Photocatalysis

In chemistry, photocatalysis is the acceleration of a photoreaction in the presence of a catalyst. In catalysed photolysis, light is absorbed by an adsorbed substrate. In photogenerated catalysis, the photocatalytic activity (PCA) depends on the ability of the catalyst to create electron–hole pairs, which generate free radicals (e.g. hydroxyl radicals: •OH) able to undergo secondary reactions. Its practical application was made possible by the discovery of water electrolysis by means of titanium dioxide. The commercially used process is called the advanced oxidation process (AOP). There are several ways the AOP can be carried out; these may (but do not necessarily) involve TiO2 or even the use of UV light. Generally the defining factor is the production and use of the hydroxyl radical.

In the experiment above, photons from a light source (out of frame on the right hand side) are absorbed by the surface of the titanium dioxide disc, exciting electrons within the material. These then react with the water molecules, splitting it into its constituents of hydrogen and oxygen. In this experiment, chemicals dissolved in the water prevent the formation of oxygen, which would otherwise recombine with the hydrogen.

Types of photocatalysis

Homogeneous photocatalysis

In homogeneous photocatalysis, the reactants and the photocatalysts exist in the same phase. The most commonly used homogeneous photocatalysts include ozone and photo-Fenton systems (Fe+ and Fe+/H2O2). The reactive species is the •OH which is used for different purposes. The mechanism of hydroxyl radical production by ozone can follow two paths.[1]

O3 + hν → O2 + O(1D) (? O3 "-" hν → O2 + O(1D) ?)
O(1D) + H2O → •OH + •OH
O(1D) + H2O → H2O2
H2O2 + hν → •OH + •OH

Similarly, the Fenton system produces hydroxyl radicals by the following mechanism[2]

Fe2+ + H2O2→ HO• + Fe3+ + OH
Fe3+ + H2O2→ Fe2+ + HO•2 + H+
Fe2+ + HO• → Fe3+ + OH

In photo-Fenton type processes, additional sources of OH radicals should be considered: through photolysis of H2O2, and through reduction of Fe3+ ions under UV light:

H2O2 + hν → HO• + HO•
Fe3+ + H2O + hν → Fe2+ + HO• + H+

The efficiency of Fenton type processes is influenced by several operating parameters like concentration of hydrogen peroxide, pH and intensity of UV. The main advantage of this process is the ability of using sunlight with light sensitivity up to 450 nm, thus avoiding the high costs of UV lamps and electrical energy. These reactions have been proven more efficient than the other photocatalysis but the disadvantages of the process are the low pH values which are required, since iron precipitates at higher pH values and the fact that iron has to be removed after treatment.

Heterogeneous photocatalysis

Heterogeneous catalysis has the catalyst in a different phase from the reactants. Heterogeneous photocatalysis is a discipline which includes a large variety of reactions: mild or total oxidations, dehydrogenation, hydrogen transfer, 18O216O2 and deuterium-alkane isotopic exchange, metal deposition, water detoxification, gaseous pollutant removal, etc.

Most common heterogeneous photocatalysts are transition metal oxides and semiconductors, which have unique characteristics. Unlike the metals which have a continuum of electronic states, semiconductors possess a void energy region where no energy levels are available to promote recombination of an electron and hole produced by photoactivation in the solid. The void region, which extends from the top of the filled valence band to the bottom of the vacant conduction band, is called the band gap.[3] When a photon with energy equal to or greater than the materials band gap is absorbed by the semiconductor, an electron is excited from the valence band to the conduction band, generating a positive hole in the valence band. The excited electron and hole can recombine and release the energy gained from the excitation of the electron as heat. Recombination is undesirable and leads to an inefficient photocatalyst. The ultimate goal of the process is to have a reaction between the excited electrons with an oxidant to produce a reduced product, and also a reaction between the generated holes with a reductant to produce an oxidized product. Due to the generation of positive holes and electrons, oxidation-reduction reactions take place at the surface of semiconductors. In the oxidative reaction, the positive holes react with the moisture present on the surface and produce a hydroxyl radical.

Oxidative reactions due to photocatalytic effect:

UV + MO → MO (h + e)

Here MO stands for metal oxide ---

h+ + H2O → H+ + •OH
2 h+ + 2 H2O → 2 H+ + H2O2
H2O2→ HO• + •OH

The reductive reaction due to photocatalytic effect:

e + O2 → •O2
•O2− + HO•2 + H+ → H2O2 + O2
HOOH → HO• + •OH

Ultimately, the hydroxyl radicals are generated in both the reactions. These hydroxyl radicals are very oxidative in nature and non selective with redox potential of (E0 = +3.06 V)[4]

Applications

Quantification of Photocatalytic Activity

ISO 22197 -1:2007 specifies a test method for the determination of the nitric oxide removal performance of materials that contain a photocatalyst or have photocatalytic films on the surface.[18]

Specific FTIR systems are used to characterise photocatalytic activity and/or passivity especially with respect to Volatile Organic Compounds VOCs and representative matrices of the binders applied.[19]

Recent studies show that mass spectrometry can be a powerful tool to determine photocatalytic activity of certain materials by following the decomposition of gaseous pollutants such as nitrogen oxides or carbon dioxide [20]

