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  •  The metal complex that is diamagnetic is <img alt="\mathrm{\text { (Atomic number: } \mathrm{Fe}, 26 ; \mathrm{Cu}, 29 \text { ) }}" src="/latex-image/?%5Cmathrm%7B%5Ctext%20%7B%20%28Ato

 The metal complex that is diamagnetic is \mathrm{\text { (Atomic number: } \mathrm{Fe}, 26 ; \mathrm{Cu}, 29 \text { ) }}

Option: 1

\mathrm{\mathrm{K}_{3}\left[\mathrm{Cu}(\mathrm{CN})_{4}\right]}


Option: 2

\mathrm{\mathrm{K}_{2}\left[\mathrm{Cu}(\mathrm{CN})_{4}\right]}


Option: 3

\mathrm{\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{4}\right]}


Option: 4

\mathrm{\mathrm{K}_{4}\left[\mathrm{FeCl}_{6}\right]}


Answers (1)

best_answer

The metal complex will be diamagnetic if all electrons are paired.

(1) \mathrm{K}_3[(\mathrm{Cu}(\mathrm{CN})_{4}] \rightarrow \mathrm{Cu^{+}} \mathrm{\rightarrow 3d'^{o}4s^{o} \rightarrow fully \; paired \; \rightarrow diamagnetic}

(2) \mathrm{K}_2[(\mathrm{Cu}(\mathrm{CN})_{4}] \rightarrow \mathrm{Cu^{2+}} \mathrm{\rightarrow 3d^{s}4s^{o} \rightarrow over \; unpaired \; \rightarrow Paramagnetic}

(3) \mathrm{K}_3[(\mathrm{Fe}(\mathrm{CN})_{4}] \rightarrow \mathrm{Fe^{+}} \mathrm{\rightarrow 3d^{6}4s^{'} \rightarrow 5 \; unpaired \;electrons}

(4) \mathrm{K}_4[(\mathrm{Fe}(\mathrm{Cl})_{6}] \rightarrow \mathrm{Fe^{2+}} \mathrm{\rightarrow 3d^{6}4s^{o} \rightarrow 4 \; unpaired \;electrons}

Hence, Option (1) is correct.

Posted by

Ritika Jonwal

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