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Article

Reductive and Coordinative Effects of Hydrazine in Structural Transformations of Copper Hydroxide Nanoparticles

by
Xenia Medvedeva
1,
Aleksandra Vidyakina
1,
Feng Li
1,
Andrey Mereshchenko
1,2 and
Anna Klinkova
1,*
1
Department of Chemistry and Waterloo Institute for Nanotechnology, University of Waterloo, Waterloo, ON N2L 3G1, Canada
2
Institute of Chemistry, Saint-Petersburg State University, 7/9 Universitetskaya emb., St. Petersburg 199034, Russia
*
Author to whom correspondence should be addressed.
Nanomaterials 2019, 9(10), 1445; https://doi.org/10.3390/nano9101445
Submission received: 9 September 2019 / Revised: 5 October 2019 / Accepted: 6 October 2019 / Published: 11 October 2019
(This article belongs to the Special Issue Novel Nanomaterials for Applications in Energy and Catalysis)
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Abstract

:
Shape-specific copper oxide nanostructures have attracted increasing attention due to their widespread applications in energy conversion, sensing, and catalysis. Advancing our understanding of structure, composition, and surface chemistry transformations in shaped copper oxide nanomaterials during changes in copper oxidation state is instrumental from both applications and preparative nanochemistry standpoints. Here, we report the study of structural and compositional evolution of amorphous copper (II) hydroxide nanoparticles under hydrazine reduction conditions that resulted in the formation of crystalline Cu2O and composite Cu2O-N2H4 branched particles. The structure of the latter was influenced by the solvent medium. We showed that hydrazine, while being a common reducing agent in nanochemistry, can not only reduce the metal ions but also coordinate to them as a bidentate ligand and thereby integrate within the lattice of a particle. In addition to shape and composition transformation of individual particles, concurrent interparticle attachment and ensemble shape evolution were induced by depleting surface stabilization of individual nanoparticles. Not only does this study provide a facile synthetic method for several copper (I) oxide structures, it also demonstrates the complex behavior of a reducing agent with multidentate coordinating ability in nanoparticle synthesis.

Graphical Abstract

1. Introduction

Controlled fabrication of copper oxides and hydroxides (e.g., CuO, Cu2O, CuOH, Cu(OH)2) nanostructures in different morphologies has attracted increasing attention in recent years due to their potential applications in energy conversion, electrode materials, sensing, and catalysis [1,2,3]. Specifically, these materials have been used as a negative electrode material for lithium-ion batteries [4,5], a stable catalyst for photochemical water splitting [6,7], a replacement for expensive noble metal catalysts in the oxidation of carbon monoxide, nitric oxide, volatile organics [8,9,10], and in C–N and C–S cross-coupling reactions [11,12]. In addition, various copper oxide materials have been used as precursors for oxide-derived copper for CO2 electroreduction [13,14,15]. Maximization of their performance metrics in these processes relies on tailoring their structure, composition, and surface chemistry to optimize their physical and chemical properties that enable these applications.
To this end, variously shaped copper oxide nanostructures [16], including cubes [17], cuboctahedra [18], octahedral [19], multipods [20], nanowires [21], nanotubes [22], and hollow structures [23], have been synthesized to date. Specifically, multipod, branched, or dendric nanoparticles are of particular interest in conventional, electro-, and photocatalysis due to their (a) highly developed surface area, (b) exposed high index facets and edges with undercoordinated sides, and (c) inability to densely pack on substrates, resulting in rough and porous material deposits, with all of these factors generally leading to higher catalytic activity [24,25]. Shaped copper oxide nanostructures are typically prepared by chemical reduction, electrodeposition, and solvothermal synthesis methods. In addition to traditional solution-based methods, shape-specific copper oxide micro- and nanostructures can be obtained from shape-defined nanostructured solid precursors via chemical oxidation in the presence of shape-directing surfactants [26] as well as via an electrochemical process [27], although few reports explored this approach and associated structural changes. At the same time, only limited information is available regarding structural transformations of amorphous copper oxide nanoparticles upon inducing changes in their oxidation state [1,2,3]. Further elucidation of shape transformations of copper oxide nanoparticles upon oxidation or reduction would expand the toolbox of preparative nanochemistry and enable the development of superior functional materials for energy and catalysis. Morphological transformations of amorphous copper oxide nanomaterials are of particular interest; the absence of short-range order could allow for integration or entrapment of polydentate ligands within the material upon changes in the oxidation state [28], introducing compositional moieties similar to metal-organic coordination polymers [29,30], which represents an unexplored and promising avenue of composite materials from both synthetic and application standpoints.
Here, we report the study of structural and compositional evolution of copper (II) hydroxide nanoparticles under hydrazine reduction conditions. Nanoparticle synthesis often relies on chemical reduction, with hydrazine being one of the most common reducing reagents in nanochemistry [31]. While hydrazine is typically used solely as a reducing agent [32,33,34], this work shows that, in the excess of hydrazine, it can not only reduce the metal ions but can also integrate within the lattice of the nanoparticle, resulting in the formation of copper coordination compound–oxide composite nanoparticles. At different hydrazine–copper ratios, we observed structural evolution of amorphous Cu(OH)2 nanocages to crystalline Cu2O nanoparticles and to composite Cu2O-N2H4 branched nanostructures. Both single particle structural evolution and multi-particle assembly and concurrent structural evolution could be performed by controlling the amount of the stabilizing polymer engulfing the nanoparticles. Interestingly, the hydrazine-containing composite nanoparticle shape could be switched from the branched to a zigzag-like structure by simply switching the reaction solvent, which suggests that the solvent plays a shape-directing role in this process. Not only does this study provide a facile and easily scalable method for several copper (I) oxide structures, but it also demonstrates the complex behavior of a reducing agent with multidentate coordinating ability in nanoparticle synthesis.

