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1 | 4505-4508 | 4 2 In the formation of metallic bonds, no eletrons from 3d-orbitals are involved
in case of zinc, while in all other metals of the 3d series, electrons from
the d-orbitals are always involved in the formation of metallic bonds 4 3 Manganese (Z = 25), as its atom has the maximum number of unpaired
electrons |
1 | 4506-4509 | 2 In the formation of metallic bonds, no eletrons from 3d-orbitals are involved
in case of zinc, while in all other metals of the 3d series, electrons from
the d-orbitals are always involved in the formation of metallic bonds 4 3 Manganese (Z = 25), as its atom has the maximum number of unpaired
electrons 4 |
1 | 4507-4510 | 4 3 Manganese (Z = 25), as its atom has the maximum number of unpaired
electrons 4 5 Irregular variation of ionisation enthalpies is mainly attributed to varying
degree of stability of different 3d-configurations (e |
1 | 4508-4511 | 3 Manganese (Z = 25), as its atom has the maximum number of unpaired
electrons 4 5 Irregular variation of ionisation enthalpies is mainly attributed to varying
degree of stability of different 3d-configurations (e g |
1 | 4509-4512 | 4 5 Irregular variation of ionisation enthalpies is mainly attributed to varying
degree of stability of different 3d-configurations (e g , d
0, d
5, d
10 are
exceptionally stable) |
1 | 4510-4513 | 5 Irregular variation of ionisation enthalpies is mainly attributed to varying
degree of stability of different 3d-configurations (e g , d
0, d
5, d
10 are
exceptionally stable) 4 |
1 | 4511-4514 | g , d
0, d
5, d
10 are
exceptionally stable) 4 6 Because of small size and high electronegativity oxygen or fluorine can
oxidise the metal to its highest oxidation state |
1 | 4512-4515 | , d
0, d
5, d
10 are
exceptionally stable) 4 6 Because of small size and high electronegativity oxygen or fluorine can
oxidise the metal to its highest oxidation state 4 |
1 | 4513-4516 | 4 6 Because of small size and high electronegativity oxygen or fluorine can
oxidise the metal to its highest oxidation state 4 7 Cr
2+ is stronger reducing agent than Fe
2+
Reason: d
4 d
3 occurs in case of Cr
2+ to Cr
3+
But d
6 d
5 occurs in case of Fe
2+ to Fe
3+
In a medium (like water) d
3 is more stable as compared to d
5 (see CFSE)
4 |
1 | 4514-4517 | 6 Because of small size and high electronegativity oxygen or fluorine can
oxidise the metal to its highest oxidation state 4 7 Cr
2+ is stronger reducing agent than Fe
2+
Reason: d
4 d
3 occurs in case of Cr
2+ to Cr
3+
But d
6 d
5 occurs in case of Fe
2+ to Fe
3+
In a medium (like water) d
3 is more stable as compared to d
5 (see CFSE)
4 9 Cu
2Cu+ in aqueous solution underoes disproportionation, i |
1 | 4515-4518 | 4 7 Cr
2+ is stronger reducing agent than Fe
2+
Reason: d
4 d
3 occurs in case of Cr
2+ to Cr
3+
But d
6 d
5 occurs in case of Fe
2+ to Fe
3+
In a medium (like water) d
3 is more stable as compared to d
5 (see CFSE)
4 9 Cu
2Cu+ in aqueous solution underoes disproportionation, i e |
1 | 4516-4519 | 7 Cr
2+ is stronger reducing agent than Fe
2+
Reason: d
4 d
3 occurs in case of Cr
2+ to Cr
3+
But d
6 d
5 occurs in case of Fe
2+ to Fe
3+
In a medium (like water) d
3 is more stable as compared to d
5 (see CFSE)
4 9 Cu
2Cu+ in aqueous solution underoes disproportionation, i e ,
+(aq) ® Cu
2+(aq) + Cu(s)
The E
0 value for this is favourable |
1 | 4517-4520 | 9 Cu
2Cu+ in aqueous solution underoes disproportionation, i e ,
+(aq) ® Cu
2+(aq) + Cu(s)
The E
0 value for this is favourable 4 |
1 | 4518-4521 | e ,
+(aq) ® Cu
2+(aq) + Cu(s)
The E
0 value for this is favourable 4 10 The 5f electrons are more effectively shielded from nuclear charge |
1 | 4519-4522 | ,
+(aq) ® Cu
2+(aq) + Cu(s)
The E
0 value for this is favourable 4 10 The 5f electrons are more effectively shielded from nuclear charge In other
words the 5f electrons themselves provide poor shielding from element to
element in the series |
1 | 4520-4523 | 4 10 The 5f electrons are more effectively shielded from nuclear charge In other
words the 5f electrons themselves provide poor shielding from element to
element in the series 4 |
1 | 4521-4524 | 10 The 5f electrons are more effectively shielded from nuclear charge In other
words the 5f electrons themselves provide poor shielding from element to
element in the series 4 31
Use Hund’s rule to derive the electronic configuration of Ce
3+ ion, and calculate
its magnetic moment on the basis of ‘spin-only’ formula |
1 | 4522-4525 | In other
words the 5f electrons themselves provide poor shielding from element to
