**2. Oxidation of hydrocarbon**

photosynthesis is a process in which fundamental scientific principles of natural photosynthe‐ sis are applied to design a solar energy conversion to make important chemicals by using manmadematerials.Manyapproachesarereported.Oneofthesuccessfulreportsprovidesanoutline for solar energy storage in fuels [2]. Another important approach is finding a new route for the chemical production and synthesis by utilizing solar energy, which is an energy-decisive industrial process. The method to synthesize organic chemical by photochemical process was first reported by Giacomo Ciamician in 1912 [3]. Presently, photochemistry is a well-devel‐ oped field of chemistry and the majority of the experiments use direct excitation of molecules by UV light [4]. To activate the photoreaction under visible light, sensitizers are applied, which transfer energy or an electron from the excited state to the molecule to be converted. Various homogeneous sensitizers are successfully used for various organic transformations [5]. The homogeneous sensitizers are substituted by heterogeneous photosensitizers using photocata‐ lytic process and which are easily separable and therefore recycled. In 1972, Fujishima and HondareportedaphotocatalyticprocessusingTiO2 semiconductoroxidee1ectrodestogenerate hydrogen from water [6]. Semiconductors can act as photocatalysts for light-induced chemi‐ cal transformations because of their unique electronic structure, which is characterized by a filledvalencebandandanemptyconductionband.Whenaphotonwithanenergyofhνmatches or exceeds the band gap energy (Eg) of the semiconductor (SC), an electron in the valence band

(VB) is promoted to the conduction band (CB), leaving a positive hole (h+

respectively. Subsequently, various oxidizing species such as •OH , O2

active oxygen species, such as HO2, H2O2 and O, are produced [8,9].

n

( ) ( ) ( ) ( ) *SC h SC h SC e vb cb*

Where SC is semiconductor, vb and cb represent the valance band and the conduction band,

The photo-excitation process over semiconductor photocatalyst is presented in **Figure 1**.

Different semiconductors (e.g., TiO2, ZnO, α-Fe2O3 and WO3) are considered for their potential use as photocatalysts. In early 1980s, great effort was placed on organic synthesis by semicon‐

+ - +® + (1)

are powerful oxidizing and reducing agents,

excitation can be written as [7]:

148 Applied Photosynthesis - New Progress

respectively. The reactive species, h+ and e<sup>−</sup>

**Figure 1** Semiconductor photocatalysed reaction.

) in VB. The photo-

•− , various forms of

Selective partial oxidation of hydrocarbon into its oxidation products, such as aldehyde, ketone, and carboxylic acid, by photocatalytic process is of great importance for chemical industries. Selective oxidation of methane into its useful oxygenates such as methanol and formaldehyde by photocatalytic method is of great challenge. Gondala et al. [13], for the first time, reported the photocatalytic transformation of methane into methanol over WO3, TiO2 (rutile) and NiO semiconductor photocatalysts, at room temperature, under the irradiation of a strong UV laser beam at 355 nm. The methanol yield in all three catalysts observed was low due to the degradation of methanol immediately after its formation in the aqueous suspension. Methane activation at low temperature and at atmospheric pressure using supported molyb‐ dena TiO2 catalyst [14] excited by band gap illumination motivated the researchers to test this reaction with various catalysts [15,16]. However, the conversion of methane was low and an advancement in the source of methane such as methane hydrates was used. Methane hydrates available in the ocean at depths between ~280 and 4000 m have higher concentration of methane in water, which is higher than that of water–methane pressurized systems. Compar‐ ison of photocatalytic conversion of methane dissolved in water and methane hydrate showed that the conversion of methane dissolved in water was observed at temperatures below 70°C. On the other hand, the photocatalytic conversions of the methane hydrate occurred at temperatures below −5°C [17]. The comparison of the photocatalytic reaction under visible and the full spectrum of UV-visible showed that the production of methanol was 50% greater in visible compared to that with the full spectrum lamp of UV-visible. Complete oxidation of methane could be avoided by changing the atmospheric condition. V-MCM-41 (acid) catalyst prepared under acidic conditions resulted in the selective formation of methanol with NO oxidant compared to O2 as oxidant under UV radiation accompanied by the formation of trace amounts of CO2 and acetaldehyde. Metal doping is used to improve the photocatalytic activity by avoiding charge recombination and to achieve visible-driven photocatalysis. Silverimpregnated WO3 was studied for the conversion of methane to methanol under laser illumination (100 mJ) in the aqueous medium [18]. The overall photonic efficiency of photo‐ catalytic conversion process based on hydroxyl radicals is ∼8%. The remaining portion of photogenerated hydroxyl radicals is consumed in oxygen formation, interaction with metha‐ nol, interaction with methanol by-products such as formaldehyde and recombination.

