Which of the following ions is paramagnetic?

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Question

(A) To determine if a complex is paramagnetic,we check for the presence of unpaired electrons in the metal ion.$1$. In $[Ni(H_2O)_6]^{2+}$,$Ni$ is in

Vedclass · Accepted Answer

$[Ni(H_2O)_6]^{2+}$

Vedclass · Answer

(A) To determine if a complex is paramagnetic,we check for the presence of unpaired electrons in the metal ion.$1$. In $[Ni(H_2O)_6]^{2+}$,$Ni$ is in the $+2$ oxidation state $(3d^8)$. $H_2O$ is a weak field ligand,so the electrons remain unpaired,resulting in $2$ unpaired electrons. Thus,it is paramagnetic.$2$. In $[Fe(CN)_6]^{4-}$,$Fe$ is in the $+2$ oxidation state $(3d^6)$. $CN^-$ is a strong field ligand,causing pairing of electrons,resulting in $0$ unpaired electrons. It is diamagnetic.$3$. In $[Ni(CO)_4]$,$Ni$ is in the $0$ oxidation state $(3d^8 4s^2)$. $CO$ is a strong field ligand,causing pairing,resulting in $0$ unpaired electrons. It is diamagnetic.$4$. In $[Ni(CN)_4]^{2-}$,$Ni$ is in the $+2$ oxidation state $(3d^8)$. $CN^-$ is a strong field ligand,causing pairing,resulting in $0$ unpaired electrons. It is diamagnetic.Therefore,$[Ni(H_2O)_6]^{2+}$ is the paramagnetic species.

List-$I$	List-$II$
$a. [Fe(CN)_{6}]^{3-}$	$i. 5.92 \ BM$
$b. [Fe(H_{2}O)_{6}]^{3+}$	$ii. 0 \ BM$
$c. [Fe(CN)_{6}]^{4-}$	$iii. 4.90 \ BM$
$d. [Fe(H_{2}O)_{6}]^{2+}$	$iv. 1.73 \ BM$

Similar Questions

Match List-$I$ with List-$II$.

List-$I$ List-$II$

$a. [Fe(CN)_{6}]^{3-}$ $i. 5.92 \ BM$

$b. [Fe(H_{2}O)_{6}]^{3+}$ $ii. 0 \ BM$

$c. [Fe(CN)_{6}]^{4-}$ $iii. 4.90 \ BM$

$d. [Fe(H_{2}O)_{6}]^{2+}$ $iv. 1.73 \ BM$

Choose the correct answer from the options given below.

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