element in the series 4 31
Use Hund’s rule to derive the electronic configuration of Ce
3+ ion, and calculate
its magnetic moment on the basis of ‘spin-only’ formula 4 |
1 | 4523-4526 | 4 31
Use Hund’s rule to derive the electronic configuration of Ce
3+ ion, and calculate
its magnetic moment on the basis of ‘spin-only’ formula 4 32
Name the members of the lanthanoid series which exhibit +4 oxidation states
and those which exhibit +2 oxidation states |
1 | 4524-4527 | 31
Use Hund’s rule to derive the electronic configuration of Ce
3+ ion, and calculate
its magnetic moment on the basis of ‘spin-only’ formula 4 32
Name the members of the lanthanoid series which exhibit +4 oxidation states
and those which exhibit +2 oxidation states Try to correlate this type of
behaviour with the electronic configurations of these elements |
1 | 4525-4528 | 4 32
Name the members of the lanthanoid series which exhibit +4 oxidation states
and those which exhibit +2 oxidation states Try to correlate this type of
behaviour with the electronic configurations of these elements 4 |
1 | 4526-4529 | 32
Name the members of the lanthanoid series which exhibit +4 oxidation states
and those which exhibit +2 oxidation states Try to correlate this type of
behaviour with the electronic configurations of these elements 4 33
Compare the chemistry of the actinoids with that of lanthanoids with reference to:
(i) electronic configuration (ii) oxidation states and (iii) chemical reactivity |
1 | 4527-4530 | Try to correlate this type of
behaviour with the electronic configurations of these elements 4 33
Compare the chemistry of the actinoids with that of lanthanoids with reference to:
(i) electronic configuration (ii) oxidation states and (iii) chemical reactivity 4 |
1 | 4528-4531 | 4 33
Compare the chemistry of the actinoids with that of lanthanoids with reference to:
(i) electronic configuration (ii) oxidation states and (iii) chemical reactivity 4 34
Write the electronic configurations of the elements with the atomic numbers
61, 91, 101, and 109 |
1 | 4529-4532 | 33
Compare the chemistry of the actinoids with that of lanthanoids with reference to:
(i) electronic configuration (ii) oxidation states and (iii) chemical reactivity 4 34
Write the electronic configurations of the elements with the atomic numbers
61, 91, 101, and 109 4 |
1 | 4530-4533 | 4 34
Write the electronic configurations of the elements with the atomic numbers
61, 91, 101, and 109 4 35
Compare the general characteristics of the first series of the transition metals
with those of the second and third series metals in the respective vertical
columns |
1 | 4531-4534 | 34
Write the electronic configurations of the elements with the atomic numbers
61, 91, 101, and 109 4 35
Compare the general characteristics of the first series of the transition metals
with those of the second and third series metals in the respective vertical
columns Give special emphasis on the following points:
(i) electronic configurations (ii) oxidation states (iii) ionisation enthalpies
and (iv) atomic sizes |
1 | 4532-4535 | 4 35
Compare the general characteristics of the first series of the transition metals
with those of the second and third series metals in the respective vertical
columns Give special emphasis on the following points:
(i) electronic configurations (ii) oxidation states (iii) ionisation enthalpies
and (iv) atomic sizes 4 |
1 | 4533-4536 | 35
Compare the general characteristics of the first series of the transition metals
with those of the second and third series metals in the respective vertical
columns Give special emphasis on the following points:
(i) electronic configurations (ii) oxidation states (iii) ionisation enthalpies
and (iv) atomic sizes 4 36
Write down the number of 3d electrons in each of the following ions: Ti
2+, V
2+,
Cr
3+, Mn
2+, Fe
2+, Fe
3+, Co
2+, Ni
2+ and Cu
2+ |
1 | 4534-4537 | Give special emphasis on the following points:
(i) electronic configurations (ii) oxidation states (iii) ionisation enthalpies
and (iv) atomic sizes 4 36
Write down the number of 3d electrons in each of the following ions: Ti
2+, V
2+,
Cr
3+, Mn
2+, Fe
2+, Fe
3+, Co
2+, Ni
2+ and Cu
2+ Indicate how would you expect the five
3d orbitals to be occupied for these hydrated ions (octahedral) |
1 | 4535-4538 | 4 36
Write down the number of 3d electrons in each of the following ions: Ti
2+, V
2+,
Cr
3+, Mn
2+, Fe
2+, Fe
3+, Co
2+, Ni
2+ and Cu
2+ Indicate how would you expect the five
3d orbitals to be occupied for these hydrated ions (octahedral) 4 |
