Brauman, John

R. Stephen Berry, University of Chicago, IL, USA John I. Brauman, Stanford University, CA, USA A. Welford Castleman, Jr., Pennsylvania State University, PA, USA Enrico Clementi, Universite Louis Pasteur, Strasbourg, France Stephen R. Langhoff, NASA Ames Research Center, Moffett Field, CA, USA K. Morokuma, Emory University, Atlanta, GA, USA Peter J. Rossky, University of Texas atAustin, TX, USA Zdenek Slanina, Czech Academy of Sciences, Prague, Czech Republic Donald G. Truhlar, University of Minnesota, Minneapolis, MN, USA IvarUgi, Technische Universitat, Munchen, Germany... 

DR. JOHN BRAUMAN (Stanford University) I have a question about the empirical correlations for quantities like charge transfer band energies versus parameters such as the Kosower Z-value. There is a very large literature of that type and there are many, many good correlations for a variety of parameters. You obtain straight lines with your simple dielectric continuum model. It seems to me, however, that one ought to be able to derive these types of relationships directly from the model. And it doesn t seem to be very helpful to say that these relationships are simply empirical and, therefore, not worth the attention. What you want to do is derive the equations and see whether they, in fact, all reduce to the same terms. 

DOUGLAS J. RARER, National Research Council 8 05 RONALD BRESLOW AND MATTHEW V. TIRRELL, Co-Chairs, Committee on Challenges for the Chemical Sciences in the 21st Century 8 20 JOHN I. BRAUMAN, Co-Chair, Organizing Committee for the Workshop on National Security and Homeland Defense... 

John L. Anderson, Carnegie Mellon University, Co-Chair John I. Brauman, Stanford University, Co-Chair... 

Many thanks to Peter Godfrey-Smith, Michael Strevens, Anthony Everett, and Deena Skolnick who helped me to clarify the main ideas of this paper tremendously. I would also like to thank Philip Kitcher, Sandra Mitchell, Paul Churchland, Roald Hoffmann, John Brauman, Paul Needham, Tania Lombrozo, and Daniel Corbett for helpful discussions of earlier drafts. The work in this paper was partially supported by an NSF Graduate Research Fellowship. 

Of equal historical significance are the contributions of the groups of John Brauman (Stanford) and Carl Lineberger (Colorado). A number of free-radicals are known to exhibit both dipole-bound and more tightly bound conventional (valence) anions. The groups of Brauman and Lineberger have reported very narrow resonance features in the photodetachment spectrum corresponding to rotationally excited shape and Feshbach resonances for many of these dipole-bound radical anions. 

John I. Brauman, James A. Dodd, and Chau-Chung Han Department of Chemistry, Stanford University, Stanford, CA 94305... 

Starting in the 1960s, a technique called ion cyclotron resonance (ICR) mass spectrometry, developed hy John Brauman (1937- ) at Stanford University, facilitated measurement of the products formed from gas-phase reactions between molecules and ions. Jesse L. Beauehamp (1942- ), at Caltech, was an early investigator of this new gas-phase chemistry. In contrast to the solution-phase chemistry, in the gas phase toluene is a stronger acid than methanol ... 

The reaction coordinate for a typical (solution-phase) 5 2 reaction is depicted in chapter 4 CH3CI and OH" react in a single step forming a transient activated complex that instantaneously transforms to the CH3OH and Cl" products. In 1977, John Brauman discovered that reactions of this type behave very differently in the gas phase, without a... 

Yet this traditional, and simple, explanation that treats alkyl groups as intrinsically electron-donating is not correct. In 1970, Professor John Brauman (b. 1937) and his co-workers at Stanford University showed that in the gas phase the opposite acidity order obtained. The intrinsic acidity of the four alcohols ofTable 6.6 is exactly opposite to that found in solution. The acidity order measured in solution reflects a powerful effect of the solvent, not the natural acidities of the alcohols themselves. Organic ions are almost all unstable species, and the formation of the alkoxide anions depends critically on how easy it is to stabilize them through interaction with solvent molecules, a process called solvation. r -Butyl alcohol is a weaker acid in solution than methyl alcohol because the large r -butyl alkoxide ion is difficult to solvate. The more alkyl groups, the more difficult it is for the stabilizing solvent molecules to approach (Fig. 6.22). Of course, in the gas phase where solvation is impossible, the natural acidity order is observed. 

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