In my book, Organic Stereochemistry, the following picture is shown:
In the lowest diagram, in Figure 1.3, which shows a π* bond, the positive lobe of the p orbital of atom A is nearest to the negative lobe of the p orbital of atom B. By contrast, in the diagram above it, which shows a π bond, the positive lobe of the p orbital of atom A is nearest to the positive lobe of the p orbital of atom B. It is said that the π* bond is higher in energy, less stable, than the π bond. I would have thought it to be the other way around, due to electrostatic repulsion when two lobes of p orbitals which have the same charge overlap, and the electrostatic attraction when two lobes of p orbitals which have opposite charges overlap.
Why am I wrong? Why is it not this way around?