1 | 4536-4539 | 36
Write down the number of 3d electrons in each of the following ions: Ti
2+, V
2+,
Cr
3+, Mn
2+, Fe
2+, Fe
3+, Co
2+, Ni
2+ and Cu
2+ Indicate how would you expect the five
3d orbitals to be occupied for these hydrated ions (octahedral) 4 37
Comment on the statement that elements of the first transition series possess
many properties different from those of heavier transition elements |
1 | 4537-4540 | Indicate how would you expect the five
3d orbitals to be occupied for these hydrated ions (octahedral) 4 37
Comment on the statement that elements of the first transition series possess
many properties different from those of heavier transition elements 4 |
1 | 4538-4541 | 4 37
Comment on the statement that elements of the first transition series possess
many properties different from those of heavier transition elements 4 38
What can be inferred from the magnetic moment values of the following complex
species |
1 | 4539-4542 | 37
Comment on the statement that elements of the first transition series possess
many properties different from those of heavier transition elements 4 38
What can be inferred from the magnetic moment values of the following complex
species Example
Magnetic Moment (BM)
K4[Mn(CN)6)
2 |
1 | 4540-4543 | 4 38
What can be inferred from the magnetic moment values of the following complex
species Example
Magnetic Moment (BM)
K4[Mn(CN)6)
2 2
[Fe(H2O)6]
2+
5 |
1 | 4541-4544 | 38
What can be inferred from the magnetic moment values of the following complex
species Example
Magnetic Moment (BM)
K4[Mn(CN)6)
2 2
[Fe(H2O)6]
2+
5 3
K2[MnCl4]
5 |
1 | 4542-4545 | Example
Magnetic Moment (BM)
K4[Mn(CN)6)
2 2
[Fe(H2O)6]
2+
5 3
K2[MnCl4]
5 9
Rationalised 2023-24
118
Chemistry
In the previous Unit we learnt that the transition metals
form a large number of complex compounds in which
the metal atoms are bound to a number of anions or
neutral molecules by sharing of electrons |
1 | 4543-4546 | 2
[Fe(H2O)6]
2+
5 3
K2[MnCl4]
5 9
Rationalised 2023-24
118
Chemistry
In the previous Unit we learnt that the transition metals
form a large number of complex compounds in which
the metal atoms are bound to a number of anions or
neutral molecules by sharing of electrons In modern
terminology such compounds are called coordination
compounds |
1 | 4544-4547 | 3
K2[MnCl4]
5 9
Rationalised 2023-24
118
Chemistry
In the previous Unit we learnt that the transition metals
form a large number of complex compounds in which
the metal atoms are bound to a number of anions or
neutral molecules by sharing of electrons In modern
terminology such compounds are called coordination
compounds The chemistry of coordination compounds
is an important and challenging area of modern
inorganic chemistry |
1 | 4545-4548 | 9
Rationalised 2023-24
118
Chemistry
In the previous Unit we learnt that the transition metals
form a large number of complex compounds in which
the metal atoms are bound to a number of anions or
neutral molecules by sharing of electrons In modern
terminology such compounds are called coordination
compounds The chemistry of coordination compounds
is an important and challenging area of modern
inorganic chemistry New concepts of chemical bonding
and molecular structure have provided insights into
the functioning of these compounds as vital components
of biological systems |
1 | 4546-4549 | In modern
terminology such compounds are called coordination
compounds The chemistry of coordination compounds
is an important and challenging area of modern
inorganic chemistry New concepts of chemical bonding
and molecular structure have provided insights into
the functioning of these compounds as vital components
of biological systems Chlorophyll, haemoglobin and
vitamin B12 are coordination compounds of magnesium,
iron and cobalt respectively |
1 | 4547-4550 | The chemistry of coordination compounds
is an important and challenging area of modern
inorganic chemistry New concepts of chemical bonding
and molecular structure have provided insights into
the functioning of these compounds as vital components
of biological systems Chlorophyll, haemoglobin and
vitamin B12 are coordination compounds of magnesium,
iron and cobalt respectively Variety of metallurgical
processes, industrial catalysts and analytical reagents
involve
the
use
of
coordination
compounds |
1 | 4548-4551 | New concepts of chemical bonding
and molecular structure have provided insights into
the functioning of these compounds as vital components
of biological systems Chlorophyll, haemoglobin and
