Coordination Compounds · Chemistry · COMEDK
MCQ (Single Correct Answer)
Which one of the following structures in Column I does not have the correct IUPAC name as given in Column II.
| S.No. | Structure | IUPAC name | |
|---|---|---|---|
| A. | $\left[\mathrm{CoBr}_2(\mathrm{en})_2\right] \mathrm{Cl}$ | P. | Dibromidodi-( ethan-1, 2 - diamine)cobalt (III) chloride |
| B. | $\mathrm{Na}\left[\mathrm{PtBrCl}\left(\mathrm{NO}_2\right)\left(\mathrm{NH}_3\right)\right]$ | Q. | Sodium amminebromidochloridonitrito- N - palatinate(II) |
| C. | $\left[\mathrm{Cr}\left(\mathrm{H}_2 \mathrm{O}\right)_2\left(\mathrm{NH}_3\right)_4 \mathrm{Cl}\right] \mathrm{SO}_4$ | R. | Tetraamminediaquachloridochromium (III) sulphate. |
| D. | $\left[\mathrm{Pt}\left(\mathrm{NH}_3\right)_4\right]\left[\mathrm{PtCl}_4\right]$ | S. | Tetraammineplatinum (II) tetrachloridoplatinate (II) |
Arrange the following compounds in the decreasing order of the molar conductivities of their aqueous solutions.
| A | B | C | D |
|---|---|---|---|
| $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_5 \mathrm{Cl}\right] \mathrm{Cl}_2$ | $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_3 \mathrm{Cl}_3\right]$ | $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_4 \mathrm{Cl}_2\right] \mathrm{Cl}$ | $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_6\right] \mathrm{Cl}_3$ |
Match the coordination compounds in Column I having the given type of hybridisation of $\mathrm{M}^{\mathrm{n}+}$ ion and magnetic moment as given in Column II.
| Coordination compounds | Hybridisation & Magnetic nature | ||
|---|---|---|---|
| A. | $\mathrm{Ni}(\mathrm{CO})_4$ | P. | $\mathrm{sp}^3, \quad \mu=5.92 \mathrm{BM}$ |
| B. | $\left[\mathrm{Ni}(\mathrm{CN})_4\right]^{2-}$ | Q. | $\mathrm{sp}^3, \quad \mu=2.84 \mathrm{BM}$ |
| C. | $\left[\mathrm{Ni}(\mathrm{Cl})_4\right]^{2-}$ | R. | $\mathrm{sp}^3, \quad \mu=0$ |
| D. | $\left[\mathrm{MnBr}_4\right]^{2-}$ | S. | $\mathrm{dsp}^2, \quad \mu=0$ |
Which of the following 2 compounds exhibit both Geometrical and Structural isomerism?
$$\begin{aligned} & \mathrm{A}=\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_4 \mathrm{Cl}_2\right] \mathrm{NO}_2 \\ & \mathrm{~B}=\left[\mathrm{Co}\left(\mathrm{NH}_3\right) \mathrm{Br}\right] \mathrm{SO}_4 \\ & \mathrm{C}=\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_3\left(\mathrm{NO}_2\right)_3\right] \\ & \mathrm{D}=\left[\mathrm{Cr}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right] \mathrm{Cl}_3 \end{aligned}$$
Based on Valence Bond Theory, match the complexes listed in Column I with the number of unpaired electrons on the central metal ion, given in Column II
| No. | Complex ions | No. | Number of unpaired electrons |
|---|---|---|---|
| (A) | $$ \left[\mathrm{Fe} \mathrm{F}_6\right]^{3-} $$ |
(P) | 0 |
| (B) | $$ \left[\mathrm{Fe}(\mathrm{CN})_6\right]^{4-} $$ |
(P) | 1 |
| (C) | $$ \left[\mathrm{Fe}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{2+} $$ |
(R) | 5 |
| (D) | $$ \left[\mathrm{Fe}(\mathrm{CN})_6\right]^{3-} $$ |
(S) | 4 |
Given below are 4 statements. Two of these are correct statements. Identify them.
A. $$\mathrm{Co}^{2+}$$ is easily oxidised to $$\mathrm{Co}^{3+}$$ in the presence of a strong ligand like $$\mathrm{CN}^{-}$$
B. $$[\mathrm{Fe}(\mathrm{CN})_6]^{4-}$$ is an octahedral complex ion which is paramagnetic in nature.
C. Removal of $$\mathrm{H}_2 \mathrm{O}$$ molecules from $$[\mathrm{Ti}(\mathrm{H}_2 \mathrm{O})_6] \mathrm{Cl}_3$$ on strong heating converts it to a colourless compound.
