JEE Main 2026 · 2 Apr · Shift 1 · Chemistry Q53

← JEE Main 2026 · 2 Apr · Shift 1

ChemistrySingle correct+4 / -1Question 53 of 75

Given below are two statements :

Statement (I) : The correct sequence of bond lengths in the following species is :
$\ce{O2+} < \ce{O2} < \ce{O2-} < \ce{O2^{2-}}$

Statement (II) : The correct sequence of number of unpaired electrons in the following species is :
$\ce{O2} > \ce{O2+} > \ce{O2-} > \ce{O2^{2-}}$

In the light of the above statements, choose the correct answer from the options given below :

Both Statement I and Statement II are true

Both Statement I and Statement II are false

Statement I is true but Statement II is false

Statement I is false but Statement II is true

Answer and worked solution

Official answer: C

Bond orders. $\ce{O2+}$ 2.5, $\ce{O2}$ 2, $\ce{O2-}$ 1.5, $\ce{O2^{2-}}$ 1. Bond length rises as bond order falls, so $\ce{O2+}<\ce{O2}<\ce{O2-}<\ce{O2^{2-}}$ : Statement I is true.

Unpaired electrons ( $\pi^*$ electrons): $\ce{O2}$ 2, $\ce{O2+}$ 1, $\ce{O2-}$ 1, $\ce{O2^{2-}}$ 0. $\ce{O2+}$ and $\ce{O2-}$ are equal, so the strict order in Statement II is false.

(C)

Topics:Molecular orbital theory

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JEE Main 2026 · 2 Apr · Shift 1, Chemistry question 53