Dual Transduction of H2O2 Detection Using ZnO/Laser-Induced Graphene Composites

Zinc oxide (ZnO)/laser-induced graphene (LIG) composites were prepared by mixing ZnO, grown by laser-assisted flow deposition, with LIG produced by laser irradiation of a polyimide, both in ambient conditions. Different ZnO:LIG ratios were used to infer the effect of this combination on the overall composite behavior. The optical properties, assessed by photoluminescence (PL), showed an intensity increase of the excitonic-related recombination with increasing LIG amounts, along with a reduction in the visible emission band. Charge-transfer processes between the two materials are proposed to justify these variations. Cyclic voltammetry (CV) and electrochemical impedance spectroscopy evidenced increased electron transfer kinetics and an electrochemically active area with the amount of LIG incorporated in the composites. As the composites were designed to be used as transducer platforms in biosensing devices, their ability to detect and quantify hydrogen peroxide (H2O2) was assessed by both PL and CV analysis. The results demonstrated that both methods can be employed for sensing, displaying slightly distinct operation ranges that allow extending the detection range by combining both transduction approaches. Moreover, limits of detection as low as 0.11 mM were calculated in a tested concentration range from 0.8 to 32.7 mM, in line with the values required for their potential application in biosensors.


Introduction
Zinc oxide (ZnO) is a well-known wide bandgap material (E g~3 .3 eV at 300 K [1]) that prevails as one of the most explored semiconductor metal oxides nowadays [2][3][4][5][6][7]. Indeed, ZnO properties remain extremely appealing for several technological applications, namely its piezoelectricity, high-energy radiation stability, non-toxicity, biocompatibility, improved electrical and optical responses as well as the ability to be grown by simple and low-cost techniques, enabling the production of numerous and tailored morphologies [1,2,5,8,9]. From the point of view of the optical emission properties, one major advantage is its large free-exciton binding energy (60 meV), which allows the observation of excitonicrelated emissions even above room temperature (RT). On the other hand, carbon materials, especially graphene and its derivatives such as graphene oxide (GO) and reduced GO (rGO), have received considerable attention due to their unique physicochemical properties. Among these, one can highlight the large surface area, mechanical properties, acceptable biocompatibility, excellent thermal and electrical conductivity (except for GO), and increased safety and ease of production in comparison to other carbon-based nanomaterials [10][11][12].

Materials' Preparation
The ZnO/LIG composites were prepared by a multi-step approach, in which the two components were synthesized separately and then mixed in the desired ratios. To do so, LIG was produced by direct laser scribing on a polyimide sheet (Kapton ® , HN500, DuPont, Wilmington, Delaware, DE, USA) using a continuous wave (cw) CO 2 laser (Redsail M500, Jinan, Shandong Province, China) with a wavelength of 10.6 µm, a maximum power output of 50 W, and a beam diameter of~100 µm. This process relies on a photothermal process that is induced by the highly localized temperatures (T > 2500 • C) attained by the focused laser beam [43]. As this process takes place, there is a breakage of the carbonyl groups, accompanied by a release in gases as CO, H 2 , N 2 , CO 2 , and even CH 4 [67,68], followed by the rearrangement of the aromatic compounds to produce few-layer graphene nanostructures, whose oxidation is minimized by the presence of a plasma formed by the expelled gases [43,69]. The protruded and highly porous structure is mostly due to the release of these gases [70]. The laser processing conditions were chosen as follows: (i) power output of~12 W; (ii) scan speed of 250 mm s −1 ; (iii) distance between scanning lines of 0.075 mm; and (iv) distance to focus of 1.8 mm (slightly defocused conditions). These parameters were selected according to previous work from our group [51,54]. The as-prepared LIG was then carefully scraped from the polyimide substrate with the aid of a razor blade, resulting in a fine powder (see a schematic representation in Figure 1).
Chemosensors 2021, 9, x FOR PEER REVIEW 4 of 30 power output of 50 W, and a beam diameter of ~100 µ m. This process relies on a photothermal process that is induced by the highly localized temperatures (T > 2500 °C) attained by the focused laser beam [43]. As this process takes place, there is a breakage of the carbonyl groups, accompanied by a release in gases as CO, H2, N2, CO2, and even CH4 [67,68], followed by the rearrangement of the aromatic compounds to produce few-layer graphene nanostructures, whose oxidation is minimized by the presence of a plasma formed by the expelled gases [43,69]. The protruded and highly porous structure is mostly due to the release of these gases [70]. The laser processing conditions were chosen as follows: (i) power output of ~12 W; (ii) scan speed of 250 mm s −1 ; (iii) distance between scanning lines of 0.075 mm; and (iv) distance to focus of 1.8 mm (slightly defocused conditions). These parameters were selected according to previous work from our group [51,54]. The as-prepared LIG was then carefully scraped from the polyimide substrate with the aid of a razor blade, resulting in a fine powder (see a schematic representation in Figure 1). ZnO was produced by laser-assisted flow deposition, whose detailed description can be found elsewhere [71][72][73]. In brief, LAFD is a technique based on a thermal evaporation process that uses a highly focused CO2 laser ( 200 W, Spectron Laser Corp, Azusa, CA, USA) as the heating source. This laser is coupled to a reflective optical setup that creates ZnO was produced by laser-assisted flow deposition, whose detailed description can be found elsewhere [71][72][73]. In brief, LAFD is a technique based on a thermal evaporation process that uses a highly focused CO 2 laser (200 W, Spectron Laser Corp, Azusa, CA, USA) as the heating source. This laser is coupled to a reflective optical setup that creates a circular crown-shaped laser incidence on top of the ZnO precursor rod, previously prepared by a cold extrusion procedure from a mixture of commercial ZnO powder (99.7%, AnalaR, VWR Chemicals, Radnor, PE, USA) and polyvinyl alcohol (0.1 g mL −1 in aqueous solution, Merck, Darmstadt, Germany), resulting in cylindrical-shaped precursor rods that are attached to motors that enable axial and rotational motion. Then, the laser beam hits the top of the precursor, promoting its thermal decomposition and leading to the formation of a vapor composed of the ZnO atomic components, which reacts with each other again (as well as with the oxygen present in the atmosphere), forming the new ZnO micro/nanocrystals [71,74,75]. In the here reported ZnO, the growth was carried out in air and a laser power of 60 W was chosen since it allows the formation of mostly tetrapodal morphologies at a high deposition rate [71]. The selection of such morphology was motivated by their high yield of production as well as their branching geometry, which provides a large surface area that is extremely beneficial for sensing purposes. Table S1 in the Supplementary Materials (SM) file summarizes the growth/synthesis condition for both materials.
For the preparation of the composites, 1 and 5 mg of scraped LIG were mixed with 50 mg of ZnO, respectively. This approach has the advantage of allowing for the control of the weight ratio of both components that comprise the composite, unlike previously reported ones [54]. The weighted powders were mixed with organic compounds, ethylcellulose (Sigma-Aldrich, Munich, Germany), terpineol (C 10 H 18 O, Sigma-Aldrich, Munich, Germany), and ethanol (absolute, analytical reagent grade, Fisher Chemical, Pittsburgh, PE, USA) to form a viscous paste for subsequent deposition into the desired substrates. The mixture was kept under magnetic stirring for 15 min, followed by an ultrasonic bath for 30 min, and another 15 min under magnetic stirring to obtain a homogeneous paste, which was then deposited on fluorine-doped tin oxide (FTO)-coated glass substrates. The paste was deposited in a 5 mm diameter circular area with the aid of a polymeric mask, assuring that the same area and thickness were kept constant for all samples. After deposition, the samples were subjected to a thermal treatment in air (10 min at 100 • C, followed by 30 min at 400 • C, with a heating rate of 5 • C min −1 ) to thermally release the organic compounds present in the deposition paste and to increase the adhesion of the ZnO to the substrate [6,74]. ZnO samples (without LIG), as well as scraped LIG, were also prepared under the same conditions to act as reference samples and to compare their properties with those of the composites. Figure 1 displays a schematic representation of all steps involved in the preparation of these composites, while Figure S1 (supplementary materials), in SM, shows images of the samples obtained after the thermal annealing treatment. Hereafter, the ZnO (without LIG), ZnO mixed with 1 mg and 5 mg of LIG samples deposited on the FTO-coated glass substrates, will be named ZnO, ZnO-LIG1, and ZnO-LIG5, respectively, for simplicity.

