We’re being asked to determine the **formal charge of chlorine** in **ClO ^{–}**.

**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:

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

The substance chlorine monoxide, ClO (g), is important in atmospheric processes that lead to depletion of the ozone layer. The ClO molecule has has an experimental dipole moment of 1.24 D and the Cl - O bond length is 1.60 Å.

The anion ClO^{-} exists. What is the formal charge on the Cl for the best Lewis structure for ClO^{-}?

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