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Electron Oxidants

Xie Q, Arias F and Echegoyen L 1993 Electrochemically-reversible, single-electron oxidation of Cgg and... [Pg.2431]

The. more tightly held an electron is. the more difficult it is to remove, hence the higher the electrode potential necessary to remove it. Make the reasonable hypothesis that the electron removed in a one-electron oxidation comes from the highest occupied orbital. HOMO. Using SHMO. determine the HOMO for ben7 ene, biphenyl, and naphthalene. [Pg.226]

Note that the moles of oxalic acid are multiplied by 2 since there are two carbon atoms, each of which undergoes a 1-electron oxidation. [Pg.23]

Subsequent studies (63,64) suggested that the nature of the chemical activation process was a one-electron oxidation of the fluorescer by (27) followed by decomposition of the dioxetanedione radical anion to a carbon dioxide radical anion. Back electron transfer to the radical cation of the fluorescer produced the excited state which emitted the luminescence characteristic of the fluorescent state of the emitter. The chemical activation mechanism was patterned after the CIEEL mechanism proposed for dioxetanones and dioxetanes discussed earher (65). Additional support for the CIEEL mechanism, was furnished by demonstration (66) that a linear correlation existed between the singlet excitation energy of the fluorescer and the chemiluminescence intensity which had been shown earher with dimethyl dioxetanone (67). [Pg.266]

Reactions with Parting of Radicals. The one-electron oxidation of cationic dyes yields a corresponding radical dication. The stabihty of the radicals depends on the molecular stmcture and concentration of the radical particles. They are susceptible to radical—radical dimerization at unsubstituted, even-membered methine carbon atoms (77) (Fig. 6). [Pg.495]

Fig. 6. One-electron oxidation and dimerization where (21a) is a dye, (21b) a radical cation, and (21c) a dimer. Fig. 6. One-electron oxidation and dimerization where (21a) is a dye, (21b) a radical cation, and (21c) a dimer.
Polymerization Initiator. Some unsaturated monomers can be polymerized through the aid of free radicals generated, as transient intermediates, in the course of a redox reaction. The electron-transfer step during the redox process causes the scission of an intermediate to produce an active free radical. The ceric ion, Ce" ", is a strong one-electron oxidizing agent that can readily initiate the redox polymerization of, for example, vinyl monomers in aqueous media at near ambient temperatures (40). The reaction scheme is... [Pg.371]

As shown in equation 12, the chemistry of this developer s oxidation and decomposition has been found to be less simple than first envisioned. One oxidation product, tetramethyl succinic acid (18), is not found under normal circumstances. Instead, the products are the a-hydroxyacid (20) and the a-ketoacid (22). When silver bromide is the oxidant, only the two-electron oxidation and hydrolysis occur to give (20). When silver chloride is the oxidant, a four-electron oxidation can occur to give (22). In model experiments the hydroxyacid was not converted to the keto acid. Therefore, it seemed that the two-electron intermediate triketone hydrate (19) in the presence of a stronger oxidant would reduce more silver, possibly involving a species such as (21) as a likely reactive intermediate. This mechanism was verified experimentally, using a controlled, constant electrochemical potential. At potentials like that of silver chloride, four electrons were used at lower potentials only two were used (104). [Pg.509]

Radical cations can be derived from aromatic hydrocarbons or alkenes by one-electron oxidation. Antimony trichloride and pentachloride are among the chemical oxidants that have been used. Photodissociation or y-radiation can generate radical cations from aromatic hydrocarbons. Most radical cations derived from hydrocarbons have limited stability, but EPR spectral parameters have permitted structural characterization. The radical cations can be generated electrochemically, and some oxidation potentials are included in Table 12.1. The potentials correlate with the HOMO levels of the hydrocarbons. The higher the HOMO, the more easily oxidized is the hydrocarbon. [Pg.681]

Wurstert salts. Generated by one-electron oxidation of the diamine. Indefinitely stable. [Pg.696]

One-electron oxidation of carboxylate ions generates acyloxy radicals, which undergo decarboxylation. Such electron-transfer reactions can be effected by strong one-electron oxidants, such as Mn(HI), Ag(II), Ce(IV), and Pb(IV) These metal ions are also capable of oxidizing the radical intermediate, so the products are those expected from carbocations. The oxidative decarboxylation by Pb(IV) in the presence of halide salts leads to alkyl halides. For example, oxidation of pentanoic acid with lead tetraacetate in the presence of lithium chloride gives 1-chlorobutane in 71% yield ... [Pg.726]