Material Characterization
The morphology of the samples was studied by scanning electron microscopy (SEM) using a TESCAN Vega3 SBH SEM microscope (TESCAN, Libušina, Czech Republic). The crystalline structure was assessed by micro-Raman at RT in backscattering configuration on a Horiba Jobin Yvon HR800 spectrometer (Horiba Scientific, Kyoto, Japan) equipped with a 600 grooves mm −1 grating, under the incidence of a 442 nm laser line of a He-Cd laser (Kimmon IK Series, Fukushima, Japan), and focused with an objective of ×50 magnification.
The optical properties of the samples were evaluated at RT by steady-state PL and PL excitation (PLE) spectroscopy in a Fluorolog-3 Horiba Scientific setup with a double additive grating Gemini 180 monochromator (1200 grooves mm −1 and 2 × 180 mm) in the excitation and a triple grating iHR550 spectrometer in the emission (1200 grooves mm −1 and 550 mm). A 450 W Xe lamp was used as the excitation source. The PLE was measured by setting the detection monochromator at the maxima of the emission that one wanted to probe and emission intensity was registered as the excitation was scanned to higher energies. Moreover, the samples were also placed on a cold finger He cryostat, allowing them to cool down to 14 K. The samples were then probed under the excitation of the 325 nm (~3.81 eV, which corresponds to the ZnO above bandgap excitation) line Chemosensors 2021, 9, 102 6 of 29 of a cw He-Cd laser (power density I 0 < 0.6 W cm −2 , Kimmon IK Series, Fukushima, Japan), and the luminescence radiation was dispersed by a SPEX 1704 monochromator (1 m, 1200 grooves mm −1 ) and detected with a cooled Hamamatsu R928 photomultiplier. Their PL signal was assessed from 14 K to RT. In this case, the experiments were carried out under a 90 • geometry and both the optical alignment and the probed region were kept fixed during the whole temperature-dependence study to enable proper comparison between the absolute intensity and spectral shape throughout the entire temperature range.
The electrochemical analysis was conducted by CV and electrochemical impedance spectroscopy (EIS) using a Versastat 3 electrochemical station (Princeton Applied Research, Princeton, NJ, USA) equipped with a homemade three-electrode configuration setup, where the prepared samples acted as the working electrode, a platinum wire was used as counter electrode and Ag/AgCl (1 M KCl) as the reference one. CV was performed either using a physiological solution (PS) as the electrolyte or using 10 mM of ferrocyanide (potassium hexacyanoferrate (II) trihydrate, K 4 [Fe(CN) 6 ]·3H 2 O, from Merck, Darmstadt, Germany) prepared in PS. The PS was prepared by dissolving 8.006 g of NaCl (Sigma-Aldrich, Munich, Germany) and 2.012 g of KCl (Sigma-Aldrich, Munich, Germany) in 1 L of deionized (DI) water. DI water was obtained from a MilliQ water purification system (resistivity of 18.2 MΩ cm). The electrolyte solution was stirred and bubbled with N 2 for 30 min. The heterogeneous electron transfer rate constants (k 0 ) were derived from cyclic voltammograms using the Nicholson method [76,77]. A dimensionless kinetic parameter Ψ is obtainable by [78] where v is the potential scan rate and ∆E p is the potential difference between the voltammograms anodic and cathodic peaks. The k 0 value is calculated through the slope of the following relation (for a single electron, n = 1, transfer reaction) [76,77]: where F is the Faraday constant (96,485.33 C mol −1 ); R is the universal gas constant (8.314 J mol −1 K −1 ); T is the absolute temperature (298.15 K); and D is the diffusion coefficient for ferri/ferrocyanide in aqueous solutions (6.66 × 10 −6 cm 2 s −1 [79]). The faradaic electrochemically active area (A eff , cm 2 ) was obtained from the [Fe(CN) 6 ] 4− anodic branches in CV via the Randles-Ševčík relation (at 25 • C and for n = 1) [76], where i p is the peak current (A) and C is the [Fe(CN) 6 ] 4− concentration in mM (10 mM).
In the case of the EIS measurements, the electrolyte consisted of a mixture of 5 mM of ferrocyanide and 5 mM of ferricyanide (potassium hexacyanoferrate(III), K 3 [Fe(CN) 6 ], from Merck) in PS. Measurements were performed within the 10 kHz to 1 Hz range, with a logarithmic distribution of 20 points per decade and applying a 10 mV AC perturbation upon the open circuit potential (0.21 V vs. Ag/AgCl). Equivalent circuit models were assembled via Gamry's E-Chem Analyst software (Gamry Instruments, Warminster, PE, USA) and fittings were performed using the built-in Levenberg-Marquart algorithm.

H 2 O 2 Sensing
Both the PL and electrochemical signals were studied in the presence of H 2 O 2 to evaluate the adequacy of the here produced composites to detect this compound and be used as transducer platforms in biosensing devices. The experimental setups used are depicted in Figure S2 in SM. In the case of the PL experiments, the samples deposited on FTO-coated glass substrates were fixed on the cold finger of the He cryostat and immersed in a quartz cuvette filled with H 2 O 2 solutions (diluted using PS) with different concentrations of 0. 9, 1.8, 4.4, 8.7, 17.0, and 32.7 mM. It is worth mentioning that these concentrations were selected since it is the range of interest for glucose detection, which is typically found to be 40-500 mg dL −1 (2.2-27.8 mM). During the tests, the cuvette support was fixed to an elevator table that only allowed vertical motion ( Figure S2a), thus enabling the removal of the cuvette after recording the signal for each solution without changing the sample position and the optical alignment. All experiments were carried out under the same conditions described above for the characterization measurements. The signal was first assessed when the samples were immersed in PS. As the intensity of the PL spectra was seen to be influenced by immersion time, several spectra were acquired until signal stabilization was attained (measurements conducted up to 3 h). After that, the last recorded spectrum was considered as the reference/blank (0 mM of H 2 O 2 ). Then, the samples were placed in the solution with the lowest H 2 O 2 concentration and the signal was collected after~5 min of immersion under UV radiation as the signal monitored at the maximum of the UV emission was rather stable after that time. After the acquisition, the sample was placed again in PS for~5 min (without irradiation) to stop the reaction with the H 2 O 2 . This procedure was adopted for each solution with increasing concentration.
In the case of the electrochemical assessment ( Figure S2b), the H 2 O 2 detection tests were carried out by acquiring the voltammogram of ZnO and ZnO/LIG composites samples using PS as the electrolyte (35 mL) at a potential range from −1 to 1 V and a scan rate of 100 mV s −1 . In this case, a saturated calomel electrode (SCE, 3.9 M KCl) was used as the reference electrode. Before the H 2 O 2 detection tests, cyclic voltammograms were run in the presence and absence of O 2 (bubbled with N 2 during 30 min and kept under N 2 blanket). The latter was used as the reference/blank (0 mM of H 2 O 2 ) for each sample. Then, different volumes of H 2 O 2 (3% v/v) were added to the electrolyte under magnetic stirring and with a N 2 flow to rapidly homogenize the electrolyte solution and to guarantee no entrance of O 2 in the cell. The magnetic stirring and N 2 flow were turned off and the voltammogram was run. This procedure was repeated in increasing order of concentration by adding 30, 60, 150, 300, 600, and 1200 µL, which corresponded to final H 2 O 2 concentrations of 0.8, 1.5, 3.8, 7.4, 14.6, and 28.3 mM, respectively.

