In the carbon-carbon bond of an alkene, a $\pi$ bond is considerably weaker than a $\sigma$ bond.

Question

In the carbon-carbon bond of an alkene, a $\pi$ bond is considerably weaker than a  $\sigma$ bond.

Quizplus · Accepted Answer

The pi bond in an alkene is weaker than the sigma bond because it is formed by the overlapping of p-orbitals, which have a diffuse electron density and are located on opposite sides of the carbon-carbon axis. In contrast, the sigma bond is formed by the overlapping of sp3 hybrid orbitals, which have a high electron density concentrated between the two carbon atoms. This makes the sigma bond stronger than the pi bond.

In the Carbon-Carbon Bond of an Alkene, A π\piπ Bond Is Considerably Weaker Than A

In the Carbon-Carbon Bond of an Alkene, A $\pi$ Bond Is Considerably Weaker Than A