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AgCl precipitate dissolves in NH${}_3$ due to the formation of –

1. [Ag(NH${}_3$)${}_2$]OH
2. [Ag(NH${}_3$)${}_4$]Cl
3. [Ag(NH${}_3$)${}_2$]Cl
4. [Ag(NH${}_3$)${}_2$]OH

Which one of the following compounds will exhibit linkage isomerism –
1. [Pt (NH${}_3$)${}_2$ Cl${}_2$]
2. [Co (NH${}_3$)${}_2$ NO${}_2$]Cl${}_2$
3. [Co (NH${}_3$)${}_4$ Cl${}_2$]Cl
4. [Co (en)${}_2$Cl${}_2$]Cl

A magnetic moment of 1.73 BM will be shown by one among of the following compounds –
1. [Cu(NH${}_3$)${}_4$]${}^{2+}$
2. [Ni(CN)${}_4$]${}^{2-}$
3. TiCl${}_4$
4. [CoCl${}_6$]${}^{-3}$

In the complex [Ni(H${}_2$O)${}_2$(NH${}_3$)${}_4$]${}^{+2}$ the magnetic moment ($\mathrm{\mu }$) of Ni is –
1. Zero
2. 2.83 BM
3. 1.73 BM
4. 3.87 BM

Identify the system with the highest number of unpaired electrons among the following is:
1. d${}^5$ (Octahedral, low spin)
2. d${}^8$ (Tetrahedral)
3. d${}^6$ (Octahedral, low spin)
4. d${}^3$ (Octahedral)

Nessler's reagent is -
1. ${\mathrm{K}}_2{\mathrm{HgI}}_4$
2. ${\mathrm{K}}_2{\mathrm{HgI}}_4+\mathrm{KOH}$
3. ${\mathrm{K}}_2{\mathrm{HgI}}_2+\mathrm{KOH}$
4. ${\mathrm{K}}_2{\mathrm{HgI}}_4+\mathrm{Hg}$

One among the following complex ions will not show optical activity –
1. $\left[\mathrm{Pt}\left(\mathrm{Br}\right)\left(\mathrm{Cl}\right)\left(\mathrm{I}\right)\left({\mathrm{NO}}_2\right)\left({\mathrm{C}}_2{\mathrm{H}}_5\mathrm{N}\right)\left({\mathrm{NH}}_3\right)\right]$
2. $\mathrm{Cis}-{\left[\mathrm{Co}{\left(\mathrm{en}\right)}_2{\mathrm{Cl}}_2\right]}^{+}$
3. ${\left[\mathrm{Co}\left(\mathrm{en}\right){\left({\mathrm{NH}}_3\right)}_2{\mathrm{Cl}}_2\right]}^{+}$
4. $\left[\mathrm{Cr}{\left({\mathrm{NH}}_3\right)}_4{\mathrm{Cl}}_2\right]$

A Planar Complex (Mabcd) gives –
1. Two Optical isomer 
2. Two geometrical isomer
3. Three optical isomer 
4. Three geometrical isomers

A complex shown below can exhibit –

1. Geometrical isomerism only
2. Optical isomerism only
3. Both Optical and geometrical isomerism
4. None

$\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_4{\mathrm{Cl}}_2\right]{\mathrm{NO}}_2 \mathrm{and} \left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_4\mathrm{Cl} {\mathrm{NO}}_2\right]\mathrm{Cl}$ are –
1. Geometrical isomers 
2. Optical isomers
3. Linkage isomers 
4. Ionisation isomers

Which of the following has two geometrical isomers, and is also a non ionisable complex –
1. ${\mathrm{PtCl}}_4 2{\mathrm{NH}}_3$
2. ${\mathrm{PtCl}}_4 3{\mathrm{NH}}_3$
3. ${\mathrm{PtCl}}_4 4{\mathrm{NH}}_3$
4. ${\mathrm{PtCl}}_4 6{\mathrm{NH}}_3$

Na₂S₂O₃.5H₂O is used in photography to –
1. Reduce AgBr to metallic Ag
2. Remove reduced Ag
3. Remove undecomposed AgBr as a soluble complex
4. Converts metallic Ag to silver salt

Which gives only 25% mole of cloride as AgCl, when reacts with excess AgNO₃
–
1. ${\mathrm{PtCl}}_2. 4{\mathrm{NH}}_3$
2. ${\mathrm{PtCl}}_4. 5{\mathrm{NH}}_3$
3. ${\mathrm{PtCl}}_4. 4{\mathrm{NH}}_3$
4. ${\mathrm{PtCl}}_4. 3{\mathrm{NH}}_3$

In [Cr(C₂O₄)₃]^3–, the isomerism shown is
1. Ligand 
2. Optical 
3. Geometrical 
4. Ionization

In the complexes ${\left[\mathrm{Fe}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6\right]}^{3+},{\left[Fe{\left(SCN\right)}_{\left(6\right)}\right]}^{3-},{\left[Fe{\left(C_2{O}_4\right)}_3\right]}^{3-} and {\left[FeC{l}_6\right]}^{3-}$, more stability is shown by 
1. ${\left[\mathrm{Fe}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6\right]}^{3+}$
2. ${\left[Fe{\left(SCN\right)}_{\left(6\right)}\right]}^{3-}$
3. ${\left[Fe{\left(C_2{O}_4\right)}_3\right]}^{3-}$
4. ${\left[FeC{l}_6\right]}^{3-}$