Morphological and Structural Analysis
The prepared samples of the ZnO and ZnO/LIG composites, as well as the assynthesized and scrapped LIG, were analyzed by SEM and the results are depicted in Figure 2. As reported in previous works [49,51,54], the as-synthesized LIG exhibited a 3D foam-like morphology (Figure 2a), with a great number of pores with a large size distribution from hundreds of nanometers to tens of micrometers, resulting from the liberation of the gases produced during the photothermal process that leads to the LIG formation [43,53,70]. The pores were distributed through all the LIG volume. In fact, smaller pores were found inside the larger ones (see inset in Figure 2a), promoting a high surface area of the carbon material. However, upon scraping from the polyimide substrate to be mixed with ZnO, this foam-like appearance was completely lost, as can be observed in Figure 2b and c, where SEM images of the scrapped LIG in powder form and after deposition on the substrate are displayed, respectively. In these cases, a crumpled morphology was observed rather than the previous foam-like one.
crystal, whose length varied from hundreds of nm to a few µ m, while the diameters were on the nm scale, as previously reported for this type of ZnO morphology produced by LAFD [6,71]. LIG was not clearly distinguished in the SEM images of the composites because at the employed accelerating voltages, 30 kV, the beam penetration depth was much larger than the graphene sheet thicknesses, hindering its visualization against the denser and thicker ZnO. Nevertheless, as corroborated by the Raman spectra presented in Figure  3, LIG was indeed present in these samples and homogeneously distributed throughout the entire composite.  Figure 3 shows the Raman spectra of the prepared ZnO/LIG composites. The ZnO and LIG samples deposited under the same conditions of the composites and an as-synthesized LIG sample were also analyzed for comparison purposes. Both LIG samples exhibited typical D and G bands associated with sp 2 coordinated carbon, as well as a symmetrical 2D band characteristic of graphene materials [46,50,54,80]. While the D band (~1372 cm −1 ) was attributed to the presence of defects and/or disordered carbon, the G band (~1583 cm −1 ), which dominated the present LIG spectra, was a common feature of graphitic-like materials and was associated with the bond stretching of all C-C pairs of sp 2 atoms [80]. On the other hand, the 2D band originated from second-order zone-boundary phonons, in particular, overtones of the D band [50,80,81], and the fact that a single and symmetric peak appeared reflects the formation of a decoupled multilayer graphene structure [46,54]. Inspection of the two spectra presented for the LIG samples revealed that the scraping process led to changes in the ratio between the peak intensity of both D Regarding the ZnO and its composites with LIG, the SEM images are presented in Figure 2d-f. In all cases, the ZnO tetrapod morphology dominated the samples, as can be better seen in the inset images. Indeed, this occurred even in the case of the composite with the highest amount of LIG (5 mg, Figure 2f), although the sample exhibited a dark grey color (see photograph in Figure S1). These tetrapods were composed of four needlelike branches connected at the center. Each of these branches corresponded to a single crystal, whose length varied from hundreds of nm to a few µm, while the diameters were on the nm scale, as previously reported for this type of ZnO morphology produced by LAFD [6,71]. LIG was not clearly distinguished in the SEM images of the composites because at the employed accelerating voltages, 30 kV, the beam penetration depth was much larger than the graphene sheet thicknesses, hindering its visualization against the denser and thicker ZnO. Nevertheless, as corroborated by the Raman spectra presented in Figure 3, LIG was indeed present in these samples and homogeneously distributed throughout the entire composite. Figure 3 shows the Raman spectra of the prepared ZnO/LIG composites. The ZnO and LIG samples deposited under the same conditions of the composites and an as-synthesized LIG sample were also analyzed for comparison purposes. Both LIG samples exhibited typical D and G bands associated with sp 2 coordinated carbon, as well as a symmetrical 2D band characteristic of graphene materials [46,50,54,80]. While the D band (~1372 cm −1 ) was attributed to the presence of defects and/or disordered carbon, the G band (~1583 cm −1 ), which dominated the present LIG spectra, was a common feature of graphitic-like materials and was associated with the bond stretching of all C-C pairs of sp 2 atoms [80]. On the other hand, the 2D band originated from second-order zone-boundary phonons, in particular, overtones of the D band [50,80,81], and the fact that a single and symmetric peak appeared reflects the formation of a decoupled multilayer graphene structure [46,54]. Inspection of the two spectra presented for the LIG samples revealed that the scraping process led to changes in the ratio between the peak intensity of both D and G bands and 2D vs. G (i.e., I D /I G and I 2D /I G , respectively), as well as in the width of those vibrational modes. For the as-synthesized LIG, I D /I G~0 .14 and I 2D /I G~0 .38, while for the scrapped samples, the ratio I D /I G increased to~0.37 and the I 2D /I G slightly decreased to~0. 22. This change in phonon intensity ratio was also accompanied by a broadening of the peaks for the scrapped LIG, mostly associated with an increase in the disorder of the structure. Indeed, such results were expected since the as-synthesized LIG foam-like structure collapsed during the scraping process, thus producing a higher defect concentration, for instance, due to an increase in the density of edges (as seen in the SEM images in Figure 2b,c) and/or from a higher oxidation state [14,50]. Besides the damage induced during the removal of LIG from the original polyimide substrate, such defects can also be promoted during mixing, deposition, and thermal treatment steps. Moreover, as this treatment was performed in air, some oxidation may have been promoted in this way. Hence, all of these processes are likely to play a significant role in the enhancement of the defect density.

Photoluminescence Assessment
The ZnO and ZnO/LIG samples were assessed by RT PL and PLE and the results are displayed in Figure 4. Figure 4a shows a comparison of the absolute PL intensity for the analyzed samples (probed with the same illumination area and alignment). As can be seen, all spectra were dominated by the near band edge (NBE) emission, peaked at ~378 nm (~3.28 eV), and by a broad visible band with its maximum in the green spectral region (GL), as typically observed for the tetrapodal ZnO produced by LAFD [15,71,74]. At RT, the NBE emission resulted from the overlap of the free exciton (FX) emission with some defect states that are often present in this spectral region, as is the case of previously reported surface-related defects [15,75,84]. This evidence is corroborated by the low and temperature-dependent PL data depicted in Figure 5 and Figure S3, respectively. Never- In the case of the ZnO sample, the spectrum resembled those often observed for highly crystalline ZnO, displaying well defined and sharp peaks that corresponded to the typical vibrational modes of the hexagonal wurtzite structure that are active in Raman, in line with the ones typically displayed by the LAFD produced ZnO [6,72]. The modes A 1 , E 1 , and E 2 were clearly identified, as well as some overtones and combined modes related to multiphonon processes [82]. Specifically, the observed first-order Raman phonon modes (at k = 0) were the A 1 (TO), which peaked at~386 cm −1 , the E 2 high placed at~442 cm −1 , A 1 (LO) at~556 cm −1 , and E 1 (LO) at~585 cm −1 . Finally, the peaks related to the second-order processes corresponded to the combined modes E 2 high -E 2 low placed at~336 cm −1 and the intense peak at~1143 cm −1 due to the 2A 1 (LO) and 2E 1 (LO), which was enhanced under the present excitation conditions [83]. A combination of both LIG and ZnO vibrational modes was seen in the case of the composite samples, according to what was observed for the components individually. Three spectra are presented in Figure 3 for each composite, corresponding to different probed spots, to infer the homogeneity of the deposited material. The fact that modes for ZnO/LIG could be observed throughout the probed regions of the samples demonstrated that the two components were uniformly mixed and that the samples were fairly homogenous. The main difference observed between the two ZnO/LIG composites was the relative intensity of the LIG-related modes when compared to the ZnO ones. This intensity was higher in the case of the composites with 5 mg, as a higher amount of LIG was present, thus having a more significant contribution to the overall spectra. Another relevant point to highlight is that the ratio I D /I G increased again when the LIG was mixed with ZnO, presenting values in the ranges of~0.56-0.73 and~0.42-0.63 for the samples with 1 mg and 5 mg, respectively. Such enhancement suggests that a higher surface disorder is promoted and that the presence of ZnO may induce additional effects.

