Chapter 20

In photography, hypo is used in the reduction of (a) Ag from AgBr (b) \(\mathrm{AgBr}\) into \(\mathrm{Ag}_{2} \mathrm{SO}_{4}\) (c) AgBr into soluble thiosulphate complex (d) both (b) and (c)

In the silver plating of copper, \(\mathrm{K}\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]\) is used instead of \(\mathrm{AgNO}_{3}\). The reason is (a) less availability of Ag+ ions, as Cu cannot displace Ag from \(\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-}\)ion (b) more voltage is required (c) a thin layer of \(\mathrm{Ag}\) is formed on \(\mathrm{Cu}\) (d) Ag ions are completely removed from solution

Among the following complex ions, the one with the highest paramagnetism is (a) \(\left[\mathrm{FeF}_{6}\right]^{2+}\) (b) \(\left[\mathrm{Cu}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) (c) \(\left[\mathrm{Zn}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) (d) \(\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}\)

What does the complex, tris-(ethylenediamine)cobalt (III) chloride exhibit? (a) cis-trans isomerism (b) fac-mer isomerism (c) linkage isomerism (d) optical isomerism

Which of the following are diamagnetic? (1) \(\mathrm{K}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\) (2) \(\mathrm{K}_{3}\left[\mathrm{Cr}(\mathrm{CN})_{6}\right]\) (3) \(\mathrm{K}_{3}\left[\mathrm{Co}(\mathrm{CN})_{6}\right]\) (4) \(\mathrm{K}_{2}\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]\) Select the correct answer using the codes given below: (a) 1 and 2 (b) 2,3 and 4 (c) 1,3 and 4 (d) 2 and 4

Which one of the following can show optical isomerism? (a) \(\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\) (b) \(\mathrm{Cr}\left[\left(\mathrm{NH}_{3}\right)\right] \mathrm{Cl}_{3}\) (c) \(\mathrm{FeSO}_{4} \cdot 7 \mathrm{H}_{2} \mathrm{O}\) (d) \(\mathrm{K}_{3}\left[\mathrm{Cr}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}\right]\)

Which of the following will give four isomers? (a) \(\left[\mathrm{Co}(\mathrm{en})_{2} \mathrm{Cl}_{2}\right] \mathrm{Br}\) (b) \(\left[\mathrm{Co}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\right] \mathrm{Cl}\) (c) \(\left[\mathrm{Co}\left(\mathrm{PPh}_{3}\right)_{2}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\right] \mathrm{Cl}\) (d) \(\left[\mathrm{Co}(\mathrm{en})_{3}\right] \mathrm{Cl}_{3}\)

Which one of the following high spin complexes has the largest CFSE (Crystal Field Stabilization Energy)? (a) \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2^{+}}\) (b) \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) (c) \(\left[\mathrm{Mn}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) (d) \(\left[\mathrm{Mn}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\)

Which one is the most likely structure of \(\mathrm{CrCl}_{3} \cdot 6 \mathrm{H}_{2} \mathrm{O}\) is \(1 / 3\) of total chlorine of the compound is precipitated by adding \(\mathrm{AgNO}_{3}\) to its aqueous solution? (a) \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{3} \mathrm{Cl}_{3}\right] .\left(\mathrm{H}_{2} \mathrm{O}\right)_{3}\) (b) \(\mathrm{CrCl}_{3}-6 \mathrm{H}_{2} \mathrm{O}\) (c) \(\left[\mathrm{CrCl}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5}\right] \mathrm{Cl}_{2} \cdot \mathrm{H}_{2} \mathrm{O}\) (d) \(\left[\mathrm{CrCl}_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}\right] . \mathrm{Cl} .{ }_{2} \mathrm{H}_{2} \mathrm{O}\)

The complex salt having the molecular composition \(\left[\mathrm{Co}\left(\mathrm{NO}_{2}\right)(\mathrm{SCN})(\mathrm{en})\right] \mathrm{Br}\) exhibits (a) linkage isomerism only (b) ionization isomerism only (c) cis-trans isomerism only (d) all of these

Isomerism shown by octahedral complex \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4}\right.\) \(\left.\mathrm{Br}_{2}\right] \mathrm{Cl}\) are (a) geometrical and ionization (b) optical and ionization (c) geometrical and optical (d) only geometrical

The complex ion which has no d electrons in the central metal atom is (Atomic number \(\mathrm{Cr}=24\), \(\mathrm{Mn}=25, \mathrm{Fe}=26, \mathrm{Co}=27)\) (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) \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\)