2. Materials and Methods

2.1. Materials

Copper(II) chloride (CuCl2, 99.995%), polyvinylpyrrolidone (PVP, Mn = 55 kDa), sodium borohydride (NaBH4, powder, 98%), hydrazine monohydrate (N2H4 65%, reagent grade, 98% purity), anhydrous methanol (99.5%) and ethanol (99.5%) were purchased from Sigma Aldrich (Oakville, ON, Canada).

2.2. Cu(OH)2 Precursor Synthesis

Amorphous Cu(OH)2 nanocages were prepared using a previously reported procedure [35]. In a typical synthesis, 40 mL of ethanol and 261 mg of PVP were placed in a 250 mL Erlenmeyer flask followed by 15 min of sonication and subsequent addition of 40 mL of 5.2 mM CuCl2 solution in ethanol under sonication. The resultant emerald solution was stirred for 30 min, followed by the addition of 20 mL of freshly prepared 20 mM NaBH4 solution in ethanol in one quick shot under vigorous stirring, resulting in the immediate color change to deep brown. The final solution was left undisturbed at room temperature for 48 h. As prepared bright-blue colloid was purified by two 15 min centrifugation cycles at 5000× g and subsequent redispersion of the precipitate in 20 mL of ethanol to give a final stock solution of Cu(OH)2 nanocages.

2.3. N2H4 Reduction of Cu(OH)2

Then, 3% solution of N2H4 in deionized water was added dropwise to 10 mL of Cu(OH)2 nanocages stock solution under vigorous vortexing, resulting in the solution color change to orange. Specifically, to obtain Cu2O and Cu2O-N2H4 nanoparticles, stochiometric (27 µL) and 20 times excess (530 µL) of N2H4 were used, respectively. The solution was stirred for another minute and purified by a 5 min centrifugation cycle at 5000× g (for electron microscopy imaging, the solution can be used without purification, giving same imaging results).
To induce simultaneous assembly and reduction of Cu(OH)2 nanocages in the excess of N2H4 and to subsequently form larger branched Cu2O-N2H4 particles, initial Cu(OH)2 nanocages stock solution was subjected to three additional washing cycles by centrifugation at 5000× g and redispersion in the same amount of ethanol, otherwise the N2H4 reduction procedure remained the same.
To obtain zigzag-like structures instead of branched structures upon five times washed Cu(OH)2 nanocage reduction with excess hydrazine, the reaction solvent was switched from ethanol to methanol by using it for redispersion of the particles during their washing.

2.4. Electrochemical Reduction of Cu2O and Cu2O-N2H4

The electroreduction experiments were performed in a one-compartment cell using a three-electrode system connected to an electrochemical workstation (Biologic SP-300, purchased from SnowHouse Solutions, Lac-Beauport, QC, Canada). As prepared colloids were diluted 10 times with ethanol and dropcasted onto carbon paper strips (Toray TGP-H-060, Fuel Cell Store, College Station, TX, USA) that were used as working electrodes. Ag/AgCl (with saturated KCl as a filling solution) and platinum gauze were used as a reference and counter electrodes, respectively. The electrolyte was 0.5M KHCO3 buffer (pH = 7.2) saturated with argon. Four cyclic voltammetry (CV) cycles from 0 to −1.2 V vs. reversible hydrogen electr0ode (RHE) at 20 mV/s scan rate were performed to yield the electroreduced structures.