Photocatalytic oxidation of cyclohexane to cyclohexanol and cyclohexanone is an important commercial reaction, used as precursors in the synthesis of adipic acid and caprolactam, in turn used in the manufacture of nylon 66 and nylon 6, respectively. The selective oxidation of cyclohexane to cyclohexanol and cyclohexanone both under liquid and gaseous phase at room temperature and pressure by photocatalytic process was studied [10,19–21]. The product selectivity depends on the nature of the catalyst, irradiation wavelength and presence of solvent and O2, etc. The comparison of oxidation of cyclohexane with and without TiO2 photocatalyst showed that under photolytic oxidation at *λ* < 275 nm (i.e., in the absence of catalyst) yielded a high selectivity to cyclohexanol (>85%). However, under photocatalytic condition with TiO2 catalyst at *λ* < 275 nm, the selectivity shifted to the ketone (>95%) [21]. In cyclohexane oxidation, nature and composition of the solvent plays an important role in the distribution of products and by-products [20]. The composition of the mixed solvent has a strong influence on the selectivity of the process: an increase in the content of dichloromethane up to 50% brings an enhancement in the rate of formation of mono-oxygenated products. At the same time, the alcohol to ketone ratio increases in the mixed solvent. Studies performed with various polar and nonpolar solvents showed that in nonpolar solvents, cyclohexanol preferentially adsorbed onto the titanium dioxide particles and underwent deep oxidation, ultimately to carbon dioxide and water. Therefore, in nonpolar solvents, the selectivity of the reaction to cyclohexanol was very low. However, in polar solvents, cyclohexanol adsorbed to the titanium dioxide particles to a lesser extent due to the competition for adsorption sites with the solvent, and the selectivity of the reaction to cyclohexanol significantly increased. Of the various solvents studied such as acetone, isopropanol, dichloromethane, chloroform, carbon tetrachloride, benzene and n-hexane, dichloromethane was the best solvent with regard to the formation rate of cyclohexanol and cyclohexanone. The most unfavorable solvents were isopropanol, chloroform and benzene [21]. Studies under different O2 partial pressures showed that the process is unaffected for O2 partial pressures >200 Torr. For lower values, the formation of dicyclohexyl becomes significant and reaches a maximum at a pO2 of 60 Torr. In O2-free media containing C(NO2)4 as the electron scavenger, the formation of cyclohexanone decreases markedly while that of cyclohexanol is essentially the same as that in oxygenated media. Studies on cyclohexane photocatalytic oxidation with 18O2 over anatase TiO2 was analyzed by in situ attenuated total reflection Fourier transform infrared (ATR-FTIR) spectroscopy suggests that oxygen incorporated in cyclohexanone, as well as in deactivating carbonates and carboxylates, originates from the catalyst surface, rather than from dissolved O2. The proposed Mars-van Krevelen cycle is completed by regeneration of surface sites by reaction with 18O2 [22]. In studies conducted at dry nitrogen containing 10–20% of oxygen, cyclohexanone is produced with high selectivity (>90%). In humidified nitrogen/oxygen gas, the cyclohexanol selectivity was increased [23]. This suggests the participation of surface hydroxyl group in the reaction mechanism. A recent study by She et al. [24] showed that the Cl• radicals enhance the oxygenation of cyclohexane by N2O to cyclohexanone. Metal doping influences the catalytic activity and selectivity in the photocatalytic oxidation of cyclohexane. Silica-entrapped Cr catalyst for cyclohexane in acetonitrile prevents the decomposition of cyclohexane, there by increased selectivity was observed. The highest turnover number of 2.5 with cyclohexanone selectivity of 68% was observed. Increasing the Cr content resulted in red shift absorption between 500 and 800 nm, which is due to the d-d transition of octahedral Cr3+ in Cr2O3. Comparison of V-doped hollow TS-1, sulfated hollow TS-1 and sulfated V-doped hollow TS-1 demonstrated that sulfated V-doped TS-1 catalysts are more efficient for selective formation of valuable products (alcohols and ketones) [25].

## **3. Oxidation of alcohol**

impregnated WO3 was studied for the conversion of methane to methanol under laser illumination (100 mJ) in the aqueous medium [18]. The overall photonic efficiency of photo‐ catalytic conversion process based on hydroxyl radicals is ∼8%. The remaining portion of photogenerated hydroxyl radicals is consumed in oxygen formation, interaction with metha‐ nol, interaction with methanol by-products such as formaldehyde and recombination.

