%) was added to 20 mL of copper chloride solution (1 mM). The mixture was purged with argon blow for 30 minutes. The solution was heated in oven at 175°C for 30 minutes. The appearance of bluish black color showed the formation of Cu nanoparticles which was ensured by electronic absorption spectroscopy. Both Au and Cu nanoparticles were stable for more than six months.Au-Cu bimetallic alloy nanoparticles were synthesized by taking 20 mL of polyethyleneimine (2%) in 20 mL of hydrogen gold chloride (1 mM) solution. 20 mL of copper chloride (1 mM) was purged with argon blow and added. The whole sample was heated at 175°C for 15 minutes. The appearance of deep yellowish black color evidenced the synthesis of Au-Cu nanoparticles which were ensured by electronic absorption spectroscopy. By changing molar ratios of both precursor salts, Au-Cu alloy nanoparticles with various compositions, that is, 3 : 1, 2 : 1, 1 : 1, 1 : 2, and 1 : 3, were manufactured. Various chemicals along with their some important physical properties are mentioned in Table1. While the chemicals and conditions required for the preparation of Au-Cu alloy nanoparticles are listed in Table 2.Table 1
Details of the chemicals used.
S. number
Compounds
Molecular mass/g
Solubility in ethylene glycol
Purity (%)
Provider
1
HAuCl4
265.5
Soluble
97.95
Fluka
2
CuCl2
134.5
Soluble
98.00
Fluka
3
PEI
10000
Soluble
90.00
FlukaTable 2
Chemicals and conditions required for preparation of various compositions of Au-Cu alloy nanoparticles.
S. number
Composition Au-Cu
Volume/mL HAuCl4
Volume/mL CuCl2
PEI/mL
Purging/min
Heating 175°C/min
1
3 : 1
15
5
10
25
15
2
2 : 1
10
5
8
30
20
3
1 : 1
5
5
5
35
25
4
1 : 2
5
10
8
45
30
5
1 : 3
5
15
10
60
60


## 2.1. Reagents and Apparatus

Copper chloride CuCl2 (98%), hydrogen gold chloride HAuCl4 (99%), ethylene glycol C2H6O2 (98%), and polyethyleneimine (2%) were purchased from Thermo Fisher Scientific Inc. (USA). Polyethyleneimine was obtained from Acros Organics. For characterization centrifuge (6000 rmp/s) (model: PRO 300, Ginotech, China), UV spectrophotometer, steady-state fluorescence spectrophotometer, Perkin Elmer LS 55 (Cary 100, Varian, Shimadzu, Tokyo, Japan), XRD (Bruker, SMART APEX diffractometer), scanning electron microscopy (SEM) (Tecnai G2 F2O X-Twin MAT), and TEM (Philips, Holand, Technai 20 model operating at 200 kV) were used.


## 2.2. Synthesis of Au and Cu Nanoparticles Using Chemical Reduction Method

10 mL of polyethyleneimine (2%) was poured to 20 mL of hydrogen gold chloride (1 mM) solution and heated at 100°C for 15 minutes. The appearance of yellowish black color evidenced the formation of Au nanoparticles that were confirmed by UV-Visible spectrophotometry. For preparation of Cu nanoparticles, 10 mL of polyethyleneimine (2%) was added to 20 mL of copper chloride solution (1 mM). The mixture was purged with argon blow for 30 minutes. The solution was heated in oven at 175°C for 30 minutes. The appearance of bluish black color showed the formation of Cu nanoparticles which was ensured by electronic absorption spectroscopy. Both Au and Cu nanoparticles were stable for more than six months.Au-Cu bimetallic alloy nanoparticles were synthesized by taking 20 mL of polyethyleneimine (2%) in 20 mL of hydrogen gold chloride (1 mM) solution. 20 mL of copper chloride (1 mM) was purged with argon blow and added. The whole sample was heated at 175°C for 15 minutes. The appearance of deep yellowish black color evidenced the synthesis of Au-Cu nanoparticles which were ensured by electronic absorption spectroscopy. By changing molar ratios of both precursor salts, Au-Cu alloy nanoparticles with various compositions, that is, 3 : 1, 2 : 1, 1 : 1, 1 : 2, and 1 : 3, were manufactured. Various chemicals along with their some important physical properties are mentioned in Table1. While the chemicals and conditions required for the preparation of Au-Cu alloy nanoparticles are listed in Table 2.Table 1
Details of the chemicals used.
S. number
Compounds
Molecular mass/g
Solubility in ethylene glycol
Purity (%)
Provider
1
HAuCl4
265.5
Soluble
97.95
Fluka
2
CuCl2
134.5
Soluble
98.00
Fluka
3
PEI
10000
Soluble
90.00
FlukaTable 2
Chemicals and conditions required for preparation of various compositions of Au-Cu alloy nanoparticles.
S. number
Composition Au-Cu
Volume/mL HAuCl4
Volume/mL CuCl2
PEI/mL
Purging/min
Heating 175°C/min
1
3 : 1
15
5
10
25
15
2
2 : 1
10
5
8
30
20
3
1 : 1
5
5
5
35
25
4
1 : 2
5
10
8
45
30
5
1 : 3
5
15
10
60
60


