Central oxygen atom has 3 regions of e-¹ density hence it is sp² hybridized.Any way u can go for u-tube videos u'll understand better.

< b="" />Hybridization of O3: Explained< />

Ozone (O3) is a chemical compound composed of three oxygen atoms. The hybridization of O3 can be explained using valence bond theory, which states that atoms in a molecule form covalent bonds by overlapping their atomic orbitals. In the case of ozone, the central oxygen atom undergoes hybridization to form three sp2 hybrid orbitals.

< b="" />Hybridization Process: < />

1. Valence Electrons: The oxygen atom in its ground state has two electrons in the 2s orbital and four electrons in the 2p orbitals (2px, 2py, 2pz), giving a total of six valence electrons.

2. Excitation: One electron from the 2s orbital is promoted to the empty 2pz orbital, resulting in the excitation of the oxygen atom. This process leads to the formation of three half-filled orbitals with one electron each in the 2px, 2py, and 2pz orbitals.

3. Hybridization: The three half-filled orbitals (2px, 2py, 2pz) and the singly occupied 2s orbital undergo hybridization to form three sp2 hybrid orbitals. This hybridization involves the mixing of one 2s orbital and two 2p orbitals, resulting in three equivalent sp2 hybrid orbitals.

4. Molecular Geometry: The three sp2 hybrid orbitals arrange themselves in a trigonal planar geometry around the central oxygen atom. The remaining two 2p orbitals perpendicular to the plane of the molecule contain the lone pairs of electrons.

< b="" />Bonding in Ozone: < />

The three oxygen atoms in ozone form covalent bonds by overlapping their hybrid orbitals. Each oxygen atom contributes one electron to form three sigma (σ) bonds and one pi (π) bond. The sigma bonds are formed by the overlap of sp2 hybrid orbitals, while the pi bond results from the overlap of two unhybridized 2p orbitals.

< b="" />Conclusion: < />

In conclusion, the hybridization of O3 involves the excitation of the central oxygen atom, resulting in the formation of three sp2 hybrid orbitals. These orbitals arrange themselves in a trigonal planar geometry, leading to the formation of covalent bonds in ozone. Understanding the hybridization of ozone is important for comprehending its molecular structure and properties.