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1 | 4005-4008 | Much larger third ionisation energy of Mn (where the required change
is d
5 to d
4) is mainly responsible for this This also explains why the
+3 state of Mn is of little importance 4 3 |
1 | 4006-4009 | This also explains why the
+3 state of Mn is of little importance 4 3 9 Magnetic
Properties
Transition metals vary widely in their chemical reactivity |
1 | 4007-4010 | 4 3 9 Magnetic
Properties
Transition metals vary widely in their chemical reactivity Many of
them are sufficiently electropositive to dissolve in mineral acids, although
a few are ‘noble’—that is, they are unaffected by single acids |
1 | 4008-4011 | 3 9 Magnetic
Properties
Transition metals vary widely in their chemical reactivity Many of
them are sufficiently electropositive to dissolve in mineral acids, although
a few are ‘noble’—that is, they are unaffected by single acids The metals of the first series with the exception of copper are relatively
more reactive and are oxidised by 1M H
+, though the actual rate at
which these metals react with oxidising agents like hydrogen ion (H
+) is
sometimes slow |
1 | 4009-4012 | 9 Magnetic
Properties
Transition metals vary widely in their chemical reactivity Many of
them are sufficiently electropositive to dissolve in mineral acids, although
a few are ‘noble’—that is, they are unaffected by single acids The metals of the first series with the exception of copper are relatively
more reactive and are oxidised by 1M H
+, though the actual rate at
which these metals react with oxidising agents like hydrogen ion (H
+) is
sometimes slow For example, titanium and vanadium, in practice, are
passive to dilute non oxidising acids at room temperature |
1 | 4010-4013 | Many of
them are sufficiently electropositive to dissolve in mineral acids, although
a few are ‘noble’—that is, they are unaffected by single acids The metals of the first series with the exception of copper are relatively
more reactive and are oxidised by 1M H
+, though the actual rate at
which these metals react with oxidising agents like hydrogen ion (H
+) is
sometimes slow For example, titanium and vanadium, in practice, are
passive to dilute non oxidising acids at room temperature The E
o values
for M
2+/M (Table 4 |
1 | 4011-4014 | The metals of the first series with the exception of copper are relatively
more reactive and are oxidised by 1M H
+, though the actual rate at
which these metals react with oxidising agents like hydrogen ion (H
+) is
sometimes slow For example, titanium and vanadium, in practice, are
passive to dilute non oxidising acids at room temperature The E
o values
for M
2+/M (Table 4 2) indicate a decreasing tendency to form divalent
cations across the series |
1 | 4012-4015 | For example, titanium and vanadium, in practice, are
passive to dilute non oxidising acids at room temperature The E
o values
for M
2+/M (Table 4 2) indicate a decreasing tendency to form divalent
cations across the series This general trend towards less negative E
o
values is related to the increase in the sum of the first and second
ionisation enthalpies |
1 | 4013-4016 | The E
o values
for M
2+/M (Table 4 2) indicate a decreasing tendency to form divalent
cations across the series This general trend towards less negative E
o
values is related to the increase in the sum of the first and second
