CBSE Questions for Class 12 Engineering Chemistry Coordination Compounds Quiz 10 - MCQExams.com

Which of the following set of isomer isomerism is/are correct -
  • $$Cis - [Co(gly)_2Cl_2]^{-}$$ - optical isomerism
  • $$[Zn(NH_3)_3Cl]^{+}$$ - Geometrical isomerism
  • $$[Fe(H_2O)_6]Cl_3$$ - Hydrate isomerism
  • $$[Co(en)_2(NCS)_2]Cl$$ - Linkage isomerism
Which of the following chemical reaction(s) is (are) involved in the developing of photographic plate?
  • $$C_6H_4(OH)_2 + 2AgBr \rightarrow 2Ag + C_6H_4O_2 + 2HBr$$
  • $$AgBr + 2Na_2S_2O_3 \rightarrow Na_3[AgS_2O_3)_2] + NaBr$$
  • $$AgBr + 2NH_3(aq) \rightarrow [Ag(NH_3)_2]Br$$
  • $$2AgBr + Na_2S_2O_3 \rightarrow Ag_2S_2O_3 + 2NaBr$$
Which plays a major role in the formation of complex compound?
  • Transition metal
  • Lanthanides & Actinoides
  • Representative elements
  • p-Block elements
Which of the following is correct about
Tetraamminedithiocyanato- S-cobat(III) tris(oxalato)cobaltate(III) ?
  • Formula of the complex is $$[Co(NH_3)_4(SCN)_2][Co(ox)_3]$$
  • It is a chelating complex and show linkage isomerism
  • It shows optical isomerism
  • It show geometrical isomerism
How many of the following reactions/ statements are correct ?
(I) $$\displaystyle CrO_{5}$$ shows blue colour in organic solvent but in aq. solution blue colour fades because $$\displaystyle CrO_{5}$$ decomposes to $$\displaystyle Cr^{3+}$$ and $$\displaystyle O_{2}$$
(II) $$\displaystyle [Co(SCN)_{4}]^{2-}$$ shows blue colour in aq. solution 
(III) The pink ppt of $$\displaystyle Co(OH)_{2}$$ converts slowly to brown ppt $$\displaystyle Co(OH)_{3}$$ on exposure to air while green ppt of $$\displaystyle Ni(OH)_{2}$$ can be black $$\displaystyle Ni(OH)_{3}$$ with an oxidising reagent like NaOCI only
  • (i) only
  • (i) and (II) only
  • (iii) only
  • (I), (II) and (III) all are correct
In which of the following molecules/species, all following characteristics are found?
(a) Tetrahedral hybridisation.
(b) Hybridisation can be considered to have taken place with the help of empty orbital(s).
(c) All bond lengths are identical, i.e., all $$A - B$$ bond lengths are identical.
  • $$B_4H_6$$
  • $$Al_2Cl_6$$
  • $$BeCl_2\, (g)\, $$
  • $${BF_4}^-$$
Amongst $$Ni(Cl_4)^{2-}, { \left[ Ni{ \left( { H }_{ 2 }O \right)  }_{ 6 } \right]  }^{ 2+ }$$,$$\left[ Ni{ \left( P{ Ph }_{ 3 } \right)  }_{ 2 }{ Cl }_{ 2 } \right] $$,$$\left[ Ni{ (CO) }_{ 4 } \right] $$ and $${ \left[ Ni{ (CN) }_{ 4 } \right]  }^{ 2- }$$, the paramagnetic species are:
  • $${ \left[ Ni{ Cl }_{ 4 } \right] }^{ 2- },{ \left[ Ni{ \left( { H }_{ 2 }O \right) }_{ 6 } \right] }^{ 2+ },\left[ Ni{ \left( P{ Ph }_{ 3 } \right) }_{ 2 }{ Cl }_{ 2 } \right] $$
  • $$\left[ Ni{ (CO) }_{ 4 } \right] ,\left[ Ni{ \left( P{ Ph }_{ 3 } \right) }_{ 2 }{ Cl }_{ 2 } \right] ,{ \left[ Ni{ Cl }_{ 4 } \right] }^{ 2- }$$
  • $${ \left[ Ni{ (CN) }_{ 4 } \right] }^{ 2- },{ \left[ Ni{ \left( { H }_{ 2 }O \right) }_{ 6 } \right] }^{ 2+ },{ \left[ Ni{ Cl }_{ 4 } \right] }^{ 2- }$$
  • $$ \left[ Ni{ \left( P{ Ph }_{ 3 } \right) }_{ 2 }{ Cl }_{ 2 } \right] ,\left[ Ni{ (CO) }_{ 4 } \right] ,{ \left[ Ni{ (CN) }_{ 4 } \right] }^{ 2- }$$
Which of the following is diamagnetic in nature?