2.5. Nanoparticle Characterization

For the structural analysis, scanning and transmission electron microscopy (SEM and TEM, respectively) imaging was performed using a scanning transmission electron microscope Hitachi S-5200 microscope (purchased from Scanservice Corp., Tustin, CA, USA) equipped with SE and STEM detectors operating at 25 kV. Samples for imaging were prepared by depositing a droplet of the colloid on a 400 mesh carbon-coated copper grid and allowing the solvent to evaporate.
For the composition and surface analysis, concentrated, dried, and powdered samples were analyzed by X-ray photoelectron spectrometry (XPS), X-ray diffraction (XRD), elemental analysis, and infrared spectrometry using ThermoFisher Scientific K-Alpha X-ray photoelectron spectrometer (Ontario Centre for the Characterisation of Advanced Materials, Toronto, ON, Canada), Bruker D8 Advance powder X-ray diffractometer (Watlab, Waterloo, ON, Canada), Flash 2000 CHNS Analyzer (Analest, Toronto, ON, Canada), and ThermoScientific Nicolet 6700 FT-IR spectrometer (Smith Lab, Waterloo, ON, Canada) operating in transmission mode, respectively.

3. Results and Discussion

3.1. Synthesis of the Starting Material

The starting material, amorphous Cu(OH)2 nanocages with a narrow size distribution and a regular shape, were synthesized according to a previously reported method based on the reduction of CuCl2 with NaBH4 in ethanol in the presence of PVP as a stabilizing polydentate ligand [35]. In this method, the formation of Cu(OH)2 nanocages proceeded through the oxidation of initially formed copper clusters. SEM and TEM images of the resultant Cu(OH)2 nanocages with average core size 165 ± 10 nm and extending 51 ± 17 nm arms are shown in Figure 1a and Figure S1. Elongated 17 ± 4 nm-wide bundles comprising the structure observed in the SEM and the TEM images were formed due to the anisotropic nature of Cu(OH)2, as it consists of complex chains formed through coordination of OH− and Cu2+, while the bundle organization and the overall size of the particles were dictated by the stabilizing surfactant [36].

3.2. Structural Evolution at a Stochiometric N2H4 to Cu Ratio

During typical reduction with hydrazine, each molecule of N2H4 provides four electrons, leaving nitrogen gas and protons as byproducts. Thus, to reduce all Cu(II) to Cu(I) in Cu(OH)2 nanocages solution, ¼ equivalent of N2H4 was required stoichiometrically. Upon introducing this amount of the reductant to the Cu(OH)2 nanocage solution, an instantaneous change in color from bright blue to orange was observed (Figure S2), and the resultant particles were imaged within 5 min from the reaction using high resolution scanning transmission electron microscope. As evident from SEM and TEM images (Figure 1c), the final particle shape was reminiscent of the original nanocage shape but appeared granular, perforated, and without arm definition. When only half the stochiometric amount of N2H4 was introduced to the original solution of Cu(OH)2 nanocages, the SEM and the TEM image analysis clearly showed that the resultant particles were not fully reduced, with some of them being more reduced than others (Figure 1b). This uneven reduction of the particle population was likely due to mass transfer limitations, as the reduction process was extremely fast. Figure 1d shows a sequence of representative high magnification SEM images of original and reduced nanostructures at different N2H4 to copper ratios. These images show that, upon hydrazine reduction, the nanostructure did not significantly reconstruct but instead preserved the three-dimensional footprint of the original particle while losing a fraction of volume, which resulted in perforations. Interestingly, this situation only applies unless an excess of hydrazine is introduced to the particles.