vitamin B12 are coordination compounds of magnesium,
iron and cobalt respectively Variety of metallurgical
processes, industrial catalysts and analytical reagents
involve
the
use
of
coordination
compounds Coordination compounds also find many applications
in electroplating, textile dyeing and medicinal chemistry |
1 | 4549-4552 | Chlorophyll, haemoglobin and
vitamin B12 are coordination compounds of magnesium,
iron and cobalt respectively Variety of metallurgical
processes, industrial catalysts and analytical reagents
involve
the
use
of
coordination
compounds Coordination compounds also find many applications
in electroplating, textile dyeing and medicinal chemistry Coordination
Compounds
After studying this Unit, you will be
•able to
appreciate
the
postulates
of
Werner’s theory of coordination
compounds;
•
know the meaning of the terms:
coordination entity, central atom/
ion, ligand, coordination number,
coordination sphere, coordination
polyhedron, oxidation number,
homoleptic and heteroleptic;
•
learn the rules of nomenclature
of coordination compounds;
•
write the formulas and names
of
mononuclear
coordination
compounds;
•
define different types of isomerism
in coordination compounds;
•
understand the nature of bonding
in coordination compounds in
terms of the Valence Bond and
Crystal Field theories;
•
appreciate the importance and
applications
of
coordination
compounds in our day to day life |
1 | 4550-4553 | Variety of metallurgical
processes, industrial catalysts and analytical reagents
involve
the
use
of
coordination
compounds Coordination compounds also find many applications
in electroplating, textile dyeing and medicinal chemistry Coordination
Compounds
After studying this Unit, you will be
•able to
appreciate
the
postulates
of
Werner’s theory of coordination
compounds;
•
know the meaning of the terms:
coordination entity, central atom/
ion, ligand, coordination number,
coordination sphere, coordination
polyhedron, oxidation number,
homoleptic and heteroleptic;
•
learn the rules of nomenclature
of coordination compounds;
•
write the formulas and names
of
mononuclear
coordination
compounds;
•
define different types of isomerism
in coordination compounds;
•
understand the nature of bonding
in coordination compounds in
terms of the Valence Bond and
Crystal Field theories;
•
appreciate the importance and
applications
of
coordination
compounds in our day to day life Objectives
Coordination Compounds are the backbone of modern inorganic
and bio–inorganic chemistry and chemical industry |
1 | 4551-4554 | Coordination compounds also find many applications
in electroplating, textile dyeing and medicinal chemistry Coordination
Compounds
After studying this Unit, you will be
•able to
appreciate
the
postulates
of
Werner’s theory of coordination
compounds;
•
know the meaning of the terms:
coordination entity, central atom/
ion, ligand, coordination number,
coordination sphere, coordination
polyhedron, oxidation number,
homoleptic and heteroleptic;
•
learn the rules of nomenclature
of coordination compounds;
•
write the formulas and names
of
mononuclear
coordination
compounds;
•
define different types of isomerism
in coordination compounds;
•
understand the nature of bonding
in coordination compounds in
terms of the Valence Bond and
Crystal Field theories;
•
appreciate the importance and
applications
of
coordination
compounds in our day to day life Objectives
Coordination Compounds are the backbone of modern inorganic
and bio–inorganic chemistry and chemical industry Coordination
Compounds
Alfred Werner (1866-1919), a Swiss chemist was the first to formulate
his ideas about the structures of coordination compounds |
1 | 4552-4555 | Coordination
Compounds
After studying this Unit, you will be
•able to
appreciate
the
postulates
of
Werner’s theory of coordination
compounds;
•
know the meaning of the terms:
coordination entity, central atom/
ion, ligand, coordination number,
coordination sphere, coordination
polyhedron, oxidation number,
homoleptic and heteroleptic;
•
learn the rules of nomenclature
of coordination compounds;
•
write the formulas and names
of
mononuclear
coordination
compounds;
•
define different types of isomerism
in coordination compounds;
•
understand the nature of bonding
in coordination compounds in
terms of the Valence Bond and
Crystal Field theories;
•
appreciate the importance and
applications
of
coordination
compounds in our day to day life Objectives
Coordination Compounds are the backbone of modern inorganic
and bio–inorganic chemistry and chemical industry Coordination
Compounds
Alfred Werner (1866-1919), a Swiss chemist was the first to formulate
his ideas about the structures of coordination compounds He prepared
and characterised a large number of coordination compounds and
studied their physical and chemical behaviour by simple experimental
techniques |
1 | 4553-4556 | Objectives
Coordination Compounds are the backbone of modern inorganic
and bio–inorganic chemistry and chemical industry Coordination
Compounds
Alfred Werner (1866-1919), a Swiss chemist was the first to formulate
his ideas about the structures of coordination compounds He prepared
and characterised a large number of coordination compounds and
studied their physical and chemical behaviour by simple experimental
techniques Werner proposed the concept of a primary valence and
a secondary valence for a metal ion |
1 | 4554-4557 | Coordination
Compounds
Alfred Werner (1866-1919), a Swiss chemist was the first to formulate
his ideas about the structures of coordination compounds He prepared
and characterised a large number of coordination compounds and
studied their physical and chemical behaviour by simple experimental
techniques Werner proposed the concept of a primary valence and
a secondary valence for a metal ion Binary compounds such as
CrCl3, CoCl2 or PdCl2 have primary valence of 3, 2 and 2 respectively |
1 | 4555-4558 | He prepared
and characterised a large number of coordination compounds and
studied their physical and chemical behaviour by simple experimental
techniques Werner proposed the concept of a primary valence and
a secondary valence for a metal ion Binary compounds such as
CrCl3, CoCl2 or PdCl2 have primary valence of 3, 2 and 2 respectively In a series of compounds of cobalt(III) chloride with ammonia, it was
found that some of the chloride ions could be precipitated as AgCl on
adding excess silver nitrate solution in cold but some remained in
solution |
1 | 4556-4559 | Werner proposed the concept of a primary valence and
a secondary valence for a metal ion Binary compounds such as
CrCl3, CoCl2 or PdCl2 have primary valence of 3, 2 and 2 respectively In a series of compounds of cobalt(III) chloride with ammonia, it was
found that some of the chloride ions could be precipitated as AgCl on
adding excess silver nitrate solution in cold but some remained in
solution 5 |
1 | 4557-4560 | Binary compounds such as
CrCl3, CoCl2 or PdCl2 have primary valence of 3, 2 and 2 respectively In a series of compounds of cobalt(III) chloride with ammonia, it was
found that some of the chloride ions could be precipitated as AgCl on
adding excess silver nitrate solution in cold but some remained in
solution 5 1
5 |
1 | 4558-4561 | In a series of compounds of cobalt(III) chloride with ammonia, it was
found that some of the chloride ions could be precipitated as AgCl on
adding excess silver nitrate solution in cold but some remained in
solution 5 1
5 1
5 |
1 | 4559-4562 | 5 1
5 1
5 1
5 |
1 | 4560-4563 | 1
5 1
5 1
5 1
5 |
1 | 4561-4564 | 1
5 1
5 1
5 1
Werner’
Werner’
Werner’
Werner’
Werner’sssss
Theory of
Theory of
Theory of
Theory of
Theory of
Coordination
Coordination
Coordination
Coordination
Coordination
Compounds
Compounds
Compounds
Compounds
Compounds
5
Unit
Unit
Unit
Unit
Unit5
Rationalised 2023-24
119
Coordination Compounds
1 mol
CoCl3 |
1 | 4562-4565 | 1
5 1
5 1
Werner’
Werner’
Werner’
Werner’
Werner’sssss
Theory of
Theory of
Theory of
Theory of
Theory of
Coordination
Coordination
Coordination
Coordination
Coordination
Compounds
Compounds
Compounds
Compounds
Compounds
5
Unit
Unit
Unit
Unit
Unit5
Rationalised 2023-24
119
Coordination Compounds
1 mol
CoCl3 6NH3 (Yellow)
gave
3 mol AgCl
1 mol
CoCl3 |
1 | 4563-4566 | 1
5 1
Werner’
Werner’
Werner’
Werner’
Werner’sssss
Theory of
Theory of
Theory of
Theory of
Theory of
Coordination
Coordination
Coordination
Coordination
Coordination
Compounds
Compounds
Compounds
Compounds
Compounds
5
Unit
Unit
Unit
Unit
Unit5
Rationalised 2023-24
119
Coordination Compounds
1 mol
CoCl3 6NH3 (Yellow)
gave
3 mol AgCl
1 mol
CoCl3 5NH3 (Purple)
gave
2 mol AgCl
1 mol
CoCl3 |
1 | 4564-4567 | 1
Werner’
Werner’
Werner’
Werner’
Werner’sssss
Theory of
Theory of
Theory of
Theory of
Theory of
Coordination
Coordination
Coordination
Coordination
Coordination
Compounds
Compounds
Compounds
Compounds
Compounds
5
Unit
Unit
Unit
Unit
Unit5
Rationalised 2023-24
119
Coordination Compounds
1 mol
CoCl3 6NH3 (Yellow)
gave
3 mol AgCl
1 mol
CoCl3 5NH3 (Purple)
gave
2 mol AgCl
1 mol
CoCl3 4NH3 (Green)
gave
1 mol AgCl
1 mol
CoCl3 |
