Question

The bond energy of a C–C single bond averages \({\rm{347 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}\); that of a

C ≡ C triple bond averages \({\rm{839 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}\). Explain why the triple bond is not three times as strong as a single bond.

Short answer

A triple bond has an \({\rm{\sigma }}\) bond and two \({\rm{\pi }}\) bonds, whereas a single bond has only an \({\rm{\sigma }}\) bond. Because sigma bonds are far stronger than \({\rm{\pi }}\) bonds, a triple bond including one \({\rm{\sigma }}\) and two \({\rm{\pi }}\) bonds are not three times as strong as a single bond.

Step-by-step solution

Define bond energy

The amount of energy required to break apart a mole of molecules into its component atoms is known as bond energy (E). It's a metric for how strong a chemical bond is.

Explanation

The triple bond has an \({\rm{\sigma }}\) bond and two \({\rm{\pi }}\) bonds rather of three sigma bonds, whereas a single bond only has an \({\rm{\sigma }}\) bond. The triple bond, which consists of an \({\rm{\sigma }}\)bond and two \({\rm{\pi }}\) bonds, is not three times as strong as a single bond because sigma bonds are much stronger than \({\rm{\pi }}\) bonds.