See also

References

  1. Wu, CH; Chang, CL (2006). "Decolorization of Reactive Red 2 by advanced oxidation processes: Comparative studies of homogeneous and heterogeneous systems". Journal of hazardous materials 128 (2–3): 265–72. doi:10.1016/j.jhazmat.2005.08.013. PMID 16182444.
  2. Peternel, IT; Koprivanac, N; Bozić, AM; Kusić, HM (2007). "Comparative study of UV/TiO2, UV/ZnO and photo-Fenton processes for the organic reactive dye degradation in aqueous solution". Journal of hazardous materials 148 (1–2): 477–84. doi:10.1016/j.jhazmat.2007.02.072. PMID 17400374.
  3. Linsebigler, Amy L.; Lu, Guangquan.; Yates, John T. (1995). "Photocatalysis on TiO2 Surfaces: Principles, Mechanisms, and Selected Results". Chemical Reviews 95 (3): 735–758. doi:10.1021/cr00035a013.
  4. Daneshvar, N; Salari, D; Khataee, A.R (2004). "Photocatalytic degradation of azo dye acid red 14 in water on ZnO as an alternative catalyst to TiO2". Journal of Photochemistry and Photobiology A: Chemistry 162 (2–3): 317–322. doi:10.1016/S1010-6030(03)00378-2.
  5. Kudo, Akihiko; Kato, Hideki; Tsuji, Issei (2004). "Strategies for the Development of Visible-light-driven Photocatalysts for Water Splitting". Chemistry Letters 33 (12): 1534. doi:10.1002/chin.200513248.
  6. "Snapcat Photo Catalytic Oxidation with Titanium Dioxide (2005)". CaluTech UV Air. Retrieved 2006-12-05.
  7. Kondrakov AO, Ignatev AN, Lunin VV, Frimmel FH, Braese S, Horn H (2016). "Roles of water and dissolved oxygen in photocatalytic generation of free OH radicals in aqueous TiO2 suspensions: An isotope labeling study". Applied Catalysis B: Environmental 182: 424–430. doi:10.1016/j.apcatb.2015.09.038.
  8. "Photocatalysis Applications of Titanium Dioxide TiO2". Titanium Information. titaniumart.com.
  9. Kondrakov AO, Ignatev AN, Frimmel FH, Braese S, Horn H, Revelsky AI (2014). "Formation of genotoxic quinones during bisphenol A degradation by TiO2 photocatalysis and UV photolysis: A comparative study". Applied Catalysis B: Environmental 160: 106–114. doi:10.1016/j.apcatb.2014.05.007.
  10. McCullagh C, Robertson JMC, Bahnemann DW, Robertson PKJ (2007). "The application of TiO2 photocatalysis for disinfection of water contaminated with pathogenic micro-organisms: a review". Research on Chemical Intermediates 33 (3–5): 359–375. doi:10.1163/156856707779238775.
  11. Hanaor, Dorian A. H.; Sorrell, Charles C. (2014). "Sand Supported Mixed-Phase TiO2 Photocatalysts for Water Decontamination Applications". Advanced Engineering Materials 16 (2): 248–254. doi:10.1002/adem.201300259.
  12. Cushnie TPT, Robertson PKJ, Officer S, Pollard PM, Prabhu R, McCullagh C, Robertson JMC (2010). "Photobactericidal effects of TiO2 thin films at low temperature". Journal of Photochemistry and Photobiology A: Chemistry 216 (2-3): 290–294. doi:10.1016/j.jphotochem.2010.06.027.
  13. Kostedt IV, William L.; Jack Drwiega; David W. Mazyck; Seung-Woo Lee; Wolfgang Sigmund; Chang-Yu Wu; Paul Chadik (2005). "Magnetically agitated photocatalytic reactor for photocatalytic oxidation of aqueous phase organic pollutants". Environmental Science & Technology (American Chemical Society) 39 (20): 8052–8056. doi:10.1021/es0508121.
  14. Tan, S. S.; L. Zou; E. Hu (2006). "Photocatalytic reduction of carbon dioxide into gaseous hydrocarbon using TiO2 pellets". Catalysis Today 115: 269–273. doi:10.1016/j.cattod.2006.02.057.
  15. Yao, Y. Yao; G. Li; S. Ciston; R. M. Lueptow; K. Gray (2008). "Photoreactive TiO2/Carbon Nanotube Composites: Synthesis and Reactivity". Environmental Science & Technology (American Chemical Society) 42 (13): 4952–4957. doi:10.1021/es800191n.
  16. Linsebigler, A. L.; G. Lu; J.T. Yates (1995). "Photocatalysis on TiO2 Surfaces: Principles, Mechanisms, and Selected Results". Chemical Reviews 95 (3): 735–758. doi:10.1021/cr00035a013.
  17. Science News
  18. ISO 22197-1:2007
  19. Unique Gas Analyser Helps to Characterize Photoactive Pigments
  20. Manuel Nuño, Richard J. Ball and Chris R. Bowen. "Study of solid/gas phase photocatalytic reactions by electron ionization mass spectrometry" J Mass Spec, 2014, 49 (8), p. 716-726
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