Photoluminescence Assessment
The ZnO and ZnO/LIG samples were assessed by RT PL and PLE and the results are displayed in Figure 4. Figure 4a shows a comparison of the absolute PL intensity for the analyzed samples (probed with the same illumination area and alignment). As can be seen, all spectra were dominated by the near band edge (NBE) emission, peaked at 378 nm (~3.28 eV), and by a broad visible band with its maximum in the green spectral region (GL), as typically observed for the tetrapodal ZnO produced by LAFD [15,71,74]. At RT, the NBE emission resulted from the overlap of the free exciton (FX) emission with some defect states that are often present in this spectral region, as is the case of previously reported surface-related defects [15,75,84]. This evidence is corroborated by the low and temperature-dependent PL data depicted in Figure 5 and Figure S3, respectively. Nevertheless, the observed peak position coincided with the one typically reported for the FX recombination at RT [1,73], pointing toward its dominant contribution in the present case. The GL is one of the most reported emission for ZnO and it has been widely discussed in the literature, particularly because countless defects have been associated with the recombination channels in this spectral region, namely impurities such as Cu [85], or intrinsic defects, like oxygen vacancies, and many others [1,86,87]. Additionally, in the case of the samples at the nanoscale, which present a high aspect ratio, there has been convincing evidence that the defects (or at least part of them) that contribute to the green emission are located at the surface of the semiconductor [5,[88][89][90]. Indeed, this hypothesis is in agreement with the data obtained in previous studies for the ZnO tetrapods produced by LAFD [75].
It was verified that the presence of LIG mixed with the ZnO led to changes in the relative intensity of the previously observed emissions. When compared to the bare ZnO sample, both composites exhibited a reduction in the overall intensity of the GL, displaying similar intensity in both cases. Moreover, the sample with 5 mg of LIG also showed an increase in the intensity of the NBE emission, while for the sample with 1 mg, the intensity remained barely the same as for ZnO. The ratio of the peak intensity between the visible band and the NBE emission was~0.75,~0.25, and~0.14 for ZnO, ZnO-LIG1, and ZnO-LIG5, respectively, highlighting the strong reduction in the GL/NBE ratio with increasing LIG content. However, one should bear in mind that for the ZnO-LIG5, this reduction in the ratio was due not only to the decrease in the GL intensity, but also to the increase in the UV intensity. This suggests that distinct/additional interactions between the ZnO surface and LIG occurred for the different amounts of carbon material in the composites. The increase in the NBE emission has also been observed in other ZnO/carbon composites previously studied [13][14][15]18] and was attributed to a higher concentration of electron-hole pairs at the surface of ZnO due to the direct contact with the carbon species (good electrical conductors). Indeed, graphene is known to have a remarkably high photon absorption capability, resulting in a larger photocarrier density when compared to traditional semiconductor materials [91], thus providing a significant number of photogenerated pairs at the surface of ZnO. This results in charge transfer to the ZnO energy bands and defect states (e.g., surface defects), improving excitonic and/or surface recombination, which occurs in the UV spectral region. Therefore, the presence of LIG in close contact with ZnO enhances the population of the excitonic levels of the semiconductor and/or the surface defects located in the UV energy range, at the same time that LIG contributes to the passivation of part of the defects that originate the green emission, leading to the reduction in its intensity. The reduction or even suppression of the green spectral component has been observed in other ZnO structures when in contact with C 60 molecules [13,14,92] or Ag micro/nanoparticles [75]. In these cases, charge transfer from surface defects of the ZnO to such materials was found to be the cause for the decrease in the radiative processes [13,14,75]. Hence, one can infer that a similar effect is taking place in the present composites. Moreover, as also reported for the C 60 case [13,14], the charge transfer is likely to occur in both ways (i.e., from LIG to ZnO) as an increase in the intensity of the NBE was observed (in the case of ZnO-LIG5), and from ZnO to LIG, since the intensity of the GL was reduced in both composites. Likewise, the passivation of the surface defects by LIG can also occur, which promotes changes in the band bending at the ZnO surface. After their growth and deposition on the substrates, the ZnO crystals presented several surface-related defects (e.g., adsorbed O 2 , OH groups, etc.) that will affect their surface charge [5,6]. Thus, there is a potential barrier at its surface, which the carriers have to overcome to radiatively recombine [5], thus inhibiting part of the bulk-related recombination, as is the case of the FX. The passivation of part of those defects by the presence of LIG would induce a reduction in the height of the barrier, promoting the decrease in the band bending. Hence, not only did the recombination of some of the surface-related centers (related to the GL) decrease, but the FX recombination was also enhanced. Therefore, it is fair to assume that both defect passivation and charge transfer can occur in the ZnO/LIG samples, explaining the observed PL behavior. It is interesting to note that these processes are influenced by the amount of LIG in the composites, as the enhancement in the NBE emission only occurred for the sample with 5 mg, even though the reduction in the GL intensity was analogous in both cases.
Additionally, previous X-ray photoelectron spectroscopy (XPS) analysis of LIG prepared under analogous conditions of the here reported ones revealed the presence of pyridine groups at its surface [51]. Pyridine possesses nitrogen lone pairs that can act as electron donors when adsorbed at the surface of ZnO, particularly at Zn-terminated ZnO surfaces [93]. Therefore, at these surfaces, a substantial interaction between the nitrogen lone pairs of the pyridine molecule with the surface zinc atoms can occur [94], forming a strong link between the two materials. Indeed, a study by Hofmann et al. [95] on the adsorption of pyridine molecules on ZnO (1010) surfaces demonstrated a reduction in the work function of the semiconductor from 4.5 eV to 1.6 eV when one monolayer of pyridine was adsorbed on its surface, lowering the ZnO potential barrier. The work function was assessed by photoelectron spectroscopy while pyridine desorption was controlled by thermal desorption. Density functional theory (DFT) calculations were also employed to better understand the obtained results. The authors found that for a closed monolayer, the pyridine molecules bind covalently to Zn atoms and that the interface potential is influenced by both the adsorption-induced dipole and the monolayer dipole, with similar contributions from both. This combination leads to a strong polar bond between the organic molecule and the surface Zn atoms. The band alignment between ZnO and pyridine (with negative electron affinity) occurs in a way that prevents the pinning of the Fermi level, which is beneficial for electron injection, as the semiconductor potential barrier is lowered [95]. The theoretical calculation performed by Turkina et al. [96] on pyridine molecules chemisorbed on the nonpolar ZnO (1010) surface also corroborated the conclusions of the previous paper. They suggested that a significant hybridization between the uppermost ZnO layer and the pyridine molecule takes place along the Zn-N bond, with the highest occupied molecular orbital (HOMO) of the organic molecule completely hybridized with the ZnO bands. Simu-lations on the optical properties of such hybrid material pointed to the existence of three distinct types of excitation that they classified as ZnO-related, hybrid, and charge-transfer excitons. The attributions were made taking into account the dominant character of the bands involved in their formation [96]. The last one is particularly interesting since it can induce additional charge at the surface of the semiconductor, involving transitions from pure pyridine bands to ZnO bands. This study revealed that despite the presence of the pyridine molecules at the ZnO surface, optical absorption features of the semiconductor remained the same [96]. All these results allowed us to infer their similarities with the present work, pointing once more to the occurrence of both phenomena: (i) the reduction of the band bending and (ii) charge transfer between the two materials. Energy (eV) The asterisks denote artifacts from the measuring system. The PLE spectra were vertically shifted for clarity in the data display.
It was verified that the presence of LIG mixed with the ZnO led to changes in the relative intensity of the previously observed emissions. When compared to the bare ZnO sample, both composites exhibited a reduction in the overall intensity of the GL, displaying similar intensity in both cases. Moreover, the sample with 5 mg of LIG also showed an increase in the intensity of the NBE emission, while for the sample with 1 mg, the in- The asterisks denote artifacts from the measuring system. The PLE spectra were vertically shifted for clarity in the data display.