150 Applied Photosynthesis - New Progress

Photocatalytic oxidation of cyclohexane to cyclohexanol and cyclohexanone is an important commercial reaction, used as precursors in the synthesis of adipic acid and caprolactam, in turn used in the manufacture of nylon 66 and nylon 6, respectively. The selective oxidation of cyclohexane to cyclohexanol and cyclohexanone both under liquid and gaseous phase at room temperature and pressure by photocatalytic process was studied [10,19–21]. The product selectivity depends on the nature of the catalyst, irradiation wavelength and presence of solvent and O2, etc. The comparison of oxidation of cyclohexane with and without TiO2 photocatalyst showed that under photolytic oxidation at *λ* < 275 nm (i.e., in the absence of catalyst) yielded a high selectivity to cyclohexanol (>85%). However, under photocatalytic condition with TiO2 catalyst at *λ* < 275 nm, the selectivity shifted to the ketone (>95%) [21]. In cyclohexane oxidation, nature and composition of the solvent plays an important role in the distribution of products and by-products [20]. The composition of the mixed solvent has a strong influence on the selectivity of the process: an increase in the content of dichloromethane up to 50% brings an enhancement in the rate of formation of mono-oxygenated products. At the same time, the alcohol to ketone ratio increases in the mixed solvent. Studies performed with various polar and nonpolar solvents showed that in nonpolar solvents, cyclohexanol preferentially adsorbed onto the titanium dioxide particles and underwent deep oxidation, ultimately to carbon dioxide and water. Therefore, in nonpolar solvents, the selectivity of the reaction to cyclohexanol was very low. However, in polar solvents, cyclohexanol adsorbed to the titanium dioxide particles to a lesser extent due to the competition for adsorption sites with the solvent, and the selectivity of the reaction to cyclohexanol significantly increased. Of the various solvents studied such as acetone, isopropanol, dichloromethane, chloroform, carbon tetrachloride, benzene and n-hexane, dichloromethane was the best solvent with regard to the formation rate of cyclohexanol and cyclohexanone. The most unfavorable solvents were isopropanol, chloroform and benzene [21]. Studies under different O2 partial pressures showed that the process is unaffected for O2 partial pressures >200 Torr. For lower values, the formation of dicyclohexyl becomes significant and reaches a maximum at a pO2 of 60 Torr. In O2-free media containing C(NO2)4 as the electron scavenger, the formation of cyclohexanone decreases markedly while that of cyclohexanol is essentially the same as that in oxygenated media. Studies on cyclohexane photocatalytic oxidation with 18O2 over anatase TiO2 was analyzed by in situ attenuated total reflection Fourier transform infrared (ATR-FTIR) spectroscopy suggests that oxygen incorporated in cyclohexanone, as well as in deactivating carbonates and carboxylates, originates from the catalyst surface, rather than from dissolved O2. The proposed Mars-van Krevelen cycle is completed by regeneration of surface sites by reaction with 18O2 [22]. In studies conducted at dry nitrogen containing 10–20% of oxygen, cyclohexanone is produced with high selectivity (>90%). In humidified nitrogen/oxygen gas, the cyclohexanol selectivity was increased [23]. This suggests the participation of surface hydroxyl group in the reaction mechanism. A recent study by She et al. [24] showed that the Cl• radicals enhance the

Selective oxidation of various primary and secondary alcohols in a gas-phase photochemical reactor using immobilized TiO2 catalyst at 463 K showed that in the absence of UV light radiation 8% conversion was obtained [26]. Irradiation of the catalyst with the UV light increased the conversion dramatically to 48%. In the presence of UV light, benzaldehyde was formed in preference to phenyl acetaldehyde, in addition to small amounts of other secondary and tertiary reaction products. Benzylic alcohols gave higher conversions, however, with more secondary reaction products. The presence of oxygen was found to be critical for photooxidation. The conversion increased from 13 to 20% when a very small quantity of oxygen (O2/alcohol = 1) was added to the nitrogen carrier gas. There was significant improvement in the conversion, from 13 to 36%, when nitrogen was replaced by air as the carrier gas. Aldehyde is formed only in the presence of O2. Mohamed et al. [27] studied the photocatalytic oxidation of selected aryl alcohols, such as benzyl alcohol, 1-phenylethanol, benzhydrol, 4-chlorobenz‐ hydrol, hydrobenzoin, 4,4'-dichlorohydrobenzoi and 4,4'-dimethoxyhydrobenzoin, in a polar, nonhydroxylic solvent (CH3CN). The main products formed are aldehydes or ketones; the carboxylic acids are formed in small amount. The selective oxidation of alcohol to aldehyde by photocatalytic process was demonstrated for the conversion of 4-methoxybenzyl alcohol (MBA) into 4-methoxybenzaldehyde (p-anisaldehyde, PAA) in organic-free water containing aqueous suspensions of commercial and home-prepared TiO2 [28]. The home-prepared catalysts, obtained under mild conditions, showed to be much more selective than TiO2 Merck and TiO2 Degussa P25 with highest selectivity to PAA. The nanostructured anatase TiO2 samples synthesized by simply boiling the aqueous solutions of titanium tetrachloride (TiCl4) showed a yield much higher (42% mol for conversions of ca. 65%) than the commercial TiO2 samples. The least crystalline sample showed higher quantum efficiency (0.116%) [29]. Wang et al. [30] showed that the photocatalytic oxidation of alcohol with O2 is accelerated by Brønsted acids adsorbed onto TiO2 or TiO2/SiO2 photocatalysts.

