Sami Barkaouia,
Noureddine Elboughdiri*bc,
Djamel Ghernaoutcd and
Yacine Benguerba
e
aLaboratoire Matériaux Traitement et Analyse, National Research Institute of Physical and Chemical Analysis, Technological Pole Sidi Thabet, 2020 Sidi Thabet, Tunisia. E-mail: samibarkaoui501@gmail.com
bChemical Engineering Process Department, National School of Engineering Gabes, University of Gabes, Gabes 6011, Tunisia. E-mail: ghilaninouri@yahoo.fr
cChemical Engineering Department, College of Engineering, University of Ha'il, PO Box 2440, Ha'il 81441, Saudi Arabia
dChemical Engineering Department, Faculty of Engineering, University of Blida, PO Box 270, Blida 09000, Algeria. E-mail: djamel_andalus@yahoo.fr
eLaboratoire de Biopharmacie et Pharmacotechnie (LBPT), Université Ferhat ABBAS Sétif-1, Sétif, Algeria. E-mail: benguerbayacine@yahoo.fr
First published on 8th July 2024
This review focuses on exploring the intricate relationship between the catalyst particle size and shape on a nanoscale level and how it affects the performance of reactions. Drawing from decades of research, valuable insights have been gained. Intentionally shaping catalyst particles makes exposing a more significant percentage of reactive facets possible, enabling the control of overactive sites. In this study, the effectiveness of Co3O4 nanoparticles (NPs) with nanometric size as a catalyst is examined, with a particular emphasis on the coordination patterns between oxygen and cobalt atoms on the surface of these NPs. Investigating the correlation between the structure and reactivity of the exposed NPs reveals that the form of Co3O4 with nanometric size can be modified to tune its catalytic capabilities finely. Morphology-dependent nanocatalysis is often attributed to the advantageous exposure of reactive crystal facets accumulating numerous active sites. However, experimental evidences highlight the importance of considering the reorganization of NPs throughout their actions and the potential synergistic effects between nearby reactive and less-active aspects. Despite the significant role played by the atomic structure of Co3O4 NPs with nanometric size, limited attention has been given to this aspect due to challenges in high-resolution characterizations. To bridge this gap, this review strongly advocates for a comprehensive understanding of the relationship between the structure and reactivity through real-time observation of individual NPs during the operation. Proposed techniques enable the assessment of dimensions, configuration, and interfacial arrangement, along with the monitoring of structural alterations caused by fluctuating temperature and gaseous conditions. Integrating this live data with spectroscopic methods commonly employed in studying inactive catalysts holds the potential for an enhanced understanding of the fundamental active sites and the dynamic behavior exhibited in catalytic settings.
Cobalt's dual oxidation state takes advantage of surplus electrons during a reaction, demonstrating its adaptability. The spinel crystal structure of Co3O4 contributes to its multifunctional semiconductor properties, and Co3O4 nanoparticles (NPs) exhibit direct optical band gaps, making them suitable for visible light photocatalysis.15,16 Co3O4's varied spin states, such as high, low, and intermediate spin, make it intriguing from a fundamental and spintronic perspective.16 Cobalt's versatility extends to its environmental impact, as demonstrated by Co3O4's ability to oxidize various compounds, including carbon monoxide (CO), volatile organic compounds, sulfur dioxide (SO2), and hydrocarbons. Co3O4 is employed in processes such as three-way catalytic conversion, phenol oxidation, diesel soot oxidation, and clean energy production, such as hydrogen through steam reforming methanol and ethanol.17–20 Additionally, Co3O4 serves as a commercial catalyst in the oxidation, hydrogenation, and hydrogenolysis of esters.21
This review examines recent advancements in the shape engineering of Co3O4 with nanometric size. It focuses on their catalytic performance, which is influenced by the coordination patterns of oxygen and cobalt atoms on their surface. The analysis encompasses progress in this field, exploring the structure–reactivity relationship concerning exposed NPs. The review concludes with a summary and a perspective on future developments, aiming to inform readers about the potential prospects involving Co3O4-based catalysts.