## 3. Results and Discussion

Au, Cu, and Au-Cu alloy nanoparticles were synthesized. Different samples of Au-Cu alloy nanoparticles were synthesized by changing molar ratios of Au and Cu salt precursors. These were characterized by UV-Visible spectroscopy, SEM, TEM, XRD, and fluorescence spectroscopy.


### 3.1. UV-Visible Spectroscopy

Figures1 and 2 show the UV-Visible spectra of Au and Cu nanoparticles. The spectra show maximum absorption at 455 and 558 nm for pure Au and Cu nanoparticles, respectively. These values are closely related to the literature reported values (i.e., λ
max
⁡ at 495 and 555 nm for Au and Cu, resp.) [15]. UV-Visible spectra of Au-Cu with various compositions of Au and Cu can also be seen in Figure 3. Such spectra show peaks having λ
max
⁡ at the mid of pure Au and Cu nanoparticles. Figure 3 shows a bathochromic shift in maximum wavelength with increase in composition of Cu in Au-Cu. It also supports the confirmation evidences of Au-Cu alloy nanoparticles formation. The λ
max
⁡ values of all the samples have been tabulated in Table 3. Molar extinction coefficient, ε, was calculated for all the samples by recording their spectra at various concentrations. By applying Beer-Lambert law, molar extinction coefficient was calculated from the plot of absorbanceversus concentration according to(1)
A
=
ε
c
l
,where A is absorbance, ε the molar extinction coefficient in M−1 cm−1, and c the concentration in mol/dm3 while l is the path length in cm. The plot showing change in slope (molar absorptivity coefficient) can be seen in Figure 4. The surface plasmon absorption band shows bathochromic shift with increasing composition of Cu as witnessed by the appearance of bluish color [16]. The appearance of single absorption peak also confirms that nanoparticles are not physically mixed nanoparticles but they have alloy structure. If they were not alloy structure, they would have shown two plasmon bands [17].Table 3
UV-Visible spectral characteristics of Au-Cu alloy nanoparticles in different ratios.
S. number
Au : Cu
X of Au
X of Cu
Absorbance
∈/M−1cm−1
λ
max/nm
1
3 : 1
0.7
0.25
0.93
284.23
490
2
2 : 1
0.6
0.33
0.85
220.53
495
3
1 : 1
0.5
0.5
0.65
186.66
500
4
1 : 2
0.4
0.6
0.5
143.68
530
5
1 : 3
0.3
0.7
0.33
116.89
555Figure 1
UV-Visible spectrum of Au nanoparticles, using ethylene glycol as a solvent as well as a reducing agent at temperature of 298 K.Figure 2
UV-Visible spectrum of Cu nanoparticles taken at 398 K, using ethylene glycol as a solvent as well as a reducing agent.Figure 3
UV-Visible spectra of Au-Cu (1 : 1), Au-Cu (1 : 2), and Au-Cu (1 : 3) nanoparticles showing bathochromic shift with increase in composition of Cu in Au-Cu alloy nanoparticles.Figure 4
Plots of absorbance versus concentration for Au-Cu.An examination of Table3 reveals that absorbance and molar absorption coefficient get lowered with increase in composition of Cu in Au-Cu alloy. The table also reveals red shift in λ
max
⁡ with elevation of Cu. The bathochromic shift is due to change in the particle size as well as some important variation in the refractive index occurring in the medium [17]. By plotting λ
max
⁡ of pure Au, samples Au-Cu 3 : 1, Au-Cu 2 : 1, Au-Cu 1 : 1, Au-Cu 1 : 2, and Au-Cu 1 : 3, and pure Cu nanoparticlesversus mole fraction of Cu, a linear relationship as shown in Figure 5 was obtained. Hence, λ
max
⁡ value gets increased by the increase in mole fraction of Cu [18, 19].Figure 5
Plot of Max. wavelength versus mole fraction of Cu in Au-Cu alloy nanoparticles.


