# N-TiO2-x Nanocatalysts: PLAL Synthesis and Photocatalytic Activity

Authors: Enza Fazio; Angela Maria Mezzasalma; Luisa D’Urso; Salvatore Spadaro; Francesco Barreca; Giovanni Gallo; Fortunato Neri; Giuseppe Compagnini
Journal: Journal of Nanomaterials
 (2020)

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## Abstract

N-TiO2-x nanocatalysts are developed by the pulsed laser ablation in liquid (PLAL) technique, a simple and surfactant-free preparation method. The PLAL approach allows synthesizing chemical-morphological fine-tuning water TiO2-based nanomaterials, starting from targets of different nature (powders and commercial high purity targets). The catalytic activity was investigated using methylene blue (cationic dye) and methyl orange (azo dye). A different photocatalytic response was found for the various kinds of N-TiO2-x. In the first 20 min, under UV and visible light, about 50% and 10% of the methyl orange were removed using the N-TiO2-x and TiO2 colloids, respectively. In addition, we observe that the response towards the methylene blue is comparable in all the synthesized samples under UV irradiation while differing by about 30% under a visible lamp. The enhanced photocatalytic response of the N-TiO2-x nanocatalysts with respect to the TiO2 one is dependent on the content of the nitrogen dopant, surface area, and nitrogen-oxygen bonding configurations.


