CBSE Questions for Class 12 Engineering Chemistry Coordination Compounds Quiz 11 - MCQExams.com

Hybridization of central atoms in the molecules $$N(CH_3)_3$$ and $$N(SiH_3)_3$$ respectively are:
  • $$sp^2$$ nad $$sp^2$$
  • $$sp^3$$ and $$sp^3$$
  • $$sp^2$$ and $$sp^3$$
  • $$sp^3$$ and $$sp^2$$
Hydrogen peroxide oxidises $$\left[ Fe\left( CN \right) _{ 6 } \right] ^{ 4- }$$ to $$\left[ Fe\left( CN \right) _{ 6 } \right] ^{ 3- }$$ in acidic medium but reduces $$\left[ Fe\left( CN \right) _{ 6 } \right] ^{ 3- }$$ to $$\left[ Fe\left( CN \right) _{ 6 } \right] ^{ 4- }$$ in alkaline medium. The other products formed are, respectively:
  • $${ H }_{ 2 }O$$ and $$({ H }_{ 2 }O+{ O }_{ 2 })$$
  • $${ H }_{ 2 }O$$ and $$({ H }_{ 2 }O+{ O }{ H }^{ - })$$
  • $$({ H }_{ 2 }O+{ O }_{ 2 })$$ and $${ H }_{ 2 }O$$
  • None of these
Which of the following a bidentate mono iron ligands?
  • Acetyl Acetoneate
  • Oxalate ion
  • Both of these
  • None of the above
In quantitative analysis of second group in lab., $$ H _ { 2 } S $$ gas is passed in acidic medium for ppt. When $$ \mathrm { Cu } ^ { + 2 } $$ and $$ \mathrm { Cd } ^ { + 2 } $$ react with $$ \mathrm { KCN } $$, then in which of the following condition, ppt will not be formed due to relative stability.
  • $$ K _ { 2 } \left[ \mathrm { Cu } ( \mathrm { CN } ) _ { 4 } \right] \text { - More stable } \mathrm { K } _ { 2 } \left[ \mathrm { Cd } ( \mathrm { CN } ) _ { 4 } \right] - \text { Less stable } $$
  • $$ K _ { 2 } \left[ \mathrm { Cu } ( \mathrm { CN } ) _ { 4 } \right] - \text { Less stable } \quad \mathrm { K } _ { 2 } \left[ \mathrm { Cd } ( \mathrm { CN } ) _ { 4 } \right] - \text { More stable } $$
  • $$ K _ { j } \left[ \mathrm { Cu } ( \mathrm { CN } ) _ { 4 } \right] \text { - More stable } \quad \mathrm { K } _ { 2 } \left[ \mathrm { Cd } ( \mathrm { CN } ) _ { 4 } \right] - \text { Less stable } $$
  • $$ \mathrm { K } _ { \mathrm { J } } \left[ \mathrm { Cu } ( \mathrm { CN } ) _ { 4 } \right] - \text { Less stable } \quad \mathrm { K } _ { \mathrm { J } } \left[ \mathrm { Cd } ( \mathrm { CN } ) _ { 4 } \right] - \text { More stable } $$
Select the correct statement
  • $$ (C{ H }_{ 3 }{ ) }_{ 3 }\bar { C } $$ is pyramidal while $$\bar { C } (CN{ ) }_{ 3 }$$ is planar
  • $$ \bar { C } (CN{ ) }_{ 3 }$$ is Pyramidal while $$\bar { C } (C{ H }_{ 3 }{ ) }_{ 3 }$$ is plannar
  • both $$ \bar { C } (CN{ ) }_{ 3 }$$and $$\bar { C } (C{ H }_{ 3 }{ ) }_{ 3 }$$ are planar
  • both $$ \bar { C } (CN{ ) }_{ 3 }$$and $$ \bar { C } (C{ H }_{ 3 }{ ) }_{ 3 }$$ are Pyramidal
$${ \left[ Ni{ (CN) }_{ 4 } \right]  }^{ 2- }$$ is isostructural with:
  • $${ HeF }_{ 4 }$$
  • $${ SiF }_{ 4 }$$
  • $${ SF }_{ 4 }$$
  • $$\left[ Pt{ (NH) }_{ 4 } \right] { Cl }_{ 2 }$$
The incorrect statement regarding $$ O(SiH_3)_2$$ and $$OCl_2$$ molecule is/are : 
  • The strength of back bonding is more in $$O(SiH_3)_2$$ molecule than $$OCl_2$$ molecule
  • $$Si - \hat{O} - Si$$ bond angle in $$O(SiH_3)_2$$ is greater than $$Cl - \hat{O} - Cl$$ bond angle in $$OCl_2$$
  • The nature of back bond in both molecules is $$2P_{\pi} - 3d_{\pi}$$
  • Hybridisation of central O-atom in both molecules is same
The conjugate base of $$[Al(H_2O)_3(OH)_3]$$ is
  • $$[Al(H_2O)_3(OH)_2]^+$$
  • $$[Al(H_2O)_3(OH)_2]^-$$
  • $$[Al(H_2O)_3(OH)_3]^-$$
  • $$[Al(H_2O)_2(OH)_4]^-$$
The correct order of increasing s-character (in percentage) in the hybrid orbitals of following molecules and ions is 

(I) $$CO_{3}^{2-}$$          (II) $$XeF_{4}$$     (III) $$I_{3}^{-}$$ (IV) $$NCl_{3}$$    (V) $$BeCl_{2}$$
  • $$II < III < IV < I < V$$
  • $$II < III < IV < V < I$$
  • $$III < II < I < V < IV$$
  • $$II < IV < III < I < V$$
Identify the correct statement(s) regarding $$[Cr(en)_{2}]^{+}$$ and $$[Co(C_{2}O_{4})_{2}(NH_{3})_{2}]$$ complex ions:
(i) Both are chelate complexes
(ii) Both have octahedral geometry
(iii) Both are low spin complexes
(iv) Both contain metal-carbon bond i.e. , they are organometallic compounds
  • I,III,IV
  • I,II
  • II,III
  • I,II,III
Which of the following is not correctly matched ? 
