Chapter 23

The octahedral complex of a metal ion \(\mathrm{M}^{3+}\) with four monodentate ligands \(L_{1}, L_{2}, L_{3}\) and \(L_{4}\) absorb wavelengths in the region of red, green, yellow and blue, respectively. The increasing order of ligand strength of the four ligands is: (a) \(L_{4}

The complex ion which has no ' \(d\) ' electron in the central metal atom is (a) \(\left[\mathrm{MnO}_{4}\right]^{-}\) (b) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}\) (c) \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}\) (d) \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\)

An octahedral complex of \(\mathrm{Co}^{3+}\) is diamagnetic. The hybridisation involved in the formation of the complex is: (a) \(s p^{3} d^{2}\) (b) \(d s p^{2}\) (c) \(d^{2} s p^{3}\) (d) \(s p^{3} d\)

Which of the following is an organometallic compound? (a) Lithium methoxide (b) Lithium acetate (c) Lithium dimethylamide (d) Methyl lithium

Consider the coordination compound, \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{3} .\) In the formation of this complex, the species which acts as the Lewis acid is: (a) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}\) (b) \(\mathrm{Cl}^{-}\) (c) \(\mathrm{Co}^{3+}\) (d) \(\mathrm{NH}_{3}\)

The total number of coordination sites in ethylenediaminetetraacetate \(\left(\mathrm{EDTA}^{4-}\right)\) is

Nickel \((Z=28)\) combines with a uninegative monodentate ligand to form a diamagnetic complex \(\left[\mathrm{NiL}_{4}\right]^{2-}\). The hybridisation involved and the number of unpaired electrons present in the complex are respectively: (a) \(s p^{3}\), two (b) \(d s p^{2}\), zero (c) \(d s p^{2}\), one (d) \(s p^{3}\), zero

Total number of cis \(\mathrm{N}-\mathrm{Mn}-\mathrm{Cl}\) bond angles (that is \(\mathrm{Mn}-\mathrm{N}\) and \(\mathrm{Mn}\) \(-\mathrm{Cl}\) bonds in cis positions) present in a molecule of cis \(\left[\mathrm{Mn}(\mathrm{en})_{2} \mathrm{Cl}_{2}\right]\) complex is \(\left(\mathrm{en}=\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\right)\)

The structure of which of the following chloro species can be explained on the basis of \(d s p^{2}\) hybridisation? (a) \(\mathrm{PdCl}_{4}^{2-}\) (b) \(\mathrm{FeCl}_{4}^{2-}\) (c) \(\mathrm{CoCl}_{4}^{2-}\) (d) \(\mathrm{NiCl}_{4}^{2-}\)

The number of geometric isomers possible for the complex \(\left[\mathrm{Co} L_{2} \mathrm{Cl}_{2}\right]^{-}\) \(\left(L=\mathrm{H}_{2} \mathrm{NCH}_{2} \mathrm{CH}_{2} \mathrm{O}^{-}\right)\)is

The magnetic moment of the complex anion \(\left[\mathrm{Cr}(\mathrm{NO})\left(\mathrm{NH}_{3}\right)(\mathrm{CN})_{4}\right]^{2-}\) is : (a) \(5.91 \mathrm{BM}\) (b) \(3.87 \mathrm{BM}\) (c) \(1.73 \mathrm{BM}\) (d) \(2.82 \mathrm{BM}\)

Among the complex ions, \(\left[\mathrm{Co}\left(\mathrm{NH}_{2}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{NH}_{2}\right)_{2} \mathrm{Cl}_{2}\right]^{+}, \quad\left[\mathrm{CrCl}_{2}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{2}\right]^{3-}, \quad\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}(\mathrm{OH})_{2}\right]^{+}\), \(\left[\mathrm{Fe}\left(\mathrm{NH}_{3}\right)_{2}(\mathrm{CN})_{4}\right]^{-}\) \(\left[\mathrm{Co}\left(\mathrm{NH}_{2}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{NH}_{2}\right)_{2}\left(\mathrm{NH}_{3}\right) \mathrm{Cl}\right]^{2+}\) and \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4}\left(\mathrm{H}_{2} \mathrm{O}\right) \mathrm{Cl}\right]^{2+}\), the number of complex ion(s) that show(s) cis- trans isomerism is

