This article is about molecular photodissociation. The term "photodissociation" may also refer to nuclear photodissociation.
Photodissociation, photolysis, or photodecomposition is a chemical reaction in which a chemical compound is broken down by photons. It is defined as the interaction of one or more photons with one target molecule. Photodissociation is not limited to visible light. Any photon with sufficient energy can affect the chemical bonds of a chemical compound. Since a photon's energy is inversely proportional to its wavelength, electromagnetic waves with the energy of visible light or higher, such as ultraviolet light, x-rays and gamma rays are usually involved in such reactions.
Contents
- 1 Photolysis in photosynthesis
- 1.1 Energy transfer models
- 2 Photolysis in the atmosphere
- 3 Astrophysics
- 4 Atmospheric gamma-ray bursts
- 5 Multiple photon dissociation
- 6 See also
- 7 References
Photolysis in photosynthesis
Photolysis is part of the light-dependent reactions of photosynthesis. The general reaction of photosynthetic photolysis can be given as
H2A + 2 photons (light) → 2 e− + 2 H+ + A
The chemical nature of "A" depends on the type of organism. In purple sulfur bacteria, hydrogen sulfide (H2S) is oxidized to sulfur (S). In oxygenic photosynthesis, water (H2O) serves as a substrate for photolysis resulting in the generation of diatomic oxygen (O2). This is the process which returns oxygen to Earth's atmosphere. Photolysis of water occurs in the thylakoids of cyanobacteria and the chloroplasts of green algae and plants.
Energy transfer models
The conventional, semi-classical, model describes the photosynthetic energy transfer process as one in which excitation energy hops from light-capturing pigment molecules to reaction center molecules step-by-step down the molecular energy ladder.
The effectiveness of photons of different wavelengths depends on the absorption spectra of the photosynthetic pigments in the organism. Chlorophylls absorb light in the violet-blue and red parts of the spectrum, while accessory pigments capture other wavelengths as well. The phycobilins of red algae absorb blue-green light which penetrates deeper into water than red light, enabling them to photosynthesize in deep waters. Each absorbed photon causes the formation of an exciton (an electron excited to a higher energy state) in the pigment molecule. The energy of the exciton is transferred to a chlorophyll molecule (P680, where P stands for pigment and 680 for its absorption maximum at 680 nm) in the reaction center of photosystem II via resonance energy transfer. P680 can also directly absorb a photon at a suitable wavelength.
Photolysis during photosynthesis occurs in a series of light-driven oxidation events. The energized electron (exciton) of P680 is captured by a primary electron acceptor of the photosynthetic electron transfer chain and thus exits photosystem II. In order to repeat the reaction, the electron in the reaction center needs to be replenished. This occurs by oxidation of water in the case of oxygenic photosynthesis. The electron-deficient reaction center of photosystem II (P680*) is the strongest biological oxidizing agent yet discovered, which allows it to break apart molecules as stable as water.[1]
The water-splitting reaction is catalyzed by the oxygen evolving complex of photosystem II. This protein-bound inorganic complex contains four manganese ions, plus calcium and chloride ions as cofactors. Two water molecules are complexed by the manganese cluster, which then undergoes a series of four electron removals (oxidations) to replenish the reaction center of photosystem II. At the end of this cycle, free oxygen (O2) is generated and the hydrogen of the water molecules has been converted to four protons released into the thylakoid lumen.
