Using Molecular Orbital theory complete the relative of the fall species and indicate their magnetic behaviour.
$\to O_{2}, O_{2}^{+}, O_{2}^{-}, O_{2}^{2 -}$

Open in App

Solution

$O_{2} \to$ Paramagnetic (2 unpaired $e^{-}$ )
$O_{2}^{-} \to$ Paramagnetic (1 unpaired $e^{-}$ )
$O_{2}^{+} \to$ Paramagnetic (1 unpaired $e^{-}$ )
$O_{2}^{2 -} \to$ no unpaired $e^{-}$ so Diamagnetic

Suggest Corrections

Similar questions

Compare the relative stability of the following species and indicate their magnetic properties;

O₂,, (superoxide), (peroxide)

M O

O_{2}

O_{2}^{2 -}

Question 32

Using molecular orbital theory, compare the bond energy and magnetic character of $O_{2}^{+}$ and $O_{2}^{+}$ species.

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

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

Join BYJU'S Learning Program