We’re being asked to determine the **formal charge of ALL ELEMENTS **in SeF_{6 }and PO_{4}^{3−}.

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

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

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

*Step 3:* Draw the Lewis structure for the molecule.

*Step 4:* Calculate the formal charge for the indicated atom.

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

$\overline{){\mathbf{F}}{\mathbf{.}}{\mathbf{C}}{\mathbf{.}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{Group}}{\mathbf{\#}}{\mathbf{}}{\mathbf{-}}{\mathbf{}}{\mathbf{(}}{\mathbf{bonds}}{\mathbf{}}{\mathbf{of}}{\mathbf{}}{\mathbf{element}}{\mathbf{}}{\mathbf{+}}{\mathbf{nonbonding}}{\mathbf{}}{\mathbf{electrons}}{\mathbf{)}}}$

Calculate the formal charge of each element in the following compounds and ions:

(a) SeF_{6}

(b) PO_{4}^{3−}

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 Lewis Dot Structure: Formal Charge concept. If you need more Lewis Dot Structure: Formal Charge practice, you can also practice Lewis Dot Structure: Formal Charge practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Sotelo Munoz's class at TEXAS.