(b) It turns out that ozone, O₃, has a small dipole moment. How is this possible, given that all the atoms are the same?

Verified step by step guidance

1. Understand that a dipole moment arises from differences in electronegativity between atoms, leading to an uneven distribution of electron density.
2. Recognize that ozone (O_3) is a molecule with a bent shape, similar to water (H_2O), due to the presence of lone pairs on the central oxygen atom.
3. Consider the molecular geometry: Ozone has a V-shaped or bent structure, which means the molecule is not linear.
4. Realize that even though the atoms are the same (oxygen), the bent shape causes an asymmetrical distribution of charge, leading to a net dipole moment.
5. Conclude that the dipole moment in ozone is due to its molecular geometry, which causes an uneven distribution of electron density despite having identical atoms.

Key Concepts

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. In the case of ozone (O3), the molecule has a bent shape due to the presence of lone pairs on the central oxygen atom. This geometry is crucial because it influences the distribution of electron density, leading to a dipole moment despite the identical atoms.

Dipole Moment

A dipole moment is a measure of the separation of positive and negative charges in a molecule, resulting from differences in electronegativity and molecular geometry. In ozone, the bent structure causes an uneven distribution of electron density, creating a dipole moment. This means that one side of the molecule is slightly more negative, while the other is slightly more positive.

Electronegativity

Electronegativity is the tendency of an atom to attract electrons in a chemical bond. Although all atoms in ozone are oxygen, the arrangement and lone pairs affect how the electrons are shared. In ozone, the effective electronegativity is influenced by the molecular shape, leading to a dipole moment even among identical atoms.