Advanced Placement (AP) Chemistry Practice Exam

A triple bond exhibits the highest bond energy because it involves three pairs of shared electrons between two atoms, which creates a strong attraction that holds the atoms together. This increased number of shared electrons contributes to greater electron density between the nuclei of the bonded atoms, resulting in more effective nuclear attraction and, consequently, higher bond energy. Bond energy refers to the amount of energy required to break a bond; thus, the stronger the bond, the higher the energy needed to break it.

In contrast, single bonds involve one pair of shared electrons, and while double bonds have two pairs, neither matches the strength of a triple bond. Metallic bonds, while also strong, operate through a different mechanism involving a 'sea' of delocalized electrons that allows for conductivity and malleability, but they do not typically exhibit bond energy values as high as those of covalent bonds. Therefore, the significant strength of a triple bond is what allows it to exhibit the highest bond energy among the options.

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