Three different precursor solutions were prepared by dissolving cobalt acetate, cobalt chloride, or cobalt nitrate in distilled water with a concentration of cobalt salt as 0.5 mol L−1.36 The starting solution was aerosolized using an ultrasonic nebulizer (Omron, model NB-150U) with a frequency of 1.75 MHz. The spray pyrolysis temperature was kept at 750 °C. The obtained powders were collected at the reactor exit. The prepared Co3O4 samples from cobalt acetate, cobalt chloride, and cobalt nitrate are denoted as A–Co3O4, C–Co3O4, and N–Co3O4. According to the X-ray diffraction (XRD) data of A–Co3O4, C–Co3O4, and N–Co3O4 samples, all the prepared samples adopted a spinel-type cubic structure. The characteristic diffraction peaks are sharp, and no impurities or a second phase were detected, affirming that high-purity Co3O4 was obtained. Scanning electron microscopy (SEM) was used to examine the shapes of the A–Co3O4, C–Co3O4, and N–Co3O4 samples. For the A–Co3O4 powders, the dimple and wrinkle surface can be observed. C–Co3O4 sample has a porous spherical morphology, and microspheres are developed from various closely packed primary particles; moreover, abundant voids are left among adjacent particles. The N–Co3O4 sample has a durian-like shape with a 0.5–3 μm size distribution, suggesting a hollow inner structure.
For example, cobalt oxalate was used as a precursor for synthesizing Co3O4NRs by thermal decomposition.37 0.6 g of cobalt oxalate and 5 mL oleylamine (as a surfactant) were placed in a 50 mL two-neck distillation flask and heated up to 140 °C for 1 h. The resulting solution was added to 5 g of triphenylphosphine (as a surfactant) at 240 °C. The black solution was maintained under stirring at 240 °C for 45 min and then cooled to room temperature. The final sample was washed with ethanol several times to remove the excessive surfactant. Transmission electron microscopy (TEM) was used to verify the size and shape of the prepared samples. The TEM images of Co3O4NRs demonstrated that the materials had rod-like shapes. The length of NRs was 400–550 nm, and their diameters were about 20 nm.
This method produces high yields, simple to operate, and efficient in terms of being environmentally friendly and energy-consuming. Also, it has been extensively applied to prepare inorganic nanostructured materials49–56 with applications, e.g., electrodes,57 humidity sensors,58 or catalytic devices.52 The method's versatility for synthesizing NPs has been especially reported.59 The microwave-assisted hydrothermal route has been developed to prepare Co3O4 with NRs' shape.40 The method involved two steps: first, NRs of cobalt hydroxide carbonate were prepared by mixing 50 mL of 0.6 M Co(NO3)2·6H2O and 2.4 g of CO(NH2)2 under 500 W microwave irradiated for 3 min. Subsequently, the cobalt hydroxide carbonate NRs were calcined under air at 400 °C for 3 h to fabricate Co3O4NRs. After the thermal decomposition of cobalt hydroxide carbonate precursor under 400 °C for three hours, a single phase of well-crystallized Co3O4 with the cubic structure was obtained, and no peaks of the other phase were detected, indicating that the sample was of high purity. The as-prepared sample was bamboo-like NRs with a diameter varying from 30 to 60 nm and a length of 100 to 1000 nm.
The solvothermal process is similar in its technology to the hydrothermal one, as it is carried out in autoclaves at high temperatures and pressure, through just one difference: instead of water, the synthesis is carried out in organic solvents. Co3O4 nanostructures with different morphologies (NCs, nanowires, nanobundles, nanoplates (NLs), and nanoflowers) have been prepared,38,52 and the experimental details of the preparation of Co3O4 nanostructures with different shapes are summarized in Table 1.
Shape | Cobalt salt (mM) | Temperature (°C) | Reaction time (h) | Structure-directing agents |
---|---|---|---|---|
Nanocubes (NCs) | 2 | 180 | 12 | 15 mL of ammonia (6%) |
Nanowires | 2 | 150 | 5 | 30 mL ethanol (99.9%) and 3 mmol of urea |
Nanobundles | 2 | 120 | 12 | 2 mmol urea |
Nanoplates (NLs) | 2 | 150 | 15 | 3 mL NaOH solution (3.25 mM) with 2 mL ammonia (6%) |
Nanoflowers | 2 | 180 | 12 | 30 mL ethanol and 15 mL ammonia (6%) |
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Fig. 1 Transmission electron microscope (TEM) and high-resolution transmission electron microscope (HRTEM) images of cobalt-based nanostructures: (a, and b) cobalt hydroxide carbonate; (c–f) Co3O4 nanorods (NRs), (c) low-magnification bright-field view, and (d–f) high-resolution views at {110}, {1–10}, and {100}; (g) NR morphological illustration. Catalytic performance of Co3O4: (h) CO conversion efficiency over time for Co3O4 nanoparticles (NPs) and NRs in a continuous-flow reactor at −77 °C; (i) reaction rate (rCO) vs. CO or O2 concentrations for Co3O4 NRs; (j) Arrhenius plots (based on ref. 64, Copyright 2009, Nature Publishing Group). |
In contrast to the spherical NPs, Co3O4 NR demonstrated an approximately one-order-of-magnitude increase in the rate of CO oxidation. At −77 °C, the Co3O4 NR reaction rate was 3.91 × 10−6 molCO g−1 s−1. Conversely, the value of the NPs was just 4.66 × 10−7 molCO g−1 s−1. The high-resolution transmission electron microscope (HRTEM) analysis revealed that the Co3O4 NPs were enclosed by a configuration consisting of eight {111} and six {001} planes. Conversely, the Co3O4 NR preferred to reveal the {110} planes, constituting an estimated 40% of their overall surface area (Fig. 1g). It was found that Co3+ species functioned as active sites for CO oxidation on the {110} plane.
