Final answer:
The bond energy is higher for a carbon and oxygen double bond (C=O) due to the combined strength of one sigma and one pi bond, with greater orbital overlap and resulting stronger bond compared to a single sigma bond. The polarity of the double bond also contributes to its strength.
Step-by-step explanation:
The bond energy is higher for double-bonded carbon and oxygen (C=O) because additional bonds require more energy to break. In a double bond, there is one σ (sigma) bond and one π (pi) bond. The σ bond has a greater degree of orbital overlap than the π bond, making it stronger. While each individual π bond is generally weaker than a corresponding σ bond between the same two atoms, the combination of one σ and one π bond in a double bond results in a greater overall bond energy compared to a single σ bond.
Furthermore, the carbon-to-oxygen double bond is quite polar, with the electronegative oxygen atom having a greater attraction for the bonding electron pairs. This polarity also contributes to the strength of the bond. As the bond strength increases, the bond length generally decreases, making the bond harder to break and thus having higher bond energy.