[Apnea]

Hi, I am having some problems visualizing the formation of the pi bonds in the sulfate ion.  i understand that since the preferred form of the ion is to have 2 double bonded Os and 2 single bonded ones.  thus the e- geometry is going to be tetrahedral on the S and the 2 single bonded Os and trigonal planar on the 2 double bonded Os.  Now, i see that the lewis model shows the S being double bonded to the 2 double bond Os, however the actual formation of the 2 separate pi bonds, aren't really that separate are they?  The sulfur atom here has almost no actual overlapping of its orbitals with that of the unhybridized p orbitals from the 2 double bonded(trigonal planar) Os does it?  IE no orbitals of the Sulfur are actually used for the pi bonds?   or am i just totally out in left field here?  any thoughts would be helpful, thanks much!