Relevant bibliographies by topics / Hydrocarbons. Photochemistry

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  2. Dissertations / Theses
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Academic literature on the topic 'Hydrocarbons. Photochemistry'

Author: Grafiati
Published: 4 June 2021
Last updated: 14 February 2022

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Journal articles on the topic "Hydrocarbons. Photochemistry"

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Luspay-Kuti, Adrienn, Kathleen Mandt, Kandis-Lea Jessup, et al. "Photochemistry on Pluto – I. Hydrocarbons and aerosols." Monthly Notices of the Royal Astronomical Society 472, no. 1 (2017): 104–17. http://dx.doi.org/10.1093/mnras/stx1362.

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Yu, Hongtao. "ENVIRONMENTAL CARCINOGENIC POLYCYCLIC AROMATIC HYDROCARBONS: PHOTOCHEMISTRY AND PHOTOTOXICITY." Journal of Environmental Science and Health, Part C 20, no. 2 (2002): 149–83. http://dx.doi.org/10.1081/gnc-120016203.

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Ostojic, Bojana D., and Dragana S. Dordevic. "Photochemistry of Nitrated Polycyclic Aromatic Hydrocarbons under Solar Radiation." Current Organic Chemistry 22, no. 10 (2018): 973–86. http://dx.doi.org/10.2174/1385272821666171116161755.

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Chemerisov, S. D., D. W. Werst, and A. D. Trifunac. "Photoionization and Energy-Dependent Photochemistry of Hydrocarbons in Zsm5†." Research on Chemical Intermediates 25, no. 6 (1999): 583–97. http://dx.doi.org/10.1163/156856799x00572.

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Plummer, Benjamin F. "Structure and Photochemistry of Cyclopentene Fused Polycyclic Aromatic Hydrocarbons." Polycyclic Aromatic Compounds 3, no. 2 (1993): 77–88. http://dx.doi.org/10.1080/10406639308047860.

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Bouwman, J., A. L. Mattioda, H. Linnartz, and L. J. Allamandola. "Photochemistry of polycyclic aromatic hydrocarbons in cosmic water ice." Astronomy & Astrophysics 525 (December 3, 2010): A93. http://dx.doi.org/10.1051/0004-6361/201015059.

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Bouwman, J., H. M. Cuppen, M. Steglich, L. J. Allamandola, and H. Linnartz. "Photochemistry of polycyclic aromatic hydrocarbons in cosmic water ice." Astronomy & Astrophysics 529 (March 30, 2011): A46. http://dx.doi.org/10.1051/0004-6361/201015762.

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Dobrijevic, M., T. Cavalié, E. Hébrard, F. Billebaud, F. Hersant, and F. Selsis. "Key reactions in the photochemistry of hydrocarbons in Neptune's stratosphere." Planetary and Space Science 58, no. 12 (2010): 1555–66. http://dx.doi.org/10.1016/j.pss.2010.07.024.

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Baird, N. Colin, Anthony M. Draper, and Paul de Mayo. "Surface photochemistry: Semiconductor mediated reactions of some saturated strained hydrocarbons." Canadian Journal of Chemistry 66, no. 7 (1988): 1579–88. http://dx.doi.org/10.1139/v88-256.

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Quadricyclane (1) and 1,8-bishoniocubane (2) have been found to undergo valence isomerization to norborndiene and tricyclo[4.2.2.02,5]deca-3,7-diene, respectively, on illuminated CdS and ZnO. An electron transfer mechanism is proposed. Quantum yield, solvent effects, the role of oxygen, and the quenching of the reaction were investigated, and were consistent with this interpretation. The thermal reaction of 1 on CdS was also suggested to be an electron transfer process involving, in this case, defects or trapped holes on the surface of the semiconductor. An examination of a series of strained
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Leigh, William J. "Techniques and applications of far-UV photochemistry in solution. The photochemistry of the C3H4 and C4H6 hydrocarbons." Chemical Reviews 93, no. 1 (1993): 487–505. http://dx.doi.org/10.1021/cr00017a021.

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Dissertations / Theses on the topic "Hydrocarbons. Photochemistry"

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Suh, Inseon. "Photochemistry of aromatic hydrocarbons: implications for ozone and secondary organic aerosol formation." Texas A&M University, 2003. http://hdl.handle.net/1969.1/3893.