1 | 4565-4568 | 6NH3 (Yellow)
gave
3 mol AgCl
1 mol
CoCl3 5NH3 (Purple)
gave
2 mol AgCl
1 mol
CoCl3 4NH3 (Green)
gave
1 mol AgCl
1 mol
CoCl3 4NH3 (Violet)
gave
1 mol AgCl
These observations, together with the results of conductivity
measurements in solution can be explained if (i) six groups in all,
either chloride ions or ammonia molecules or both, remain bonded to
the cobalt ion during the reaction and (ii) the compounds are formulated
as shown in Table 5 |
1 | 4566-4569 | 5NH3 (Purple)
gave
2 mol AgCl
1 mol
CoCl3 4NH3 (Green)
gave
1 mol AgCl
1 mol
CoCl3 4NH3 (Violet)
gave
1 mol AgCl
These observations, together with the results of conductivity
measurements in solution can be explained if (i) six groups in all,
either chloride ions or ammonia molecules or both, remain bonded to
the cobalt ion during the reaction and (ii) the compounds are formulated
as shown in Table 5 1, where the atoms within the square brackets
form a single entity which does not dissociate under the reaction
conditions |
1 | 4567-4570 | 4NH3 (Green)
gave
1 mol AgCl
1 mol
CoCl3 4NH3 (Violet)
gave
1 mol AgCl
These observations, together with the results of conductivity
measurements in solution can be explained if (i) six groups in all,
either chloride ions or ammonia molecules or both, remain bonded to
the cobalt ion during the reaction and (ii) the compounds are formulated
as shown in Table 5 1, where the atoms within the square brackets
form a single entity which does not dissociate under the reaction
conditions Werner proposed the term secondary valence for the
number of groups bound directly to the metal ion; in each of these
examples the secondary valences are six |
1 | 4568-4571 | 4NH3 (Violet)
gave
1 mol AgCl
These observations, together with the results of conductivity
measurements in solution can be explained if (i) six groups in all,
either chloride ions or ammonia molecules or both, remain bonded to
the cobalt ion during the reaction and (ii) the compounds are formulated
as shown in Table 5 1, where the atoms within the square brackets
form a single entity which does not dissociate under the reaction
conditions Werner proposed the term secondary valence for the
number of groups bound directly to the metal ion; in each of these
examples the secondary valences are six Note that the last two compounds in Table 5 |
1 | 4569-4572 | 1, where the atoms within the square brackets
form a single entity which does not dissociate under the reaction
conditions Werner proposed the term secondary valence for the
number of groups bound directly to the metal ion; in each of these
examples the secondary valences are six Note that the last two compounds in Table 5 1 have identical empirical
formula, CoCl3 |
1 | 4570-4573 | Werner proposed the term secondary valence for the
number of groups bound directly to the metal ion; in each of these
examples the secondary valences are six Note that the last two compounds in Table 5 1 have identical empirical
formula, CoCl3 4NH3, but distinct properties |
1 | 4571-4574 | Note that the last two compounds in Table 5 1 have identical empirical
formula, CoCl3 4NH3, but distinct properties Such compounds are
termed as isomers |
1 | 4572-4575 | 1 have identical empirical
formula, CoCl3 4NH3, but distinct properties Such compounds are
termed as isomers Werner in 1898, propounded his theory of
coordination compounds |
1 | 4573-4576 | 4NH3, but distinct properties Such compounds are
termed as isomers Werner in 1898, propounded his theory of
coordination compounds The main postulates are:
1 |
1 | 4574-4577 | Such compounds are
termed as isomers Werner in 1898, propounded his theory of
coordination compounds The main postulates are:
1 In coordination compounds metals show two types of linkages
(valences)-primary and secondary |
1 | 4575-4578 | Werner in 1898, propounded his theory of
coordination compounds The main postulates are:
1 In coordination compounds metals show two types of linkages
(valences)-primary and secondary 2 |
1 | 4576-4579 | The main postulates are:
1 In coordination compounds metals show two types of linkages
(valences)-primary and secondary 2 The primary valences are normally ionisable and are satisfied by
negative ions |
1 | 4577-4580 | In coordination compounds metals show two types of linkages
(valences)-primary and secondary 2 The primary valences are normally ionisable and are satisfied by
negative ions 3 |
1 | 4578-4581 | 2 The primary valences are normally ionisable and are satisfied by
negative ions 3 The secondary valences are non ionisable |