An intriguing class of persistent radicals are those formed by the one-electron oxidation of the hexagonal prismatic clusters Li2[E(N Bu)3] 2 (3.21, E = S, Se). The air oxidation of 3.21 produces deep blue (E = S) or green (E = Se) solutions in toluene. The EPR spectra of these solutions consist of a septet (1 3 6 7 6 3 1) of decets (Eig. 3.5). This pattern results from interaction of the unpaired electron with three equivalent 7=1 nuclei, i.e., and three equivalent I = 3/2 nuclei, i.e., Ei. It has been proposed that the one-electron oxidation of 3.21 is accompanied by the removal of an Ei" cation from the cluster to give the neutral radical 3.22 in which the dianion [S(N Bu)3] and the radical monoanion [S(N Bu)3] are bridged by three Ei" cations. [Pg.40]

FIGURE 18.30 The physiological effects of ascorbic acid (vitamin C) are the result of its action as a reducing agent. A two-electron oxidation of ascorbic acid yields dehy-droascorbic acid. [Pg.599]

In the 4-electron oxidation of acidified N2H4 to N2, it has been shown by the use of N2H4 iso-topically enriched in that both the N atoms of each molecule of N2 originated in the same molecule of N2H4. This reaction is also the basis for the most commonly used method for the analytical determination of N2H4 in dilute aqueous solution ... [Pg.430]

If [(NHi)5Co-02-Co(NH )5] + is treated with aqueous KOH another brown com-plex, [(NH3)4Co(p.-NH2)0J.-O2)Co(NH,),] is obtained and, again, a 1-electron oxidation yields a green superoxo species, [(NH3)4Co(tJL-NH2)-(tJL-02)Co(NH3). J The sulfate of this latter is actually one component of Vortmann s sulfate — the other is the red [(NH3)4Co(tx-NH2>-(tx-OH)Co(NH3)4](S04)2- They are obtained by aerial oxidation of ammoniacal solutions of coball(II) nitrate followed by neutralization with H2S0.1. [Pg.1127]

The oxidation of the macrocycle in phthalocyanines does not generally lead to stable molecules. One-electron oxidations of the macrocyclc(s) in bis(phthalocyanines) leading to species which can be isolated have been carried out chemically or electrochemically,... [Pg.821]

Tetrabutylammonium [bismuth(III) bis(phthalocyanine)] undergoes a one-electron oxidation (dichloromethane, U = IV, platinum electrode, several days) to give bismuth bis(phthalocyanine).167... [Pg.821]

Scheme 10.16 Redox cycle of flavins. The cycle is depicted with a two-electron reduction of flavin by NAD(P)H and two one-electron oxidations. Scheme 10.16 Redox cycle of flavins. The cycle is depicted with a two-electron reduction of flavin by NAD(P)H and two one-electron oxidations.

See other pages where Electron Oxidants is mentioned: [Pg.427]    [Pg.17]    [Pg.19]    [Pg.347]    [Pg.268]    [Pg.454]    [Pg.390]    [Pg.254]    [Pg.247]    [Pg.472]    [Pg.396]    [Pg.282]    [Pg.303]    [Pg.626]    [Pg.280]    [Pg.112]    [Pg.428]    [Pg.616]    [Pg.59]    [Pg.127]    [Pg.143]    [Pg.187]    [Pg.190]    [Pg.206]    [Pg.207]    [Pg.13]    [Pg.69]    [Pg.196]    [Pg.125]    [Pg.357]    [Pg.96]   


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1.3- Diphenyl pyridine one-electron anodic oxidation

Active electronics, oxide dielectric films

Aluminum oxide electron configurations

Auger electron spectroscopy oxidized

Benzene, 1,3,5-trialkylsterically crowded electron-transfer oxidation

Binary oxides electronic band structures

Bulk electronic structure of simple oxides

Calcium oxide electron configurations

Carbonyl oxides electronic structure

Cerium oxide electronic structure models

Contact ion pairs electron-transfer oxidation

Coordinated diimine ligands, oxidation electron transfer

Core electrons oxidation numbers

Diffusion in Mixed Electronic-Ionic Conducting Oxides (MEICs)

