# Large-Scale Cu Nanowire Synthesis by PVP-Ethylene Glycol Route

Authors: Jhon L. Cuya Huaman; Iori Urushizaki; Balachandran Jeyadevan
Journal: Journal of Nanomaterials
 (2018)

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## Abstract

Cu nanowire (NW) is a promising cost-benefit conducting material that could be considered for the development of transparent conducting films (TCF). However, the development of Cu NW as an alternating material for Ag or Au is not only limited by its stability in atmospheric conditions in the nanometer range but also due to the nonavailability of a simple synthetic route to produce them in high yields and in large-scale. Here, a scheme to synthesize Cu NWs by reducing Cu nitrate in a Cl− ion-polyvinylpyrrolidine- (PVP-) ethylene glycol (EG) system is proposed. Cu NWs with average diameter around 60 nm and average length of about 40 μm was obtained under optimized experimental conditions. Furthermore, the formation of Cu NW was elucidated to be through the progression of the following sequential reduction steps: at first, Cu ions underwent partial reduction to form spherical Cu2O. Then, the spherical Cu2O particles were redissolved and reduced to metallic Cu0 atoms that subsequently formed the Cu seeds. Thereafter, Cu seeds underwent etching to form multiply-twinned particles (MTP). Finally, these Cu MTP grew unidirectionally to form metallic Cu NWs.


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## Body

## 1. Introduction

In recent years, the development of TCF such as touching screens, thin-film solar cells, organic light-emitting diodes, and sensors using metallic NWs as an alternative conducting material for indium tin oxide is being researched intensively [1–3]. In fact, the optical and electrical properties of TCF prepared using Ag NWs with diameters ~20 nm and lengths higher than 20 μm have outperformed the ones prepared using commercial ITO and exhibited transmittance higher than 85% and electrical resistivity less than 45 Ω/sq. [2, 3]. However, the material cost and migration caused in moist conditions are considered detrimental to their use in TCF and researches on alternative metallic NWs are being considered. Consequently, the research on the development of Cu NWs are on the rise due to the availability of cheap and abundant resources, high electrical properties, and low migration problem despite the fact that Cu has showed low stability in moist and oxidizing atmospheres [4–8]. Consequently, several physical and chemical routes have been developed to synthesize Cu NWs; however, in most cases, the chemical routes are considered due to simplicity and scalability of these techniques in contrast to other routes [9–22]. Among the developed chemical techniques, aqueous synthetic route using hydrazine as the reducing agent is researched intensively [13–18]. However, this technique uses high concentrations of sodium hydroxide (NaOH) and requires stringent washing technique to remove the alkali that could hamper the conductivity of Cu NWs due to surface oxidation. On the other hand, long alkyl amine-mediated synthesis of Cu NWs has gained importance due to the possibility of dispersing and storing the products in organic solvents that could avoid rapid oxidation [19–22]. In this method, alkyl amines function as the reducing, protecting, and growth-controlling agent. The adsorption of alkyl amine on specific {100} planes of Cu seeds facilitates the unidirectional growth the seeds in the [110] direction [20]. Though the organic route is considered simpler than the aqueous route, the heterogeneous dispersion of NWs has been observed when the suspension was deposited on substrates; thus, additional processing steps such as ligand exchange are required to enhance the dispersing ability of NWs in polar and nonpolar solvents. Even though the issues such as inhibition of oxidation and enhancement in the stability of suspension remain, large-scale synthesis is also considered a serious issue that needs to be resolved.On the other hand, the success of Ag NWs as an alternative material for ITO in TCF could be ascribed to their large-scale production using a simple and scalable polyol process that enables dimensional control of NWs through the control of concentrations of Cl− ion, AgNO3, and PVP in ethylene glycol [23–26]. In addition, the fine tuning of the dimensional properties of NWs such as the length and diameter could also be achieved by introducing chemical additives at various stages of the process [24–28]. However, it should be noted that the above technique has not been successfully applied to large-scale synthesis of Cu NWs with dimensional properties suitable for conductive electrodes, that is, 20 nm in diameter and 20 μm in length [2, 3]. One of the reasons could be the low redox potential of Cu ions compared to Ag ions, which requires the synthesis at elevated temperatures or the use of weak reducing agents such as either sodium hypophosphite or sodium borohydride along with alcohol that enhances the overall reducing ability of the system [29–31]. However, the products obtained were mostly Cu nanoparticles (NPs) and not Cu NWs. And also, unlike in the case of Ag NWs, the formation of intermediate phases such as cupric and cuprous compounds [32–34] seems to play an important role in determining the reduction rate, which is quite vital and decisive step defining the final morphology of metallic Cu. Cu NWs have been obtained in alkylamine-glucose or glycerol systems at relatively high temperatures [4]. Although, alkylamine enhanced the reducing ability of polyol and controlled the unidirectional growth on {100} planes, this was not adequate to avoid the generation of NPs in large quantities. On the other hand, the synthesis of Cu NWs by using propylene glycol as reducing agent and PVP as surfactant has also been reported [35]. Here, the use of tetraphenylphosphonium chloride is considered to have played an important role in obtaining nanowires. Though the yield of Cu NWs was very low and their diameters were thick (<300 nm), this technique can be improved by considering stronger reducing agents.In the case of Ag NWs in EG-PVP system, two closely related elements, namely, Cl− ions and PVP molecules that specifically adsorb on the {100} planes of Ag NPs, are reported to facilitate the unidirectional growth of Ag seeds [23–26, 28, 36–40]. In addition, PVP molecules are reported to enhance the reduction of metal salts by forming complexes through coordination between metallic ions and C=O groups and also stabilize the products subsequently [36, 37]. However, the specific adsorption of PVP for the unidirectional growth of metallic seeds is only realized at specific Cl− ion concentrations [28, 36, 40]. At conditions suitable for the reduction of Ag ions to metallic Ag, Cl− ions control the morphology of Ag products through the etching processes that generate multitwinned Ag seeds. The etching mechanism that consists of selective removal of twinned structures into solution by the presence of an oxidative pair such as Cl−/O2 or Fe3+/Fe2+ was initially proposed by Wiley et al. [23]. They claimed that the shape of the particles can be controlled by controlling the degree of etching or in other words by controlling the concentration of Cl ions. For example, in the absence of Cl− ions, where the etching does not occur, the product will be constituted of spherical and polyhedral particles only. However, at higher Cl− ion concentrations, the total dissolution of nanoparticles occurs. Furthermore, at appropriate concentration of Cl− ions, the formation of MTP is facilitated and product becomes almost only of NWs.Here, the synthesis of Cu NWs in high yield using the EG-PVP system under optimized conditions is reported. The formation mechanism of Cu NWs based on the analytical results acquired from the solution as well as the solids obtained during synthesis of Cu NWs using UV-visible spectroscopy (UV-Vis), scanning electron microscopy (SEM), and X-ray diffractometry (XRD) is also proposed. The study revealed that Cu NWs originated from the dissolution of the intermediate oxide compounds such as Cu2O. The dissolution rate of Cu2O and the subsequent reduction to metallic Cu were considered to be the critical and rate determining steps for the formation of Cu NW.


