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Article

Exploration of Copper Oxide Nanoneedle Electrosynthesis Applied in the Degradation of Methylene Blue

by
Diego P. Oyarzún
1,*,
Alejandra Tello
1,
Julio Sánchez
2,
Andrés Boulett
2,
Omar E. Linarez Pérez
3,
Rudy Martin-Trasanco
4,
Guadalupe del C. Pizarro
4,
Marcos Flores
5 and
César Zúñiga
6,*
1
Departamento de Química y Biología, Facultad de Ciencias Naturales, Universidad de Atacama, Copayapu 485, Copiapó 1531772, Chile
2
Departamento de Ciencias del Ambiente, Facultad de Química y Biología, Universidad de Santiago de Chile (USACH), Santiago 9170022, Chile
3
Instituto de Investigaciones en Fisicoquímica de Córdoba (INFIQC), Universidad Nacional de Córdoba, Córdoba 5000, Argentina
4
Departamento de Química, Universidad Tecnológica Metropolitana, Avda. Las Palmeras 3360, Santiago 7810000, Chile
5
Laboratorio de Superficies y Nanomateriales, Facultad de Física y Ciencias Matemáticas, Universidad de Chile, Beauchef 850, Santiago 8370448, Chile
6
Instituto de Ciencias Naturales, Facultad de Medicina Veterinaria y Agronomía, Universidad de Las Americas, Manuel Montt 948, Santiago 7500975, Chile
*
Authors to whom correspondence should be addressed.
Nanomaterials 2021, 11(11), 2994; https://doi.org/10.3390/nano11112994
Submission received: 28 August 2021 / Revised: 14 October 2021 / Accepted: 2 November 2021 / Published: 8 November 2021
(This article belongs to the Section Environmental Nanoscience and Nanotechnology)
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Abstract

:
In this study, we report a low cost, fast and unexplored electrochemical synthesis strategy of copper oxide nanoneedles films as well as their morphological and chemical characterization. The nanostructured films were prepared using electrochemical anodization in alkaline electrolyte solutions of ethylene glycol, water and fluoride ions. The film morphology shows nanoneedle-shaped structures, with lengths up to 1–2 μm; meanwhile, high-resolution X-ray photoelectron spectroscopy (HRXPS) and spectroscopy Raman analyses indicate that a mixture of Cu(II) and Cu(I) oxides, or only Cu(I) oxide, is obtained as the percentage of water in the electrolyte solution decreases. A preliminary study was also carried out for the photocatalytic degradation of the methylene blue (MB) dye under irradiation with simulated sunlight in the presence of the nanoneedles obtained, presenting a maximum degradation value of 88% of MB and, thus, demonstrating the potential characteristics of the material investigated in the degradation of organic dyes.

