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Related Concept Videos

Redox Reactions01:24

Redox Reactions

Oxidation-reduction or redox reactions involve the transfer of electrons from one molecule or atom to another. When an atom gains an electron, another atom must lose an electron, meaning oxidation and reduction must occur together. Since the redox occurs in pairs, the atom that gets oxidized is also called the reducing agent or reductant, and the atom that is reduced is also called the oxidizing agent or oxidant. A straightforward way to remember the definitions of oxidation and reduction is...
Redox Reactions01:27

Redox Reactions

Redox reactions are vital biochemical processes that underpin energy metabolism in cells. These reactions involve the transfer of electrons between molecules, occurring in tandem as oxidation and reduction. Oxidation refers to the loss of electrons, while reduction denotes their gain. This coupling ensures the seamless flow of electrons through metabolic pathways. For example, in bacterial metabolism, glucose undergoes oxidation to carbon dioxide, while oxygen is simultaneously reduced to...
Oxidation and Reduction of Organic Molecules01:19

Oxidation and Reduction of Organic Molecules

Energy production within a cell involves many coordinated chemical pathways. Most of these pathways are combinations of oxidation and reduction reactions, which occur at the same time. An oxidation reaction strips an electron from an atom in a compound, and the addition of this electron to another compound is a reduction reaction. Because oxidation and reduction usually occur together, these pairs of reactions are called redox reactions.
The removal of an electron from a molecule, results in a...
Redox Equilibria: Overview01:23

Redox Equilibria: Overview

A reduction-oxidation reaction is commonly called a redox reaction. In a redox reaction, electrons are transferred from one species to another rather than being shared between or among atoms. The reducing agent or reductant is the species that loses electrons and gets oxidized in the process. The species that gains electrons and gets reduced in the process is the oxidizing agent or oxidant. Redox reactions are represented as two separate equations called half-reactions, where one equation...
Role of Reduced Coenzymes NADH and FADH₂01:29

Role of Reduced Coenzymes NADH and FADH₂

The energy released from the breakdown of the chemical bonds within nutrients can be stored either through the reduction of electron carriers or in the bonds of adenosine triphosphate (ATP). In living systems, a small class of compounds functions as mobile electron carriers, molecules that bind to and shuttle high-energy electrons between compounds in pathways. The principal electron carriers that will be considered originate from the B vitamin group and are derivatives of nucleotides; they are...
Reduction of Alkenes: Asymmetric Catalytic Hydrogenation02:17

Reduction of Alkenes: Asymmetric Catalytic Hydrogenation

Catalytic hydrogenation of alkenes is a transition-metal catalyzed reduction of the double bond using molecular hydrogen to give alkanes. The mode of hydrogen addition follows syn stereochemistry.
The metal catalyst used can be either heterogeneous or homogeneous. When hydrogenation of an alkene generates a chiral center, a pair of enantiomeric products is expected to form. However, an enantiomeric excess of one of the products can be facilitated using an enantioselective reaction or an...

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Protein Film Infrared Electrochemistry Demonstrated for Study of H2 Oxidation by a [NiFe] Hydrogenase
10:01

Protein Film Infrared Electrochemistry Demonstrated for Study of H2 Oxidation by a [NiFe] Hydrogenase

Published on: December 4, 2017

Mild redox complementation enables H2 activation by [FeFe]-hydrogenase models.

James M Camara1, Thomas B Rauchfuss

  • 1School of Chemical Sciences, University of Illinois, Urbana, Illinois 61801, USA.

Journal of the American Chemical Society
|May 10, 2011
PubMed
Summary

Mild oxidants accelerate hydrogen activation by iron complexes, independent of oxidant concentration. This suggests a rate-limiting H2 binding step followed by proton-coupled electron transfer, crucial for understanding catalytic mechanisms.

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Area of Science:

  • Organometallic chemistry
  • Catalysis
  • Bioinorganic chemistry

Background:

  • Hydrogen activation is a key step in many catalytic processes.
  • Iron complexes serve as models for metalloenzyme active sites.
  • Understanding the mechanism of hydrogen activation is crucial for developing efficient catalysts.

Purpose of the Study:

  • To investigate the mechanism of hydrogen activation by novel iron complexes.
  • To explore the role of mild oxidants in accelerating hydrogen activation.
  • To characterize the H(ox) state model for active site investigation.

Main Methods:

  • Kinetic studies of H2 and D2 activation by iron complexes.
  • Spectroscopic analysis.
  • Crystallographic characterization of a key intermediate.

Main Results:

  • Mild oxidants accelerate H2 activation by iron complex [1](+) without direct oxidation.
  • The reaction kinetics are first-order in [1](+) and [H2], independent of oxidant concentration.
  • An inverse kinetic isotope effect (0.75(8)) was observed with D2.
  • Hydrogen activation is significantly enhanced (10^4-fold) by iron complex [2](+), a model for the H(ox) state.

Conclusions:

  • The findings suggest a mechanism involving rate-determining H2 binding followed by proton-coupled electron transfer.
  • The enhanced activity of [2](+) highlights the importance of the amine cofactor in H(ox) state models.
  • These studies provide insights into the fundamental steps of hydrogen activation relevant to catalysis.