Which bond is stronger, the carbon-oxygen double bond or the carbon-carbon double bond?

The carbon-oxygen double bond is stronger than the carbon-carbon double bond due to several factors related to the specific characteristics and properties of the atoms involved.

Oxygen is more electronegative than carbon, which results in a significant amount of electron sharing in the carbon-oxygen double bond, creating a stronger bond due to the effective overlap of orbitals. The greater electronegativity of oxygen also leads to a bond that is more polar, contributing to stability through stronger charge interactions. Additionally, the shorter bond length typically associated with the carbon-oxygen double bond compared to the carbon-carbon double bond leads to increased bond strength; shorter bonds generally indicate greater overlap of atomic orbitals and a stronger bond.

In contrast, carbon-carbon bonds, although also important in organic chemistry, do not have this same degree of effective orbital overlap or polarity, leading to relatively weaker interactions compared to their carbon-oxygen counterparts. The differences in atomic size and electronegativity also play a crucial role in the overall strength of these bonds, with the oxygen atom contributing increased stability and bond strength when bonded to carbon.

This understanding helps clarify why the carbon-oxygen double bond is stronger, highlighting the influence of atomic properties on bond strength.