NEET UG CHEMISTRY MCQ: CO-ORDINATION COMPOUNDS

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Analyzing +4 | -1

Among the following complexes (

A-F

\begin{aligned} & {K}_3\left[{Fe}({CN})_6\right] ({A}),\left[{Co}\left({NH}_3\right)_6\right] {Cl}_3 (B)\\ & {Na}_3\left[{Co}(\text { oxalate })_3\right]({C}),\left[{Ni}_2\left({H}_2 {O}\right)_6\right] {Cl}_2 (D),\\ & {~K}_2\left[{Pt}({CN})_4\right]({E}) \text { and }\left[{Zn}\left({H}_2 {O}\right)_6\right]\left({NO}_3\right)_2({~F}) \end{aligned}

The diamagnetic complexes are:

View answer and explanation

Correct option: C

B, C, E, F

Option C is correct because B, C, E, and F are all diamagnetic complexes, meaning they have no unpaired electrons.

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\left[ {\mathrm{PtC}{\mathrm{l}_2}{{\left( {\mathrm{N}{\mathrm{H}_3}} \right)}_4}} \right]\mathrm{B}{\mathrm{r}_2}\mathrm{\;and\;}\left[ {\mathrm{PtB}{\mathrm{r}_2}{{\left( {\mathrm{N}{\mathrm{H}_3}} \right)}_4}} \right]\mathrm{C}{\mathrm{l}_2}\mathrm{\;}

\left[\mathrm{Cr}(\mathrm{Ox})_{2} \mathrm{ClBr}\right]^{3-}

\text{ox =}

x

{\left[ {\mathrm{Ni}{{\left( {\mathrm{CN}} \right)}_4}} \right]^x}

\mathrm{M}{\mathrm{n}^{2 + }}

\mathrm{CuS}{\mathrm{O}_4}

{\mathrm{K}_2}\left[ {\mathrm{Ni}{{\left( {\mathrm{CN}} \right)}_4}} \right]