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## Body

## 1. Introduction

TiO2 is extensively studied in view of photocatalytic applications thanks to its low cost, high photogenerated hole oxidizing power, and long lifetime of electron/hole pairs when irradiated with light. Such photoinduced electron-hole pairs have been utilized to generate electricity in solar cells, to split water into hydrogen and oxygen, and to oxidize and degrade inorganic/organic/biological compounds in environments as well as to create superhydrophilicity [1].The first reliable paper on photocatalytic activity of TiO2 was published in 1938. It has been shown that UV absorption produced active oxygen species on TiO2 surfaces, causing photobleaching of dyes [2]. Subsequent works to this have shown the oxidation of organic solvents and the formation of H2O2 under an UV irradiation of a mercury lamp under ambient conditions while the water photolysis was demonstrated for the first time in 1969 on TiO2 semiconductors [3]. Fundamental processes of TiO2 photoelectrochemistry have been studied intensively, mainly analyzing the behavior of TiO2 nanomaterials, interesting for their high surface-volume ratio. TiO2 nanostructures provide increased surface area at which photoinduced reactions may occur, enhancing the light absorption rate, increasing the surface photoinduced carrier density, enhancing the photoreduction rate, and resulting in higher surface photoactivity. At the same time, the high surface-volume ratio of the nanoparticles enhances the surface absorption of OH− and H2O, increasing the photocatalytic reaction rate [4, 5]. Based on the basic research results, industrial applications of photocatalytic TiO2 have been achieved since the end of the 1990s and will develop further in the 21st century. Among them are photocatalytic water splitting [6], purification of pollutants [7], photocatalytic self-cleaning [8], photocatalytic antibacteria, and photoinduced super hydrophilicity [9], as well as photovoltaics and photosynthesis [10] (see Figure 1).Figure 1
Dependence graph of photo-activated TiO2 materials applications. The flow goes from the top to the bottom direction.However, the large bandgap of TiO2 (3.2 eV for anatase and 3 eV for rutile) limits its light absorption only to the UV region [11]. Thus, pure TiO2 works as a photocatalytic material under UV light (4-5% of solar light), but it has very low photocatalytic activity in visible light (45% of solar spectrum). Some efforts have been made to overcome this limitation. Some aspects have been identified as essential to resolve the issue such as to tailor TiO2 bulk/surface electronic structures and the interfaces in order to tune surface band-bending, surface state distribution, and charge separation, which could significantly influence TiO2 photocatalysis response in the visible spectral range. The main requirements are (1) a high surface/volume ratio and a controlled anatase-rutile ratio to provide a large number of active sites for the degradation reaction and (2) shifting the absorption limit of the material in the visible range, searching for an increase in reaction rate of photocatalysis and hydrogen production.Doping appears as a good alternative for changing the activity of TiO2 catalysts through the optoelectrical modification of this material by the introduction of dopants with different energy levels between the conduction and valence bands. The applied dopants can be (1) noble metals (such as Ag, Au, Pd, and Pt), which absorb the visible light due to the surface plasmon resonance, but the high cost associated with these materials should be considered a disadvantage [12]; (2) transition metals cheaper than noble metals, but their leaching behavior leads to the fast deactivation of the catalyst and constitutes a second source of pollution [13]; and (3) nonmetals (N, B, S, F, and C) able to extend optical absorption of TiO2 to the visible light region and then to improve visible-light-driven photocatalytic processes [14, 15]. Among the above-mentioned nonmetals, the most suitable and commonly used is nitrogen.Nitrogen, as sulfur and fluorine species, is an anionic dopant which confers greater stability