Which of the following is the paramagnetic oxide of chlorine?

Chlorine forms several oxides, including Cl₂O₇, Cl₂O₆, and ClO₂. Among these, chlorine dioxide (ClO₂) is unique because it is paramagnetic, meaning it has one unpaired electron in its molecular structure. Paramagnetism arises when molecules or ions contain unpaired electrons that interact with an external magnetic field, causing attraction.

ClO₂ has an odd number of valence electrons (19 total), which leaves one unpaired electron on the oxygen-chlorine framework. This unpaired electron makes ClO₂ paramagnetic, which can be detected using magnetic susceptibility measurements. In contrast, Cl₂O₆ (chlorine hexaoxide) and Cl₂O₇ (dichlorine heptaoxide) have all electrons paired in their molecular orbitals, making them diamagnetic.

The paramagnetic property of ClO₂ is also responsible for its reactivity and radical behavior in chemical reactions. Chlorine dioxide is widely used in industry as a bleaching agent and disinfectant, where its high reactivity is partly due to the unpaired electron. Its molecular structure, bond angles, and electron distribution contribute to its unusual magnetic behavior among chlorine oxides.

Understanding which oxides are paramagnetic is important in inorganic chemistry, particularly when studying oxidation states, electronic configurations, and magnetic properties of compounds. It helps predict reactivity and bonding patterns for halogen oxides.

In summary, the paramagnetic oxide of chlorine is ClO₂ due to its unpaired electron, while Cl₂O₆ and Cl₂O₇ are diamagnetic. Recognizing this property helps students and chemists understand chlorine dioxide’s unique electronic and chemical characteristics