Molecular orbital theory
Why this is asked: MOT's headline NEET question is O₂'s paramagnetism — two unpaired electrons in its degenerate π*2p orbitals, which the paired-electron double-bond picture from Lewis structures or VBT can't show at all. Watch the filling order too: from Li₂ to N₂, σ2p fills after π2p (s–p mixing pushes it up); from O₂ onward σ2p drops back below π2p.
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Given below are two statements:
Statement I: A hypothetical diatomic molecule with bond order zero is quite stable.
Statement II: As bond order increases, the bond length increases.
In the light of the above statements, choose the most appropriate answer from the options given below:
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Match List I with List II.
List I (Molecule) List II (Number and type of bonds between two carbon atoms) A. ethane I. one -bond and two -bonds B. ethene II. two -bonds C. carbon molecule, III. one -bond D. ethyne IV. one -bond and one -bond Choose the correct answer from the options given below:
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