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Hydrogen-bonded protons

Figures 2.a-c show the pyridine adsorption results. Bronsted acidity is manifested by the bands at 1440-1445,1630-1640 and 1530-1550 cm . Bands at 1600-1630 cm are assigned to pyridine bonded to Lewis acid sites. Certain bands such as the 1440-1460 and 1480-1490 cm can be due to hydrogen-bonded, protonated or Lewis-coordinated pyridine species. Under continuous nitrogen purging, spectra labeled as "A" in Figures 2a-c represent saturation of the surface at room temperature (90 25 unol pyridine/g found in all three tungsta catalysts) and "F" show the baseline due to the dry catalyst. We cannot entirely rule out the possibility of some extent of weakly bound pyridine at room temperature. Nevertheless, the pyridine DRIFTS experiments show the presence of Brpnsted acidity, which is expected to be the result of water of reduction that did not desorb upon purging at the reduction temperature. It is noted that, regardless of the presence of Pt, the intensity of the DRIFTS signals due to pyridine are... Figures 2.a-c show the pyridine adsorption results. Bronsted acidity is manifested by the bands at 1440-1445,1630-1640 and 1530-1550 cm . Bands at 1600-1630 cm are assigned to pyridine bonded to Lewis acid sites. Certain bands such as the 1440-1460 and 1480-1490 cm can be due to hydrogen-bonded, protonated or Lewis-coordinated pyridine species. Under continuous nitrogen purging, spectra labeled as "A" in Figures 2a-c represent saturation of the surface at room temperature (90 25 unol pyridine/g found in all three tungsta catalysts) and "F" show the baseline due to the dry catalyst. We cannot entirely rule out the possibility of some extent of weakly bound pyridine at room temperature. Nevertheless, the pyridine DRIFTS experiments show the presence of Brpnsted acidity, which is expected to be the result of water of reduction that did not desorb upon purging at the reduction temperature. It is noted that, regardless of the presence of Pt, the intensity of the DRIFTS signals due to pyridine are...
Over the past 20 years, with the availability of fast reaction techniques (Eigen and de Maeyer, 1963 Hammes, 1974 Bemasconi, 1976), numerous kinetic studies have been made of the reactivity of hydrogen-bonded protons towards an external base (52). The majority of such studies have been made with hydroxide ion as the external base. Some examples of proton transfer to... [Pg.149]

The conclusions reached about proton transfer from phenylazoresorcinol monoanions are quite different from the behaviour which has been described for other hydrogen-bonded acids. For phenylazoresorcinol monoanions, it appears that direct attack by base on the hydrogen-bonded proton is an important process and can compete with two-step proton removal. For two-step proton transfer through an open form of the phenylazoresorcinol monoanion it is found that the rate of proton transfer from the open form is... [Pg.183]

The hydrogen-bonded protons wander all over the lot. Where you find them, and how sharp their signals are, depends at least on the solvent, the concentration, and the temperature. [Pg.284]

Table 5 Isotope effects on the chemical shift of hydrogen-bonded protons. Table 5 Isotope effects on the chemical shift of hydrogen-bonded protons.
The value of the fractionation factor for any site will be determined by the shape of the potential well. If it is assumed that the potential well for the hydrogen-bonded proton in (2) is broader, with a lower force constant, than that for the proton in the monocarboxylic acid (Fig. 8), the value of the fractionation factor will be lower for the hydrogen-bonded proton than for the proton in the monocarboxylic acid. It follows that the equilibrium isotope effect on (2) will be less than unity. As a consequence, the isotope-exchange equilibrium will lie towards the left, and the heavier isotope (deuterium in this case) will fractionate into the monocarboxylic acid, where the bond has the larger force constant. [Pg.283]

The equilibrium constant for the isotope-exchange equilibrium can be expressed (6) in terms of the solvent isotope effects on the acid-dissociation constants and of the monocarboxylic acid and dicarboxylic acid monoanion, respectively. It follows that a lower value for the fractionation factor of the hydrogen-bonded proton means that the solvent isotope effect on the acid-dissociation constant will be lower for the dicarboxylic acid monoanion than for the monocarboxylic acid. [Pg.283]

The values of the fractionation factors in structures [15]-[21] are not strictly comparable since they are defined relative to the fractionation in different solvent standards. However, in aqueous solution, fractionation factors for alcohols and carboxylic acids relative to water are similar and close to unity (Schowen, 1972 Albery, 1975 More O Ferrall, 1975), and it seems clear that the species [15]-[21] involving intermolecular hydrogen bonds with solvent have values of cp consistently below unity. These observations mean that fractionation of deuterium into the solvent rather than the hydrogen-bonded site is preferred, and this is compatible with a broader potential well for the hydrogen-bonded proton than for the protons of the solvents water, alcohol and acetic acid. [Pg.286]

