What term do we use to describe a reaction that liberates heat to its surroundings? How does the chemical energy change during such a reaction? What is the algebraic sign of \(q\) for such a reaction?

Chemical potential energy is the energy stored within the chemical bonds of substances. It's a form of potential energy based on the position and arrangement of atoms and molecules. During a chemical reaction, this potential energy can change as old bonds break and new ones form. In an exothermic reaction, such as combustion, the chemical potential energy of the reactants is higher than that of the products.

As the reactants undergo a transformation to become the products, a portion of the stored energy is released into the surroundings. This release occurs because the energy required to break the bonds in the reactants is less than the energy released when new bonds form in the products. Therefore, the overall potential energy drops, and this excess energy is emitted as heat. Understanding chemical potential energy is crucial for grasping why some reactions release heat while others absorb it.

Heat flow in reactions refers to the transfer of energy due to a temperature difference between the system and its surroundings. In the context of chemical reactions, when we talk about a system, we're typically referring to the reactants and products involved in the reaction, while everything else constitutes the surroundings.

In an exothermic reaction, heat flows out of the system and into the surroundings, which can often be observed as an increase in temperature. The 'q' value, which represents the quantity of heat involved, is assigned a negative sign to indicate this outward flow of heat. Conversely, for an endothermic reaction, where the system absorbs heat from the surroundings, 'q' would be positive. Visualizing heat flow can help students grasp why the temperature changes in their surroundings during different types of chemical reactions.

Thermochemistry is the branch of chemistry that deals with the energy changes involved in chemical reactions and the exchange of energy with the surroundings. It's a subfield of thermodynamics focused primarily on heat and work—two primary forms of energy transfer. Through the study of thermochemistry, students can understand how energy conservation plays a role in chemical reactions and how these energy changes affect matter at the molecular level.

Key concepts in thermochemistry include enthalpy, which is the total heat content of a system, and the first law of thermodynamics, which states that energy cannot be created or destroyed, only transformed or transferred. By applying these concepts, it becomes clear why exothermic reactions, which release heat, have a negative 'q' value and why these reactions often occur spontaneously—because the system tends to move towards a state of lower energy and greater stability.