## 2. Materials and Methods

### 2.1. Preparation of Cu NWs

Cu(NO3)2·3H2O (10 mM), polyvinylpyrrolidone (PVPK30, 0 to 75 mM considering the monomer unit), and cetyltrimethylammonium chloride (CTAC, 0 to 10 mM) were introduced into a 200 ml two-necked flask containing 100 ml of EG. This solution was heated between 172 and 186°C for 4 h under continuous mechanical stirring and N2 purging (0 to 200 ml/min). The solid products were collected by centrifuging the suspension at 3000 rpm for 10 min. The recovered sediment was washed by methanol several times, dispersed in methanol and stored.


### 2.2. Characterization of Cu NWs

Identification of the crystal phases present in the sediment was analyzed by X-ray diffractometry (XRD, Rigaku SmartLab) using Cu Kα in the angle 2θ ranging from 20 to 80 degrees. The optical properties of Cu NWs suspended in methanol were evaluated using ultraviolet visible spectroscopy (UV4900, Rigaku) in the range of 300 to 800 nm using quartz cells. The morphology of the products was examined by using field emission scanning electron microscopy (FE-SEM, Hitachi 4400) and transmission electron microscopy (TEM, Hitachi-8100). The adsorption of PVP on the Cu NW surface was verified by Fourier transformed infrared spectroscopy (FT-IR) in transmittance mode in the range of 500 to 4000 cm−1 (Nicolet iS5, Thermo Scientific), and the concentration of PVP attached to the NW surface was determined by thermogravimetry (TG) under N2 gas flow from room temperature to 500°C by heating at the rate of 10°C/min using TG8120-Shimadzu device.


## 2.1. Preparation of Cu NWs

Cu(NO3)2·3H2O (10 mM), polyvinylpyrrolidone (PVPK30, 0 to 75 mM considering the monomer unit), and cetyltrimethylammonium chloride (CTAC, 0 to 10 mM) were introduced into a 200 ml two-necked flask containing 100 ml of EG. This solution was heated between 172 and 186°C for 4 h under continuous mechanical stirring and N2 purging (0 to 200 ml/min). The solid products were collected by centrifuging the suspension at 3000 rpm for 10 min. The recovered sediment was washed by methanol several times, dispersed in methanol and stored.


## 2.2. Characterization of Cu NWs

Identification of the crystal phases present in the sediment was analyzed by X-ray diffractometry (XRD, Rigaku SmartLab) using Cu Kα in the angle 2θ ranging from 20 to 80 degrees. The optical properties of Cu NWs suspended in methanol were evaluated using ultraviolet visible spectroscopy (UV4900, Rigaku) in the range of 300 to 800 nm using quartz cells. The morphology of the products was examined by using field emission scanning electron microscopy (FE-SEM, Hitachi 4400) and transmission electron microscopy (TEM, Hitachi-8100). The adsorption of PVP on the Cu NW surface was verified by Fourier transformed infrared spectroscopy (FT-IR) in transmittance mode in the range of 500 to 4000 cm−1 (Nicolet iS5, Thermo Scientific), and the concentration of PVP attached to the NW surface was determined by thermogravimetry (TG) under N2 gas flow from room temperature to 500°C by heating at the rate of 10°C/min using TG8120-Shimadzu device.


## 3. Results and Discussion

Taking the experimental conditions to obtain Ag NWs in EG-PVP system into consideration, the tuning of Cl− ion concentration was considered vital to control the etching mechanism and the subsequent formation of NWs. Thus, in the first instance, the concentration of Cl− ions required to obtain NWs was examined while keeping the concentration of PVP constant. And then, the influences of PVP concentration and other parameters such as the reducing atmosphere and temperature were also studied.


