What do you call the energy required to start a chemical reaction?

The energy required to initiate a chemical reaction is known as activation energy. This is the minimum amount of energy that reactants must possess for a reaction to occur. The concept of activation energy is crucial because, during a chemical reaction, bonds in the reactants must be broken, which requires energy input. Without sufficient activation energy, the reactants remain unreactive regardless of their concentration or temperature.

Activation energy can be thought of as a barrier that reactants must overcome for a reaction to proceed. It determines the rate of a reaction; higher activation energy means that fewer molecules will have enough energy to react at a given temperature. This is why catalysts are often used to lower the activation energy, making it easier for the reaction to occur.

In contrast, potential energy is related to the stored energy within a system due to its position, while kinetic energy relates to the energy of motion. Catalytic energy is not a standard term in chemistry; rather, catalysts work by lowering the activation energy needed for a reaction to take place. Understanding activation energy is key when studying reaction dynamics and thermodynamics in chemistry.