Which one of the following is diamagnetic ? (a) O2 (b) O2^2- (c) O2^- (d) None of these

We must identify which oxygen species has no unpaired electrons (diamagnetic). > [!TLDR] > The peroxide ion, O2^2-, is diamagnetic because all its electrons are paired; molecular O2 and the superoxide ion O2^- are paramagnetic. Using molecular orbital theory for these O2 species: - O2 (16 electrons) has two electrons singly occupying the two degenerate π* antibonding orbitals (Hund's rule), giving 2 unpaired electrons — so O2 is paramagnetic (bond order 2). - O2^- (superoxide, 17 electrons) has 1 unpaired electron in a π* orbital — paramagnetic (bond order 1.5). …

Which one of the following is diamagnetic ? (a) O2 (b) O2²- (c) O2^- (d) None of these

Question 82 of 84

Q. Which one of the following is diamagnetic ?

(a) O2

(b) O2^2-

(d) None of these

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We must identify which oxygen species has no unpaired electrons (diamagnetic).

The peroxide ion, O2^2-, is diamagnetic because all its electrons are paired; molecular O2 and the superoxide ion O2^- are paramagnetic.

Using molecular orbital theory for these O2 species:

O2 (16 electrons) has two electrons singly occupying the two degenerate π* antibonding orbitals (Hund's rule), giving 2 unpaired electrons — so O2 is paramagnetic (bond order 2).
O2^- (superoxide, 17 electrons) has 1 unpaired electron in a π* orbital — paramagnetic (bond order 1.5). …

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Q.Which one of the following is diamagnetic ?

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