to the catalyst with respect to the conventional transition-metal dopants and also determines a significant red shift of the band gap into the visible range. According to theoretical modelling [16], the p-orbitals of the nitrogen dopant extensively overlapped, favouring the transfer of photogenerated charge carriers to the TiO2 surface, in turn increasing its photocatalytic activity [17]. It was proven that both in the anatase and rutile phases of TiO2, the N2p states were located just above the top of the O2p valence band, which means a red shift of the absorption band edge to the visible region [18].Despite the potential, data about the main changes provided by nitrogen doping in TiO2 is not well established. Moreover, for large scale usage of TiO2-xNx nanomaterials in all the solar radiation ranges, none of the results actually reached are satisfactory due to their low nitrogen/oxygen content, low chemical-physical stability, and increased carrier trapping.There are multiple and assorted methods to prepare N-TiO2 catalysts. Physical vapor deposition (PVD), reactive sputtering, cathodic arc deposition, plasma-gas reaction, and Chemical Vapor Deposition (CVD) are the common methods used to deposit N-doped titania films. However, all these techniques allow the deposition of low level N-doped titania with micron-sized structures only at high vacuum conditions (10-8-10-9 Pa) and at high temperature (1200-1500°C) to avoid sample reoxidation. The methods based on plasma-gas phase reactions with the use of TiN powders seem to be a good and low cost alternative to obtain films with a small particle size (about 10 nm). However, these samples show a high oxygen content (ca. 15–20 at.%) [19]. Recently TiO2, loading a different percentage of nitrogen, was prepared by nitridation of a nano-TiO2 powder in a mixed ammonia/argon atmosphere at a range of temperatures from 400 to 1100°C [17]. According to the results obtained by Zhang et al. [20], the samples prepared at 700°C are oxygen deficient, which may be partly responsible for the shifting band gap and for the significant photocatalytic activity. On the other hand, nanocolloid production generally involves the use of surfactants and derivatives which cause secondary pollution to the environment.For all these reasons, further studies will be useful mainly to (1) clarify whether oxygen deficiency has a bigger effect on photocatalytic activity than N-doping at low levels, (2) give a systematic and complete characterization of the chemical-morphological and optical properties of the synthesized N-TiO2-x nanomaterials, and (3) identify green methods and define a synthesis protocol in order to produce nanocolloids. This latter should be usable directly in the liquid phase in an innovative photocatalytic device, with a high degradation time (even in extreme conditions).In this work, we presented and discussed the results obtained using the potentiality of the pulsed laser ablation in liquid (PLAL) technique to prepare N-TiO2-x nanocolloids. The syntheses were carried out in water to favour the formation of (Ti-O-N), (−NH2), NO2−, N2, NHx, and (−OH) species, inducing their incorporation into the TiO2 lattice as nitride through dehydration. To this aim, the optimal PLAL deposition parameters (i.e., laser fluence and irradiation time) were found as well as the optimal composition of the targets (TiO2 mixed to TiN powders or TiN rod purchased from Matek Srl). PLAL processes were performed in ambient condition (room temperature) using the water as solvent, with the advantage to obtain nanocolloids, without by-products, suitable for mechanical deposition on photoanode materials or to be incorporated in integrated solar water-splitting devices.All the synthesized colloids were characterized by scanning transmission electron microscopy (STEM), X-ray photoelectron (XPS), and conventional optical spectroscopies, providing complementary information which allows drawing a picture of the compositional, morphological, and optical properties of the nanocomposites, constituting the starting point for their successive photocatalysis applications which require moderate operating temperatures and limited energy consumptions.


