Final answer:
Energy release actions in chemical reactions rely on the breaking and forming of chemical bonds, involving kinetic energy to drive collisions and potential energy released as heat and/or work. Free energy represents usable energy post-losses, and activation energy initiates reactions.
Step-by-step explanation:
The energy release action in chemical reactions depends on the breaking and forming of chemical bonds. When a chemical bond is formed, energy is released, while the breaking of a bond requires energy. For the same type of bond, the amount of energy needed to break it is equal to the energy released upon making it. The measure of energy transfer during chemical reactions is known as free energy, which is the usable energy available to do work after losses are accounted for.
Kinetic energy drives the collisions necessary for bond breakage and formation during chemical reactions, while potential energy stored in the molecular bonds is released during this process. All systems tend to move toward the lowest possible energy state, meaning that during a reaction, potential energy is released as heat and/or work into the surroundings. Activation energy is required for a reaction to proceed, which is the energy needed to initiate the reaction, usually facilitated by a catalyst.