Spectroscopic studies of strong hydrogen bonds.
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Spectroscopic studies of strong hydrogen bonds. by Michael Frederick Claydon

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Published by University of East Anglia in Norwich .
Written in English


Book details:

Edition Notes

Thesis (Ph.D.) - University of East Anglia, School of Chemical Sciences, 1968.

ID Numbers
Open LibraryOL13844819M

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The spectroscopic phenomena of strong hydrogen bonds (band shifts, band broadening, intensity increase) are attributed to the interaction of the π electrons with the hydrogen atom, using the latter's distorted p-orbit. The analogy of the spectral phenomena in the hydrogen-chelated and metal-chelated compounds is stressed. Book Search tips Selecting this option will search all publications across the Scitation platform Selecting this option will search all publications for the Publisher/Society in context. Spectroscopic Studies of the Hydrogen Bond. II. The Shift of the O–H Vibrational Frequency in the Formation of the Hydrogen Bond J. Chem. Phys. 5, Cited by: A review is given of the literature on spectroscopic studies of the hydrogen bond. Discussed in turn are self-association due to hydrogen bonding, hydrogen bonding between donors and acceptors, intramolecular hydrogen bonding, and bonding in aqueous systems. For each category the results obtained by IR, NMR, and electronic spectroscopy are Cited by: 4. INFRARED SPECTROSCOPIC STUDIES OF HYDROGEN BONDING IN PHENOLIC POLYMERS A Thesis in Material Science and Engineering by Andrea Choperena Guerra Andrea Choperena Guerra Submitted in Partial Fulfillment of the Requirements for the .

It presents readers with hydrogen bonding studies by vibrational spectroscopy and quantum chemistry, as well as vibrational spectroscopy and quantum chemistry studies on both biological systems and nano science. The book also looks at vibrational anharmonicity and overtones, and nonlinear and time-resolved spectroscopy. Historically, infrared spectroscopy has been the most important spectroscopic method in the study of hydrogen bonding, and the possibility to predict the vibrational transitions of hydrogen‐bonded systems by theoretical calculations has been of great interest for decades. The intramolecular hydrogen bond in benzoylacetone has been studied with high-level ab initio Hartree−Fock and density functional theory methods. The results are compared to the experimental structure as obtained from low-temperature neutron and X-ray diffraction experiments. The calculations reveal that electron correlation effects are essential for modeling the experimental low-temperature. Atomic fluorescence spectroscopy Short answer questions TrueFalse ques electrons elements emission emitted energy levels example excited field filter flame frequency give given greater ground hence higher hydrogen important increases infrared intensity interaction involved known length light lines longer lower measured metal method 3/5(5).

Thermal and infrared spectroscopic studies were performed on the hydrogen-bonding interaction in the blends of biodegradable atactic, highly syndiotactic and isotactic poly(3-hydroxybutyrate)s with the analysis of Fourier-transform infrared spectra, it was found that the crystalline phase could greatly restrain the formation of inter-associated hydrogen-bonds. IR spectroscopy studies on ethanol water mixtures have demonstrated that hydrogen bonding between the two molecules results in an overall decrease in intensity of the O-H stretch vibration. Hydrogen bonds are involved in the species, which are combined bond distances of the A–HB compared to the sum of the van der Waals radius, as listed in Table [21].The types of various hydrogen bonding between atoms A and B are located closer than the estimated distance of the sum of the van der Waals radii. The structures of the mono- and the dihalogenated N-unsubstituted 2-aminobenzamides were characterized by means of the spectroscopic (1H-NMR, UV-Vis, FT-IR, and FT-Raman) and X-ray crystallographic techniques complemented with a density functional theory (DFT) method. The hindered rotation of the C(O)–NH2 single bond resulted in non-equivalence of the amide protons and therefore .