The performance of Co3O4 nanobelts (NBs) and NCs in CO oxidation has been investigated.63 The reaction rate of Co3O4 NC, which mostly exposed the ∼{001} facets, was 0.62 μmol g−1 s−1, as opposed to the 0.85 μmol g−1 s−1 seen on NBs terminated by the {110} plane. The specific conversion rate indicates that at 56 °C, Co3O4 NB exhibits 1.37 times the activity of CO3O4 NCs, demonstrating that the Co3O4 NB are significantly more active than Co3O4 NC. As shown by these studies, the activation of the surface layer lattice oxygen on the {110} planes is more pronounced in the presence of Co3+ species compared to the {001} planes. Furthermore, it was shown that Co3O4 nanowires (NWs) enclosed in {111} planes and measuring around 3 nm in diameter had a notably increased rate of CO oxidation at 248 °C, amounting to 161.75 μmol CO g−1 s−1.61 The enhanced performance resulted from the increased surface area and the profusion of Co3+ cations on the surfaces.
A catalytic study for CO oxidation62 indicates that Co3O4 NR exposed to {111} planes exhibited enhanced activity at an activation energy of 40 kJ mol−1, whereas Co3O4NLs exposed to the same planes had superior activity at a reduced activation energy of 21 kJ mol−1. Significant morphology-dependent effects on CO oxidation have been observed, contradicting prior hypotheses to some degree (maybe due to the porous structures amid cracks and interspaces in the Co3O4 nanostructures). The formation of Co3O4 NS, Co3O4 NB, and Co3O4 NC by hydrothermal synthesis of a cobalt hydroxide precursor followed by direct thermal breakdown was investigated in kinetic experiments for methane (CH4) combustion (Fig. 2a–f).30 The specific rates (rCH4) for Co3O4 NC (343 °C), Co3O4 NB (319 °C), and Co3O4 NS (313 °C) were 1.25, 2.28, and 2.72 μmol g−1, respectively, as shown in Fig. 2g. Additionally, the T50, representing the temperature at which half of the methane conversion occurred, exhibited a decreasing trend in the same sequence. The structural study indicated that the most prevalent planes on Co3O4 NS, Co3O4 NB, and Co3O4 NC were {112}, {110}, and {001}, respectively. Beyond these crystal planes, the methane combustion process persisted in the following order: {112} > {110} {001}. It can be deduced that manipulating the structure of nanostructured cobalt oxides leads to a substantial display of catalytically active sites. This is supported by the enhanced CH4 combustion activity observed in Co3O4 as a nanosheet, which exposes the more reactive {112} planes. The catalytic activity of Co3O4 supported on stainless steel wire mesh, produced by the ammonia evaporation process, was investigated with the preferred oxidation (PROX) of CO.68 The 500 nm-diameter mesoporous Co3O4 nanowires' diameter is 3.4 nm, and they have a Brunauer–Emmett–Teller (BET) surface area of 71 m2 g−1. This structured catalytic system is very stable over the whole temperature range of 100–175 °C due to its low-pressure drop and high heat exchange rate; furthermore, its exceptional catalytic activity is twice that of the highest-performing Co3O4 catalyst previously documented.
