Suppose a hydrogen atom is excited up to a $\underset{1s}{[\;]} \underset{2s}{[\uparrow]}$ state which takes about 1000 kJ/mol.

Due to electron shielding f orbitals tend to be higher energy than d orbitals which are higher than p orbitals which are higher than s orbitals. But in a hydrogen atom there is only one electron so the 2s and 2p orbitals are equivalent in energy.

So there's no difference in energy with $\underset{1s}{[\;]} \underset{2s}{[\;]} \underset{2p}{[\uparrow \vert \; \vert \;]}$.

Now there are three different symmetrical p orbitals so I think the end result might still be spherical. But would the radius of the excited hydrogen atom be an overall higher radius then one would typically expect?

I don't know how to square this with http://physics.stackexchange.com/questions/144819/how-big-is-an-excited-hydrogen-atom which seems to be mostly talking about general approximations for very highly excited states or the fine details of the Schrodinger equation which I don't really understand.

I also don't know if this applies to molecules. Are the 2p orbitals and 2s orbitals equivalent in energy when a hydrogen atom is bounded to another atom?