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(B) $KO_2$ contains the superoxide ion $O_2^-$,which has one unpaired electron,making it paramagnetic.In $cis-[Co(en)_2Cl_2]^+$,$Co$ is in the $+3$ ox

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$A, D$

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(B) $KO_2$ contains the superoxide ion $O_2^-$,which has one unpaired electron,making it paramagnetic.In $cis-[Co(en)_2Cl_2]^+$,$Co$ is in the $+3$ oxidation state $(d^6)$. Since $en$ is a strong field ligand,all electrons are paired,making it diamagnetic.In $K_3[Co(Ox)_3]$,$Co$ is in the $+3$ oxidation state $(d^6)$. $Ox^{2-}$ is a strong field ligand,so all electrons are paired,making it diamagnetic.In $[CoCl_3]^{2-}$,$Co$ is in the $+2$ oxidation state $(d^7)$. $Cl^-$ is a weak field ligand,resulting in $3$ unpaired electrons,making it paramagnetic.Therefore,$KO_2$ and $[CoCl_3]^{2-}$ are paramagnetic.

Complex	Magnetic Moment $(BM)$
$K_4[Mn(CN)_6]$	$2.2$
$[Fe(H_2O)_6]^{2+}$	$5.3$
$K_2[MnCl_4]$	$5.9$

Select the paramagnetic molecule$(s)$ from the following:

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