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Fig. 2 Scanning electron microscopy (SEM) and high-resolution transmission electron microscope (HRTEM) analysis with structural models of Co3O4 nanostructures: (a and b) Co3O4NS; (c and d) Co3O4NB; (e and f) Co3O4NC. (g) Methane conversion efficiency vs. temperature for Co3O4 at a GHSV of 40![]() |
Although PROX was believed to have an active Co3+ site, its mechanism may have been distinct from the low-temperature oxidation of the CO reaction. Researchers69 stated that the turnover frequency of Co3O4 NC, composed of six 100-facet facets, was 3.5 to 4 times more than that of Co3O4 NS, Co3O4 NB, and Co3O4 NP. Besides reducing Co2+ in hydrogen-rich environments, spectroscopic investigations revealed that Co3O4 NC's bulk and surface Co3+ sites were only modestly stabilized. For selective CO oxidation, the optimum pair Co3+/Co2+ was used. By using a sequence of Co3O4 catalysts, including exposed {111}, {110}, and {100} planes, it was verified that Co3+ functioned as the active site. As shown from the linear relationship between the number of Co3+ surface areas and the quantity of CO2 produced,70 the 100 facets positively impacted the PROX. Analyses of different Co3O4 attributes indicate that the phase and surface characteristics, including shape, surface area, and facets, significantly affect the catalytic activity. As seen in Fig. 3a–l,16 the synthesis of Co3O4, including a variety of Co3O4 NR {110}, Co3O4 NC {100}, and nano-octahedron {111} (NO) facets has been completed. The catalytic reactivity of Co3O4 NR, Co3O4 NC, and Co3O4 NO was the highest for phenol oxidation by the persulfate (PS) process. Fig. 3m and n demonstrated that the Co3O4 NR exhibited the lowest adsorption energy estimated by the density functional theory (DFT). This confirms that PS is more easily activated via a non-radical pathway on the Co3O4 {110} plane.16
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Fig. 3 Morphological and catalytic characteristics of Co3O4 nanostructures: scanning electron microscopy (SEM) and high-resolution transmission electron microscope (HRTEM) images of (a–d) Co3O4NR {110}, (e–h) Co3O4NC {100}, and (i–l) Octahedra {111}; (m) phenol oxidation reaction rates using peroxydisulfate and Co3O4 at pH 11; (n) comparison of rate constants and Brunauer–Emmett–Teller (BET)-normalized rate constants for different Co3O4 facets (adapted from ref. 16, © 2020 Elsevier Ltd). |
To degrade 5-sulfosalicylic acid, four distinct 3D Co3O4 catalysts were fabricated, each with a unique morphology (Fig. 4): Co3O4 NC {111}, Co3O4 NLs {110}, Co3O4 NNs (nanoneedles, {110}), and Co3O4NFs (nanoflowers, {112}).71 Primarily, Co3O4 NF ({112} facets) is the most beneficial 3D Co3O4 catalyst for the oxidation activation to degrade 5-sulfosalicylic acid71 due to its plentiful Co2+ and more reactive surface, in addition to its most excellent surface area (121.1 m2 g−1). The core–shell contrast ratio of the as-prepared Co3S4@Co3O4 core–shell octahedron catalyst via hydrothermal and post-surface lattice anion exchange is comparatively less than that of the other core–shell structures.72 This is because the concentrations of Co3S4 and Co3O4 are close. The hexagonal shape of the selected area electron diffraction pattern, as seen in Fig. 5E, corresponds to both the {111} facet exposure and the close-packed hexagonal pattern observed in the inset of Fig. 5D in HRTEM. The lattice spacing of the {220} pattern is 0.33 nm. As seen in Fig. 5G, electrochemical CO2 reduction reaction (CRR) and oxygen reduction reaction (ORR) were investigated using a core–shell configuration of Co3O4 NO coated with a Co3S4 surface. A distinctive electronic configuration is bestowed by the heterojunction separating the p-type Co3O4 core and the n-type Co3S4 shell, enabling both catalytic processes.
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Fig. 4 Morphological analysis of 3D Co3O4: (A) scanning electron microscopy (SEM) images of (a and b) Co3O4NC, (c and d) Co3O4nanoplates (NLs), (e and f) Co3O4NN, and (g and h) Co3O4NF. (B) Transmission electron microscope (TEM) images with electron diffraction patterns of (a–c) Co3O4NC, (d–f) Co3O4NLs, (g–i) Co3O4NN, and (j–l) Co3O4NF. (C) Comparative analysis of Co3O4 catalysts in oxone activation for 5-sulfosalicylic acid degradation of (a) Co3O4NC, (b) Co3O4NLs, (c) Co3O4NN, and (d) Co3O4NF (adapted from ref. 71, © 2020 Elsevier BV). |