  • $$[Fe (CN)_6]^{3-} d^2 sp^3$$, paramagnetic
  • $$[Ni (CO)_4] -sp^3$$, diamagnetic
  • $$[Fe(en)_3]^{+3} - sp^3 d^2$$, paramagnetic
  • $$[FeCl_2 (H_2O)_2] sp^3$$, paramagnetic
In $$[Co(NH_3)_6]Cl_3$$, the number of covalent bonds is
  • 3
  • 6
  • 9
  • 18
which has the maximum conductivity in thier 0.1M solution?
  • A) $$\left[ Co{ (NH }_{ 3 })_{ 3 }{ Cl }_{ 3 } \right] $$
  • B) $$\left[ Co({ NH }_{ 3 })_{ 4 }Cl \right] { Cl }_{ 2 }$$
  • C) $$\left[ Co({ NH }_{ 3 })_{ 5 }Cl \right] { Cl }_{ 2 }$$
  • D) $$\left[ Co({ NH }_{ 3 })_{ 6 } \right] { Cl }_{ 3 }$$
Which of these statements about $$[Co(CN)_{6}]^{3-}$$ is true?
  • $$[Co(CN)_{6}]^{3-}$$ has zero unpaired electrons and will be in a low-spin configuration.
  • $$[Co(CN)_{6}]^{3-}$$ has four unpaired electrons and will be in a high-spin configuration.
  • $$[Co(CN)_{6}]^{3-}$$ has zero unpaired electrons and will be in a high-spin configuration.
  • $$[Co(CN)_{6}]^{3-}$$ has four unpaired electrons and will be in a low-spin configuration.
Total number of possible isomers of $$\left[ Cu({ NH }_{ 3 })_{ 4 } \right] \left[ { PtCl }_{ 4 } \right]$$ is:
  • 3
  • 4
  • 5
  • 6
Given the molecular formula of the hexa coordinated complexes (A) $${ CoCl }_{ 3 }.{ 6NH }_{ 3 }$$ (B) $${ CoCl }_{ 3 }.{ 5NH }_{ 3 }$$ (C) $${ CoCl }_{ 3 }.{ 4NH }_{ 3 }$$. If the number of coordinated $${ NH }_{ 3 }$$ molecules in $$A, B$$ and $$C$$ respectively are $$6, 5$$ and $$4$$, primary valency in $$(A), (B)$$ and $$(C)$$ are
  • $$0, 1, 2$$
  • $$3, 2, 1$$
  • $$6, 5, 4$$
  • $$3, 3, 3$$
$$[Fe(H_{2}O)_{6}]^{+2}$$ has a crystal field splitting energy value of $$10,400\ cm^{-1}$$ and a pairing energy value of $$17,600\ cm^{-1}$$. Then, the compound is:
  • a low spin complex
  • paramagnetic in nature
  • diamagnetic in nature
  • none of these
In the co-ordination compound $$Na_{4}$$$$[Fe)CN)_{5}NOS]$$ oxidation state of $$Fe$$ is:
  • +1
  • +2
  • +3
  • +4
Which isomer of $$CrCl_{3} . 6H_{2}O$$ is dark green in colour and forms one mole of $$AgCl$$ with excess of $$AgNO_{3}$$ solution ?