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Aromatic hydrocarbons constitute an important fraction (~20%) of total volatile organic compounds (VOCs) in the urban atmosphere. A better understanding of the aromatic oxidation and its association in urban and regional ozone and organic aerosol formation is essential to assess the urban air pollution. This dissertation consists of two parts: (1) theoretical investigation of the toluene oxidation initiated by OH radical using quantum chemical and kinetic calculations to understand the mechanism of O3 and SOA precursors and (2) experimental investigation of atmospheric new particle formation f
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Gong, Xingyi. "A comparison of NMHC oxidation mechanisms using specified gas mixtures and trace-P field data." Diss., Available online, Georgia Institute of Technology, 2005, 2005. http://etd.gatech.edu/theses/available/etd-11142005-045424/.

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Thesis (Ph. D.)--Earth and Atmospheric Sciences, Georgia Institute of Technology, 2006.<br>Davis, Douglas, Committee Chair ; Cunnold, Derek, Committee Member ; Mulholland, James, Committee Member ; Wang, Yuhang, Committee Member ; Wine, Paul, Committee Member. Vita. Includes bibliographical references.
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Fortner, Jason C. "Illuminating whole effluent toxicity testing : ultraviolet radiation, phototoxicity, and PAH-contaminated groundwater /." Online version, 2009. http://content.wwu.edu/cdm4/item_viewer.php?CISOROOT=/theses&CISOPTR=314&CISOBOX=1&REC=10.

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Sharma, Divya. "Computational investigation of the photochemistry and spectroscopy of cyclic aromatic hydrocarbons in interstellar ice analogs." Thesis, Heriot-Watt University, 2015. http://hdl.handle.net/10399/2965.

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This thesis describes the photochemistry and ultraviolet (UV) spectroscopy of cyclic aromatic hydrocarbons such as benzene and naphthalene, along with small water clusters and crystalline water ice clusters. Firstly, benzene and naphthalene interactions with small water hexamer (W6) clusters, and then benzene interactions with crystalline water ice clusters are investigated. This thesis primarily focuses on the applications of a range of computational chemistry techniques to investigate and characterize excited states of these complex systems, which are generated following one-photon absorptio
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Jacobs, Laura Elizabeth. "Photochemical Transformation of Three Polycyclic Aromatic Hydrocarbons, Ibuprofen, and Caffeine in Natural Waters." The Ohio State University, 2008. http://rave.ohiolink.edu/etdc/view?acc_num=osu1213299624.

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Kuhlmann, Rolf von. "Tropospheric photochemistry of ozone, its precursors and the hydroxyl radical a 3d-modeling study considering non-methane hydrocarbons /." [S.l.] : [s.n.], 2001. http://ArchiMeD.uni-mainz.de/pub/2001/0141/diss.pdf.

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Rocha, Otidene Rossiter S? da. "Avalia??o de diferentes processos oxidativos avan?ados no tratamento de res?duos de petr?leo." Universidade Federal do Rio Grande do Norte, 2010. http://repositorio.ufrn.br:8080/jspui/handle/123456789/15902.

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Made available in DSpace on 2014-12-17T15:01:50Z (GMT). No. of bitstreams: 1 OtideneRSR_DISSERT.pdf: 1647726 bytes, checksum: 2a45d120fb2b82e3a84f67c77eff85a3 (MD5) Previous issue date: 2010-09-01<br>Conselho Nacional de Desenvolvimento Cient?fico e Tecnol?gico<br>The petroleum industry deals with problems which are difficult to solve because of their relation to environmental issues. This is because amounts of residue are generated which vary in type and danger level. The soil contamination by non aqueous liquid phase mixtures, specifically hydrocarbon petroleum has been a reason for great
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Kuhlmann, Rolf von [Verfasser]. "Tropospheric photochemistry of ozone, its precursors and the hydroxyl radical : a 3d-modeling study considering non-methane hydrocarbons / Rolf von Kuhlmann." 2001. http://d-nb.info/963248766/34.

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Books on the topic "Hydrocarbons. Photochemistry"

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Jeffries, H. E. Technical discussion related to the choice of photolytic rates for carbon bond mechanisms in OZIPM4/EKMA. U.S. Environmental Protection Agency, Office of Air and Radiation, Office of Air Quality Planning and Standards, 1987.

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Dibben, Mark J. Fourier transform ion cyclotron resonance mass spectrometry investigation of the photolysis of polycyclic aromatic hydrocarbons. 2001.

