draw the lewis structure for the sulfur dioxide (so₂) molecule. be sure to include all resonance structures…

Explanation:

Step1: Determine valence electrons

Sulfur (S) has 6 valence electrons and each oxygen (O) has 6 valence electrons. So for $SO_2$, the total number of valence electrons is $6 + 2\times6=18$.

Step2: Place central atom

Sulfur is the central atom. Connect sulfur to each oxygen with a single - bond, using 4 electrons. So, $18 - 4 = 14$ electrons left.

Step3: Distribute remaining electrons

Place 6 electrons as 3 lone - pairs on each oxygen atom. Now, all 18 electrons are used, but sulfur has only 4 electrons around it.

Step4: Form double - bond for octet

Move one lone - pair from one of the oxygen atoms to form a double - bond with sulfur to satisfy the octet rule for sulfur. There are two possible resonance structures: one with a double - bond between sulfur and one oxygen and a single - bond between sulfur and the other oxygen, and the other with the double - bond and single - bond reversed.

Answer:

The two resonance structures of $SO_2$: In one structure, sulfur is double - bonded to one oxygen and single - bonded to the other oxygen. The double - bonded oxygen has 2 lone - pairs and the single - bonded oxygen has 3 lone - pairs. In the second resonance structure, the double - bond and single - bond are reversed between the two oxygen atoms with respect to the first structure.