Collision Theory Flashcards
Activation energy
The minimum energy required to start a chemical reaction OR the energy required to form the activated complex
Transition state
The state which corresponds to the highest potential energy along it’s reaction coordinate
The heat of reaction/Enthalpy
The net change in the chemical potential energy of the system
In order for a reaction to take place THREE things must occur:
1) In the correct orientation
2) Must have sufficient energy
3) They must collide with each other
Exothermic Reaction
Reactions which transform chemical potential energy into thermal energy
Endothermic Reaction
Reactions which transform thermal energy into chemical potential energy
Activated Complex
A high energy, unstable, temporary transition state between the reactants and the products
Reaction Rate
The change in concentration per unit time of either a reactant or product
Catalyst
A substance that increases the rate of the reaction but remains unchanged at the end of the reaction