## 2. Experimental Section

TiO2-xNx powders, pressed into a disk at room temperature, were prepared starting from powders of TiN and TiO2 (P25), mixed at the TiN/TiO2 mass ratios of 75/25, 50/50, and 25/75. Then, the compacts were maintained in a furnace at around 250°C for 1 hour. Pulsed laser ablation in liquid (PLAL) processes of the pressed powders as well as of commercial TiN and TiO2 rod targets (synthesized by Matek Srl at 1200°C) were carried out in deionized water (H2O). The targets were irradiated at the laser fluence of 0.5 J/cm2 for an irradiation time of 15 min (samples labelled TION3-5 and TION1P-5P-17P-12P) and of 1.5 J/cm2 for 30 min (TION4), by the 532 nm radiation coming from a Nd:YAG laser source, operating at the repetition rate of 10 Hz and at the pulse width of 6 ns. The scheme of the PLAL setup and an overview of the sample set are shown in Figure 2.Figure 2
Scheme of PLAL setup and synthesis parameters for each adopted target.Scanning transmission electron microscopy (STEM) images were acquired using a Zeiss electronic microscope which operates at an accelerating voltage of 30 kV. Samples for the STEM analysis were prepared by dropping a suspension of the sonicated colloids on a 400 mesh holey-carbon support sputter-coated with chromium.A PerkinElmer (Lambda 750) spectrometer, working in the 300-900 nm range, was used to collect optical absorbance spectra.The crystalline phase of the oxide was also investigated by analyzing Raman scattering data. Raman spectra have been excited with the 532 and 638 nm diode laser lines mounted in the XploRA spectrometer coupled with an Olympus microscope. Spectra have been collected with a 50x objective (spot size of about 2μm) and a Charged Coupled Device (CCD) used as a sensor. An acquisition time of 80 s granted a sufficient S/N ratio.The chemical bonding states and the relative atomic content in the nanocomposites were investigated by X-ray Photoelectron Spectroscopy (XPS), using the Thermo Scientific K-Alpha system equipped with a monochromatic Al-Kα source (1486.6 eV) and operating with a pass energy of 50 eV in the CAE mode.Some aqueous solutions of methyl orange (MO) and methylene blue (MB) (Sigma-Aldrich) were prepared by dissolving the analytical grade dyes in the synthesized colloids at a1.5·10−5M concentration.MO and MB were used as probe molecules for a first evaluation of the photocatalytic activities of N-TiO2 nanostructures. The reaction was conducted in 3 ml of aqueous solution containing the dye, previously maintained in a beaker for 30 min at a temperature of about 10°C. The photocatalytic reaction was carried out under stirring. 0.5 mg of catalyst was dispersed in 3 ml of dye aqueous solution placed in an ice bath; in this way, the temperature of aqueous dispersion was maintained at around 14±2°C.A 40 W Hg lamp (for UV irradiation) and a 450 W xenon lamp (as a visible light source blocking UV radiation by a 400 nm glass filter) were used as light sources placed at a distance of about 15 cm. Prior to irradiation, the dye catalyst suspensions were kept in the dark for 30 min to ensure an adsorption/desorption equilibrium. Then, the photodecolourization of MO and MB was studied.Analytical samples were filtered through a 0.2μm Millipore® filter to remove the solid, at well-defined time intervals during the irradiation, and placed into a 0.35 ml microquartz cuvette. Then, the residual dye concentrations in the filtrates were analyzed by UV-visible spectrophotometer (PerkinElmer 750) at maximum absorption wavelengths (λmax) of 464 and 664 nm for MO and MB, respectively. Direct photolysis decolourization of the respective dye was estimated by performing blank experiments.