  • $$[Fe(CN)_{6}]^{3-}$$
  • $$NiCl_{4}^{2-}$$
  • $$[Ni(CO)_{4}]$$
  • $$[MnCl_{4}]^{2-}$$
Which of the following statements is incorrect?
  • In $$K_{3}[Fe(CN)_{6}]$$, the ligand has satisfied only the secondary valency of ferric ion
  • In $$K_{3}[Fe(CN)_{6}]$$, the ligand has satisfied both primary and secondary valencies of ferric ion
  • In $$K_{4}[Fe(CN)_{6}]$$ the ligand has satisfied both primary and secondary valencies of ferrous ion
  • In $$[Cu(NH_{3})_{4}]SO_{4}$$ the ligand has satisfied only the secondary valency of copper
What is the oxidation number of Pt in $$K[PtNH_3Cl_5]$$?
  • 0
  • +1
  • +2
  • +4
The hybridizations of atomic orbitals of nitrogen in $$NO_2^+ ,\ N{ O }_3^-$$ and $$NH_4^+$$ respectively are :
  • $$sp,\ sp^2 $$ and $$sp^3$$
  • $$sp^2,\ sp$$ and $$sp^3$$
  • $$sp,\ sp^3$$ and $$sp^2$$
  • $$sp^2,\ sp^3$$ and $$sp$$
What is hybridization?
  •  The mixing of two or more atomic orbitals to form new orbitals that describe the covalent bonding in molecules.
  • The mixing of electrons in the electron sea model to account for the number of bonds in a molecule.
  • The mixing of two or more atomic orbitals to form new orbitals that describe the location of electrons in atoms.
  • The mixing of two or more molecules
  • The mixing of two or more atoms to make a new compound or molecule.
What is the first thing you need to know to use the hybridization theory?
  • The number of valence electrons in the participating atoms.
  • The number of total electrons in the participating atoms.
  • Where the element lies on the periodic table.
  • How many of each molecule are being made.
  • The valence bond theory.
The energies of $$d_{xy}$$ and $$d^2_z$$ orbitals in octahedral and tetrahedral transition metal complexes are such that:
  • $$E(d_{xy})> E(d^2_z)^{xy}$$ in both tetrahedral and octahedral complexes
  • $$E(d_{xy})< E(d^2_z)$$ in both tetrahedral and octahedral complexes
  • $$E(d_{xy})>E(d^2_z)$$ in tetrahedral a but $$E(d_{xy})< E(d^2_z)$$ in octahedral complexes
  • $$E(d_{xy})< E(d^2_z)$$ in tetrahedral a but $$E(d_{xy})< E(d^2_z)$$ in octahedral complexes
Which one of the following is not correct in respect of hybridization of orbitals?
  • The orbitals presentt in valence shell only are hybridized
  • The orbitals undergoing hybridization have almost equal energy
  • Promotion of electron is not essential condition for hybridization
  • It is not always that only partially filled orbitals participate in hybridization in some cases even filled orbitals in valence shell take part
  • Pure atomic orbitals are more effective in forming stable bonds than hybrid orbitals
In addition reactions of aldehydes, the carbonyl carbon atom changes from:
  • $$sp^3$$ to $$sp^2$$
  • $$sp^2$$ to $$sp^3$$
  • $$sp$$ to $$sp^3$$
  • $$sp^3$$ to $$sp$$
The colour of the solution/precipitate obtained in the elemental analysis of an organic compound and the molecule/ion responsible for the colour are given below. Choose the incorrectly matched pair.
  • Prussian blue - $$Fe_{4}[Fe(CN)_{6}]_{3}]\cdot xH_{2}O$$
  • Black - $$PbS$$
  • Violet colour - $$[Fe(CN)_{5}NOS]^{4-}$$
  • Blood red colour - $$[Fe(SCN)^{2+}$$
  • Yellow - $$(NH_{4})_{2}MoO_{4}$$
Excess of silver nitrate solution is added to 100 mL of 0.01 M pentaaquachlorochromium (III) chloride solution. The mass of silver chloride obtained in grams is: (atomic mass of silver is 108).
