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Question

Consider the following species:
CN+, CN, NO and CN
Which one of these will have the highest bond order?

A
CN+
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B
CN
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C
NO
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D
CN
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Solution

The correct option is B CN
According to molecular orbital theory (MOT), bond order is given as

bond order = (no. of bonding electrons - no. of antibonding electrons )/2

CN+ : (σ1s)2, (σ1s)2, (σ2s)2, (σ2s)2, (π2px)2, (π2py)2

bond order = (8-4)/2 = 2

CN : (σ1s)2, (σ1s)2, (σ2s)2, (σ2s)2, (π2px)2, (π2py)2, (π2pz)1

bond order = (9-4)/2 = 2.5

CN : (σ1s)2, (σ1s)2, (σ2s)2, (σ2s)2, (π2px)2, (π2py)2, (π2pz)2

bond order = (10-4)/2 = 3

NO : (σ1s)2, (σ1s)2, (σ2s)2, (σ2s)2, (π2pz)2, (π2px)2 = (π2py)2, (π2px)1 = (π2py)0

bond order = (10-5)/2 = 2.5

so, CN has the highest bond order

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