### 3.1. Influence of Halide Ion Source and Its Concentration on Cu NW Formation

Figure1 shows the SEM images of Cu-based products obtained in the EG-PVP system using 0.5 to 2.5 mM of CTAC as the source of Cl− ions. At Cl− ion concentration less than 0.5 mM, Cu nitrate was reduced by ethylene glycol to irregular and faceted metallic Cu particles ranging between 1 and 2 μm along with few rods. When the concentration of Cl− ions ranged between 0.5 and 1.0 mM, the Cu particles became larger in size, and rods, plates, and triangular crystals were also observed (Figure 1(a)). The formation of Cu particles with different shapes could be due to presence of twinned Cu crystals that were not etched sufficiently due to the deficiency of Cl− ions. A remarkable change was observed when the alcoholic solution contained 1.0 mM CTAC; the product was constituted mainly of thicker rods with an average aspect ratio (length/diameter) of 10 and small quantities of Cu particles with triangular facets that originated from decahedral or icosahedral crystals (Figure 1(b)).Figure 1
SEM images of Cu nanostructures obtained by reducing Cu nitrate in EG-PVP system in the presence of (a) 0.5, (b) 1.0, (c) 1.25, and (d) 2.5 mM of CTAC and (e) a schematic illustration showing the effect of Cl− ion concentration in the formation of Cu NWs. SEM images of halide type in the synthesis of Cu NWs: (f) NaF, (g) NaCl, (h) CTAB, and (i) KI at a concentration of 1.25 mM and (j) a schematic illustration that shows the effect of Ksp of Cu(I) halides in the formation of Cu NWs.
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(j)When Cl− ion concentration reached 1.25 mM, the product was constituted only of Cu NWs (Figure 1(c)). Under these conditions, the average diameter and length of NWs were 74.1 nm and 31.5 μm, respectively (aspect ratio of 423). However, when the concentration of Cl− ion concentration resulted to be too high, the shape of NW was not retained and the yield decreased progressively (Figure 1(d)) and disappeared totally at 10 mM. On the contrary, micrometer-sized spherical particles were formed at higher concentration of Cl− ions (Figure 1(d)). Usually in the presence of high concentrations of Cl− ions, the formation of nanocubes is favored as in the case of Ag NPs due to the preferential adsorption on the {100} planes [23, 24, 28]; however, this was not observed here. The XRD pattern of the spherical particles corresponded to the cubic phase of Cu2O. This suggests that the reduction of Cu2O to Cu was delayed or reduction and dissolution occurred repeatedly under high concentration of CTAC and subsequently neither the formation of Cu NWs nor nanocubes was realized.The above results suggested that at low Cl− ion concentrations, the reduction rate of Cu was too high for the seeds to undergo etching to generate preferential planes prior to growth, resulting in the formation of irregular and faceted nanostructures. On the other hand, at high Cl− ion concentrations, the etching was too strong and the concentration of Cu ions in the solution became high and led to the formation of spherical shaped Cu2O particles (Figure 1(e)). Thus, the optimum Cl concentration was determined to be around 1.25 mM, or in other words, the Cl/Cu molar ratio was 0.125. This value was relatively high compared to the one used by Whitcomb, which is 0.026 [35]. Although, the low concentration of Cl− ions could be one of the reasons for low yield, the formation of insoluble or partially soluble intermediate compound, CuCl could be another. Though the presence of CuCl was not detected when the concentration of Cl− ions was low, their presence was confirmed in the structural and morphological analysis in the products obtained during the synthesis of Cu NWs under high CTAC concentrations (5 mM) (Figure S1).Then, to determine the influence of halide type on the formation of NWs, CTAC was replaced by equal concentrations of sodium fluoride (NaF), sodium chloride (NaCl), cetyltrimethylammonium bromide (CTAB), and potassium iodide (KI). As observed in the SEM photographs shown in Figures1(f)–1(i), high yield of NWs was obtained in NaCl and CTAB cases. The above results suggested that the optimal halide concentration is very vital than the type or source of halide for the formation of Cu NWs in high yield. On the other hand, the formation of cuprous halides and their solubility product constants (Ksp) [41] could be an important factor to consider in the control of the final structure and the complete reduction of Cu salts as shown in Figure 1(j). Thus, the synthesis of high-yield Cu NWs proceeded in the following order:
(1)CuCl1.72×10−7>CuBr6.27×10−9>CuI1.27×10−12.Hence, the reduction and formation of Cu NWs is favored at high solubility of intermediate products in the solvent as in the cases of CuCl and CuBr. But, in the case of low solubility CuI, the products resulted to be a mixture of CuI, Cu2O, and Cu phases (Figure S2). On the other hand, in the case of highly soluble CuF and the instability to form CuF2 enhances the formation of Cu NPs than Cu NWs.The formation of NWs is influenced by the control over the reduction of Cu ions to form metallic Cu seeds and their subsequent etching to form MTPs that facilitate the formation of NWs. The dimensional properties of the NW are influenced very much by the unidirectional growth facilitated by the preferential adsorption of the capping agent on the crystal planes of the NWs. Thus, the role of the capping agent on the yield as well as the dimensional properties of Cu NWs will be discussed in the next section.


### 3.2. Influence of PVP on the Yield and Dimensional Properties of Cu NWs

The molecular weight and concentration of PVP have been reported to control the yield and dimensions of NWs [36–39] due to their preferential adsorption on {100} planes of metallic surface compared to {111}. Thus, the effect of PVP concentration on the synthesis of Cu NWs at the reaction temperature of 182°C is investigated, while keeping Cl−/Cu2+ molar ratio and the amount of N2 purged constant. Figure 2 shows that decreasing the PVP concentration facilitated the formation of irregular-shaped Cu NPs at the expense of Cu NWs. At low PVP concentration of 25 mM, the nucleus grew isotropically due to insufficient concentration of capping agent. In contrast, at higher PVP concentration of 75 mM, the Cu NWs became thicker and shorter. When the concentration was increased further, only NPs were formed. This is believed due to the nonpreferential adsorption of PVP molecules on the crystal faces of Cu NPs, even on the {111} planes that facilitate the unidirectional growth of NWs as shown in Figure 2(g). The FT-IR spectra of pure PVP and the Cu NWs are shown in Figure 2(e), and the adsorption of PVP on the surface of NWs was confirmed. The spectrum of the NWs synthesized using the above technique shows absorption bands at 3400 cm−1 that could be ascribed to the overtone of C=O bond. In addition, a band corresponding to O-H groups at around 3500 cm−1 was also recorded. This could due to the presence of methanol used during washing. The stretching vibrations of C-H and C=O were observed at 2920 cm−1 and 1640 cm−1, respectively. Likewise, the absorption band corresponding to the stretching mode of C-N was also observed at around 1300 cm−1. Furthermore, the PVP concentration adsorbed on the metallic surface was evaluated by thermogravimetry under N2 gas flow. As observed in Figure 2(f), the weight loss at temperatures below 180°C was around 8% and it could be ascribed to the removal of solvents such as methanol and adsorbed water. The weight loss between 180 and 200°C was steep and amounted to almost 15%. Then, the weight loss progressed slowly and an additional 5% decrease was recorded at around 600°C. These results suggested that PVP is strongly adsorbed on the Cu surface, and thermal treatments at higher temperatures are necessary to remove PVP molecules completely.Figure 2
SEM images of Cu products obtained under different PVP concentrations: (a) 25, (b) 45, (c) 55, and (d) 75 mM (scale bar: 10μm). (e) FT-IR spectra of pure PVP and PVP-capped Cu NWs. (f) Thermal behavior of PVP-capped Cu NWs measured under N2 flow. (g) Schematic illustration describing the effect of concentration on the adsorption of PVP on Cu surface.
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(g)The optimal concentration of Cl− ions to facilitate the formation of MTPs and the optimal concentration of the capping agent for their subsequent growth have been studied in the previous sections. The diameter of the NW is very much influenced by the size of the seed as well as the MTP formed subsequently. This is believed to depend on the reduction and the etching rates of the reactions. The etching rate is believed to depend on the concentration of oxygen in the reaction system besides the concentration of Cl− ions. Thus, the influence of dissolved oxygen amount on the synthesis of Cu NWs is discussed in the next section.


