What is the molecular geometry of sulfate ion?

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To determine the molecular geometry of sulfate ion $\ce{(SO4^{2-})}$ , first we need to draw its Lewis structure.

Both sulfur and oxygen have $6$ valence electrons, and since the charge of the ion is $-2$ , we will add $2$ more electron when calculating the total number of valence electrons.

\ce{Total number of e- = 6 e- + 4 \times 6 e- + 2 e- = 32 e-}

Sulfur is the least electronegative atom, so we will put it in the center, and place the oxygen atoms around it.

We will put 2 electrons between the atoms, to form bonds, and place the rest of them to complete the octet.

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