The photocatalytic oxidation of benzyl alcohol and its derivatives, such as 4-methoxybenzyl alcohol, 4-chlorobenzyl alcohol, 4-nitrobenzyl alcohol, 4-methylbenzyl alcohol, 4-(trifluoro‐ methyl)benzyl alcohol and 4-tertiary-butylbenzyl alcohol, into corresponding aldehydes was achieved at stoichiometric conversion and selectivity (>99%) on a TiO2 photocatalyst under irradiation of light from a blue LED (*λ*max = 460 nm) in O2 atmosphere [31]. A red shift of the wavelength of light could be achieved by Au/CeO2, which exhibited stronger photo-absorption due to SPR than Au/TiO2 [32]. Aromatic alcohols (benzyl alcohol and substituted benzyl alcohol such as o-CH3, m-CH3 and p-CH3, m-Cl and p-Cl substituted benzyl alcohol) oxidized to corresponding aldehydes almost quantitatively (>99% conversion, >99% selectivity and >99% carbon balance), in an aqueous suspension of Au/CeO2 under irradiation of green light [33]. The electronic properties of the substituent groups play a very significant role on the reaction rate, which is enhanced by electron donating substituents and retarded by electronwithdrawing substituents [34].

#### **4. Hydroxylation of aromatics**

Conversion of benzene to phenol is an industrially important reaction. With TiO2 based photocatalysis, the yield and selectivity of phenol production from benzene were about ca. 0.5 and 80%, respectively [35], which are lower than the conventional Fenton process (5% and 80– 90%) [36]. The by-product formed in the photocatalytic oxidation of benzene is biphenol. The efficiency of the photocatalytic phenol synthesis can be enhanced by structural modification of the catalyst, and by using additives. Noble metal deposits on TiO2 surface often enhance the photocatalytic reactivity because they trap CB electrons with reducing charge pair recombi‐ nation and promoting interfacial electron transfer. Pt/TiO2 exhibited an enhanced yield (1.7 times, i.e., 4.4%) and selectivity (96%). The addition of various electron acceptors such as O2, Fe3+, H2O2, Ag+ and N2O further enhanced the yield and selectivity. TiO2 along with polyoxo‐ metalate PW12O403− increased the phenol production yield (i.e., 11 and 70% selectivity) [37]. Here, polyoxometalate performs dual roles of both as a photocatalyst and as an electron shuttle. 2 atom % vanadium incorporated into the lattice of disordered mesoporous titania, 1 wt% Au incorporated into Ti0.98V0.02O2 (TV2), showed two times higher activity than bare TV2 [38]. Zheng et al. [39] compared three photocatalysts M@TiO2 (M = Au, Pt, Ag) for the oxidation of benzene to phenol in aqueous phenol under visible light (*λ* ≥ 400 nm). Au@TiO2 exhibited a high yield (63%) and selectivity (91%) compared to Pt@TiO2-(yield = 34% and selectivity = 53%). Ag@TiO2-microspheres resulted in negligible activity. The optimum Au loading for higher yield and selectivity was 2 wt% in Au@TiO2 loading and this catalyst exhibited enhanced visible-light absorption as well as the strongest SPR effect. Comparison of the photocatalytic activity of Au@TiO2-nanosheets and Au@TiO2-microspheres showed that Au@TiO2-nano‐ sheets resulted in lower activity compared with that of Au@TiO2-microspheres. The Au@TiO2 microspheres produced a strong interaction between Au and TiO2. Comparison of the synthesis of Au@TiO2 by two different methods such as Ti3+ ion-assisted method and direct photodeposition route showed that the catalyst prepared by direct photodeposition route produced only traces of phenol. The direct photodeposition route leads to an inhomogeneous loading of noble metal on TiO2, and the Au NPs exhibit a wide size distribution in the range of 20–80 nm. By changing the hydrophobicity of the catalyst, the adsorption of reactants (benzene, hydrophobic) and the desorption of the desired products (phenol, hydrophilic) could be improved [40]. With this idea, titania is incorporated in hydrophobically modified mesocellular siliceous foam (MCF) and is used for the photocatalytic hydroxylation of benzene to phenol in aqueous solutions. The inner environment of the MCF cage was turned hydro‐ phobic by surface organo-grafting with silylation agent (TiO2-MCF/CH3). The hydrophobically modified TiO2@MCF/CH3/UV sample showed the highest phenol selectivity (70%) and phenol yield (12.5%) after 2 hours of irradiation. FeCl3 and mesoporous carbon nitride (FeCl3/mpg-C3N4) hybrids exhibited 38% benzene conversion with 97% selectivity for phenol under visible light [41], which is due to faster reduction of Fe3+ to Fe2+ by light-irradiated electrons from mpg-C3N4. Metal-exchanged BEA zeolites dispersed in benzene-acetonitrile-water mixtures at room temperature with O2 as oxidant showed that Pd2+-, Fe3+- and Cu2+-exchanged BEA were shown to be effective for the formation of phenols (hydroquinone, resorcinol, catechol and phenol) [42].