3.3. Structural Evolution in Excess N2H4

A 20-fold excess of hydrazine introduced to Cu(OH)2 nanocages purified according to the standard protocol resulted in a drastic change of the particle shape. Figure 2a,c shows SEM and TEM images of the resultant branched particles with an average size of 256 ± 35 nm, which was comparable to the size of the original nanocages, indicating that each of these particles originated from individual Cu(OH)2 nanocages or single-particle transformation regime.
However, when a 20-fold excess of hydrazine was introduced to extensively washed Cu(OH)2 nanocages, the resultant branched particles were substantially larger in size (ranging from 250 nm up to 2 µm) and had a large size variation (Figure 2b,d). This increase in size suggests that extensive removal of PVP ligands enabled interparticle surface interaction and their subsequent association coinciding with the structural transition. Considering the presence of the excess hydrazine during the reaction and the accessibility of the particle surface due to the lack of PVP, interparticle attachment could be induced by hydrazine acting as a linker between particles. Indeed, due to the presence of lone pairs on both nitrogen atoms in N2H4, hydrazine could behave as a bidentate ligand, and a number of coordination compounds of Cu(II) and Cu(I) containing hydrazine were reported in earlier literature [37,38,39]. Thus, particle attachment regime was the first indication of excess hydrazine integrating into the final structure. A further compositional analysis is provided in the following section.
The structures obtained in this particle attachment regime exhibited predominantly octahedron-derived hexapod shape, which has been observed for Cu2O nanoparticles [40]. However, in our case, the pods of some hexapods were not symmetrically distributed around the particle center, and their surface was very rough—a morphology that has not been previously reported for Cu2O. These branched particles degraded during imaging under continuous electron beam exposure (Figure S3). In addition, while being structurally stable in air for many hours, after two days, the solution darkened (Figure S4), and dense particles mixed with the original branched structures were observed in SEM and TEM (Figures S5 and S6). These denser particles were metal copper (confirmed by XRD, Figure S7), indicating that the remaining hydrazine was capable of slowly reducing Cu(I) further to Cu(0) over time.
To gain further insight into the structural evolution in the particle attachment regime [28] in the excess hydrazine, we analyzed the structures obtained at its 4-, 5-, 10-, 15-, 20-, 50-, and 100-fold excess compared to the stochiometric ratio. At 4-fold excess hydrazine, we were able to capture intermediate structures consisting of granular and perforated Cu2O mixed with less electron-dense material and composed of smaller particles with sizes comparable to those of the precursor Cu(OH)2 nanocages (Figure 3). The lower electron density of the material observed in TEM (Figure 3b) indicated [41] that the spacing between copper atoms was increased compared to Cu2O, which could be explained by coordinative integration of hydrazine within the material. A patchy distribution of electron density suggested that such integration could be uneven throughout the particles (including partial transformation to metal copper, see Section 3.4 for further discussion on the composition evolution), which matches the void-containing nature of the precursor Cu(OH)2 nanocages and stoichiometrically reduced Cu2O.
The structural evolution of the reaction mixture at higher excess of hydrazine is presented in Figure 4. Granular and perforated Cu2O particles along with the small (sub-20 nm) nanoparticles could be found in the mixture with up to 15-fold N2H4 excess (Figure 4a–c and Figure S8). The arms of the nanocages (see inset in Figure 1a) breaking off during the initial reduction of Cu(OH)2 bundles could explain the origin of the small nanoparticles. The presence of small and large branched particles along with the particles noted above pointed at the rate of hydrazine incorporation being comparable with that of Cu(II) reduction, which enabled a simultaneous formation of these structures. Interestingly, the structures appeared to have approached a stable shape around 20-fold excess N2H4 (Figure 4d), as no significant structural changes or particle size increases were observed at above this hydrazine–copper ratio (Figure 4e,f and Figure S9).

