Vivek Ramakrishnana,
Hyun Kima,
Jucheol Parkb and
Beelyong Yang*a
aSchool of Advanced Materials and System Engineering, Kumoh National of Institute of Technology, Yangho-dong, Gumi-si, Gyeongsangbuk-do, Korea. E-mail: blyang@kumoh.ac.kr
bElectronics& Information Technology Research Institute Gumi, 17 Chomdangieop 1 St. Sandong, Gumi, Gyeongbuk 730-853, Korea
First published on 13th January 2016
Cobalt oxide nanoparticles were sensitized on hydrothermally grown TiO2 nanorods on FTO (fluorine-doped tin oxide) by electrochemical deposition, followed by rapid thermal annealing under air and N2. We investigated the formation of the nanostructure with different electrodeposition times, electrolyte concentrations, and annealing temperatures for improved photoelectrochemical (PEC) properties. A structural investigation showed the formation of a mixture of CoO/Co3O4 oxides dependant on annealing temperature and atmosphere. The oxide formation equilibrium shifted from Co3O4 to a mixture of CoO/Co3O4 and finally to monoxide when temperature is lowered from 700 °C to 350 °C. Improved PEC properties were shown by the mixture of oxides compared to a system with CoO and Co3O4 alone on TiO2. Electrodeposition time was found to have a linear relationship with the nanoparticle size of cobalt oxide formed on TiO2. Here we propose a cost effective and simple method to fabricate a hetero-junction system with improved PEC properties.
In recent years, there have been many reports on efficient semiconductor based photocatalysts.4–8 One of the methods includes the preparation of nanostructures involving more than one type of semiconductor system. A tandem nanostructure consisting of n-type and p-type semiconductors for overall water splitting is always desirable without external bias.9 Achieving this type of multi-junction photoelectrode for overall water splitting is always challenging on the basis of electronic and thermodynamic requirements.10–15 Titanium dioxide (TiO2) based nanostructures have been well studied in the field of photocatalysis. TiO2 nanostructures are preferred because of their chemical stability, low cost, abundance and favourable band edge alignment with water redox potentials, which make them potential candidates as photoanode materials for water oxidation.16–21
Cobalt oxide systems (Co3O4 and CoO) are well studied in the field of photocatalysis. They have got a wide variety of applications as well, such as in heterogeneous catalysis, Li-ion batteries, photocatalysis, solar absorbers and so on. For these applications, Co3O4 has more prominence because of its high chemical stability. The Co3O4 unit cell has a spinel structure and a direct optical band gap of ∼1.5–2 eV in the bulk state. However, the nanoparticles of Co3O4 are reported to have a much larger band gap (∼2.5 eV) with the top level of the valence band and the bottom level of the conduction band being 2.52 V and 0.09 V, respectively, relative to the normal hydrogen electrode (NHE). Compared to this, CoO systems are not widely studied because of their lower stability and difficulty in selective preparation.22–29 The coupling of CoO with TiO2 with specific nanostructures could be a suitable system for overall water splitting. The bottleneck in preparing such types of nanostructures lies in the selective oxidation of cobalt as it has three types of oxide forms which are very sensitive to the formation conditions:30 (1) Co3O4, which has a spinel (a = 8.108 Å) structure with a band gap of 2.07 eV; (2) Co2O3, whose unit cell has a hexagonal structure (a = 4.64 Å, c = 5.750 Å) with no photocatalytic activity reported best to our knowledge; (3) CoO which is face centred cubic (a = 4.22) with both bulk and nanoparticle forms reported to have a band gap of 2.6 eV. There were some attempts already carried out to prepare pure nanoparticle systems of cobalt oxide (CoOx) and TiO2 using a sol–gel method,26 CoO flakes spread over TiO2 nanotubes by cathodic deposition,27 and Co3O4/TiO2 by photodeposition for photocatalytic applications.31 We prepared a system with a specific nanostructure, comprising nanoparticles of cobalt oxide uniformly anchored even on a dense substrate and a selective form of oxide, utilising simple and cost effective instrumentation.