3.31 eV emission, thus leading to an enhancement in the radiative recombination involving those states. As the LIG amount increases, besides the surface defect levels, the carriers will be further transferred to the conduction band, thus increasing the excitonic emissions. Therefore, these results suggest the possibility of controlling the emission outcome to some extent by increasing the LIG amount on the ZnO surface in a way that the excitonicrelated emission can be maximized over the visible one, which can be beneficial for applications where deep level emission needs to be avoided/reduced.  The temperature-dependent PL spectra were also assessed for the three samples, evidencing a similar behavior in all cases, as can be seen in Figure S3. With increasing temperature, the DX dissociated, leading to a strong reduction in the intensity of their radiative transitions for temperatures higher than ~70 K. Above these temperatures, the contributions from the FX and the 3.31 eV line (as well as its phonon replicas) remained and their peak positions shifted to lower energies with increasing temperature due to the bandgap shrinkage. At RT, the UV emission was comprised of a single band that resulted  Figure 4b shows the normalized PL and PLE spectra for ZnO and the ZnO/LIG composites. It is interesting to note that no significant changes in the PLE spectral shape were identified with the addition of LIG, corroborating our assumption that LIG does not promote the formation of other radiative recombination channels and that the composites keep the same optical absorption features of the semiconductor, as above-mentioned for the case of the pyridine molecules at the ZnO surface [96]. In all cases, the PLE was monitored at the visible band and showed a steep absorption for wavelengths shorter thañ 414 nm (~3.0 eV) due to absorption into near bandgap electronic states, also presenting a well-defined excitation peak at~376 nm (~3.298 eV), related with the thermally broadened FX excitation [97][98][99]. This peak was coincident in all samples, in agreement with the observed FX emission. As the ZnO FX binding energy is known to be 60 meV, taking into account its emission at~3.28 eV, a value of~3.34 eV can be estimated for the bandgap energy at RT. This value is in line with others previously reported in the literature [97,100]. Hence, the observed spectral shape of the PLE spectra indicates that the probed emission is mainly populated via band-edge absorption and toward higher energies (shorter wavelengths), although subgap electronic states are also present as a tail of states toward longer wavelengths.
To gain further insight regarding the PL features of the composites, low-temperature spectra were recorded ( Figure 5) as well as temperature dependence studies, as depicted in Figure S3 in the SM file. Figure 5 shows a comparison of the RT and 14 K normalized spectra obtained for the ZnO sample and the two ZnO/LIG composites under study. In this case, the spectra were obtained with a higher excitation density than the previous ones (He-Cd laser vs. Xe lamp), even though the same excitation energy was used (325 nm/~3.81 eV). The RT spectra normalized to the peak intensity of the NBE emission showed only minor changes in the GL/NBE ratio between the three samples, which was slightly different from what was observed under Xe lamp excitation. This variation in the intensity ratio is likely to be related to the presence of a higher number of photogenerated carriers when the laser is used as an excitation source, which may overcome the reduction in the green recombination paths induced by the presence of LIG at the ZnO surface. Notwithstanding, a significant decrease in the GL emission for the sample ZnO-LIG5 was still observed. Inspection of the low-temperature spectra indicated that a well-defined NBE was present at 14 K and barely any visible bands could be detected in any case. The low-temperature PL of ZnO is often used as a reference of the samples' optical quality, where the presence of a highly resolved NBE, as in the present case, denotes high optical quality. Another indication for this is the high NBE recombination vs. the deep level emission intensity ratio. In the here reported samples, the most intense line observed at higher energies was due to the donor-bound excitons (DX) recombination, likely overlapped with the FX, while the line at~3.31 eV also identified was proven to be related to the presence of surface states in the case of the LAFD-produced ZnO samples [84]. The relative intensity of this line, when compared to the FX + DX region (labelled as DX in Figure 5 for simplicity and as these should be the dominant transitions at such low temperatures), was seen to be higher in the case of the ZnO-LIG1 sample. On the other hand, for the ZnO-LIG5, the relative intensity remained the same as in the case of the ZnO sample. However, when one considered the absolute intensity of the emissions (inset in Figure 5), it is clear that this is due to an increase in the FX + DX transitions in ZnO-LIG5, in line with what was observed at RT and displayed in Figure 4a. A slight increase in the intensity of this emission line was also observed for ZnO-LIG1, but was much less pronounced. Moreover, in both composites, the intensity of the 3.31 eV line increased when compared with the bare ZnO and remained closely the same for the two LIG compositions. As above-mentioned, such phenomena indicate that the carbon material at the surface of the ZnO semiconductor promotes a preferential population of the surface states that are responsible for the 3.31 eV emission, thus leading to an enhancement in the radiative recombination involving those states. As the LIG amount increases, besides the surface defect levels, the carriers will be further transferred to the conduction band, thus increasing the excitonic emissions. Therefore, these results suggest the possibility of controlling the emission outcome to some extent by increasing the LIG amount on the ZnO surface in a way that the excitonic-related emission can be maximized over the visible one, which can be beneficial for applications where deep level emission needs to be avoided/reduced.
The temperature-dependent PL spectra were also assessed for the three samples, evidencing a similar behavior in all cases, as can be seen in Figure S3. With increasing temperature, the DX dissociated, leading to a strong reduction in the intensity of their radiative transitions for temperatures higher than~70 K. Above these temperatures, the contributions from the FX and the 3.31 eV line (as well as its phonon replicas) remained and their peak positions shifted to lower energies with increasing temperature due to the bandgap shrinkage. At RT, the UV emission was comprised of a single band that resulted from the overlap of those contributions, as above-mentioned in the discussion of Figure 4a.

Electrochemical Evaluation
The general electrochemical characteristics of the ZnO and ZnO/LIG samples were assessed prior to H 2 O 2 detection. In particular, CV and EIS measurements were performed employing ferro/ferricyanide ([Fe(CN) 6 ] 4−/3− ), which constitutes a standard, well-behaved redox probe widely used to characterize and compare electrode electrochemical responses. First, CV in PS, followed by CV in 10 mM of [Fe(CN) 6 ] 4− in PS, were recorded and are displayed in Figure 6.

Electrochemical Evaluation
The general electrochemical characteristics of the ZnO and ZnO/LIG samples were assessed prior to H2O2 detection. In particular, CV and EIS measurements were performed employing ferro/ferricyanide ([Fe(CN)6] 4−/3− ), which constitutes a standard, well-behaved redox probe widely used to characterize and compare electrode electrochemical responses. First, CV in PS, followed by CV in 10 mM of [Fe(CN)6] 4− in PS, were recorded and are displayed in Figure 6. All samples denoted a quasi-rectangular shape even at a high scan rate of 100 mV s −1 , indicating well-behaved capacitance with no relevant resistive losses. Anodic (cathodic) current increase at more positive (negative) potentials indicates the beginning of faradaic reactions involving O2, as explained in the next section. By increasing the LIG amount in the composite, an increase of the overall current background is observed (Figure 6a), indicating an enhancement in the transducer capacitance. Moreover, a well-defined pair of peaks was observed when the CV was run in the presence of [Fe(CN)6] 4− (see Figure 6b). All samples denoted a quasi-rectangular shape even at a high scan rate of 100 mV s −1 , indicating well-behaved capacitance with no relevant resistive losses. Anodic (cathodic) current increase at more positive (negative) potentials indicates the beginning of faradaic reactions involving O 2 , as explained in the next section. By increasing the LIG amount in the composite, an increase of the overall current background is observed (Figure 6a), indicating an enhancement in the transducer capacitance. Moreover, a well-defined pair of peaks was observed when the CV was run in the presence of [Fe(CN) 6 ] 4− (see Figure 6b). This was the result of the electrochemical oxidation of the Fe(II) on the ferrocyanide complex to Fe(III), anodic peak, and then the reduction of Fe(III), the cathodic peak. For all samples, the half-wave potential (E 1/2 ) of this pair of peaks was at~0.215 V vs. Ag/AgCl (1 M KCl). The current was higher with increasing LIG content, in accordance with the trends of Figure 6a. This is a clear indication that the electrochemically active area increased after the addition of LIG, both regarding capacitive and faradaic phenomena.
