Chemistry - Coordination Compounds and Organometallics
Exam Duration: 45 Mins Total Questions : 30
Which one of the following ompounds will exhibit optical isomerism?
- (a)
[Co(NH3)4Cl2]+
- (b)
[Co(NH3)Cl3]
- (c)
Cis [Co(en)3]3+
- (d)
trans[Co(en)3]3+
The oxidation state of Pt [(en)H2O)4(NO2)Cl]2+ is
- (a)
+2
- (b)
+4
- (c)
+6
- (d)
-4
Which one is an example of octahedral complex?
- (a)
FeF3-
- (b)
[Zn(NH3)4]2+
- (c)
[Ni(CN)4]2-
- (d)
[Cu(NH3)4]2+
Which one of the following compounds is most stable?
- (a)
[Ag(NH3)2]Cl
- (b)
[Cu(NH3)4]SO4
- (c)
K2[Cu(CN)4]
- (d)
[CO(NH3)5]Cl3
Which one of the following is Wilkinson's catalyst?
- (a)
Ph3p
- (b)
(Ph3p)3
- (c)
(Ph3P)3 Rh Cl
- (d)
NONE OF THESE
Haemoglobin is a complex compound with a metal in the centre; the metal is
- (a)
Mg
- (b)
Ca
- (c)
K
- (d)
Fe
For an octahedral complex which one of the following electronic predicts it to be diamagnetic?
- (a)
d8 high spin
- (b)
d4 low spin
- (c)
d6 low spin
- (d)
d3 (low or high spin)
The oxidation number of Ni in the complex K4Ni(CN)6 is
- (a)
-2
- (b)
-1
- (c)
0
- (d)
+1
E.D.T.A has
- (a)
monodentate ligand
- (b)
bidentate ligand
- (c)
tetradentate ligand
- (d)
hexadentate ligand
Fe2(Co)9 is diamagnetic. Which of the following reasons is correct?
- (a)
Presence of one Co as bridge group
- (b)
Presecse of monodentate ligand
- (c)
Metel-Metal (Fe-Fe) bond in molecule
- (d)
Resonance hybridization of CO
A group of atoms can function as a ligand only when
- (a)
it is a small molecules
- (b)
it has an unshared electron pair
- (c)
it is a negatively charged ion
- (d)
it is a positively charged ion
A solution of a potassium ferrocyanide would contain......ions
- (a)
2
- (b)
3
- (c)
4
- (d)
5
K4[Fe(CN)6]is called
- (a)
Potassium hexacyanoferrate (II)
- (b)
Potassium ferricyanide
- (c)
Potassium hexacyanoferrate (III)
- (d)
Praussian blue
The possiible number of isomers for the complex [MCl2Br2]SO4 is
- (a)
1
- (b)
2
- (c)
4
- (d)
5
The number of d-electrons in [Cr(H2O)6]3+[At No. of Cr=24] is
- (a)
2
- (b)
3
- (c)
4
- (d)
5
The oxidation number of Pt in [Pt(C2H4)Cl3] is
- (a)
+1
- (b)
+2
- (c)
+3
- (d)
+4
Which one of the following is not expected to show paramagnetism?
