Ozone (O3) is polar because of its bent molecular geometry and the presence of a lone pair of electrons on the central oxygen atom.
Bent Molecular Geometry and Polarity
The video reference states that ozone has a bent molecular geometry. This shape is critical to its polarity. If ozone were linear, the bond dipoles (resulting from the difference in electronegativity between oxygen atoms) would cancel each other out, making the molecule nonpolar. However, the bent shape prevents this cancellation.
Lone Pair of Electrons
The central oxygen atom in ozone also has a lone pair of electrons. This lone pair contributes to the uneven distribution of electron density within the molecule. The lone pair repels the bonding pairs of electrons, further distorting the geometry and enhancing the polarity.
Uneven Electron Distribution
Due to the bent shape and the influence of the lone pair, the electron density is not evenly distributed across the ozone molecule. This uneven distribution creates a net dipole moment, making ozone a polar molecule. The central oxygen atom has a partial positive charge, while the two terminal oxygen atoms have partial negative charges.
