Difference Between Collision Theory and Transition State Theory

Key Difference – Collision这oryvsTransition State Theory

Collision theory and transition state theory are two theories that are used to explain the反应速率of different chemical reactions at the molecular level. Collision theory describes the collisions of gas molecules in gas-phase chemical reactions. Transition state theory explains the reaction rates by assuming the formation of intermediate compounds that are过渡状态。这key difference在碰撞理论和过渡状态理论之间collision theory relates to the collisions between gas molecules whereas transition state theory relates to the formation of intermediate compounds in transition states.

内容

1.Overview and Key Difference
2.What is Collision Theory
3.What is Transition State Theory
4.Side by Side Comparison – Collision Theory vs Transition State Theory in Tabular Form
5.概括

What is Collision Theory?

这collision theory explains that gas-phase chemical reactions occur when molecules collide with sufficientkinetic energy。该理论是基于气体动力学理论建立的（气体的动力学理论描述的是，气体含有没有定义的体积，但具有定义的质量，并且在这些气体颗粒之间没有分子间的景点或排斥）。

According to the collision theory, only a few collisions between gas particles cause these particles to undergo considerable chemical reactions. These collisions are known as successful collisions. The energy required for these successful collisions is known as activation energy. These collisions can cause breakage and formation of chemical bonds.

什么是过渡状态理论？

过渡状态理论表明，在分子为反应物的状态和分子是产物的状态之间，有一个称为过渡状态的状态。过渡状态理论可用于确定基本反应的反应速率。根据这一理论，反应物，产物和过渡态化合物相互平衡。

过渡态理论可以用来能听懂and the mechanism of an elementary chemical reaction. This theory is a more accurate alternative to theArrhenius equation。According to the transition state theory, there are three major factors affecting the mechanism of a reaction;

1. 这concentration of the transition state compound (known as activated complex)
2. 崩溃的速度activated complex- 这决定了所需产品的形成速率
3. 活化复合物的分解方式 - 这确定了化学反应中形成的产物

However, according to this theory, there are two approaches to a chemical reaction; the activated complex may return to the reactant form, or it can break apart in order to form product(s). The energy difference between reactant energy and transition state energy is known as the activation energy.

What is the Difference Between Collision Theory and Transition State Theory?

Collision Theory vs Transition State Theory
碰撞理论解释说，当分子与足够的动能碰撞时，气相化学反应发生。	过渡状态理论表明，在分子为反应物的状态和分子是产物的状态之间，有一个称为过渡状态的状态。
Principle
Collision theory states that chemical reactions (in the gas phase) occur due to collisions between reactants.	过渡状态理论指出，化学反应通过过渡状态发生。
Requirements
According to the collision theory, only successful collisions cause chemical reactions to occur.	根据过渡状态理论，如果反应物能够克服活化能屏障，则化学反应将进展。

概括– Collision这oryvsTransition State Theory

Collision theory and transition state theory are used to explain the reaction rates and mechanisms of different chemical reactions. The difference between collision theory and transition state theory is that collision theory relates to the collisions between gas molecules whereas transition state theory relates to the formation of intermediate compounds in transition states.

Reference:

1.“Collision Theory.” Chemistry LibreTexts, Libretexts, 22 May 2017.Available here
2.“过渡状态理论”。Wikipedia，Wikimedia基金会，2018年2月28日。Available here
3.“9.7: Theories of Reaction Rates.” Chemistry LibreTexts, Libretexts, 21 July 2016.Available here

Image Courtesy:

1.’MOLECULAL-COLLISIONS’SADI_CARNOT（公共领域）通过Commons Wikimedia
2.’Rxn coordinate diagram 5’By Chem540grp1f08 – Own work,(CC BY-SA 3.0)viaCommons Wikimedia