Question

Draw a Lewis structure for SO 2 in which all atoms have a formal charge of zero. Do not consider ringed structures.

Answer 1

Answer : The Lewis-dot structure of
`SO_2` is shown below.

Explanation :

Lewis-dot structure : It shows the bonding between the atoms of a molecule and it also shows the unpaired electrons present in the molecule.

In the Lewis-dot structure the valance electrons are shown by 'dot'.

The given molecule is,
`SO_2`

As we know that sulfur and oxygen has '6' valence electrons.

Therefore, the total number of valence electrons in
`SO_2` = 6 + 2(6) = 18

According to Lewis-dot structure, there are 8 number of bonding electrons and 10 number of non-bonding electrons.

Now we have to determine the formal charge for each atom.

Formula for formal charge :

`\text{Formal charge}=\text{Valence electrons}-\text{Non-bonding electrons}-\frac{\text{Bonding electrons}}{2}`

`\text{Formal charge on S}=6-2-(8)/(2)=0`

`\text{Formal charge on }O_1=6-4-(4)/(2)=0`

`\text{Formal charge on }O_2=6-4-(4)/(2)=0`