ELECTRON MICROSCOPY OF HIGH TEMPERATURE SUPERCONDUCTING OXIDES

Electron Configurations and Oxidation States

Electron Counting and Oxidation State

Electron Oxidative phosphorylation

Electron Pushing for the Baeyer-Villiger Oxidation

Electron Transfer Pathway Coupled to the Oxidation of Ammonia

Electron Transfer System Coupled to Oxidation of Ferrous Ion

Electron Transfer-Sensitized Photo-oxidation

Electron Transport, Oxidative Phosphorylation, and Hydroxylation

Electron backscatter diffraction (EBSD) analyses of oxide scale structure

Electron carriers in oxidative phosphorylation

Electron layered oxides

Electron microscopy - oxides

Electron microscopy - oxides applied

Electron oxidation activation

Electron oxide electrodes

Electron probe microanalysis, metal oxides

Electron scavenger nitrous oxide

Electron transfer Oxidative halogenation

Electron transfer metal oxide surfaces

Electron transfer nitric oxide synthase flavins

Electron transfer oxidation

Electron transfer oxidation inhibition mechanism

Electron transfer oxidized ions

Electron transfer processes oxidative fluorination

Electron transfer quenching oxidative

Electron transfer reactions oxide metal complexes

Electron transfer through oxide

Electron transfer, coupled with oxidative

Electron transfer, coupled with oxidative phosphorylation

Electron transfer, oxides

Electron transport chain and oxidative phosphorylation

Electron transport oxidative phosphorylation

Electron transport oxides

Electron transport, directed metal oxidation

Electron-Deficient C2 Fragments (Cycloadditions Involving Azomethines, Nitrones, Nitrile Oxides, and Dienes)

Electron-conducting oxide

Electron-transfer oxidation chain process

Electron-transfer oxidation formulation

Electron-transfer oxidation photochemical activation

Electron-transfer oxidation radical ions

Electron-transfer oxidation synthetic transformations

Electron-transfer oxidation thermal activation

Electron-transport system oxidative phosphorylation

Electronic Configuration and Oxidation States

Electronic Configuration, Oxidation States, Structures

Electronic Properties of Zinc Oxide

Electronic Structure of Copper Oxide Superconductors

Electronic Structure of Oxide Surfaces

Electronic conductivity in oxides

Electronic configurations oxides

Electronic materials oxidation processing

Electronic materials traditional oxidation technique

Electronic of oxides

Electronic oxidation reactions

Electronic oxides

Electronic oxides

Electronic properties, layer anodic oxide layers

Electronic properties, passive layers oxide layer

Electronic state oxide materials

Electronic states oxide glass modeling

Electronic structure indium oxide film

Electronic structure nitrous oxide

Electronic structure of oxide

Electronic structure oxidation

Electronic structure oxidation states

Electrons as Reagents for Oxidation and Reduction

Electrons in oxidation-reduction reactions

Electrons oxidation

Electrons oxidation

Electrons oxidation-reduction reactions

Electrons oxidized forms

Four-electron oxidation

Gate oxide thickness, electronic devices

Glucose oxidation electron transfer with metal

Graphene oxide electron transfer

High resolution electron microscopy oxides

Inner-sphere electron transfer oxidative addition

Introduction single-electron oxidation

Ionization potentials, electron affinities and stabilities of oxidation states

Iridium-catalyzed water oxidation electronic structure

Iron oxide electron transport

Iron oxides electronic structure

Iron oxides high pressure electronic structure

Lose electrons oxidation

Magnesium oxide electron transport

Metal oxide clusters electronic structures

Metal oxide electronic structures

Metal oxide reduction electron-transfer reactions

Metal oxide-adsorbate interactions electron transfer

Metal oxide-based compounds electron transfer reaction

Metal oxides electron transport

Metal oxides reactions yielding electronically excited

Metal oxides, electronic nose technology

Metal oxides, interfacial electron

Metal oxides, interfacial electron ions effect

Metal oxides, secondary electron emission

Mitochondrial electron transport and oxidative phosphorylation

Mixed ionic and electronic conducting oxides

Mixed proton—electron conducting oxide

Molybdenum oxidation, electron spin

New understanding of defect mechanisms in oxidation catalysis from dynamic electron microscopy

