Among the following ions,which one has the hi | vedclass

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(B) To determine the highest paramagnetism,we calculate the number of unpaired electrons in each complex:$1$. $[Cr(H_2O)_6]^{3+}$: $Cr$ is in $+3$ oxi

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

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(B) To determine the highest paramagnetism,we calculate the number of unpaired electrons in each complex:$1$. $[Cr(H_2O)_6]^{3+}$: $Cr$ is in $+3$ oxidation state. $Cr(Z=24)$ configuration is $[Ar] 3d^5 4s^1$. $Cr^{3+}$ is $[Ar] 3d^3$. It has $3$ unpaired electrons.$2$. $[Fe(H_2O)_6]^{2+}$: $Fe$ is in $+2$ oxidation state. $Fe(Z=26)$ configuration is $[Ar] 3d^6 4s^2$. $Fe^{2+}$ is $[Ar] 3d^6$. Since $H_2O$ is a weak field ligand,the electrons are arranged as $t_{2g}^4 e_g^2$,resulting in $4$ unpaired electrons.$3$. $[Cu(H_2O)_6]^{2+}$: $Cu$ is in $+2$ oxidation state. $Cu(Z=29)$ configuration is $[Ar] 3d^{10} 4s^1$. $Cu^{2+}$ is $[Ar] 3d^9$. It has $1$ unpaired electron.$4$. $[Zn(H_2O)_6]^{2+}$: $Zn$ is in $+2$ oxidation state. $Zn(Z=30)$ configuration is $[Ar] 3d^{10} 4s^2$. $Zn^{2+}$ is $[Ar] 3d^{10}$. It has $0$ unpaired electrons.Since $[Fe(H_2O)_6]^{2+}$ has the maximum number of unpaired electrons $(4)$,it exhibits the highest paramagnetism.

Among the following ions,which one has the highest paramagnetism?

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