Sulfur has the same electron configuration as oxygen, though as a larger atom and one with a d-orbital into which it can hybridize, sulfur has different properties and can make different molecular geometries than oxygen. (The wireframe simply indicates the boundary of the n=3 shell, since there are no electrons defining the boundary of its sphere.)
The outer spheres above simply indicate the directions of maximum electron density. The orbitals themselves will be more like spherical tetrahedra that can only occupy volume within their shell. The entire shell will be filled with electron density. It will be highest at the center of the face of each orbital and will decrease toward the nodal regions that divide the shell into four equal volumes, where electron density will be lowest. Like argon, sulfur features two nested spherical tetrahedra, the inner 2nd shell comprising 4 di-electrons, the outer 3rd shell comprising 2 di-electrons and 2 single electrons. In this case the two orbitals containing the di-electrons (dark pink) will occupy slightly more volume than the two containing an unpaired electron.
As the structure below indicates, it is common for sulfur to make two bonds. In its natural crystalline form, sulfur forms S8 rings where each sulfur atoms is bonded to two adjacent sulfur atoms. Like oxygen (though not quite as strongly), sulfur is keen to gain two electrons in an ionic interaction in order to reach the stability of the 3s23p6 noble gas configuration of argon, which is a multi-di-electron state with three concentric full shells. That is why sulfur forms a 2– ionic state. The negative ion is much larger than its neutral version because electrons now outnumber protons by two. This results in a lower effective nuclear charge — a lower average attraction by the nucleus on each electron, which expands the size of the electron shell as it is attracted inward with less force.
But if sulfur is approached by highly electronegative atoms like oxygen or fluorine, they can induce sulfur’s paired valence electrons to uncouple, yielding 6 unpaired electrons available for bonding. This is only possible because the 3rd shell contains a d-orbital. While sulfur does not usually have electrons in its 3d-orbital, the 3rd shell has enough volume to accommodate those orbitals. This allows sulfur to hybridize into those empty d-orbitals and to make up to 6 covalent bonds, as we see in the octahedral SF6 molecule.
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