3.4. Composition Evolution

The crystallinity of the structures was assessed using XRD (Figure 5a), and while the initial Cu(OH)2 nanocages were amorphous, the particles obtained at the stochiometric hydrazine–copper ratio had a typical pattern of Cu2O with peak broadening characteristic of nanoparticles. However, the material obtained at 20-fold excess N2H4 showed several additional peaks to those of Cu2O, which were indicative of a mixed phase containing Cu2O. Another phase was likely a coordination compound containing N2H4 as a Cu(I) ligand.
Infrared spectra of Cu(OH)2 nanocages and reduced particles obtained at the stoichiometric and the excess amounts of hydrazine are shown in Figure 5b. A strong broad peak at 3000–3600 cm−1 characteristic of O–H stretching [42] present in the initial Cu(OH)2 drastically decreased in the reduced structures, indicating a significant decrease in the number of OH groups. Both Cu(OH)2 and Cu2O obtained at a stochiometric hydrazine–copper ratio showed moderate C=O and C–N stretching and C–H bending peaks between 1660 and 1250 cm−1 as well as C–H stretching peaks between 2850 and 2950 cm−1 corresponding to the functional groups in PVP, present in all of these samples. Particles obtained in 20-fold excess hydrazine showed additional peaks at 3150–3350 cm−1 and 1600 cm−1, corresponding to N–H stretching and bending, respectively. This result further supported the integration of N2H4 within the final structures.
XPS analysis confirmed the reduction of Cu(II) to Cu(I) in Cu(OH)2 nanocages upon introduction of the stochiometric amount of hydrazine (Figure 5c). At 20-fold excess hydrazine, the XPS spectrum remained unchanged, and the satellite peak at 944 eV characteristic of Cu(I) was still present. The XPS analysis of the structures obtained at different hydrazine excess (from 0- to 50-fold) provided the information about the hydrazine uptake within the structure. Specifically, Figure 5d shows nitrogen–oxygen, nitrogen–copper, and oxygen–copper ratios as a function of the amount of introduced hydrazine obtained from the quantitative analysis of the characteristic peaks of these elements in the samples. At hydrazine–copper ratio above stoichiometric (or molar ratio above [N2H4]:[Cu(OH)2] = 0.25), a significant increase in N–O and N–Cu ratios was observed, in agreement with hydrazine integration within the structure. At equimolar hydrazine–copper ratio, a drastic drop in O–Cu ratio was observed, indicative of a nearly complete Cu(II) to Cu(I) reduction, while at a slight excess of hydrazine, O–Cu ratio continued to decrease. With further hydrazine–copper ratio increase, the content of oxygen in the samples began to increase, suggesting a possible solvent incorporation within the structure along with hydrazine.
According to the elemental analysis (see Supplementary Materials, Figures S12, 13, and Tables S1–S3 for details of the composition calculations), at 20-fold excess hydrazine, its NH2 groups were only coordinated to approximately 7–9% of Cu ions on average throughout the sample, while ethanol was coordinated to ~10% of Cu ions. This result demonstrated that the fraction of Cu2O phase dominated over the hydrazine-containing coordination compound, in agreement with XRD and XPS data. In addition, it pointed at the significant incorporation of the solvent within the structure under conditions favoring the hydrazine coordination.
To gain further insight into the structural integrity and the distribution of the two phases within the particles, we performed electrochemical reduction of the structures obtained at stoichiometric and excess amounts of hydrazine. Specifically, the hydrazine treatment was performed directly on the particles tethered to a carbon paper substrate used for the subsequent electrochemical reduction. To obtain tethered particles, Cu(OH)2 nanocages solution was dropcasted and dried on carbon paper strips (Figure 6a,a’), which were then dipped into the solution of hydrazine with corresponding N2H4 amounts. The obtained tethered structures are shown in Figure 6b,b’. Upon electrochemical reduction under the same cathodic conditions, the particles obtained at the stoichiometric hydrazine–copper ratio primarily preserved their overall shape while losing a fraction of their mass, which was evident from the increased size of the perforations (Figure 6c). In contrast, the particles obtained at hydrazine excess completely disintegrated, and only shape-undefined nanoporous copper deposits could be observed in their place (Figure 6c’). These deposits contained clumps of copper under 50 nm in size, with pores corresponding to those of the particles observed in Figure 6c. This result suggests that the Cu2O phase existed in the unreduced structures in the form of sub-50 nm granules, which were interconnected with the hydrazine-based complex of copper, assuming that the latter was easily destroyed during the electrochemical reduction.

3.5. Solvent Effect

The integration of the solvent within the structure in the excess of hydrazine revealed in the compositional analysis of the materials motivated us to explore the effect of the solvent on the structural transformation of Cu(OH)2 nanocages. To this end, we performed their reduction with 20-fold excess hydrazine ([N2H4]:[Cu(OH)2] = 5) in methanol in place of ethanol as a solvent. The obtained structures were consistently of zigzag-like shape and in 1–2 µm range (Figure 7), regardless of the number of washing cycles (2–5) used to purify the initial Cu(OH)2 nanocages and exchange their solvent to methanol. This was likely due to higher solubility of PVP in methanol compared to ethanol [43] and subsequent surface exposure of the particles, which enabled their interparticle assembly via hydrazine linking. Indeed, when the reaction was performed in 1- or 2-propanol (slightly worth solvents for PVP compared to ethanol) [39] under the same conditions otherwise, the obtained structures matched the initial nanocages in size and showed little shape definition (Figure S10). When the same reaction was performed in water as a solvent instead of alcohols, dense Cu2O crystallites were observed upon imaging (Figure S11), further highlighting the shape-directing importance of the presence of alcohols in these reactions.
While the mechanism of shape selectivity in Cu(OH)2 reduction in excess hydrazine remains unclear and requires further investigation, our results suggest that the reaction solvent has a shape-directing effect, either via surface or bulk interaction with the transforming particle.

