The bond having the highest bond energy is

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(C) The bond energy depends on the extent of orbital overlap and the bond length. Oxygen has a smaller atomic size compared to sulfur,and carbon has a

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$C = O$

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(C) The bond energy depends on the extent of orbital overlap and the bond length. Oxygen has a smaller atomic size compared to sulfur,and carbon has a smaller size compared to phosphorus. Due to the smaller size of the $O$ atom,the $2p-2p$ sideways overlap between $C$ and $O$ is more effective than the $2p-3p$ overlap in $C=S$ or other combinations. Additionally,oxygen is highly electronegative,which contributes to a stronger bond. Therefore,the $C = O$ bond has the highest bond energy among the given options.

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