### 3.2. Fluorescence Spectroscopy

Fluorescence signals of copper and gold nanoparticles appear at 645 and 530 nm, respectively [5, 20]. Fluorescence signals shown by Au-Cu bimetallic alloy nanoparticles are in the mid-range of pure gold and copper nanoparticles. The basic concept for the fluorescence of Au involves the transition of electrons from its d orbital to excited electronic states in the sp-band [21]. In a similar way, emission spectrum of Cu is due to deexcitation of electron from excited states to d orbital. Physically mixed solutions of gold and copper nanoparticles give two distinct emission spectra but their alloy nanoparticles register a single emission peak as expected. Confirmation of the synthetic process as revealed by single absorption spectrum is also supported by the appearance of single emission signal as shown in Figure 6, for the alloys nanoparticles with varying copper content. Figure 6 shows that Cu acts as quencher, because an increase in its composition in Au-Cu nanoparticles causes decrease in its intensity. The emission λ
max
⁡ for fluorescence is higher than absorption λ
max
⁡ as expected [22]. Tabulated data from fluorescence spectroscopy demonstrates a blue shift in λ
max
⁡ and hypochromic effect in the intensity from Au-Cu 3 : 1 to Au-Cu 1 : 1, but that from Au-Cu 1 : 1 to Au-Cu 1 : 3 remains the same as shown in Table 4. An equation showing relation between relative intensity and concentration of the quencher to sample is given here:(2)
log
⁡
I
0
I
Q
=
Q
N
X
,where I
Q and I
0 represent the intensity with and without quencher, Q is the concentration of quencher, X is the concentration of sample in mM, and N is the number of atoms in nanoparticles. Plotting log I
0
/
I
Q versus Q
/
X, using (2), number of atoms, N, can be determined from the slope.Table 4
Parameters obtained from fluorescence spectroscopy.
S. number
Au : Cu
I
0
I
Q
λ
max/nm
Number of atoms (n)
Binding sites
Binding constant
Δ
G
b/(KJ/mol)
1
3 : 1
320
250
558
350
0.19
7.89
-
3.30
2
2 : 1
320
235
559
425
0.33
24.60
-
5.40
3
1 : 1
320
225
560
485
0.56
115.5
-
15.50
4
1 : 2
320
215
560
505
0.65
180.3
-
20.25
5
1 : 3
320
200
560
530
0.72
195.25
-
25.50Figure 6
Fluorescence accumulative spectra of Au-Cu alloy nanoparticles.Similarly, another relation showing relative change in the intensity (logI
0
-
I
Q
/
I
Q), binding constant (k
b), and quencher concentration can be represented as(3)
log
⁡
I
0
-
I
Q
I
Q
=
log
⁡
k
b
+
n
log
⁡
Q
.Binding constant and binding sites can be evaluated from the intercept and slope of the plot of log
⁡
I
0
-
I
Q
/
I
Q as a function of log Q. Number of binding sites, n, and binding constant, k
b, were found to increase with the increase in the amount of Cu as shown in Table 4.To study spontaneity of the aggregation, Gibb’s free energy relating to binding constant is given as(4)
Δ
G
b
=
R
T
ln
⁡
k
b
.In order to know whether the process is spontaneous or nonspontaneous, free energy of binding was calculated from (4). Variations in the intensity as evidenced by Figure 6 can be attributed to the crystal structures [23]. Table 4 shows data obtained from fluorescence spectroscopy. The number of atoms, N, increases with increase in composition of Cu due to its comparatively smaller atomic radius. The values of n and k
b and Δ
G
b also increase with increasing Cu content. Hence, increasing amount of Cu in Au-Cu makes the process more spontaneous as revealed by negative values of Δ
G
b.


