Which of the following complexes is paramagne | vedclass

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(D) To determine if a complex is paramagnetic,we check for the presence of unpaired electrons in the central metal ion.$1$. In $[Fe(CN)_6]^{4-}$,$Fe$

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Both $B$ and $C$

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(D) To determine if a complex is paramagnetic,we check for the presence of unpaired electrons in the central metal ion.$1$. In $[Fe(CN)_6]^{4-}$,$Fe$ is in $+2$ oxidation state $(d^6)$. $CN^-$ is a strong field ligand,causing pairing of electrons,resulting in $0$ unpaired electrons (diamagnetic).$2$. In $[Cu(NH_3)_4]^{2+}$,$Cu$ is in $+2$ oxidation state $(d^9)$. It has $1$ unpaired electron in the $3d$ orbital (paramagnetic).$3$. In $[Ti(H_2O)_6]^{3+}$,$Ti$ is in $+3$ oxidation state $(d^1)$. It has $1$ unpaired electron in the $3d$ orbital (paramagnetic).Therefore,both $[Cu(NH_3)_4]^{2+}$ and $[Ti(H_2O)_6]^{3+}$ are paramagnetic.

Which of the following complexes is paramagnetic?

Similar Questions

Total number of cis $N-Mn-Cl$ bond angles (that is,$Mn-N$ and $Mn-Cl$ bonds in cis positions) present in $cis-[Mn(en)_2Cl_2]$ is: $(en = NH_2CH_2CH_2NH_2)$

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$d$. $[Pt(NH_3)_4Cl_2]$
$e$. $[Pt(NH_3)_2Cl_2]$

What type of isomerism is exhibited by $[Cr(H_2O)_6]Cl_3$ and $[Cr(H_2O)_5Cl]Cl_2 \cdot H_2O$?

Which of the following sets represents an example of coordination isomerism in complexes?

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