How does MO theory differ from valence bond theory?
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.
Does valence bond theory predict that N2 is diamagnetic?
And, there are no unpaired electrons in the MO descriptions of N2 and F2, and this sufficiently accounts for their observed diamagnetism. The valence bond theory is unable give any satisfactory reason for the paramagnetism of simple molecules having even number of electrons such as B2, O2 and S2.
Why MO diagram is different from N2 and O2?
The 2pz orbitals of N2 and O2 also differ because of the energy difference between the p orbitals of each atomic orbital. In order to offset the s and p mixing present in the 2s orbital, N2 will have a higher energy bonding sigma bond in the 2p orbital that is greater in energy than the bonding pi bonds.
What is the similarities between valence bond theory and molecular orbital theory?
Both valence bond theory and molecular orbital theory are based on quantum mechanical principles and make use of atomic orbital wave functions to carry the interactions between atomic orbitals. Both postulate the formation of bonds on account of interacting overlaps of concerned atomic orbitals.
What is an advantage of MO theory over valence bond theory?
Molecular Orbital Theory has several advantages and differences over VESPR & VB theory: • MO does a good job of predicting electronic spectra and paramagnetism, when VSEPR and the VB theories don’t.
How can you explain the stability of N2 molecule using MO theory?
Answer. As bond order of nitrogen is more than that of oxygen, nitrogen is more stable than oxygen.
What is the bond order in the nitrogen molecule as predicted by MO theory?
What is the bond order for N2+? The MO method for N2+ gives the bond order equal to 2.5.
How does N2 and O2 have different linear combinations of their 2s and 2pz orbitals?
N2 and O2 have different linear combinations of their 2s and 2pz orbitals because of the difference in energy between their respective 2s and 2pz orbitals. N2’s difference is less than 13 eV while O2’s difference is greater than 13 eV, resulting in different linear combinations.
Why N2 is more stable than O2 explain the basis of MOT?
As bond order of nitrogen is more than that of oxygen, nitrogen is more stable than oxygen.