Final answer:
The bond with the highest bond energy among the given options is the carbon-nitrogen triple bond (C≡N), as triple bonds generally have higher bond energies due to tighter orbital overlap and C and N are small, highly electronegative atoms which contribute to stronger bonds. The correct answer is D. C=N.
Step-by-step explanation:
To identify the bond with the highest bond energy among the options given, we can refer to general trends in bond energies. Typically, multiple bonds (double and triple bonds) are stronger than single bonds and shorter bonds are generally stronger than longer bonds. In most cases, triple bonds have higher bond energies than double bonds due to more extensive overlap of orbitals.
Comparing the provided options:
- Si=O: Silicon-oxygen double bonds are relatively strong, but not as strong as the bonds involving lighter elements.
- C=C: Carbon-carbon double bonds are quite strong.
- N=N: Nitrogen-nitrogen double bonds are strong due to the smaller size and greater electronegativity of nitrogen compared to carbon.
- C≡N: Carbon-nitrogen triple bonds are very strong because of the triple bond.
- O=O: Oxygen-oxygen double bonds are also strong, but typically, bonds with nitrogen are stronger due to the smaller size and higher electronegativity.
Considering these points, the C≡N bond is expected to have the highest bond energy compared to the other bonds listed, as it is a triple bond between relatively small and highly electronegative atoms, which allows for a greater orbital overlap and therefore a stronger bond.