A scan rate dependence study was carried out to better understand how the ferri/ ferrocyanide species interacted with the surface of the samples (i.e., surface control or mass transport) and to determine the standard heterogeneous electron transfer rate constant (k 0 ) of each one. Figure 7a shows the CVs obtained at varying scan rates (from 20 to 500 mV s −1 ) of the ZnO-LIG5 sample. Similar studies for the remaining samples are depicted in Figure S4 in the SM. Note that these measurements were performed in triplicate for all samples.   The swifter faradaic electron transfer occurring with the addition of LIG to ZnO was also visible in the EIS measurements presented in Figure 8.Indeed, the impedimetric response of the electrode to an AC perturbation in a particular frequency range depends on k 0 . The swifter the electron transfer, the smaller the overpotentials will be to drive the redox reaction and thus the associated electron transfer resistance (RET) decreases. The RET is identifiable by the partial semicircle at higher frequencies and, in simple terms, the larger its diameter, the higher the resistance [76]. One can see that RET was larger for the  Figure 7b shows that the correspondent peak current density scaled linearly with the square root of the scan rate, indicating a ferri/ferrocyanide diffusion-limited process with limited contribution from strongly adsorbed species, if any. The faradaic electrochemically active areas (A eff ) were calculated from the slope of the linear regressions of the anodic branches using the Randles-Ševčík relation (Equation (3)), and the results are shown in Table 1. The calculated A eff for the ZnO sample was somewhat lower than the geometrical area of the electrode (0.125 cm 2 ), however, the increasing amount of LIG incorporated in the samples led to a noticeable increase in A eff , especially for the ZnO-LIG5 sample. This is in accordance with the enhanced electrochemical activity provided by graphene-based materials [101,102]. Table 1. Summary of relevant electrochemical parameters for the ZnO and ZnO/LIG composites. For k 0 and A eff , the results are mean ± standard deviations from independent triplicate measurements. For R s and R ET , the results show standard deviations from EIS fitting procedures. As seen in Figure 7a, anodic to cathodic peak separation (∆E p ) increased with increasing scan rate, meaning that the ferro/ferricyanide redox reaction was not completely reversible and entered a quasi-reversible regime. In such conditions, one can apply the Nicholson method (as described in the Materials' Characterization section) to assess the k 0 of the different samples by constructing a dimensionless Ψ function and correspondent slope analysis within its linear range. The k 0 gives important information on the ability of the electrodes to undergo faradaic charge transfer, a crucial aspect in many types of biosensors. As seen in Table 1, the k 0 values tended to increase with increasing concentration of LIG, from (3.0 ± 0.4) × 10 −3 (ZnO) to (4.3 ± 0.4) × 10 −3 cm s −1 (ZnO-LIG5). This was due to the swift electron transfer capabilities provided by the edgy/platelet-like graphene morphologies [51,103,104], the values of k 0 for the as-synthesized LIG in the literature reaching ca. 10 −2 cm s −1 [51].
The swifter faradaic electron transfer occurring with the addition of LIG to ZnO was also visible in the EIS measurements presented in Figure 8.Indeed, the impedimetric response of the electrode to an AC perturbation in a particular frequency range depends on k 0 . The swifter the electron transfer, the smaller the overpotentials will be to drive the redox reaction and thus the associated electron transfer resistance (R ET ) decreases. The R ET is identifiable by the partial semicircle at higher frequencies and, in simple terms, the larger its diameter, the higher the resistance [76]. One can see that R ET was larger for the bare FTO and decreased following the ZnO, ZnO-LIG1, and ZnO-LIG5 order (see also Table 1), in qualitative accordance with the derived k 0 values. For all samples, the impedimetric response was composed of regions dominated by R ET and mass transfer (diffusion); the latter was identifiable by the straight line with a positive slope toward lower frequencies.
Hence, a R s [Q[R ET W]] equivalent circuit (EC) was employed to model the impedimetric response of all electrodes (inset of Figure 8), except for the ZnO-LIG5 electrode, which was modeled via a R s [Q[R ET Q]] EC. These types of ECs, often referred to as modified Randles circuits, contemplate an equivalent series ohmic resistance R s , a constant phase element Q, which models non-ideal capacitive phenomena arising from surface roughness, and a diffusional element W or Q, accounting for the diffusion-limited mass transfer toward the electrode surface at lower frequencies. The Warburg (W) element was identifiable by a straight line with a unitary slope and resulted from a semi-infinite planar diffusion mechanism [76], which is adequate for the case of the FTO, ZnO, and ZnO-LIG1 electrodes. However, this was not the case for the ZnO-LIG5 electrode, for which the lower frequency diffusion-governed portion of the Nyquist plot presented a slope higher than unity. The Q element is a general mathematical construction from which the W element can be derived as a special case and herein another Q is needed to properly model the cell impedimetric response. This suggests limitations of the semi-infinite diffusional regime posed by the ZnO-LIG5 composite electrodes. This behavior needs clarification in future works (e.g., by extending the frequency range down to 10 mHz or lower).
transfer toward the electrode surface at lower frequencies. The Warburg (W) element was identifiable by a straight line with a unitary slope and resulted from a semi-infinite planar diffusion mechanism [76], which is adequate for the case of the FTO, ZnO, and ZnO-LIG1 electrodes. However, this was not the case for the ZnO-LIG5 electrode, for which the lower frequency diffusion-governed portion of the Nyquist plot presented a slope higher than unity. The Q element is a general mathematical construction from which the W element can be derived as a special case and herein another Q is needed to properly model the cell impedimetric response. This suggests limitations of the semi-infinite diffusional regime posed by the ZnO-LIG5 composite electrodes. This behavior needs clarification in future works (e.g., by extending the frequency range down to 10 mHz or lower).   Finally, it is noteworthy that the total ohmic series resistance R s was seen to increase by ca. 50 Ω after ZnO or ZnO/LIG composite deposition, as expected due to the additional ohmic barrier posed by the deposited material. Nevertheless, in general, the parameters determined in all these measurements are encouraging for the application of these transducers in electrochemical detection of important analytes such as H 2 O 2 , as performed in the next section.

H 2 O 2 Sensing via PL and CV
As the main goal was to use these materials to construct transducer platforms for sensing devices such as enzymatic biosensors, the first approach to infer their suitability to the envisaged application was to test them in the presence of several H 2 O 2 concentrations and assess their response. Hence, both PL and CV studies were conducted on the prepared samples when in contact with H 2 O 2 . Acquiring these two distinct types of physical signals enabled a more accurate and reliable detection, as the interactions that led to them may originate from different phenomena, providing complementary information that is highly beneficial for improving the response of sensing devices. Figure 9 shows the results for the PL signal measured for different H 2 O 2 concentrations (in PS). In this case, ZnO and ZnO-LIG5 samples were selected, as they were the ones that exhibited more distinct PL outcomes. Figure 9a,b display the representative spectra for each type of sample. However, before discussing the H 2 O 2 effect, it is worth mentioning that the immersion of the ZnO and ZnO/LIG samples into the PS already induced significant and reproducible variations in the PL signal, as shown in Figure S5. This behavior indicates that changes in the surface charge density, and therefore in the band bending dynamics, happen upon the immersion (see the schemes in Figure S6). In brief, a strong reduction of the PL intensity and a change in the GL/UV ratio were identified in both samples after their immersion in PS and under UV radiation. However, under continuous UV irradiation, the PL signal of the ZnO sample fairly recovered its initial intensity and spectral shape, remaining constant for further illumination after nearly~2.5 h ( Figure S5a). On the other hand, the changes in the PL spectra of the ZnO/LIG composite after immersion and under irradiation seemed to be rather stable ( Figure S6b), and the signal was seen to be constant after only~30 min. A discussion of the possible phenomena occurring for both cases is detailed in the SM.   