The Lewis structure for ozone (O3) is a representation that helps us understand the bonding and structure of the molecule. To draw the Lewis structure, start with the total number of valence electrons: oxygen has 6 valence electrons, and because there are three oxygen atoms in ozone, the total is 18 valence electrons.
1. **Lewis Structure**: The central atom in O3 can be one of the oxygen atoms, surrounded by the other two. A double bond forms between one of the outer oxygens and the central oxygen, while a single bond is formed with the other outer oxygen. To complete the octets, you will find resonance structures where the double bond can switch between the two outer oxygen atoms. Hence, the structure can be represented as:
O / \ O O
Here, one outer oxygen is bonded through a double bond, and the other through a single bond.
a. Molecular Geometry
The molecular geometry of O3 is bent. The VSEPR theory (Valence Shell Electron Pair Repulsion) indicates that the two bonded pairs and one lone pair on the central oxygen will repel each other, causing the molecule to adopt a bent shape.
b. Electron Geometry
The electron geometry around the central oxygen atom is trigonal planar, as there are three areas of electron density (two bonding pairs and one lone pair). This geometry takes into account all electron pairs around the central atom.
c. Hybridization of the Central Atom
The hybridization of the central oxygen atom in ozone is sp2. The presence of the double bond and the lone pair requires the mixing of one s orbital and two p orbitals to form three sp2 hybrid orbitals.
d. Polarity
Ozone (O3) is a polar molecule. Although the molecule has a symmetrical bent shape, the electronegativity difference between the oxygen atoms and the lone pair on the central atom creates a dipole moment, leading to an overall polar character.