According to MO theory the bond orders for \(O_2^{2−},CO\,\, \text {and} \,\,NO^+\) respectively, are
- 1, 2 and 3
- 1,3 and 2
- 2,3 and 3
- 1, 3 and 3
The Correct Option is D
Solution and Explanation
\[ \text{BO} = \frac{\text{(Number of bonding electrons - Number of antibonding electrons)}}{2} \] - For \(\text{O}_2^-\): Adding one electron to \(\text{O}_2\) decreases the bond order from 2 to 1.
- For CO: The bond order remains 3 because of strong triple bonding.
- For NO$^+$: Removal of one electron from NO increases the bond order from 2.5 to 3.
Thus, the bond orders are 1, 3, and 3, respectively.
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Concepts Used:
Molecular Orbital Theory
The Molecular Orbital Theory is a more sophisticated model of chemical bonding where new molecular orbitals are generated using a mathematical process called Linear Combination of Atomic Orbitals (LCAO).
Molecular Orbital theory is a chemical bonding theory that states that individual atoms combine together to form molecular orbitals. Due to this arrangement in MOT Theory, electrons associated with different nuclei can be found in different atomic orbitals. In molecular orbital theory, the electrons present in a molecule are not assigned to individual chemical bonds between the atoms. Rather, they are treated as moving under the influence of the atomic nuclei in the entire molecule.