Graphical Abstract

1. Introduction

The obtention of the nanostructures of different materials has been a subject of increasing interest in the last decade due to their novel physicochemical properties that allow their application in fields such as medicine, acoustics, optoelectronics, photonics, sensors and electrocatalysts [1,2,3,4]. Commonly, nanostructures can be present in various geometries such as wires, rods, points, pores and tubes, among others [4,5].
In addition, nanomaterials produce interesting physical phenomena such as photoluminescence, which make them attractive for the manufacture of electronic devices. The high surface area of these materials could improve the performance of luminescent modules, piezoelectric transducers, semiconductor electrodes, chemical sensors and electrocatalysts [2,5,6]. The most studied nanostructures in the last few years correspond to carbon nanotubes [6], titanium dioxide nanotubes [7] and copper oxides nanostructures [8,9,10]. Among them, copper oxide-based nanomaterials attract attention due to its non-toxic nature, low cost and their low bandgap values of 1.2 to 1.8 eV and 1.8 to 2.5 eV for CuO and Cu2O, respectively [11]. Additionally, their conduction and valence bands are close to the water reduction and oxidation potentials, respectively, thus allowing the oxide film to produce hydrogen by direct water photolysis without the need for the application of an external potential. These properties make CuO and Cu2O very promising materials for use in converters of solar energy into electrical energy through the design of CuO-based solar cells [12,13] as well as in water photolysis. However, the absorption profile of CuO is rather weak in most of the visible range [14], which implies that if an electrode formed by a smooth CuO film is subjected to solar irradiation, a significant part of the photogenerated charge carriers within the material are lost in recombination processes [15,16]. Nevertheless, as has been demonstrated for other materials such as GaP and SiC [17,18], the use of electrodes composed of nanostructured CuO or Cu2O films, could solve this problem. For nanoporous structures, the charge carriers are photogenerated at a small distance from the semiconductor/electrolyte interface, which, in turn, promotes the separation of charge carriers more efficiently [18], while light absorption is reinforced through dispersion [17].
Currently, several methods for obtaining copper oxide-based nanostructures have been widely reported in the literature. In this, the thermal oxidation of metallic copper at high temperatures stands out [19,20], the growth assisted by templates [21,22], the use of colloidal methods [23,24] and using electrochemical anodization techniques. However, high-temperature processes generally limit the control over the interfacial characteristics of copper oxides thin films, which significantly affect their optical and photoelectrochemical properties [25]. Furthermore, the use of templates and routes of colloidal synthesis are generally characterized by obtaining copper oxides that have a low adhesion on the conductive substrates, which limits their use or integration in electronic devices. Conversely, electrochemical anodization is a surface treatment process that has been successfully used to synthesize a wide variety of nanostructures using various metal substrates, such as titanium, zinc, thallium and copper [26,27,28,29,30,31], and employing these films in various applications [32,33,34,35,36]. In particular, the preparation of copper oxide films by anodizing the metallic copper used as a substrate is also the source of the copper ions that are subsequently oxidized by the presence of water molecules composing the electrolyte solution and the voltage applied to the medium [37]. In this context, various morphologies of anodized copper oxide nanostructures, such as nanoneedles, nanorods, nanopores, nanowires and nanoparticles, have been reported [38]. Among these reported morphologies, nanowires stand out due to their high surface area, which increases the reactivity area of the material [13,31]; this offers potential advantages for their integration in electronic devices since they have a much more efficient electrical contact with the metal [13,31], for biomaterial applications or as a non-toxic photocatalyst, low cost and easy to obtain, for the photodegradation of organic molecules, such as dyes and wastewater pollutants [13,31]. Although it has been reported to obtain copper oxide nanoneedles by anodization using an electrolytic medium composed of KOH [31,39,40,41], in no case has an ethylene glycol-based electrolyte medium been used in conjunction with fluoride ions [11,31,39,40,41,42,43]. Tello et al., during 2021, have reported that an electrolytic medium based on the mentioned chemical compounds benefit the morphological order of anodized nanostructures, due to the high viscosity of the solvent and the interference generated by the fluoride ions on the surface of the copper layer during anodization [13,31]. In addition, only one of these studies has used the anodization technique without subsequent heat treatment to dehydrate the Cu(OH)2 nanoneedles to CuO [41].
Effluents from the textile, plastic and paper industries contain colorants such as methylene blue (MB) [44], which is a well-known toxic, mutagenic and carcinogenic dye. For this reason, its elimination from wastewater is essential to minimize the effects on aquatic life and the associated problems. In this regard, many conventional methods have been developed for the removal of dyes from wastewater, such as ozonation, liquid–liquid extraction, photodegradation, precipitation, membrane filtration, ion exchange, coagulation and adsorption [45]. However, the advantage of photodegradation compared to these techniques and others used to degrade dyes, such as degradation by algae, enzymes, metal nanoparticles and electrochemistry, is that solar energy is used to produce the reaction that will degrade the dye, which significantly reduces operating costs [46]. To perform the photocatalytic process, a semiconductor material with bandgap energy values Eg < 4 eV is used, which favors the excitation of its valence electrons (VB) toward the conduction band (CB) by means of a light energy source [47].
In this work, we report an unexplored electrochemical strategy synthesis of CuO/Cu2O nanoneedles films as well as their chemical and morphological characterization. The anodization was performed in alkaline electrolyte mixtures of ethylene glycol, water and fluoride ions. The film characterization was performed by means of Raman spectroscopy, field emission scanning electron microscopy (FESEM), atomic force microscopy (AFM), transmission electron microscopy (TEM) and HRXPS. Additionally, the previously obtained copper oxide nanostructures were used to perform a study of the photocatalytic degradation of MB in aqueous solution.