Consider the following complex ions, \(P, Q\) and \(R\). \(P=\left[\mathrm{FeF}_{6}\right]^{3-}, Q=\left[\mathrm{V}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) and \(R=\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) The correct order of the complex ions, according to their spin-only magnetic moment values (in B.M.) is (a) \(R

In the complex acetylbromidodicarbonylbis (triethylphosphine) iron (II), the number of \(\mathrm{Fe}-\mathrm{C}\) bond(s) is

\(\mathrm{NiCl}_{2}\left\\{\mathrm{P}\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{2}\left(\mathrm{C}_{6} \mathrm{H}_{5}\right)\right\\}_{2}\) exhibits temperature depend-ent magnetic behaviour (paramagnetic/diamagnetic). The coordination geometries of \(\mathrm{Ni}^{2+}\) in the paramagnetic and diamagnetic states are respectively (a) tetrahedral and tetrahedral (b) square planar and square planar (c) tetrahedral and square planar (d) square planar and tetrahedral

Among the following complexes \((\mathbf{K}-\mathbf{P})\) \(\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right](\mathbf{K}),\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{3}(\mathrm{~L}), \mathrm{Na}_{3}\left[\mathrm{Co}(\text { oxalate })_{3}\right](\mathbf{M})\), the \(\left[\mathrm{Ni}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{Cl}_{2}(\mathbf{N}), \mathrm{K}_{2}\left[\mathrm{Pt}(\mathrm{CN})_{4}\right](\mathbf{O})\) and \(\left[\mathrm{Zn}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]\left(\mathrm{NO}_{3}\right)_{2}(\mathbf{P})\) the diamagnetic complexes are (a) \(\mathrm{K}, \mathrm{L}, \mathrm{M}, \mathrm{N}\) (b) \(\mathrm{K}, \mathrm{M}, \mathrm{O}, \mathrm{P}\) (c) \(\mathrm{L}, \mathrm{M}, \mathrm{O}, \mathrm{P}\) (d) \(\mathrm{L}, \mathrm{M}, \mathrm{N}, \mathrm{O}\)

The volume (in \(\mathrm{mL}\) ) of \(0.1 \mathrm{M} \mathrm{AgNO}_{3}\) required for complete precipitation of chloride ions present in \(30 \mathrm{~mL}\) of \(0.01 \mathrm{M}\) solution of \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{Cl}\right] \mathrm{Cl}_{2}\), as silver chloride is close to

Geometrical shapes of the complexes formed by the reaction of \(\mathrm{Ni}^{2+}\) with \(\mathrm{Cl}^{-}, \mathrm{CN}^{-}\)and \(\mathrm{H}_{2} \mathrm{O}\), respectively, are [2011] (a) octahedral, tetrahedral and square planar (b) tetrahedral, square planar and octahedral (c) square planar, tetrahedral and octahedral (d) octahedral, square planar and octahedral

The complex showing a spin-only magnetic moment of \(2.82\) B.M. is : (a) \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]\) (b) \(\left[\mathrm{NiCl}_{4}\right]^{2-}\) (c) \(\left[\mathrm{Ni}\left(\mathrm{PPh}_{3}\right)_{4}\right]\) (d) \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\)

The number of water molecule(s) directly bonded to the metal centre in \(\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}\) is

The IUPAC name of \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{3}\) is \(\ldots \ldots \ldots \ldots\)

Both \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]\) and \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\) are diamagnetic. The hybridisations of nickel in these complexes, respectively, are (a) \(s p^{3}, s p^{3}\) (b) \(s p^{3}, d s p^{2}\) (c) \(d s p^{2}, s p^{3}\) (d) \(d s p^{2}, s p^{2}\)

The pair(s) of coordination complexes/ions exhibiting the same kind of isomerism is(are) (a) \(\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}\right] \mathrm{Cl}_{2}\) and \(\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right] \mathrm{Cl}\) (b) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right]^{+}\)and \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2}\left(\mathrm{H}_{2} \mathrm{O}\right) \mathrm{Cl}\right]^{+}\) (c) \(\left[\mathrm{CoBr}_{2} \mathrm{Cl}_{2}\right]^{2-}\) and \(\left[\mathrm{PtBr}_{2} \mathrm{Cl}_{2}\right]^{2}\) (d) \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{3}\left(\mathrm{NO}_{3}\right)\right] \mathrm{Cl}\) and \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{3} \mathrm{Cl}\right] \mathrm{Br}\)

