Final answer:
In chemical reactions, breaking bonds is commonly associated with the consumption of energy, but usually leads to the release of energy. While synthesis reactions require energy to form bonds, decomposition reactions release energy when bonds are broken.
Step-by-step explanation:
A chemical reaction in which bonds are broken is usually associated with the consumption of energy. However, it's important to note that although energy is required to initiate the breaking of bonds, when bonds break, energy is often released. In chemistry, we have different types of chemical reactions, two of which include synthesis and decomposition reactions. Synthesis reactions involve combining two or more reactants to form a new, larger molecule and require the input of energy. On the other hand, in decomposition reactions, a compound breaks down into two or more components, and energy is released in the process.
Based on the provided information, when addressing the type of chemical reaction where bonds are broken, it is generally related to either decomposition reactions or one part of exchange reactions. Decomposition reactions are notable for breaking bonds within a molecule resulting in the release of energy. Exchange reactions are more complex, involving both the breaking and forming of bonds, and entail both the absorption and release of energy.
Therefore, breaking of bonds in chemical reactions is most commonly associated with the consumption of energy to initiate the reaction, but followed by the release of energy as the reaction proceeds.