### 3.3. Effect of the Amount of N2 Gas Flow on the Dimensional Properties of Cu NWs

Cl− ions are assumed to form an oxidant Cl−/O2 pair with atmospheric oxygen that etches and dissolves the preferential planes of the nucleus to form MTP. Thus, the control of this mechanism is important to facilitate the formation rate of multitwinned metallic seeds that grow unidirectionally in [110] orientation with the assistance of the preferential adsorption of the capping agent in {100} planes. On the other hand, Cu NPs are unstable in air inclusively during synthesis and it is common that the reduction needs to be carried out under inert atmospheres using either N2 or Ar gas for the formation of Cu NWs [42, 43]. The reaction atmosphere also influences the rate of the reduction. Thus, the change in the N2 flow rate between 0 and 150 ml/min influenced the morphology of Cu nanostructures as shown in Figure 3. It is clear that EG-PVP system can reduce Cu even in atmospheric conditions, and Cu NWs with diameters around 60.6 nm were obtained; however, nanometer-sized Cu oxide particles attached to the surface of NW were observed. On the other hand, at N2 flow rate of 150 ml/min, the wires became thicker, ~87.5 nm, and the formation of nanocrystals with different sizes and shapes was observed at the expense of low yield of NWs. Here, the amount of O2 is reduced by adding N2 gas or other inert gases to the system, and subsequently, the selective dissolution of specific crystal planes could be inhibited favoring the growth of cubic crystals as observed in other metallic systems [44]. Thus, the formation of wires and the inhibition of oxidation of the synthesized NWs and NPs were realized under an optimum N2 flow rate of 100 ml/min.Figure 3
SEM images of Cu NWs synthesized under different N2 flow rates: (a) 0, (b) 50, (c) 100, and (d) 150 ml/min. (e) Schematic illustration describing the effect of N2 flow rate in the formation of Cu NWs.
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(e)Optimization of the reaction atmosphere facilitated the control over the etching rate and also the stability of the Cu nanostructures. The average diameter and length of the NWs were 67.4 nm and 44μm, respectively, and the aspect ratio was around 650. However, for further reduction in the diameter, the reduction rate should be enhanced. One of the parameters that could enhance the reduction rate is the reaction temperature. Thus, the results obtained by varying the reaction temperature and their influence on the dimensional properties of Cu NW are discussed in the next section.


### 3.4. Effect of Temperature

The synthesis of Cu NPs at low temperatures is realized only when additives that promote the reduction such as sodium hypophosphite monohydrate or sodium borohydride were added to the alcoholic system [29–31]. Increasing the reaction temperature near to the boiling point of ethylene glycol should enhance its reducing ability and facilitate the reduction of Cu2+ ions within a short period of time. Figure 4 and Figure S3 show the effect of reaction temperature on the synthesis of Cu NWs, while all other experimental parameters were kept constant. At 174°C, the formation of spherical Cu2O particles was concluded from SEM and XRD measurements (Figure S4). At this temperature, Cu2+ ions were reduced to form Cu2O but not to Cu metal even after a reaction time of 10 h. Even though the formation Cu NWs was confirmed at 178°C, the presence of Cu2O particles was also identified as shown in Figure 4(b). This suggested that the reaction temperature was not high enough to reduce the Cu ions completely. However, the products obtained at 182°C contained Cu NWs and free of oxide NPs (Figure 4(c)). At higher temperatures, high yield of thicker NWs free of NPs was obtained as shown in Figure 4(d). The kinetic of the reaction is expected to get accelerated at higher temperatures, and the formation of large particles is expected. In this case, the nanowires can grow in axial and radial directions easily. Thus, it was found that the diameter of Cu NWs obtained at different temperatures is influenced by the reaction temperature and NWs with average diameters ~58 nm and ~103 nm were obtained at 178°C and 186°C, respectively. Figure 4(e) shows the effect of temperature in the reduction and formation of nanowires.Figure 4
SEM images of Cu nanostructures obtained by reducing Cu nitrate in EG-PVP under different reaction temperatures: (a) 174, (b) 178 (c) 182, and (d) 186°C. (e) Schematic illustration of the effect of temperature on the formation of Cu NWs.
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(e)Our results demonstrated that Cu NWs can be synthesized in high yield in a Cl− ion-EG-PVP system by controlling the experimental parameter such as type and concentration of chloride source, concentration of PVP, the amount of N2 gas flow, and the reaction temperature. However, the physical characteristics of Cu NWs, specially the diameter, obtained under optimal conditions are not suitable to be used in the development of TCF. Thus, understanding the formation mechanism of Cu NWs is considered vital for further optimization of the process to develop of Cu NWs with high aspect ratio. In the next section, we attempted to elucidate the formation mechanism of NWs through structural and spectral analyses of the reaction solution and solids using XRD, UV-Vis, and SEM.


