Draw the Lewis structure for the ozone (O3) molecule Be sure to include all resonance structures that satisfy the octet rule
The Correct Answer and Explanation is:
To draw the Lewis structure for the ozone (O₃) molecule, we begin by calculating the total number of valence electrons. Each oxygen atom is in Group 16 of the periodic table, so it has 6 valence electrons. For three oxygen atoms, the total is 3 atoms × 6 electrons/atom = 18 valence electrons.
Next, we create a skeletal structure by placing one oxygen atom in the center and connecting it to the other two with single bonds (O-O-O). This uses 4 electrons, leaving 14 to be distributed. We then add lone pairs to the terminal (outer) atoms to satisfy their octets first. Each terminal oxygen receives 6 electrons (3 lone pairs), using up 12 electrons. The remaining 2 electrons are placed on the central oxygen atom as a single lone pair.
At this stage, the central oxygen atom has only 6 electrons in its valence shell (one lone pair and two single bonds), which does not satisfy the octet rule. To complete the octet for the central atom, we must form a double bond. A lone pair from one of the terminal oxygen atoms is moved to create a double bond with the central oxygen. This results in a structure where all atoms have a complete octet.
Because the double bond can be formed with either of the two terminal oxygen atoms, two equivalent resonance structures exist. In each structure, the central oxygen has a formal charge of +1, while the singly bonded terminal oxygen has a formal charge of -1. The doubly bonded oxygen is neutral. These two structures are connected by a double-headed arrow to show that the true structure of ozone is a resonance hybrid of both forms, with the electrons delocalized across the molecule.
Here is the final drawing:thumb_upthumb_down
