We’re being asked to draw the Lewis Structure for SO_{2} and show its formal charges

**To do so, we need to do the following steps:**

* Step 1:* Determine the central atom in this molecule.

**Step 2:**** **Calculate the total number of valence electrons present.

**Step 3: **Draw the Lewis structure for SO

**Step 4:**** **Calculate the formal charge for **SO _{2} **

Recall that the formula for the ** formal charge** is:

$\overline{){\mathbf{F}}{\mathbf{.}}{\mathbf{C}}{\mathbf{.}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{Group}}{\mathbf{}}{\mathbf{Number}}{\mathbf{}}{\mathbf{-}}{\mathbf{}}{\mathbf{(}}{\mathbf{Bonds}}{\mathbf{}}{\mathbf{+}}{\mathbf{}}{\mathbf{Nonbonding}}{\mathbf{}}{{\mathbf{e}}}^{{\mathbf{-}}}{\mathbf{)}}}$

Draw a Lewis structure for SO_{2} in which all atoms obey the octet rule. Show formal charges. Do not consider ringed structures.

Draw a Lewis structure for SO_{2} in which all atoms have a formal charge of zero. Explicitly showing the zero charges is optional. Do not consider ringed structures.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Formal Charge concept. You can view video lessons to learn Formal Charge. Or if you need more Formal Charge practice, you can also practice Formal Charge practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Hascall's class at NAU.