- (a)
[Ni(H2O)6]2+
- (b)
Ni(CO)4
- (c)
[Zn(NH3)4]2+
- (d)
[Co(NH3)6]+3
Identify the species with an atom in + 6 oxidation state present in the following complexes
- (a)
\(Cr{ O }_{ 2 }{ Cl }_{ 2 }\)
- (b)
\(\left[ Cr{ \left( CN \right) }_{ 6 } \right] ^{ 3- }\)
- (c)
\(\left[ Cr{ \left( CN \right) }_{ 6 } \right] ^{ 3- }\)
- (d)
\(Mn{ O }_{ 4 }^{ - }\)
The most stable complex compound is formed by
- (a)
\(Cu^{2+}\)
- (b)
\(Ni^{2+}\)
- (c)
\(Mn^{2+}\)
- (d)
\(Fe^{3+}\)
Geometrical isomerism is shown by
- (a)
\([Ni(NH_{3})_{5}Br]^{+}\)
- (b)
\([Cr(NH_{3})_{4}(en)]^{3+}\)
- (c)
\([Co(en)_{3}]^{3+}\)
- (d)
\([Co(NH_{3})_{2}(en)_{2}]^{3+}\)
Optical isomerism is exhibited by
- (a)
\([Cr(NH_{3})_{6}]^{3+}\)
- (b)
\([Cr(en)(H_{2}O)_{4}]^{3+}\)
- (c)
\(trans-[Cr(en)_{2}Cl_{2}]^{+}\)
- (d)
\([Cr(en)_{3}]^{3+}\)
In spectrochemical series, chlorine lies above water because
- (a)
chlorine is good \(\pi\) -acceptor ligand than water
- (b)
chlorine is good \(\pi\) -donor than water
- (c)
chlorine has larger size than water
- (d)
chlorine is a strong \(\sigma\) -donor than water
The value for crystal field stabilisation energy for an octahedral complex \([CoCl_{6}]^{4-}\) is 18000 \(cm^{-1}\). The Value for crystal field stabilisation energy for tetrahedral complex is
- (a)
\(16,000\ cm^{-1}\)
- (b)
\(8,000\ cm^{-1}\)
- (c)
\(20,000\ cm^{-1}\)
- (d)
\(18,000\ cm^{-1}\)
High spin complex formed by
- (a)
\([FeF_{6}]^{3-}\)
- (b)
\([Co(NH_{3})_{6}]^{2+}\)
- (c)
\([Co(CN)_{6}]^{3-}\)
- (d)
\([Zn(NH_{3})_{6}]^{2+}\)
The colour of the coordination compounds depends on the crystal field splittings.What will be the correct order of absorption of the wavelength of light in the visible region. for the complexes, \([Co(NH_{3})_{6}]^{3+} , [Co(CN)_{6}]^{3-}\) and \([Co(H_{2}O)_{6}]^{3+}\)
- (a)
\([Co(CN)_{6}]^{3-} > [Co(NH_{3})_{6}]^{3+}>[Co(H_{2}O)_{6}]^{3+}\)
- (b)
\([Co(NH_{3})_{6}]^{3+}>[Co(H_{2}O)_{6}]^{3+}>[Co(CN)_{6}]^{3+}\)
- (c)
\([Co(H_{2}O)_{6}]^{3+} > [Co(NH_{3})_{6}]^{3+}>[Co(CN)_{6}]^{3-}\)
- (d)
\([Co(CN)_{6}]^{3-} > [Co(NH_{3})_{6}]^{3+}>[Co(H_{2}O)_{6}]^{3+}\)
The equation which is balanced and represents the correct product (s) is
- (a)
\(Li_{2}O + 2KCl \rightarrow 2LiCl + K_{2}O\)
- (b)
\([CoCl(NH_{3})_{5}]^{+} + 5H^{+} \rightarrow Co^{2+} + 5NH_{4}^{+} + Cl^{-}\)
- (c)
\([Mg(H_{2}O)_{6}]^{2+} + (EDTA)^{4-} \xrightarrow[NaoH]{excess} [Mg(EDTA)]^{2+} + 6H_{2}O\)
- (d)
\(CuSO_{4} + 4KCN \longrightarrow K_{2}[Cu(CN)_{4}]+K_{2}SO_{4}\)
A solution containing 2.675 g of \(CoCl_{3}.6NH_{4}\) (molar mass = \(267.5 \ g \ mol^{-1}\)) is passed through a cation exchanger. The chloride ions obtained in solution were treated with excess of \(AgNo_{3}\) to give 4.78 g of \(AgCl\) (molar mass = \(143.5 \ g\ mol^{-1}\)). The formula of the complex is (Atomic mass of Ag = 108 u)
- (a)
\([CoCl(NH_{3})_{5}]Cl_{2}\)
- (b)
\([Co(NH_{3})_{6}]Cl_{3}\)
- (c)
\([CoCl_{2}(NH_{3})_{4}]Cl\)
- (d)
\([CoCl_{3}(NH_{3})_{3}]\)