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Redox Equilibria: Overview01:23

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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...
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Ladder diagrams are useful tools for understanding redox equilibrium reactions, especially the effects of concentration changes on the electrochemical potential of the reaction. The vertical axis in the redox ladder diagrams represents the electrochemical potential, E. The area of predominance is demarcated using the Nernst equation.
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On comparing the reactivity of silver and lead, it is observed that the two ionic species, Ag+ (aq) and Pb2+ (aq), show a difference in their redox reactivity towards copper: the silver ion undergoes spontaneous reduction, while the lead ion does not. This relative redox activity can be easily quantified in electrochemical cells by a property called cell potential. This property is commonly known as cell voltage in electrochemistry, and it is a measure of the energy which accompanies the charge...
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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...
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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...
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General Method for Determining Redox Potentials without Electrolyte.

Matthew J Bird1, Matthew A Pearson2, Sadayuki Asaoka3

  • 1Chemistry Department, Brookhaven National Laboratory, Upton, New York 11793-5000, United States.

The Journal of Physical Chemistry. A
|May 22, 2020
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Summary
This summary is machine-generated.

A new method determines redox potentials without electrolytes by measuring ion pair dissociation constants. This allows accurate shifts from electrolyte-influenced to electrolyte-free potentials for various molecules.

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Area of Science:

  • Electrochemistry
  • Physical Chemistry
  • Photochemistry

Background:

  • Redox potentials are crucial for understanding electron transfer reactions.
  • Electrolytes significantly influence measured redox potentials.
  • Accurate electrolyte-free redox potentials are needed for fundamental studies.

Purpose of the Study:

  • To develop a novel method for determining redox potentials without electrolytes.
  • To establish a way to quantify ion pair dissociation constants for radical anions and counterions.
  • To correlate electrolyte-influenced potentials with electrolyte-free values.

Main Methods:

  • Utilized pulse radiolysis to generate radical anions.
  • Determined composite equilibrium constants for electron transfer as a function of electrolyte concentration in THF.
  • Calculated dissociation constants for ion pairs between radical anions and tetrabutylammonium (TBA+) counterions.

Main Results:

  • Quantified dissociation constants for various radical anions with TBA+.
  • Observed significant shifts in reduction potentials for small molecules (+130 mV) versus delocalized systems (+25 mV).
  • Demonstrated that charge delocalization weakens ion pair binding, reducing potential shifts.

Conclusions:

  • The novel method accurately determines electrolyte-free redox potentials.
  • Ion pair dissociation constants are key to understanding and predicting potential shifts.
  • Molecular structure, specifically charge delocalization, dictates the impact of electrolytes on redox potentials.