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1 | 5105-5108 | The treatment provides for quantitative estimations of
orbital separation energies, magnetic moments and spectral and stability
parameters However, the assumption that ligands consititute point charges
creates many theoretical difficulties The metal–carbon bond in metal carbonyls possesses both s and p character The ligand to metal is s bond and metal to ligand is p bond |
1 | 5106-5109 | However, the assumption that ligands consititute point charges
creates many theoretical difficulties The metal–carbon bond in metal carbonyls possesses both s and p character The ligand to metal is s bond and metal to ligand is p bond This unique synergic
bonding provides stability to metal carbonyls |
1 | 5107-5110 | The metal–carbon bond in metal carbonyls possesses both s and p character The ligand to metal is s bond and metal to ligand is p bond This unique synergic
bonding provides stability to metal carbonyls Coordination compounds are of great importance |
1 | 5108-5111 | The ligand to metal is s bond and metal to ligand is p bond This unique synergic
bonding provides stability to metal carbonyls Coordination compounds are of great importance These compounds provide
critical insights into the functioning and structures of vital components of
biological systems |
1 | 5109-5112 | This unique synergic
bonding provides stability to metal carbonyls Coordination compounds are of great importance These compounds provide
critical insights into the functioning and structures of vital components of
biological systems Coordination compounds also find extensive applications in
metallurgical processes, analytical and medicinal chemistry |
1 | 5110-5113 | Coordination compounds are of great importance These compounds provide
critical insights into the functioning and structures of vital components of
biological systems Coordination compounds also find extensive applications in
metallurgical processes, analytical and medicinal chemistry Exercises
5 |
1 | 5111-5114 | These compounds provide
critical insights into the functioning and structures of vital components of
biological systems Coordination compounds also find extensive applications in
metallurgical processes, analytical and medicinal chemistry Exercises
5 1
Explain the bonding in coordination compounds in terms of Werner’s postulates |
1 | 5112-5115 | Coordination compounds also find extensive applications in
metallurgical processes, analytical and medicinal chemistry Exercises
5 1
Explain the bonding in coordination compounds in terms of Werner’s postulates 5 |
1 | 5113-5116 | Exercises
5 1
Explain the bonding in coordination compounds in terms of Werner’s postulates 5 2
FeSO4 solution mixed with (NH4)2SO4 solution in 1:1 molar ratio gives the
test of Fe
2+ ion but CuSO4 solution mixed with aqueous ammonia in 1:4
molar ratio does not give the test of Cu
2+ ion |
1 | 5114-5117 | 1
Explain the bonding in coordination compounds in terms of Werner’s postulates 5 2
FeSO4 solution mixed with (NH4)2SO4 solution in 1:1 molar ratio gives the
test of Fe
2+ ion but CuSO4 solution mixed with aqueous ammonia in 1:4
molar ratio does not give the test of Cu
2+ ion Explain why |
1 | 5115-5118 | 5 2
FeSO4 solution mixed with (NH4)2SO4 solution in 1:1 molar ratio gives the
test of Fe
2+ ion but CuSO4 solution mixed with aqueous ammonia in 1:4
molar ratio does not give the test of Cu
2+ ion Explain why 5 |
1 | 5116-5119 | 2
FeSO4 solution mixed with (NH4)2SO4 solution in 1:1 molar ratio gives the
test of Fe
2+ ion but CuSO4 solution mixed with aqueous ammonia in 1:4
molar ratio does not give the test of Cu
2+ ion Explain why 5 3
Explain with two examples each of the following: coordination entity, ligand,
coordination number, coordination polyhedron, homoleptic and heteroleptic |
1 | 5117-5120 | Explain why 5 3
Explain with two examples each of the following: coordination entity, ligand,
coordination number, coordination polyhedron, homoleptic and heteroleptic 5 |
1 | 5118-5121 | 5 3
