Use energy levels of diatomic molecules derived from molecular orbital theory to predict the magnetic properties of the oxygen molecule O₂ and the peroxide anion O₂²^-. A) oxygen (paramagnetic); peroxide (paramagnetic) B) oxygen (paramagnetic); peroxide (diamagnetic) C) oxygen (diamagnetic); peroxide (paramagnetic) D) oxygen (diamagnetic); peroxide (diamagnetic) E) Neither have magnetic properties; only metals have magnetic properties.

Question

Quizplus · Accepted Answer

According to molecular orbital theory, the oxygen molecule has two unpaired electrons in its highest energy level, making it paramagnetic. Similarly, the peroxide anion also has two unpaired electrons in its highest energy level, making it also paramagnetic. Therefore, the correct choice is B, where oxygen is predicted to be paramagnetic and peroxide is predicted to be paramagnetic.

Use Energy Levels of Diatomic Molecules Derived from Molecular Orbital