  • $$[Cr(H_{2}O)_{6}]Cl_{3}$$
  • $$[Cr(H_{2}O)_{5}Cl] Cl_{2} . H_{2}O$$
  • $$[Cr(H_{2}O)_{4}Cl_{2}] Cl . 2H_{2}O$$
  • $$[Cr(H_{2}O)_{3}Cl_{3}]3H_{2}O$$
The complex ion having minimum wavelength of absorption in the visible region is:
  • $$[Co(NH_3)_6]^{3+}$$
  • $$[CoCl(NH_3)_5]^{2+}$$
  • $$ Cis-[CoCl_2(NH_3)_4]^{+}$$
  • $$Trans-[CoCl_2(NH_3)_4]^{+}$$
Select the incorrect statement.
  • Crystal field stabilisation energy of $$d^2$$ configuration in an octahedral complex of a weak field ligand is $$-0.8\triangle _o$$.
  • $$[MnF_6]^{4-}$$ is an example of a coordination compound having a weak field ligand and $$d^5$$ configuration.
  • Effective atomic number of Pt in $$[PtCl_6]^{2-}$$ is 84.
  • Geometrical isomerism is shown by $$[Pt(NH_3)_4Cl_2]$$.
The number of unpaired electron in complex $$[Cr(NO_{2})_{3}(NH_{3})_{3}]$$ is
  • 2
  • 3
  • 1
  • 0
Nickel $$(Z=28)$$ combines with a uni negative monodentate ligand $$X^{-}$$ to form a paramagnetic complex, $$[NiX_{4}]^{2-}$$. The number of unpaired electrons in the nickel and geometry of this complexion are, respectively:
  • One, tetrahedral
  • Two, tetrahedral
  • One, square planar
  • None of these
The number of chloride ions which would be precipitated, when $$CrCl_{3}.4NH_{3}$$ is treated with silver nitrate solution:
  • 3
  • 2
  • 1
  • 0
Both geometrical and optical isomerism was shown by
  • [Pt(NH$$_3$$)$$_2$$Cl$$_2$$]
  • [Pt(NH$$_3$$)$$_4$$Cl$$_2$$]
  • [Pt(en)$$_2$$Cl$$_2$$]
  • [Pt(en)$$_3$$Cl$$_2$$]
The oxidation state of $$Cr$$ in $$[Cr(NH_{3})_{4} Cl_{2}]^{+}$$ is:
  • +2
  • +3
  • 0
  • +1
$$LiH + \underline {B}_2H_6 \rightarrow 2Li \underline{B}H_4$$

Find the change in hybridization of the underlined atom.
  • $$sp^2 \rightarrow sp^3$$
  • $$sp^3 \rightarrow sp^2$$
  • $$sp \rightarrow sp^3$$
  • None
For the following two complexes 
$$A:[NiCl_6]^{4-}$$ and $$[NiCl_4]^{2-}$$ the ratio of CFSE will be nearly:
  • $$\dfrac{3}{2}$$
  • $$\dfrac{4}{9}$$
  • $$\dfrac{9}{4}$$
  • $$\dfrac{27}{8}$$
Correct formula of potassium ferrocyanide is
  • $${ K }_{ 4 }\left[ { Fe(CN) }_{ 6 } \right] $$
  • $${ K }_{ 2 }\left[ { Fe(CN) }_{ 6 } \right]. { H }_{ 2 }O$$
  • $${ K }_{ 3 }\left[ { Fe(CN) }_{ 6 } \right] $$
  • None of these
Number of isomers of $$[Pt(NH_{3})_{4}]$$$$[CuCl_{4}]$$ complex are
  • $$2$$
  • $$3$$
  • $$4$$
  • $$5$$
Copper sulphate when dissolved in excess of $$KCN$$ gives
  • $$Cu(CN)_2$$
  • $$[Cu(CN)_4]^{3-}$$
  • $$[Cu(CN)_4]^{2-}$$
  • $$CuCN$$
The number of moles of $$BaSO_{4}$$ precipitate obtained, when reagent $$[Cu(NH_{3})_{4}]SO_{4}$$ is treated with an excess of $$BaCl_{2}$$:-
  • 2
  • 0
  • 1
  • None of these
Which of the following complex has no optical isomers, where $$a,b,c$$ are monodentate ligands and $$(AA)$$ is symmetrical bidentate ligand:
  • $$[Ma_{2}b_{2}]$$
  • $$[Ma_{2}b_{2}c_{2}]$$
  • $$[M(AA)_{2}a_{2}]$$
  • $$[M(AA)_{2}ab]$$
On adding $$AgNO_3$$ solution to a solution of $$[Pt(NH_3)_3Cl_3]Cl,$$ the percentage of total chloride ion precipitate is:
  • 100
  • 75
  • 50
  • 25
The hybridization of Fe in $$K_4[Fe(CN)_6]$$ is: 
  • $$sp^3$$
  • $$sp^3d^2$$
  • $$d^2$$ $$sp^3$$
  • $$dsp^2$$
The species in which $$(n-1)d_{{x^2}-{y^2}}$$ orbital take part in hybridization?