## **5. Epoxidation of alkenes**

due to SPR than Au/TiO2 [32]. Aromatic alcohols (benzyl alcohol and substituted benzyl alcohol such as o-CH3, m-CH3 and p-CH3, m-Cl and p-Cl substituted benzyl alcohol) oxidized to corresponding aldehydes almost quantitatively (>99% conversion, >99% selectivity and >99% carbon balance), in an aqueous suspension of Au/CeO2 under irradiation of green light [33]. The electronic properties of the substituent groups play a very significant role on the reaction rate, which is enhanced by electron donating substituents and retarded by electron-

Conversion of benzene to phenol is an industrially important reaction. With TiO2 based photocatalysis, the yield and selectivity of phenol production from benzene were about ca. 0.5 and 80%, respectively [35], which are lower than the conventional Fenton process (5% and 80– 90%) [36]. The by-product formed in the photocatalytic oxidation of benzene is biphenol. The efficiency of the photocatalytic phenol synthesis can be enhanced by structural modification of the catalyst, and by using additives. Noble metal deposits on TiO2 surface often enhance the photocatalytic reactivity because they trap CB electrons with reducing charge pair recombi‐ nation and promoting interfacial electron transfer. Pt/TiO2 exhibited an enhanced yield (1.7 times, i.e., 4.4%) and selectivity (96%). The addition of various electron acceptors such as O2,

metalate PW12O403− increased the phenol production yield (i.e., 11 and 70% selectivity) [37]. Here, polyoxometalate performs dual roles of both as a photocatalyst and as an electron shuttle. 2 atom % vanadium incorporated into the lattice of disordered mesoporous titania, 1 wt% Au incorporated into Ti0.98V0.02O2 (TV2), showed two times higher activity than bare TV2 [38]. Zheng et al. [39] compared three photocatalysts M@TiO2 (M = Au, Pt, Ag) for the oxidation of benzene to phenol in aqueous phenol under visible light (*λ* ≥ 400 nm). Au@TiO2 exhibited a high yield (63%) and selectivity (91%) compared to Pt@TiO2-(yield = 34% and selectivity = 53%). Ag@TiO2-microspheres resulted in negligible activity. The optimum Au loading for higher yield and selectivity was 2 wt% in Au@TiO2 loading and this catalyst exhibited enhanced visible-light absorption as well as the strongest SPR effect. Comparison of the photocatalytic activity of Au@TiO2-nanosheets and Au@TiO2-microspheres showed that Au@TiO2-nano‐ sheets resulted in lower activity compared with that of Au@TiO2-microspheres. The Au@TiO2 microspheres produced a strong interaction between Au and TiO2. Comparison of the synthesis of Au@TiO2 by two different methods such as Ti3+ ion-assisted method and direct photodeposition route showed that the catalyst prepared by direct photodeposition route produced only traces of phenol. The direct photodeposition route leads to an inhomogeneous loading of noble metal on TiO2, and the Au NPs exhibit a wide size distribution in the range of 20–80 nm. By changing the hydrophobicity of the catalyst, the adsorption of reactants (benzene, hydrophobic) and the desorption of the desired products (phenol, hydrophilic) could be improved [40]. With this idea, titania is incorporated in hydrophobically modified mesocellular siliceous foam (MCF) and is used for the photocatalytic hydroxylation of benzene to phenol in aqueous solutions. The inner environment of the MCF cage was turned hydro‐

and N2O further enhanced the yield and selectivity. TiO2 along with polyoxo‐

withdrawing substituents [34].

