Coordination Compounds · Chemistry · Class 12

Write the IUPAC names of the following coordination compounds (any three):

(a) $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_4 \mathrm{Cl}\left(\mathrm{NO}_2\right)\right] \mathrm{Cl}$

(b) $\left[\mathrm{Ni}\left(\mathrm{NH}_3\right)_6\right] \mathrm{Cl}_2$

(c) $\mathrm{K}_3\left[\mathrm{Cr}\left(\mathrm{C}_2 \mathrm{O}_4\right)_3\right]$

(d) $\left[\mathrm{Co}(\mathrm{en})_2 \mathrm{Br}_2\right]^{+}$

The oxidation number of the central atom in a complex is defined as the charge it would carry if all the ligands are removed along with the electron pairs that are shared with the central atom. Similarly the charge on the complex is the sum of the charges of the constituent parts i.e. the sum of the charges on the central metal ion and its surrounding ligands. Based on this, the complex is called neutral if the sum of the charges of the constituents is equal to zero. However, for an anion or cationic complex, the sum of the charges of the constituents is equal to the charge on the coordination sphere.

Based on the above information, answer the following questions:

(a) Define ambidentate ligand with an example.

(b) What type of isomerism is shown by

$$\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_5 \mathrm{Cl}\right] \mathrm{SO}_4 \text { and }\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_5 \mathrm{SO}_4\right] \mathrm{Cl} \text { ? }$$

(c) Define chelate effect. How it affects the stability of complex?

OR

(c) Find the coordination number and oxidation state of chromium in $\mathrm{Na}_3\left[\mathrm{Cr}\left(\mathrm{C}_2 \mathrm{O}_4\right)_3\right]$.

(a) Which of the following species cannot act as a ligand? Give reason.

$$\mathrm{OH}^{-}, \mathrm{NH}_4^{+}, \mathrm{CH}_3 \mathrm{NH}_2, \mathrm{H}_2 \mathrm{O}$$

(b) The complex $$\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_5\left(\mathrm{NO}_2\right)\right] \mathrm{Cl}_2$$ is red in colour. Give IUPAC name of its linkage isomer.

(a) On the basic of crystal field theory write the electronic configuration for $$\mathrm{d}^5$$ ion with a strong field ligand for which $$\Delta_0>\mathrm{P}$$.

(b) $$\left[\mathrm{Ni}(\mathrm{CO})_4\right]$$ has tetrahedral geometry while $$\left[\mathrm{Ni}(\mathrm{CN})_4\right]^{2-}$$ has square planar yet both exhibit diamagnetism. Explain.

[Atomic number : $$\mathrm{Ni}=28$$ ]

In the two tetrahedral structures of dichromate ion

The magnetic moment of $$\left[\mathrm{NiCl}_4\right]^{2-}$$

[Atomic number : $$\mathrm{Ni}=28$$ ]

Assertion (A): Trans $$\left[\mathrm{Cr} \mathrm{Cl}_2(\mathrm{ox})_2\right]^{3-}$$ shows optical isomerism.

Reason (R): Optical isomerism is common in octahedral complexes involving bidentate ligands.