Which of the following statement is incorrect? (a) in \(\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\), the ligand has satisfied both primary and secondary valencies of ferric ion (b) in \(\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\) the ligand has satisfied only the secondary valency of ferric ion (c) in \(\mathrm{K}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\) the ligand has satisfied both primary and secondary valencies of ferrous ion (d) in \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{SO}_{4}\), the ligand has satisfied only the secondary valency of copper

The number of chloride ions produced by the complex tetraamminechloroplatinum(IV) chloride in an aqueous solution is (a) 1 (b) 2 (c) 3 (d) 4

While \(\mathrm{Ti}^{3+}, \mathrm{V}^{3+}, \mathrm{Fe}^{3+}\) and \(\mathrm{Co}^{2+}\) can afford a large number of tetrahedral complexes, \(\mathrm{Cr}^{3+}\) never does this, the reason being (a) crystal field stabilisation energy in octahedral vis-à-vis tetrahedral \(\mathrm{Cr}^{3+}\) system plays the deciding role (b) \(\mathrm{Cr}^{3^{+}}\)forces high crystal field splitting with a varieties of ligands (c) electronegativity of \(\mathrm{Cr}^{3+}\) is the largest among these trivalent 3 d-metals and so chromium prefers to be associated with as many ligands as its radius permits (d) both (b) and (c)

The blue colour obtained in the Lassaigne's test is due to formation of the compound (a) \(\mathrm{Fe}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]_{3}\) (b) \(\mathrm{Fe}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\) (c) \(\mathrm{Na}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\) (d) \(\mathrm{Fe}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]_{4}\)

The formula of tetrachlorodiammineplatinum(IV), is (a) \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2}\right] \mathrm{Cl}_{4}\) (b) \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{4}\right]\) (c) \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\right] \mathrm{Cl}_{2}\) (d) \(\mathrm{K}_{4}\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{4}\right]\)

Predict which is the strongest ligand from the stability constant (hypothetical values) given below? (a) \(\mathrm{Cu}^{2^{+}}+4 \mathrm{H}_{2} \mathrm{O} \rightleftharpoons\left[\mathrm{Cu}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}\right]^{2^{+}}, \mathrm{K}=9.5 \times 10^{8}\) (b) \(\mathrm{Cu}^{2+}+2 \mathrm{en} \rightleftharpoons\left[\mathrm{Cu}(\mathrm{en})_{2}\right]^{2^{+}}, \quad \mathrm{K}=3.0 \times 10^{15}\) (c) \(\mathrm{Cu}^{2+}+4 \mathrm{CN} \rightleftharpoons\left[\mathrm{Cu}(\mathrm{CN})_{4}\right]^{2}, \quad \mathrm{~K}=2.0 \times 10^{27}\) (d) \(\mathrm{Cu}^{2+}+4 \mathrm{NH}_{3} \rightleftharpoons\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2^{+}}, \mathrm{K}=4.5 \times 10^{11}\)

In which of the following pairs, the EAN of the central metal atom is not the same? (a) \(\left[\mathrm{FeF}_{6}\right]^{3+}\) and \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}\) (b) \(\left[\mathrm{Fe}\left(\mathrm{CN}_{6}\right)\right]^{3-}\) and \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4}\) (c) \(\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}\) and \(\left[\mathrm{Cr}(\mathrm{CN})_{6}\right]^{3-}\) (d) \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]\) and \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2}\)

Name the metal \(\mathrm{M}\) which is extracted on the basis of following reactions: \(4 \mathrm{M}+8 \mathrm{CN}+2 \mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2} \longrightarrow 4[\mathrm{M}(\mathrm{CN})]^{-1}+4 \mathrm{OH}^{-}\) \(2\left[\mathrm{M}(\mathrm{CN})_{2}\right]^{-1}+\mathrm{Zn} \longrightarrow\left[\mathrm{Zn}(\mathrm{CN})_{4}\right]^{2^{-}}+2 \mathrm{M}\) (a) \(\mathrm{Ag}\) (b) \(\mathrm{Cu}\) (c) \(\mathrm{Hg}\) (d) \(\mathrm{Ni}\)

Which of the following complex ions will not show optical activity? (a) \(\left[\mathrm{Co}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\right]^{+}\) (b) \(\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right]^{+}\) (c) \(\left[\mathrm{Pt}(\mathrm{Br})(\mathrm{Cl})\right.\) (I) \(\left(\mathrm{NO}_{2}\right)\) (Py) \(\left.\mathrm{NH}_{3}\right]\) (d) \(\operatorname{cis}-\left[\mathrm{Co}(\mathrm{en}), \mathrm{Cl}_{2}\right]^{+}\)

