Glossary of Medical Terms

Our online medical glossary of medical terms and definitions includes definitions for terms related to treatment, and general medicine


This theory assumes that molecules should collide in order to react. The more collisions the more likely it is for a reaction to occur. However, depending on the conditions, only a little fraction of the collisions are effective in producing a reaction. There are different constraints. In order for a reaction to occur, bonds initially are broken, which requires energy. This energy depends on the type of the reaction and comes from the kinetic energies that the molecules possess till the collision. It is called the activation energy. Increasing the temperature increases the kinetic energies and more collisions will occur. In adition, at a higher temperature a greater number of the reacting molecules might possess an energy equal to or greater than the activation energy. However the molecules should also collide in a specific orientation, called the steric factor in order for a reaction to occur. A reaction will only be successful, if the collision has satis energy to be either equal to or greater than the activation energy and if the orientation of the collision allows for correct bond formation. These factors are in the Arrhenius equation: k = zp The course constant k is proportional to the Arrhenius factor A. A is the product of the collision frequency z, and the steric factor p. The fraction of collisions with sufficient energy to manufacture a reaction are in the term of the equation.
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