2. Materials and Methods

Copper anodization was performed in an electrochemical cell with a two-electrode configuration. The anode electrodes consisted of polycrystalline copper foils (Sigma Aldrich (Spruce Street, LA, USA), 99.99% purity) of 250 μm in thickness (0.5 cm2 of exposed geometric area) mounted in Teflon holders. A 0.5-centimeter-thick carbon sponge of 3.0 × 3.5 cm2 was used as a cathode electrode. Prior to anodization, the samples were mechanically polished using a 0.05-micrometer alumina aqueous suspension and then, degreased by sonication in a 50:50% acetone/ethanol mixture for 15 min. After cleaning, the foils were rinsed with deionized water and dried under N2 flux. The anodization was carried out at 5 °C by applying a voltage of 10 using a high-power source, for 180 s. The electrolyte solution was prepared from analytical grade reagents and was based on ethylene glycol + [0.5; 10]% v/v water, 0.1 M NaOH or 0.1 M KOH and 0.1% w/v NH4F Merck (Darmstadt, Germany).
The morphology features of the nanostructured layers were characterized by FE-SEM using a Carl Zeiss Sigma microscope (Oberkochen, Germany). Raman experiments were performed ex situ (in air) using a Horiba LabRAM HR spectrometer (Sunnyvale, CA, USA), employing a He/Ne laser (632.8 nm wavelength). Using an XPS-Auger Perkin Elmer Model PHI 1257 spectrometer (Waltham, MA, USA) was employed to determine the chemical composition of samples, by means of HRXPS and using the method described previously [48,49,50]. For AFM measurements, a Nanonics Multi View MV1000 was employed using n-type silicon cantilevers (tip radius ≈ 20 nm; f = 39.4 kHz; Q = 1576) for the intermittent mode. TEM was performed using LEO 1420VP equipment (Oberkochen, Germany). Prior to the TEM measurements, a dispersion of copper oxide nanoneedles was obtained by sonication during 15 min of the oxide films in isopropyl alcohol. The analysis of images was performed with the image processing software Gwyddion 2.37. The photocatalytic activity was carried out using a 1000 W Xe/Hg lamp (Oriel 6295) as a simulation of a source of sunlight. In order to avoid the overheating of the MB solution, the infrared radiation was eliminated through a water filter. The copper oxide nanoneedles were immersed in a quartz cell containing 15 mL of a 2.5 mM dye solution. In order to reach the adsorption equilibrium, the samples were held one hour in the dark with permanent air bubbling for also assuring dissolved oxygen saturation at the beginning of the photocatalytic degradation process. The experiments were performed in triplicate for 120 min, and the dye concentration measurements were taken at λmax = 660 nm every 30 min in comparison to a previously recorded calibration curve.

