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Bond order and magnetic property of CO is:

Answer
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Hint: The molecular orbital theory helps us find out the bond order on the basis of molecular order diagrams. The Atomic no, of C=6 and O=8

Complete answer:
The electronic configuration of C is 1s22s22p2and that of O+is 1s22s22p4.
Steps for drawing the Molecular Orbital Diagram
Since CO is a heteronuclear atom, the atom with more electronegativity will be placed lower in the energy level.
So
For the 1s degenerate orbital, 2 electrons will go to σ1s and 2 electrons will go to σ1s
For the 2s degenerate orbital, 2 electrons will go to σ2s and 2 electrons will go to σ2s
For the 2p degenerate orbital , 2electrons go to π2px ,2electrons will go to π2py and 2 electrons will go to σ2pz.
Formula to calculate bond order is:12(No. of ein bonding subshell - No. of e-in antibonding subshell)
Acc. To the diagram 10 es are in bonding subshell and 4 in antibonding subshell.
Putting the values in the formula:
12(104)
=3
Hence the Bond order of CO is =3
Since all the electrons are paired in the molecular orbital diagram the CO molecule is diamagnetic with the bond order =3

Note:
CO+ does not have a symmetric Molecular diagram because it is a heteronuclear molecule. The more electronegative atom i.e., O is placed lower on the energy level. Due to this discrepancy in energies σ2s is placed higher than π2px, π2py, σ2pz.
If all the electrons of the molecule are paired in the molecular orbital diagram the molecule is said to be diamagnetic.
If there are unpaired electrons present in the molecular orbital diagram the molecule is said to be paramagnetic.