### 3.3. X-Ray Diffraction Spectroscopy (XRD)

For the study and evaluation of some important parameters like composition studies and calculation of average diameter of the nanoparticles, the combined XRD spectra were recorded for all the prepared samples. XRD results revealed that upon addition of one element in the matrix of the other a shift in the signal occurs as observable from the shift of Au signal due to continuous addition of Cu in Au matrixes [24]. Three peaks, that is, (111), (200), and (210), can be seen in the spectra shown in Figure 7.Figure 7
XRD spectra for samples Au-Cu 3 : 1, Au-Cu 2 : 1, Au-Cu 1 : 1, Au-Cu 1 : 2, and Au-Cu 1 : 3.Using XRD, different lattice points exposed in crystallite were determined. Possible crystal structure was determined from XRD analysis. Figure7 shows that two distinct peaks, that is, (111) at 32 and (200) at 37, are more intense and show more exposure of the lattice points at these positions. These signals were considered the desired peaks for calculation of the size of nanoparticles. Hence, average diameter of all the nanoparticles was calculated by using Debye Scherrer formula as shown in (5). The 2
θ of the XRD signal moves positively with increasing mole fraction of Cu, due to which size of the crystalloid gets retarded. Due to crystallite contraction, size of the alloy nanoparticles decreases. Slight broadening in the width of the desired peak occurred which points to the decrease in size of nanoparticles. The XRD signal also suggests that the sample consists of two kinds of metals, that is, Au and Cu. However, Cu seems to be dispersed in the Au matrixes due to its smaller size. The atomic radius of Cu (0.14 nm) is smaller than Au (0.18 nm) [25]. Size of all the nanoparticles was calculated applying Debye Scherrer’s equation:(5)
D
=
k
λ
β
cos
⁡
θ
,where k stands for particle shape factor and is taken as 0.899 for Au-Cu, λ the wavelength of radiation, β the calibrated half intensity width of the desired diffraction peak, and θ the half of peak position angle called Bragg’s angle. The values of calculated average diameters of all the samples are listed in Table 5 showing a decrease with increase in mole fraction of Cu.Table 5
Size of nanoparticles calculated from SEM, TEM, and XRD.
S. number
Au : Cu
Average diameter/nm
1
3 : 1
80
2
2 : 1
75
3
1 : 1
70
4
1 : 2
68
5
1 : 3
65


### 3.4. Scanning Electron Microscopic (SEM) Studies

SEM images depicted in Figure8 show that sizes of monometallic as well as bimetallic alloy nanoparticles are nonuniform. The observed mismatch in lattice spacing is due to very similar lattice parameters of Au and Cu [26]. The morphological structures of Au NPs, Cu NPs, and Au-Cu alloy nanoparticles prepared with various ratios can be seen in Figures 8(a)–8(e).Figure 8
SEM images of (a) Au, (b) Cu, (c) Au-Cu (1 : 1), (d) Au-Cu (1 : 2), and (e) Au-Cu (1 : 3) alloy nanoparticles.
(a)
(b)
(c)
(d)
(e)


### 3.5. Transmission Electron Microscopic (TEM) Studies

TEM photographs of Au-Cu bimetallic alloy nanoparticles at various ratios can be seen in Figures9(a)–9(c). Au-Cu alloy particle size ranges from 80 to 65 nm. A typical TEM image of Au-Cu (1 : 2) nanoparticles as shown in Figure 9(b) is nonspherical; however, shapes of Au-Cu (1 : 1) and Au-Cu (1 : 3) nanoparticles are close to spherical shape as evidenced by Figures 9(a) and 9(c). Interestingly, sizes shown by these images are the same as calculated from XRD. The size of nanoparticles evaluated from XRD as well as TEM can be seen in Table 5.Figure 9
TEM images of (a) Au-Cu (1 : 1), (b) Au-Cu (1 : 2), and (c) Au-Cu (1 : 3) alloy nanoparticles.
(a)
(b)
(c)


### 3.6. Conclusion

Chemical reduction process is the most simple and effective method for the synthesis of bimetallic Au-Cu alloy nanoparticles. This method can also be used successfully for the synthesis of monometallic Au and Cu nanoparticles. UV-Visible spectroscopy is the sensitive technique used for the confirmation of the synthetic process. Change in the composition of nanoparticles was studied by UV-Visible spectroscopy and XRD. Morphology was studied by SEM and TEM. Quenching effect of Cu in Au-Cu alloy nanoparticles was revealed by the results obtained from fluorescence spectroscopy. SEM and TEM were applied for the calculation of average diameters and shape of the nanoparticles. EDS analysis revealed more than 90% purity of the synthesized Au-Cu alloy nanoparticles. Nanoparticles were found nearly spherical in shape but modified slightly with change in composition of Au and Cu. TEM results revealed that the shapes of Au-Cu alloy in the ratio of 3 : 1 are more uniformly spherical. The applied synthetic method excels other methods owing to its higher efficiency and environmental friendliness. Moreover, it is easy to handle and does not require extensive instrumentation.


