Students will be guided through modeling a full chemical reaction by counting the number of bonds that must be broken versus the number of bonds formed in order to determine if the overall reaction is likely endothermic or exothermic. Individual bond breaking and bond making steps will be included in the model as well as the PE/KE of the system/surroundings throughout the reaction.
The Law of Conservation of Energy states that energy is neither created nor destroyed in any chemical reaction. Thus, we can determine if a chemical reaction is endothermic or exothermic by quantifying both the amount of energy transferred from the surroundings into the system to break bonds, and the amount of energy released from the system back into the surroundings when bonds are formed.
You will need the following resources to complete this assignment.
Your instructor will begin by modeling an endothermic chemical reaction on the board for you using a set amount of energy (potential energy + kinetic energy) that will be traced from the surroundings into the system and back out again. The amount of energy absorbed or released will be based on the number of bonds that are broken versus the number of new bonds formed in the chemical reaction.
After your instructor models the endothermic reaction, you will model an exothermic reaction on your handout using the same principles and ideas demonstrated in your instructor's model on the board. Then you will practice modeling two more chemical reactions; you will need to determine if these reactions are endothermic or exothermic during the modeling process to ensure the correct amount of energy absorbed or transferred throughout the chemical reaction