1 | 4579-4582 | The primary valences are normally ionisable and are satisfied by
negative ions 3 The secondary valences are non ionisable These are satisfied by
neutral molecules or negative ions |
1 | 4580-4583 | 3 The secondary valences are non ionisable These are satisfied by
neutral molecules or negative ions The secondary valence is equal to
the coordination number and is fixed for a metal |
1 | 4581-4584 | The secondary valences are non ionisable These are satisfied by
neutral molecules or negative ions The secondary valence is equal to
the coordination number and is fixed for a metal 4 |
1 | 4582-4585 | These are satisfied by
neutral molecules or negative ions The secondary valence is equal to
the coordination number and is fixed for a metal 4 The ions/groups bound by the secondary linkages to the metal have
characteristic spatial arrangements corresponding to different
coordination numbers |
1 | 4583-4586 | The secondary valence is equal to
the coordination number and is fixed for a metal 4 The ions/groups bound by the secondary linkages to the metal have
characteristic spatial arrangements corresponding to different
coordination numbers In modern formulations, such spatial arrangements are called
coordination polyhedra |
1 | 4584-4587 | 4 The ions/groups bound by the secondary linkages to the metal have
characteristic spatial arrangements corresponding to different
coordination numbers In modern formulations, such spatial arrangements are called
coordination polyhedra The species within the square bracket are
coordination entities or complexes and the ions outside the square
bracket are called counter ions |
1 | 4585-4588 | The ions/groups bound by the secondary linkages to the metal have
characteristic spatial arrangements corresponding to different
coordination numbers In modern formulations, such spatial arrangements are called
coordination polyhedra The species within the square bracket are
coordination entities or complexes and the ions outside the square
bracket are called counter ions He further postulated that octahedral, tetrahedral and square planar
geometrical shapes are more common in coordination compounds of
transition metals |
1 | 4586-4589 | In modern formulations, such spatial arrangements are called
coordination polyhedra The species within the square bracket are
coordination entities or complexes and the ions outside the square
bracket are called counter ions He further postulated that octahedral, tetrahedral and square planar
geometrical shapes are more common in coordination compounds of
transition metals Thus, [Co(NH3)6]
3+, [CoCl(NH3)5]
2+ and [CoCl2(NH3)4]
+
are octahedral entities, while [Ni(CO)4] and [PtCl4]
2– are tetrahedral and
square planar, respectively |
1 | 4587-4590 | The species within the square bracket are
coordination entities or complexes and the ions outside the square
bracket are called counter ions He further postulated that octahedral, tetrahedral and square planar
geometrical shapes are more common in coordination compounds of
transition metals Thus, [Co(NH3)6]
3+, [CoCl(NH3)5]
2+ and [CoCl2(NH3)4]
+
are octahedral entities, while [Ni(CO)4] and [PtCl4]
2– are tetrahedral and
square planar, respectively Colour
Formula
Solution conductivity
corresponds to
Table 5 |
1 | 4588-4591 | He further postulated that octahedral, tetrahedral and square planar
geometrical shapes are more common in coordination compounds of
transition metals Thus, [Co(NH3)6]
3+, [CoCl(NH3)5]
2+ and [CoCl2(NH3)4]
+
are octahedral entities, while [Ni(CO)4] and [PtCl4]
2– are tetrahedral and
square planar, respectively Colour
Formula
Solution conductivity
corresponds to
Table 5 1: Formulation of Cobalt(III) Chloride-Ammonia Complexes
Yellow
[Co(NH3)6]
3+3Cl
–
1:3 electrolyte
Purple
[CoCl(NH3)5]
2+2Cl
–
1:2 electrolyte
Green
[CoCl2(NH3)4]
+Cl
–
1:1 electrolyte
Violet
[CoCl2(NH3)4]
+Cl
–
1:1 electrolyte
Rationalised 2023-24
120
Chemistry
(i) Secondary 4
(ii) Secondary 6
(iii) Secondary 6
(iv) Secondary 6
(v) Secondary 4
On the basis of the following observations made with aqueous solutions,
assign secondary valences to metals in the following compounds:
Solution
Solution
Solution
Solution
Solution
Difference between a double salt and a complex
Both double salts as well as complexes are formed by the combination
of two or more stable compounds in stoichiometric ratio |
1 | 4589-4592 | Thus, [Co(NH3)6]
3+, [CoCl(NH3)5]
2+ and [CoCl2(NH3)4]
+
are octahedral entities, while [Ni(CO)4] and [PtCl4]
2– are tetrahedral and
square planar, respectively Colour