### 3.5. Formation Mechanism of Cu NWs

Figure5 shows the XRD patterns of samples collected at different reaction times using the following experimental conditions: 10 mM Cu nitrate, 0.125 mM of CTAC, 50 mM of PVP, 182°C, and under a N2 gas flow rate of 100 ml/min. During heating, at temperatures below 150°C, neither color variation of the alcoholic solution nor precipitation occurred. However, at temperatures between 150 and 160°C, the color of the solution turned from light blue to orange with vigorous evolution of NO2 [45]. The XRD analysis of precipitated powders taken after completion of the evolution of gases showed a unique phase that matched well with cubic structured Cu2O, and this phase remained stable even at higher temperatures as shown in Figure 5. It is clear that at this temperature, the reducing potential of ethylene glycol was only sufficient to reduce Cu2+ ions to Cu+, but not to Cu0 due to the presence of chloride which delayed the reduction as observed above. The Cu oxide phase remained for nearly 100 min at 182°C, and then, the orange colored solution turned progressively to red caused by the transformation of Cu2O to Cu as confirmed by XRD. The reduction of Cu2O to Cu0 was totally completed in 10 minutes, and no further change was observed until the end of reaction. It is necessary to emphasize that intermediate phases such as hydroxide, chloride, or oxide (CuO) were not observed during the reduction of Cu nitrate to Cu metal.Figure 5
XRD patterns and UV-Vis spectra of Cu products collected during heating at 182°C. Inset of UV-Vis spectra corresponds to the UV-Vis spectra of solution at 50 and 150°C.Cu2O and Cu NPs possess localized surface plasmon resonance at around 400 to 700 nm [32], which depends on the particle size and morphology. Thus, the progression of the reaction Cu2+ → Cu+ → Cu0 during heating at 182°C at different reaction times was analyzed using UV-Vis spectroscopy (Figure 5). At 50°C and at 150°C, the UV-Vis spectra revealed a broad absorption peak at around 800 nm that could be ascribed to Cu2+ ions coordinated with ethylene glycol and disappeared totally when Cu2O was formed at higher temperatures. When the temperature reached 182°C, a broad absorption band centered at around 440 nm was observed. This could be assigned to the presence of Cu2O particles, and this was not present in the spectra measured at temperatures lower than 182°C (inset Figure 5). After 60 min, at 182°C, the UV-Vis spectrum exhibited a shift in the peak corresponding to Cu2O from 440 nm to 470 nm, which is believed due to particle growth. After 100 min, at 182°C, the color changed from orange to red and a new absorption peak appeared at 570 nm. This could be as a consequence of Cu2O reduction to metallic Cu seeds [32]. The reduction reaction from Cu2O to Cu was relatively faster and the Cu2O absorption peak disappeared totally in 10 minutes leaving the peak corresponding to Cu NWs at 575 nm [21]. No change was observed after 120 min, and absorption peak corresponding to Cu remained even at the end of the reaction.The FE-SEM images of these samples (Figure6) showed sphere-shaped Cu2O particles with a broad size distribution and an average size of 500 nm in the first few minutes of reaction at 182°C. After 60 min of reaction, the spherical Cu2O particles began to dissolve as shown in the inset. However, the dissolved particles precipitated again as Cu2O and no other oxide phase was detected in the XRD pattern. As reaction progressed, the dissolution proceeded, and after 100 min, the dissolved oxide was reduced to Cu metal in alcoholic solution. Then, due to the presence of Cl− ions and PVP, the metallic Cu seeds grew in a preferential direction, whereas rest of the Cu ions in the solution precipitated into small Cu2O cubes as observed in the inset. However, it is not clear whether these cubes originated during cooling the Cu2+ ions that remained in the solution or they existed prior to cooling. After 120 min of reaction, product constituted mainly of Cu NWs; however, the presence of Cu2O on the NW surfaces still remained. At the end of reaction, Cu NWs were the unique nanostructure. The diameter and length were ~72 nm and 39 microns (aspect ratio of ~540), respectively. The TEM analysis and the selected area electron diffraction (SAED) of one section of Cu NWs are shown in Figures 6(g) and 6(h). The microphotographs showed that the NW had an average diameter of 71 nm and grew in the [110] direction [20]. Likewise, the sample exhibited diffraction spots corresponding to Cu2O phase. A careful observation of the microphotograph revealed the presence of a thin oxide layer on the wire surface indicating that PVP did not offer a good protection to the oxidation as already observed in the synthesis of Cu NPs by using 1-heptanol as reducing agent [43].Figure 6
SEM images of Cu nanostructures obtained during heating at different reaction times: (a) 0, (b) 60, (c) 100, (d) 110, (e) 120, and (f) 240 min. Insets in (b) and (c) correspond to the dissolution of the synthesized spherical Cu2O particles and the formed Cu2O cubes, respectively. (g) TEM image of Cu NWs showing the direction of growth. (h) SAED pattern of the Cu NWs.
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(h)With the above results, the following scheme can be proposed for the formation of Cu NWs. At the beginning, Cu nitrate and ethylene glycol react to give Cu2O particles through the decomposition of copper nitrate. The evolution of NO2 gas is detected. At higher temperatures, the Cu2O particles undergo dissolution and subsequently Cu+ ions get reduced to form Cu0. The dissolution and subsequent reduction of Cu+ ions to Cu0 is the rate determining a step that strikes a balance between nucleation of metallic particle and their subsequent etching to form the MTP seed. Then, the unidirectional growth of the MTPs is facilitated by the preferential absorption of the capping agent, PVP on the {100} crystal planes of Cu NWs. A graphical scheme for the formation of Cu NWs is shown in Figure 7.Figure 7
Formation scheme proposed for the synthesis of Cu NWs in Cu(NO3)2-EG-PVP system.


