We’re being asked to determine the **Lewis structures and assign a formal charge to each atom of N _{3}^{–}**.

**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 the molecule.

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

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

$\overline{){\mathbf{FC}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{Group}}{\mathbf{}}{\mathbf{\#}}{\mathbf{}}{\mathbf{-}}{\mathbf{}}{\mathbf{(}}{\mathbf{Bonds}}{\mathbf{}}{\mathbf{+}}{\mathbf{}}{\mathbf{nonbonding}}{\mathbf{}}{{\mathbf{e}}}^{{\mathbf{-}}}{\mathbf{)}}}$

Write the correct Lewis structures and assign a formal charge to each atom.

(b) N_{3}^{–}

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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.