One mole of the complex compound $\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_5{\mathrm{Cl}}_3$, gives 3 moles of ions on dissolution in water. One mole of the same complex reacts with two moles of AgNO₃ solution to yield two moles of AgCl (s). The structure of the complex is
1. $\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_3{\mathrm{Cl}}_3\right].2N{H}_3$
2. $\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_4{\mathrm{Cl}}_2\right].\mathrm{Cl}.N{H}_3$
3. $\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_4\mathrm{Cl}\right].{\mathrm{Cl}}_2.N{H}_3$
4. $\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_5\mathrm{Cl}\right].{\mathrm{Cl}}_2$

In the coordination compound K${}_4$[Ni(CN)${}_4$], the oxidation state of nickel is –
1. 0
2. +1
3. +2
4. -1

The number of 3d-electrons remained in Fe${}^{2+}$ (At.no. of Fe = 26) ion is –
1. 4
2. 5
3. 6
4. 3

Ammonia forms the complex ion [Cu(NH${}_3$)${}_4$]${}^{2+}$ with copper ions in alkaline solutions but not in acidic solution. What is the reason for it :-
1. In acidic solutions hydration protects copper ions
2. In acidic solutions protons coordinate with ammonia molecules forming NH${}_4^{+}$ ions and NH${}_3$ molecules are not available
3. In alkaline solutions insoluble Cu(OH)${}_2$ is precipitated which is soluble in excess of any alkali
4. Copper hydroxide is an amphoteric substance

Among the properties (a) reducing (b) oxidising (c) complexing, the set of properties shown by CN–
ion towards metal
species is
1. c, a
2. b, c
3. a, b
4. a, b, c

The coordination number of a central metal atom in a complex is determined by
1. The number of ligands around a metal ion bonded by sigma and pi-bonds both
2. The number of ligands around a metal ion bonded by pi-bonds
3. The number of ligands around a metal ion bonded by sigma bonds
4. The number of only anionic ligands bonded to the metal ion

Which one of the following complexes is an outer orbital complex :-
1. [Co(NH${}_3$)${}_6$]${}^{3+}$
2. [Mn(CN)${}_6$]${}^{4-}$
3. [Fe(CN)${}_6$]${}^{4-}$
4. [Ni(NH${}_3$)${}_6$]${}^{2+}$
(Atomic nos.:Mn=25 ; Fe=26 ; Co=27 ; Ni = 28)

Coordination compounds have great importance in biological systems. In this contect which of the following statements
is incorrect ?
1. Cyanocobalamin is vitamin B${}_{12}$ and contains cobalt
2. Haemoglobin is the red pigment of blood and contains iron
3. Chlorophylls are green pigments in plants and contain calcium
4. Carboxypeptidase - A is an enzyme and contains zinc

The correct order of magnetic moments (spin only values in B.M.) among is
1. [Fe(CN)${}_6$]${}^{4-}$ > [MnCl${}_4$]${}^{2-}$ > [CoCl${}_4$]${}^{2-}$
2. [MnCl${}_4$]${}^{2-}$ > [Fe(Cn)${}_6$]${}^{4-}$ > [CoCl${}_4$]${}^{2-}$
3. [MnCl${}_4$]${}^{4-}$ > [CoCl${}_4$]${}^{2-}$ > [Fe(Cn)${}_6$]${}^{4-}$
4. [Fe(Cn)${}_6$]${}^{4-}$ >  [CoCl${}_4$]${}^{2-}$ > [MnCl${}_4$]${}^{2-}$

For octahedral complex, the value of the 'spin only' magnetic moment for one of the following configurations is 2.84
BM. The correct one is
1. d${}^4$ (in strong ligand field)
2. d${}^4$ (in weak ligand field)
3. d${}^3$ (in weak as well as in strong field)
4. d${}^5$ (in strong ligand field)

The IUPAC name for the complex [Co(NO${}_2$) (NH${}_3$)${}_5$ ]Cl${}_2$ is
1. pentaammine nitrito-N- cobalt (II) chloride
2. pentaammine nitrito-N- cobalt (III) chloride
3. nitrito-N- pentaamminecobalt (III) chloride
4. nitrito-N- pentaamminecobalt (II) chloride

Nickel (Z=28) combines with a uninegative monodentate ligand X– to form a paramagnetic complex [NiX${}_4$]${}^{2-}$. The number of unpaired electron in the nickel and geometry of this complex ion are, respectively.
1. one, square planar
2. two, square planar
3. one, tetrahedral
4. two, tetrahedra

In Fe (CO)${}_5$ , the Fe–C bond possesses
1. ionic character
2. $\mathrm{\sigma }$ – character only
3. $\mathrm{\pi }$ – character only
4. both $\mathrm{\sigma }$ and $\mathrm{\pi }$ character

How many EDTA (ethylenediaminetetraacetic acid) molecules are required to make an octahedral complex with a Ca${}^{2+}$ ion ?
1. One
2. Two
3. Six
4. Three

The "spin-only" magnetic moment [in units of Bohr magneton, (${\mathrm{\mu }}_{\mathrm{B}}$)] of Ni${}^{2+}$ in aqueous solution would be
(At. No. Ni= 28)
1. 0
2. 1.73 
3. 2.84 
4. 4.90