Beryllium has that p orbital but there just isn't any electrons in it. That's why he showed the configuration with the 2p0. It's there it just isn't occupied. There is the difference between electrons and orbitals. I might be wrong but that's what I am getting out of it.
it is in the 2nd energy level so it technically has a p sublevel that is empty. this is also why we have expanded octets but that occurs with d sublevels.
Nice explanation, but can somebody help me out with the relavance of making the comparison of a simple H1s- Be sp [hybrid] overlap against the H1s - Be2p overlap? Since Be has no p electrons, why would it undergo hybridization when it has a 2s orbital with two electrons that can overlap with the 1s orbitals of the two H atoms? S orbitals are spherically symmetrical, so there sould be ample overlapping and hence stability. Thanks!
I understand the answer now. If anyone was confused by this here's the answer. So when the orbitals 'combine' they don't merge they just create a new type of orbital, which didn't exist before. So in the case of SP hybridization you start of with 1 2P orbital and 1 2S orbital and you make 2 new SP orbitals. Each SP orbital is 50 percent S orbital and 50 percent P orbital. So half the S orbital goes into one SP orbital and the other half goes into the other SP orbital.
Is this the same as bonding/antibonding ? For example if the question was , sketch the resulting bonding/antibonding orbitals between S and Py orbitals