Explain with two examples each of the following: coordination entity, ligand,
coordination number, coordination polyhedron, homoleptic and heteroleptic 5 4
What is meant by unidentate, didentate and ambidentate ligands |
1 | 5119-5122 | 3
Explain with two examples each of the following: coordination entity, ligand,
coordination number, coordination polyhedron, homoleptic and heteroleptic 5 4
What is meant by unidentate, didentate and ambidentate ligands Give two
examples for each |
1 | 5120-5123 | 5 4
What is meant by unidentate, didentate and ambidentate ligands Give two
examples for each 5 |
1 | 5121-5124 | 4
What is meant by unidentate, didentate and ambidentate ligands Give two
examples for each 5 5
Specify the oxidation numbers of the metals in the following coordination entities:
(i) [Co(H2O)(CN)(en)2]
2+
(iii) [PtCl4]
2–
(v) [Cr(NH3)3Cl3]
(ii) [CoBr2(en)2]
+
(iv) K3[Fe(CN)6]
5 |
1 | 5122-5125 | Give two
examples for each 5 5
Specify the oxidation numbers of the metals in the following coordination entities:
(i) [Co(H2O)(CN)(en)2]
2+
(iii) [PtCl4]
2–
(v) [Cr(NH3)3Cl3]
(ii) [CoBr2(en)2]
+
(iv) K3[Fe(CN)6]
5 6
Using IUPAC norms write the formulas for the following:
(i) Tetrahydroxidozincate(II)
(vi) Hexaamminecobalt(III) sulphate
(ii) Potassium tetrachloridopalladate(II)
(vii) Potassium tri(oxalato)chromate(III)
(iii) Diamminedichloridoplatinum(II)
(viii) Hexaammineplatinum(IV)
(iv) Potassium tetracyanidonickelate(II) (ix) Tetrabromidocuprate(II)
(v) Pentaamminenitrito-O-cobalt(III)
(x) Pentaamminenitrito-N-cobalt(III)
5 |
1 | 5123-5126 | 5 5
Specify the oxidation numbers of the metals in the following coordination entities:
(i) [Co(H2O)(CN)(en)2]
2+
(iii) [PtCl4]
2–
(v) [Cr(NH3)3Cl3]
(ii) [CoBr2(en)2]
+
(iv) K3[Fe(CN)6]
5 6
Using IUPAC norms write the formulas for the following:
(i) Tetrahydroxidozincate(II)
(vi) Hexaamminecobalt(III) sulphate
(ii) Potassium tetrachloridopalladate(II)
(vii) Potassium tri(oxalato)chromate(III)
(iii) Diamminedichloridoplatinum(II)
(viii) Hexaammineplatinum(IV)
(iv) Potassium tetracyanidonickelate(II) (ix) Tetrabromidocuprate(II)
(v) Pentaamminenitrito-O-cobalt(III)
(x) Pentaamminenitrito-N-cobalt(III)
5 7
Using IUPAC norms write the systematic names of the following:
(i) [Co(NH3)6]Cl3
(iv) [Co(NH3)4Cl(NO2)]Cl
(vii) [Ni(NH3)6]Cl2
(ii) [Pt(NH3)2Cl(NH2CH3)]Cl
(v) [Mn(H2O)6]
2+
(viii) [Co(en)3]
3+
(iii) [Ti(H2O)6]
3+
(vi) [NiCl4]
2–
(ix) [Ni(CO)4]
5 |
1 | 5124-5127 | 5
Specify the oxidation numbers of the metals in the following coordination entities:
(i) [Co(H2O)(CN)(en)2]
2+
(iii) [PtCl4]
2–
(v) [Cr(NH3)3Cl3]
(ii) [CoBr2(en)2]
+
(iv) K3[Fe(CN)6]
5 6
Using IUPAC norms write the formulas for the following:
(i) Tetrahydroxidozincate(II)
(vi) Hexaamminecobalt(III) sulphate
(ii) Potassium tetrachloridopalladate(II)
(vii) Potassium tri(oxalato)chromate(III)
(iii) Diamminedichloridoplatinum(II)
(viii) Hexaammineplatinum(IV)
(iv) Potassium tetracyanidonickelate(II) (ix) Tetrabromidocuprate(II)
(v) Pentaamminenitrito-O-cobalt(III)
(x) Pentaamminenitrito-N-cobalt(III)
5 7
Using IUPAC norms write the systematic names of the following:
(i) [Co(NH3)6]Cl3
(iv) [Co(NH3)4Cl(NO2)]Cl
(vii) [Ni(NH3)6]Cl2
(ii) [Pt(NH3)2Cl(NH2CH3)]Cl
(v) [Mn(H2O)6]
2+
(viii) [Co(en)3]
3+
(iii) [Ti(H2O)6]
3+
(vi) [NiCl4]
2–
(ix) [Ni(CO)4]
5 8
List various types of isomerism possible for coordination compounds, giving
an example of each |
1 | 5125-5128 | 6
Using IUPAC norms write the formulas for the following:
(i) Tetrahydroxidozincate(II)
(vi) Hexaamminecobalt(III) sulphate
(ii) Potassium tetrachloridopalladate(II)
(vii) Potassium tri(oxalato)chromate(III)
(iii) Diamminedichloridoplatinum(II)
(viii) Hexaammineplatinum(IV)
(iv) Potassium tetracyanidonickelate(II) (ix) Tetrabromidocuprate(II)
(v) Pentaamminenitrito-O-cobalt(III)
(x) Pentaamminenitrito-N-cobalt(III)
5 7
Using IUPAC norms write the systematic names of the following:
(i) [Co(NH3)6]Cl3
(iv) [Co(NH3)4Cl(NO2)]Cl
(vii) [Ni(NH3)6]Cl2
(ii) [Pt(NH3)2Cl(NH2CH3)]Cl
(v) [Mn(H2O)6]
2+
(viii) [Co(en)3]
3+
(iii) [Ti(H2O)6]
3+
(vi) [NiCl4]
2–
(ix) [Ni(CO)4]
5 8
List various types of isomerism possible for coordination compounds, giving
an example of each 5 |
1 | 5126-5129 | 7
Using IUPAC norms write the systematic names of the following:
(i) [Co(NH3)6]Cl3
(iv) [Co(NH3)4Cl(NO2)]Cl
(vii) [Ni(NH3)6]Cl2
(ii) [Pt(NH3)2Cl(NH2CH3)]Cl
(v) [Mn(H2O)6]
2+
(viii) [Co(en)3]
3+
(iii) [Ti(H2O)6]
3+
(vi) [NiCl4]
2–
(ix) [Ni(CO)4]
5 8
List various types of isomerism possible for coordination compounds, giving
an example of each 5 9
How many geometrical isomers are possible in the following coordination entities |
1 | 5127-5130 | 8
List various types of isomerism possible for coordination compounds, giving
an example of each 5 9
How many geometrical isomers are possible in the following coordination entities (i) [Cr(C2O4)3]
3–
(ii) [Co(NH3)3Cl3]
5 |
1 | 5128-5131 | 5 9
How many geometrical isomers are possible in the following coordination entities (i) [Cr(C2O4)3]
3–
(ii) [Co(NH3)3Cl3]
5 10
Draw the structures of optical isomers of:
(i) [Cr(C2O4)3]
3–
(ii) [PtCl2(en)2]
2+
(iii) [Cr(NH3)2Cl2(en)]
+
Rationalised 2023-24
139
Coordination Compounds
5 |
1 | 5129-5132 | 9
How many geometrical isomers are possible in the following coordination entities (i) [Cr(C2O4)3]
3–
(ii) [Co(NH3)3Cl3]
5 10
Draw the structures of optical isomers of:
(i) [Cr(C2O4)3]
3–
(ii) [PtCl2(en)2]
2+
(iii) [Cr(NH3)2Cl2(en)]
+
Rationalised 2023-24
139
Coordination Compounds
5 11
Draw all the isomers (geometrical and optical) of:
(i) [CoCl2(en)2]
+
(ii) [Co(NH3)Cl(en)2]
2+
(iii) [Co(NH3)2Cl2(en)]
+
5 |
1 | 5130-5133 | (i) [Cr(C2O4)3]
3–
(ii) [Co(NH3)3Cl3]
5 10
Draw the structures of optical isomers of:
(i) [Cr(C2O4)3]
3–
(ii) [PtCl2(en)2]
2+
(iii) [Cr(NH3)2Cl2(en)]
+
Rationalised 2023-24
139
Coordination Compounds
5 11
Draw all the isomers (geometrical and optical) of:
(i) [CoCl2(en)2]
+
(ii) [Co(NH3)Cl(en)2]
2+
(iii) [Co(NH3)2Cl2(en)]
+
5 12
Write all the geometrical isomers of [Pt(NH3)(Br)(Cl)(py)] and how many of
these will exhibit optical isomers |
1 | 5131-5134 | 10
Draw the structures of optical isomers of:
(i) [Cr(C2O4)3]
3–
(ii) [PtCl2(en)2]
2+
(iii) [Cr(NH3)2Cl2(en)]
+
Rationalised 2023-24
139
Coordination Compounds
5 11
Draw all the isomers (geometrical and optical) of:
(i) [CoCl2(en)2]
+
(ii) [Co(NH3)Cl(en)2]
2+
(iii) [Co(NH3)2Cl2(en)]
+
5 12
Write all the geometrical isomers of [Pt(NH3)(Br)(Cl)(py)] and how many of
these will exhibit optical isomers 5 |
1 | 5132-5135 | 11
Draw all the isomers (geometrical and optical) of:
(i) [CoCl2(en)2]
+
(ii) [Co(NH3)Cl(en)2]
2+
(iii) [Co(NH3)2Cl2(en)]
+
5 12
Write all the geometrical isomers of [Pt(NH3)(Br)(Cl)(py)] and how many of
these will exhibit optical isomers 5 13
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 |
1 | 5133-5136 | 12
Write all the geometrical isomers of [Pt(NH3)(Br)(Cl)(py)] and how many of
these will exhibit optical isomers 5 13
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 |
1 | 5134-5137 | 5 13
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 5 |
1 | 5135-5138 | 13
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 5 14
What is the coordination entity formed when excess of aqueous KCN is
added to an aqueous solution of copper sulphate |
1 | 5136-5139 | Explain these
experimental results 5 14
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 H2S(g) is passed through this solution |
1 | 5137-5140 | 5 14
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 H2S(g) is passed through this solution 5 |
1 | 5138-5141 | 14
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 H2S(g) is passed through this solution 5 15
Discuss the nature of bonding in the following coordination entities on the
basis of valence bond theory:
(i) [Fe(CN)6]
4–
(ii) [FeF6]
3–
(iii) [Co(C2O4)3]
3–
(iv) [CoF6]
3–
5 |
1 | 5139-5142 | Why is it that no precipitate
of copper sulphide is obtained when H2S(g) is passed through this solution 5 15
Discuss the nature of bonding in the following coordination entities on the
basis of valence bond theory:
(i) [Fe(CN)6]
4–
(ii) [FeF6]
3–
(iii) [Co(C2O4)3]
3–
(iv) [CoF6]
3–
5 16
Draw figure to show the splitting of d orbitals in an octahedral crystal field |
1 | 5140-5143 | 5 15
Discuss the nature of bonding in the following coordination entities on the
basis of valence bond theory:
(i) [Fe(CN)6]
4–
(ii) [FeF6]
3–
(iii) [Co(C2O4)3]
3–
(iv) [CoF6]
3–
5 16
Draw figure to show the splitting of d orbitals in an octahedral crystal field 5 |
1 | 5141-5144 | 15
Discuss the nature of bonding in the following coordination entities on the
basis of valence bond theory:
(i) [Fe(CN)6]
4–
(ii) [FeF6]
3–
(iii) [Co(C2O4)3]
3–
(iv) [CoF6]
3–
5 16
Draw figure to show the splitting of d orbitals in an octahedral crystal field 5 17
What is spectrochemical series |
1 | 5142-5145 | 16
Draw figure to show the splitting of d orbitals in an octahedral crystal field 5 17
What is spectrochemical series Explain the difference between a weak
field ligand and a strong field ligand |
1 | 5143-5146 | 5 17
What is spectrochemical series Explain the difference between a weak
field ligand and a strong field ligand 5 |
1 | 5144-5147 | 17
What is spectrochemical series Explain the difference between a weak
field ligand and a strong field ligand 5 18
What is crystal field splitting energy |
1 | 5145-5148 | Explain the difference between a weak
field ligand and a strong field ligand 5 18
What is crystal field splitting energy How does the magnitude of Do decide
the actual configuration of d orbitals in a coordination entity |
1 | 5146-5149 | 5 18
What is crystal field splitting energy How does the magnitude of Do decide
the actual configuration of d orbitals in a coordination entity 5 |
1 | 5147-5150 | 18
What is crystal field splitting energy How does the magnitude of Do decide
the actual configuration of d orbitals in a coordination entity 5 19
[Cr(NH3)6]
3+ is paramagnetic while [Ni(CN)4]
2– is diamagnetic |
1 | 5148-5151 | How does the magnitude of Do decide
the actual configuration of d orbitals in a coordination entity 5 19
[Cr(NH3)6]
3+ is paramagnetic while [Ni(CN)4]
2– is diamagnetic Explain why |
1 | 5149-5152 | 5 19
[Cr(NH3)6]
3+ is paramagnetic while [Ni(CN)4]
2– is diamagnetic Explain why 5 |
1 | 5150-5153 | 19
[Cr(NH3)6]
3+ is paramagnetic while [Ni(CN)4]
2– is diamagnetic Explain why 5 20
A solution of [Ni(H2O)6]
2+ is green but a solution of [Ni(CN)4]
2– is colourless |
1 | 5151-5154 | Explain why 5 20
A solution of [Ni(H2O)6]
2+ is green but a solution of [Ni(CN)4]
2– is colourless Explain |
1 | 5152-5155 | 5 20
A solution of [Ni(H2O)6]
2+ is green but a solution of [Ni(CN)4]
2– is colourless Explain 5 |
1 | 5153-5156 | 20
A solution of [Ni(H2O)6]
2+ is green but a solution of [Ni(CN)4]
2– is colourless Explain 5 21
[Fe(CN)6]
4– and [Fe(H2O)6]
2+ are of different colours in dilute solutions |
1 | 5154-5157 | Explain 5 21
[Fe(CN)6]
4– and [Fe(H2O)6]
2+ are of different colours in dilute solutions Why |
1 | 5155-5158 | 5 21
[Fe(CN)6]
4– and [Fe(H2O)6]
2+ are of different colours in dilute solutions Why 5 |
1 | 5156-5159 | 21
[Fe(CN)6]
4– and [Fe(H2O)6]
2+ are of different colours in dilute solutions Why 5 22
Discuss the nature of bonding in metal carbonyls |
1 | 5157-5160 | Why 5 22
Discuss the nature of bonding in metal carbonyls 5 |
1 | 5158-5161 | 5 22
Discuss the nature of bonding in metal carbonyls 5 23
Give the oxidation state, d orbital occupation and coordination number of
the central metal ion in the following complexes:
(i) K3[Co(C2O4)3]
(iii) (NH4)2[CoF4]
(ii) cis-[CrCl2(en)2]Cl
(iv) [Mn(H2O)6]SO4
5 |
1 | 5159-5162 | 22
Discuss the nature of bonding in metal carbonyls 5 23
Give the oxidation state, d orbital occupation and coordination number of
the central metal ion in the following complexes:
(i) K3[Co(C2O4)3]
(iii) (NH4)2[CoF4]
(ii) cis-[CrCl2(en)2]Cl
(iv) [Mn(H2O)6]SO4
5 24
Write down the IUPAC name for each of the following complexes and indicate
the oxidation state, electronic configuration and coordination number |
1 | 5160-5163 | 5 23
Give the oxidation state, d orbital occupation and coordination number of
the central metal ion in the following complexes:
(i) K3[Co(C2O4)3]
(iii) (NH4)2[CoF4]
(ii) cis-[CrCl2(en)2]Cl
(iv) [Mn(H2O)6]SO4
5 24
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[Cr(H2O)2(C2O4)2] |
1 | 5161-5164 | 23
Give the oxidation state, d orbital occupation and coordination number of
the central metal ion in the following complexes:
(i) K3[Co(C2O4)3]
(iii) (NH4)2[CoF4]
(ii) cis-[CrCl2(en)2]Cl
(iv) [Mn(H2O)6]SO4
5 24
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[Cr(H2O)2(C2O4)2] 3H2O
(iii) [CrCl3(py)3]
(v) K4[Mn(CN)6]
(ii) [Co(NH3)5Cl-]Cl2
(iv) Cs[FeCl4]
5 |
1 | 5162-5165 | 24
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[Cr(H2O)2(C2O4)2] 3H2O
(iii) [CrCl3(py)3]
(v) K4[Mn(CN)6]
(ii) [Co(NH3)5Cl-]Cl2
(iv) Cs[FeCl4]
5 25
Explain the violet colour of the complex [Ti(H2O)6]
3+ on the basis of crystal
field theory |
1 | 5163-5166 | Also
give stereochemistry and magnetic moment of the complex:
(i) K[Cr(H2O)2(C2O4)2] 3H2O
(iii) [CrCl3(py)3]
(v) K4[Mn(CN)6]
(ii) [Co(NH3)5Cl-]Cl2
(iv) Cs[FeCl4]
5 25
Explain the violet colour of the complex [Ti(H2O)6]
3+ on the basis of crystal
field theory 5 |
1 | 5164-5167 | 3H2O
(iii) [CrCl3(py)3]
(v) K4[Mn(CN)6]
(ii) [Co(NH3)5Cl-]Cl2
(iv) Cs[FeCl4]
5 25
Explain the violet colour of the complex [Ti(H2O)6]
3+ on the basis of crystal
field theory 5 26
What is meant by the chelate effect |
1 | 5165-5168 | 25
Explain the violet colour of the complex [Ti(H2O)6]
3+ on the basis of crystal
field theory 5 26
What is meant by the chelate effect Give an example |
1 | 5166-5169 | 5 26
What is meant by the chelate effect Give an example 5 |
1 | 5167-5170 | 26
What is meant by the chelate effect Give an example 5 27
Discuss briefly giving an example in each case the role of coordination
compounds in:
(i) biological systems
(iii) analytical chemistry
(ii) medicinal chemistry and
(iv) extraction/metallurgy of metals |
1 | 5168-5171 | Give an example 5 27
Discuss briefly giving an example in each case the role of coordination
compounds in:
(i) biological systems
(iii) analytical chemistry
(ii) medicinal chemistry and
(iv) extraction/metallurgy of metals 5 |
1 | 5169-5172 | 5 27
Discuss briefly giving an example in each case the role of coordination
compounds in:
(i) biological systems
(iii) analytical chemistry
(ii) medicinal chemistry and
(iv) extraction/metallurgy of metals 5 28
How many ions are produced from the complex Co(NH3)6Cl2 in solution |
1 | 5170-5173 | 27
Discuss briefly giving an example in each case the role of coordination
compounds in:
(i) biological systems
(iii) analytical chemistry
(ii) medicinal chemistry and
(iv) extraction/metallurgy of metals 5 28
How many ions are produced from the complex Co(NH3)6Cl2 in solution (i) 6
(ii) 4
(iii) 3
(iv) 2
Rationalised 2023-24
140
Chemistry
Answers to Some Intext Questions
5 |
1 | 5171-5174 | 5 28
How many ions are produced from the complex Co(NH3)6Cl2 in solution (i) 6
(ii) 4
(iii) 3
(iv) 2
Rationalised 2023-24
140
Chemistry
Answers to Some Intext Questions
5 1
(i) [Co(NH3)4(H2O)2]Cl3
(iv) [Pt(NH3)BrCl(NO2)]
–
(ii) K2[Ni(CN)4]
(v) [PtCl2(en)2](NO3)2
(iii) [Cr(en)3]Cl3
(vi) Fe4[Fe(CN)6]3
5 |
1 | 5172-5175 | 28
How many ions are produced from the complex Co(NH3)6Cl2 in solution (i) 6
(ii) 4
(iii) 3
(iv) 2
Rationalised 2023-24
140
Chemistry
Answers to Some Intext Questions
5 1
(i) [Co(NH3)4(H2O)2]Cl3
(iv) [Pt(NH3)BrCl(NO2)]
–
(ii) K2[Ni(CN)4]
(v) [PtCl2(en)2](NO3)2
(iii) [Cr(en)3]Cl3
(vi) Fe4[Fe(CN)6]3
5 2
(i) Hexaamminecobalt(III) chloride
(ii) Pentaamminechloridocobalt(III) chloride
(iii) Potassium hexacyanidoferrate(III)
(iv) Potassium trioxalatoferrate(III)
(v) Potassium tetrachloridopalladate(II)
(vi) Diamminechlorido(methanamine)platinum(II) chloride
5 |
1 | 5173-5176 | (i) 6
(ii) 4
(iii) 3
(iv) 2
Rationalised 2023-24
140
Chemistry
Answers to Some Intext Questions
5 1
(i) [Co(NH3)4(H2O)2]Cl3
(iv) [Pt(NH3)BrCl(NO2)]
–
(ii) K2[Ni(CN)4]
(v) [PtCl2(en)2](NO3)2
(iii) [Cr(en)3]Cl3
(vi) Fe4[Fe(CN)6]3
5 2
(i) Hexaamminecobalt(III) chloride
(ii) Pentaamminechloridocobalt(III) chloride
(iii) Potassium hexacyanidoferrate(III)
(iv) Potassium trioxalatoferrate(III)
(v) Potassium tetrachloridopalladate(II)
(vi) Diamminechlorido(methanamine)platinum(II) chloride
5 3
(i) Both geometrical (cis-, trans-) and optical isomers for cis can exist |
1 | 5174-5177 | 1
(i) [Co(NH3)4(H2O)2]Cl3
(iv) [Pt(NH3)BrCl(NO2)]
–
(ii) K2[Ni(CN)4]
(v) [PtCl2(en)2](NO3)2
(iii) [Cr(en)3]Cl3
(vi) Fe4[Fe(CN)6]3
5 2
(i) Hexaamminecobalt(III) chloride
(ii) Pentaamminechloridocobalt(III) chloride
(iii) Potassium hexacyanidoferrate(III)
(iv) Potassium trioxalatoferrate(III)
(v) Potassium tetrachloridopalladate(II)
(vi) Diamminechlorido(methanamine)platinum(II) chloride
5 3
(i) Both geometrical (cis-, trans-) and optical isomers for cis can exist (ii) Two optical isomers can exist |
1 | 5175-5178 | 2
(i) Hexaamminecobalt(III) chloride
(ii) Pentaamminechloridocobalt(III) chloride
(iii) Potassium hexacyanidoferrate(III)
(iv) Potassium trioxalatoferrate(III)
(v) Potassium tetrachloridopalladate(II)
(vi) Diamminechlorido(methanamine)platinum(II) chloride
5 3
(i) Both geometrical (cis-, trans-) and optical isomers for cis can exist (ii) Two optical isomers can exist (iii) There are 10 possible isomers |
1 | 5176-5179 | 3
(i) Both geometrical (cis-, trans-) and optical isomers for cis can exist (ii) Two optical isomers can exist (iii) There are 10 possible isomers (Hint: There are geometrical, ionisation and
linkage isomers possible) |
1 | 5177-5180 | (ii) Two optical isomers can exist (iii) There are 10 possible isomers (Hint: There are geometrical, ionisation and
linkage isomers possible) (iv) Geometrical (cis-, trans-) isomers can exist |
1 | 5178-5181 | (iii) There are 10 possible isomers (Hint: There are geometrical, ionisation and
linkage isomers possible) (iv) Geometrical (cis-, trans-) isomers can exist 5 |
1 | 5179-5182 | (Hint: There are geometrical, ionisation and
linkage isomers possible) (iv) Geometrical (cis-, trans-) isomers can exist 5 4 The ionisation isomers dissolve in water to yield different ions and thus react
differently to various reagents:
[Co(NH3)5Br]SO4
+ Ba
2+ ® BaSO4 (s)
[Co(NH3)5SO4]Br
+ Ba
2+ ® No reaction
[Co(NH3)5Br]SO4
+ Ag
+ ® No reaction
[Co(NH3)5SO4]Br
+ Ag
+ ® AgBr (s)
5 |
1 | 5180-5183 | (iv) Geometrical (cis-, trans-) isomers can exist 5 4 The ionisation isomers dissolve in water to yield different ions and thus react
differently to various reagents:
[Co(NH3)5Br]SO4
+ Ba
2+ ® BaSO4 (s)
[Co(NH3)5SO4]Br
+ Ba
2+ ® No reaction
[Co(NH3)5Br]SO4
+ Ag
+ ® No reaction
[Co(NH3)5SO4]Br
+ Ag
+ ® AgBr (s)
5 6 In Ni(CO)4, Ni is in zero oxidation state whereas in NiCl4
2–, it is in +2 oxidation
state |
1 | 5181-5184 | 5 4 The ionisation isomers dissolve in water to yield different ions and thus react
differently to various reagents:
[Co(NH3)5Br]SO4
+ Ba
2+ ® BaSO4 (s)
[Co(NH3)5SO4]Br
+ Ba
2+ ® No reaction
[Co(NH3)5Br]SO4
+ Ag
+ ® No reaction
[Co(NH3)5SO4]Br
+ Ag
+ ® AgBr (s)
5 6 In Ni(CO)4, Ni is in zero oxidation state whereas in NiCl4
2–, it is in +2 oxidation
state In the presence of CO ligand, the unpaired d electrons of Ni pair up but
Cl
– being a weak ligand is unable to pair up the unpaired electrons |
1 | 5182-5185 | 4 The ionisation isomers dissolve in water to yield different ions and thus react
differently to various reagents:
[Co(NH3)5Br]SO4
+ Ba
2+ ® BaSO4 (s)
[Co(NH3)5SO4]Br
+ Ba
2+ ® No reaction
[Co(NH3)5Br]SO4
+ Ag
+ ® No reaction
[Co(NH3)5SO4]Br
+ Ag
+ ® AgBr (s)
5 6 In Ni(CO)4, Ni is in zero oxidation state whereas in NiCl4
2–, it is in +2 oxidation
state In the presence of CO ligand, the unpaired d electrons of Ni pair up but
Cl
– being a weak ligand is unable to pair up the unpaired electrons 5 |
1 | 5183-5186 | 6 In Ni(CO)4, Ni is in zero oxidation state whereas in NiCl4
2–, it is in +2 oxidation
state In the presence of CO ligand, the unpaired d electrons of Ni pair up but
Cl
– being a weak ligand is unable to pair up the unpaired electrons 5 7 In presence of CN
–, (a strong ligand) the 3d electrons pair up leaving only one
unpaired electron |
1 | 5184-5187 | In the presence of CO ligand, the unpaired d electrons of Ni pair up but
Cl
– being a weak ligand is unable to pair up the unpaired electrons 5 7 In presence of CN