The number of ions produced from one molecule of \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Br}\right] \mathrm{Br}_{3}\) in the aqueous solution will be (a) 4 (b) 5 (c) 6 (d) 7

The stability constants of the complexes formed by a metal ions \(\left(\mathrm{M}^{2^{+}}\right)\)with \(\mathrm{NH}_{3}, \mathrm{CN}^{-}, \mathrm{H}_{2} \mathrm{O}\) and 'en' are of the order of \(10^{11}, 10^{27}, 10^{15}\) and \(10^{8}\) respectively. Then (en = ethylene diamine) (a) en is the strongest ligand (b) these values cannot predict the strength of the ligand (c) \(\mathrm{CN}^{-}\)is the strongest ligand (d) all ligands are equally strong

For a complex \(\mathrm{MA}_{3} \mathrm{~B}_{3}\) possessing a trigonal prismatic geometry, the number of possible isomers are (a) 3 (b) 4 (c) 5 (d) 6

The coordination number and oxidation number of \(\mathrm{M}\) in the compound \(\left[\mathrm{M}\left(\mathrm{SO}_{4}\right)\left(\mathrm{NH}_{3}\right)_{5}\right]\) will be (a) 6 and 3 (b) 2 and 6 (c) 6 and 2 (d) 3 and 6

The number of isomers possible for complex \(\mathrm{K}_{2}[\mathrm{Pd}\) \(\left.\mathrm{Cl} \mathrm{Br}(\mathrm{SCN})_{2}\right]\) is (a) 1 (b) 2 (c) 3 (d) 4

Which of the following will have three stereo-isomeric forms? (1) \(\left[\mathrm{Cr}\left(\mathrm{NO}_{3}\right)_{3}\left(\mathrm{NH}_{3}\right)_{3}\right]\) (2) \(\mathrm{K}_{3}\left[\mathrm{Co}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}\right]\) (3) \(\mathrm{K}_{3}\left[\mathrm{Co}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{2} \mathrm{Cl}_{2}\right]\) (4) \(\left[\mathrm{Co}\left(\mathrm{en}_{2}\right) \mathrm{ClBr}\right]\) (Here, en = ethylene diamine) (a) 1 and 2 (b) 1 and 3 (c) 1 and 4 (d) 3 and 4

The number of unpaired electrons in the complex ion \(\left[\mathrm{CoF}_{6}\right]^{3}\) is (Atomic number of \(\mathrm{Co}=27\) ) (a) 4 (b) zero (c) 2 (d) 3

In the silver plating of copper, \(\mathrm{K}\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]\) is used instead of \(\mathrm{AgNO}_{3} .\) The reason is (a) less availability of \(\mathrm{Ag}^{+}\)ions, as \(\mathrm{Cu}\) cannot displace Ag from \(\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-}\)ion (b) more voltage is required (c) a thin layer of \(\mathrm{Ag}\) is formed on \(\mathrm{Cu}\) (d) Ag ions are completely removed from solution

Which of the following will exhibit geometrical isomerism? (M stands for a metal, and a and \(\mathrm{b}\) are achiral ligands, (1) \(\mathrm{Ma}_{2} \mathrm{~b}_{2}\) (2) \(\mathrm{Ma}_{4} \mathrm{~b}_{2}\) (3) \(\mathrm{Ma}_{5} \mathrm{~b}\) (4) \(\mathrm{Ma}_{6}\) (a) 1 and 2 (b) 2 and 3 (c) 1 and 3 (d) 2 and 4

When concentrated \(\mathrm{HCl}\) is added to a solution of \(\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2^{+}}\)ion, an intense blue colour develops due to the formation of which one of the following? (a) \(\left[\mathrm{CoCl}_{4}\right]^{2}\) (b) \(\left[\mathrm{CoCl}_{6}\right]^{4-}\) (c) \(\left[\mathrm{CoCl}\left(\mathrm{H}_{2} \mathrm{O}\right)_{3}\right]^{+}\) (d) \(\left[\mathrm{CoCl}_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}\right]\)

Which one of the following complexes is diamagnetic in nature? (1) \(\mathrm{K}_{2}\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]\) (2) \(\left[\mathrm{Ni}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]\left(\mathrm{NO}_{3}\right)_{2}\) (3) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{3}\) (4) \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{Cl}_{2}\) Select the correct answer (a) 1 and 2 (b) 2 and 3 (c) 1,2 and 4 (d) 1,3 and 4