The major conclusion which was reached from the work of Jarret and Saunders was that intramolecularly hydrogen-bonded protons generally give values of (p below the value for a similar proton which is not involved in an intramolecular hydrogen bond. For example, a value of (p of 0.77 was obtained for the hydrogen-bonded site in the maleate ion [12] compared to 0.94 for acetic acid. The value for the phthalate ion [10] was higher, (p = 0.95. The value of (p = 0.95 was obtained for the salicylate ion [22] in comparison to the result for phenol, tp = 1.13. [Pg.287]

There is no clear correlation between the chemical shift or the ir absorption frequency and the length and linearity of the hydrogen bonds in the protonated diamines. The most reliable test for the nature of the potential function appears to be the sign of the isotope effect on the chemical shift of the hydrogen-bonded proton. [Pg.326]

Eyring (Haslam et ai, 1965a Eyring and Haslam, 1966 Jensen et ai, 1966) preferred to explain the reduced rate in terms of a one-step mechanism in which the base directly attacked the hydrogen-bonded proton as in (24). [Pg.330]


See other pages where Hydrogen-bonded protons is mentioned: [Pg.193]    [Pg.250]    [Pg.91]    [Pg.110]    [Pg.202]    [Pg.215]    [Pg.130]    [Pg.135]    [Pg.135]    [Pg.138]    [Pg.140]    [Pg.141]    [Pg.142]    [Pg.144]    [Pg.144]    [Pg.145]    [Pg.161]    [Pg.179]    [Pg.182]    [Pg.183]    [Pg.184]    [Pg.260]    [Pg.10]    [Pg.162]    [Pg.208]    [Pg.361]    [Pg.390]    [Pg.258]    [Pg.261]    [Pg.264]    [Pg.271]    [Pg.277]    [Pg.287]    [Pg.288]    [Pg.292]    [Pg.293]    [Pg.303]    [Pg.317]    [Pg.319]    [Pg.324]   
See also in sourсe #XX -- [ Pg.571 ]

See also in sourсe #XX -- [ Pg.309 ]




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Acidic and Exchangeable Protons Hydrogen Bonding

Bonded protons

Coherent Proton Tunneling in Hydrogen Bonds of Isolated Molecules Malonaldehyde and Tropolone

Coupled protons, hydrogen bonds, tunneling

Hard hydrogen-bonded protons

Hydrated proton hydrogen bonding

Hydrogen Bonding, Tautomerism and Proton Exchange

Hydrogen Bonds and Proton Abstraction Reactions

Hydrogen bond, free proton

Hydrogen bond, independent proton

Hydrogen bond, independent proton model

Hydrogen bond, isotropic proton

Hydrogen bonded proton clusters

Hydrogen bonding proton acidity

Hydrogen bonding proton sponges

Hydrogen bonding proton transfer and

Hydrogen bonding, protons

Hydrogen bonds proton donors

Hydrogen bonds proton ejection

Hydrogen bonds proton ordering

Hydrogen bonds proton ordering model

Hydrogen bonds proton path active site

Hydrogen bonds proton polaron

Hydrogen bonds proton transfer process

Hydrogen bonds proton-phonon coupling

Hydrogen bonds tunneling transition, coupled protons

Hydrogen bonds, charge-assisted proton transfer

Hydrogen bonds, proton sponges

Hydrogen protons

Hydrogen-bonded amide protons

Hydrogen-bonded imide protons

Hydrogen-bonded systems proton tunneling

Hydrogenation protonation

Intramolecular hydrogen bonds proton sponges

Naphthalene hydrogen bonding Proton

PKa values of hydrogen-bonded protons

Phenolic hydrogen-bonded protons

Proton Dynamics in Hydrogen-bonded Crystals

Proton Transfer in Systems with the Intramolecular Hydrogen Bonding

Proton Transfers in Hydrogen-Bonded Systems

Proton bifurcation, hydrogen bonds

Proton conductivity hydrogen bonds

Proton donors, hydrogen-bonded complexes

Proton nuclear magnetic resonance hydrogen bonding

Proton ordering, hydrogen bonds quantum mechanics

Proton ordering, hydrogen bonds systems

Proton removal from intramolecular hydrogen bonds

Proton transfer along hydrogen bonds

Proton transfer, hydrogen bonding

Proton transfer, hydrogen bonds

Proton transfer, hydrogen bonds aqueous systems

Proton transfer, hydrogen bonds bacteriorhodopsin

Proton transfer, hydrogen bonds bond vibrations

Proton transfer, hydrogen bonds cluster formation

Proton transfer, hydrogen bonds dynamics

Proton transfer, hydrogen bonds experimental results

Proton transfer, hydrogen bonds mechanisms

Proton transfer, hydrogen bonds molecular associates

Proton transfer, hydrogen bonds molecular clustering

Proton transfer, hydrogen bonds quantum mechanics

Proton transfer, hydrogen bonds switching

Proton transfer, hydrogen bonds thermodynamics

Proton transfer, hydrogen bonds tunneling

Proton-Deficient Hydrogen Bonds

Schiff base protonation, hydrogen bonds

Solid-State Tautomerism, Proton Transfer, and Hydrogen Bonding

Tautomerism, Proton Transfer, and Resonance-Assisted Hydrogen Bonding

Tunneling mechanisms, hydrogen bonds proton transfer

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