## 3.1. UV-Visible Spectroscopy

Figures1 and 2 show the UV-Visible spectra of Au and Cu nanoparticles. The spectra show maximum absorption at 455 and 558 nm for pure Au and Cu nanoparticles, respectively. These values are closely related to the literature reported values (i.e., λ
max
⁡ at 495 and 555 nm for Au and Cu, resp.) [15]. UV-Visible spectra of Au-Cu with various compositions of Au and Cu can also be seen in Figure 3. Such spectra show peaks having λ
max
⁡ at the mid of pure Au and Cu nanoparticles. Figure 3 shows a bathochromic shift in maximum wavelength with increase in composition of Cu in Au-Cu. It also supports the confirmation evidences of Au-Cu alloy nanoparticles formation. The λ
max
⁡ values of all the samples have been tabulated in Table 3. Molar extinction coefficient, ε, was calculated for all the samples by recording their spectra at various concentrations. By applying Beer-Lambert law, molar extinction coefficient was calculated from the plot of absorbanceversus concentration according to(1)
A
=
ε
c
l
,where A is absorbance, ε the molar extinction coefficient in M−1 cm−1, and c the concentration in mol/dm3 while l is the path length in cm. The plot showing change in slope (molar absorptivity coefficient) can be seen in Figure 4. The surface plasmon absorption band shows bathochromic shift with increasing composition of Cu as witnessed by the appearance of bluish color [16]. The appearance of single absorption peak also confirms that nanoparticles are not physically mixed nanoparticles but they have alloy structure. If they were not alloy structure, they would have shown two plasmon bands [17].Table 3
UV-Visible spectral characteristics of Au-Cu alloy nanoparticles in different ratios.
S. number
Au : Cu
X of Au
X of Cu
Absorbance
∈/M−1cm−1
λ
max/nm
1
3 : 1
0.7
0.25
0.93
284.23
490
2
2 : 1
0.6
0.33
0.85
220.53
495
3
1 : 1
0.5
0.5
0.65
186.66
500
4
1 : 2
0.4
0.6
0.5
143.68
530
5
1 : 3
0.3
0.7
0.33
116.89
555Figure 1
UV-Visible spectrum of Au nanoparticles, using ethylene glycol as a solvent as well as a reducing agent at temperature of 298 K.Figure 2
UV-Visible spectrum of Cu nanoparticles taken at 398 K, using ethylene glycol as a solvent as well as a reducing agent.Figure 3
UV-Visible spectra of Au-Cu (1 : 1), Au-Cu (1 : 2), and Au-Cu (1 : 3) nanoparticles showing bathochromic shift with increase in composition of Cu in Au-Cu alloy nanoparticles.Figure 4
Plots of absorbance versus concentration for Au-Cu.An examination of Table3 reveals that absorbance and molar absorption coefficient get lowered with increase in composition of Cu in Au-Cu alloy. The table also reveals red shift in λ
max
⁡ with elevation of Cu. The bathochromic shift is due to change in the particle size as well as some important variation in the refractive index occurring in the medium [17]. By plotting λ
max
⁡ of pure Au, samples Au-Cu 3 : 1, Au-Cu 2 : 1, Au-Cu 1 : 1, Au-Cu 1 : 2, and Au-Cu 1 : 3, and pure Cu nanoparticlesversus mole fraction of Cu, a linear relationship as shown in Figure 5 was obtained. Hence, λ
max
⁡ value gets increased by the increase in mole fraction of Cu [18, 19].Figure 5
Plot of Max. wavelength versus mole fraction of Cu in Au-Cu alloy nanoparticles.