ionisation enthalpies It is interesting to note that the E
o values for Mn,
Ni and Zn are more negative than expected from the general trend |
1 | 4014-4017 | 2) indicate a decreasing tendency to form divalent
cations across the series This general trend towards less negative E
o
values is related to the increase in the sum of the first and second
ionisation enthalpies It is interesting to note that the E
o values for Mn,
Ni and Zn are more negative than expected from the general trend Whereas the stabilities of half-filled d subshell (d
5) in Mn
2+ and completely
filled d subshell (d
10) in zinc are related to their E
e values; for nickel, Eo
value is related to the highest negative enthalpy of hydration |
1 | 4015-4018 | This general trend towards less negative E
o
values is related to the increase in the sum of the first and second
ionisation enthalpies It is interesting to note that the E
o values for Mn,
Ni and Zn are more negative than expected from the general trend Whereas the stabilities of half-filled d subshell (d
5) in Mn
2+ and completely
filled d subshell (d
10) in zinc are related to their E
e values; for nickel, Eo
value is related to the highest negative enthalpy of hydration An examination of the E
o values for the redox couple M
3+/M
2+ (Table
4 |
1 | 4016-4019 | It is interesting to note that the E
o values for Mn,
Ni and Zn are more negative than expected from the general trend Whereas the stabilities of half-filled d subshell (d
5) in Mn
2+ and completely
filled d subshell (d
10) in zinc are related to their E
e values; for nickel, Eo
value is related to the highest negative enthalpy of hydration An examination of the E
o values for the redox couple M
3+/M
2+ (Table
4 2) shows that Mn
3+ and Co
3+ ions are the strongest oxidising agents
in aqueous solutions |
1 | 4017-4020 | Whereas the stabilities of half-filled d subshell (d
5) in Mn
2+ and completely
filled d subshell (d
10) in zinc are related to their E
e values; for nickel, Eo
value is related to the highest negative enthalpy of hydration An examination of the E
o values for the redox couple M
3+/M
2+ (Table
4 2) shows that Mn
3+ and Co
3+ ions are the strongest oxidising agents
in aqueous solutions The ions Ti
2+, V
2+ and Cr
2+ are strong reducing
agents and will liberate hydrogen from a dilute acid, e |
1 | 4018-4021 | An examination of the E
o values for the redox couple M
3+/M
2+ (Table
4 2) shows that Mn
3+ and Co
3+ ions are the strongest oxidising agents
in aqueous solutions The ions Ti
2+, V
2+ and Cr
2+ are strong reducing
agents and will liberate hydrogen from a dilute acid, e g |
1 | 4019-4022 | 2) shows that Mn
3+ and Co
3+ ions are the strongest oxidising agents
in aqueous solutions The ions Ti
2+, V
2+ and Cr
2+ are strong reducing
agents and will liberate hydrogen from a dilute acid, e g ,
2 Cr
2+(aq) + 2 H
+(aq) ® 2 Cr
3+(aq) + H2(g)
4 |
1 | 4020-4023 | The ions Ti
2+, V
2+ and Cr
2+ are strong reducing
agents and will liberate hydrogen from a dilute acid, e g ,
2 Cr
2+(aq) + 2 H
+(aq) ® 2 Cr
3+(aq) + H2(g)
4 3 |
1 | 4021-4024 | g ,
2 Cr
2+(aq) + 2 H
+(aq) ® 2 Cr
3+(aq) + H2(g)
4 3 8 Chemical
Reactivity
and E
o
Values
Example 4 |
1 | 4022-4025 | ,
2 Cr
2+(aq) + 2 H
+(aq) ® 2 Cr
3+(aq) + H2(g)
4 3 8 Chemical
Reactivity
and E
o
Values
Example 4 6
Example 4 |
1 | 4023-4026 | 3 8 Chemical