The electrochemical assessment of H2O2 detection was performed by CV analysis. First, the electrodes were swept from −1 to 1 V in the presence and absence of O2, as depicted in Figure 10. It is worth noting that the measurements were carried out in a homemade electrochemical cell with an inlet of N2 and an outlet for the O2 (see Figure S2b). The electrolyte was bubbled for 30 min with N2 to remove the O2 from the solution and kept under a N2 gas blanket. The ZnO electrode presented one reduction peak at −0.627 V (see Figure 10a), which was ascribed to the electrochemical reduction of O2 (Equation (4)) as it disappeared after being purged from the electrolyte (Figure 10b). After this initial stabilization in PS, the samples were probed when immersed in different concentrations of H 2 O 2 . Therefore, further analysis was made by comparing the spectra obtained in the PS (0 mM of H 2 O 2 , after signal stabilization) with the ones recorded after adding H 2 O 2 . As such, it was verified that in both cases, a blue luminescence (BL) band peaked at~438 nm/~2.83 eV developed with increasing H 2 O 2 concentration, being more evident for the concentration of 4.4 mM and above. With the enhancement of the BL, both blue and green bands became overlapped, hampering a proper evaluation of the evolution of the latter. Nonetheless, the BL was seen to dominate over the GL above the concentration of~8.7 mM. This blue band was due to H 2 O 2 emission, as corroborated by the spectrum in Figure S7a, where a comparison between the PL of the 100 mM H 2 O 2 solution and the ZnO sample immersed in a similar solution was made. Furthermore, the peak intensity of the UV recombination also increased with the H 2 O 2 concentration, and this change in the intensity was maintained even after being removed from the solution, indicating that the H 2 O 2 reacted with the ZnO surface (see Figure S7b). This behavior plays a more noteworthy role in the case of the bare ZnO sample than in the case of the composite. These results contradict the ones obtained by Sodzel et al. [60], who reported the evolution of the PL signal of ZnO nanoparticles (commercially acquired from Sigma-Aldrich) in the presence of H 2 O 2 and recorded the decrease in both UV and GL intensity with H 2 O 2 increasing concentration (similar range as the present work). According to them, this effect was mediated by the defects located at the surface of the semiconductor, which were influenced by the presence of H 2 O 2 . They claimed that this compound decomposed catalytically on the ZnO surface into H 2 O and O 2 , accepting electrons from the conduction band of ZnO during the reaction, and thus inhibiting the radiative recombination of the carriers, which led to the PL quenching [60]. However, one can infer that the presence of H 2 O 2 may have a direct impact on the surface defects in ZnO. The hydrogen peroxide solution is known to be unstable and can be easily decomposed, providing active oxygen atoms that can fill oxygen vacancies [64,105]. Assuming that these defects are surfacerelated ones that contribute to the band bending, their reduction expectably leads to a higher probability of radiative recombination by the electron-hole pairs, hence enhancing the FX-related transitions in the UV spectral region. Figure 9c depicts the average evolution of the BL/UV intensity ratio for the ZnO and ZnO-LIG5 samples, which exhibited a very distinct behavior from each other (see the behavior for each sample in Figure S8). The data were fairly linear in the concentration range between 1.8 mM and 32.7 mM. Therefore, assuming the BL/UV ratio as the response of the present sensors to the concentration of H 2 O 2 in the solution, a linear calibration curve could be defined, as plotted in Figure 9c. Linearity is an important characteristic in a sensing device as it is related to the accuracy of the response assessed and can be linked to the resolution of the biosensor in the analyzed range of analyte concentrations [106][107][108]. This property is directly associated with the sensitivity (S) of the sensor, which is defined as the minimum concentration variation that the device is capable of distinguishing and it is given by the slope of the calibration curve [106,107]. From the present results, it was verified that the slope of the data points for the case of the composite was higher than the one for the bare ZnO (0.026 vs. 0.0079 mM −1 ), suggesting that greater sensitivity was achieved for the ZnO-LIG5 sample. The LOD parameter is also critical in biosensors and can be expressed as LOD = 3σ/S, where σ corresponds to the standard deviation from the calibration curve [109,110]. In this case, LODs of 0.8 mM and 0.45 mM were estimated for the ZnO and ZnO-LIG5 samples, respectively. Hence, the obtained results indicate that the changes observed in the PL signal of the present samples with H 2 O 2 can be exploited as a possible transduction mechanism to assess the concentration of this chemical compound.
Even though the use of PL for direct sensing of this compound is not widely employed, some reports can be found in the literature using different materials as transducers [60,63,111,112]. For instance, Sarangi et al. [63] used ZnO nanorods to probe H 2 O 2 and glucose (via H 2 O 2 detection). In line with the work by Sodzel et al. [60], they observed the quenching of the UV intensity with increasing glucose concentration. Despite observing different effects on the PL response of their samples than those reported here, they obtained a linear detection range between 0.5 and 30 mM, which is in agreement with the present one. Moreover, these authors reported a sensitivity of 0.014 mM −1 , which was slightly lower than that identified here for the ZnO-LIG5 sample.
The electrochemical assessment of H 2 O 2 detection was performed by CV analysis. First, the electrodes were swept from −1 to 1 V in the presence and absence of O 2 , as depicted in Figure 10. It is worth noting that the measurements were carried out in a homemade electrochemical cell with an inlet of N 2 and an outlet for the O 2 (see Figure S2b). The electrolyte was bubbled for 30 min with N 2 to remove the O 2 from the solution and kept under a N 2 gas blanket. The ZnO electrode presented one reduction peak at −0.627 V (see Figure 10a), which was ascribed to the electrochemical reduction of O 2 (Equation (4)) as it disappeared after being purged from the electrolyte (Figure 10b).
Chemosensors 2021, 9, x FOR PEER REVIEW 22 of 30 Moreover, the electrodes containing LIG presented an additional reduction peak at −0.467 V and −0.481 V for the composites with 1 mg and 5 mg of LIG, respectively, in the presence of O2 (Figure 10a). In the absence of O2, these peaks were still observed, but shifted to lower negative potentials, as can be observed in Figure 10b. The nature of these peaks is not clear, since it was not noticeable neither in the ZnO sample nor in other works using as-synthesized LIG. Nevertheless, as it increased with the LIG content, one possible explanation is the involvement of new electroactive groups present in LIG and promoted by its mixture with the organic compounds and the subsequent thermal treatment performed in air at 400 °C. As discussed for the Raman data concerning the change in the ID/IG between the as-synthesized and deposited LIG (see Figure 3), the employed processing steps may introduce new functional groups and/or defects in LIG, particularly an increase in the oxidation due to the thermal treatment in air. Therefore, it is fair to assume that these groups/defects can be responsible for the observed peak. The contributions from additional effects due to ZnO-LIG interaction can also play a role, as it was also seen to induce changes in the Raman spectra and, thus, in the density/type of defects. Concerning the electrochemical detection of H2O2, it is important to mention that the homemade electrochemical cell has a small aperture that allows for the addition of small volumes of the analyte, in absence of O2 and under stirring (see Figure S2 in SM). Therefore, the experiments on the detection of H2O2 were performed without O2 and a welldefined volume of PS was used as the electrolyte. Small volumes of H2O2 stock solution were added and the cyclic voltammograms recorded as displayed in Figure 11. The ZnO and ZnO-LIG5 electrodes were evaluated and displayed similar electrochemical behavior, with an anodic peak between 0.5 and 0.6 V observed with the increase in H2O2 concentration. This peak arises from the electrochemical oxidation of H2O2 following Equation (5).
An increase of cathodic current intensity was also observed in the more negative potentials due to the generation of O2, as a result of H2O2 electrooxidation (Equation (5)), which was then reduced according to Equation (4). Moreover, the electrodes containing LIG presented an additional reduction peak at −0.467 V and −0.481 V for the composites with 1 mg and 5 mg of LIG, respectively, in the presence of O 2 (Figure 10a). In the absence of O 2 , these peaks were still observed, but shifted to lower negative potentials, as can be observed in Figure 10b. The nature of these peaks is not clear, since it was not noticeable neither in the ZnO sample nor in other works using as-synthesized LIG. Nevertheless, as it increased with the LIG content, one possible explanation is the involvement of new electroactive groups present in LIG and promoted by its mixture with the organic compounds and the subsequent thermal treatment performed in air at 400 • C. As discussed for the Raman data concerning the change in the I D /I G between the as-synthesized and deposited LIG (see Figure 3), the employed processing steps may introduce new functional groups and/or defects in LIG, particularly an increase in the oxidation due to the thermal treatment in air. Therefore, it is fair to assume that these groups/defects can be responsible for the observed peak. The contributions from additional effects due to ZnO-LIG interaction can also play a role, as it was also seen to induce changes in the Raman spectra and, thus, in the density/type of defects.