152 Applied Photosynthesis - New Progress

Fe3+, H2O2, Ag+

**4. Hydroxylation of aromatics**

Epoxidation of alkenes to epoxide is a very useful transformation in organic synthesis. A series of highly dispersed transition metals such as Ti4+, Cr6+, Mg2+ and Zn2+, in SiO2 matrix, exhibited photocatalytic activity for propene oxide formation [43]. Various studies reported on silica supported that metal oxide catalysts are effective photocatalysts for propylene epoxidation in a closed reactor system. Studies on silica supported on V, Ti and Cr showed that the conversion rate of propylene and the formation rate of propylene oxide were increased in the order Cr < Ti < V oxides on silica [44]. Gradual deactivation was observed for CrO3/SiO2 with the course of the photoreaction, although the initial activity was almost same as that of TiO2/SiO2. Shiraishi et al. [45] prepared Cr-SiO2 catalyst containing highly dispersed chromate species by a sol-gel method and when subjected to photocatalytic oxidation reaction under visible light irradiation (*λ* > 400 nm) showed very high selectivity (>90%), which is higher than Cr/SiO2 catalysts prepared by an impregnation method or Cr/MCM-41 prepared by a templating method. The yield and selectivity to propylene oxide were improved significantly by modification of silica with 1 wt% magnesium oxide loading [46]. Photo-oxidation of propene over V2O5/SiO2 with O2 under UV irradiation in a closed circulation reactor produced ethanal (acetaldehyde, AA), acrylaldehyde (AL) and propanal (propionaldehyde, PA). However, propene oxide was not detected as a product [47]. On the other hand, the same catalyst system with flow reactor system, which provide short contact time between the substrates and the catalysts produced acetaldehyde and propene oxide as main products; the selectivities were 43 and 30%, respec‐ tively [48]. The non-loaded amorphous SiO2 did not show any photocatalytic activity. It is clear that the surface vanadium oxide species are the photocatalytic active sites. Comparison of commercial and home-prepared TiO2 catalysts for partial photo-oxidation of cyclopentene oxidation produced cyclopent-2-en-1-one, cyclopent-2-en-1-ol, 6-oxabicyclo[3.1.0]hexane, penta-1,5-dial (glutaraldehyde) [49]. The commercial catalysts showed lower photo-activity in terms of cyclopentene conversion (51–57%) compared to the home-prepared ones (53–69%). The commercial photocatalyst produced ketone as the major fraction in the range of 35–49% and epoxide fraction in the range of 12–17%, while the home-prepared catalysts gave mainly the epoxide fraction in the range of 26–49% and ketone fraction in the range 9–16%. The difference in catalytic behavior of TiO2 commercial and TiO2 homemade is due to the difference in structural properties, which resulted in different reaction mechanisms. Selective epoxida‐ tion was achieved by Shiraishi et al. [50] in Ti-containing MCM-41 mesoporous silica (T-S) with isolated and tetrahedrally coordinated Ti-oxide species (Ti-O4), when photo-activated in acetonitrile (MeCN) with molecular oxygen. The high epoxide selectivity (>98%) of the T-S system is due to a "shield effect" driven by MeCN. TiO2 photocatalyst incorporated in highly hydrophobic Y zeolite under UV-light irradiation using molecular oxygen as an oxygen source exhibited a markedly enhanced photocatalytic activity compared with bare TiO2 [51].