Our group have been actively studying nanostructured semiconductor systems for photocatalytic applications.32–35 In this work, we have systematically investigated the preparation, microstructure, selective oxide formation, and photoelectrochemical properties of a hetero-junction cobalt oxide/TiO2 system (Fig. 1). Using a two-step process, cobalt oxide nanoparticles were engineered on TiO2 nanorods which subsequently showed improvement in visible light sensitization attributed to the band gap of CoO and Co3O4.
The morphology and microstructural characterizations of the nanostructured samples were performed using a field emission scanning electron microscope (FE-SEM, JSM-6500 F, JEOL), a field emission transmission electron microscope (FETEM, 200 kV/JEM-ARM200F, JEOL), and an X-ray diffractometer (XRD, SWXD, Rigaku). EELS spectra were taken on a STEM (JEM-ARM200F, JEOL) at 200 kV with a spherical aberration (Cs) corrector and Gatan image filter (GIF Quantum ER, Gatan). Electrochemical measurements were carried out using a potentiostat (AMT VERSASTAT 3, Princeton Applied Research) with a three electrode configuration consisting of a platinum (Pt) wire counter electrode and a saturated Ag/AgCl reference electrode in a 0.1 M Na2S (pH ∼ 12.5) electrolyte. A working electrode with a 1 cm2 area was illuminated using a 1 kW xenon lamp (Newport) with its infrared wavelengths filtered out by water, and wavelengths below 420 nm removed by an optical filter, enabling measurements under visible light. The light irradiance, measured by a thermopile detector, was 100 mW cm−2.
Chemical and crystal structures were further confirmed by XRD analysis. To get a clear cut idea about the characteristic peaks of cobalt oxide (JCPDS#01-070-2855, JCPDS#01-074-1656), the peaks due to the TiO2 nanorods and FTO are shown in Fig. 3 (JCPDS#01-070-7347). XRD analysis of the TiO2 nanorods shown in Fig. 3 reveals that the nanorods are single-crystalline with a tetragonal rutile structure growing predominantly in the (002) direction. In the XRD analysis, the diffraction peak of TiO2 (002) is prominent among diffraction peaks corresponding to TiO2. From Fig. 3 we can clearly see that the cobalt deposited was oxidised, leading to the formation of both CoO and Co3O4 (electrodeposition for 60 seconds, at −0.5 V, annealed at 500 °C in air). The (200) and (311) planes in the XRD pattern are assigned to the cubic phase of CoO and Co3O4. The formation of a mixture of cobalt oxides is quite expected in our system, as the annealing temperature is below 1000 °C. Above 1000 °C, all oxides of cobalt will be converted to CoO.
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Fig. 3 Comparison of the XRD peaks of the FTO substrate, TiO2 nanorods on FTO and cobalt oxide on TiO2 nanorod/FTO annealed at 500 °C in air. |
TEM analysis of cobalt oxide nanoparticles on TiO2 nanorods, which were electrodeposited as a function of time, was carried out (ESI Fig. SI 3†) under the same conditions as in the SEM analysis. Nanoparticles anchored on nanorods are quite obvious from the images in Fig. 2. The size of the nanoparticles was found to vary between 5 and 15 nm in diameter. SAED patterns of both cobalt oxide and TiO2 nanoparticles were determined, the (220) and (200) planes corresponding to Co3O4 and CoO respectively. The existence of (100) and (200) planes corresponding to TiO2 were observed. From the lattice-fringe analysis, shown in Fig. SI 3,† the (220) plane confirmed the presence of Co3O4, and the (200) plane further confirmed the presence of CoO. By comparing with standard data (JCPDS#01-070-2855, JCPDS#01-074-1656), the nanoparticles formed on the nanorods of TiO2 were further confirmed to be a mixture of both CoO and Co3O4.
