Coordination Compounds 2 Question 56
####58. Match the complexes in Column I with their properties listed in Column II.
$(2007,6 M)$
| Column I | Column II | ||
|---|---|---|---|
| (A) | $\left[Co\left(NH _3\right) _4\left(H _2 O\right) _2\right] Cl _2$ | p. | Geometrical isomers |
| (B) | $\left[Pt\left(NH _3\right) _2 Cl _2\right]$ | q. | Paramagnetic |
| (C) | $\left[Co\left(H _2 O\right) _5 Cl\right] Cl$ | r. | Diamagnetic |
| (D) | $\left[Ni\left(H _2 O\right) _6\right] Cl _2$ | s. | Metal ion with +2 oxidation state |
Fill in the Blanks
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Solution:
- (A) $\left[Co\left(NH _3\right) _4\left(H _2 O\right) _2\right] Cl _2: Co^{2+}, 3 d^{7}$ show geometrical isomerism, paramagnetic.
(B) $Pt\left(NH _3\right) _2 Cl _2: Pt^{2+}$ has $d^{8}$-configuration with all paired electrons. Show geometrical isomerism, diamagnetic.
(C) $\left[Co\left(H _2 O\right) _5 Cl\right] Cl: Co^{2+}, 3 d^{7}$
Cannot show geometrical isomerism, paramagnetic.
(D) $\left[Ni\left(H _2 O\right) _6\right] Cl _2: Ni^{2+}, 3 d^{8}$, weak ligand, has two unpaired electrons. Paramagnetic but cannot show geometrical isomerism.