## 3.2. Fluorescence Spectroscopy

Fluorescence signals of copper and gold nanoparticles appear at 645 and 530 nm, respectively [5, 20]. Fluorescence signals shown by Au-Cu bimetallic alloy nanoparticles are in the mid-range of pure gold and copper nanoparticles. The basic concept for the fluorescence of Au involves the transition of electrons from its d orbital to excited electronic states in the sp-band [21]. In a similar way, emission spectrum of Cu is due to deexcitation of electron from excited states to d orbital. Physically mixed solutions of gold and copper nanoparticles give two distinct emission spectra but their alloy nanoparticles register a single emission peak as expected. Confirmation of the synthetic process as revealed by single absorption spectrum is also supported by the appearance of single emission signal as shown in Figure 6, for the alloys nanoparticles with varying copper content. Figure 6 shows that Cu acts as quencher, because an increase in its composition in Au-Cu nanoparticles causes decrease in its intensity. The emission λ
max
⁡ for fluorescence is higher than absorption λ
max
⁡ as expected [22]. Tabulated data from fluorescence spectroscopy demonstrates a blue shift in λ
max
⁡ and hypochromic effect in the intensity from Au-Cu 3 : 1 to Au-Cu 1 : 1, but that from Au-Cu 1 : 1 to Au-Cu 1 : 3 remains the same as shown in Table 4. An equation showing relation between relative intensity and concentration of the quencher to sample is given here:(2)
log
⁡
I
0
I
Q
=
Q
N
X
,where I
Q and I
0 represent the intensity with and without quencher, Q is the concentration of quencher, X is the concentration of sample in mM, and N is the number of atoms in nanoparticles. Plotting log I
0
/
I
Q versus Q
/
X, using (2), number of atoms, N, can be determined from the slope.Table 4
Parameters obtained from fluorescence spectroscopy.
S. number
Au : Cu
I
0
I
Q
λ
max/nm
Number of atoms (n)
Binding sites
Binding constant
Δ
G
b/(KJ/mol)
1
3 : 1
320
250
558
350
0.19
7.89
-
3.30
2
2 : 1
320
235
559
425
0.33
24.60
-
5.40
3
1 : 1
320
225
560
485
0.56
115.5
-
15.50
4
1 : 2
320
215
560
505
0.65
180.3
-
20.25
5
1 : 3
320
200
560
530
0.72
195.25
-
25.50Figure 6
Fluorescence accumulative spectra of Au-Cu alloy nanoparticles.Similarly, another relation showing relative change in the intensity (logI
0
-
I
Q
/
I
Q), binding constant (k
b), and quencher concentration can be represented as(3)
log
⁡
I
0
-
I
Q
I
Q
=
log
⁡
k
b
+
n
log
⁡
Q
.Binding constant and binding sites can be evaluated from the intercept and slope of the plot of log
⁡
I
0
-
I
Q
/
I
Q as a function of log Q. Number of binding sites, n, and binding constant, k
b, were found to increase with the increase in the amount of Cu as shown in Table 4.To study spontaneity of the aggregation, Gibb’s free energy relating to binding constant is given as(4)
Δ
G
b
=
R
T
ln
⁡
k
b
.In order to know whether the process is spontaneous or nonspontaneous, free energy of binding was calculated from (4). Variations in the intensity as evidenced by Figure 6 can be attributed to the crystal structures [23]. Table 4 shows data obtained from fluorescence spectroscopy. The number of atoms, N, increases with increase in composition of Cu due to its comparatively smaller atomic radius. The values of n and k
b and Δ
G
b also increase with increasing Cu content. Hence, increasing amount of Cu in Au-Cu makes the process more spontaneous as revealed by negative values of Δ
G
b.