Nickel oxide electronic properties

Nitric oxide synthase electron transfer

Nitric oxide, reaction mechanisms with electron transfer reactions

Nitrile oxides, cycloaddition with electron-deficient dipolarophiles

Nitrogen oxidation electron transfer

Nitrogen oxide three-electron bond

Nitrous oxide electron scavenging

One electron oxidation and reduction

One-Electron Oxidation Processes

One-Electron Oxidation of Nucleobases

One-Electron Reduction and Oxidation in Nonaqueous Solvents

One-electron enzymatic oxidation

One-electron oxidant

One-electron oxidation activation

One-electron oxidation mechanism

One-electron oxidation of nucleobase

One-electron oxidation of selenium and tellurium compounds

One-electron oxidation potential

One-electron oxidation/reduction

Organic electron acceptors oxidants

Outlook Higher Electron Mobilities in Zinc Oxide

Over-oxidation single electron transfer mechanism

Oxidants reduction, electron transfer

Oxidation Numbers Keeping Tabs on Electrons

Oxidation Numbers Keeping Track of Electrons

Oxidation State and Electron Count

Oxidation States Electron Bookkeeping

Oxidation and Reduction Reactions Electronic Interpretations

Oxidation by Loss of Electrons

Oxidation catalysts, tunable electronic

Oxidation chain-breaking electron acceptors

Oxidation electron donor

Oxidation electron transfer-induced

Oxidation inhibition mechanism, electron

Oxidation numbers using valence electrons

Oxidation of Metallocenes and Electron Transfer Reactions

Oxidation of electrons

Oxidation one-electron

Oxidation potentials electron donors

Oxidation processing of electronic materials

Oxidation reactions, nonadiabatic electron transfer

Oxidation, aerobic, site electron transport

Oxidation, by electron transfer

Oxidation-reduction electron transfer

Oxidation-reduction reaction with partial electron transfer

Oxidation-reduction reactions Electron configuration

Oxidation-reduction reactions Intermolecular electron transfer

Oxidation-reduction reactions Intramolecular electron transfer

Oxidation-reduction reactions electron movement

Oxidation-reduction reactions electron transfer

Oxidation-reduction reactions hydrated electron

Oxidative activation electronic structure

Oxidative addition electron transfer

Oxidative addition outer-sphere electron-transfer

Oxidative electron transfer

Oxidative electron transfer, molecular

Oxidative phosphorylation and the electron transport chain

Oxidative phosphorylation electron transfer

Oxidative phosphorylation electron transport release from

Oxidative phosphorylation electron-motive force

Oxidative phosphorylation electron-transfer potential

Oxidative stability electron spin resonance spectroscopy

Oxide electron tunneling

Oxide electronic structures

Oxide valence electronic structure

Oxides electronic properties

Oxides, electronic state

Oxidized Having lost electrons

Oxidized Having lost electrons chemical reaction

Oxidized electron transfer mediator

Oxidizing agent reactant that accepts electrons from another

Perovskite oxides oxygen pressure dependence, electronic

Photoinduced Electron-transfer Oxidation

Proton-Electron Conducting Oxides

Quinone diacetals electron-transfer oxidation

Radical cations electron-transfer oxidation

Radical electron oxidation

Reduction potentials electron-transfer oxidation

Reorganization energy electron-transfer oxidation

Scanning electron microscopy aluminium oxide

Scanning electron microscopy copper oxide

Scanning electron microscopy metal oxide deposition

Scanning electron microscopy oxide

Scanning electron microscopy oxide layer thickness

Scanning electron microscopy oxide precipitate

Scanning electron microscopy zinc oxide

Sensitizers electronically excited, oxidation

Simple oxides, structural and electronic phase transitions

Single electron transfer oxidation

Single-electron oxidant

Single-electron oxidation

Singly occupied molecular orbital single electron transfer oxidation

Skill 22.1 Using chemical principles (including thermodynamics) to analyze important biochemical processes (e.g., synthesis, degradation, electron transport, oxidative phosphorylation)

Solvated electron standard oxidation potential

Solvent cage electron-transfer oxidation

Sputtering, Electron Bombardment, Oxide-Chloride Conversion

Titanium oxide electronic properties

Titanium oxide electronic structure

Titanium oxidized, Auger electron

Transmission electron microscopy manganese oxide

Trapped Electrons in Water and Deuterium Oxide

Tungsten oxide electron microscopy

Two-Electron Oxidation Processes

Two-electron oxidation

Two-electron oxidation mechanisms

Vanadium oxide, electron paramagnetic

Vanadium oxide, electron paramagnetic complexation

Vanadium oxides, bulk electronic

Water four-electron oxidation

Zirconium oxide electronic conductivity

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