The paramagnetic property of oxygen as well explained by:A.Molecular orbital theoryB.Resonance theoryC.Valence bond theoryD.VSEPR theory

The paramagnetic property of oxygen is best explained by molecular orbital theory.

In molecular orbital theory, the concept of molecular orbitals is used to describe the distribution of electrons in molecules. Oxygen (O2) has a total of 16 electrons (8 from each oxygen atom) and its electronic configuration is 1s2 2s2 2px2 2py1 2pz1, with two unpaired electrons in its molecular orbitals.

According to Hund's rule, when filling the molecular orbitals, electrons prefer to occupy separate orbitals with parallel spins before pairing up. In the case of oxygen, the two unpaired electrons occupy two degenerate (having the same energy) π* molecular orbitals, resulting in a net spin and making oxygen paramagnetic.

Resonance theory, valence bond theory, and VSEPR theory do not specifically address the paramagnetic property of oxygen. Resonance theory explains the delocalization of electrons in molecules with multiple resonance structures. Valence bond theory describes chemical bonding in terms of overlapping atomic orbitals. VSEPR theory explains the three-dimensional geometry of molecules based on the repulsion between electron pairs around the central atom.

Therefore, the best explanation for the paramagnetic property of oxygen is molecular orbital theory.