4. Conclusions

This study provides a new synthetic approach to complex copper (I) oxide particles’ branched and zigzag-like structures and describes reductive and coordinative effects of hydrazine when its excess is used for copper hydroxide reduction. More generally, we demonstrated that (1) hydrazine, while being a common reducing agent, also has coordinative ability that needs to be considered in nanochemistry reactions, especially if excess hydrazine is used; (2) when polydentate ligating species are present in the reaction medium during particle transformation, crystallization by particle attachment can take place, resulting in the addition of higher-order colloidal species (as opposed to solution-state precursors) to fully formed particles; (3) during reduction of Cu(OH)2 with excess hydrazine, not only hydrazine itself but also the solvent species are capable of coordinative integration within the lattice of the formed particles. In addition, these findings open the door for exploring this type of concurrent reductive/coordinative chemistry in other transition metal systems with multiple stable oxidation states.

Supplementary Materials

The following are available online at https://www.mdpi.com/2079-4991/9/10/1445/s1, Figure S1: TEM image of as synthesized Cu(OH)2 nanocages, Figure S2: A photograph of Cu(OH)2 nanocages colloid before (left) and after (right) introducing N2H4. Note that the color of hydrazine-treated solutions was the same at a stoichiometric N2H4 amount and excess N2H4 added to Cu(OH)2 nanocages, Figure S3: TEM image of Cu2O-N2H4 obtained at [N2H4]:[Cu(OH)2] = 5 at 25 kV accelerating voltage at 15,000× magnification. Inset shows the effect of electron beam exposure obtained at 25 kV accelerating voltage and 70,000× magnification after 30 s exposure time (scale in the inset matches the figure), Figure S4: A photograph of Cu2O-N2H4 colloid (obtained by treating Cu(OH)2 nanocages in ethanol with hydrazine ([N2H4]:[Cu(OH)2] = 5) immediately after hydrazine addition (left) and after aging the mixture for 2 days (right), Figure S5: TEM (top left) and SEM (top right and bottom) images of Cu2O-N2H4 colloid (obtained by treating Cu(OH)2 nanocages in ethanol with hydrazine ([N2H4]:[Cu(OH)2] = 5) after its aging for 2 days, Figure S6: TEM (left) and SEM (right) images of Cu2O-N2H4 colloid (obtained by treating Cu(OH)2 nanocages in ethanol with hydrazine ([N2H4]:[Cu(OH)2] = 5) after its aging for 5 days, Figure S7: XRD patterns of Cu2O-N2H4 colloid (obtained by treating Cu(OH)2 nanocages in ethanol with hydrazine ([N2H4]:[Cu(OH)2] = 5) within a day of hydrazine addition (red) and after aging the mixture for 5 days (green), Figure S8: SEM images of the intermediate structures observed upon treatment of Cu(OH)2 with 5-fold excess hydrazine compared to the stoichiometric ratio ([N2H4]:[Cu(OH)2] = 1.25), Figure S9: TEM image of the structures obtained from Cu(OH)2 upon their reduction with 100-fold excess hydrazine compared to the stoichiometric ratio ([N2H4]:[Cu(OH)2] = 25), Figure S10: SEM images of the structures obtained by the reduction of Cu(OH)2 nanocages with excess hydrazine ([N2H4]:[Cu(OH)2] = 5) in 1-propanol (a,b) and in 2-propanol (c,d), Figure S11: SEM images of the structures obtained by the reduction of Cu(OH)2 nanocages with excess hydrazine ([N2H4]:[Cu(OH)2] = 5) in water, Figure S12: The composition of Cu(OH)2 nanocages and the structures obtained upon their reduction with a stoichiometric amount and 20-fold excess of hydrazine ([N2H4]:[Cu(OH)2] 0, 0.25, and 5, respectively). (a) Atomic fractions of H, C, and N from CHN derived from the elemental analysis. (b) Molar fractions of the molecular components calculated from the elemental analysis assuming (1) the samples contained only Cu(OH)2, CuO/Cu2O, PVP, EtOH and N2H4, and (2) all three studied samples had the same amount of PVP (i.e., no loss if PVP upon hydrazine reduction), Figure S13: Comparison of the atomic ratios (N/O, N/Cu and O/Cu), calculated from the XPS and CHN analyses’ data for the initial Cu(OH)2 nanocages and structures obtained by the reduction thereof with stoichiometric and excessive amounts of hydrazine ([N2H4]:[Cu(OH)2] 0.25 and 5, respectively), Table S1: Elemental analysis data: weight percentages (ω%) of N, C, and H in Cu(OH)2 nanocages and structures obtained by their reduction with a stoichiometric amount and the excess of hydrazine ([N2H4]:[Cu(OH)2] 0, 0.25, and 5, respectively), Table S2: Elemental analysis data converted to atomic percentages (a%) of N, C, and H, and calculated molar fractions (in %) of the components in Cu(OH)2 nanocages and structures obtained by their reduction with a stoichiometric amount and the excess of hydrazine ([N2H4]:[Cu(OH)2] 0, 0.25, and 5, respectively), Table S3: Comparison of atomic percentages (a%) of Cu, O, and N, obtained from XPS analysis and calculated from the CHN data for Cu(OH)2 nanocages and the structures obtained upon their reduction with a stoichiometric amount and 20-fold excess of hydrazine ([N2H4]:[Cu(OH)2] 0, 0.25, and 5, respectively).

