What are the formal charges of each oxygen atom, from left to right? The image shows a Lewis structure for ozone (O3) with a double bond between the first and second oxygen and a single bond between the second and third oxygen.

Answer

To find the formal charge of an atom, use the formula: Formal Charge = (Valence Electrons) - (Non-bonding Electrons) - (Bonding Electrons / 2). Oxygen has 6 valence electrons. 1) For the leftmost oxygen: Formal Charge = 6 (valence) - 4 (lone pair electrons) - (4 bonding electrons / 2) = 6 - 4 - 2 = 0. 2) For the middle oxygen: Formal Charge = 6 (valence) - 2 (lone pair electrons) - (6 bonding electrons / 2) = 6 - 2 - 3 = +1. 3) For the rightmost oxygen: Formal Charge = 6 (valence) - 6 (lone pair electrons) - (2 bonding electrons / 2) = 6 - 6 - 1 = -1. Reading from left to right, the formal charges are 0, +1, -1.