Looking at 1,3-Butadiene and Isoprene, I'm wondering: why does Isoprene have a higher boiling point, but a lower melting point than 1,3-Butadiene?

I'm thinking this might be because the Methyl group on C(2) in Isoprene might cause it's lattice to be less tightly packed, thus requiring less energy to be split (-> lower melting point). As both substances can't form any ion-ion, nor dipole-dipole, nor hydrogen bonds, Isoprene probably has a higher boiling point than 1,3-Butadiene because it has a larger surface, enabling it to develop stronger London (VdW) forces.

Can anyone confirm/ disprove this?

Thanks a lot in advance!


Your Answer

By clicking “Post Your Answer”, you agree to our terms of service, privacy policy and cookie policy

Browse other questions tagged or ask your own question.