Question

Draw the resonance hybrid of $S{{O}_{3}}$

Answer 1

Hint: The concept of resonance was formerly introduced in order to deal with the kind of difficulty experienced in the depiction of accurate structures of molecules.
The phenomena of resonance is represented by a double headed arrow. Each structure of resonance has an equal contribution to the resonance hybrid structure and no individual structure is totally responsible for the final structure.

Complete step by step answer:
According to the concept of resonance, whenever a single Lewis structure cannot describe a molecule accurately, a number of structures with similar energy, positions of nuclei, bonding as well as non-bonding pairs of the involved electrons are taken as the resonating structures of the hybrid which describes the molecule accurately.
In the given structures, we can see that the double bond characteristics of the sulphur and oxygen is not present at any one oxygen, it keeps on delocalisation, or in other words, the pi electron cloud present in the double bond, keeps on delocalisation and shifting between the three oxygen atoms which are attached to the sulphur.

We can see that the Lewis structure, in each of them the sulphur has a formal charge of $+2$ and two of the oxygen atoms have $-1$ charge.
Now, in each of the three structures which are present in the middle, we can see that the $S$ has a formal charge of $+1$ and one of $O$ atoms has a formal charge of $-1$.
Now if we consider each of the structures present at the bottom, the formal charge is zero.

Note: The phenomena of resonance results in stabilisation of a molecule, as the electron clouds are more delocalised throughout the whole molecule, and no electron cloud is localised in just one atom.
Due to which the energy of the resonance hybrid is much less as compared to the energy of any single resonating structure.