Collision theory

Collision theory is a theory in physical chemistry that explains how chemical reactions occur and why reaction rates differ for different reactions. The theory was proposed independently by Max Trautz in 1916 and William Lewis in 1918.

Pronunciation

• /kəˈlɪʒən θɪəri/

Etymology

The term "collision theory" is derived from the concept of molecules colliding, which is a fundamental aspect of the theory. The word "collision" comes from the Latin collisio, meaning "a striking together", and the word "theory" comes from the Greek theoria, meaning "a looking at, viewing, beholding".

Definition

Collision theory states that for a reaction to occur, it is necessary for the reacting species (atoms or molecules) to come together or collide with one another. Not all collisions, however, bring about chemical change. A collision will be effective in bringing about a chemical change only if the species brought together possess a certain minimum amount of energy, called the activation energy.

Related Terms

• Activation energy
• Chemical kinetics
• Molecular dynamics
• Reaction rate
• Stoichiometry

See Also

• Transition state theory
• Rate equation
• Arrhenius equation

References

• Lewis, W. K. (1918). "The Theory of Rate of Reaction". Journal of Physical Chemistry. 22 (4): 198–210.
• Trautz, M. (1916). "The Theory of Reaction Speeds". Zeitschrift für anorganische und allgemeine Chemie. 156 (1): 245–253.

External links

• Medical encyclopedia article on Collision theory
• Wikipedia's article - Collision theory

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