  • $$PCl_5$$
  • $$[NiCl_4]^{2-}$$
  • $$[Cr(NH_3)_6]^{3+}$$
  • $$[Ni(CO)_4]$$
If the bidentate ligand $$L^{2-}$$ in $$[ML_2]^{n - 4}$$ is replaced by neutral monodentate ligand $$X$$, the formula of the resulting complex ion is:
  • $$[MX_4]^{n+}$$
  • $$[MX_2]^{n+}$$
  • $$[MX_2]^{n-1}$$
  • $$[MX_4]^{2+}$$
Iron from $$Hb$$ is stored in liver in the form of:
  • Ferric
  • Ferritin
  • Ferrous
  • all of the above
According to Werner's theory state, which of the following statements are correct?

Ligands are connected to the metal ions by covalent bonds
Secondary valencies have directional properties
Secondary valencies are non-ionisable.
  • 1, 2, and 3 are correct
  • 2 and 3 are correct
  • 1 and 2 are correct
  • 1 ,2 are correct,and 3 is not correct
Which of the following will give maximum number of isomers:-
  • $$[Co(py)_3(NH_3)_3]^{3+}$$
  • $$[Ni(en)(NH_3)_4]^{2+}$$
  • $$[Fe(C_2O_4)(en)_2]^{2-}$$
  • $$[Cr(NO_2)_2(NH_3)_4]^{+}$$
The hybridization of the complex  $$ [CrCl _ { 2 } \left(N O_{ 2 } \right) _ { 2 } \left( N H _ { 3 } \right) _ { 2 } ]^- $$ is:
  • $$s p ^ {3}d^{2}$$
  • $$d ^ { 2 } s p ^ { 3 }$$
  • $$s p ^ {3}d$$
  • Cannot be predicted
Which one of the following high spin complexes has the largest $$CFSE$$ (crystal field stabilization energy)?
  • $$[Cr(H_{2}O_{6})]^{2+}$$
  • $$[Cr(H_{2}O)_{6}]^{3+}$$
  • $$[Mn(H_{2}O)_{6}]^{2+}$$
  • $$[Mn(H_{2}O)_{6}]^{3+}$$
The number of electrons present in $$e_{g}$$ set of orbital of triquatrifluoro cobalt $$(III)$$ is:
  • $$2$$
  • $$3$$
  • $$4$$
  • $$0$$
Which one is more stable in the following pairs of complexes? Give reasons.
  • $$[Co(NO_2)_6]^{4-}$$ and $$[Co(NO_2)_6]^{3-}$$
  • $$K_4[Fe(CN)_6]$$ and$$K_3[Fe(CN)_6]$$
  • $$[Co(H_2O)_6]^{2+}$$ and$$ [Co(NH_3)_6]^{2+}$$
  • None of them
Number of chlorides satisfying the secondary valency in $$CoCl_{3}.4NH_{3}$$ is:
  • $$1$$
  • $$2$$
  • $$3$$
  • $$6$$
$$ [Cr(H_{2}O)_{6}]Cl_{3}$$ (atomic number of Cr =24) has a magnetic moment of 3.83 B.M. The correct distribution of 3d -electrons in the chromium present in the complex is:
  • $$ 3d^{1}_{xy},3d^{1}_{yz},3d^{1}_{zx}$$
  • $$3d^{1}_{xy},3d^{1}_{yz},3d^{1}_{z^{2}}$$
  • $$ 3d^{1}_{x^{2}-y^{2}},3d^{1}_{z^{2}},3d^{1}_{zx}$$
  • $$ 3d^{1}_{xy},3d^{1}_({x^{2}-y^{2}}),3d^{1}_{xz}$$
State the correct statement(s):
  • $$[Co(EDTA)^-]$$ has two optical isomers
  • $$[Co(NH_3)_3(NO_2)]^{2+}$$ show linkage isomerism
  • For $$[Pt(NH_3)BrCl(NO_2)py]$$, theoretically fifteen different geometrical isomers are possible
  • $$[Cr(H_2O)_4Cl_2]Cl_2.2H_2O$$ is an example of hydrate as well as ionisation isomerism
Which of the following complexes is/are optically inactive due to the presence of plane of symmetry?
The number of possible isomers of an octahedral complex $$[Co(C_{2}O_{4})_{2}(NH_{3})_{2}]$$ is-
  • $$1$$
  • $$2$$
  • $$3$$
  • $$4$$
Square planar complex that can not show cis-trans isomerism is:
  • $$[Cu(NH_3)_4]^{2+}$$
  • $$[Pt Cl_2(NH_3)_2]$$
  • $$[Pt(NH_3)(H_2O)(NO_2)(Cl)]$$
  • $$[Pt(gly)_2]$$
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