## 3. Results and Discussion

### 3.1. Sample Characterization

In Figure3 are shown representative STEM images of the samples obtained ablating in water targets of different nature. Specifically, the colloids, obtained ablating the (25/75) TiN/TiO2 powder targets, show a porous morphology with some spherical nanostructures with a mean diameter of about 50 nm (Figure 3(a)). It is to be noted that the observation of perfectly rounded submicrometer particles, probably associated with TiO2 species, is in agreement with what was observed by Felice et al. [21]. On the other hand, a high density of nanoparticles with a spherical shape and size mainly below 30 nm characterizes the colloids prepared ablating the high purity (99.99%) commercial TiN rod target (Figure 3(c)). An analogous morphology is shown by the colloids prepared ablating the TiN powder target (Figure 3(b)). More details can be observed from images d–h collected for the samples obtained ablating the (25/75) TiN/TiO2 powder targets and the TiN rod and powder targets.Figure 3
STEM images of the samples obtained ablating the (25/75) TiN/TiO2 powder targets (a, d, e), the TiN powder target (b, f), and the high purity (99.99%) commercial TiN rod target (c, g, h).
(a)(b)(c)(d)(e)(f)(g)(h)The sample obtained from the (25/75) mixed TiN/TiO2 powders show Raman features typical of the anatase-rich TiO2 material [6]. It is important to highlight that first-order Raman features of TiN (at 225 cm-1 (TA), 310 cm-1 (LA), and 540 cm-1(TO)) are almost absent, suggesting that nitrogen could be incorporated as a defect in the crystalline TiO2 lattice. Samples, obtained from TiN powder (red line) and rod (blue line) targets, showed very similar Raman spectra; in this case, TiN vibrational features are well observable (see Figure 4(a)) as indicated by the pronounced peak at about 550 cm-1 related to the TiN-TO mode [22]. Moreover, we observe that the Eg (associated to the anatase phase) signal below 200 cm-1 is totally absent and that the intensity ratio between the observed peaks at 200 and 290 cm-1 is very similar to that of a possible formation of a rutile TiO2 phase. Unfortunately, TiN and rutile features overlapped in this region, so a correct attribution for the rutile is not possible exclusively from Raman analyses. All this evidence indicates a tendency towards an anatase-rutile conversion and/or an oxygen replacement by nitrogen with the formation of Ti-N bonds [22]. Interstitial nitrogen species are expected as a result of the ablation of a TiN target in water.Figure 4
(a) Raman and (b) optical absorbance spectra of the synthesized samples.
(a)(b)In Figure4(b) are shown the optical absorbance spectra of the synthesized nanocolloids. We observe that (1) the colloid obtained by a TiN rod target is transparent (over 90%) in the visible range with a sharp absorption edge at about 350 nm, (2) a broad band at around 420 nm characterizes the sample prepared from the TiO2 powder target, and (3) a slight blue shift is evident in the colloids prepared using the pressed and sintered target with a (75/25) TiN/TiO2 mass ratio; for these samples, the 420 nm band is totally absent, while a significant visible light absorption contribution up to 600 nm is evident, probably due to the electronic transition from the localized N doping level to the conduction band of TiO2 (see also the scheme reported in Figure 5).Figure 5
Schematic diagram showing the valence and conduction bands of N-doped TiO2.The incorporation of nitrogen into the TiO2 lattice leads to the formation of a new midgap energy state, i.e., the N2p band above the O2p valence band. So, upon a visible light irradiation, the electrons can migrate from the valence band to the conduction band (Figure 5) and from here the expected visible light activity of N-dopedTiO2 or TiO2-xNx materials (see Catalytic Activities). Nitrogen can replace one or more oxygen atoms (“substitutional doping”), or nitrogen can be positioned in interstitial TiO2 sites (“interstitial doping”). In both cases, as shown in Figure 5, N doping leads to a change in the electronic behavior of the nanoparticle due to a change in the electronic band structures and/or a decrease of electron-hole recombination [23].XPS analysis allows investigating the surface chemical composition and bonding configurations of our samples, in which it is known that the surface chemical coordination greatly influences the catalytic response [24]. In Figures 6(a)–6(c) are shown representative Ti2p and N1s deconvoluted profiles, while the chemical atomic percentage of the detected species and the relative surface bonding configurations are reported in Table 1. Two different Ti2p profiles characterize our samples: those obtained starting from the TiN rod target (Figure 6(a)) show a broad band whose features are ascribed to the titanium nitride, the titanium dioxide (TiO2), and the intermediate phase of titanium oxynitride [25, 26]. Otherwise, in the samples obtained by the TiN powder (Figure 6(b)), narrower profiles are obtained and the binding energy of the Ti2p3/2 peak is brought closer to 458.5 eV (typical of TiO2 compound), while the binding energies of the other phases still fall within the possible ranges. Interestingly, no resolved N1s signal was collected from the powder targets while the N1s profile is well structured and defined for samples obtained from the rod targets (Figure 6(c)). The main components are located at around 396 and in the 397-400 eV range. These features are ascribed to the titanium oxynitride phase and to the nitrogen in substitutional and interstitial positions [26–31]. The NHx, NO/NO2, and NO3− contributions are generally reported at a binding energy higher than 400 eV [29–31] but, in our case, are less pronounced (see Figures 6(c) and 6(d)).Figure 6
Ti2p (a, b) deconvoluted profiles of the samples obtained from the TiN rod and TiN powder targets, respectively. We outline that all the samples obtained from the mixed powders show Ti2p line shapes similar to those of the sample starting from the TiN powder. The N1s deconvoluted profile of the sample obtained starting from the TiN rod target (c) and a scheme of the potential nitrogen allocation into the TiO2 structure (d).Table 1
Atomic surface chemical composition and bonding fraction estimated by the deconvoluted XPS spectra.
SampleChemical composition (%)Bonding configurations (%)Ti2pN1sN (%)Ti (%)O (%)Ti-NTi-O-NTi-O2N-Ti-ONsubst.Nint.NO/NO2TION1p1.128.870.10.86.492.8——100—TION5p0.728.471.00.53.596.0——100—TION12p5.923.870.30.93.495.7——100—TION17p4.619.875.60.03.796.3——100—TION312.228.859.115.526.058.567.418.59.54.6TION417.824.158.117.829.153.159.726.610.72.9TION514.825.759.617.430.152.665.522.09.92.7