3. Results and Discussion

Figure 1a shows the j/t potentiostatic profile applying a constant potential of 10 V during 3 min in a 0.1 M KOH + 10%v/v H2O + 0.1%w/v NH4F dissolved in ethylene glycol solution. After an abrupt initial current density increase, the current profile shows a rapid diminution in current density within the first milliseconds and then a slight variation from around 5 to 3 mA/cm2 for the subsequent 3 min due to the passivation of the copper surface [51]. The presence of ethylene glycol and hydroxyl ions in the electrolytic medium may stabilize the current density during the anodization due to its density and polarity as well as the alkaline pH employed [13,31]. On the other hand, the Raman spectrum for the anodized copper foil (see Figure 1b) shows typical intense signals at around 284 and 335 cm−1, indicating the presence of CuO species [52,53]. Additionally, signals at 150, 545.6 and 625.6 cm−1, which are characteristic of Cu2O, are obtained. It should be mentioned that these signals are less intense than those for CuO, which would indicate a low presence of Cu (I) on the surface of the copper foil [52].
Additionally, the chemical analysis performed using XPS measurements indicates the presence of a Cu2O/CuO oxides mixture in the anodized surfaces [37,54]. The high resolution Cu2p spectrum (see Figure 2a) shows important contributions at a binding of 932.2 and 933.9 eV; these signals are attributed to Cu + Cu2O, CuO and [49], for the case of the Cu-Auger signal, the Cu + CuO and Cu2O contributions are identified at binding energy of 567.0 and 569.3 eV, respectively (see Figure 2b). Additionally, high resolution O1s spectrum (see Figure 2c) evidences the presence of both CuO and Cu2O oxides as well as hydrated species in the sample, which are in agreement with the above showed Raman results. Such hydrated species are also identified in the Cu2p main signal at 936.2 eV in binding energy.
Table 1 shows a summary of the results obtained from the XPS measurements; from these values and by using the formulation of Platzman, we estimate the percent for each copper oxidation state [50]. It can be observed that the formation of Cu(I) species predominates in electrode surfaces (46%) after the synthesis process. However, the minor proportion of oxidized Cu(II) species (22%) may be attributed to an excessive amount of H2O in the electrolytic bath as well as the high voltage applied during the anodization, given also a high amount of hydrated species, 25%. A small amount of metallic copper (6%) was identified. From the values of this table, the alpha parameter can be determined, which is independent of charge effects, alpha = KE(LMM) + BE(2p) = 917.3 eV + 932.2 eV = 1849.5 eV and 917.3 eV + 933.9 eV = 1851.2 eV. These values are in agree with the literature [55], and in the Wagner plot, can be labeled as Cu2O and CuO, respectively.
In order to study the morphology of the obtained films, several microcopy techniques were employed. Figure 3a,b show a top view FESEM micrography of the CuO/Cu2O film obtained, which shows a highly homogeneous self-assembled nanoneedles array. The main length of the needles is between ca. 1 and 2 µm. A more detailed study morphology was performed using TEM measurements of a CuO/Cu2O nanoneedles dispersion (see Figure 3c). Long and thin structures with lengths ranging between 200 and 500 nm corresponding to the entire and fragmented nanoneedles are observed (see Figure 3c and inset). In addition, Figure 3d shows a 3D AFM image for the anodic films obtained, showing a similar morphology as those obtained from FESEM (see Figure 3a,b).
On the other hand, by decreasing the percentage of water in the electrolyte solution below 10%v/v during anodization, CuO/Cu2O or Cu2O nanoneedles are obtained on a flake surface and the nanoneedles have a smaller average length as the percentage of water decreases. The Raman spectra of the nanoneedles obtained using 5%v/v water in their synthesis show signals at 146.2, 540.3 and 621.4 cm−1, which are characteristic of Cu2O, together with the signals at 286.7 and 345.5 cm−1, which further indicate the presence of CuO in the sample (see Figure 4) [37,52,53,56], whereas, when further reducing the percentage of water in the synthesis, only characteristic signals for the presence of Cu2O in the samples are observed [57]. The formation of these nanostructures is explained by the basic medium in which it is found, since the presence of OH−, H2O and ethylene glycol ions tend to the formation of CuO nanostructures from metallic copper (Equation (1)) [38,40,56]. Moreover, the presence of fluoride ions tends to the redissolution of the CuO previously obtained and the subsequent formation of Cu2O (Equations (2) and (3)). Finally, a higher presence of hydroxyl ions when using higher percentages of water again produces CuO from the previously formed Cu2O, obtaining a mixture of copper (I) and (II) oxides (Equation (4)) [40,50]. On the other hand, the FESEM images obtained show a highly rough surface made up of a thin film of nanoneedles with diameters apparently below 100 nm. The homogeneity and chemical composition of the synthesized material varies according to the increase in the quantity of water in the electrolytic medium, showing an apparent length diminishing as the water content augments (see Figure 4I–IV). Figure 5 shows a summary diagram of the morphology, diameter and chemical composition of the copper oxide nanostructures obtained as a function of the percentage of water used in their respective anodizations.
Cu(s) + 2OH−(aq) → CuO(s) + H2O(l) + 2e−
Cu(sup) + F−(aq) → Cu-F(ad) + e−
2Cu-F(ad) + 2OH−(aq) → Cu2O(s) + H2O(l)+ 2F−
Cu2O(s) + 2OH−(aq) → 2CuO(s) + H2O(l) +2e−
Based on the discussion of the figures above, it can be deduced that during anodization, a layer of Cu2O flakes is generated on the surface of the copper foil, and Cu2O or Cu2O/CuO nanowires start to emerge on them, depending on the percentage of water used in the synthesis (see Figure 5). This interface, generated between the flakes adhered to the anode surface and the nanowires, allows the nanowires to reach longer lengths as the percentage of water in the synthesis increases [31,37,39,40,41].
