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(B) For $[Co(NH_3)_6]Cl_2$:$Co$ is in $+2$ oxidation state. The electronic configuration of $Co^{2+}$ is $[Ar] 3d^7$.Since $NH_3$ is a weak field liga

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$3$

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(B) For $[Co(NH_3)_6]Cl_2$:$Co$ is in $+2$ oxidation state. The electronic configuration of $Co^{2+}$ is $[Ar] 3d^7$.Since $NH_3$ is a weak field ligand for $Co^{2+}$,no pairing occurs.The configuration is $t_{2g}^5 e_g^2$,resulting in $3$ unpaired electrons.For $[Co(NH_3)_6]Cl_3$:$Co$ is in $+3$ oxidation state. The electronic configuration of $Co^{3+}$ is $[Ar] 3d^6$.Since $NH_3$ is a strong field ligand for $Co^{3+}$,pairing occurs.The configuration is $t_{2g}^6 e_g^0$,resulting in $0$ unpaired electrons.Total number of unpaired electrons = $3 + 0 = 3$.

List-$I$	List-$II$
$A$. $[MnBr_4]^{2-}$	$I$. $d^2sp^3$ and diamagnetic
$B$. $[FeF_6]^{3-}$	$II$. $sp^3d^2$ and paramagnetic
$C$. $[Co(C_2O_4)_3]^{3-}$	$III$. $sp^3$ and diamagnetic
$D$. $[Ni(CO)_4]$	$IV$. $sp^3$ and paramagnetic

The total number of unpaired electrons present in $[Co(NH_3)_6]Cl_2$ and $[Co(NH_3)_6]Cl_3$ is $......$

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