Chemistry
Activation Energy in Transition States
Quick fact
Even exothermic reactions need an initial boost of energy to get started!
Why this is interesting
Ever wondered why some reactions happen quickly while others take ages? It all starts with a tiny energy hurdle called activation energy.
Read the full explanation
Understanding Activation Energy in Transition States
When reactants collide, they must overcome an energy barrier to form products. This high-energy state is the transition state, and the minimum energy needed to reach it is the activation energy. Imagine pushing a ball up a hill – you need some push to get it over the top.
A deeper explanation
Activation energy is the energy required for reactants to enter the transition state, which is the highest point on the reaction pathway. It determines how fast a reaction occurs. Lowering the activation energy (e.g., using a catalyst) makes reactions happen more readily, while higher barriers slow them down.