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Fig. 5 Structural and compositional analysis of Co3O4 and Co3S4 nanostructures: (A) FE-scanning electron microscopy (FE-SEM) image of Co3O4NO; (B) Co3S4@Co3O4NO; (C) Co3S4 nanoneedles. (D) Transmission electron microscope (TEM) and high-resolution transmission electron microscope (HRTEM) images of Co3S4@Co3O4. (E) Selected area electron diffraction pattern of Co3S4@Co3O4. (F) EDX elemental mapping of Co3S4@Co3O4. (G) Schematic of heterojunction-assisted Co3S4@Co3O4 for oxygen reduction reaction (ORR) and CO2 reduction reaction (CRR) (adapted from ref. 72, © 2017 WILEY-VCH Verlag GmbH & Co. KGaA, Weinheim). |
To solve the recovery issue and make a reusable, eco-friendly “green” catalyst, the optimum catalyst is Co3O4 with nanometric size attached to a particular substrate with solid adhesion. Chemical (sol–gel), physical (pulsed laser deposition, or PLD), and electrochemical (electroless) methods have been used to create coatings that are reconstructed with Co3O4 with nanometric size. Fig. 6a and b shows that the Co3O4 NPs generated using the PLD approach without post-annealing treatment have a mixed amorphous–nanocrystalline phase, a tiny average size of 18 nm, a narrow size distribution of σ = 3 nm, a perfectly spherical form, and allow a degree of accumulation.73,74
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Fig. 6 Co3O4 catalysts synthesized via various methods and their photocatalytic performance: (a) SEM images of coatings prepared by PLD, (b) particle size distribution histogram for PLD coatings, (c) time-dependent photocatalytic degradation of MB using Co3O4 NPs assembled coating via PLD and cobalt nitrate and (d–g) SEM images respectively of coatings prepared by (d) electroless, (e) electron beam, (f) sol–gel depositions, and powder form; (h) comparative photocatalytic efficiency of powder Co3O4 and coatings by different methods (adapted from ref. 73 and 74 © 2012 Elsevier BV). |
In a methylene blue (MB) solution, the activity of a homogeneous catalyst generating Co2+ ions was compared to that of a thin coating catalyst constructed with heterogeneous Co3O4 with nanometric size. Complete mineralization of MB dye was achieved in 240 min, indicating a far greater degradation rate than the 40% removed by Co2+ ions (Fig. 6c). In the same study, researchers73 found that coatings made of assembled Co3O4 with nanometric size had a slightly lower catalytic activity but still demonstrated good recycling capability. Fig. 6d–g shows that PLD-deposited Co3O4 coatings have the superior photo-degradation rate of MB dye when compared to Co3O4 coatings made using other processes (i.e., electro-beam deposition, sol–gel, and electroless) that have almost equal particle-like morphology (Fig. 6h).
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Fig. 7 Microscopic analysis of 5% Pd-doped Co3O4NS: (a) scanning electron microscopy (SEM), (b) transmission electron microscope (TEM), and (c) high-resolution transmission electron microscope (HRTEM) images highlighting of PdO {002} and 0.466 nm of Co3O4 {111} (reproduced with permission from ref. 75, Copyright 2011, WILEY-VCH Verlag Gmbh& Co). Detailed TEM and scanning transmission electron microscopy (STEM) analysis of Co3O4NR catalysts: (d) TEM, (e) HRTEM, and (f) STEM image of Pt atoms singularly dispersed on Co3O4NR (reproduced with Permission from ref. 77, Copyright; American Chemical Society). |
Due to its low activation barrier of 29.6 kJ mol−1, single Pt atoms attached to Co3O4 demonstrate significant catalytic activity in the water gas shift process at 200 °C (turnover frequency = 0.58 molH2 per sitePt per s). The significantly decreased activation energy observed for these individual Pt atoms may indicate that the interaction between the atoms and the 110-faced Co3O4 NR substantially customized the chemical environment of the active sites (Fig. 7d–f).77
Using straightforward hydrothermal and solvothermal techniques, anion adsorption was employed to deposit gold NPs onto Co3O4 materials produced in various forms, including rods, polyhedra, and cubes.78 Au catalysts based on Co3O4 were characterized using TEM and HRTEM. The predicted morphologies of the Co3O4 supports are cube-shaped, rod-shaped, and polyhedron (NH)-shaped (Fig. 8). Research into the exposed planes of various morphological Co3O4 materials has led to the discovery that the morphology of the support plays a crucial role in determining the catalytic activity. Co3O4 NR shows {110} planes most of the time on HRTEM, whereas the {011} and {001} planes are the most prominent on Co3O4 NH and Co3O4 NC structures, respectively. The {110} plane has the most excellent oxygen vacancies, which are very important for the oxidation of ethylene, in comparison to the {011} and {001} planes. Consequently, the ethylene conversion rate of 93.7% was achieved by Au/Co3O4 NR, demonstrating their exceptional catalytic activity. Ethanol conversion was 85.5% for the Au/Co3O4 NH catalyst. At 0 °C, the ethylene conversion on Au/Co3O4 NC was 26.8%, which was the lowest value recorded.
