Find out sum of bond order of CO & NO⁺.

The correct answer is 6.

To find the sum of the bond orders of CO and NO⁺, we first determine the bond order of each individual species using Molecular Orbital (MO) theory.

1. Bond Order of CO:
Carbon (C) has 6 electrons and Oxygen (O) has 8 electrons.
Total number of electrons in CO = 6 + 8 = 14 electrons.
Since CO has 14 electrons, it is isoelectronic with the nitrogen molecule (N₂).
The molecular orbital configuration for a 14-electron system is:
σ1s² σ*1s² σ2s² σ*2s² (π2p_x² = π2p_y²) σ2p_z²
Here, the number of bonding electrons (N_b) is 10, and the number of anti-bonding electrons (N_a) is 4.
We can calculate the bond order using the following formula:

$$\text{Bond Order of CO}=\frac{N_b-N_a}{2}=\frac{10-4}{2}=3$$

2. Bond Order of NO⁺:
Nitrogen (N) has 7 electrons, Oxygen (O) has 8 electrons, and the positive charge (+) indicates the loss of 1 electron.
Total number of electrons in NO⁺ = 7 + 8 − 1 = 14 electrons.
Since NO⁺ also has 14 electrons, it is isoelectronic with CO and N₂. Thus, it has the exact same molecular orbital configuration and bond order.

$$\text{Bond Order of}{\text{NO}}^{+}=\frac{10-4}{2}=3$$

3. Sum of the Bond Orders:
Now, we sum the bond orders of both species:

$$\text{Sum}=\text{Bond Order of CO}+\text{Bond Order of}{\text{NO}}^{+}$$

$$\text{Sum}=3+3=6$$

Therefore, the sum of the bond orders of CO and NO⁺ is 6.