#### **6. Oxidation of amines to imines**

In organic synthesis, selective oxidation of amines to imines are considered as important reactions, because imines and their derivatives have immense applications in the synthesis of nitrogen heterocycles, especially alkaloid synthesis, which are biologically important com‐ pounds. Lang et al. [52] have studied extensively and achieved highly selective photocatalytic conversion of various amines into its corresponding imines on TiO2 using 1 atm of air as the oxidant in acetonitrile under UV irradiation. It is documented that it is a challenging task to achieve high selectivity in water medium as complete degradation is potential to occur by over oxidation. The reaction rate in terms of conversion of amine is much higher in water medium than in CH3CN with high selectivity of imine formation [53]. However, the selectivity de‐ creased to some extent because of free radical intermediates, which are comparable to photocatalytic oxidation of amine in CH3CN. Studies on substituents' effect on the catalytic activity of amine to imine showed that substituents on the benzylic amines did not affect the selectivity significantly both in CH3CN and in water medium [59]. The presence of electrondonating substituents (CH3– and CH3O–) and electron withdrawing substituents (F– and Cl–) on the phenyl ring had little effect on the reaction rate and product selectivity of the oxidation reaction. The halo-substituted benzylamines provided good selectivity, as the halo-substituted positions along with the imine functionality are useful for further transformations. Compari‐ son of benzylic and nonbenzylic amines showed that no imines formation occurred in nonbenzylic amines such as cyclohexylamine and n-hexylamine and only fragmentation products were detected by unselective auto-oxidation at multiple reactive sites. Utilization of visible/solar energy is the prime concept to make the synthesis a economically and environ‐ mentally viable process. Nb2O5 converts amine to imine with high selectivity under visible light >390 nm to about 460 nm in benzene [54]. Studies on the photocatalytic activity and selectivity in the aerobic oxidation of benzylamine over various metal oxides illustrate that TiO2 exhibited higher yield than Nb2O5 and ZnO. However, the selectivity to N-benzylidene benzylamine was comparatively low because benzaldehyde was formed as a by-product. In V2O5, benzylamine-N-carbaldehyde was formed as a main by-product. Hiroaki Tada and his research group have used the "plasmon photocatalysts", in which noble metal nanoparticles are dispersed into semiconductor photocatalysts, which possesses two prominent features: a Schottky junction and localized surface plasmonic resonance (LSPR) [55]. Au NPs supported on various metal oxides (anatase and rutile TiO2, SrTiO3, ZnO, WO3, In2O3, Nb2O5) under visible-light irradiation (*λ* > 430 nm) showed that Au supported on rutile TiO2 exhibited high level of visible-light activity for aerobic oxidation of amines to yield the corresponding imines with high selectivity (>99%) compared to other supports. The high activity of Au NP on rutile TiO2 is due to multiple factors such as significant red shift of the LSPR peak of Au/ rutile TiO2 due to its very large permittivity (*ε* = 114) as compared with that of anatase TiO2 (*ε* = 48), smaller Au particle size, good adsorptivity of rutile TiO2 for amine owing to the presence of acid sites on the surface.

#### **7. Oxidation of polycyclic aromatic hydrocarbons**

isolated and tetrahedrally coordinated Ti-oxide species (Ti-O4), when photo-activated in acetonitrile (MeCN) with molecular oxygen. The high epoxide selectivity (>98%) of the T-S system is due to a "shield effect" driven by MeCN. TiO2 photocatalyst incorporated in highly hydrophobic Y zeolite under UV-light irradiation using molecular oxygen as an oxygen source

In organic synthesis, selective oxidation of amines to imines are considered as important reactions, because imines and their derivatives have immense applications in the synthesis of nitrogen heterocycles, especially alkaloid synthesis, which are biologically important com‐ pounds. Lang et al. [52] have studied extensively and achieved highly selective photocatalytic conversion of various amines into its corresponding imines on TiO2 using 1 atm of air as the oxidant in acetonitrile under UV irradiation. It is documented that it is a challenging task to achieve high selectivity in water medium as complete degradation is potential to occur by over oxidation. The reaction rate in terms of conversion of amine is much higher in water medium than in CH3CN with high selectivity of imine formation [53]. However, the selectivity de‐ creased to some extent because of free radical intermediates, which are comparable to photocatalytic oxidation of amine in CH3CN. Studies on substituents' effect on the catalytic activity of amine to imine showed that substituents on the benzylic amines did not affect the selectivity significantly both in CH3CN and in water medium [59]. The presence of electrondonating substituents (CH3– and CH3O–) and electron withdrawing substituents (F– and Cl–) on the phenyl ring had little effect on the reaction rate and product selectivity of the oxidation reaction. The halo-substituted benzylamines provided good selectivity, as the halo-substituted positions along with the imine functionality are useful for further transformations. Compari‐ son of benzylic and nonbenzylic amines showed that no imines formation occurred in nonbenzylic amines such as cyclohexylamine and n-hexylamine and only fragmentation products were detected by unselective auto-oxidation at multiple reactive sites. Utilization of visible/solar energy is the prime concept to make the synthesis a economically and environ‐ mentally viable process. Nb2O5 converts amine to imine with high selectivity under visible light >390 nm to about 460 nm in benzene [54]. Studies on the photocatalytic activity and selectivity in the aerobic oxidation of benzylamine over various metal oxides illustrate that TiO2 exhibited higher yield than Nb2O5 and ZnO. However, the selectivity to N-benzylidene benzylamine was comparatively low because benzaldehyde was formed as a by-product. In V2O5, benzylamine-N-carbaldehyde was formed as a main by-product. Hiroaki Tada and his research group have used the "plasmon photocatalysts", in which noble metal nanoparticles are dispersed into semiconductor photocatalysts, which possesses two prominent features: a Schottky junction and localized surface plasmonic resonance (LSPR) [55]. Au NPs supported on various metal oxides (anatase and rutile TiO2, SrTiO3, ZnO, WO3, In2O3, Nb2O5) under visible-light irradiation (*λ* > 430 nm) showed that Au supported on rutile TiO2 exhibited high level of visible-light activity for aerobic oxidation of amines to yield the corresponding imines with high selectivity (>99%) compared to other supports. The high activity of Au NP on rutile

exhibited a markedly enhanced photocatalytic activity compared with bare TiO2 [51].