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Book chapters on the topic "Hydrocarbons. Photochemistry"

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Lipp, Benjamin, and Till Opatz. "Aromatic hydrocarbons as catalysts and mediators in photoinduced electron transfer reactions." In Photochemistry. Royal Society of Chemistry, 2018. http://dx.doi.org/10.1039/9781788013598-00370.

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Niki, Hiromi, and Paul D. Maker. "Atmospheric Reactions Involving Hydrocarbons: Long Path-FTIR Studies." In Advances in Photochemistry. John Wiley & Sons, Inc., 2007. http://dx.doi.org/10.1002/9780470133453.ch2.

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Kevan, Larry, and W. F. Libby. "The Chemistry of Ionic States in Solid Saturated Hydrocarbons." In Advances in Photochemistry. John Wiley & Sons, Inc., 2007. http://dx.doi.org/10.1002/9780470133323.ch5.

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Koppmann, R., C. Plass-Dülmer, B. Ramacher, et al. "Measurements of Carbon Monoxide and Nonmethane Hydrocarbons During POPCORN." In Atmospheric Measurements during POPCORN — Characterisation of the Photochemistry over a Rural Area. Springer Netherlands, 1998. http://dx.doi.org/10.1007/978-94-017-0813-5_3.

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DE MAYO, P., L. V. NATARAJAN, and W. R. WARE. "Surface Photochemistry: Temperature Effects on the Emission of Aromatic Hydrocarbons Adsorbed on Silica Gel." In ACS Symposium Series. American Chemical Society, 1985. http://dx.doi.org/10.1021/bk-1985-0278.ch001.

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Bowen, E. J. "The Photochemistry of Aromatic Hydrocarbon Solutions." In Advances in Photochemistry. John Wiley & Sons, Inc., 2007. http://dx.doi.org/10.1002/9780470133316.ch2.

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Marx, D. E., and A. J. Lees. "Kinetics and Mechanism of C-H Activation Following Photoexcitation of (η5-C5H5) Ir(CO)2 in Hydrocarbon Solutions." In Photochemistry and Photophysics of Coordination Compounds. Springer Berlin Heidelberg, 1987. http://dx.doi.org/10.1007/978-3-642-72666-8_43.

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Calvert, Jack G., John J. Orlando, William R. Stockwell, and Timothy J. Wallington. "Photodecomposition of Light-Absorbing Oxygenates and Its Influence on Ozone Levels in the Atmosphere." In The Mechanisms of Reactions Influencing Atmospheric Ozone. Oxford University Press, 2015. http://dx.doi.org/10.1093/oso/9780190233020.003.0011.

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Photochemistry provides the important driving force that initiates chemistry in the atmosphere. We saw in Chapter II how light absorbed by ozone generates the important HO radical, and, in Chapter III, we reviewed how light absorption by NO2 leads to ozone formation. In this chapter, we discuss the photochemistry of the light-absorbing oxygenates: their photochemical lifetimes and the nature of the modes of photodecomposition they undergo. Of course, light of sufficient energy per quantum must be absorbed by a molecule if its photodecomposition is to occur. The hydrocarbons do not absorb tropospheric sunlight, as seen in Figure VIII-A-1. The light gray and dark gray lines, respectively, show the distribution of actinic flux present in the troposphere and upper stratosphere for overhead Sun. It can be seen that the larger alkanes, alkenes, and aromatic hydrocarbons absorb at somewhat longer wavelengths than the first member of the family, but none can be electronically excited by tropospheric radiation. Among the hydrocarbons, only the polycyclic aromatics absorb appreciable tropospheric sunlight, and their π → π* excitation does not result in decomposition but likely generates O2(1Δg) molecules by energy transfer; these molecules are usually quenched by collision to ground state O2(3Σg−) molecules (see Calvert et al., 2000). As atmospheric oxidation of the hydrocarbons occurs, initiated largely by HO radicals, a multitude of oxygenated organic species are generated. The absorption region for the oxygenates is generally shifted to longer wavelengths, although the alcohols, ethers, acids, and esters still show no overlap of the regions of tropospheric actinic flux. For the families of compounds shown, the only significant absorbers of tropospheric sunlight are the aldehydes (e.g., CH2O) and the ketones (e.g., CH3C(O)CH3). Formic acid and methyl formate, as well as the larger members of the acid and ester families, absorb sunlight available only at the higher altitudes of the stratosphere, where they are expected to photodecompose. However, these species are not expected to be present in the stratosphere because they are removed in the troposphere largely via HO reactions. In this chapter, we focus on the rates and pathways for photodecomposition of the aldehydes and ketones with less detailed considerations of the other less prevalent light-absorbing trace compounds.
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Yung, Yuk L., and William B. DeMore. "Earth: Imprint of Life." In Photochemistry of Planetary Atmospheres. Oxford University Press, 1999. http://dx.doi.org/10.1093/oso/9780195105018.003.0012.