Reactivity
and E
o
Values
Example 4 6
Example 4 6
Example 4 |
1 | 4024-4027 | 8 Chemical
Reactivity
and E
o
Values
Example 4 6
Example 4 6
Example 4 6
Example 4 |
1 | 4025-4028 | 6
Example 4 6
Example 4 6
Example 4 6
Example 4 |
1 | 4026-4029 | 6
Example 4 6
Example 4 6
Example 4 6
Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
4 |
1 | 4027-4030 | 6
Example 4 6
Example 4 6
Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
4 6 Why is the highest oxidation state of a metal exhibited in its oxide or
fluoride only |
1 | 4028-4031 | 6
Example 4 6
Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
4 6 Why is the highest oxidation state of a metal exhibited in its oxide or
fluoride only 4 |
1 | 4029-4032 | 6
Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
4 6 Why is the highest oxidation state of a metal exhibited in its oxide or
fluoride only 4 7 Which is a stronger reducing agent Cr
2+ or Fe
2+ and why |
1 | 4030-4033 | 6 Why is the highest oxidation state of a metal exhibited in its oxide or
fluoride only 4 7 Which is a stronger reducing agent Cr
2+ or Fe
2+ and why When a magnetic field is applied to substances, mainly two types of
magnetic behaviour are observed: diamagnetism and paramagnetism |
1 | 4031-4034 | 4 7 Which is a stronger reducing agent Cr
2+ or Fe
2+ and why When a magnetic field is applied to substances, mainly two types of
magnetic behaviour are observed: diamagnetism and paramagnetism Diamagnetic substances are repelled by the applied field while the
paramagnetic substances are attracted |
1 | 4032-4035 | 7 Which is a stronger reducing agent Cr
2+ or Fe
2+ and why When a magnetic field is applied to substances, mainly two types of
magnetic behaviour are observed: diamagnetism and paramagnetism Diamagnetic substances are repelled by the applied field while the
paramagnetic substances are attracted Substances which are
Solution
Solution
Solution
Solution
Solution
Example 4 |
1 | 4033-4036 | When a magnetic field is applied to substances, mainly two types of
magnetic behaviour are observed: diamagnetism and paramagnetism Diamagnetic substances are repelled by the applied field while the
paramagnetic substances are attracted Substances which are
Solution
Solution
Solution
Solution
Solution
Example 4 7
Example 4 |
1 | 4034-4037 | Diamagnetic substances are repelled by the applied field while the
paramagnetic substances are attracted Substances which are
Solution
Solution
Solution
Solution
Solution
Example 4 7
Example 4 7
Example 4 |
1 | 4035-4038 | Substances which are
Solution
Solution
Solution
Solution
Solution
Example 4 7
Example 4 7
Example 4 7
Example 4 |
1 | 4036-4039 | 7
Example 4 7
Example 4 7
Example 4 7
Example 4 |
1 | 4037-4040 | 7
Example 4 7
Example 4 7
Example 4 7
Solution
Solution
Solution
Solution
Solution
Rationalised 2023-24
102
Chemistry
attracted very strongly are said to be ferromagnetic |
1 | 4038-4041 | 7
Example 4 7
Example 4 7
Solution
Solution
Solution
Solution
Solution
Rationalised 2023-24
102
Chemistry
attracted very strongly are said to be ferromagnetic In fact,
ferromagnetism is an extreme form of paramagnetism |
1 | 4039-4042 | 7
Example 4 7
Solution
Solution
Solution
Solution
Solution
Rationalised 2023-24
102
Chemistry
attracted very strongly are said to be ferromagnetic In fact,
ferromagnetism is an extreme form of paramagnetism Many of the