The photocatalytic activity was evaluated by performing a preliminary study (without adjusting the conditions, such as the amount of xerogel, solution pH, dye concentration and volume) on the degradation of the MB dye, evaluating as a function of the simulated solar irradiation time of CuO/Cu2O nanoneedles obtained by anodization with 10 or 3.0%v/v water in the electrolyte solution during their synthesis, and Cu2O nanoneedles obtained by anodization with 1.0% water in the electrolyte solution during their synthesis (see Figure 6a). It is observed that the photocatalytic activity of the CuO/Cu2O nanoneedles photocatalysts reaches maximum values of 88 and 82% for the syntheses with 10 and 5% water, respectively; while, for the Cu2O nanoneedles obtained with 1% water, in the synthesis it reaches a maximum value of 74%, which indicates that the photocatalytic activity of the materials decreases as a function of the percentage of water used during the synthesis of each photocatalyst, that is, the photocatalytic activity of CuO/Cu2O nanoneedles is higher than that of Cu2O. This is attributed to the chemical nature of the photocatalyst, since upon irradiation with solar energy (Equation (5)), the electrons (e−) and holes (h+) generated in the CuO/Cu2O heterojunction network have a longer lifetime than those of a Cu2O photocatalyst, because the VB and CB of CuO have a lower energy level than the VB and CB of Cu2O, respectively, generating a transfer of photoinduced e− from the CB of Cu2O to that of CuO and h+ from the VB of CuO to that of Cu2O and, in turn, increasing the lifetime of the promoted electrons and the photocatalytic activity of the material (see Figure 6b) [11]. Subsequently, these e−/h+ pairs can react with water molecules in the vicinity of the semiconductor, generating reductive reactions between the promoted electrons and the O2 in the water, producing superoxide (O2−•) (Equations (6) and (7)) and hydroxyl (OH•) radicals (Equation (8)), and oxidative reactions between the holes formed and the OH− coming from the water (Equation (9)) or with the water molecules themselves (Equation (10)), also producing hydroxyl (OH•) radicals [11]. In addition, it has been reported in the scientific literature that the Eg values for Cu2O/CuO nanostructures estimated from their UV–Vis absorbance spectra are between 1.5 and 1.9 eV [11], while, for Cu2O, it reaches values of between 1.8 and 2.5 eV, i.e., a higher amount of energy is needed to photoinduce e− from VB to CB in a semiconductor composed of Cu2O than in a semiconductor composed of a mixture of copper oxides, which also justifies the lower photocatalytic activity obtained for the Cu2O nanoneedles [11].
On the other hand, when comparing the photocatalytic activity at lower irradiation times, it is observed that the percentage of MB degradation for the Cu2O/CuO nanoneedles obtained with 10% water during the synthesis is lower than those obtained with 5% water during the synthesis, which is attributed to the fact that the photoinduced e− and h+ generated in the Cu2O/CuO nanoneedles obtained with 10% water have a longer lifetime, but need a longer interaction time between the photocatalyst and the dye to present a significantly higher photocatalytic activity [11].
Semiconductor + hv > Eg → e−(VB) + h+(CB)
e− + O2 → O2−•
2O2−• + 2H+ → H2O2 + O2
H2O2 + e− + H+ → H2O + OH•
h+ + OH− → OH•
h+ + H2O → H+ + OH•
The structural decomposition of MB is mainly caused by the effect of the hydroxyl radicals generated between the reactions of the water molecules with the e− and mainly the h+ generated in the photocatalyst. It has been reported that the first thing that is detached from the MB molecules during degradation are the methyl groups attached to the amine group; subsequently, several unstable intermediates are formed with minimum existence periods, until obtaining compounds less complex than the dye, such as SO42−, NO3−, Cl−, NH4+ and mainly H2O and CO2 [58]. The level of the highest energy occupied molecular orbital (HOMO) and the lowest energy unoccupied molecular orbital (LUMO) of MB have values of 4.25 and 6.11 eV, respectively. MB, when irradiated with an energy higher than 6.11 eV (1.48 × 1015 Hz), causes an electron to be promoted from the HOMO to the LUMO, leading to the breaking of a bond and the subsequent degradation of MB [59]. The simulated sunlight used fulfills this characteristic, as it is mainly composed of infrared, visible and, to a lesser extent, UV light (7.5 × 1014—3 × 1015 Hz), producing a synergistic effect between the degradation of MB due to the UV light portion (approximately 5% of the sunlight) and the free radicals generated in the semiconductor during photodegradation [58]. In repeated photocatalytic degradation tests, the recycling stability of the copper oxide nanoneedles was evaluated for the synthesized system under the experimental conditions of 10 V, 3 min, 10% H2O (see Figure 6c). After each repeated cycle, the Cu2O/CuO nanostructures were filtered, washed rigorously several times and dried. After five cycles of experiments, the photocatalytic activity of the material continues to show a high degradation index, demonstrating the high stability of this type of copper oxides nanostructures over time, in addition to having all the attributes of reusable materials, to promote sustainable development.
As mentioned above, in this study a maximum photocatalytic activity of 86% was achieved in the degradation of MB using Cu2O/CuO nanowires and solar energy. This obtained value is lower than the values previously reported in the scientific literature for various photocatalysts composed of mixtures of metal oxides photo exposed with visible light (see Table 2) [60,61,62,63]. These are attributed to the formation of a heterojunction network between the VB and CB of the metal oxides of different chemical nature, which benefits the lifetime of the photogenerated reactive species [60,61,62,63]. Specifically, Li et al., in 2021, reported the highest photocatalytic activity for MB degradation (99%) using a Cu2O/Ag/TiO2/polyacrylonitrile nanofiber composite system; however, when studying the material composed only of Cu2O nanoparticles stabilized on polyacrylonitrile nanofibers (Cu2O/NFs-PAN), a photocatalytic activity of only 60% was reported, which is lower than those obtained in this study [63]. While comparing the materials studied in this research with the standard P25 TiO2 degussa applied in the photodegradation of MB, higher or equal photocatalytic activity values were obtained in the preliminary study carried out with anodized Cu2O/CuO nanowires, which shows that this material presents potential characteristics to be applied in the photodegradation of organic dyes [43]. On the other hand, the application of CuO nanowires in the photodegradation of various dyes, such as methyl orange (MO), direct red 81 (DR) and victoria blue (VB), have been reported [31,39,40,41,42]. However, these photocatalysts have been obtained by solution chemistry in basic media or by anodization with an electrolytic medium of only KOH [31,39,40,41], and in no case has an electrolytic medium based on ethylene glycol together with fluoride ions been used [11,31,39,40,41,42,43]. The electrolytic medium benefits the morphological order of the anodized nanostructures due to the high viscosity of the solvent and the interference generated by the fluoride ions on the surface of the copper layer during anodization [13,31].

