= (6 (\textfrom S) + 24 (\textfrom 4 O) + 2 (\textfrom charge) = 32) electrons.
Formal Charge = (Valence electrons) - (Non-bonding electrons) - ½(Bonding electrons) so4 lewis structure
This is an . Sulfur, being in period 3 of the periodic table, has access to empty 3d orbitals. It can “promote” or utilize these d orbitals to accommodate more than 8 electrons. In valence bond theory, this is described by using d orbitals to form dsp³ hybrid orbitals (for 5 electron domains) or sp³d² (for 6). For sulfate, the most common model involves sp³d² hybridization for sulfur, using two d orbitals to form the two pi bonds (S=O) in each resonance structure. = (6 (\textfrom S) + 24 (\textfrom 4
Comparing the options:
The above resonance model (using two double bonds) is excellent for explaining formal charge and bond equivalence. However, it violates a subtle but important rule: (four from each of two double bonds and two from each of two single bonds = 4+4+2+2 = 12? Wait, recalc carefully). It can “promote” or utilize these d orbitals