## 3.3. X-Ray Diffraction Spectroscopy (XRD)

For the study and evaluation of some important parameters like composition studies and calculation of average diameter of the nanoparticles, the combined XRD spectra were recorded for all the prepared samples. XRD results revealed that upon addition of one element in the matrix of the other a shift in the signal occurs as observable from the shift of Au signal due to continuous addition of Cu in Au matrixes [24]. Three peaks, that is, (111), (200), and (210), can be seen in the spectra shown in Figure 7.Figure 7
XRD spectra for samples Au-Cu 3 : 1, Au-Cu 2 : 1, Au-Cu 1 : 1, Au-Cu 1 : 2, and Au-Cu 1 : 3.Using XRD, different lattice points exposed in crystallite were determined. Possible crystal structure was determined from XRD analysis. Figure7 shows that two distinct peaks, that is, (111) at 32 and (200) at 37, are more intense and show more exposure of the lattice points at these positions. These signals were considered the desired peaks for calculation of the size of nanoparticles. Hence, average diameter of all the nanoparticles was calculated by using Debye Scherrer formula as shown in (5). The 2
θ of the XRD signal moves positively with increasing mole fraction of Cu, due to which size of the crystalloid gets retarded. Due to crystallite contraction, size of the alloy nanoparticles decreases. Slight broadening in the width of the desired peak occurred which points to the decrease in size of nanoparticles. The XRD signal also suggests that the sample consists of two kinds of metals, that is, Au and Cu. However, Cu seems to be dispersed in the Au matrixes due to its smaller size. The atomic radius of Cu (0.14 nm) is smaller than Au (0.18 nm) [25]. Size of all the nanoparticles was calculated applying Debye Scherrer’s equation:(5)
D
=
k
λ
β
cos
⁡
θ
,where k stands for particle shape factor and is taken as 0.899 for Au-Cu, λ the wavelength of radiation, β the calibrated half intensity width of the desired diffraction peak, and θ the half of peak position angle called Bragg’s angle. The values of calculated average diameters of all the samples are listed in Table 5 showing a decrease with increase in mole fraction of Cu.Table 5
Size of nanoparticles calculated from SEM, TEM, and XRD.
S. number
Au : Cu
Average diameter/nm
1
3 : 1
80
2
2 : 1
75
3
1 : 1
70
4
1 : 2
68
5
1 : 3
65


## 3.4. Scanning Electron Microscopic (SEM) Studies

SEM images depicted in Figure8 show that sizes of monometallic as well as bimetallic alloy nanoparticles are nonuniform. The observed mismatch in lattice spacing is due to very similar lattice parameters of Au and Cu [26]. The morphological structures of Au NPs, Cu NPs, and Au-Cu alloy nanoparticles prepared with various ratios can be seen in Figures 8(a)–8(e).Figure 8
SEM images of (a) Au, (b) Cu, (c) Au-Cu (1 : 1), (d) Au-Cu (1 : 2), and (e) Au-Cu (1 : 3) alloy nanoparticles.
(a)
(b)
(c)
(d)
(e)


## 3.5. Transmission Electron Microscopic (TEM) Studies

TEM photographs of Au-Cu bimetallic alloy nanoparticles at various ratios can be seen in Figures9(a)–9(c). Au-Cu alloy particle size ranges from 80 to 65 nm. A typical TEM image of Au-Cu (1 : 2) nanoparticles as shown in Figure 9(b) is nonspherical; however, shapes of Au-Cu (1 : 1) and Au-Cu (1 : 3) nanoparticles are close to spherical shape as evidenced by Figures 9(a) and 9(c). Interestingly, sizes shown by these images are the same as calculated from XRD. The size of nanoparticles evaluated from XRD as well as TEM can be seen in Table 5.Figure 9
TEM images of (a) Au-Cu (1 : 1), (b) Au-Cu (1 : 2), and (c) Au-Cu (1 : 3) alloy nanoparticles.
(a)
(b)
(c)


## 3.6. Conclusion

Chemical reduction process is the most simple and effective method for the synthesis of bimetallic Au-Cu alloy nanoparticles. This method can also be used successfully for the synthesis of monometallic Au and Cu nanoparticles. UV-Visible spectroscopy is the sensitive technique used for the confirmation of the synthetic process. Change in the composition of nanoparticles was studied by UV-Visible spectroscopy and XRD. Morphology was studied by SEM and TEM. Quenching effect of Cu in Au-Cu alloy nanoparticles was revealed by the results obtained from fluorescence spectroscopy. SEM and TEM were applied for the calculation of average diameters and shape of the nanoparticles. EDS analysis revealed more than 90% purity of the synthesized Au-Cu alloy nanoparticles. Nanoparticles were found nearly spherical in shape but modified slightly with change in composition of Au and Cu. TEM results revealed that the shapes of Au-Cu alloy in the ratio of 3 : 1 are more uniformly spherical. The applied synthetic method excels other methods owing to its higher efficiency and environmental friendliness. Moreover, it is easy to handle and does not require extensive instrumentation.



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*Source: 638629-2015-03-29.xml*