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Fig. 8 Transmission electron microscope (TEM) images of Co3O4NR (a), Co3O4NH (d), and Co3O4NC (g). High-resolution transmission electron microscope (HRTEM) images of Au/Co3O4NR (b, and c), Au/Co3O4NH (e, and f), and Au/Co3O4NC (h, and i). Source: reprinted with permission from ref. 78, ©2011 Elsevier BV. |
Our prior research79 examined the effect of Co3O4 crystallization on EG oxidation supports in the form of Co3O4 NCs and NLs. As shown in Fig. 9a–c, Au NPs in the Au/Co3O4 NCs samples exhibited a quasi-truncated octahedron structure with Au {111} and {100} faces and had an average size of 2.0 nm. As shown by the interplanar distance of 0.29 nm, corresponding to the {220} crystal plane of cubic Co3O4 oxides, Au NPs are anchored consistently on the Co3O4 {001} facet. Furthermore, the inter-planar spacing of 0.46 nm corresponds to the lattice fringes seen in Au/Co3O4 NL catalysts and is caused by the Co3O4{111} facets of Co3O4 NL oxides. The uniform loading of Au particles onto the Co3O4 {111} facet resulted in the formation of a quasi-truncated octahedron encircled by Au {111} and {100} facets, as seen in Fig. 9d–f. Under these conditions, the Co3O4 NC and Co3O4 NL constituents remained dormant during the aerobic oxidation of EG. With the addition of Au NPs, the catalytic activity of EG oxidation processes was substantially enhanced. Therefore, when subjected to glycol oxidation facilitated by intrinsic defects and surface oxygen vacancies, Au/Co3O4 NL {111} exhibited much greater selectivity and catalytic activity than its Au/Co3O4 NC {001} counterpart (Fig. 9g). One potential catalyst for the oxidation of EG using Au NPs is Co3O4 NL {111}, which facilitates the activation of O2 via the oxygen vacancies on its surface.
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Fig. 9 Scanning transmission electron microscopy (STEM) imaging and catalytic performance of Au-doped Co3O4: (a–c) Au particles on Co3O4 {001} in Au/Co3O4NC; (d–f) Au particles on Co3O4 {111} in Au/Co3O4 nanoparticles (NPs); (g) catalytic efficiency of Au/Co3O4NPs and Au/Co3O4NC in ethylene glycol (EG) oxidation. Reprinted with Permission from ref. 79, 2021 Royal Society of Chemistry. Performance analysis of Co3O4 and Au/Co3O4 in CO oxidation: (h) temperature-dependent catalytic activity for CO oxidation; (i) Arrhenius plots showing rate vs. 1/T for CO oxidation over Au/Co3O4; (j) durability tests at 25 °C and 60 °C with CO conversion rates from 25% to 45%. Reprinted with Permission from ref. 80, 2023 Royal Society of Chemistry. |
Furthermore, the catalysts Au/Co3O4 P were evaluated in the CO oxidation processes.80 The catalytic activity was substantially enhanced by adding Au NPs, as shown in Fig. 9h. This resulted in a noteworthy CO conversion of 35% at 20 °C and complete at 80 °C. As depicted in Fig. 9i, the activation energy (Ea) for CO oxidation in Au/Co3O4 P is 15.49 kJ mol−1. Therefore, oxygen molecules follow the Langmuir–Hinshelwood mechanism, which catalyzes CO oxidation at low temperatures (20–60 °C) via Au/Co3O4 P {111}. In particular, rather than traversing the surface lattice oxygen sites, CO should be adsorbed onto oxygen vacancies at the surface and activated by Au NPs. The durability of the Au/Co3O4 P catalysts was also evaluated at temperatures of 25 and 60 °C (Fig. 9j). Throughout the twelve-hours CO oxidation process at 25 °C, the Au/Co3O4 P catalyst activity decreased from 2.92 to 1.87 molreactedCO gAu−1 s−1. A minimum activity of 5.26–5.39 molreactedCO gAu−1 s−1 was recorded for 9 h at 60 °C. This phenomenon might be primarily attributed to the surface oxygen vacancies and inherent defects of Co3O4 {111}, which activated O2. Similarly, the presence of Au0, Auδ+, and Au+ species on the surface of Au NPs further enhanced the activation of CO.