As described earlier, both the SEM and TEM analyses clearly showed that the electrodeposition time was found to have a crucial role in the size of the cobalt oxide nanoparticles. The particle size of cobalt oxide, irrespective of the nature of the oxide, was averaged and is shown in Fig. 4 schematically. Detailed information is shown in the ESI (Fig. SI 3†). We can see that there is a linear relation between the electrodeposition time and particle size. As is expected when oxidized, the average size of the particle was also found to be increased. The linearity in the relationship of the electrodeposition time was found to be applicable for the cobalt oxide nanoparticle density as well (Fig. 4). Particle density was calculated over a specific area for nanoparticles anchored on TiO2 nanorods (200 × 200 nm2). Nanoparticle size and density have significant importance in photocatalytic semiconductor systems. It is reported that the band gap of cobalt oxide has a large dependence on particle size. Bao et al., showed that microcrystalline CoO can be potentially made active for overall water splitting just by changing the particle size. The band position was shifted ∼1.5 eV with the band gap remaining to be almost the same (2.6 eV). In our system the particle size may not have a crucial influence on the photocatalytic activity as we use a p–n hetero-junction system which already causes Fermi level alignment leading to a shift in band positions.25
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Fig. 4 Relation between particle size and particle density with respect to the electrodeposition time of cobalt and its oxide formed on TiO2 nanorods with and without annealing at 500 °C in air. |
RTA | CoO | Co3O4 | ||
---|---|---|---|---|
Air | N2 | Air | N2 | |
350 °C | ✓ | ✓ | ✗ | ✗ |
375 °C | ✓ | ✓ | ✓ | ✗ |
400 °C | ✓ | ✓ | ✓ | ✓ |
500 °C | ✓ | ✓ | ✓ | ✓ |
600 °C | ✗ | ✓ | ✓ | ✓ |
700 °C | ✗ | ✗ | ✓ | ✓ |
The formation of a mixture of cobalt oxide nanoparticles on TiO2 nanostructures was further confirmed by EELS spectra (ESI SI 2†). Cobalt oxide was characterized by the shape and position of the O-K edge at 532 eV and Co-L peak at 779 eV.36 The data obtained in the EELS measurements was very well matched to the TEM results. In the case of the sample annealed at 500 °C, mixtures of oxides of cobalt were formed. This was confirmed by the splitting of the peak at 532 eV into two, which is characteristic of Co3O4. The peak at 565 eV corresponds to cobalt monoxide. In addition, the ratio of intensity of Co-L peaks (L2 and L3) showed the presence of a mixture of oxides having the values of ∼4.9 and ∼2.9 which correspond to CoO and Co3O4 respectively. At the same time, the sample prepared at 600 °C annealed in air was found to contain a monotonic L2/L3 intensity ratio of ∼3.0 corresponding to Co3O4.
In addition, we have also tried to investigate the effect of the concentration of the electrodeposition solution on the photocatalytic activity. We found that lowering the concentration of the electrodeposition solution resulted in improved PEC properties. We varied the concentration from 60 mM to 4 mM. This clearly shows that the amount of nanoparticles formed on the nanostructure has a saturation limit. Large amounts of nanoparticles lead to a decrease in the photocurrent with poor p–n junction formation plausibly due to steric factors.
A schematic representation of the hetero-junction formed in our case is depicted in Fig. 1c. Since we anchored the nanoparticles of cobalt oxide on TiO2, both were in contact with the electrolyte solution and upon light irradiation electron–hole pairs were formed in both semiconductors. As previously described, photogenerated electrons move from the conduction band of cobalt oxide to that of TiO2 and then to the FTO substrate, finally reaching the metallic counter electrode. Hole movement occurs in the reverse direction. Direct evidence for the formation of an effective hetero-junction is shown in Fig. 7. Transient times of the TiO2 nanorods with and without cobalt oxide nanoparticles were measured to comparatively investigate the recombination rates. Transient changes in the photocurrents as a function of elapsed time were measured by irradiating with pulsed light (on and off). Charge carrier lifetimes were calculated by relating the following standard equations:32
D = [I(t) − I(f)]/[I(i) − I(f)] | (1) |
D = exp(−t/τ) | (2) |
Footnote |
† Electronic supplementary information (ESI) available. See DOI: 10.1039/c5ra23200g |
This journal is © The Royal Society of Chemistry 2016 |