This statement is false. Activation energy is not the energy that is released when molecules collide; rather, it is the minimum energy required to initiate a chemical reaction.
When two molecules collide, they need to possess a certain amount of energy for a reaction to occur. This energy is referred to as activation energy. If the colliding molecules do not have enough energy, no reaction will take place, even though they may collide. The energy given off during a reaction typically occurs after the reaction has taken place, not during the initial collision.
Essentially, activation energy acts as a barrier to a reaction; only those collisions that provide sufficient energy can successfully lead to products. So, while collisions are essential, the energy involved in overcoming the activation barrier is what truly matters for the reaction to proceed.