Contrary to comparable nanostructures, there have been consistent findings on the shape influence of Co3O4 with nanometric size in catalyzing oxidation processes (as shown above). The many reaction routes can contribute, including changing the reaction conditions (primarily the gas and temperature). CO may be oxidized by the Langmuir–Hinshelwood method, which requires surface oxygen species, or the Mars-van Krevelen mechanism, which utilizes lattice oxygen species, according to spectroscopic observations82 and the spectroscopically examined possible reaction pathways/elementary steps of CO oxidation on Co3O4 are configured in Fig. 10, the former exhibited dominance at over 100 °C due to oxygen vacancy formation and the Co3+/Co2+ redox cycle. Conversely, at lower temperatures, the latter demonstrated dominance. One possible reaction mechanism is that CO adsorbs onto Co3+cations and then absorbs oxygen from the surface lattice coordinated to three Co3+ cations. The oxygen vacancy is then filled with oxygen from the gas phase, according to the Mars–van Krevelen mechanism.64
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Fig. 10 Schematic representation of CO oxidation on Co3O4. Reprinted with Permission from ref. 82, 2018 American Chemical Society. |
Spectroscopic evidence is lacking, although an interaction between molecularly adsorbed CO and O–O peroxo species has been postulated by analyzing the impact of pretreatment conditions,65 although no peroxo O–O species were found using in situ Raman spectroscopy.81 According to in situ infrared research, CO adsorbed on Co2+ sites interacted with an oxygen atom bound to a nearby Co3+ cation, and the gas phase oxygen was used to fill the oxygen vacancy.83 Isotopes are vital in the redox Mars–van Krevelen process and are responsible for CO oxidation.84,85
Theoretical investigations into the CO oxidation pathway on Co3O4 have also shown differences.86–89 For instance, a Mars–van Krevelen process involving mostly exposed {110} planes in Co3O4 has been proposed, as shown in Fig. 11.88
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Fig. 11 Three adsorption configurations of CO on Co3O4(110): (a) on O2f; (b) on O3f; (c) on Co. Bond lengths are in angstroms; bond angle are in degrees. Co, green, O, blue, and C, red. Reprinted with Permission from ref. 88, 2011 Royal Society of Chemistry. |
Theoretically, the octahedrally coordinated Co2+ site in CoO90 would be the most active site for the PROX of CO in the hydrogen-rich stream. According to DFT calculations, the generated carbonates should make the {001} facet of Co3O4 less reactive by blocking the surface sites on that facet but not on CoO {001}, as shown in Fig. 12.
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Fig. 12 Potential energy diagrams for (a) the hydrogenation of Co3O4 {001} and (b) the oxidation of CO to CO2 on Co3O4 {001} and CoO {001}. For each transition state (hollow boxes), reaction barriers are given in kJ mol−1. Selected intermediates are shown as a side view along [110], using the following color codes: black (C), blue (Co), red (O), and white (H). Reprinted with Permission from ref. 90, 2019 American Chemical Society. |
Surface and lattice oxygen species interact concurrently in the reaction network, making methane oxidation on Co3O4 catalysts more difficult. There were three distinct temperature/conversion phases in the methane oxidation process, identified by the presence or absence of the adsorbed or lattice oxygen and the catalyst's redox state.91 At temperatures between 300 and 450 °C, the dominating superficial Langmuir–Hinshelwood structure produces a stoichiometric {100} surface on Co3O4 NC with a regular size of around 40–60 nm and with the preferential exposure {100}, as previously shown for CH4 combustion on these particles. At temperatures ranging from 450 to 650 °C, where O2 nearly occupies the oxygen vacancies generated by the emission of CO2 and H2O, the imperfect surface area is delineated by the coexistence of the interfacial (Mars–van Krevelen) and suprafacial (Langmuir–Hinshelwood) mechanisms.92,93 At temperatures over 650 °C and with a non-stoichiometric surface area, the completion of oxygen vacancies is only partial, resulting in a substantial reduction in catalyst activity and the combustion of CH4 via the Mars–van Krevelen technique.91
Theoretical computations have led to the notion that the C–H bond in CH4 would be activated by the doubly coordinated lattice oxygen (O2c) across the {110} surface. Therefore, the {110} surface is expected to exhibit more activity than the {100} surface, devoid of any O2c sites.94 Assuming dissociation of CH4 on the Co–O pair; researchers95 indicated that the reactivity of methane combustion increased as follows: {001} < {011} < {112}. Experimental observation of cubic Co3O4 revealed the less active {001} facet, while flower-shaped Co3O4 exhibited the active {111} facet.96 As compared to spherical NPs enclosed in the {001} and {111} facets or Co3O4 NRs exposed to the {110} and {001} facets, Co3O4 NLs encased in the {112} facet showed higher activity in the CH4 combustion process.97 The surface remodeling during reaction circumstances may contribute to the contradicting findings on the reactive facets. It has been shown by molecular modeling of Co3O4 NPs that the form may be maintained; however, when exposed to oxidizing and reducing atmospheres, the