transition metal ions are paramagnetic |
1 | 4040-4043 | 7
Solution
Solution
Solution
Solution
Solution
Rationalised 2023-24
102
Chemistry
attracted very strongly are said to be ferromagnetic In fact,
ferromagnetism is an extreme form of paramagnetism Many of the
transition metal ions are paramagnetic Paramagnetism arises from the presence of unpaired electrons, each
such electron having a magnetic moment associated with its spin angular
momentum and orbital angular momentum |
1 | 4041-4044 | In fact,
ferromagnetism is an extreme form of paramagnetism Many of the
transition metal ions are paramagnetic Paramagnetism arises from the presence of unpaired electrons, each
such electron having a magnetic moment associated with its spin angular
momentum and orbital angular momentum For the compounds of the
first series of transition metals, the contribution of the orbital angular
momentum is effectively quenched and hence is of no significance |
1 | 4042-4045 | Many of the
transition metal ions are paramagnetic Paramagnetism arises from the presence of unpaired electrons, each
such electron having a magnetic moment associated with its spin angular
momentum and orbital angular momentum For the compounds of the
first series of transition metals, the contribution of the orbital angular
momentum is effectively quenched and hence is of no significance For
these, the magnetic moment is determined by the number of unpaired
electrons and is calculated by using the ‘spin-only’ formula, i |
1 | 4043-4046 | Paramagnetism arises from the presence of unpaired electrons, each
such electron having a magnetic moment associated with its spin angular
momentum and orbital angular momentum For the compounds of the
first series of transition metals, the contribution of the orbital angular
momentum is effectively quenched and hence is of no significance For
these, the magnetic moment is determined by the number of unpaired
electrons and is calculated by using the ‘spin-only’ formula, i e |
1 | 4044-4047 | For the compounds of the
first series of transition metals, the contribution of the orbital angular
momentum is effectively quenched and hence is of no significance For
these, the magnetic moment is determined by the number of unpaired
electrons and is calculated by using the ‘spin-only’ formula, i e ,
n n
2
where n is the number of unpaired electrons and µ is the magnetic
moment in units of Bohr magneton (BM) |
1 | 4045-4048 | For
these, the magnetic moment is determined by the number of unpaired
electrons and is calculated by using the ‘spin-only’ formula, i e ,
n n
2
where n is the number of unpaired electrons and µ is the magnetic
moment in units of Bohr magneton (BM) A single unpaired electron
has a magnetic moment of 1 |
1 | 4046-4049 | e ,
n n
2
where n is the number of unpaired electrons and µ is the magnetic
moment in units of Bohr magneton (BM) A single unpaired electron
has a magnetic moment of 1 73 Bohr magnetons (BM) |
1 | 4047-4050 | ,
n n
2
where n is the number of unpaired electrons and µ is the magnetic
moment in units of Bohr magneton (BM) A single unpaired electron
has a magnetic moment of 1 73 Bohr magnetons (BM) The magnetic moment increases with the increasing number of
unpaired electrons |
1 | 4048-4051 | A single unpaired electron
