The term that describes the gain or loss of energy when bonds are made or broken is "enthalpy."
Explanation:
1. Enthalpy is a thermodynamic quantity that represents the total heat content of a system. It includes the internal energy of the system plus the product of pressure and volume.
2. When bonds are made, energy is usually released, and this process is exothermic. In an exothermic reaction, the enthalpy change (∆H) is negative because the system loses energy to the surroundings.
3. On the other hand, when bonds are broken, energy is absorbed, and this process is endothermic. In an endothermic reaction, the enthalpy change is positive (∆H > 0) because the system gains energy from the surroundings.
4. Enthalpy is a crucial concept in understanding chemical reactions as it helps us predict whether a reaction is exothermic or endothermic based on the enthalpy change.
Therefore, in the context of energy changes during bond formation or breaking, enthalpy is the term that best describes this phenomenon.
