KCET2015ChemistryChemical Bonding and Molecular Structure
Using MOT, compare ( O ₂⁺ )and ( O ₂⁻ )species and choose the incorrect option.
Options
- A( O ₂⁺ )have higher bond order than ( O ₂ )
- B( O ₂⁻ ).is less stable.
- C( O ₂ ⁺ )is diamagnetic while ( O ₂ ⁻ )is paramagnetic.
- DBoth ( O ₂⁺ )and ( O ₂⁻ )is paramagnetic.
Correct answer
C. ( O ₂ ⁺ )is diamagnetic while ( O ₂ ⁻ )is paramagnetic.
Step-by-step solution
Molecular orbital configurations: ( O₂⁺ (15 e⁻ s ): ) ( 1 s² ^ * 1 s² 2 s² * 2 s² 2 p_ z ² 2 p_ x ²= 2 p_ y ² ^ * 2 p_ x ¹ ) Bond order ( = 1 2 (10-5)=2.5 ), and paramagnetic due to one unpaired electron. ( O ₂⁻ (17 e⁻ s ): ) ( 1 s² ^ * 1 s² 2 s² * 2 s² 2 p_ z ² 2 p_ x ²= 2 p_ y ² ^ * 2 p_ x ²= ^ * 2 p_ y ¹ ) Bond order ( = 1 2 (10-7)=1.5 ) and paramagnetic due to one unpaired electron. Therefore, both ( O ₂⁺ )and ( O ₂⁻ )are paramagnetic and ( O ₂⁺ )have higher bond order than ( O ₂⁻ )Also, ( O ₂⁻ )is less stable.