### 3.2. Catalytic Activities

All the photocatalytic reactions were undertaken in air as the photobleaching of MB is irreversible in an oxygen-saturated aqueous solution such as ours, and in an ice bath to avoid degradation effects due to light irradiation-induced heating. The photodegradation was monitored by recording UV-visible extinction spectra as a function of light irradiation exposure time. The percentage of MB decolourization under ultraviolet and visible radiation for the synthesized and TiO2 reference samples is shown in Figure 7. Under UV and visible irradiation, all the produced nanostructures show a photocatalytic activity towards the degradation of methylene blue (MB) dye molecule. However, the response is comparable in all the samples under UV irradiation while, under the visible lamp, the estimated percentages differ by about 30%. In fact, for the samples obtained by ablating TiN powder and TiN/TiO2-mixed powder in 75/25 ratio, MB decolourization is about 45% but increases in the samples obtained from the TiN rod or from the TiN/TiO2-mixed powders at the 25/75 ratio. Photocatalytic decolourization behavior of MB dye (during visible irradiation, over the 1 h time frame of the experiment) seems to be influenced by the amount of N, Ti, and O and their bonding coordination and by the increasing absorption in the visible light region [32].Figure 7
Photocatalytic activity towards the methylene blue (MB) dye molecule under UV and visible irradiation (60 min exposure time).In Figure8 is shown the percentage of MO decolourization under UV and visible lamp for the synthesized and reference samples. MO is an azo dye characterized by a N=N linkage, which is anionic in aqueous media and absorbs light in the visible region (450–550 nm) with an absorption maxima at 464 nm [33]. The samples obtained by TiN rod or TiN powder targets as well as those in which the TiN fraction is higher than the TiO2 one (75/25 ratio) are the most active nanocomposites, both under UV and visible irradiation. For the colloids going from the TiN rod, we observe that, in the first 20 min, 50% and 60% of the dye were removed under UV and visible light, respectively, while only about 10% of the dye is removed for the TiO2 colloid. Moreover, 70% of MO decolourization occurs within 80 min under visible irradiation while the other samples, for which Ti-O chemical bonds dominate in comparison to TiN/Ti-O-N ones, show significantly less efficiency in the same range of time.Figure 8
Photocatalytic activity towards the methyl orange (MO) dye molecule under UV and visible irradiation (60 min exposure time).
(a)(b)In order to have a quantitative estimation of the photocatalytic activity, we carried out a simple fitting procedure already adopted to test photodegradation efficiency of MB using zinc oxide nanocolloids, prepared by picosecond pulsed laser ablation, as catalysts [34]. If a semilogarithm scale of the relative absorbance as function of irradiation time is employed, it is possible to obtain a pseudoorder constant rate for all analyzed samples (see Table 2). In detail, by following the equation
(1)lnAA0=−kct,with A0 and At as the starting absorbance and the absorbance at the time t, respectively, a linear fitting procedure, limited to the first 30 minutes of irradiation, is evidence that both dyes degrade faster under the visible source and that the highest kc value is obtained with nanocatalysts from the TiN rod target.Table 2
Photodegradation rate constants of MB and MO with different catalysts usinglnA/A0=−kct as the fitting equation model.
Samplekc (min-1)MBMOUV lampVisible lampUV lampVisible lampTION5 (TiN rod target)-0.0118-0.0211-0.0333-0.0426TION1P (TiN powder target)-0.0129-0.0126-0.0300-0.0326TION5P (TiN/TiO2 (25/75) target)-0.0103-0.0242-0.0043-0.0176TION12P (TiN/TiO2 (75/25) target)-0.0139-0.0113-0.0153-0.0158TiO2 target-0.0091-0.0211-0.0026-0.0046Hence, on the basis of the obtained results, we suggest that the sample obtained from TiN characterized by the higher N content could be photosensitized by the “N-doping.” In this case, oxygen vacancies promoted the charge recombination, resulting in weak reduction power. Otherwise, the high activity of the sample synthesized from the TiN/TiO2 mixed powder in 25/75 ratio was attributed to the abundance of hydroxy groups in its porous structure (see STEM image), which provided more active sites for the degradation reaction as well as to the high available surface/volume ratio of the catalyst, since this sample shows a porous structure (Figure 3(a)). Nevertheless, no clear correlation between the MB or MO photocatalytic activity and the chemical-structural properties of the synthesized nanocolloids is found, since dye decolourization is also affected by the ionic nature, structure and stability, adsorption, and orientation of the dye molecules on the surface of the catalyst [35, 36]. The synthesized N-TiO2 nanocatalysts should be further investigated in depth to improve their catalytic response in the visible spectral region by a more rational and environment-friendly PLAL approach.


