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The formula for formal charge is fc = v ( lp +. 5 * be) where fc (formal charge) is equal to v (# of valence electrons ) minus (lone electrons + half the bonding electrons). So, for our molecule, we see: The overall formal charge on so 2 lewis structure is zero so it is a stable molecule.
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Here, the given molecule is so2 (sulfur dioxide). In order to draw the lewis structure of so2, first of all you have to find the total number of valence electrons present in the so2 molecule. (valence electrons are the number of electrons present in the outermost shell of an atom). So, lets calculate this first.
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Calculation of valence electrons in. Draw the lewis structure of so 2 (with minimized formal charges) and then determine the ideal bonding angle (s) of the central atom. To determine the ideal bonding angle in the sulfur dioxide (so2) molecule, let's go through the steps to draw the lewis structure and then figure out the bond angle. Sulfur (s) has 6 valence electrons. To assign formal charges to the atoms in the so 2 molecule, use the formula:
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