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 ▸

(Essay question) How are cycles important in biology?


What is the rate-determining step?


Why is the first ionisation energy lower in barium compared to calcium?


In terms of structure and bonding explain why the boiling point of magnesium is much higher than that of bromine?


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences