Class 12
Dashboard
Chemistry
Coordination Compounds
NCERT Solutions
NCERT Solutions
Coordination Compounds
41 Solutions
Exercise:
All Exercises
Exercises
Intext Questions
Q1
Exercises
Explain the bonding in coordination compounds in terms of Werner's postulates.
Q2
Exercises
F
e
S
O
4
FeSO_4
F
e
S
O
4
solution mixed with
(
N
H
4
)
2
S
O
4
(NH_4)_2SO_4
(
N
H
4
)
2
S
O
4
solution in 1:1 molar ratio gives the test of
F
e
2
+
Fe^{2+}
F
e
2
+
ion but
C
u
S
O
4
CuSO_4
C
u
S
O
4
solution mixed with aqueous ammonia in 1:4 molar ratio does not give the test of
C
u
2
+
Cu^{2+}
C
u
2
+
ion. Explain why?
Q3
Exercises
Explain with two examples each of the following: coordination entity, ligand, coordination number, coordination polyhedron, homoleptic and heteroleptic.
Q4
Exercises
What is meant by unidentate, didentate and ambidentate ligands? Give two examples for each.
Q5
Exercises
Specify the oxidation numbers of the metals in the following coordination entities:
(i)
[
C
o
(
H
2
O
)
(
C
N
)
(
e
n
)
2
]
2
+
[Co(H_2O)(CN)(en)_2]^{2+}
[
C
o
(
H
2
O
)
(
CN
)
(
e
n
)
2
]
2
+
(ii)
[
C
o
B
r
2
(
e
n
)
2
]
−
[CoBr_2(en)_2]^−
[
C
o
B
r
2
(
e
n
)
2
]
−
(iii)
[
P
t
C
l
4
]
2
−
[PtCl_4]^{2−}
[
PtC
l
4
]
2
−
(iv)
K
3
[
F
e
(
C
N
)
6
]
K_3[Fe(CN)_6]
K
3
[
F
e
(
CN
)
6
]
(v)
[
C
r
(
N
H
3
)
3
C
l
3
]
[Cr(NH_3)_3Cl_3]
[
C
r
(
N
H
3
)
3
C
l
3
]
Q6
Exercises
Using IUPAC norms write the formulas for the following:
(i)
Tetrahydroxidozincate(II)
(ii)
Potassium tetrachloridopalladate(II)
(iii)
Diamminedichloridoplatinum(II)
(iv)
Potassium tetracyanidonickelate(II)
(v)
Pentaamminenitrito-O-cobalt(III)
(vi)
Hexaamminecobalt(III) sulphate
(vii)
Potassium tri(oxalato)chromate(III)
(viii)
Hexaammineplatinum(IV)
(ix)
Tetrabromidocuprate(II)
(x)
Pentaamminenitrito-N-cobalt(III)
Q7
Exercises
Using IUPAC norms write the systematic names of the following:
(i)
[
C
o
(
N
H
3
)
6
]
C
l
3
[Co(NH_3)_6]Cl_3
[
C
o
(
N
H
3
)
6
]
C
l
3
(ii)
[
P
t
(
N
H
3
)
2
C
l
(
N
H
2
C
H
3
)
]
C
l
[Pt(NH_3)_2Cl(NH_2CH_3)]Cl
[
Pt
(
N
H
3
)
2
Cl
(
N
H
2
C
H
3
)]
Cl
(iii)
[
T
i
(
H
2
O
)
6
]
3
+
[Ti(H_2O)_6]^{3+}
[
T
i
(
H
2
O
)
6
]
3
+
(iv)
[
C
o
(
N
H
3
)
4
C
l
(
N
O
2
)
]
C
l
[Co(NH_3)_4Cl(NO_2)]Cl
[
C
o
(
N
H
3
)
4
Cl
(
N
O
2
)]
Cl
(v)
[
M
n
(
H
2
O
)
6
]
2
+
[Mn(H_2O)_6]^{2+}
[
M
n
(
H
2
O
)
6
]
2
+
(vi)
[
N
i
C
l
4
]
2
−
[NiCl_4]^{2−}
[
N
i
C
l
4
]
2
−
(vii)
[
N
i
(
N
H
3
)
6
]
C
l
2
[Ni(NH_3)_6]Cl_2
[
N
i
(
N
H
3
)
6
]
C
l
2
(viii)
[
C
o
(
e
n
)
3
]
3
+
[Co(en)_3]^{3+}
[
C
o
(
e
n
)
3
]
3
+
(ix)
[
N
i
(
C
O
)
4
]
[Ni(CO)_4]
[
N
i
(
CO
)
4
]
Q8
Exercises
List various types of isomerism possible for coordination compounds, giving an example of each.
Q9
Exercises
How many geometrical isomers are possible in the following coordination entities?
(i)
[
C
r
(
C
2
O
4
)
3
]
3
−
[Cr(C_2O_4)_3]^{3−}
[
C
r
(
C
2
O
4
)
3
]
3
−
(ii)
[
C
o
(
N
H
3
)
3
C
l
3
]
[Co(NH_3)_3Cl_3]
[
C
o
(
N
H
3
)
3
C
l
3
]
Q10
Exercises
Draw the structures of optical isomers of:
(i)
[
C
r
(
C
2
O
4
)
3
]
3
−
[Cr(C_2O_4)_3]^{3−}
[
C
r
(
C
2
O
4
)
3
]
3
−
(ii)
[
P
t
C
l
2
(
e
n
)
2
]
2
+
[PtCl_2(en)_2]^{2+}
[
PtC
l
2
(
e
n
)
2
]
2
+
(iii)
[
C
r
(
N
H
3
)
2
C
l
2
(
e
n
)
]
+
[Cr(NH_3)_2Cl_2(en)]^+
[
C
r
(
N
H
3
)
2
C
l
2
(
e
n
)
]
+
Q11
Exercises
Draw all the isomers (geometrical and optical) of:
(i)
[
C
o
C
l
2
(
e
n
)
2
]
−
[CoCl_2(en)_2]^−
[
C
o
C
l
2
(
e
n
)
2
]
−
(ii)
[
C
o
(
N
H
3
)
C
l
(
e
n
)
2
]
2
+
[Co(NH_3)Cl(en)_2]^{2+}
[
C
o
(
N
H
3
)
Cl
(
e
n
)
2
]
2
+
(iii)
[
C
o
(
N
H
3
)
2
C
l
2
(
e
n
)
]
+
[Co(NH_3)_2Cl_2(en)]^+
[
C
o
(
N
H
3
)
2
C
l
2
(
e
n
)
]
+
Q12
Exercises
Write all the geometrical isomers of
[
P
t
(
N
H
3
)
(
B
r
)
(
C
l
)
(
p
y
)
]
[Pt(NH_3)(Br)(Cl)(py)]
[
Pt
(
N
H
3
)
(
B
r
)
(
Cl
)
(
p
y
)]
and how many of these will exhibit optical isomers?
Q13
Exercises
Aqueous copper sulphate solution (blue in colour) gives:
(i)
a green precipitate with aqueous potassium fluoride and
(ii)
a bright green solution with aqueous potassium chloride. Explain these experimental results.
Q14
Exercises
What is the coordination entity formed when excess of aqueous KCN is added to an aqueous solution of copper sulphate? Why is it that no precipitate of copper sulphide is obtained when
H
2
S
(
g
)
H_2S(g)
H
2
S
(
g
)
is passed through this solution?
Q15
Exercises
Discuss the nature of bonding in the following coordination entities on the basis of valence bond theory:
(i)
[
F
e
(
C
N
)
6
]
4
−
[Fe(CN)_6]^{4−}
[
F
e
(
CN
)
6
]
4
−
(ii)
[
F
e
F
6
]
3
−
[FeF_6]^{3−}
[
F
e
F
6
]
3
−
(iii)
[
C
o
(
C
2
O
4
)
3
]
3
−
[Co(C_2O_4)_3]^{3−}
[
C
o
(
C
2
O
4
)
3
]
3
−
(iv)
[
C
o
F
6
]
3
−
[CoF_6]^{3−}
[
C
o
F
6
]
3
−
Q16
Exercises
Draw figure to show the splitting of d orbitals in an octahedral crystal field.
Q17
Exercises
What is spectrochemical series? Explain the difference between a weak field ligand and a strong field ligand.
Q18
Exercises
What is crystal field splitting energy? How does the magnitude of
Δ
o
Δ_o
Δ
o
decide the actual configuration of d orbitals in a coordination entity?
Q19
Exercises
[
C
r
(
N
H
3
)
6
]
3
+
[Cr(NH_3)_6]^{3+}
[
C
r
(
N
H
3
)
6
]
3
+
is paramagnetic while
[
N
i
(
C
N
)
4
]
2
−
[Ni(CN)_4]^{2−}
[
N
i
(
CN
)
4
]
2
−
is diamagnetic. Explain why?
Q20
Exercises
A solution of
[
N
i
(
H
2
O
)
6
]
2
+
[Ni(H_2O)_6]^{2+}
[
N
i
(
H
2
O
)
6
]
2
+
is green but a solution of
[
N
i
(
C
N
)
4
]
2
−
[Ni(CN)_4]^{2−}
[
N
i
(
CN
)
4
]
2
−
is colourless. Explain.
Q21
Exercises
[
F
e
(
C
N
)
6
]
4
−
[Fe(CN)_6]^{4−}
[
F
e
(
CN
)
6
]
4
−
and
[
F
e
(
H
2
O
)
6
]
2
+
[Fe(H_2O)_6]^{2+}
[
F
e
(
H
2
O
)
6
]
2
+
are of different colours in dilute solutions. Why?
Q22
Exercises
Discuss the nature of bonding in metal carbonyls.
Q23
Exercises
Give the oxidation state, d orbital occupation and coordination number of the central metal ion in the following complexes:
(i)
K
3
[
C
o
(
C
2
O
4
)
3
]
K_3[Co(C_2O_4)_3]
K
3
[
C
o
(
C
2
O
4
)
3
]
(ii)
cis-
[
C
r
C
l
2
(
e
n
)
2
]
C
l
[CrCl_2(en)_2]Cl
[
C
r
C
l
2
(
e
n
)
2
]
Cl
(iii)
(
N
H
4
)
2
[
C
o
F
4
]
(NH_4)_2[CoF_4]
(
N
H
4
)
2
[
C
o
F
4
]
(iv)
[
M
n
(
H
2
O
)
6
]
S
O
4
[Mn(H_2O)_6]SO_4
[
M
n
(
H
2
O
)
6
]
S
O
4
Q24
Exercises
Write down the IUPAC name for each of the following complexes and indicate the oxidation state, electronic configuration and coordination number. Also give stereochemistry and magnetic moment of the complex:
(i)
K
[
C
r
(
H
2
O
)
2
(
C
2
O
4
)
2
]
⋅
3
H
2
O
K[Cr(H_2O)_2(C_2O_4)_2] \cdot 3H_2O
K
[
C
r
(
H
2
O
)
2
(
C
2
O
4
)
2
]
⋅
3
H
2
O
(ii)
[
C
o
(
N
H
3
)
5
C
l
]
C
l
2
[Co(NH_3)_5Cl]Cl_2
[
C
o
(
N
H
3
)
5
Cl
]
C
l
2
(iii)
[
C
r
C
l
3
(
p
y
)
3
]
[CrCl_3(py)_3]
[
C
r
C
l
3
(
p
y
)
3
]
(iv)
C
s
[
F
e
C
l
4
]
Cs[FeCl_4]
C
s
[
F
e
C
l
4
]
(v)
K
4
[
M
n
(
C
N
)
6
]
K_4[Mn(CN)_6]
K
4
[
M
n
(
CN
)
6
]
Q25
Exercises
Explain the violet colour of the complex
[
T
i
(
H
2
O
)
6
]
3
+
[Ti(H_2O)_6]^{3+}
[
T
i
(
H
2
O
)
6
]
3
+
on the basis of crystal field theory.
Q26
Exercises
What is meant by the chelate effect? Give an example.
Q27
Exercises
Discuss briefly giving an example in each case the role of coordination compounds in:
(i)
biological systems
(ii)
medicinal chemistry and
(iii)
analytical chemistry
(iv)
extraction/metallurgy of metals.
Q28
Exercises
How many ions are produced from the complex
C
o
(
N
H
3
)
6
C
l
2
Co(NH_3)_6Cl_2
C
o
(
N
H
3
)
6
C
l
2
in solution?
(i)
6
(ii)
4
(iii)
3
(iv)
2
Q29
Exercises
Amongst the following ions which one has the highest magnetic moment value?
(i)
[
C
r
(
H
2
O
)
6
]
3
+
[Cr(H_2O)_6]^{3+}
[
C
r
(
H
2
O
)
6
]
3
+
(ii)
[
F
e
(
H
2
O
)
6
]
2
+
[Fe(H_2O)_6]^{2+}
[
F
e
(
H
2
O
)
6
]
2
+
(iii)
[
Z
n
(
H
2
O
)
6
]
2
+
[Zn(H_2O)_6]^{2+}
[
Z
n
(
H
2
O
)
6
]
2
+
Q30
Exercises
Amongst the following, the most stable complex is
(i)
[
F
e
(
H
2
O
)
6
]
3
+
[Fe(H_2O)_6]^{3+}
[
F
e
(
H
2
O
)
6
]
3
+
(ii)
[
F
e
(
N
H
3
)
6
]
3
+
[Fe(NH_3)_6]^{3+}
[
F
e
(
N
H
3
)
6
]
3
+
(iii)
[
F
e
(
C
2
O
4
)
3
]
3
−
[Fe(C_2O_4)_3]^{3−}
[
F
e
(
C
2
O
4
)
3
]
3
−
(iv)
[
F
e
C
l
6
]
3
−
[FeCl_6]^{3−}
[
F
e
C
l
6
]
3
−
Q31
Exercises
What will be the correct order for the wavelengths of absorption in the visible region for the following:
[
N
i
(
N
O
2
)
6
]
4
−
,
[
N
i
(
N
H
3
)
6
]
2
+
,
[
N
i
(
H
2
O
)
6
]
2
+
[Ni(NO_2)_6]^{4−}, [Ni(NH_3)_6]^{2+}, [Ni(H_2O)_6]^{2+}
[
N
i
(
N
O
2
)
6
]
4
−
,
[
N
i
(
N
H
3
)
6
]
2
+
,
[
N
i
(
H
2
O
)
6
]
2
+
?
Q1
Intext Questions
Write the formulas for the following coordination compounds:
(i)
tetraamminediaquacobalt(III) chloride
(ii)
potassium tetracyanidonickelate(II)
(iii)
tris(ethane-1,2-diamine) chromium(III) chloride
(iv)
amminebromidochloridonitrito-N-platinate(II)
(v)
dichloridobis(ethane-1,2-diamine)platinum(IV) nitrate
(vi)
iron(III) hexacyanidoferrate(II)
Q2
Intext Questions
Write the IUPAC names of the following coordination compounds:
(i)
[
C
o
(
N
H
3
)
6
]
C
l
3
[Co(NH_3)_6]Cl_3
[
C
o
(
N
H
3
)
6
]
C
l
3
(ii)
[
C
o
(
N
H
3
)
5
C
l
]
C
l
2
[Co(NH_3)_5Cl]Cl_2
[
C
o
(
N
H
3
)
5
Cl
]
C
l
2
(iii)
K
3
[
F
e
(
C
N
)
6
]
K_3[Fe(CN)_6]
K
3
[
F
e
(
CN
)
6
]
(iv)
K
3
[
F
e
(
C
2
O
4
)
3
]
K_3[Fe(C_2O_4)_3]
K
3
[
F
e
(
C
2
O
4
)
3
]
(v)
K
2
[
P
d
C
l
4
]
K_2[PdCl_4]
K
2
[
P
d
C
l
4
]
(vi)
[
P
t
(
N
H
3
)
2
C
l
(
N
H
2
C
H
3
)
]
C
l
[Pt(NH_3)_2Cl(NH_2CH_3)]Cl
[
Pt
(
N
H
3
)
2
Cl
(
N
H
2
C
H
3
)]
Cl
Q3
Intext Questions
Indicate the types of isomerism exhibited by the following complexes and draw the structures for these isomers:
(i)
K
[
C
r
(
H
2
O
)
2
(
C
2
O
4
)
2
]
K[Cr(H_2O)_2(C_2O_4)_2]
K
[
C
r
(
H
2
O
)
2
(
C
2
O
4
)
2
]
(ii)
[
C
o
(
e
n
)
3
]
C
l
3
[Co(en)_3]Cl_3
[
C
o
(
e
n
)
3
]
C
l
3
(iii)
[
C
o
(
N
H
3
)
5
(
N
O
2
)
]
(
N
O
3
)
2
[Co(NH_3)_5(NO_2)](NO_3)_2
[
C
o
(
N
H
3
)
5
(
N
O
2
)]
(
N
O
3
)
2
(iv)
[
P
t
(
N
H
3
)
(
H
2
O
)
C
l
2
]
[Pt(NH_3)(H_2O)Cl_2]
[
Pt
(
N
H
3
)
(
H
2
O
)
C
l
2
]
Q4
Intext Questions
Give evidence that
[
C
o
(
N
H
3
)
5
C
l
]
S
O
4
[Co(NH_3)_5Cl]SO_4
[
C
o
(
N
H
3
)
5
Cl
]
S
O
4
and
[
C
o
(
N
H
3
)
5
(
S
O
4
)
]
C
l
[Co(NH_3)_5(SO_4)]Cl
[
C
o
(
N
H
3
)
5
(
S
O
4
)]
Cl
are ionisation isomers.
Q5
Intext Questions
Explain on the basis of valence bond theory that
[
N
i
(
C
N
)
4
]
2
−
[Ni(CN)_4]^{2−}
[
N
i
(
CN
)
4
]
2
−
ion with square planar structure is diamagnetic and the
[
N
i
C
l
4
]
2
−
[NiCl_4]^{2−}
[
N
i
C
l
4
]
2
−
ion with tetrahedral geometry is paramagnetic.
Q6
Intext Questions
[
N
i
C
l
4
]
2
−
[NiCl_4]^{2−}
[
N
i
C
l
4
]
2
−
is paramagnetic while
[
N
i
(
C
O
)
4
]
[Ni(CO)_4]
[
N
i
(
CO
)
4
]
is diamagnetic though both are tetrahedral. Why?
Q7
Intext Questions
[
F
e
(
H
2
O
)
6
]
3
+
[Fe(H_2O)_6]^{3+}
[
F
e
(
H
2
O
)
6
]
3
+
is strongly paramagnetic whereas
[
F
e
(
C
N
)
6
]
3
−
[Fe(CN)_6]^{3−}
[
F
e
(
CN
)
6
]
3
−
is weakly paramagnetic. Explain.
Q8
Intext Questions
Explain
[
C
o
(
N
H
3
)
6
]
3
+
[Co(NH_3)_6]^{3+}
[
C
o
(
N
H
3
)
6
]
3
+
is an inner orbital complex whereas
[
N
i
(
N
H
3
)
6
]
2
+
[Ni(NH_3)_6]^{2+}
[
N
i
(
N
H
3
)
6
]
2
+
is an outer orbital complex.
Q9
Intext Questions
Predict the number of unpaired electrons in the square planar
[
P
t
(
C
N
)
4
]
2
−
[Pt(CN)_4]^{2−}
[
Pt
(
CN
)
4
]
2
−
ion.
Q10
Intext Questions
The hexaquo manganese(II) ion contains five unpaired electrons, while the hexacyanoion contains only one unpaired electron. Explain using Crystal Field Theory.
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