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NEET CHEMISTRYMedium

Which one of the following pairs of species have the same bond order?

A

CO\text{CO}, NO\text{NO}

B

O2−\text{O}_2^-, CN−\text{CN}^-

C

CN−\text{CN}^-, NO+\text{NO}^+

D

N+\text{N}^+, CN+\text{CN}^+

Step-by-Step Solution

Species with the same number of electrons (isoelectronic species) generally have the same bond order according to Molecular Orbital Theory.

  • CN−\text{CN}^-: The total number of electrons is 6 (C)+7 (N)+1 (negative charge)=146 \text{ (C)} + 7 \text{ (N)} + 1 \text{ (negative charge)} = 14 electrons. Its bond order is 3.
  • NO+\text{NO}^+: The total number of electrons is 7 (N)+8 (O)−1 (positive charge)=147 \text{ (N)} + 8 \text{ (O)} - 1 \text{ (positive charge)} = 14 electrons. Its bond order is also 3.

Let's check the other pairs:

  • CO\text{CO} has 14 electrons (bond order 3) while NO\text{NO} has 15 electrons (bond order 2.5).
  • O2−\text{O}_2^- has 17 electrons (bond order 1.5) while CN−\text{CN}^- has 14 electrons (bond order 3). Therefore, CN−\text{CN}^- and NO+\text{NO}^+ are the pair with the same bond order.
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