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How is bond order calculated and why is Bond order of CO+ 3.5 ?

Answer
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Hint :Bond order is the difference of bonding and anti bonding electrons divided by two. Draw the Molecular Orbital diagram for CO and remove an electron from oxygen to get the molecular orbital diagram for CO+ . Atomic no, of C =6 and O =8 .

Complete Step By Step Answer:
The electronic configuration of C is 1s22s22p2 and that of O+ is 1s22s22p3 .
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.
For the 1s degenerate orbital, 2 electrons will go to σ 1s and 2 electrons will go to σ 1s
For the 2s degenerate orbital, 2 electrons will go to σ 2s and 2 electrons will go to σ 2s
For the 2p degenerate orbital , 2 electrons go to π2px , 2 electrons will go to π2py and 2 electrons will go to σ 2pz .
Formula to calculate bond order is: 12(No. of ein bonding subshell - No. of e-in antibonding subshell)
Acc. To the diagram 10 e s are in bonding subshell and 4 in antibonding subshell.
But this is the Molecular diagram for CO , to get Molecular orbital diagram for CO+ , we will remove an e for the Subshell with higher energy level.
In case of heteronuclear molecules like CO+ the σ 2s is placed higher than π2px , π2py , σ 2pz . So, the e is removed from σ 2s subshell.
Therefore, No. of ein bonding subshell  =10 and No. of e-in antibonding subshell =3
Putting the values in the formula:
 12(103)
 =3.5
Hence the Bond order of CO+ is 3.5.

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 σ 2s is placed higher than π2px , π2py , σ 2pz .