The ozone (O₃) molecule contains which type of chemical bonding?

Ozone (O₃) is a triatomic molecule composed of three oxygen atoms. Its chemical bonding is unique, as it involves both covalent and dative (coordinate) bonds, which explains its structure and reactivity.

In ozone, one oxygen atom forms a double bond with one oxygen and a coordinate (dative) bond with the other oxygen, where a lone pair of electrons from one atom is shared with another. The covalent bonds are formed when two atoms share electrons equally, whereas the dative bond occurs when both shared electrons come from the same atom. This combination gives ozone a resonance structure, meaning the electrons are delocalized across the molecule, and neither bond is a simple single or double bond.

The ozone molecule has a bent shape with a bond angle of approximately 117°, which is slightly less than the ideal 120° of a perfect trigonal planar geometry due to lone pair repulsion. The delocalized bonding also contributes to the molecule’s stability and unique chemical properties, such as its strong oxidizing ability, which makes ozone useful in air purification, water treatment, and chemical reactions.

Other types of bonds are not present in ozone. There is no ionic bonding, as all atoms share electrons rather than transfer them. While covalent bonds exist, the presence of a coordinate bond is essential for explaining the molecular structure and resonance of ozone.

Understanding the bonding in ozone is a fundamental part of chemistry, particularly in the study of molecular structure and bonding theories. It helps students grasp how molecules with resonance and dative bonding behave differently from simple covalent compounds. In summary, the ozone molecule contains both covalent and dative bonds, making it a classic example of resonance and coordinate bonding in chemistry.