Try and two S–O⁻ bonds (resonance hybrid actually has all S–O bonds equivalent).
S /|\ / | \ O O O O
: Sulfur has 6 valence electrons, and each oxygen has 6 valence electrons. The total number of valence electrons in SO4 2- is: $$6 (S) + 4 \times 6 (O) + 2 (charge) = 6 + 24 + 2 = 32$$ so4 2 lewis structure
: The sulfur atom is the central atom, and the four oxygen atoms are bonded to it. Try and two S–O⁻ bonds (resonance hybrid actually
Sulfur can form double bonds by moving lone pairs from oxygen to form S=O. so4 2 lewis structure
With formal charges: two oxygens have –1, sulfur 0, two oxygens 0. The ion is enclosed in brackets with a superscript ( 2^- ).