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Can Valence Bond Theory explain paramagnetic nature of oxygen molecule?

Can Valence Bond Theory explain paramagnetic nature of oxygen molecule?

Valence Bond Theory cannot explain paramagnetic nature of oxygen molecule.

Can Valence Bond Theory explain paramagnetism?

Paramagnetism is a form of magnetism whereby certain materials are attracted by an externally applied magnetic field. Valence bond theory (VBT) and hybridisation doesn’t really do a good job at predicting whether a molecule is paramagnetic or diamagnetic (isn’t attracted by an external magnetic field).

What does Valence Bond Theory not explain?

Limitaions of Valence Bond Theory. It fails to explain the tetravalency of carbon. This theory does not discuss the electrons’ energies. The assumptions are about the electrons being localized to specific locations.

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Which theory shows that oxygen is paramagnetic?

molecular orbital Theory
According to molecular orbital Theory (MOT), there is 1 unpaired electron in the π2px antibonding orbital and another unpaired electron in π2py antibonding orbital. As molecules containing unpaired electrons are strongly attracted by magnetic field, hence oxygen has paramagnetic nature.

How does bonding theory explain the observation that O2 is paramagnetic?

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 last two electrons go into separate, degenerate π orbitals, according to Hund’s Rule. Thus, oxygen has two unpaired electrons and is paramagnetic.

How does it differ from valence bond theory?

An atom is composed of orbitals where electrons reside. The main difference between valence bond theory and the molecular orbital theory is that valence bond theory explains the hybridization of orbitals whereas the molecular orbital theory does not give details about the hybridization of orbitals.

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Why oxygen is paramagnetic explain?

Based on molecular orbital theory, orbitals are formed by overlapping atomic orbitals of oxygen atoms. Due to the presence of two unpaired electrons, we can say that the oxygen molecule is paramagnetic in nature. The reason why oxygen is paramagnetic is because of the presence of two unpaired electrons.

What is bond order in O2 explain its paramagnetic nature using molecular orbital theory?

Thus, oxygen molecule has two bonds. i.e., one is bond and one p bond. The last two electrons in p2px∙​ and p2py∙​ orbitals will remain unpaired. Therefore, oxygen molecule has paramagnetic character due to the presence of two unpaired electrons.

What are the limitations of the valence bond theory?

Limitations of Valence Bond Theory They are: It fails to explain the tetravalency of carbon. This theory does not discuss the electrons’ energies. The assumptions are about the electrons being localized to specific locations.

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What are the assumptions of the valence bond theory?

Valence bond (VB) theory assumes that all bonds are localized bonds formed between two atoms by the donation of an electron from each atom. This is actually an invalid assumption because many atoms bond using delocalized electrons. In molecular oxygen VB theory predict that there are no unpaired electrons.

Why O2 is paramagnetic on the basis of molecular orbital theory?