Why is benzene more stable than expected?
All the carbons in benzene are sp2 hybridised. The carbons are each bonded to one hydrogen and all bonds to other carbon atoms in the ring are the same length. This bond is in between the bond length of a C=C and C-C bond. This is because there is a system of p orbitals that can overlap to form a delocalised system of electrons above and below the plane of carbon atoms. This system leads to the benzene ring being more stable than expected.
Related Chemistry A Level answers
All answers ▸(See word doc for complete info) An experiment is carried out whereby the decomposition of hydrogen iodide is observed. Given the equilibrium compositions of each species, calculate the initial mass of hydrogen iodide.
What is the difference between empirical and molecular formula?
Why does phenol readily undergo electrophilic substitution but benzene does not without the aid of a catalyst?
What is the difference between 'Electrospray Ionisation' and 'Electron Impact' during the ionisation stage in a mass spectrometer?