Electron delocalisation in conjugated bonds

[nobahar]

Hello!
I'm confused about something I've read.
It says that double bonds that are separated by single bonds can delocalise the electrons, forming conjugated bonds. I guess this is what happens in benzene with the formation of the pi-ring of electrons. It also states that this lowers the energy required to promote the outer electrons. Now, I read, and have held the belief for sometime, that electorn delocalisation increases the stability of the molecule. I took this to mean that the electrons were in a lower energy state when delocalised. This, however, would contradict the statement that the electrons are easier to promote; since if they were in a lower energy state it would require more energy to remove the electrons: if it was in a lower energy state, it would be closer to the nucleus and have a more negative potential energy. I'm starting to wonder if perhaps the stability conferred upon the molecule is due to the delocalisaiton of the electron, but is not due to the electrons being in a lower energy level.
Which is correct? Are electrons in conjugated bonds easier to promote?, or more difficult?
Thanks in advance.

 

[Nino MMP]

Conjugated bonds can indeed lower the energy required to promote the outer electrons, but they also increase the stability of the molecule. The increased stability comes from the fact that the electrons are delocalized and spread out, making them less likely to react with other molecules. This delocalization also reduces the overall energy of the molecule, meaning that it takes less energy to break the bonds between atoms. Therefore, conjugated bonds can both make it easier to promote the outer electrons and make the molecule more stable.