–, (a strong ligand) the 3d electrons pair up leaving only one
unpaired electron The hybridisation is d
2sp
3 forming inner orbital complex |
1 | 5185-5188 | 5 7 In presence of CN
–, (a strong ligand) the 3d electrons pair up leaving only one
unpaired electron The hybridisation is d
2sp
3 forming inner orbital complex In
the presence of H2O, (a weak ligand), 3d electrons do not pair up |
1 | 5186-5189 | 7 In presence of CN
–, (a strong ligand) the 3d electrons pair up leaving only one
unpaired electron The hybridisation is d
2sp
3 forming inner orbital complex In
the presence of H2O, (a weak ligand), 3d electrons do not pair up The
hybridisation is sp
3d
2 forming an outer orbital complex containing five unpaired
electrons, it is strongly paramagnetic |
1 | 5187-5190 | The hybridisation is d
2sp
3 forming inner orbital complex In
the presence of H2O, (a weak ligand), 3d electrons do not pair up The
hybridisation is sp
3d
2 forming an outer orbital complex containing five unpaired
electrons, it is strongly paramagnetic 5 |
1 | 5188-5191 | In
the presence of H2O, (a weak ligand), 3d electrons do not pair up The
hybridisation is sp
3d
2 forming an outer orbital complex containing five unpaired
electrons, it is strongly paramagnetic 5 8 In the presence of NH3, the 3d electrons pair up leaving two d orbitals empty
to be involved in d
2sp
3 hybridisation forming inner orbital complex in case of [Co(NH3)6]
3+ |
1 | 5189-5192 | The
hybridisation is sp
3d
2 forming an outer orbital complex containing five unpaired
electrons, it is strongly paramagnetic 5 8 In the presence of NH3, the 3d electrons pair up leaving two d orbitals empty
to be involved in d
2sp
3 hybridisation forming inner orbital complex in case of [Co(NH3)6]
3+ In Ni(NH3)6
2+, Ni is in +2 oxidation state and has d
8 configuration, the
hybridisation involved is sp
3d
2 forming outer orbital complex |
1 | 5190-5193 | 5 8 In the presence of NH3, the 3d electrons pair up leaving two d orbitals empty
to be involved in d
2sp
3 hybridisation forming inner orbital complex in case of [Co(NH3)6]
3+ In Ni(NH3)6
2+, Ni is in +2 oxidation state and has d
8 configuration, the
hybridisation involved is sp
3d
2 forming outer orbital complex 5 |
1 | 5191-5194 | 8 In the presence of NH3, the 3d electrons pair up leaving two d orbitals empty
to be involved in d
2sp
3 hybridisation forming inner orbital complex in case of [Co(NH3)6]
3+ In Ni(NH3)6
2+, Ni is in +2 oxidation state and has d
8 configuration, the
hybridisation involved is sp
3d
2 forming outer orbital complex 5 9 For square planar shape, the hybridisation is dsp
2 |
1 | 5192-5195 | In Ni(NH3)6
2+, Ni is in +2 oxidation state and has d
8 configuration, the
hybridisation involved is sp
3d
2 forming outer orbital complex 5 9 For square planar shape, the hybridisation is dsp
2 Hence the unpaired electrons
in 5d orbital pair up to make one d orbital empty for dsp
2 hybridisation |
1 | 5193-5196 | 5 9 For square planar shape, the hybridisation is dsp
2 Hence the unpaired electrons
in 5d orbital pair up to make one d orbital empty for dsp
2 hybridisation Thus
there is no unpaired electron |
1 | 5194-5197 | 9 For square planar shape, the hybridisation is dsp
2 Hence the unpaired electrons
in 5d orbital pair up to make one d orbital empty for dsp
2 hybridisation Thus
there is no unpaired electron 5 |
1 | 5195-5198 | Hence the unpaired electrons
in 5d orbital pair up to make one d orbital empty for dsp
2 hybridisation Thus
there is no unpaired electron 5 29
Amongst the following ions which one has the highest magnetic moment value |
1 | 5196-5199 | Thus
there is no unpaired electron 5 29
Amongst the following ions which one has the highest magnetic moment value (i) [Cr(H2O)6]
3+
(ii) [Fe(H2O)6]
2+ (iii) [Zn(H2O)6]
2+
5 |
1 | 5197-5200 | 5 29
Amongst the following ions which one has the highest magnetic moment value (i) [Cr(H2O)6]
3+
(ii) [Fe(H2O)6]
2+ (iii) [Zn(H2O)6]
2+
5 30
Amongst the following, the most stable complex is
(i) [Fe(H2O)6]
3+
(ii) [Fe(NH3)6]
3+ (iii) [Fe(C2O4)3]
3–
(iv) [FeCl6]
3–
5 |
1 | 5198-5201 | 29