The oxidation number of \(\mathrm{Fe}\) in \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4}, \mathrm{Cr}\) in \(\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{3}\left(\mathrm{NO}_{2}\right)_{3}\right]\) and \(\mathrm{Ni}\) in \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]\) are respectively (a) \(0,+3,+2\) (b) \(+3,+3,0\) (c) \(+3,0,+3\) (d) \(+2,+3,0\)

The coordination number of \(\mathrm{Ni}^{2+}\) is 4 . \(\mathrm{NiCl}_{2}+\mathrm{KCN}\) (excess) \(\longrightarrow \mathrm{A}\) (Cyano complex) \(\mathrm{NiCl}_{2}+\) conc. HCl (excess) \(\longrightarrow \mathrm{B}\) (chloro complex) The IUPAC name of \(\mathrm{A}\) and \(\mathrm{B}\) are (a) potassiumtetracyanonickelate(II), potassiumtetrachloronickelate (II) (b) tetracyanopotassiumnickelate (II), tetrachloropota-ssiumnickelate(II) (c) tetracyanonickel(II), tetrachloronickel(II) (d) potassium tetracyanonickel(II), potassium tetra-chloronickel(II)

In the complex \(\left[\mathrm{Cu}(\mathrm{CN})_{4}\right]^{3-}\) the hybridization state, oxidation state and number of unpaired electrons are (a) \(\mathrm{dsp}^{2},+1,1\) (b) sp \(^{3},+1\), zero (c) \(\mathrm{sp}^{3},+2,1\) (d) \(\mathrm{dsp}^{2},+2\), zero

Consider the following complex \(\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{CO}_{3}\right] \mathrm{ClO}_{4}\) The coordination number, oxidation number, number of d electrons and number of unpaired d electrons on the metal are, respectively (a) \(6,3,6,0\) (b) \(6,3,6,3\) (c) \(6,0,6,3\) (d) \(6,2,6,3\)

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

Which of the following pairs of isomers and types of isomerism are correctly matched? (1) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5}\left(\mathrm{NO}_{2}\right)\right] \mathrm{Cl}_{2}\) and \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5}(\mathrm{ONO})\right] \mathrm{Cl}_{2}\) Linkage isomers (2) \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]\left[\mathrm{PtCl}_{4}\right]\) and \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4}\right]\left[\mathrm{CuCl}_{4}\right]\) Co-ordinationIsomers (3) \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right] \mathrm{Br}_{2}\) and \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4} \quad \mathrm{Br}_{2}\right] \mathrm{Cl}_{2}\) Ionisation Isomers Select the correct answer using the codes given below: (a) 1 and 2 (b) 2 and 3 (c) 1 and 3 (d) 1,2 and 3

The correct order of magnetic moment (spin only values in BM) among the following is (a) \(\left[\mathrm{MnCl}_{4}\right]^{2}>\left[\mathrm{CoCl}_{4}\right]^{2-}>\mathrm{Fe}\left(\mathrm{CN}_{6}\right)^{4}\) (b) \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4}>\left[\mathrm{MnCl}_{4}\right]^{2-}>\left[\mathrm{CoCl}_{4}\right]^{2-}\) (c) \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}>\left[\mathrm{CoCl}_{4}\right]^{2-}>\left[\mathrm{MnCl}_{4}\right]^{2-}\) (d) \(\left[\mathrm{MnCl}_{4}\right]^{2}>\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4^{-}}>\left[\mathrm{CoCl}_{4}\right]^{2}\) (Atomic number of \(\mathrm{Mn}=25, \mathrm{Fe}=26, \mathrm{Co}=27, \mathrm{Ni}=28\) )

Match the list I and II, pick the correct matching from the codes given below List I List II (a) \(\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]\) 1\. square planar and \(1.73 \mathrm{BM}\) (b) \(\left[\mathrm{Cu}\left(\mathrm{CN}_{4}\right)\right]^{3}\) 2\. linear and zero (c) \(\left[\mathrm{Cu}(\mathrm{CN})_{6}\right]^{3-}\) 3\. octahedral and zero (d) \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}\) 4\. tetrahedral and zero (e) \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4} \quad\) 5. octahedral and \(1.73 \mathrm{BM}\) (a) \(a-4, b-2, c-5, d-3, e-1\) (b) \(a-4, b-5, c-2, d-1, e-3\) (c) a-2, b-4, c-5, d-1, e-3 (d) a-5, b-4, c-1, d-3, e-2

