5 posts • Page 1 of 1
Pi bonds inhibit rotation in a molecule because the orbitals that are interacting to form the bond are arranged side-by-side, not end-to-end. Since they are arranged side-by-side, rotating the molecule would prevent the orbitals from overlapping, break the pi bond, and would require a chemical reaction.
The region of electron density for an pi bond is not actually on the bond axis, but rather parallel "on top" and "below" it, creating a bean-shaped region of e- density. Therefore, if the bond rotates, the bean-shape will break because the regions of electron density are no longer parallel. Sorry if this explanation confuses instead of helps you. I suggest googling a picture of pi bonds, it makes much more sense if you have a visual.
Who is online
Users browsing this forum: No registered users and 1 guest