4. Conclusions

Based on the results obtained in this research, we conclude that it is possible to synthesize CuO and/or Cu2O nanostructures (nanoneedles) using a very simple, one-step and low-cost method. The anodization of copper electrodes in a hydroxyl containing aqueous electrolytic medium, unlike other known methods for the formation of CuO or Cu2O nanostructures, does not require special electrolytes, chemicals or surfactants. The chemical characterization of the samples showed that nanowires of Cu2O or CuO/Cu2O are obtained depending on the conditions of synthesis carried out; in addition, it was determined that nanowires are up to 1–2 μm in length. In the photocatalytic degradation of the methylene blue dye (MB) in the presence of the prepared copper oxide nanostructures, an 88% degradation of MB was obtained for the optimal morphologies. The photocatalytic activity of the material continues to show a high rate of degradation after five cycles of photodegradation, demonstrating the high stability of copper oxide nanostructures over time and the fundamental characteristics of reusable materials. These results are promising for the application of these types of nanostructured copper oxide films for designing new electronic devices with an easy-to-obtain and non-toxic photocatalyst for the photodegradation of organic molecules, such methylene blue dye.

Author Contributions

Conceptualization, A.T.; methodology, software, A.B.; validation, R.M.-T. and D.P.O.; formal analysis, M.F.; investigation, D.P.O.; resources, J.S.; data curation, J.S.; writing—original draft preparation, O.E.L.P.; writing—review and editing, C.Z. and D.P.O.; visualization, C.Z.; supervision, G.d.C.P.; project administration, funding acquisition, D.P.O. All authors have read and agreed to the published version of the manuscript.