  • $$287\times10^{-3}$$
  • $$28.7 \times10^{-3}$$
  • $$2\times10^{-3}$$
  • $$2870\times10^{-3}$$
A 0.001 mol sample of $$Co(NH_3)_5(NO_3)(SO_4)$$, is passed through a cation exchanger and the acid coming out of it requires 20 mL of 0.1 M NaOH for neutralisation. Hence, the complex is:
  • $$[Co(NH_3)_5(SO_4)NO_3]$$
  • $$[Co(NH_3)_5(NO_3)SO_4]$$
  • $$[Co(NH_3)_5NO_3SO_4]$$
  • None of these
For square planar complex of platinum  (II), $${ \left[ Pt\left( { NH }_{ 3 } \right) \left( Br \right) \left( Cl \right) py \right]  }^{ 0 }$$, how many isomeric forms are possible?
  • Two
  • Three
  • Four
  • Six




Out of given reaction which show change in hybridization of central atom__________.
  • $${ H }_{ 2 }{ BO }_{ 3 }$$ dissolve in water
  • $${ H }_{ 2 }{ SO }_{ 4 }$$ dissolve in water
  • $${ N }_{ 2 }{ O }_{ 5(g) }\longrightarrow { N }_{ 2 }{ O }_{ 5(s) }$$
  • $$P{ Br }_{ 5(g) }\longrightarrow P{ Br }_{ 5(s) }$$
  • $${ C }_{ 2 }{ H }_{ 6 }\xrightarrow [ bond\ cleavage\ of\ C-C\ bond ]{ Homolytic } $$
Which of the following primary and secondary valencies are not correctly marked against the compound?
  • $$[Cr(NH_3)_6]Cl_3,\, p= 3, \,s= 6$$
  • $$K_2[PtCl_4],\, p=2,\,s= 4$$
  • $$[Pt(NH_3)_2Cl_2],\, p= 0, \, s=4$$
  • $$[Cu(NH_3)_4]SO_4,\, p=4, \, s= 4$$
Hybridisation of carbon in $${ CH }_{ 2 }=CH-\overset { \oplus  }{ { CH }_{ 2 } }$$ is:
  • $${ sp }^{ 2 }$$
  • $$sp$$
  • $${ sp }^{ 3 }$$
  • all of these
The orbital angular momentum of a p-electron is given as :
Which one of the following complexes will have six isomers?
  • $$[Co(en)(NH_3)_2Cl_2]Cl$$
  • $$[Cr(H_2O)_4Cl_2]Cl$$
  • $$[Co(ox)_3]^{3-}$$
  • $$[Co(en)_2Br_2]Cl$$
Which complex possess facial isomer?
  • $$K\left[ Fe{ \left( { NH }_{ 3 } \right) }_{ 2 }{ \left( CN \right) }_{ 4 } \right] $$
  • $$\left[ Co{ \left( { NH }_{ 3 } \right) }_{ 3 }{ \left( { NO }_{ 2 } \right) }_{ 3 } \right] $$
  • $$\left[ Co{ \left( { NH }_{ 3 } \right) }_{ 3 }{ \left( CO \right) }_{ 3 } \right] Cl\quad $$
  • $$\left[ Ni{ \left( { H }_{ 2 }O \right) }_{ 4 }{ \left( { NH }_{ 3 } \right) }_{ 2 } \right] { SO }_{ 4 }$$
The hybridisation of each carbon in the following compound is:
$$\underset {i}{CH_{3}} - \underset {ii}{\overset {\overset {O}{||}}{C}} - \underset {iii}{CH_{2}} - \underset {iv}{CN}$$
  • $$sp^{3}\ sp^{2}\ sp^{3}\ sp$$
  • $$sp^{3}\ sp^{3}\ sp^{2}\ sp$$
  • $$sp^{3}\ sp\ sp^{3}\ sp^{2}$$
  • $$sp^{3}\ sp^{2}\ sp\ sp^{3}$$
Isostructural species are those which have the same shape and hybridisation. Among the given species, identify the isostructural pairs.
  • [$$NF_3$$ and $$BF_3$$]
  • [$$BF_4^-$$ and $$NH_4^+$$]
  • [$$BCl_3$$ and $$BrCl_3$$]
  • [$$NH_3$$ and $$NO^-_3$$]
The correct name of $$[Pt{({NH}_{3})}_{4}{Cl}_{2}][Pt{Cl}_{4}]$$ is:
  • Tetraammine dichloro platinum (IV) tetrachloro platinate(II)
  • Dicholoro tetra mmine platinum (IV) tetrachloro platinate (II)
  • Tetrachloro platinum (II) tetraammine platinate (IV)
  • Tetrachloro platinum (II) dichloro tetraamine platinate (IV)
Which of the following complex is useful in the dehydrogenation of alkanes?