In the complexes \(\left[\mathrm{Cr}(\mathrm{CN})_{6}\right]^{3},\left[\mathrm{CuCl}_{4}\right]^{2-},\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+} .\) The number of unpaired electrons are respectively (a) 1,3 and 0 (b) 3,2 and 1 (c) 3,2 and 0 (d) 3,1 and 0

Which of the following are paramagnetic tetrahedral species? (a) \(\left[\mathrm{FeCl}_{4}\right]^{-}\) (b) \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\) (c) \(\left[\mathrm{NiCl}_{4}\right]^{2-}\) (d) \(\left[\mathrm{Zn}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}\)

Which of the following are diamagnetic? (a) \(\left[\mathrm{Ni}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) (b) \(\left[\mathrm{Zn}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}\) (c) \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\) (d) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}\)

The proposed complex with the nomenclature chlorodiaquatriammine cobalt (III) chloride can be represented wrongly as (a) \(\left[\mathrm{CoCl}\left(\mathrm{NH}_{3}\right)_{3}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right] \mathrm{Cl}_{2}\) (b) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{3}\left(\mathrm{H}_{2} \mathrm{O}\right) \mathrm{Cl}_{3}\right]\) (c) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{3}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2} \mathrm{Cl}_{2}\right] \mathrm{Cl}\) (d) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{3}\left(\mathrm{H}_{2} \mathrm{O}\right)_{3}\right] \mathrm{Cl}_{3}\)

Which of the following statements is/are correct regarding metal carbonyl? (a) \(\operatorname{In} \mathrm{Fe}_{3}(\mathrm{CO})_{12}\) no. of \(\mathrm{Fe}-\mathrm{Fe}\) bonds are 3 (b) In \(\mathrm{Mn}_{2}(\mathrm{CO})_{10}\) bond order of \(\mathrm{Mn}-\mathrm{Mn}\) is 0 (c) \(\mathrm{Fe}(\mathrm{CO})_{5}\) is diamagnetic (d) In \(\mathrm{Fe}_{2}(\mathrm{CO})_{4}\) all bond length are same

For the complex \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}\) (a) Shape is tetrahedral (b) Hybridization state of central ion is \(\mathrm{sp}^{3}\) (c) Effective atomic number of central ion is 35 (d) Number of unpaired electrons present in the central ion is 1

Identify the coordination compounds (a) \(\mathrm{FeSO}_{4} \cdot\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4} \cdot 6 \mathrm{H}_{2} \mathrm{O}\) (b) \(\mathrm{Fe}(\mathrm{CN})_{2} \cdot 4 \mathrm{KCN}\) (c) \(\mathrm{KCl} \cdot \mathrm{MgCl}_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O}\) (d) \(\mathrm{CuSO}_{4} \cdot 4 \mathrm{NH}_{3}\)

The main draw back of valence bond theory is/are (a) It cannot explain magnetic properties of co-ordination compounds (b) It cannot distinguish between high spin and low spin complex (c) It does not provide an answer to the origin of characteristic colours of complex ions (d) It is a qualitative approach

The coordination compound is a complex substance which contains a central metal atom or ion surrounded by oppositely charged ions or neutral molecules. These compounds exhibit structural as well as stereoisomerism. Hybridisation theory explains the geometry of the complex. Crystal field theory explains the colour of complexes and magnetic properties. Which one of the following does not show optical activity? (a) \(\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right]^{+}\) (b) \(\left[\mathrm{Pt}(\mathrm{Br})(\mathrm{Cl})(\mathrm{I})\left(\mathrm{NO}_{2}\right)\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{~N}\right)\left(\mathrm{NH}_{3}\right)\right]^{-}\) (c) \(\operatorname{Cis}\left[\mathrm{Co}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\right]^{+}\) (d) \(\operatorname{Cis}\left[\mathrm{Co}(\mathrm{en})_{2} \mathrm{Cl}_{2}\right]^{+}\)

The coordination compound is a complex substance which contains a central metal atom or ion surrounded by oppositely charged ions or neutral molecules. These compounds exhibit structural as well as stereoisomerism. Hybridisation theory explains the geometry of the complex. Crystal field theory explains the colour of complexes and magnetic properties. Identify the correct statement (a) \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\) is tetrahedral and paramagnetic (b) \(\left[\mathrm{NiCl}_{4}\right]^{2-}\) is square planar and paramagnetic (c) \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]\) is square planar and paramagnetic (d) \(\left[\mathrm{Cu}(\mathrm{CN})_{4}\right]^{3-}\) is tetrahedral and diamagnetic