Funding

The authors are grateful for support from the PAI77200065 project and Fondecyt 1191336 and the financial assistance by the fund Scientific and Technological Equipment, year 2019 code LE19-01, Universidad Tecnológica Metropolitana (UTEM). Microscopy facilities at LAMARX, FAMAF-UNC/CONICET, Sistema Nacional de Microscopía—MINCyT, are gratefully acknowledged. RAMAN equipment at LANN, INFIQC-UNC/CONICET. OLP thanks the financial support from Project PUE-2017 CONICET #22920170100092, PICT2019-2545 and SECYT-UNC.

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

Data available on request.

Conflicts of Interest

The authors declare no conflict of interest.

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Nanomaterials 11 02994 g001 550
Figure 1. j/t potentiostatic profile (a) and Raman spectrum (b) for Cu foils anodized at 5 °C applying constant potential of 10 V during 3 min in a 0.1 M KOH + 10%v/v H2O + 0.1%w/v NH4F electrolyte and dissolved in ethylene glycol.
Figure 1. j/t potentiostatic profile (a) and Raman spectrum (b) for Cu foils anodized at 5 °C applying constant potential of 10 V during 3 min in a 0.1 M KOH + 10%v/v H2O + 0.1%w/v NH4F electrolyte and dissolved in ethylene glycol.
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Nanomaterials 11 02994 g002 550
Figure 2. HRXPS spectra of (a) Cu-2p, (b) Cu-Auger and (c) O-1s, for Cu foils anodized at 5 °C applying constant potential of 10 V during 3 min in a 0.1 M KOH + 10%v/v H2O electrolyte + 0.1%w/v NH4F and dissolved in ethylene glycol.
Figure 2. HRXPS spectra of (a) Cu-2p, (b) Cu-Auger and (c) O-1s, for Cu foils anodized at 5 °C applying constant potential of 10 V during 3 min in a 0.1 M KOH + 10%v/v H2O electrolyte + 0.1%w/v NH4F and dissolved in ethylene glycol.
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Nanomaterials 11 02994 g003 550
Figure 3. Morphology of anodic CuO/Cu2O nanoneedles obtained for Cu foils anodized at 5 °C applying a constant potential of 10 V during 3 min in a 0.1 M KOH + 10%v/v H2O electrolyte + 0.1%w/v NH4F and dissolved in ethylene glycol film obtained by means of (a) and (b) FESEM, (c) TEM and (d) AFM.
Figure 3. Morphology of anodic CuO/Cu2O nanoneedles obtained for Cu foils anodized at 5 °C applying a constant potential of 10 V during 3 min in a 0.1 M KOH + 10%v/v H2O electrolyte + 0.1%w/v NH4F and dissolved in ethylene glycol film obtained by means of (a) and (b) FESEM, (c) TEM and (d) AFM.
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Nanomaterials 11 02994 g004 550
Figure 4. Raman spectra and FESEM images (I–IV) of copper oxides nanoneedles synthesized by electrochemical anodization at 10 V, for 3 min and 5 °C, using X%v/v H2O (I = 5.0, II = 1.5, III = 1.0, IV = 0.5) + 0.1 M NaOH + 0.1%w/v NH4F, dissolved in ethylene glycol.
Figure 4. Raman spectra and FESEM images (I–IV) of copper oxides nanoneedles synthesized by electrochemical anodization at 10 V, for 3 min and 5 °C, using X%v/v H2O (I = 5.0, II = 1.5, III = 1.0, IV = 0.5) + 0.1 M NaOH + 0.1%w/v NH4F, dissolved in ethylene glycol.
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Nanomaterials 11 02994 g005 550
Figure 5. Schematic diagram of the morphology, diameter and chemical composition of the copper oxide nanostructures obtained as a function of the percentage of water used in their respective anodizations.
Figure 5. Schematic diagram of the morphology, diameter and chemical composition of the copper oxide nanostructures obtained as a function of the percentage of water used in their respective anodizations.
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Nanomaterials 11 02994 g006 550
