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Related Concept Videos

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:
Temperature Dependence on Reaction Rate02:55

Temperature Dependence on Reaction Rate

The Collision Theory
Atoms, molecules, or ions must collide before they can react with each other. Atoms must be close together to form chemical bonds. This premise is the basis for a theory that explains many observations regarding chemical kinetics, including factors affecting reaction rates.
The collision theory is based on the postulates that (i) the reaction rate is proportional to the rate of reactant collisions, (ii) the reacting species collide in an orientation allowing contact between...
Predicting Reaction Outcomes02:24

Predicting Reaction Outcomes

Kinetics describes the rate and path by which a reaction occurs. In contrast, thermodynamics deals with state functions and describes the properties, behavior, and components of a system. It is not concerned with the path taken by the process and cannot address the rate at which a reaction occurs. Although it does provide information about what can happen during a reaction process, it does not describe the detailed steps of what appears on an atomic or a molecular level. On the other hand,...
Reversible or Opposing Reactions01:26

Reversible or Opposing Reactions

Reversible or opposing reactions play a crucial role in understanding the dynamic nature of chemical processes. While kinetics focuses on how reactions proceed, thermodynamics emphasizes that most reactions do not reach completion. Instead, a reverse reaction starts occurring over time, and when its rate equals that of the forward reaction, a dynamic equilibrium is established.For example, consider a simple chemical process where A forms B reversibly. The rate constants for the forward and...
Dynamic Equilibrium02:20

Dynamic Equilibrium

A reversible chemical reaction represents a chemical process that proceeds in both forward (left to right) and reverse (right to left) directions. When the rates of the forward and reverse reactions are equal, the concentrations of the reactant and product species remain constant over time and the system is at equilibrium. A special double arrow is used to emphasize the reversible nature of the reaction. The relative concentrations of reactants and products in equilibrium systems vary greatly;...
Radical Reactivity: Overview01:11

Radical Reactivity: Overview

Radicals, the highly reactive species, gain stability by undergoing three different reactions. The first reaction involves a radical-radical coupling, in which a radical combines with another radical, forming a spin‐paired molecule. The second reaction is between a radical and a spin‐paired molecule, generating a new radical and a new spin‐paired molecule. The third reaction is radical decomposition in a unimolecular reaction, forming a new radical and a spin‐paired molecule. These three...

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An Analog Macroscopic Technique for Studying Molecular Hydrodynamic Processes in Dense Gases and Liquids
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Dynamics of reactions between two closed-shell molecules.

Jim J Lin1

  • 1Institute of Atomic and Molecular Sciences, Academia Sinica, Taipei 10617, Taiwan. jimlin@gate.sinica.edu.tw

Physical Chemistry Chemical Physics : PCCP
|October 1, 2011
PubMed
Summary
This summary is machine-generated.

Reactions between two stable molecules are rarely studied using crossed molecular beams. This review highlights barrierless F(2) + organosulfur reactions and discusses discrepancies in F(2) + alkene reaction barriers.

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Area of Science:

  • Chemical Kinetics
  • Molecular Dynamics
  • Reaction Mechanisms

Background:

  • The crossed molecular beam technique is a powerful tool for studying elementary chemical reactions.
  • Most studies focus on reactions involving atoms or radicals, with fewer investigating reactions between two stable molecules.

Purpose of the Study:

  • To review and discuss reactions between two stable molecular reactants studied using the crossed molecular beam method.
  • To provide insights into reaction paths, barriers, and unique features of these reactions.

Main Methods:

  • Utilized the crossed molecular beam technique.
  • Employed vacuum ultraviolet (VUV) photoionization for unambiguous identification of nascent products.
  • Integrated experimental data with ab initio calculations to construct reaction path models.

Main Results:

  • Identified unambiguous nascent products for reactions between stable molecules.
  • Demonstrated barrierless F(2) + organosulfur reactions, the first such examples between closed-shell reactants.
  • Observed a decrease in the F(2) + alkene reaction barrier with increased methyl substitution, though experimental and theoretical barrier heights show a ~2 kcal mol(-1) discrepancy.

Conclusions:

  • Crossed molecular beam studies provide detailed insights into reactions between stable molecules.
  • Barrierless reactions between closed-shell molecules are feasible, as shown by F(2) + organosulfur systems.
  • Discrepancies in F(2) + alkene reaction barriers highlight areas for future theoretical and experimental investigation.