## 3.1. Sample Characterization

In Figure3 are shown representative STEM images of the samples obtained ablating in water targets of different nature. Specifically, the colloids, obtained ablating the (25/75) TiN/TiO2 powder targets, show a porous morphology with some spherical nanostructures with a mean diameter of about 50 nm (Figure 3(a)). It is to be noted that the observation of perfectly rounded submicrometer particles, probably associated with TiO2 species, is in agreement with what was observed by Felice et al. [21]. On the other hand, a high density of nanoparticles with a spherical shape and size mainly below 30 nm characterizes the colloids prepared ablating the high purity (99.99%) commercial TiN rod target (Figure 3(c)). An analogous morphology is shown by the colloids prepared ablating the TiN powder target (Figure 3(b)). More details can be observed from images d–h collected for the samples obtained ablating the (25/75) TiN/TiO2 powder targets and the TiN rod and powder targets.Figure 3
STEM images of the samples obtained ablating the (25/75) TiN/TiO2 powder targets (a, d, e), the TiN powder target (b, f), and the high purity (99.99%) commercial TiN rod target (c, g, h).
(a)(b)(c)(d)(e)(f)(g)(h)The sample obtained from the (25/75) mixed TiN/TiO2 powders show Raman features typical of the anatase-rich TiO2 material [6]. It is important to highlight that first-order Raman features of TiN (at 225 cm-1 (TA), 310 cm-1 (LA), and 540 cm-1(TO)) are almost absent, suggesting that nitrogen could be incorporated as a defect in the crystalline TiO2 lattice. Samples, obtained from TiN powder (red line) and rod (blue line) targets, showed very similar Raman spectra; in this case, TiN vibrational features are well observable (see Figure 4(a)) as indicated by the pronounced peak at about 550 cm-1 related to the TiN-TO mode [22]. Moreover, we observe that the Eg (associated to the anatase phase) signal below 200 cm-1 is totally absent and that the intensity ratio between the observed peaks at 200 and 290 cm-1 is very similar to that of a possible formation of a rutile TiO2 phase. Unfortunately, TiN and rutile features overlapped in this region, so a correct attribution for the rutile is not possible exclusively from Raman analyses. All this evidence indicates a tendency towards an anatase-rutile conversion and/or an oxygen replacement by nitrogen with the formation of Ti-N bonds [22]. Interstitial nitrogen species are expected as a result of the ablation of a TiN target in water.Figure 4
(a) Raman and (b) optical absorbance spectra of the synthesized samples.
(a)(b)In Figure4(b) are shown the optical absorbance spectra of the synthesized nanocolloids. We observe that (1) the colloid obtained by a TiN rod target is transparent (over 90%) in the visible range with a sharp absorption edge at about 350 nm, (2) a broad band at around 420 nm characterizes the sample prepared from the TiO2 powder target, and (3) a slight blue shift is evident in the colloids prepared using the pressed and sintered target with a (75/25) TiN/TiO2 mass ratio; for these samples, the 420 nm band is totally absent, while a significant visible light absorption contribution up to 600 nm is evident, probably due to the electronic transition from the localized N doping level to the conduction band of TiO2 (see also the scheme reported in Figure 5).Figure 5
Schematic diagram showing the valence and conduction bands of N-doped TiO2.The incorporation of nitrogen into the TiO2 lattice leads to the formation of a new midgap energy state, i.e., the N2p band above the O2p valence band. So, upon a visible light irradiation, the electrons can migrate from the valence band to the conduction band (Figure 5) and from here the expected visible light activity of N-dopedTiO2 or TiO2-xNx materials (see Catalytic Activities). Nitrogen can replace one or more oxygen atoms (“substitutional doping”), or nitrogen can be positioned in interstitial TiO2 sites (“interstitial doping”). In both cases, as shown in Figure 5, N doping leads to a change in the electronic behavior of the nanoparticle due to a change in the electronic band structures and/or a decrease of electron-hole recombination [23].XPS analysis allows investigating the surface chemical composition and bonding configurations of our samples, in which it is known that the surface chemical coordination greatly influences the catalytic response [24]. In Figures 6(a)–6(c) are shown representative Ti2p and N1s deconvoluted profiles, while the chemical atomic percentage of the detected species and the relative surface bonding configurations are reported in Table 1. Two different Ti2p profiles characterize our samples: those obtained starting from the TiN rod target (Figure 6(a)) show a broad band whose features are ascribed to the titanium nitride, the titanium dioxide (TiO2), and the intermediate phase of titanium oxynitride [25, 26]. Otherwise, in the samples obtained by the TiN powder (Figure 6(b)), narrower profiles are obtained and the binding energy of the Ti2p3/2 peak is brought closer to 458.5 eV (typical of TiO2 compound), while the binding energies of the other phases still fall within the possible ranges. Interestingly, no resolved N1s signal was collected from the powder targets while the N1s profile is well structured and defined for samples obtained from the rod targets (Figure 6(c)). The main components are located at around 396 and in the 397-400 eV range. These features are ascribed to the titanium oxynitride phase and to the nitrogen in substitutional and interstitial positions [26–31]. The NHx, NO/NO2, and NO3− contributions are generally reported at a binding energy higher than 400 eV [29–31] but, in our case, are less pronounced (see Figures 6(c) and 6(d)).Figure 6
Ti2p (a, b) deconvoluted profiles of the samples obtained from the TiN rod and TiN powder targets, respectively. We outline that all the samples obtained from the mixed powders show Ti2p line shapes similar to those of the sample starting from the TiN powder. The N1s deconvoluted profile of the sample obtained starting from the TiN rod target (c) and a scheme of the potential nitrogen allocation into the TiO2 structure (d).Table 1
Atomic surface chemical composition and bonding fraction estimated by the deconvoluted XPS spectra.
SampleChemical composition (%)Bonding configurations (%)Ti2pN1sN (%)Ti (%)O (%)Ti-NTi-O-NTi-O2N-Ti-ONsubst.Nint.NO/NO2TION1p1.128.870.10.86.492.8——100—TION5p0.728.471.00.53.596.0——100—TION12p5.923.870.30.93.495.7——100—TION17p4.619.875.60.03.796.3——100—TION312.228.859.115.526.058.567.418.59.54.6TION417.824.158.117.829.153.159.726.610.72.9TION514.825.759.617.430.152.665.522.09.92.7


