Draw the Lewis Structure of O3 Including Any Resonance Forms

To draw the Lewis structure of O₃ (ozone), follow these steps:

1. Count the total number of valence electrons: Oxygen is in group 16 of the periodic table, so each oxygen atom has 6 valence electrons. For O₃, the total number of valence electrons is 6 × 3 = 18.
2. Determine the central atom: In O₃, the central atom is one of the oxygen atoms, and the other two oxygen atoms are connected to it.
3. Draw the skeletal structure: Place the central oxygen atom in the middle and connect it to the other two oxygen atoms with single bonds. This uses 4 electrons (2 for each bond).
4. Distribute the remaining electrons: You have 14 electrons left. Place 6 electrons around each of the outer oxygen atoms to complete their octets. This uses 12 electrons. You now have 2 electrons left, which you place on the central oxygen atom.
5. Check for octets: The central oxygen atom has only 6 electrons (2 from the bonds and 4 lone pairs). To complete its octet, you need to form a double bond with one of the outer oxygen atoms. This can be done by moving a lone pair from one of the outer oxygen atoms to form a double bond with the central oxygen atom.
6. Draw resonance structures: O₃ has two resonance structures because the double bond can be formed with either of the two outer oxygen atoms. The actual structure of O₃ is a hybrid of these two resonance forms.

Here is the final Lewis structure of O₃ including resonance forms:

  O
  ||
O--O

In this structure, the double bond can be on either side, representing the resonance forms.