Author Contributions

Conceptualization, A.K.; methodology, A.V., X.M.; validation, X.M., A.V. and F.L.; formal analysis, X.M.; writing—original draft preparation, X.M., A.K.; writing—review and editing, A.K., A.M.; visualization, X.M.; supervision, A.K.; project administration, A.K.; funding acquisition, A.K.

Funding

This research was funded by the University of Waterloo, the Natural Sciences and Engineering Research Council of Canada, and Canadian Foundation for Innovation.

Conflicts of Interest

The authors declare no conflict of interest.

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Figure 1. Structural evolution of Cu(OH)2 particles during the reduction with a stoichiometric hydrazine–copper ratio. SEM and TEM images of Cu(OH)2 nanocages (a) and reduction products obtained at [N2H4]:[Cu] = 1:8 (b) and at [N2H4]:[Cu] = 1:4, which corresponded to the stoichiometric hydrazine–copper ratio (c). TEM and high magnification SEM images of the corresponding structures are shown in the insets in (a–c) and in (d), respectively.
Figure 1. Structural evolution of Cu(OH)2 particles during the reduction with a stoichiometric hydrazine–copper ratio. SEM and TEM images of Cu(OH)2 nanocages (a) and reduction products obtained at [N2H4]:[Cu] = 1:8 (b) and at [N2H4]:[Cu] = 1:4, which corresponded to the stoichiometric hydrazine–copper ratio (c). TEM and high magnification SEM images of the corresponding structures are shown in the insets in (a–c) and in (d), respectively.
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Figure 2. Structures obtained from Cu(OH)2 particles upon their reduction with excess hydrazine (20-fold compared to the stoichiometric ratio). SEM (a,b) and TEM (c,d) images of the particles obtained in the single-particle transformation regime (a,c) and in the particle attachment regime (b,d).
Figure 2. Structures obtained from Cu(OH)2 particles upon their reduction with excess hydrazine (20-fold compared to the stoichiometric ratio). SEM (a,b) and TEM (c,d) images of the particles obtained in the single-particle transformation regime (a,c) and in the particle attachment regime (b,d).
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Figure 3. Structures obtained from Cu(OH)2 nanocages upon their reduction with 4-fold excess hydrazine compared to the stoichiometric ratio. SEM (a) and TEM (b) images correspond to the same sample area. Red circles in (a) correspond to the average size of Cu(OH)2 cores and are shown for eye guidance and comparison.
Figure 3. Structures obtained from Cu(OH)2 nanocages upon their reduction with 4-fold excess hydrazine compared to the stoichiometric ratio. SEM (a) and TEM (b) images correspond to the same sample area. Red circles in (a) correspond to the average size of Cu(OH)2 cores and are shown for eye guidance and comparison.
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Figure 4. SEM images of the structures obtained from Cu(OH)2 particles upon their reduction with 5-fold (a), 10-fold (b), 15-fold (c), 20-fold (d), 50-fold (e), and 100-fold (f) excess hydrazine compared to the stoichiometric ratio.
Figure 4. SEM images of the structures obtained from Cu(OH)2 particles upon their reduction with 5-fold (a), 10-fold (b), 15-fold (c), 20-fold (d), 50-fold (e), and 100-fold (f) excess hydrazine compared to the stoichiometric ratio.