Amongst the following ions which one has the highest magnetic moment value (i) [Cr(H2O)6]
3+
(ii) [Fe(H2O)6]
2+ (iii) [Zn(H2O)6]
2+
5 30
Amongst the following, the most stable complex is
(i) [Fe(H2O)6]
3+
(ii) [Fe(NH3)6]
3+ (iii) [Fe(C2O4)3]
3–
(iv) [FeCl6]
3–
5 31
What will be the correct order for the wavelengths of absorption in the visible
region for the following:
[Ni(NO2)6]
4–, [Ni(NH3)6]
2+, [Ni(H2O)6]
2+ |
1 | 5199-5202 | (i) [Cr(H2O)6]
3+
(ii) [Fe(H2O)6]
2+ (iii) [Zn(H2O)6]
2+
5 30
Amongst the following, the most stable complex is
(i) [Fe(H2O)6]
3+
(ii) [Fe(NH3)6]
3+ (iii) [Fe(C2O4)3]
3–
(iv) [FeCl6]
3–
5 31
What will be the correct order for the wavelengths of absorption in the visible
region for the following:
[Ni(NO2)6]
4–, [Ni(NH3)6]
2+, [Ni(H2O)6]
2+ Rationalised 2023-24
The replacement of hydrogen atom(s) in an aliphatic
or aromatic hydrocarbon by halogen atom(s) results
in the formation of alkyl halide (haloalkane) and aryl
halide (haloarene), respectively |
1 | 5200-5203 | 30
Amongst the following, the most stable complex is
(i) [Fe(H2O)6]
3+
(ii) [Fe(NH3)6]
3+ (iii) [Fe(C2O4)3]
3–
(iv) [FeCl6]
3–
5 31
What will be the correct order for the wavelengths of absorption in the visible
region for the following:
[Ni(NO2)6]
4–, [Ni(NH3)6]
2+, [Ni(H2O)6]
2+ Rationalised 2023-24
The replacement of hydrogen atom(s) in an aliphatic
or aromatic hydrocarbon by halogen atom(s) results
in the formation of alkyl halide (haloalkane) and aryl
halide (haloarene), respectively Haloalkanes contain
halogen atom(s) attached to the sp3 hybridised carbon
atom of an alkyl group whereas haloarenes contain
halogen atom(s) attached to sp2 hybridised carbon
atom(s) of an aryl group |
1 | 5201-5204 | 31
What will be the correct order for the wavelengths of absorption in the visible
region for the following:
[Ni(NO2)6]
4–, [Ni(NH3)6]
2+, [Ni(H2O)6]
2+ Rationalised 2023-24
The replacement of hydrogen atom(s) in an aliphatic
or aromatic hydrocarbon by halogen atom(s) results
in the formation of alkyl halide (haloalkane) and aryl
halide (haloarene), respectively Haloalkanes contain
halogen atom(s) attached to the sp3 hybridised carbon
atom of an alkyl group whereas haloarenes contain
halogen atom(s) attached to sp2 hybridised carbon
atom(s) of an aryl group Many halogen containing
organic compounds occur in nature and some of
these are clinically useful |
1 | 5202-5205 | Rationalised 2023-24
The replacement of hydrogen atom(s) in an aliphatic
or aromatic hydrocarbon by halogen atom(s) results
in the formation of alkyl halide (haloalkane) and aryl
halide (haloarene), respectively Haloalkanes contain
halogen atom(s) attached to the sp3 hybridised carbon
atom of an alkyl group whereas haloarenes contain
halogen atom(s) attached to sp2 hybridised carbon
atom(s) of an aryl group Many halogen containing
organic compounds occur in nature and some of
these are clinically useful These classes of compounds
find wide applications in industry as well as in day-
to-day life |
1 | 5203-5206 | Haloalkanes contain
halogen atom(s) attached to the sp3 hybridised carbon
atom of an alkyl group whereas haloarenes contain
halogen atom(s) attached to sp2 hybridised carbon
atom(s) of an aryl group Many halogen containing
organic compounds occur in nature and some of
these are clinically useful These classes of compounds
find wide applications in industry as well as in day-
to-day life They are used as solvents for relatively
non-polar compounds and as starting materials for
the synthesis of wide range of organic compounds |
1 | 5204-5207 | Many halogen containing
organic compounds occur in nature and some of
these are clinically useful These classes of compounds
find wide applications in industry as well as in day-
to-day life They are used as solvents for relatively
non-polar compounds and as starting materials for
the synthesis of wide range of organic compounds Chlorine containing antibiotic, chloramphenicol,
produced by microorganisms is very effective for the
treatment of typhoid fever |
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