We’re being asked to determine the **formal charge of ALL ELEMENTS **in H_{2}CCH_{2 }and ClF_{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) H_{2}CCH_{2}

(b) ClF_{3}

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