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Figure 5. Composition characterization of Cu(OH)2 nanocages and the structures obtained upon their treatment with hydrazine. XRD patterns (a), infrared spectra (b), and XPS spectra of the initial Cu(OH)2 nanocages (black traces), reduced structures obtained at a stoichiometric hydrazine–copper ratio (blue traces) and at 20-fold excess hydrazine (red traces) (c). (d) N/O (red triangles), O/Cu (green squares), and N/Cu (blue circles) ratios obtained from quantitative X-ray photoelectron spectrometry (XPS) analysis of Cu(OH)2 nanocages and products obtained from their treatment with different [N2H4]:[Cu(OH)2] molar ratios (with [N2H4]:[Cu(OH)2] = 0.25 being the stoichiometric ratio).
Figure 5. Composition characterization of Cu(OH)2 nanocages and the structures obtained upon their treatment with hydrazine. XRD patterns (a), infrared spectra (b), and XPS spectra of the initial Cu(OH)2 nanocages (black traces), reduced structures obtained at a stoichiometric hydrazine–copper ratio (blue traces) and at 20-fold excess hydrazine (red traces) (c). (d) N/O (red triangles), O/Cu (green squares), and N/Cu (blue circles) ratios obtained from quantitative X-ray photoelectron spectrometry (XPS) analysis of Cu(OH)2 nanocages and products obtained from their treatment with different [N2H4]:[Cu(OH)2] molar ratios (with [N2H4]:[Cu(OH)2] = 0.25 being the stoichiometric ratio).
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Figure 6. SEM images of Cu(OH)2 nanocages dropcasted on a carbon paper substrates (a,a’) that were treated with stoichiometric (b) and 20-fold excess (b’) amounts of hydrazine and subsequently electroreduced using four cathodic cyclic voltammetry (CV) cycles (c,c’).
Figure 6. SEM images of Cu(OH)2 nanocages dropcasted on a carbon paper substrates (a,a’) that were treated with stoichiometric (b) and 20-fold excess (b’) amounts of hydrazine and subsequently electroreduced using four cathodic cyclic voltammetry (CV) cycles (c,c’).
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Figure 7. SEM (a–d) and TEM (e) images of the structures obtained by the reduction of Cu(OH)2 nanocages with excess hydrazine ([N2H4]:[Cu(OH)2] = 5) in methanol.
Figure 7. SEM (a–d) and TEM (e) images of the structures obtained by the reduction of Cu(OH)2 nanocages with excess hydrazine ([N2H4]:[Cu(OH)2] = 5) in methanol.
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MDPI and ACS Style

Medvedeva, X.; Vidyakina, A.; Li, F.; Mereshchenko, A.; Klinkova, A. Reductive and Coordinative Effects of Hydrazine in Structural Transformations of Copper Hydroxide Nanoparticles. Nanomaterials 2019, 9, 1445. https://doi.org/10.3390/nano9101445

AMA Style

Medvedeva X, Vidyakina A, Li F, Mereshchenko A, Klinkova A. Reductive and Coordinative Effects of Hydrazine in Structural Transformations of Copper Hydroxide Nanoparticles. Nanomaterials. 2019; 9(10):1445. https://doi.org/10.3390/nano9101445

Chicago/Turabian Style

Medvedeva, Xenia, Aleksandra Vidyakina, Feng Li, Andrey Mereshchenko, and Anna Klinkova. 2019. "Reductive and Coordinative Effects of Hydrazine in Structural Transformations of Copper Hydroxide Nanoparticles" Nanomaterials 9, no. 10: 1445. https://doi.org/10.3390/nano9101445

APA Style

Medvedeva, X., Vidyakina, A., Li, F., Mereshchenko, A., & Klinkova, A. (2019). Reductive and Coordinative Effects of Hydrazine in Structural Transformations of Copper Hydroxide Nanoparticles. Nanomaterials, 9(10), 1445. https://doi.org/10.3390/nano9101445

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