## 3.2. Catalytic Activities

All the photocatalytic reactions were undertaken in air as the photobleaching of MB is irreversible in an oxygen-saturated aqueous solution such as ours, and in an ice bath to avoid degradation effects due to light irradiation-induced heating. The photodegradation was monitored by recording UV-visible extinction spectra as a function of light irradiation exposure time. The percentage of MB decolourization under ultraviolet and visible radiation for the synthesized and TiO2 reference samples is shown in Figure 7. Under UV and visible irradiation, all the produced nanostructures show a photocatalytic activity towards the degradation of methylene blue (MB) dye molecule. However, the response is comparable in all the samples under UV irradiation while, under the visible lamp, the estimated percentages differ by about 30%. In fact, for the samples obtained by ablating TiN powder and TiN/TiO2-mixed powder in 75/25 ratio, MB decolourization is about 45% but increases in the samples obtained from the TiN rod or from the TiN/TiO2-mixed powders at the 25/75 ratio. Photocatalytic decolourization behavior of MB dye (during visible irradiation, over the 1 h time frame of the experiment) seems to be influenced by the amount of N, Ti, and O and their bonding coordination and by the increasing absorption in the visible light region [32].Figure 7
Photocatalytic activity towards the methylene blue (MB) dye molecule under UV and visible irradiation (60 min exposure time).In Figure8 is shown the percentage of MO decolourization under UV and visible lamp for the synthesized and reference samples. MO is an azo dye characterized by a N=N linkage, which is anionic in aqueous media and absorbs light in the visible region (450–550 nm) with an absorption maxima at 464 nm [33]. The samples obtained by TiN rod or TiN powder targets as well as those in which the TiN fraction is higher than the TiO2 one (75/25 ratio) are the most active nanocomposites, both under UV and visible irradiation. For the colloids going from the TiN rod, we observe that, in the first 20 min, 50% and 60% of the dye were removed under UV and visible light, respectively, while only about 10% of the dye is removed for the TiO2 colloid. Moreover, 70% of MO decolourization occurs within 80 min under visible irradiation while the other samples, for which Ti-O chemical bonds dominate in comparison to TiN/Ti-O-N ones, show significantly less efficiency in the same range of time.Figure 8
Photocatalytic activity towards the methyl orange (MO) dye molecule under UV and visible irradiation (60 min exposure time).
(a)(b)In order to have a quantitative estimation of the photocatalytic activity, we carried out a simple fitting procedure already adopted to test photodegradation efficiency of MB using zinc oxide nanocolloids, prepared by picosecond pulsed laser ablation, as catalysts [34]. If a semilogarithm scale of the relative absorbance as function of irradiation time is employed, it is possible to obtain a pseudoorder constant rate for all analyzed samples (see Table 2). In detail, by following the equation
(1)lnAA0=−kct,with A0 and At as the starting absorbance and the absorbance at the time t, respectively, a linear fitting procedure, limited to the first 30 minutes of irradiation, is evidence that both dyes degrade faster under the visible source and that the highest kc value is obtained with nanocatalysts from the TiN rod target.Table 2
Photodegradation rate constants of MB and MO with different catalysts usinglnA/A0=−kct as the fitting equation model.
Samplekc (min-1)MBMOUV lampVisible lampUV lampVisible lampTION5 (TiN rod target)-0.0118-0.0211-0.0333-0.0426TION1P (TiN powder target)-0.0129-0.0126-0.0300-0.0326TION5P (TiN/TiO2 (25/75) target)-0.0103-0.0242-0.0043-0.0176TION12P (TiN/TiO2 (75/25) target)-0.0139-0.0113-0.0153-0.0158TiO2 target-0.0091-0.0211-0.0026-0.0046Hence, on the basis of the obtained results, we suggest that the sample obtained from TiN characterized by the higher N content could be photosensitized by the “N-doping.” In this case, oxygen vacancies promoted the charge recombination, resulting in weak reduction power. Otherwise, the high activity of the sample synthesized from the TiN/TiO2 mixed powder in 25/75 ratio was attributed to the abundance of hydroxy groups in its porous structure (see STEM image), which provided more active sites for the degradation reaction as well as to the high available surface/volume ratio of the catalyst, since this sample shows a porous structure (Figure 3(a)). Nevertheless, no clear correlation between the MB or MO photocatalytic activity and the chemical-structural properties of the synthesized nanocolloids is found, since dye decolourization is also affected by the ionic nature, structure and stability, adsorption, and orientation of the dye molecules on the surface of the catalyst [35, 36]. The synthesized N-TiO2 nanocatalysts should be further investigated in depth to improve their catalytic response in the visible spectral region by a more rational and environment-friendly PLAL approach.


## 4. Conclusions

In this work, the potentiality of the pulsed laser ablation in liquid (PLAL) technique to prepare N-TiO2-x nanocolloids, suitable for mechanical deposition on photoanode materials by conventional spraying technique, or to be incorporated in integrated solar water-splitting devices was reported. Synthesis processes were carried out in water, using targets with different nature and composition, to favour the formation of (Ti-O-N), (−NH2), NO2−, N2, NHx, and (−OH) species, and the nitrogen incorporation into the TiO2 lattice as nitride through dehydration. PLAL processes were performed in ambient condition (room temperature) using the water as solvent, without the need to provide high temperature (T) and pressures (P), thus preparing nanocolloids, ready to use without by-products. The observed photoactivity response of the synthesized nanocatalysts is explained in terms of their surface composition and bonding configurations and optical and morphological properties, which has been tuned changing the incorporation of nitrogen into the TiO2 lattice, beneficial for potentially separating the photogenerated carriers in space.



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