Why is SO3 a Lewis acid?

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Answer 1 · 2018-05-14T07:49:49

Well a $Lewis-acid$ $"Lewis-acid"$ is an electron-pair acceptor....

And certainly the electron-deficient sulfur atom in $S O_{3}$ $SO_3$ is such an electron pair acceptor...i.e...

$S O_{3} (g) + H_{2} O (l) \to H_{2} S O_{4} (a q)$ $SO_3(g) + H_2O(l) rarr H_2SO_4(aq)$

$S O_{3} + C_{6} H_{5} N \to {C_{6} H_{5} N \cdot S O_{3}}$ $SO_3 +C_6H_5Nrarr{C_6H_5N*SO_3}$ ...

We would give the following Lewis structure for $S O_{3}$ $SO_3$ as...

$O = 2 + S {(- O^{-})}_{2}^{-}$ $O=stackrel(2+)S(-O^(-))_2$

...which illustrates the electron paucity of the sulfur centre.

What is the expected geometry for this molecule?