(Polar molecules, Non-polar molecules, etc.)
4 posts • Page 1 of 1
It is safe to assume that whenever you see a single bond, it is a sigma bond because sigma bonds overlap two orbitals end to end, creating one single bond. There is only one overlap, and within this overlap is the single area of electron density. This one overlap gives you a single bond.
Who is online
Users browsing this forum: No registered users and 5 guests