Final answer:
Weaker chemical bonds imply a less stable structure with higher potential energy. Greater bond energy signifies stronger bonds resulting in less reactivity. Single, double, and triple bonds show increasing bond strength and stability with higher bond energies.
Step-by-step explanation:
When the question states 'Weaker bonds= less stable= ___ energy,' the blank is to be filled with the concept of higher energy. This is because weaker bonds in molecules represent a less stable structure, which inherently contains higher potential energy. Bond energy is a critical concept here, signifying the amount of energy required to break a covalent bond between two atoms. Compounds with higher bond energies have stronger bonds and are more stable, thus, they are less reactive. Conversely, molecules with weaker bonds are less stable and have higher potential energy, making them more reactive due to the lower energy required to disrupt those bonds.
A good example is comparing single, double, and triple bonds: Triple bonds are stronger and shorter than double bonds, and double bonds are stronger and shorter than single bonds. This varying bond strength correlates to different bond energies — a triple bond has a higher bond energy and is more stable compared to a single bond.