## 3.1. Influence of Halide Ion Source and Its Concentration on Cu NW Formation

Figure1 shows the SEM images of Cu-based products obtained in the EG-PVP system using 0.5 to 2.5 mM of CTAC as the source of Cl− ions. At Cl− ion concentration less than 0.5 mM, Cu nitrate was reduced by ethylene glycol to irregular and faceted metallic Cu particles ranging between 1 and 2 μm along with few rods. When the concentration of Cl− ions ranged between 0.5 and 1.0 mM, the Cu particles became larger in size, and rods, plates, and triangular crystals were also observed (Figure 1(a)). The formation of Cu particles with different shapes could be due to presence of twinned Cu crystals that were not etched sufficiently due to the deficiency of Cl− ions. A remarkable change was observed when the alcoholic solution contained 1.0 mM CTAC; the product was constituted mainly of thicker rods with an average aspect ratio (length/diameter) of 10 and small quantities of Cu particles with triangular facets that originated from decahedral or icosahedral crystals (Figure 1(b)).Figure 1
SEM images of Cu nanostructures obtained by reducing Cu nitrate in EG-PVP system in the presence of (a) 0.5, (b) 1.0, (c) 1.25, and (d) 2.5 mM of CTAC and (e) a schematic illustration showing the effect of Cl− ion concentration in the formation of Cu NWs. SEM images of halide type in the synthesis of Cu NWs: (f) NaF, (g) NaCl, (h) CTAB, and (i) KI at a concentration of 1.25 mM and (j) a schematic illustration that shows the effect of Ksp of Cu(I) halides in the formation of Cu NWs.
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(j)When Cl− ion concentration reached 1.25 mM, the product was constituted only of Cu NWs (Figure 1(c)). Under these conditions, the average diameter and length of NWs were 74.1 nm and 31.5 μm, respectively (aspect ratio of 423). However, when the concentration of Cl− ion concentration resulted to be too high, the shape of NW was not retained and the yield decreased progressively (Figure 1(d)) and disappeared totally at 10 mM. On the contrary, micrometer-sized spherical particles were formed at higher concentration of Cl− ions (Figure 1(d)). Usually in the presence of high concentrations of Cl− ions, the formation of nanocubes is favored as in the case of Ag NPs due to the preferential adsorption on the {100} planes [23, 24, 28]; however, this was not observed here. The XRD pattern of the spherical particles corresponded to the cubic phase of Cu2O. This suggests that the reduction of Cu2O to Cu was delayed or reduction and dissolution occurred repeatedly under high concentration of CTAC and subsequently neither the formation of Cu NWs nor nanocubes was realized.The above results suggested that at low Cl− ion concentrations, the reduction rate of Cu was too high for the seeds to undergo etching to generate preferential planes prior to growth, resulting in the formation of irregular and faceted nanostructures. On the other hand, at high Cl− ion concentrations, the etching was too strong and the concentration of Cu ions in the solution became high and led to the formation of spherical shaped Cu2O particles (Figure 1(e)). Thus, the optimum Cl concentration was determined to be around 1.25 mM, or in other words, the Cl/Cu molar ratio was 0.125. This value was relatively high compared to the one used by Whitcomb, which is 0.026 [35]. Although, the low concentration of Cl− ions could be one of the reasons for low yield, the formation of insoluble or partially soluble intermediate compound, CuCl could be another. Though the presence of CuCl was not detected when the concentration of Cl− ions was low, their presence was confirmed in the structural and morphological analysis in the products obtained during the synthesis of Cu NWs under high CTAC concentrations (5 mM) (Figure S1).Then, to determine the influence of halide type on the formation of NWs, CTAC was replaced by equal concentrations of sodium fluoride (NaF), sodium chloride (NaCl), cetyltrimethylammonium bromide (CTAB), and potassium iodide (KI). As observed in the SEM photographs shown in Figures1(f)–1(i), high yield of NWs was obtained in NaCl and CTAB cases. The above results suggested that the optimal halide concentration is very vital than the type or source of halide for the formation of Cu NWs in high yield. On the other hand, the formation of cuprous halides and their solubility product constants (Ksp) [41] could be an important factor to consider in the control of the final structure and the complete reduction of Cu salts as shown in Figure 1(j). Thus, the synthesis of high-yield Cu NWs proceeded in the following order:
(1)CuCl1.72×10−7>CuBr6.27×10−9>CuI1.27×10−12.Hence, the reduction and formation of Cu NWs is favored at high solubility of intermediate products in the solvent as in the cases of CuCl and CuBr. But, in the case of low solubility CuI, the products resulted to be a mixture of CuI, Cu2O, and Cu phases (Figure S2). On the other hand, in the case of highly soluble CuF and the instability to form CuF2 enhances the formation of Cu NPs than Cu NWs.The formation of NWs is influenced by the control over the reduction of Cu ions to form metallic Cu seeds and their subsequent etching to form MTPs that facilitate the formation of NWs. The dimensional properties of the NW are influenced very much by the unidirectional growth facilitated by the preferential adsorption of the capping agent on the crystal planes of the NWs. Thus, the role of the capping agent on the yield as well as the dimensional properties of Cu NWs will be discussed in the next section.


## 3.2. Influence of PVP on the Yield and Dimensional Properties of Cu NWs

The molecular weight and concentration of PVP have been reported to control the yield and dimensions of NWs [36–39] due to their preferential adsorption on {100} planes of metallic surface compared to {111}. Thus, the effect of PVP concentration on the synthesis of Cu NWs at the reaction temperature of 182°C is investigated, while keeping Cl−/Cu2+ molar ratio and the amount of N2 purged constant. Figure 2 shows that decreasing the PVP concentration facilitated the formation of irregular-shaped Cu NPs at the expense of Cu NWs. At low PVP concentration of 25 mM, the nucleus grew isotropically due to insufficient concentration of capping agent. In contrast, at higher PVP concentration of 75 mM, the Cu NWs became thicker and shorter. When the concentration was increased further, only NPs were formed. This is believed due to the nonpreferential adsorption of PVP molecules on the crystal faces of Cu NPs, even on the {111} planes that facilitate the unidirectional growth of NWs as shown in Figure 2(g). The FT-IR spectra of pure PVP and the Cu NWs are shown in Figure 2(e), and the adsorption of PVP on the surface of NWs was confirmed. The spectrum of the NWs synthesized using the above technique shows absorption bands at 3400 cm−1 that could be ascribed to the overtone of C=O bond. In addition, a band corresponding to O-H groups at around 3500 cm−1 was also recorded. This could due to the presence of methanol used during washing. The stretching vibrations of C-H and C=O were observed at 2920 cm−1 and 1640 cm−1, respectively. Likewise, the absorption band corresponding to the stretching mode of C-N was also observed at around 1300 cm−1. Furthermore, the PVP concentration adsorbed on the metallic surface was evaluated by thermogravimetry under N2 gas flow. As observed in Figure 2(f), the weight loss at temperatures below 180°C was around 8% and it could be ascribed to the removal of solvents such as methanol and adsorbed water. The weight loss between 180 and 200°C was steep and amounted to almost 15%. Then, the weight loss progressed slowly and an additional 5% decrease was recorded at around 600°C. These results suggested that PVP is strongly adsorbed on the Cu surface, and thermal treatments at higher temperatures are necessary to remove PVP molecules completely.Figure 2
SEM images of Cu products obtained under different PVP concentrations: (a) 25, (b) 45, (c) 55, and (d) 75 mM (scale bar: 10μm). (e) FT-IR spectra of pure PVP and PVP-capped Cu NWs. (f) Thermal behavior of PVP-capped Cu NWs measured under N2 flow. (g) Schematic illustration describing the effect of concentration on the adsorption of PVP on Cu surface.
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(g)The optimal concentration of Cl− ions to facilitate the formation of MTPs and the optimal concentration of the capping agent for their subsequent growth have been studied in the previous sections. The diameter of the NW is very much influenced by the size of the seed as well as the MTP formed subsequently. This is believed to depend on the reduction and the etching rates of the reactions. The etching rate is believed to depend on the concentration of oxygen in the reaction system besides the concentration of Cl− ions. Thus, the influence of dissolved oxygen amount on the synthesis of Cu NWs is discussed in the next section.


