Well, sulphur in SF6 for istance has got a sp3d2 hybridization and I can see why, it has got the principal quantum numer n=3 and therefore it has got the possibility to
occupy atomic orbitals of "d" kind and it finally has got (after the hybridization) 6 unpaired elctrons.
But why in H2SO4 sulphur has got a sp3 hybridization? How is it possible? I see, the structure is tetrahedral but, if it has got a sp3 hybridization, the hybridized orbitals are s (1) and p (3) and consequently the structure should be with two lone pairs and two unpaired electrons. On the contrary there are, in the H2SO4 structure, 6 unpaired electrons (which should be obtained from the sp3d2 hybridization).
Conclusion: why in H2SO4 the hybridization is sp3 and not sp3d2?
How can the sp3 hybridization (which should involve just 1 "s" orbital and 3 "p" orbitals gives rise to 6 unpaired electrons?
p.s = it's all the same for SO3, isn't it? But there why is the hybridization sp2 and not sp3d2 again?
I'm sorry, I know it will be surely easy for you but I've been looking for the answer everywhere, but I really can't understand.
Thanks to all who will try to help me out.