  • $$[(Ph_{3}P)Rh Cl]$$
  • $$[(Ph_{3}P)_{3}Rh_{2} Cl]$$
  • $$[(Ph_{3}P)_{3}Rh Cl]$$
  • $$[(Ph_{3}P)_{3}Rh Cl_{2}]$$
The magnitude of CFSE (Crystal Field Splitting Energy, $$\Delta_0$$) can be related to the configuration of d - orbitals in a coordination entity as?
  • If $$\Delta_0$$ < P, the configuration is $$t_{2g}^{3}e_{g}^{1}$$ = weak filed ligand and high spin complex.
  • If $$\Delta_0$$ > P, the configuration is $$t_{2g}^{3}e_{g}^{1}$$ = strong filed ligand and high spin complex.
  • If $$\Delta_0$$ > P, the configuration is $$t_{2g}^{4}e_{g}^{0}$$ = strong filed ligand and high spin complex.
  • If $$\Delta_0=$$ P, the configuration is $$t_{2g}^{4}e_{g}^{0}$$ = strong filed ligand and high spin complex.
The sum of coordination number and oxidation number of the metal $$M$$ in the complex $$[M{(en)}_{2}({C}_{2}{O}_{4})]Cl$$ (where $$en$$ is ethylenediamine) is :
  • 7
  • 8
  • 9
  • 6
Aqueous solution of nickel sulphate on treating with pyridine and then adding a solution of sodium nitrate gives dark blue crystals of:
  • $$[Ni(py)_4]SO_4$$
  • $$[Ni(py)_2(NO_2)_2]$$
  • $$[Ni(py)_4(NO_2)_2]$$
  • $$[Ni(py)_3(NO_2)]_2SO_4$$
The terminal and bridged $$CO$$ ligands in the compound $$[Co_2(CO)_8]$$ are respectively:
  • 0, 2
  • 6, 1
  • 5, 2
  • 6, 2
The two isomers X and Y with the formula $$Cr(H_2O)_5ClBr_2$$ were taken for experiment on depression in freezing point. It was found that one mole of X gave depression corresponding to $$2$$ moles of particles and one mole of Y gave depression due to $$3$$ moles of particles. The structural formulae of X and Y respectively are:
  • $$[Cr(H_2O)_5Cl]Br_2$$; $$[Cr(H_2O)_4Br_2]Cl\cdot H_2O$$
  • $$[Cr(H_2O)_5Cl)]Br_2$$; $$[Cr(H_2O)_3ClBr]\cdot 2H_2O$$
  • $$[Cr(H_2O)_5Br]BrCl$$; $$[Cr(H_2O)_4ClBr]Br\cdot H_2O$$
  • $$[Cr(H_2O)_4Br_2]Cl\cdot H_2O$$; $$[Cr(H_2O)_5Cl]Br_2$$
Which of the following complex species is not expected to exhibit optical isomerism? 
  • $$[Co(en)(NH_3)_2Cl_2]^+$$
  • $$ [Co(en)_3]^{3+}$$
  • $$[Co(en)_2Cl_2]^+$$
  • $$ [Co(NH_3)_3Cl_3]$$
Highest conductivity is seen in:
  • K2 [PtCl6]
  • K4 [Fe(CN)6]
  • [Co (NH3)6] Cl3
  • [ Co( NH3)3 (NO2)3]
Select the incorrect order of stability:
  • $$[Ni{(dmg)}_{2}]> {[Ni{(en)}_{2}]}^{+2}$$
  • $${[Fe(edta)]}^{-2}> {[Fe(edta)]}^{-}$$
  • $${[Co{(Ox)}_{3}]}^{-3}> { \left[ { Co\left( { NH }_{ 3 } \right) }_{ 6 } \right] }^{ +3 }$$
  • $${ \left[ { Co\left( { NH }_{ 3 } \right) }_{ 6 } \right] }^{ +3 }>{ \left[ { Co\left( { H }_{ 2 }O \right) }_{ 6 } \right] }^{ +3 }$$
Which of the following complex ions will not show optical activity?
  • $$Pt[(Br)(Cl)(I)({NO}_{2})(Py){NH}_{3}]$$
  • cis-$$[Co{(en)}_{2}{Cl}_{2}]$$
  • $$[Co(en){({NH}_{3})}_{2}{Cl}_{2}]$$
  • $$[Cr{({NH}_{3})}_{4}{Cl}_{2}]$$
In the complex ion $$ML_{6}^{n+}, M^{n+}$$ has five d-electrons and $$L$$ is weak field ligand. According to crystal field theory the magnetic properties of the complex ion corresponds to how many unpaired electrons?