## 3.3. Effect of the Amount of N2 Gas Flow on the Dimensional Properties of Cu NWs

Cl− ions are assumed to form an oxidant Cl−/O2 pair with atmospheric oxygen that etches and dissolves the preferential planes of the nucleus to form MTP. Thus, the control of this mechanism is important to facilitate the formation rate of multitwinned metallic seeds that grow unidirectionally in [110] orientation with the assistance of the preferential adsorption of the capping agent in {100} planes. On the other hand, Cu NPs are unstable in air inclusively during synthesis and it is common that the reduction needs to be carried out under inert atmospheres using either N2 or Ar gas for the formation of Cu NWs [42, 43]. The reaction atmosphere also influences the rate of the reduction. Thus, the change in the N2 flow rate between 0 and 150 ml/min influenced the morphology of Cu nanostructures as shown in Figure 3. It is clear that EG-PVP system can reduce Cu even in atmospheric conditions, and Cu NWs with diameters around 60.6 nm were obtained; however, nanometer-sized Cu oxide particles attached to the surface of NW were observed. On the other hand, at N2 flow rate of 150 ml/min, the wires became thicker, ~87.5 nm, and the formation of nanocrystals with different sizes and shapes was observed at the expense of low yield of NWs. Here, the amount of O2 is reduced by adding N2 gas or other inert gases to the system, and subsequently, the selective dissolution of specific crystal planes could be inhibited favoring the growth of cubic crystals as observed in other metallic systems [44]. Thus, the formation of wires and the inhibition of oxidation of the synthesized NWs and NPs were realized under an optimum N2 flow rate of 100 ml/min.Figure 3
SEM images of Cu NWs synthesized under different N2 flow rates: (a) 0, (b) 50, (c) 100, and (d) 150 ml/min. (e) Schematic illustration describing the effect of N2 flow rate in the formation of Cu NWs.
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(e)Optimization of the reaction atmosphere facilitated the control over the etching rate and also the stability of the Cu nanostructures. The average diameter and length of the NWs were 67.4 nm and 44μm, respectively, and the aspect ratio was around 650. However, for further reduction in the diameter, the reduction rate should be enhanced. One of the parameters that could enhance the reduction rate is the reaction temperature. Thus, the results obtained by varying the reaction temperature and their influence on the dimensional properties of Cu NW are discussed in the next section.


## 3.4. Effect of Temperature

The synthesis of Cu NPs at low temperatures is realized only when additives that promote the reduction such as sodium hypophosphite monohydrate or sodium borohydride were added to the alcoholic system [29–31]. Increasing the reaction temperature near to the boiling point of ethylene glycol should enhance its reducing ability and facilitate the reduction of Cu2+ ions within a short period of time. Figure 4 and Figure S3 show the effect of reaction temperature on the synthesis of Cu NWs, while all other experimental parameters were kept constant. At 174°C, the formation of spherical Cu2O particles was concluded from SEM and XRD measurements (Figure S4). At this temperature, Cu2+ ions were reduced to form Cu2O but not to Cu metal even after a reaction time of 10 h. Even though the formation Cu NWs was confirmed at 178°C, the presence of Cu2O particles was also identified as shown in Figure 4(b). This suggested that the reaction temperature was not high enough to reduce the Cu ions completely. However, the products obtained at 182°C contained Cu NWs and free of oxide NPs (Figure 4(c)). At higher temperatures, high yield of thicker NWs free of NPs was obtained as shown in Figure 4(d). The kinetic of the reaction is expected to get accelerated at higher temperatures, and the formation of large particles is expected. In this case, the nanowires can grow in axial and radial directions easily. Thus, it was found that the diameter of Cu NWs obtained at different temperatures is influenced by the reaction temperature and NWs with average diameters ~58 nm and ~103 nm were obtained at 178°C and 186°C, respectively. Figure 4(e) shows the effect of temperature in the reduction and formation of nanowires.Figure 4
SEM images of Cu nanostructures obtained by reducing Cu nitrate in EG-PVP under different reaction temperatures: (a) 174, (b) 178 (c) 182, and (d) 186°C. (e) Schematic illustration of the effect of temperature on the formation of Cu NWs.
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(e)Our results demonstrated that Cu NWs can be synthesized in high yield in a Cl− ion-EG-PVP system by controlling the experimental parameter such as type and concentration of chloride source, concentration of PVP, the amount of N2 gas flow, and the reaction temperature. However, the physical characteristics of Cu NWs, specially the diameter, obtained under optimal conditions are not suitable to be used in the development of TCF. Thus, understanding the formation mechanism of Cu NWs is considered vital for further optimization of the process to develop of Cu NWs with high aspect ratio. In the next section, we attempted to elucidate the formation mechanism of NWs through structural and spectral analyses of the reaction solution and solids using XRD, UV-Vis, and SEM.


