Determine the Lewis structure of the nitrogen oxide (NO) and calculate for the** formal charge of N**

**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:

$\overline{){\mathbf{F}}{\mathbf{.}}{\mathbf{C}}{\mathbf{.}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{Group}}{\mathbf{}}{\mathbf{number}}{\mathbf{}}{\mathbf{-}}{\mathbf{}}{\mathbf{(}}{\mathbf{bonds}}{\mathbf{}}{\mathbf{+}}{\mathbf{\hspace{0.17em}}}{\mathbf{nonbonding}}{\mathbf{}}{{\mathbf{e}}}^{{\mathbf{-}}}{\mathbf{)}}}$

What is the formal charge on nitrogen in nitric oxide (NO)?

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