Question

according to valence bond
theory, oxygen have no free electrons,still it is paramagnetic.

explain the reason ,with complete explaination with structure.


avoid copy paste..........

50 points question



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Answer 1

Answer:

as u can clearly see in oxygen molecule there are unpaired electrons in π*2px and π*2py orbits therefore Oxygen molecule is paramagnetic

Answer 2

Explanation:

The Lewis structure of O2 gives a misleading impression.

The Lewis structure of O2 gives a misleading impression.i.stack.imgur.com

The Lewis structure of O2 gives a misleading impression.i.stack.imgur.comIt shows that all the electrons in oxygen are paired, so oxygen should be diamagnetic.

The Lewis structure of O2 gives a misleading impression.i.stack.imgur.comIt shows that all the electrons in oxygen are paired, so oxygen should be diamagnetic.Yet oxygen is paramagnetic.

The Lewis structure of O2 gives a misleading impression.i.stack.imgur.comIt shows that all the electrons in oxygen are paired, so oxygen should be diamagnetic.Yet oxygen is paramagnetic.The correct explanation comes from Molecular Orbital theory.

The Lewis structure of O2 gives a misleading impression.i.stack.imgur.comIt shows that all the electrons in oxygen are paired, so oxygen should be diamagnetic.Yet oxygen is paramagnetic.The correct explanation comes from Molecular Orbital theory.The atomic orbitals of the O atoms overlap to form the σ and π orbitals of the O2 molecule as shown in the diagram above.

The Lewis structure of O2 gives a misleading impression.i.stack.imgur.comIt shows that all the electrons in oxygen are paired, so oxygen should be diamagnetic.Yet oxygen is paramagnetic.The correct explanation comes from Molecular Orbital theory.The atomic orbitals of the O atoms overlap to form the σ and π orbitals of the O2 molecule as shown in the diagram above.We add the 12 valence electrons according to the Aufbau principle.

The Lewis structure of O2 gives a misleading impression.i.stack.imgur.comIt shows that all the electrons in oxygen are paired, so oxygen should be diamagnetic.Yet oxygen is paramagnetic.The correct explanation comes from Molecular Orbital theory.The atomic orbitals of the O atoms overlap to form the σ and π orbitals of the O2 molecule as shown in the diagram above.We add the 12 valence electrons according to the Aufbau principle.The last two electrons go into separate, degenerate π orbitals, according to Hund's Rule.

The Lewis structure of O2 gives a misleading impression.i.stack.imgur.comIt shows that all the electrons in oxygen are paired, so oxygen should be diamagnetic.Yet oxygen is paramagnetic.The correct explanation comes from Molecular Orbital theory.The atomic orbitals of the O atoms overlap to form the σ and π orbitals of the O2 molecule as shown in the diagram above.We add the 12 valence electrons according to the Aufbau principle.The last two electrons go into separate, degenerate π orbitals, according to Hund's Rule.Thus, oxygen has two unpaired electrons and is paramagnetic.