These protons, as well as additional protons pumped across the thylakoid membrane coupled with the electron transfer chain, form a proton gradient across the membrane that drives photophosphorylation and thus the generation of chemical energy in the form of adenosine triphosphate (ATP). The electrons reach the P700 reaction center of photosystem I where they are energized again by light. They are passed down another electron transfer chain and finally combine with the coenzyme NADP+ and protons outside the thylakoids to NADPH. Thus, the net oxidation reaction of water photolysis can be written as:
2 H2O + 2 NADP+ + 8 photons (light) → 2 NADPH + 2 H+ + O2
The free energy change (ΔG) for this reaction is 102 kilocalories per mole. Since the energy of light at 700 nm is about 40 kilocalories per mole of photons, approximately 320 kilocalories of light energy are available for the reaction. Therefore, approximately one-third of the available light energy is captured as NADPH during photolysis and electron transfer. An equal amount of ATP is generated by the resulting proton gradient. Oxygen as a byproduct is of no further use to the reaction and thus released into the atmosphere.[2]
Quantum models
In 2007 a quantum model was proposed by Graham Fleming and his co-workers which includes the possibility that photosynthetic energy transfer might involve quantum oscillations, explaining its unusually high efficiency.[3]
According to Fleming[4] there is direct evidence that remarkably long-lived wavelike electronic quantum coherence plays an important part in energy transfer processes during photosynthesis, which can explain the extreme efficiency of the energy transfer because it enables the system to sample all the potential energy pathways, with low loss, and choose the most efficient one. This claim has, however, since been proven wrong in several publications [5] [6] [7] .[8][9]
This approach has been further investigated by Gregory Scholes and his team at the University of Toronto, which in early 2010 published research results that indicate that some marine algae make use of quantum-coherent electronic energy transfer (EET) to enhance the efficiency of their energy harnessing.[10][11][12]
Photolysis in the atmosphere
Photolysis occurs in the atmosphere as part of a series of reactions by which primary pollutants such as hydrocarbons and nitrogen oxides react to form secondary pollutants such as peroxyacyl nitrates. See photochemical smog.
The two most important photodissociaton reactions in the troposphere are firstly:
- O3 + hν → O2 + O(1D) λ < 320 nm
which generates an excited oxygen atom which can react with water to give the hydroxyl radical:
- O(1D) + H2O → 2 •OH
The hydroxyl radical is central to atmospheric chemistry as it initiates the oxidation of hydrocarbons in the atmosphere and so acts as a detergent.
Secondly the reaction:
- NO2 + hν → NO + O
is a key reaction in the formation of tropospheric ozone.
The formation of the ozone layer is also caused by photodissociation. Ozone in the Earth's stratosphere is created by ultraviolet light striking oxygen molecules containing two oxygen atoms (O2), splitting them into individual oxygen atoms (atomic oxygen). The atomic oxygen then combines with unbroken O2 to create ozone, O3. In addition, photolysis is the process by which CFCs are broken down in the upper atmosphere to form ozone-destroying chlorine free radicals.
Astrophysics
In astrophysics, photodissociation is one of the major processes through which molecules are broken down (but new molecules are being formed). Because of the vacuum of the interstellar medium, molecules and free radicals can exist for a long time. Photodissociation is the main path by which molecules are broken down. Photodissociation rates are important in the study of the composition of interstellar clouds in which stars are formed.
Examples of photodissociation in the interstellar medium are ( is the energy of a single photon of frequency ):
Atmospheric gamma-ray bursts
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Currently orbiting satellites detect an average of about one gamma-ray burst per day. Because gamma-ray bursts are visible to distances encompassing most of the observable universe, a volume encompassing many billions of galaxies, this suggests that gamma-ray bursts must be exceedingly rare events per galaxy.
Measuring the exact rate of gamma-ray bursts is difficult, but for a galaxy of approximately the same size as the Milky Way, the expected rate (for long GRBs) is about one burst every 100,000 to 1,000,000 years.[13] Only a few percent of these would be beamed towards Earth. Estimates of rates of short GRBs are even more uncertain because of the unknown beaming fraction, but are probably comparable.[14]
A gamma-ray burst in the Milky Way, if close enough to Earth and beamed towards it, could have significant effects on the biosphere. The absorption of radiation in the atmosphere would cause photodissociation of nitrogen, generating nitric oxide that would act as a catalyst to destroy ozone.[15]
The atmospheric photodissociation
- N2 -> 2N
- O2 -> 2O
- CO2 -> C + 2O
- H2O -> 2H + O
- 2NH3 -> 3H2 + N2
would yield
- NO2 (consumes up to 400 ozone molecules)
- CH2 (nominal)
- CH4 (nominal)
- CO2
(incomplete)
According to a 2004 study, a GRB at a distance of about a kiloparsec could destroy up to half of Earth's ozone layer; the direct UV irradiation from the burst combined with additional solar UV radiation passing through the diminished ozone layer could then have potentially significant impacts on the food chain and potentially trigger a mass extinction.[16][17] The authors estimate that one such burst is expected per billion years, and hypothesize that the Ordovician-Silurian extinction event could have been the result of such a burst.
