What happens during a chemical reaction that involves activation energy?

In a chemical reaction, activation energy refers to the minimum amount of energy that must be supplied for the reactants to undergo a transformation into products. This energy is needed to break existing bonds in the reactants and allow new bonds to form, resulting in the creation of products.

When energy is provided, it can cause the reactants to overcome the energy barrier necessary for the reaction to take place. This can occur through various means, such as thermal energy, where heat increases the kinetic energy of molecules, or through the action of a catalyst, which lowers the activation energy required. Upon overcoming this barrier, the reactants can successfully convert into products.

The remaining options either misunderstand the role of activation energy or imply that reactions can happen without overcoming the energy barrier required for bond rearrangement and transformation. The role of activation energy is crucial—without providing the necessary energy, the reaction would not proceed, which solidifies the correct choice as the one that describes the transformation of reactants into products once sufficient energy has been supplied.