Among the following metal carbonyls, the C-O bond order is lowest in (a) \(\left[\mathrm{Mn}(\mathrm{CO})_{6}\right]^{+}\) (b) \(\left[\mathrm{Fe}(\mathrm{CO})_{5}\right]\) (c) \(\left[\mathrm{Cr}(\mathrm{CO})_{6}\right]\) (d) \(\left[\mathrm{V}(\mathrm{CO})_{6}\right]^{-}\)

The compound(s) that exhibit(s) geometrical isomerism is (are) (a) \(\left[\mathrm{Pt}(\mathrm{en}) \mathrm{Cl}_{2}\right]\) (b) \(\left[\mathrm{Pt}(\mathrm{en})_{2}\right] \mathrm{Cl}_{2}\) (c) \(\left[\mathrm{Pt}(\mathrm{en})_{2} \mathrm{Cl}_{2}\right] \mathrm{Cl}_{2}\) (d) \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\right]\)

\(\mathrm{Ag}^{+}+\mathrm{NH}_{3} \rightleftharpoons\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)\right]^{+} ; k_{1}=6.8 \times 10^{-3}\) \(\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)\right]^{+}+\mathrm{NH}_{3} \rightleftharpoons\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+} ; \mathrm{k}_{2}=1.6 \times 10^{-3}\) then the formation constant of \(\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+}\)is \([2006-3 \mathrm{M},-1]\) (a) \(6.8 \times 10^{-6}\) (b) \(1.08 \times 10^{-5}\) (c) \(1.08 \times 10^{-6}\) (d) \(6.8 \times 10^{-5}\)

Statement-1 : The geometrical isomers of the complex \(\left[M\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right]\) are optically inactive. Statement-2 : Both geometrical isomers of the complex \(\left[M\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right]\) possess axis of symmetry.

The species having tetrahedral shape is (a) \(\left[\mathrm{PdCl}_{4}\right]^{2-}\) (b) \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\) (c) \(\left[\mathrm{Pd}(\mathrm{CN})_{4}\right]^{2-}\) (d) \(\left[\mathrm{NiCl}_{4}\right]^{2-}\)

Write the formulae of the following complexes: (i) Pentaamminechlorocobalt(III) (ii) Lithium tetrahydroaluminate(III).

The geometry of \(\mathrm{Ni}(\mathrm{CO})_{4}\) and \(\mathrm{Ni}\left(\mathrm{PPh}_{3}\right)_{2} \mathrm{Cl}_{2}\) are (a) both square planar (b) tetrahedral and square planar, respectively (c) both tetrahedral (d) square planar and tetrahedral, respectively

Write down the IUPAC names of the following compounds: (i) \(\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{CO}_{3}\right] \mathrm{Cl}\) (ii) \(\mathrm{K}_{3}\left[\mathrm{Cr}(\mathrm{CN})_{6}\right]\) (iii) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{ONO}\right] \mathrm{Cl}_{2}\)

Amongst \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right],\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\) and \(\left[\mathrm{NiCl}_{4}^{2-}\right]\) (a) \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]\) and \(\left[\mathrm{NiCl}_{4}^{2-}\right]\) are diamagnetic and \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\) is paramagnetic (b) \(\left[\mathrm{NiCl}_{4}^{2}\right]\) and \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\) are diamagnetic and \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]\) is paramagnetic (c) \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]\) and \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\) are diamagnetic and \(\left[\mathrm{NiCl}_{4}^{2-}\right]\) is paramagnetic (d) \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]\) is diamagnetic and \(\left[\mathrm{NiCl}_{4}^{2-}\right]\) and \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\) are paramagnetic

Amongst the following, the lowest degree of paramagnetism per mole of the compound at \(298 \mathrm{~K}\) will be shown by (a) \(\mathrm{MnSO}_{4} \cdot 4 \mathrm{H}_{2} \mathrm{O}\) (b) \(\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}\) (c) \(\mathrm{FeSO}_{4} \cdot 6 \mathrm{H}_{2} \mathrm{O}\) (d) \(\mathrm{NiSO}_{4} \cdot 6 \mathrm{H}_{2} \mathrm{O}\)