  • $$0$$
  • $$5$$
  • $$2$$
  • $$3$$
How many number of unpaired electrons is present in the complex Hg[Co(SCN)$$_4]$$?
  • One
  • Two
  • Three
  • Four
Primary and secondary valency of platinum in the complex $$[Pt(en)_{2}Cl_{2}]$$ are:
  • $$4,6$$
  • $$2,6$$
  • $$4,4$$
  • $$2,4$$
No. of $$5$$ membered ring in $${[(Ca(EDTA)]}^{-2}$$ is:
  • 5
  • 6
  • 7
  • 8
In the separation of $$Cu^{2+}$$ and $$Cd^{2+}$$ ions in the second group of qualitative analysis of cations, tetraamine copper (ll) sulphate and tetraamine cadmium (ll) sulphate react with $$KCN$$ to form the corresponding cyano complexes. 

Which of the following pairs of complexes and their relative stability enables the separation of $$Cu^{2+}$$ and $$Cd^{2+}$$?
  • $$K_2[Cu(CN)_4]$$ is less stable and $$K_2[Cd(CN)_4]$$ is more stable
  • $$K_3[Cu(CN)_4]$$ is more stable and $$K_2[Cd(CN)_4]$$ is less stable
  • $$K_3[Cu(CN)_4]$$ is less stable and $$K_2[Cd(CN)_4]$$ is more stable
  • $$K_2[Cu(CN)_4]$$ is more stable and $$K_2[Cd(CN)_4]$$ is less stable
$$CFSE$$ value of $$[Fe({ H }_{ 2 }O)_{ 5 }(NO)]{ SO }_{ 4 }$$ (brown ring complex) is :
  • $$-0.8\triangle \circ $$
  • $$-0.4\triangle \circ $$
  • $$-1.8\triangle \circ $$
  • $$-2.4\triangle \circ $$
Choose the incorrect order of stability:
  • $${ \left[ Cu{ \left( { NH }_{ 3 } \right) }_{ 4 } \right] }^{ 2+ }<{ \left[ Cu{ \left( en \right) }_{ 2 } \right] }^{ 2+ }<{ \left[ Cu\left( trien \right) \right] }^{ 2+ }$$
  • $${ \left[ Fe{ \left( { { H }_{ 2 }O }_{ } \right) }_{ 6 } \right] }^{ 3+ }<{ \left[ Fe{ \left( { NO }_{ 2 } \right) }_{ 6 } \right] }^{ 3- }<{ \left[ Fe{ \left( { NH }_{ 3 } \right) }_{ 6 } \right] }^{ 3+ }\quad $$
  • $${ \left[ Fe{ \left( { { H }_{ 2 }O }_{ } \right) }_{ 6 } \right] }^{ 2+ }<{ \left[ Fe{ \left( { { H }_{ 2 }O }_{ } \right) }_{ 6 } \right] }^{ 3+ }<{ \left[ Co{ \left( { NH }_{ 3 } \right) }_{ 6 } \right] }^{ 3+ }\quad $$
  • $${ \left[ Co{ \left( { { H }_{ 2 }O }_{ } \right) }_{ 6 } \right] }^{ 3+ }<{ \left[ Rh{ \left( { { H }_{ 2 }O }_{ } \right) }_{ 6 } \right] }^{ 2+ }<{ \left[ Ir{ \left( { { H }_{ 2 }O }_{ } \right) }_{ 6 } \right] }^{ 3+ }$$
Consider the following three halides:
(i) $${CH}_{3}-{CH}_{2}Cl$$
(ii) $${CH}_{2}=CH-Cl$$
(iii) $${C}_{6}{H}_{5}-Cl$$
Arrange $$C-Cl$$ bond lenght of these compounds in decreasing order:
  • $$i> ii> iii$$
  • $$i> iii> ii$$
  • $$iii> ii> i$$
  • $$ii> iii> i$$
Which of the following complex will give white precipitate with $$BaCl_2(aq)$$
  • $$[Co(NH_3)_4SO_4]NO_2$$
  • $$[Cr(NH_3)_5SO_4]Cl$$
  • $$[Cr(NH_3)_5Cl]SO_4$$
  • Both $$(B)$$ and $$(C)$$
Which of the following statements is/are correct?
  • $${NH}_{2}^{+}$$ shows $${sp}^{2}$$-hybridization where as $${NH}_{2}^{-}$$ shows $${sp}^{3}$$-hybrid
  • $$Al{(OH)}_{4}$$ has a regular tetrahedral geometry
  • $$sp^2 -$$ hybridized orbitals have equal $$s-$$ and $$p-$$ character 
  • Usually hybridized orbitals form  $$σ -$$ bonds
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