## 3.5. Formation Mechanism of Cu NWs

Figure5 shows the XRD patterns of samples collected at different reaction times using the following experimental conditions: 10 mM Cu nitrate, 0.125 mM of CTAC, 50 mM of PVP, 182°C, and under a N2 gas flow rate of 100 ml/min. During heating, at temperatures below 150°C, neither color variation of the alcoholic solution nor precipitation occurred. However, at temperatures between 150 and 160°C, the color of the solution turned from light blue to orange with vigorous evolution of NO2 [45]. The XRD analysis of precipitated powders taken after completion of the evolution of gases showed a unique phase that matched well with cubic structured Cu2O, and this phase remained stable even at higher temperatures as shown in Figure 5. It is clear that at this temperature, the reducing potential of ethylene glycol was only sufficient to reduce Cu2+ ions to Cu+, but not to Cu0 due to the presence of chloride which delayed the reduction as observed above. The Cu oxide phase remained for nearly 100 min at 182°C, and then, the orange colored solution turned progressively to red caused by the transformation of Cu2O to Cu as confirmed by XRD. The reduction of Cu2O to Cu0 was totally completed in 10 minutes, and no further change was observed until the end of reaction. It is necessary to emphasize that intermediate phases such as hydroxide, chloride, or oxide (CuO) were not observed during the reduction of Cu nitrate to Cu metal.Figure 5
XRD patterns and UV-Vis spectra of Cu products collected during heating at 182°C. Inset of UV-Vis spectra corresponds to the UV-Vis spectra of solution at 50 and 150°C.Cu2O and Cu NPs possess localized surface plasmon resonance at around 400 to 700 nm [32], which depends on the particle size and morphology. Thus, the progression of the reaction Cu2+ → Cu+ → Cu0 during heating at 182°C at different reaction times was analyzed using UV-Vis spectroscopy (Figure 5). At 50°C and at 150°C, the UV-Vis spectra revealed a broad absorption peak at around 800 nm that could be ascribed to Cu2+ ions coordinated with ethylene glycol and disappeared totally when Cu2O was formed at higher temperatures. When the temperature reached 182°C, a broad absorption band centered at around 440 nm was observed. This could be assigned to the presence of Cu2O particles, and this was not present in the spectra measured at temperatures lower than 182°C (inset Figure 5). After 60 min, at 182°C, the UV-Vis spectrum exhibited a shift in the peak corresponding to Cu2O from 440 nm to 470 nm, which is believed due to particle growth. After 100 min, at 182°C, the color changed from orange to red and a new absorption peak appeared at 570 nm. This could be as a consequence of Cu2O reduction to metallic Cu seeds [32]. The reduction reaction from Cu2O to Cu was relatively faster and the Cu2O absorption peak disappeared totally in 10 minutes leaving the peak corresponding to Cu NWs at 575 nm [21]. No change was observed after 120 min, and absorption peak corresponding to Cu remained even at the end of the reaction.The FE-SEM images of these samples (Figure6) showed sphere-shaped Cu2O particles with a broad size distribution and an average size of 500 nm in the first few minutes of reaction at 182°C. After 60 min of reaction, the spherical Cu2O particles began to dissolve as shown in the inset. However, the dissolved particles precipitated again as Cu2O and no other oxide phase was detected in the XRD pattern. As reaction progressed, the dissolution proceeded, and after 100 min, the dissolved oxide was reduced to Cu metal in alcoholic solution. Then, due to the presence of Cl− ions and PVP, the metallic Cu seeds grew in a preferential direction, whereas rest of the Cu ions in the solution precipitated into small Cu2O cubes as observed in the inset. However, it is not clear whether these cubes originated during cooling the Cu2+ ions that remained in the solution or they existed prior to cooling. After 120 min of reaction, product constituted mainly of Cu NWs; however, the presence of Cu2O on the NW surfaces still remained. At the end of reaction, Cu NWs were the unique nanostructure. The diameter and length were ~72 nm and 39 microns (aspect ratio of ~540), respectively. The TEM analysis and the selected area electron diffraction (SAED) of one section of Cu NWs are shown in Figures 6(g) and 6(h). The microphotographs showed that the NW had an average diameter of 71 nm and grew in the [110] direction [20]. Likewise, the sample exhibited diffraction spots corresponding to Cu2O phase. A careful observation of the microphotograph revealed the presence of a thin oxide layer on the wire surface indicating that PVP did not offer a good protection to the oxidation as already observed in the synthesis of Cu NPs by using 1-heptanol as reducing agent [43].Figure 6
SEM images of Cu nanostructures obtained during heating at different reaction times: (a) 0, (b) 60, (c) 100, (d) 110, (e) 120, and (f) 240 min. Insets in (b) and (c) correspond to the dissolution of the synthesized spherical Cu2O particles and the formed Cu2O cubes, respectively. (g) TEM image of Cu NWs showing the direction of growth. (h) SAED pattern of the Cu NWs.
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(h)With the above results, the following scheme can be proposed for the formation of Cu NWs. At the beginning, Cu nitrate and ethylene glycol react to give Cu2O particles through the decomposition of copper nitrate. The evolution of NO2 gas is detected. At higher temperatures, the Cu2O particles undergo dissolution and subsequently Cu+ ions get reduced to form Cu0. The dissolution and subsequent reduction of Cu+ ions to Cu0 is the rate determining a step that strikes a balance between nucleation of metallic particle and their subsequent etching to form the MTP seed. Then, the unidirectional growth of the MTPs is facilitated by the preferential absorption of the capping agent, PVP on the {100} crystal planes of Cu NWs. A graphical scheme for the formation of Cu NWs is shown in Figure 7.Figure 7
Formation scheme proposed for the synthesis of Cu NWs in Cu(NO3)2-EG-PVP system.


## 4. Conclusions

The synthesis of Cu nanowires (NWs) in high yield has been developed using Cu(NO3)2-EG-PVP system. A formation mechanism was proposed and summarized as follows: (1) partially reduction of Cu ions to Cu2O, (2) redissolution of Cu2O and reduction to Cu0, (3) formation of Cu seeds, and (4) unidirectional growth of Cu0. The concentration of Cl− ions and the dissolved oxygen was found vital to control the etching rate of copper seeds. Furthermore, the reaction temperature was important to obtain copper seeds in large quantities, which get etched subsequently to form and control the number of MTPs. Finally, the PVP concentration was a decisive factor that facilitates the unidirectional growth of the MTPs through specific adsorption on the {100} planes to inhibit the lateral growth of the NWs. The NWs obtained under the optimum conditions derived in this study resulted in the synthesis of Cu NWs that were more 40 microns in length and 60 nm in diameter or aspect ratio higher than 667 that could become a potential material for the fabrication of conducting films.



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*Source: 1698357-2018-08-08.xml*