Figure 6. (a) Percentage of methylene blue (2.5 mM of MB with 0.001 g/15 mL of CuO/Cu2O nanoneedles) degradation as a function of illumination time for different copper oxides nanostructures. (b) photodegradation diagram of MB with CuO/Cu2O and (c) recycling histogram after five cycles of MB degradation.
Figure 6. (a) Percentage of methylene blue (2.5 mM of MB with 0.001 g/15 mL of CuO/Cu2O nanoneedles) degradation as a function of illumination time for different copper oxides nanostructures. (b) photodegradation diagram of MB with CuO/Cu2O and (c) recycling histogram after five cycles of MB degradation.
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Table
Table 1. Cu-2p and O-1s data table of XPS spectra, for Cu foils anodized at 5 °C applying a constant potential of 10 V during 3 min in a 0.1 M KOH + 10%v/v H2O electrolyte and dissolved in ethylene glycol.
Table 1. Cu-2p and O-1s data table of XPS spectra, for Cu foils anodized at 5 °C applying a constant potential of 10 V during 3 min in a 0.1 M KOH + 10%v/v H2O electrolyte and dissolved in ethylene glycol.
Cu-2p3/2
Chemical CompositioneVArea%At Conc
Cu + Cu2O932.2251,54842
CuO933.9104,50318
Cu(OH)2936.2120,91120
Cu-Auger
Chemical CompositioneVArea%At Conc
Cu + CuO567.048,45614
Cu2O569.3103,02531
O-1s
Chemical CompositioneVArea%At Conc
OH + Cu(OH)2529.617,55616
Cu2O + CuO531.030,61528
H2O532.561,58956
Table
Table 2. Comparison of copper oxide nanoneedles with other metal oxide based photocatalysts previously reported in the scientific literature, their applications and their photocatalytic activity in dye degradation.
Table 2. Comparison of copper oxide nanoneedles with other metal oxide based photocatalysts previously reported in the scientific literature, their applications and their photocatalytic activity in dye degradation.
OxidesCopper Oxide MorphologyCopper Oxide Synthesis TypeComposition of the Electrolyte SolutionApplicationLight SourceDegradation (%)DyeRefs.
Fe2O3/Cu2ONanoparticlesHydrothermal--PhotocatalysisVisible light90MB[60]
Cu2O/Ag/TiO293MB[61]
Cu2O/Ag/TiO2electrodepositionCu(NO3)2 + NaOH + lactic acid98MB[62]
Cu2O/Ag/TiO2/NFs PANElectrospinning--99MB[63]
Cu2O/NFs PAN60MB[63]
P25-TiO2 (commercial standard)----UV light81MB[43]
CuONanoneedlesSolution chemistry in basic media95DR and VB[42]
Cu2O/CuOChemical-thermal oxidationVisible light80MB[11]
CuOAnodization and thermal treatmentKOHAnticorrosive surface------[39]
CuOAnodization and thermal treatmentKOH--[31]
Cu2OAnodizationKOH[40]
CuOKOHPhotocatalisisVisible light93MO[41]
Cu2O/CuOKOH + 10% H2O + NH4F + ethylene glycolSunlight88MBThis study
Cu2O/CuONaOH + 5% H2O + NH4F + ethylene glycol82MBThis study
Cu2ONaOH + 1% H2O + NH4F + ethylene glycol74MBThis study
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Oyarzún, D.P.; Tello, A.; Sánchez, J.; Boulett, A.; Linarez Pérez, O.E.; Martin-Trasanco, R.; Pizarro, G.d.C.; Flores, M.; Zúñiga, C. Exploration of Copper Oxide Nanoneedle Electrosynthesis Applied in the Degradation of Methylene Blue. Nanomaterials 2021, 11, 2994. https://doi.org/10.3390/nano11112994

AMA Style

Oyarzún DP, Tello A, Sánchez J, Boulett A, Linarez Pérez OE, Martin-Trasanco R, Pizarro GdC, Flores M, Zúñiga C. Exploration of Copper Oxide Nanoneedle Electrosynthesis Applied in the Degradation of Methylene Blue. Nanomaterials. 2021; 11(11):2994. https://doi.org/10.3390/nano11112994

Chicago/Turabian Style

Oyarzún, Diego P., Alejandra Tello, Julio Sánchez, Andrés Boulett, Omar E. Linarez Pérez, Rudy Martin-Trasanco, Guadalupe del C. Pizarro, Marcos Flores, and César Zúñiga. 2021. "Exploration of Copper Oxide Nanoneedle Electrosynthesis Applied in the Degradation of Methylene Blue" Nanomaterials 11, no. 11: 2994. https://doi.org/10.3390/nano11112994

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