There are strong indications that long gamma-ray bursts preferentially or exclusively occur in regions of low metallicity. Because the Milky Way has been metal-rich since before the Earth formed, this effect may diminish or even eliminate the possibility that a long gamma-ray burst has occurred within the Milky Way within the past billion years.[18] No such metallicity biases are known for short gamma-ray bursts. Thus, depending on their local rate and beaming properties, the possibility for a nearby event to have had a large impact on Earth at some point in geological time may still be significant.[19]
Multiple photon dissociation
Single photons in the infrared spectral range usually are not energetic enough for direct photodissociation of molecules. However, after absorption of multiple infrared photons a molecule may gain internal energy to overcome its barrier for dissociation. Multiple photon dissociation (MPD, IRMPD with infrared radiation) can be achieved by applying high power lasers, e.g. a carbon dioxide laser, or a free electron laser, or by long interaction times of the molecule with the radiation field without the possibility for rapid cooling, e.g. by collisions. The latter method allows even for MPD induced by black body radiation, a technique called blackbody infrared radiative dissociation (BIRD).
See also
- Flash photolysis
- Photocatalysis
- Photohydrogen
- Photochemistry
References
- ^ Campbell, Neil A.; Reece, Jane B. (2005). Biology (7th ed.). San Francisco: Pearson - Benjamin Cummings. pp. 186–191. ISBN 0-8053-7171-0.
- ^ Raven, Peter H.; Ray F. Evert; Susan E. Eichhorn (2005). Biology of Plants (7th ed.). New York: W.H. Freeman and Company Publishers. pp. 115–127. ISBN 0-7167-1007-2.
- ^ Gregory S. Engel, Tessa R. Calhoun, Elizabeth L. Read, Tae-Kyu Ahn, Tomáš Mančal, Yuan-Chung Cheng, Robert E. Blankenship and Graham R. Fleming, "Evidence for wavelike energy transfer through quantum coherence in photosynthetic systems", in Nature 446, 782-786 (12 April 2007)
- ^ http://www.physorg.com/news95605211.html Quantum secrets of photosynthesis revealed
- ^ R. Tempelaar; T. L. C. Jansen; J. Knoester (2014). "Vibrational Beatings Conceal Evidence of Electronic Coherence in the FMO Light-Harvesting Complex". J. Phys. Chem. B. 118 (45): 12865–12872. doi:10.1021/jp510074q.
- ^ N. Christenson; H. F. Kauffmann; T. Pullerits; T. Mancal (2012). "Origin of Long-Lived Coherences in Light-Harvesting Complexes". J. Phys. Chem. B. 116: 7449–7454.
- ^ E. Thyrhaug; K. Zidek; J. Dostal; D. Bina; D. Zigmantas (2016). "Exciton Structure and Energy Transfer in the Fenna−Matthews− Olson Complex". J. Phys. Chem. Lett. 7 (9): 1653–1660. doi:10.1021/acs.jpclett.6b00534.
- ^ A. G. Dijkstra; Y. Tanimura (2012). "The role of the environment time scale in light-harvesting efficiency and coherent oscillations". New J. Phys. 14 (7): 073027. doi:10.1088/1367-2630/14/7/073027.
- ^ D. M. Monahan; L. Whaley-Mayda; A. Ishizaki; G. R. Fleming (2015). "Influence of weak vibrational-electronic couplings on 2D electronic spectra and inter-site coherence in weakly coupled photosynthetic complexes". J. Chem. Phys. 143 (6): 065101. PMID 26277167. doi:10.1063/1.4928068.
- ^ Scholes Group Research
- ^ Gregory D. Scholes (7 January 2010), "Quantum-coherent electronic energy transfer: Did Nature think of it first?", Journal of Physical Chemistry Letters, 1 (1): 2–8, doi:10.1021/jz900062f
- ^ Elisabetta Collini; Cathy Y. Wong; Krystyna E. Wilk; Paul M. G. Curmi; Paul Brumer; Gregory D. Scholes (4 February 2010), "Coherently wired light-harvesting in photosynthetic marine algae at ambient temperature", Nature, 463 (7281): 644–7, Bibcode:2010Natur.463..644C, PMID 20130647, doi:10.1038/nature08811
- ^ Podsiadlowski 2004[dead link]
- ^ Guetta 2006[dead link]
- ^ Thorsett 1995[dead link]
- ^ Melott 2004[dead link]
- ^ Wanjek 2005[dead link]
- ^ Stanek 2006[dead link]
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