relative ratio of {111}/{100}/{110} facets changes dynamically.98 Under conditions rich in hydrogen gas, the faceting {110} plane was preferentially exposed. At the same time, the {111} surface remained untreated due to the development of oxygen surface vacancies and their subsequent diffusion toward the bulk. Nevertheless, the oxygen-rich conditions promoted the {111} termination. Therefore, it was necessary to describe the shape of the active catalysts. Recent breakthroughs in high-resolution microscopic and spectroscopic methods have opened the door to studying the functions of shaped-synchronized NPs in terms of their dynamic performance. Nitric oxide (NO) may be reduced with CO by reshaping Co3O4 NRs with an exposed {110} surface into non-stoichiometric CoO1−x NR (Fig. 13a and b).99 The structure-modified NRs generate nitrogen gas by selectively reducing nitrogen oxides (NOx) with CO at temperatures ranging from 250 to 520 °C. Environmental transmission electron microscopy (ETEM) and ambient pressure X-ray photoelectron spectroscopy showed that the non-stoichiometric CoO1−x NRs had a rock-salt (RS) structure. The 100% selectivity was brought about by the active phase, which included around 25% oxygen vacancies. Electron transport microscopy measurements in environments rich in hydrogen showed that CO3 was reduced to CO, indicating the formation of a boundary contact for particles larger than 15 nm but not for smaller ones, showing that smaller NPs undergo rapid reduction.100 ETEM identified a two-step phase transition during the heating experiment, as shown in Fig. 13c and d. In the low-temperature range of 200 to 280 °C, the wurtzite (WZ) CoO was spontaneously oxidized to spinel (SP) Co3O4 owing to the residual oxygen in the TEM. Secondly, under low oxygen partial pressure conditions, SP Co3O4 was reduced to RS CoO at temperatures reaching 280 °C.101 These visual results show that the as-prepared oxide NPs changed significantly under response conditions.
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Fig. 13 Structural transformation of Co3O4NR: (a) high-resolution transmission electron microscope (HRTEM) image; (b) schematic illustration of Co3O4 to CoO transformation under reaction conditions; (c) HRTEM image of CoO hexagonal pyramid; (d) illustration of the phase transformation from metastable wurtzite (WZ) CoO to stable rock-salt (RS) CoO via the intermediate spinel (SP) Co3O4. Reprinted with Permission from ref. 90 and 101 Copyrights 2013 and 2019, American Chemical Society. |
The relationship between the catalytic activities of nanometric Co3O4 and the selectively exposed facets induced by shape has been demonstrated through experimental evidence. However, it cannot be ruled out that adjacent facets may work together synergistically. Initially designed nanostructures may undergo structure, morphology, and chemistry changes under actual reaction conditions. The catalytic properties observed in the experiments are determined by the dynamic behavior of the catalyst particles in response to temperature and the reactive environment rather than their state when prepared or recently used. In some instances, the activation of species in a multi-molecule chemical reaction may occur through diffusion on adjacent facets, resulting in a synergistic effect where the species activated by the adsorbed reactant can adsorb and stimulate a different type of reactant. In situ studies, physical and chemical analyses, and dynamic characterization techniques must be employed in operational environments to fully understand functional nanostructures.
To gain a deeper understanding of the relationships within nanostructured catalysts, further exploration is needed to develop improved experimental and theoretical methods.105–107 Variations in temperature and reactive gas fluctuations can impact the well-defined form of Co3O4 nanometric, leading to changes in its electrical and geometric properties. This, in turn, influences the proportion of active surfaces and the coordination environments of oxygen and cobalt atoms on the surface, ultimately affecting the development of active sites. The lack of published studies on the atomic structure of nanometric Co3O4 can be attributed to the limited availability of high-resolution spectroscopic and microscopic characterizations among researchers worldwide. Also, studying active sites' dynamic performance under operational conditions would provide valuable insights into the structure–reactivity relationship. By employing techniques that allow for real-time assessment of size, shape, interfacial structure, and gas-induced structural changes at the active sites of individual nanoparticles, combined with spectroscopic methods, we can significantly enhance our understanding of the inherent active regions and dynamic capabilities of nanostructured catalysts within catalytic environments.
BET | Brunauer–Emmett–Teller |
CRR | CO2 reduction reaction |
DFT | Density functional theory |
EG | Ethylene glycol |
MB | Methylene blue |
NBs | Nanobelts |
NCs | Nanocubes |
NH | Polyhedron |
NLs | Nanoplates |
NPs | Nanoparticles |
NRs | Nanorods |
ORR | Oxygen reduction reaction |
PLD | Pulsed laser deposition |
PS | Persulfate |
PROX | Preferred oxidation |
SEM | Scanning electron microscopy |
TEM | Transmission electron microscopy |
XRD | X-ray diffraction |
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