State true or false.
$O_{2}, O_{2}^{-}$ are paramagnetic while $O_{3}, O_{2}^{2 -}$ are diamagnetic.

True

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False

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Solution

The correct option is A True
The given statement is true.
$O_{2}$ and $O_{2}^{-}$ are paramagnetic while $O_{3}$ and $O_{2}^{2 -}$ are diamagnetic.
If unpaired electrons are present in an ion/molecule, then it is paramagnetic.
If all electrons are paired, then the ion/molecule is diamagnetic
The MO electronic configurations are given.
$O_{2} : K K (σ 2 s)^{2} (σ * 2 s)^{2} (σ 2 p x)^{2} (π 2 p y)^{2} (π 2 p z)^{2} (π * 2 p y)^{1} (π * 2 p z)^{1}$ 2 unpaired electrons.
$O_{2}^{-} : K K (σ 2 s)^{2} (σ * 2 s)^{2} (σ 2 p x)^{2} (π 2 p y)^{2} (π 2 p z)^{2} (π * 2 p y)^{2} (π * 2 p z)^{1}$ 1 unpaired electron.
$O_{2}^{2 -} : K K (σ 2 s)^{2} (σ * 2 s)^{2} (σ 2 p x)^{2} (π 2 p y)^{2} (π 2 p z)^{2} (π * 2 p y)^{2} (π * 2 p z)^{2}$ 0 unpaired electrons.
The Lewis structure of ozone is shown in image.

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O_{2}, O_{2}^{-}

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