redox

(noun)

a shorthand term for "reduction-oxidation," two methods of electron transfer that always occur together

Related Terms

  • donor atom
  • oxidation
  • voltaic cell
  • half-cell
  • reaction
  • coordination
  • reduction
  • half-reactions
  • combustion

(noun)

A reversible chemical reaction in which one reaction is an oxidation and the reverse is a reduction.

Related Terms

  • donor atom
  • oxidation
  • voltaic cell
  • half-cell
  • reaction
  • coordination
  • reduction
  • half-reactions
  • combustion

Examples of redox in the following topics:

  • Redox Titrations

    • Redox titration determines the concentration of an analyte containing either an oxidizing or a reducing agent.
    • A student conducts the redox titration and reaches the endpoint after adding 25 mL of the titrant.
    • There are various other types of redox titrations that can be very useful.
    • A redox titration using potassium permanganate as the titrant.
    • Calculate the concentration of an unknown analyte by performing a redox titration.
  • Types of Redox Reactions

    • Redox reactions are all around us.
    • In fact, much of our technology, from fire to laptop batteries, is largely based on redox reactions.
    • Redox (reduction-oxidation) reactions are those in which the oxidation states of the reactants change.
    • In some redox reactions, substances can be both oxidized and reduced.
    • This is an example of a combustion reaction, a redox process.
  • Balancing Redox Equations

    • For example, look at the following redox reaction between iron and copper:
    • If a reaction occurs in an acidic environment, you can balance the redox equation as follows:
    • The following is an unbalanced redox equation that takes place in acidic solution:
    • A great walkthrough on how to balance a redox reaction in basic solution.
    • A great walkthrough on how to balance a redox reaction in acidic solution.
  • Thermodynamics of Redox Reactions

    • The thermodynamics of redox reactions can be determined using their standard reduction potentials and the Nernst equation.
    • In order to calculate thermodynamic quantities like change in Gibbs free energy $\Delta G$ for a general redox reaction, an equation called the Nernst equation must be used.
    • Translate between the equilibrium constant/reaction quotient, the standard reduction potential, and the Gibbs free energy change for a given redox reaction
  • Predicting Spontaneous Direction of a Redox Reaction

    • The direction of a redox reaction depends on the relative strengths of the oxidants and reductants in a solution.
    • Generally, the direction of a redox reaction depends on the relative strengths of oxidants and reductants in a solution.
    • In order to predict if two reactants will take part in a spontaneous redox reaction, it is important to know how they rank in an electrochemical series.
    • Predict the direction of electron flow in a redox reaction given the reduction potentials of the two half-reactions
  • Balancing Redox Equations

    • Balancing redox reactions depends on conservation of mass and electrons; the exact method varies with basic or acidic solutions.
    • Redox (oxidation-reduction) reactions include all chemical reactions in which atoms have their oxidation states changed.
    • An alternative method for balancing reduction/oxidation (redox) reactions.
    • It consists of four steps that, if followed, can balance any redox equation.
    • Produce a balanced redox equation from an unbalanced one in either acidic or basic media
  • Free Energy and Cell Potential

    • In a galvanic cell, where a spontaneous redox reaction drives the cell to produce an electric potential, the change in Gibbs free energy must be negative.
    • In a galvanic cell, where a spontaneous redox reaction drives the cell to produce an electric potential, the change in Gibbs free energy must be negative.
    • Calculate the change in Gibbs free energy of an electrochemical cell where the following redox reaction is taking place:
    • Because the change in Gibbs free energy is negative, the redox process is spontaneous.
    • Calculate the change in Gibbs free energy of an electrochemical cell, and discuss its implications for whether a redox reaction will be spontaneous
  • Oxidation of Phenols

    • The redox equilibria between the dihydroxybenzenes hydroquinone and catechol and their quinone oxidation states are so facile that milder oxidants than chromate (Jones reagent) are generally preferred.
    • The position of the quinone-hydroquinone redox equilibrium is proportional to the square of the hydrogen ion concentration, as shown by the following half-reactions (electrons are colored blue).
  • Voltaic Cells

    • A voltaic cell is a device that produces an electric current from energy released by a spontaneous redox reaction in two half-cells.
    • An electrochemical cell is a device that produces an electric current from energy released by a spontaneous redox reaction.
    • The operating principle of the voltaic cell is a simultaneous oxidation and reduction reaction, called a redox reaction.
    • This redox reaction consists of two half-reactions.
    • In a typical voltaic cell, the redox pair is copper and zinc, represented in the following half-cell reactions:
  • Standard Reduction Potentials

    • Reduction potential (also known as redox potential, oxidation/reduction potential, or Eh) measures the tendency of a chemical species to acquire electrons and thereby be reduced.
    • However, because these can also be referred to as "redox potentials," the terms "reduction potentials" and "oxidation potentials" are preferred by the IUPAC.
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