By drawing one of the resonance structures of SO3 , the the formal charge of S is?

To draw one of the resonance structures of SO3, we can show a double bond between sulfur (S) and one of the oxygen atoms (O), while the other two oxygen atoms have single bonds with sulfur. This results in a formal charge of +1 on sulfur.

The Lewis structure of SO3 with a double bond between sulfur and one oxygen atom is as follows:

O=S=O
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O

In this structure, sulfur has 6 valence electrons (group 6A element) and is bonded to 3 oxygen atoms, giving it a total of 6 electrons in its valence shell. Since sulfur has 6 valence electrons in this structure, it has a formal charge of +1.

In one of the resonance structures of SO3, sulfur has a formal charge of +2.

This can be seen by drawing the Lewis structure of SO3 and then assigning formal charges to each atom. The formal charge of an atom is calculated by subtracting the number of electrons it has in its valence shell from the number of bonds it has to other atoms.

In the case of sulfur in SO3, it has six valence electrons and it forms four bonds to the three oxygen atoms. This means that it has a formal charge of +2.

The other two resonance structures of SO3 have sulfur with a formal charge of 0 and -2.