has a magnetic moment of 1 73 Bohr magnetons (BM) The magnetic moment increases with the increasing number of
unpaired electrons Thus, the observed magnetic moment gives a useful
indication about the number of unpaired electrons present in the atom,
molecule or ion |
1 | 4049-4052 | 73 Bohr magnetons (BM) The magnetic moment increases with the increasing number of
unpaired electrons Thus, the observed magnetic moment gives a useful
indication about the number of unpaired electrons present in the atom,
molecule or ion The magnetic moments calculated from the ‘spin-only’
formula and those derived experimentally for some ions of the first row
transition elements are given in Table 4 |
1 | 4050-4053 | The magnetic moment increases with the increasing number of
unpaired electrons Thus, the observed magnetic moment gives a useful
indication about the number of unpaired electrons present in the atom,
molecule or ion The magnetic moments calculated from the ‘spin-only’
formula and those derived experimentally for some ions of the first row
transition elements are given in Table 4 7 |
1 | 4051-4054 | Thus, the observed magnetic moment gives a useful
indication about the number of unpaired electrons present in the atom,
molecule or ion The magnetic moments calculated from the ‘spin-only’
formula and those derived experimentally for some ions of the first row
transition elements are given in Table 4 7 The experimental data are
mainly for hydrated ions in solution or in the solid state |
1 | 4052-4055 | The magnetic moments calculated from the ‘spin-only’
formula and those derived experimentally for some ions of the first row
transition elements are given in Table 4 7 The experimental data are
mainly for hydrated ions in solution or in the solid state Sc
3+
3d
0
0
0
0
Ti
3+
3d
1
1
1 |
1 | 4053-4056 | 7 The experimental data are
mainly for hydrated ions in solution or in the solid state Sc
3+
3d
0
0
0
0
Ti
3+
3d
1
1
1 73
1 |
1 | 4054-4057 | The experimental data are
mainly for hydrated ions in solution or in the solid state Sc
3+
3d
0
0
0
0
Ti
3+
3d
1
1
1 73
1 75
Tl
2+
3d
2
2
2 |
1 | 4055-4058 | Sc
3+
3d
0
0
0
0
Ti
3+
3d
1
1
1 73
1 75
Tl
2+
3d
2
2
2 84
2 |
1 | 4056-4059 | 73
1 75
Tl
2+
3d
2
2
2 84
2 76
V
2+
3d
3
3
3 |
1 | 4057-4060 | 75
Tl
2+
3d
2
2
2 84
2 76
V
2+
3d
3
3
3 87
3 |
1 | 4058-4061 | 84
2 76
V
2+
3d
3
3
3 87
3 86
Cr
2+
3d
4
4
4 |
1 | 4059-4062 | 76
V
2+
3d
3
3
3 87
3 86
Cr
2+
3d
4
4
4 90
4 |
1 | 4060-4063 | 87
3 86
Cr
2+
3d
4
4
4 90
4 80
Mn
2+
3d
5
5
5 |
1 | 4061-4064 | 86
Cr
2+
3d
4
4
4 90
4 80
Mn
2+
3d
5
5
5 92
5 |
1 | 4062-4065 | 90
4 80
Mn
2+
3d
5
5
5 92
5 96
Fe
2+
3d
6
4
4 |
1 | 4063-4066 | 80
Mn
2+
3d
5
5
5 92
5 96
Fe
2+
3d
6
4
4 90
5 |
1 | 4064-4067 | 92
5 96
Fe
2+
3d
6
4
4 90
5 3 – 5 |
1 | 4065-4068 | 96
Fe
2+
3d
6
4
4 90
5 3 – 5 5
Co
2+
3d
7
3
3 |
1 | 4066-4069 | 90
5 3 – 5 5
Co
2+
3d
7
3
3 87
4 |
1 | 4067-4070 | 3 – 5 5
Co
2+
3d
7
3
3 87
4 4 – 5 |
1 | 4068-4071 | 5
Co
2+
3d
7
3
3 87
4 4 – 5 2
Ni
2+
3d
8
2
2 |
1 | 4069-4072 | 87
4 4 – 5 2
Ni
2+
3d
8
2
2 84
2 |
1 | 4070-4073 | 4 – 5 2
Ni
2+
3d
8
2
2 84
2 9 – 3, 4
Cu
2+
3d
9
1
1 |
1 | 4071-4074 | 2
Ni
2+
3d
8
2
2 84
2 9 – 3, 4
Cu
2+
3d
9
1
1 73
1 |
1 | 4072-4075 | 84
2 9 – 3, 4
Cu
2+
3d
9
1
1 73
1 8 – 2 |
1 | 4073-4076 | 9 – 3, 4
Cu
2+
3d
9
1
1 73
1 8 – 2 2
Zn
2+
3d
10
0
0
Ion
Configuration
Unpaired
electron(s)
Magnetic moment
Calculated
Observed
Table 4 |
1 | 4074-4077 | 73
1 8 – 2 2
