Final answer:
To draw the dot structure for Ozone (O3), arrange two oxygen atoms around a central oxygen and form single bonds. Complete their octets and consider the resonance hybrid with partial double bonds, assigning formal charges to the oxygen atoms where the central oxygen has +1, one of the outer oxygens has -1, and the other has 0.
Step-by-step explanation:
The student has asked to draw the dot structure for Ozone (O3) and assign formal charges. Ozone has a resonance structure, which means that it has more than one valid Lewis structure. To draw a Lewis structure for ozone:
- Place one oxygen atom as the central atom and connect the other two oxygen atoms to it with single bonds.
- Complete the octets of the outer oxygen atoms by adding six electrons each.
- The central oxygen atom will have four electrons after forming single bonds with the outer oxygens, therefore add two additional electrons to the central atom to complete its octet.
- Now you have a structure with one double bond and one single bond which is not the only resonance structure. So it's important to consider the resonance hybrid of O3, which implies partial double bonds between the central oxygen and the outer oxygens.
- Assign formal charges accordingly: The central oxygen atom will have a formal charge of +1, and the oxygen atom with a single bond will have a formal charge of -1, while the oxygen with a double bond to the central oxygen will have a formal charge of 0.
- The formal charges must add up to the overall charge of the molecule, which is zero for ozone.
Remember that the most stable structure for a molecule is the one with the least formal charges and where negative formal charges reside on the more electronegative atoms. In the case of ozone, the resonance structures equally contribute to the true structure of the molecule, which is a blend of all resonance structures.