Draw all resonance structures for the ozone molecule, 03.
Explicitly draw all H atoms.
Include all valence lone pairs in your answer.
Do not include overall ion charges or formal charges in your drawing.
Do not draw double bonds to oxygen unless they are needed for the central atom to obey the octet rule. Draw one structure per sketcher. Add additional sketchers by selecting in the drop-down menu
The correct answer and explanation is :
Here’s the resonance structures for the ozone molecule (O₃), including explicit hydrogen atoms and lone pairs:
Resonance Structures:
Ozone (O₃) is a molecule composed of three oxygen atoms. It exhibits resonance, meaning that the bonding within the molecule can be represented by multiple structures, with each oxygen atom involved in double bonds, single bonds, and lone pairs of electrons. These structures indicate that the true bonding in the molecule is a hybrid of all these forms. Here’s how it works:
- Structure 1:
- The molecule has a single bond between the central oxygen atom and one of the terminal oxygen atoms.
- The other terminal oxygen atom has a double bond with the central oxygen atom.
- The central oxygen has a lone pair of electrons.
- Each oxygen atom has lone pairs where they aren’t involved in bonding.
- Structure 2:
- The bonds switch positions with the terminal oxygens.
- The central oxygen atom now has a double bond to the other oxygen atom, while the first terminal oxygen has a single bond to the central oxygen.
Explanation:
In ozone, each oxygen atom must obey the octet rule. The central oxygen atom is connected to the other two oxygen atoms, and the molecule experiences resonance between two possible structures. Since oxygen prefers to have a full octet of electrons, the molecule switches between these structures to minimize electron repulsion and maintain stability.
Each structure has some key features:
- The central oxygen atom has a lone pair of electrons.
- Oxygen atoms are connected through single or double bonds.
- Lone pairs are placed on each oxygen atom to fulfill the octet rule for all.
The hybrid of these structures is what makes the true bonding in O₃, resulting in a bond order that is intermediate between a single bond and a double bond for the bonds between the central oxygen and terminal oxygens.