Among the species given below, the total number of diamagnetic species is \(\mathrm{H}\) atom, \(\mathrm{NO}_{2}\) monomer, \(\mathrm{O}_{2}^{-}\)(superoxide), dimeric sulphur in vapour phase, \(\mathrm{Mn}_{3} \mathrm{O}_{4},\left(\mathrm{NH}_{4}\right)_{2}\left[\mathrm{FeCl}_{4}\right],\left(\mathrm{NH}_{4}\right)_{2}\left[\mathrm{NiCl}_{4}\right], \mathrm{K}_{2} \mathrm{MnO}_{4}, \mathrm{~K}_{2} \mathrm{CrO}_{4}\).

For the octahedral complexes of \(\mathrm{Fe}^{3+}\) in \(\mathrm{SCN}^{-}\)(thiocyanato-S) and in \(\mathrm{CN}^{-}\)ligand environments, the difference between the spin-only magnetic moments in Bohr magnetons (when approximated to the nearest integer) is [Atomic number of \(\mathrm{Fe}=26]\)

The volume (in \(\mathrm{mL}\) ) of \(0.125 \mathrm{M} \mathrm{AgNO}_{3}\) required to quantitatively precipitate chloride ions in \(0.3 \mathrm{~g}\) of \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{3}\) is [Main Jan. \(\mathbf{0 8}, \mathbf{2 0 2 0}\) (I)] \(\mathrm{M}_{\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{j} \mathrm{Cl}_{3}\right.}=267.46 \mathrm{~g} / \mathrm{mol}\) \(\mathrm{M}_{\mathrm{AgNO}_{3}}=169.87 \mathrm{~g} / \mathrm{mol}\)

Complexes \(\left(\mathrm{ML}_{5}\right)\) of metals \(\mathrm{Ni}\) and \(\mathrm{Fe}\) have ideal square pyramidal and trigonal bipyramidal geometries, respectively. The sum of the \(90^{\circ}\), \(120^{\circ}\) and \(180^{\circ}\) L-M-L angles in the two complexes is ______.

The type of magnetism exhibited by \(\left[\mathrm{Mn}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) ion is \(\ldots \ldots \ldots \ldots .\)

The correct option(s) regarding the complex \(\left[\mathrm{Co}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{3}\left(\mathrm{H}_{2} \mathrm{O}\right)\right]^{3+}\) \(\left(\right.\) en \(=\mathrm{H}_{2} \mathrm{NCH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\) ) is (are) (a) It has two geometrical isomers (b) It will have three geometrical isomers if bidentate 'en' is replaced by two cyanide ligands (c) It is paramagnetic (d) It absorbs light at longer wavelength as compared to \(\left[\mathrm{Co}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{4}\right]^{3+}\)

The correct statement(s) regarding the binary transition metal carbonyl compounds is (are) (Atomic numbers: \(\mathrm{Fe}=26, \mathrm{Ni}=28\) ) (a) Total number of valence shell electrons at metal centre in \(\mathrm{Fe}(\mathrm{CO})_{5}\) or \(\mathrm{Ni}(\mathrm{CO})_{4}\) is 16 (b) These are predominantly low spin in nature (c) Metal-carbon bond strengthens when the oxidation state of the metal is lowered (d) The carbonyl C-O bond weakens when the oxidation state of the metal is increased

Addition of excess aqueous ammonia to a pink coloured aqueous solution of \(\mathrm{MCl}_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O}(\mathrm{X})\) and \(\mathrm{NH}_{4} \mathrm{Cl}\) gives an octahedral complex \(Y\) in the presence of air. In aqueous solution, complex \(Y\) behaves as \(1: 3\) electrolyte. The reaction of \(X\) with excess \(\mathrm{HCl}\) at room temperature results in the formation of a blue coloured complex \(Z\). The calculated spin only magnetic moment of \(X\) and \(Z\) is \(3.87\) B.M., whereas it is zero for complex \(Y\). Among the following options, which statement(s) is (are) correct? (a) Addition of silver nitrate to \(Y\) gives only two equivalents of silver chloride (b) The hybridization of the central metal ion in \(Y\) is \(d^{2} s p^{3}\) (c) \(Z\) is a tetrahedral complex (d) When \(X\) and \(Z\) are in equilibrium at \(0^{\circ} \mathrm{C}\), the colour of the solution is pink