Formula
Solution conductivity
corresponds to
Table 5 1: Formulation of Cobalt(III) Chloride-Ammonia Complexes
Yellow
[Co(NH3)6]
3+3Cl
–
1:3 electrolyte
Purple
[CoCl(NH3)5]
2+2Cl
–
1:2 electrolyte
Green
[CoCl2(NH3)4]
+Cl
–
1:1 electrolyte
Violet
[CoCl2(NH3)4]
+Cl
–
1:1 electrolyte
Rationalised 2023-24
120
Chemistry
(i) Secondary 4
(ii) Secondary 6
(iii) Secondary 6
(iv) Secondary 6
(v) Secondary 4
On the basis of the following observations made with aqueous solutions,
assign secondary valences to metals in the following compounds:
Solution
Solution
Solution
Solution
Solution
Difference between a double salt and a complex
Both double salts as well as complexes are formed by the combination
of two or more stable compounds in stoichiometric ratio However, they
differ in the fact that double salts such as carnallite, KCl |
1 | 4590-4593 | Colour
Formula
Solution conductivity
corresponds to
Table 5 1: Formulation of Cobalt(III) Chloride-Ammonia Complexes
Yellow
[Co(NH3)6]
3+3Cl
–
1:3 electrolyte
Purple
[CoCl(NH3)5]
2+2Cl
–
1:2 electrolyte
Green
[CoCl2(NH3)4]
+Cl
–
1:1 electrolyte
Violet
[CoCl2(NH3)4]
+Cl
–
1:1 electrolyte
Rationalised 2023-24
120
Chemistry
(i) Secondary 4
(ii) Secondary 6
(iii) Secondary 6
(iv) Secondary 6
(v) Secondary 4
On the basis of the following observations made with aqueous solutions,
assign secondary valences to metals in the following compounds:
Solution
Solution
Solution
Solution
Solution
Difference between a double salt and a complex
Both double salts as well as complexes are formed by the combination
of two or more stable compounds in stoichiometric ratio However, they
differ in the fact that double salts such as carnallite, KCl MgCl2 |
1 | 4591-4594 | 1: Formulation of Cobalt(III) Chloride-Ammonia Complexes
Yellow
[Co(NH3)6]
3+3Cl
–
1:3 electrolyte
Purple
[CoCl(NH3)5]
2+2Cl
–
1:2 electrolyte
Green
[CoCl2(NH3)4]
+Cl
–
1:1 electrolyte
Violet
[CoCl2(NH3)4]
+Cl
–
1:1 electrolyte
Rationalised 2023-24
120
Chemistry
(i) Secondary 4
(ii) Secondary 6
(iii) Secondary 6
(iv) Secondary 6
(v) Secondary 4
On the basis of the following observations made with aqueous solutions,
assign secondary valences to metals in the following compounds:
Solution
Solution
Solution
Solution
Solution
Difference between a double salt and a complex
Both double salts as well as complexes are formed by the combination
of two or more stable compounds in stoichiometric ratio However, they
differ in the fact that double salts such as carnallite, KCl MgCl2 6H2O,
Mohr’s salt, FeSO4 |
1 | 4592-4595 | However, they
differ in the fact that double salts such as carnallite, KCl MgCl2 6H2O,
Mohr’s salt, FeSO4 (NH4)2SO4 |
1 | 4593-4596 | MgCl2 6H2O,
Mohr’s salt, FeSO4 (NH4)2SO4 6H2O, potash alum, KAl(SO4)2 |
1 | 4594-4597 | 6H2O,
Mohr’s salt, FeSO4 (NH4)2SO4 6H2O, potash alum, KAl(SO4)2 12H2O, etc |
1 | 4595-4598 | (NH4)2SO4 6H2O, potash alum, KAl(SO4)2 12H2O, etc dissociate into simple ions completely when dissolved in water |
1 | 4596-4599 | 6H2O, potash alum, KAl(SO4)2 12H2O, etc dissociate into simple ions completely when dissolved in water However,
complex ions such as [Fe(CN)6]
4– of K4[Fe(CN)6] do not dissociate into
Fe
2+ and CN
– ions |
1 | 4597-4600 | 12H2O, etc dissociate into simple ions completely when dissolved in water However,
complex ions such as [Fe(CN)6]
4– of K4[Fe(CN)6] do not dissociate into
Fe
2+ and CN
– ions Formula
Moles of AgCl precipitated per mole of
the compounds with excess AgNO3
(i) PdCl2 |
1 | 4598-4601 | dissociate into simple ions completely when dissolved in water However,
complex ions such as [Fe(CN)6]
4– of K4[Fe(CN)6] do not dissociate into
Fe
2+ and CN
– ions Formula
Moles of AgCl precipitated per mole of
the compounds with excess AgNO3
(i) PdCl2 4NH3
2
(ii) NiCl2 |
1 | 4599-4602 | However,
complex ions such as [Fe(CN)6]
4– of K4[Fe(CN)6] do not dissociate into
Fe
2+ and CN
– ions Formula
Moles of AgCl precipitated per mole of
the compounds with excess AgNO3
(i) PdCl2 4NH3
2
(ii) NiCl2 6H2O
2
(iii) PtCl4 |
1 | 4600-4603 | Formula
Moles of AgCl precipitated per mole of
the compounds with excess AgNO3
(i) PdCl2 4NH3
2
(ii) NiCl2 6H2O
2
(iii) PtCl4 2HCl
0
(iv) CoCl3 |
1 | 4601-4604 | 4NH3
2
(ii) NiCl2 6H2O
2
(iii) PtCl4 2HCl
0
(iv) CoCl3 4NH3
1
(v) PtCl2 |
1 | 4602-4605 | 6H2O
2
(iii) PtCl4 2HCl
0
(iv) CoCl3 4NH3
1
(v) PtCl2 2NH3
0
Example 5 |
1 | 4603-4606 | 2HCl
0
(iv) CoCl3 4NH3
1
(v) PtCl2 2NH3
0
Example 5 1
Example 5 |
1 | 4604-4607 | 4NH3
1
(v) PtCl2 2NH3
0
Example 5 1
Example 5 1
Example 5 |
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