D. Crystal Field splitting in Octahedral and Tetrahedral complexes is given by the equation $$\Delta_0=4 / 9 \Delta_t$$
Based on Crystal Field theory, match the Complex ions listed in Column I with the electronic configuration in the d orbitals of the central metal ion listed in Column II.
| No. | Complexion | No. | d orbital configuration of central metal ion. |
|---|---|---|---|
| (A) | $$ \left[M n(C N)_6\right]^{4-} $$ |
(P) | $$ e_g^2 t_{2 g}^3 $$ |
| (B) | $$ \left[\mathrm{Co}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{2+} $$ |
(Q) | $$ t_{2 g}^4 e_g^2 $$ |
| (C) | $$ \left[\mathrm{Fe}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{2+} $$ |
(R) | $$ t_{2 g}^5 $$ |
| (D) | $$ \left[\mathrm{MnCl}_4\right]^{2-} $$ |
(S) | $$ t_{2 g}^5 e_g^2 $$ |
On the basis of crystal field theory, electronic configuration of a low spin $$\mathrm{d}^4$$ complex is:
The molar conductivity of the complex $$\mathrm{CoCl}_3 \cdot 4 \mathrm{NH}_3 \cdot 2 \mathrm{H}_2 \mathrm{O}$$ is found to be the same as that of a $$1: 3$$ electrolyte. The structural formula of the compound is :
The type of hybridisation and the spin only magnetic moment for the complex $$[\mathrm{Ni}(\mathrm{CO})_4]$$ are respectively:
A d - block metal $$\mathrm{X}(\mathrm{Z}=26)$$ forms a compound $$[\mathrm{X}(\mathrm{CN})_2(\mathrm{CO})_4]^{+}$$. Calculate its spin magnetic moment value.
A Coordination compound is represented by the formula $$[\mathrm{CoBr}_3(e n) x]$$. This compound required one mole of $$\mathrm{AgNO}_3$$ to form a pale yellow precipitate of $$\mathrm{AgBr}$$. What is the value of $$\mathrm{x}$$ in the compound?
Choose the incorrect statement from the following.
Which among the following is diamagnetic?
The complex $$\left[\mathrm{PtCl}_2(\mathrm{en})_2\right]^{2+}$$ ion shows
The blue colouration obtained from the Lassaigne's test of nitrogen is due to the formation of
Aqueous $$\mathrm{CuSO}_4$$ changes its colour from sky blue to deep blue on addition of $$\mathrm{NH}_3$$ because
Which of the following complex show optical isomerism?
(i) $$c i s-\left[\mathrm{COCl}(\mathrm{en})_2\left(\mathrm{NH}_3\right)\right]^{2+}$$
(ii) $$cis-\left[\mathrm{CrCl}_2(\mathrm{ox})_2\right]^{3-}$$
(iii) $$cis-[ \left.\mathrm{CO}(\mathrm{en})_2 \mathrm{Cl}_2\right] \mathrm{Cl}$$
(iv) $$cis- \left[\mathrm{CO}\left(\mathrm{NH}_3\right)_4 \mathrm{Cl}_2\right]^{+}$$
Mohr's salt has the formula
Identify the correct IUPAC name of $$[\mathrm{CoCl}_2(\mathrm{NO}_2)(\mathrm{NH}_3)_3]$$
Match the Coordination compounds given in Column I with their characteristic features listed in Column II.
| S.No. | Coordination compounds | S.No. | Characteristic features |
|---|---|---|---|
| W | $$ \left[\mathrm{Co}\left(\mathrm{NH}_3\right)_5 \mathrm{Cl}\right] \mathrm{Cl}_3 $$ |
P | $$ \text { Oxidation state }=+3 \text { Configuration }=\mathrm{d}^5 \quad \mu=5.92 \mathrm{BM} $$ |
| X | $$ \mathrm{K}_4\left[\mathrm{Mn}(\mathrm{CN})_6\right. $$ |
Q | $$ \text { Oxidation state }=+3 \text { Configuration }=\mathrm{d}^3 \quad \mu=3.87 \mathrm{BM} $$ |
| Y | $$ \left[\mathrm{CrCl}_3(\mathrm{py})_3\right] $$ |
R | $$ \text { Oxidation state }=+3 \text { Configuration }=d^6 \quad \mu=0 \mathrm{BM} $$ |
| Z | $$ \mathrm{Cs}\left[\mathrm{FeCl}_4\right] $$ |
S | $$ \text { Oxidation state }=+2 \text { Configuration }=\mathrm{d}^5 \quad \mu=1.732 \mathrm{BM} $$ |
Which one of the following is an incorrect statement pertaining to the properties of Coordination compounds?
Which one of the following Coordination entities exhibits Facial and Meridional isomerism?
The complex which does not show optical isomerism is
The oxidation state of nickel in [Ni(CO$$_4$$)] is
Which type of ligand is EDTA?
The correct IUPAC name of the coordination compound K$$_3$$[Fe(CN)$$_5$$NO] is
IUPAC name of Na$$_3$$[Co(NO$$_2$$)$$_6$$] is
The number of unidentate ligands in the complex ion is called
The oxidation state of iron in K$$_4$$[Fe(CN)$$_6$$] is,
Which complex cannot ionise in solution?