If the bond length of \(\mathrm{CO}\) bond in carbon monoxide is \(1.128 \AA\), then what is the value of \(\mathrm{CO}\) bond length in \(\mathrm{Fe}(\mathrm{CO})_{5} ?\) (a) \(1.15 \AA\) (b) \(1.128 \AA\) (c) \(1.13 \AA\) (d) \(1.118 \AA\)

In nitroprusside ion the iron and NO exist as \(\mathrm{Fe}^{\mathrm{II}}\) and \(\mathrm{NO}^{+}\)rather than \(\mathrm{Fe}^{\mathrm{III}}\) and NO. These forms can be differentiated by (a) estimating the concentration of iron (b) measuring the concentration of \(\mathrm{CN}^{-}\) (c) measuring the solid state magnetic moment (d) thermally decomposing the compound.

Among the following ions which one has the highest paramagnetism? (a) \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) (b) \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) (c) \(\left[\mathrm{Cu}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) (d) \(\left[\mathrm{Zn}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\)

Match each coordination compound in List-I with an appropriate pair of characteristics from List- II and select the correct answer using the code given below the lists. \(\left\\{\right.\) en \(=\mathrm{H}_{2} \mathrm{NCH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2} ;\) atomic numbers : \(\mathrm{Ti}=22 ; \mathrm{Cr}=24 ; \mathrm{Co}=27 ; \mathrm{Pt}=\) \(\quad 78\\}\) List-I (A) \(\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right] \mathrm{Cl}\) (B) \(\left[\mathrm{Ti}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{Cl}\right]\left(\mathrm{NO}_{3}\right)_{2}\) (C) \(\left[\mathrm{Pt}(\mathrm{en})\left(\mathrm{NH}_{3}\right) \mathrm{Cl}\right] \mathrm{NO}_{3}\) (D) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4}\left(\mathrm{NO}_{3}\right)_{2}\right] \mathrm{NO}_{3}\) ListII (p) Paramagnetic and exhibits ionisation isomerism (q) Diamagnetic and exhibits cistrans isomerism (r) Paramagnetic and exhibits cistrans isomerism \((\mathrm{s})\) Diamagnetic and exhibits ionisation isomerism A B C D (a) (s) (q) (r) (p) (b) (r) (p) (s) (q) (c) (q) (p) (r) (s) (d) (p) (r) (s) (q)

Match the complexes in Column I with their properties listed in Column II. Column I (A) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right] \mathrm{Cl}_{2}\) (B) \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\right]\) (C) \(\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{Cl}\right] \mathrm{Cl}\) (D) \(\left[\mathrm{Ni}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{Cl}_{2}\) Column II (p) geometrical isomers (q) paramagnetic (r) diamagnetic (s) metal ion with \(+2\) oxidation state

The IUPAC name of \(A\) and \(B\) are \([2006-5 \mathrm{M},-2]\) (a) Potassium tetracyanonickelate (II), potassium tetrachloronickelate (II) (b) Tetracyanopotassiumnickelate, tetrachloropotassiumnickelate (II) (c) Tetracyanonickel (II), tetrachloronickel (II) (d) Potassium tetracyanonickel (II), potassium tetrachloronickel (II)

Statement-1: \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{NO}\right] \mathrm{SO}_{4}\) is paramagnetic. Statement- \(\mathbf{2}:\) The \(\mathrm{Fe}\) in \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{NO}\right] \mathrm{SO}_{4}\) has three unpaired electrons.

Write the IUPAC nomenclature of the given complex along with its hybridisation and structure. \(\mathrm{K}_{2}\left[\mathrm{Cr}(\mathrm{NO})\left(\mathrm{NH}_{3}\right)(\mathrm{CN})_{4}\right], \mu=1.73 \mathrm{BM}\)

A metal complex having composition \(\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2} \mathrm{Br}\) has been isolated in two forms \((A)\) and \((B)\). The form \((A)\) reacts with \(\mathrm{AgNO}_{3}\) to give a white precipitate readily soluble in dilute aqueous ammonia, whereas \((B)\) gives a pale yellow precipitate soluble in concentrated ammonia. Write the formula of \((A)\) and \((B)\) and state the hybridization of chromium in each. Calculate their magnetic moments (spin-only value).