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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...
Complexometric Titration: Overview00:39

Complexometric Titration: Overview

Complexometric titration involves the formation of a complex by reacting a metal ion with one or more ligands. A visual indicator often detects the end point of a complexometric titration. It is added to the metal solution before the titration, forming a stable metal–indicator complex and imparting color to the solution. As the titration approaches the equivalence point, the excess of the added ligand displaces the indicator from the metal–indicator complex, releasing the free indicator. The...
Cycloaddition Reactions: MO Requirements for Photochemical Activation01:12

Cycloaddition Reactions: MO Requirements for Photochemical Activation

Some cycloaddition reactions are activated by heat, while others are initiated by light. For example, a [2 + 2] cycloaddition between two ethylene molecules occurs only in the presence of light. It is photochemically allowed but thermally forbidden.
Reaction Mechanisms03:06

Reaction Mechanisms

Chemical reactions often occur in a stepwise fashion, involving two or more distinct reactions taking place in a sequence. A balanced equation indicates the reacting species and the product species, but it reveals no details about how the reaction occurs at the molecular level. The reaction mechanism (or reaction path) provides details regarding the precise, step-by-step process by which a reaction occurs.
For instance, the decomposition of ozone appears to follow a mechanism with two steps:
Redox Titration: Overview01:21

Redox Titration: Overview

Redox titration is a chemical analysis technique used to determine the concentration of an unknown substance by measuring the electron transfer in a redox (reduction-oxidation) reaction. The process involves gradually adding a titrant with a known concentration of an oxidizing or reducing agent, to the analyte, the solution with an unknown concentration, until reaching the endpoint, which indicates the completion of the reaction between the two substances. Ensuring the analyte is in a single...
Redox Titration: Other Oxidizing and Reducing Agents01:26

Redox Titration: Other Oxidizing and Reducing Agents

Besides iodine, other oxidizing or reducing agents can serve as titrants in redox titrations. Common oxidizing titrants include KMnO4, cerium(IV), and K2Cr2O7. The choice of oxidizing titrants depends on factors like stability, cost, analyte strength, and reaction rate between the analyte and titrant. KMnO4 is a strong oxidizing titrant that reduces from Mn(VII) to Mn(II) in a highly acidic solution, simultaneously oxidizing the analyte to a higher oxidation state. In this case, KMnO4 acts as a...

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A clock reaction based on molybdenum blue.

Ulrich Neuenschwander1, Arnaldo Negron, Klavs F Jensen

  • 1Department of Chemical Engineering, Massachusetts Institute of Technology, 77 Massachusetts Avenue, Cambridge, Massachusetts 02139, USA.

The Journal of Physical Chemistry. A
|May 3, 2013
PubMed
Summary
This summary is machine-generated.

Researchers discovered a novel reversible clock reaction in cyclohexanol using a molybdenum complex and hydrogen peroxide. This finding expands the known scope of clock reactions and suggests potential applications in catalysis.

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Area of Science:

  • Chemical Kinetics
  • Catalysis

Background:

  • Clock reactions are rare kinetic phenomena, typically observed in aqueous systems with ionic oxoacids.
  • Previous studies have primarily focused on ionic species in water for clock reactions.

Purpose of the Study:

  • To report a new clock reaction in a non-aqueous solvent (cyclohexanol).
  • To investigate a reversible clock reaction involving a noncharged molybdenum complex and hydrogen peroxide.
  • To elucidate the reaction mechanism and its potential applications.

Main Methods:

  • Experimental characterization of the reaction kinetics.
  • Quantum chemical calculations to support mechanistic insights.
  • Numerical kinetic modeling to validate the proposed mechanism.

Main Results:

  • A novel, reversible clock reaction was observed in cyclohexanol, forming molybdenum blue from a yellow molybdenum precursor.
  • The reaction exhibits multiple, consecutive clock cycles due to its reversible nature.
  • The mechanism involves sigmatropic rearrangements and is linked to hydrogen peroxide depletion.

Conclusions:

  • The study introduces a new class of clock reactions in organic solvents.
  • The reversible nature and potential catalytic applications in alcohol oxidation are highlighted.
  • The findings contribute to understanding complex kinetic phenomena and molybdenum chemistry.