Concerning the electrochemical detection of H 2 O 2 , it is important to mention that the homemade electrochemical cell has a small aperture that allows for the addition of small volumes of the analyte, in absence of O 2 and under stirring (see Figure S2 in SM). Therefore, the experiments on the detection of H 2 O 2 were performed without O 2 and a well-defined volume of PS was used as the electrolyte. Small volumes of H 2 O 2 stock solution were added and the cyclic voltammograms recorded as displayed in Figure 11. The ZnO and ZnO-LIG5 electrodes were evaluated and displayed similar electrochemical behavior, with an anodic peak between 0.5 and 0.6 V observed with the increase in H 2 O 2 concentration. This peak arises from the electrochemical oxidation of H 2 O 2 following Equation (5). Similarly, and as explained before in the PL studies, a calibration curve was calculated ( Figure 11c) to assess the sensor response for ZnO and ZnO-LIG5 electrodes. The maximum intensity of the anodic peak related to H2O2 oxidation (between 0.5 and 0.6 V) was plotted as a function of the H2O2 concentration for all electrode samples, as depicted in Figure S9, and the average is displayed in Figure 11c. Here, the response was found to be linear in the concentration range from 0 to 14.6 mM, evidencing sensitivities of ~308.8 and ~276.8 μA mM −1 cm −2 for ZnO and ZnO-LIG5, respectively. LOD values of 0.11 and 0.19 mM were obtained for ZnO and ZnO-LIG5, respectively. Even though the ZnO-LIG5 composite showed an enhanced electron transfer compared with ZnO (see Section 3.3), these results indicate that the H2O2 detection occurred due to the electrocatalytic activity of ZnO, and in this case, LIG had no significant effect on H2O2 detection via CV using the potential at ~+0.6V vs. SCE.
An overall overview of the performance of the electrode points to a better response of the electrochemical sensors in the low concentration range, while the PL-based sensing An increase of cathodic current intensity was also observed in the more negative potentials due to the generation of O 2 , as a result of H 2 O 2 electrooxidation (Equation (5)), which was then reduced according to Equation (4).
Similarly, and as explained before in the PL studies, a calibration curve was calculated (Figure 11c) to assess the sensor response for ZnO and ZnO-LIG5 electrodes. The maximum intensity of the anodic peak related to H 2 O 2 oxidation (between 0.5 and 0.6 V) was plotted as a function of the H 2 O 2 concentration for all electrode samples, as depicted in Figure S9, and the average is displayed in Figure 11c. Here, the response was found to be linear in the concentration range from 0 to 14.6 mM, evidencing sensitivities of~308.8 and 276.8 µA mM −1 cm −2 for ZnO and ZnO-LIG5, respectively. LOD values of 0.11 and 0.19 mM were obtained for ZnO and ZnO-LIG5, respectively. Even though the ZnO-LIG5 composite showed an enhanced electron transfer compared with ZnO (see Section 3.3), these results indicate that the H 2 O 2 detection occurred due to the electrocatalytic activity of ZnO, and in this case, LIG had no significant effect on H 2 O 2 detection via CV using the potential at~+0.6V vs. SCE.
An overall overview of the performance of the electrode points to a better response of the electrochemical sensors in the low concentration range, while the PL-based sensing maintained linearity for higher concentrations. In this way, the sensor detection range can be extended using the same transducer platform and by analyzing the analyte-containing sample using a combination of both methods. Moreover, the possibility of a cross-checking of the results by the inspection of the two types of calibration curves makes a device constructed in this way more interesting, offering in situ counter-proof analyses without the need of collecting another sample, with the potential to be a major improvement in the biosensing field. Table 2 displays a summary of the sensing figures of merit for the here studied sensors, as well as a comparison with those reported in the literature for ZnO-based H 2 O 2 sensors. As above-mentioned, PL sensing is scarcely used in this type of sensor, whereas transduction via electrochemical assessment using ZnO and ZnO-based composites is far more common [113][114][115][116][117][118][119]. A brief literature comparison from recently published papers revealed that the values obtained for the sensitivity in the present samples were superior to most of those reported for ZnO-based electrodes [117][118][119][120]. Regarding the LOD, values in the µM range can already be attained for ZnO composites with noble metals or mesoporous carbon [117][118][119]. Nevertheless, the here estimated LODs are well in line with the ones required for glucose sensing, for instance, indicating the suitability of these materials to be used as transducers in further biosensing applications. Besides, a great number of works devoted to H 2 O 2 detection via CV analysis operates at negative potentials, where the O 2 interference can play a non-negligible role. Conversely, in the present work, this probing was performed at~+0.6 V vs. SCE, which is advantageous to reduce the O 2 contribution. Furthermore, to the best of our knowledge, it is the first time that PL and CV signals were combined to provide the final sensing response, which can be useful when counter-proof measurements are needed, as well as to assess different concentration ranges. (a) lower concentration tested. (b) µA mM−1 (c) using square wave voltammetry (d) H2O2 detection following the potential at +0.6 V vs. SCE.

Conclusions
In summary, ZnO/LIG composites were prepared using LAFD produced ZnO and LIG scraped from the original polyimide substrate, mixed at controlled ZnO:LIG weight ratios (50:1 and 50:5). The photoluminescence assessment showed that by mixing LIG with the ZnO tetrapods, changes occurred to the spectra when compared with bare ZnO. The intensity of the UV emission at RT, mostly related to the FX recombination, was seen to significantly increase for the ZnO-LIG5 sample, while a similar reduction in the GL intensity was observed for both composites. Such phenomena were attributed to charge transfer processes both from ZnO to LIG (decrease in the GL associated with surface states), as well as from LIG to the semiconductor (increase in the excitonic-related transitions). By cooling down the samples to 14 K, a strong enhancement in the intensity of the emission line resultant from the overlapping of FX and DX recombination was clearly identified for the ZnO-LIG5 sample, in line with the results recorded at RT. Furthermore, the intensity of the 3.31 eV line (related to surface defects) also experienced a similar increase in both composites, suggesting a higher population of those states promoted by the presence of LIG.
The CV and EIS measurements using the [Fe(CN) 6 ] 4−/3− redox pair indicated swifter electron transfer kinetics and increased electrochemically active area with the amount of LIG incorporated in the samples. The heterogeneous electron transfer rate constants were within~3.0 to 4.3 × 10 −3 cm s −1 , which supports the adequateness of these electrodes for faradaic biosensing.
H 2 O 2 monitoring using ZnO and ZnO-LIG5 materials as transducers was proven to be feasible and evidenced promising results. Both PL and CV analysis enabled tracing the calibration curves for each type of sample. In the case of the detection via PL, the ZnO and ZnO-LIG5 samples were revealed to be sensitive in the range of 1.8 to 32.7 mM (maximum concentration tested), with the composite sample exhibiting a higher sensitivity and a lower limit of detection, 0.45 mM of H 2 O 2 vs. the 0.68 mM obtained for ZnO. Contrasting with the PL results where a marked difference was observed for the calibration curve of two types of samples, CV measurements evidenced similar behavior for both samples. In this case, the linear range was found between 0.8-14.6 mM, and LOD values of 0.11 and 0.19 mM were estimated for ZnO and ZnO-LIG5, respectively, indicating that the CV detection yielded lower LODs compared to PL. Therefore, it was verified that both signals can effectively be used for transduction anddisplay different detection ranges that can be used to complement the sensing response in a single device.
Overall, the present results indicate that the prepared materials exhibit promising properties for several technological applications, namely in the biosensing field.
Supplementary Materials: The following are available online at https://www.mdpi.com/article/ 10.3390/chemosensors9050102/s1; Figure S1: Pictures of the produced samples that were obtained after the thermal treatment; Figure S2 PL spectra of a ZnO sample before, during and after its immersion in a 25 mM of H 2 O 2 solution (in DI water); Figure S8: Peak intensity ratio BL/UV (measured at 438 nm and 380 nm, respectively) as a function of the H 2 O 2 concentration for the tested (a) ZnO and (b) ZnO-LIG5 samples; Figure S9: Current density at the peak maxima (located at~0.5 -0.6 V) as a function of the H 2 O 2 concentration obtained for the three replicas of (a) ZnO and (b) ZnO-LIG5 samples; Table S1: Summary of the growth/synthesis condition employed for both materials comprising the ZnO/LIG composites.  Data Availability Statement: The raw/processed data required to reproduce these findings can be shared upon request.