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Earth is the largest of the four terrestrial planets, three of which have substantial atmospheres. The astronomical and orbital parameters are summarized in table 9.1. Our planet has an obliquity of 23.5°, giving rise to well-known seasonal variations in solar insolation. The orbital elements are slightly perturbed by other planets in the solar system (primarily Jupiter), with time scales from 20 to 100 kyr, and these changes are believed to cause the advance and retreat of ice sheets. The last glacial maximum (LGM) occurred 18 kyr ago, at which time the planet was colder by several degrees centigrade on average. At present Earth is in an interglacial warm period. The origin of Earth may not be very different from that of the other terrestrial bodies. However, three properties may be unique to this planet. One is the formation of the Moon, probably via collision between Earth and a Mars-sized body. Second is the release of a huge amount of water from the interior (see discussion in section 8.5). Third, Earth is endowed with a large magnetic field that protects it from direct impact by the solar wind. Seventy percent of Earth's surface is covered by oceans, which have a mean depth of 3 km. There is so much water that Arthur C. Clarke proposed that "Ocean" might be a better name for our planet than "Earth." The enormous body of water became the cradle of life as early as 3.85 Gyr ago. The present terrestrial environment is the end-product of billions of years of evolution driven by the hydrological cycle and global biogeochemical cycles, in addition to the slower forces of geodynamics and geochemistry. The massive hydrological cycle and the biogeochemical cycles that operate on Earth are absent from other planets in the solar system. Mars in the remote past might have had a milder climate with liquid water on the surface, but the planet dried up a few eons ago. There is to date no observational evidence for the hypothetical oceans (composed of liquid hydrocarbons) on Titan. Life on a planetary scale equivalent to the terrestrial biosphere does not exist elsewhere in the solar system.
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Atkins, Peter. "Irritating Atmospheres: Atmospheric Photochemistry." In Reactions. Oxford University Press, 2011. http://dx.doi.org/10.1093/oso/9780199695126.003.0030.

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The problem of photochemically generated smog begins inside internal combustion engines, where at the high temperatures within the combustion cylinders and the hot exhaust manifold nitrogen molecules and oxygen molecule combine to form nitric oxide, NO. Almost as soon as it is formed, and when the exhaust gases mingle with the atmosphere, some NO is oxidized to the pungent and chemically pugnacious brown gas nitrogen dioxide, NO2, 1. We need to watch what happens when one of these NO2 molecules is exposed to the energetic ultraviolet photons in sunlight. We see a photon strike the molecule and cause a convulsive tremor of its electron cloud. In the brief instant that the electron cloud has swarmed away from one of the bonding regions, an O atom makes its escape, leaving behind an NO molecule. We now continue to watch the liberated O atom. We see it collide with an oxygen molecule, O2, and stick to it to form ozone, O3, 2. This ozone is formed near ground level and is an irritant; ozone at stratospheric levels is a benign ultraviolet shield. Now keep your eye on the ozone molecule. In one instance we see it collide with an NO molecule, which plucks off one of ozone’s O atoms, forming NO2 and letting O3 revert to O2. Another fate awaiting NO2 is for it to react with oxygen and any unburned hydrocarbon fuel and its fragments that have escaped into the atmosphere. We can watch that happening too where the air includes surviving fragments of hydrocarbon fuel molecules. A lot of little steps are involved, and they occur at a wide range of rates. Let’s suppose that some unburned fuel escapes as ethane molecules, CH3CH3, 3. Although ethane is not present in gasoline, a CH3CH2· radical (Reaction 12) would have been formed in its combustion and then combined with an H atom in the tumult of reactions going on there. You already know that vicious little O atoms are lurking in the sunlit NO2-ridden air. We catch sight of one of their venomous acts: in a collision with an H2O molecule they extract an H atom, so forming two ·OH radicals.
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