**6. Oxidation of amines to imines**

154 Applied Photosynthesis - New Progress

Polycyclic aromatic compounds (PHA) are compounds containing multiple aromatic rings which are fused together. The highly efficient photocatalytic method was adopted to various PAHs and it was found that it can be degraded under UV or visible light irradiation [56]. The reaction mechanism illustrated that the toxic PAHs degraded through various useful inter‐ mediates. The selectivity of the product depends on the type of catalysts used. Other factors which influence the catalytic activity are solvent medium, atmospheric condition and wave length of light radiation, etc. Photocatalytic oxidation of naphthalene in water medium with Degussa P25 under UV radiation (345 nm, 500 Watt) produced 2-formyl-3-hydroxycinnamal‐ dehyde and 5,8-dihydroxy-2,4-naphthaquinone as stable intermediates [57]. Bahnemann and coworkers found 15 different intermediates when naphthalene is in water medium with Degussa P25 under UV radiation (366 nm, 50 Watt) [56]. The main intermediates observed are coumarin, 1,4-naphthalenedione, 2,3-dihydro-2,3-epoxy-1,4-naphthalenedione, 2-formyl-Zcinnamaldehyde, 1,2-benzenedicarboxaldehyde and phthalic acid. Karam et al. synthesized 1,4-naphthaquinone in a closed system reactor under UV radiation [58]. Solvent plays an important role in the photocatalytic degradation of naphthalene. In water containing 1% MeCN produced significant amounts of three intermediates: isomeric 2-formylcinnamalde‐ hydes and 1,4-naphthoquinone. In organic solvent, the oxidation rate was almost an order of magnitude slower than in water and produced significant amount of naphthoquinone and phthalic anhydride [59]. In acetonitrile and water mixture, with UV light (*λ* < 340 nm) produced 2-formylcinnamaldehyde (85%), Z isomer is the original product that is spontaneously transformed into the thermodynamically more stable E isomer. Addition of acetone can cause an accumulation of intermediates. For example, higher concentrations and more types of intermediates were found in degradation of naphthalene with the high acetone level [60]. In mixed solvents such as acetonitrile and water bubbled with molecular oxygen, naphthalene is efficiently oxidized to 2-formylcinnamaldehyde when irradiated with 500 W super-highpressure mercury lamp (*λ* < 340 nm) light [61]. Under the same condition, phenanthrene was converted into a coumarin compound with 45% yield [62]. Photocatalytic activity of different kinds of TiO2 powders for naphthalene oxidation showed that Degussa P25 TiO2 powders, which contain mixture of anatase and rutile, showed the highest photocatalytic activity for the production of 2-formylcinnamaldehyde from naphthalene. Similarly, powders containing both rutile and anatase phases showed high activity, even if the component of the anatase phase is a few percent. Pure anatase particles and pure rutile particles exhibited lower activity for the photocatalytic oxidation of naphthalene into 2-formylcinnamaldehyde [63]. Visible active photocatalysts are developed to convert the PAHs to useful compounds. Kohtani and coworkers showed that BiVO4 (band gap 2.4 eV) [64] and Ag-loaded BiVO4 photocatalysts are visible light-driven for photo-oxidation of various PAHs in acetonitrile in O2 atmosphere. Compared to pure BiVO4, Ag-loaded BiVO4 photocatalyst remarkably improves adsorptive and photo-oxidative performance on the degradation. Anthraquinone is obtained in both pure and Ag-loaded BiVO4 solutions, while the amount of formation using Ag-BiVO4 is much larger than that using pure BiVO4. Anthrone is obtained only from the irradiated Ag-BiVO4 solution but not from the pure BiVO4 one. The amount of anthraquinone formation is largest in O2 saturated solution compared to that in N2 atmosphere. Bz[a]A was degraded by Ag-BiVO4 and converted into a considerable amount of 7,12-dione. Substituent effects on the photocatalytic oxidation of naphthalene demonstrate that in dinitronaphthalene isomers, namely 1,3 dinitronaphthalene (1,3-diNN), 1,5-dinitronaphthalene (1,5-diNN) and 1,8-dinitronaphtha‐ lene (1,8-diNN), the photocatalytic oxidation rates followed in the order 1,3-diNN > 1,8-diNN > 1,5-diNN [65].
