Vibrational Relaxation Measurements in C<mml:math xmlns:mml="http://www.w3.org/1998/Math/MathML" display="inline"><mml:mrow><mml:msub><mml:mrow><mml:mi mathvariant="normal">O</mml:mi></mml:mrow><mml:mrow><mml:mn>2</mml:mn></mml:mrow></mml:msub></mml:mrow></mml:math>Using an Induced-Fluorescence Technique

Hocker, L. O.; Kovacs, Mark A.; Rhodes, C. K.; Flynn, George W.; Javan, A.

doi:10.1103/physrevlett.17.233

Cited by 175 publications

(19 citation statements)

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“…In 1966, Javan and coworkers (45) discovered that the CO 2 laser could excite the asymmetric stretch of CO 2 from the thermally populated symmetric stretch lower-laser level, and laser-excited vibrational fluorescence was easily detected. This initiated an avalanche of studies of the vibrational relaxation of the asymmetric stretch (ν 3 ) of CO 2 .…”

Section: Carbon Dioxidementioning

confidence: 99%

A Spectroscopist's View of Energy States, Energy Transfers, and Chemical Reactions

Moore

2007

Annu. Rev. Phys. Chem.

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This chapter describes a research career beginning at Berkeley in 1960, shortly after Sputnik and the invention of the laser. Following thesis work on vibrational spectroscopy and the chemical reactivity of small molecules, we studied vibrational energy transfers in my own lab. Collision-induced transfers among vibrations of a single molecule, from one molecule to another, and from vibration to rotation and translation were elucidated. My research group also studied the competition between vibrational relaxation and chemical reaction for potentially reactive collisions with one molecule vibrationally excited. Lasers were used to enrich isotopes by the excitation of a predissociative transition of a selected isotopomer. We also tested the hypotheses of transition-state theory for unimolecular reactions of ketene, formaldehyde, and formyl fluoride by (a) resolving individual molecular eigenstates above a dissociation threshold, (b) locating vibrational levels at the transition state, (c) observing quantum resonances in the barrier region for motion along a reaction coordinate, and (d) studying energy release to fragments. GETTING STARTEDI had the good fortune to grow up on a farm in eastern Pennsylvania, where hard work produced good crops, poultry, and livestock; where I could help my father take apart, repair, and reassemble farm equipment; and where I could manufacture and experiment with gun powder. In those days, parents could still give chemistry sets to their children, and the East Coast sky was often clear enough to observe shooting stars while lying flat on the bed of a hay wagon. This constituted my first spectroscopic observations of chemistry in action. My initial in-class chemistry lab was a study of sulfur combustion carried out by placing a fumigation candle in the ink well of my third-grade desk and lighting it on departure for recess. This early initiative was not encouraged on my return from the playground. One of Princeton Professor Hubert Alyea's renowned lectures on the marvels of chemistry at a nearby high school provided my first look at cryogenics as he exhaled through a mouth full of dry ice. By the time I finished a series of integrated courses in the physical sciences, a one-week visit by J. Robert Oppenheimer, and a challenging course in analytical/inorganic chemistry in high school (Phillips Exeter Academy in New Hampshire), I was well on my way to becoming a physical chemist. The launching of Sputnik during my first month of college (October 1957) at Harvard sharply increased federal funding for scientific research and greatly encouraged scientific career paths. That fall, the intensity of lab courses in physics and organic chemistry, a fourth-semester calculus course, and a humanities course quickly ended my aspiration to extend my high-school crew experience to intercollegiate rowing. A series of research projects in Paul D. Bartlett's personal lab at Harvard and summer jobs at Arthur D. Little and General Electric's corporate research lab deepened my interest and experi...

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Section: Carbon Dioxidementioning

confidence: 99%

A Spectroscopist's View of Energy States, Energy Transfers, and Chemical Reactions

Moore

2007

Annu. Rev. Phys. Chem.

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“…2X 10 The calculated rate is too fast by a factor 4 to 8. Henderson 9 ,12 has measured the deactivation of the oxygen vibration (()= 2230 0 K) by small amounts of carbon dioxide.…”

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Deactivation of Vibrations by Collision in the Presence of Fermi Resonance

Herzfeld

1967

The Journal of Chemical Physics

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Downloaded 02 Oct 2012 to 139.184.30.132. Redistribution subject to AIP license or copyright; see http://jcp.aip.org/about/rights_and_permissions ARGON-FLUORINE PHASE DIAGRAM 743 demonstrates again that size effects cannot be the dominant influence in determining solubility limits in these two-component systems of simple van der Waals lattices.The structure of a-F2 is still unknown. In the course of this investigation we got good Debye-Scherrer patterns from a-F 2 and we are trying to determine the structure.The rate of vibrational deactivation by collision of polyatomic molecules is discussed. Previous calculations for CO2 by the author are corrected. A systematic method to find the steric factor in complex collisions is proposed, and the best procedure for evaluation of such collisions is discussed. Mixture of vibrational wavefunctions may increase the rate appreciably, particularly in the presence of Fermi resonance. The agreement with experiment is good for the deactivation of the transversal vibration and for the effect of CO 2 admixture on O2 deactivation, but the experimental rate of deactivation of the asymmetric longitudinal C02 vibration is much greater (60 to 90 times) then the calculated one.

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“…1. The calculated values of (T. for Be: (1) without any autoionizing levels, (2) with the 2p3s Ip level, and (3) with the 2p4s Ip level. For all figures, e is the energy above the ionization threshold for the ground state in rydbergs, and the cross section <F is in megabarns where 1 Mb= 10- 18 were solved by a method similar to that used by Altick and Moore.'…”

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“…Previous work indicates that for Hartree-Fock wavefunctions the CT. form is best. 5 The CT. curve (2) shows the effect of the 2p3s I P level. While it introduces an additional minimum in the cross section, its effect is quite broad and does not have the shape associated with an isolated resonance.…”

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confidence: 99%