Question

Explain the paramagnetic nature of oxygen molecule using molecular orbital theory.

Answer 1

Explanation:

see the attachment and

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Answer 2

Answer:

The oxygen molecule is paramagnetic in nature because of the presence of unpaired electrons.

Explanation:

• The electronic configuration of oxygen atom: [He]2s²2p⁴. One oxygen atom has 8 valence electrons. Then in O₂ molecule has 16 electrons to fill molecular orbitals formed by the overlapping of atomic orbitals.  

• The electronic configuration of oxygen molecule on the basis of molecular orbital theory is:

       $\sigma1s^2 \;\sigma^*1s^2\; \sigma2s^2\; \sigma^*2s^2\; \sigma2p^2_{z}\; \; \pi 2p^2_{x}\; \pi 2p^2_{y}\; \; \pi^* 2p^1_{x}\; \; \pi ^*2p^1_{y}$

• The bond order O₂ molecule $=\frac{1}{2}[N_{A.B.}-N_{B}]$

                                                         $=\frac{1}{2}[10-6]$

                                                         $=2$

• Paramagnetic nature of any substance due to presence of unpaired electrons in that substance.

• The two unpaired electrons present in the antibonding molecular orbitals of oxygen molecules are the reason of paramagnetic nature of oxygen molecule.