NEET2026ChemistryChapterActual
Four diatomic species are given below. Which of the following represents the correct sequence of their increasing bond length?
Options
- ANO ⁺ < NO < O ₂ < O ₂⁻
- BO ₂⁻ < O ₂ < NO < NO ⁺
- CNO < NO ⁺ < O ₂⁻ < O ₂
- DO ₂ < O ₂⁻ < NO ⁺ < NO
Correct answer
A. NO ⁺ < NO < O ₂ < O ₂⁻
Step-by-step solution
The bond order of a diatomic species can be determined from its total number of electrons. For NO ⁺ , the total number of electrons is 7 + 8 - 1 = 14 . Its bond order is 3 . For NO , the total number of electrons is 7 + 8 = 15 . Its bond order is 2.5 . For O ₂ , the total number of electrons is 8 + 8 = 16 . Its bond order is 2 . For O ₂⁻ , the total number of electrons is 8 + 8 + 1 = 17 . Its bond order is 1.5 . Bond length is inversely proportional to bond order. Since the bond order decreases in the sequence NO ⁺