Question

consider the lewis structure for ozone (o₃), which has one single bond and one double bond. what are the possible formal charges on the central oxygen atom? -1 both +1 and -1 are possible depending on the resonance structure. +1 0 which of the following resonance structures for sulfur dioxide (so₂) is likely to be the most stable based on formal charges? (assume s is the central atom) o-s=o (formal charges: o=-1, s=+1, o=0) all resonance structures have equal stability o=s=o (formal charges: o=0, s=0, o=0) o=s-o (formal charges: o=0, s=+1, o=-1) in a molecule with multiple resonance structures, the actual structure of the molecule is best described as

Explanation:

1. For ozone ($O_3$), the central oxygen atom has a formal - charge of +1 in one resonance structure. The formula for formal charge is $FC = V - N - \frac{B}{2}$, where $V$ is the number of valence electrons, $N$ is the number of non - bonding electrons, and $B$ is the number of bonding electrons. In ozone's resonance structures, the central oxygen has different bonding and non - bonding electron arrangements, resulting in a formal charge of +1.
2. For sulfur dioxide ($SO_2$), the most stable resonance structure is the one with formal charges closest to zero. In the structure $O = S = O$ with formal charges $O = 0,S = 0,O = 0$, the formal charges are more favorable compared to other structures with non - zero formal charges. A lower formal charge indicates a more stable structure.

Answer:

1. +1
2. $O = S = O$ (formal charges: $O = 0,S = 0,O = 0$)