Zn
2+
3d
10
0
0
Ion
Configuration
Unpaired
electron(s)
Magnetic moment
Calculated
Observed
Table 4 7: Calculated and Observed Magnetic Moments (BM)
Calculate the magnetic moment of a divalent ion in aqueous solution
if its atomic number is 25 |
1 | 4075-4078 | 8 – 2 2
Zn
2+
3d
10
0
0
Ion
Configuration
Unpaired
electron(s)
Magnetic moment
Calculated
Observed
Table 4 7: Calculated and Observed Magnetic Moments (BM)
Calculate the magnetic moment of a divalent ion in aqueous solution
if its atomic number is 25 dWith atomic number 25, the divalent ion in aqueous solution will have
5 configuration (five unpaired electrons) |
1 | 4076-4079 | 2
Zn
2+
3d
10
0
0
Ion
Configuration
Unpaired
electron(s)
Magnetic moment
Calculated
Observed
Table 4 7: Calculated and Observed Magnetic Moments (BM)
Calculate the magnetic moment of a divalent ion in aqueous solution
if its atomic number is 25 dWith atomic number 25, the divalent ion in aqueous solution will have
5 configuration (five unpaired electrons) The magnetic moment, µ is
5
5 |
1 | 4077-4080 | 7: Calculated and Observed Magnetic Moments (BM)
Calculate the magnetic moment of a divalent ion in aqueous solution
if its atomic number is 25 dWith atomic number 25, the divalent ion in aqueous solution will have
5 configuration (five unpaired electrons) The magnetic moment, µ is
5
5 92BM
5
2
Example 4 |
1 | 4078-4081 | dWith atomic number 25, the divalent ion in aqueous solution will have
5 configuration (five unpaired electrons) The magnetic moment, µ is
5
5 92BM
5
2
Example 4 8
Example 4 |
1 | 4079-4082 | The magnetic moment, µ is
5
5 92BM
5
2
Example 4 8
Example 4 8
Example 4 |
1 | 4080-4083 | 92BM
5
2
Example 4 8
Example 4 8
Example 4 8
Example 4 |
1 | 4081-4084 | 8
Example 4 8
Example 4 8
Example 4 8
Example 4 |
1 | 4082-4085 | 8
Example 4 8
Example 4 8
Example 4 8
Solution
Solution
Solution
Solution
Solution
Rationalised 2023-24
103
The d- and f- Block Elements
3d
0
Sc
3+
colourless
3d
0
Ti
4+
colourless
3d
1
Ti
3+
purple
3d
1
V
4+
blue
3d
2
V
3+
green
3d
3
V
2+
violet
3d
3
Cr
3+
violet
3d
4
Mn
3+
violet
3d
4
Cr
2+
blue
3d
5
Mn
2+
pink
3d
5
Fe
3+
yellow
3d
6
Fe
2+
green
3d
63d
7
Co
3+Co
2+
bluepink
3d
8
Ni
2+
green
3d
9
Cu
2+
blue
3d
10
Zn
2+
colourless
Configuration
Example
Colour
Table 4 |
1 | 4083-4086 | 8
Example 4 8
Example 4 8
Solution
Solution
Solution
Solution
Solution
Rationalised 2023-24
103
The d- and f- Block Elements
3d
0
Sc
3+
colourless
3d
0
Ti
4+
colourless
3d
1
Ti
3+
purple
3d
1
V
4+
blue
3d
2
V
3+
green
3d
3
V
2+
violet
3d
3
Cr
3+
violet
3d
4
Mn
3+
violet
3d
4
Cr
2+
blue
3d
5
Mn
2+
pink
3d
5
Fe
3+
yellow
3d
6
Fe
2+
green
3d
63d
7
Co
3+Co
2+
bluepink
3d
8
Ni
2+
green
3d
9
Cu
2+
blue
3d
10
Zn
2+
colourless
Configuration
Example
Colour
Table 4 8: Colours of Some of the First Row
(aquated) Transition Metal Ions
4 |
1 | 4084-4087 | 8
Example 4 8
Solution
Solution
Solution
Solution
Solution
Rationalised 2023-24
103
The d- and f- Block Elements
3d
0
Sc
3+
colourless
3d
0
Ti
4+
colourless
3d
1
Ti
3+
purple
3d
1
V
4+
blue
3d
2
V
3+
green
3d
3
V
2+
violet
3d
3
Cr
3+
violet
3d
4
Mn
3+
violet
3d
4
Cr
2+
blue
3d
5
Mn
2+
pink
3d
5
Fe
3+
yellow
3d
6
Fe
2+
green
3d
63d
7
Co
3+Co
2+
bluepink
3d
8
Ni
2+
green
3d
9
Cu
2+
blue
3d
10
Zn
2+
colourless
Configuration
Example
Colour
Table 4 8: Colours of Some of the First Row
(aquated) Transition Metal Ions
4 3 |
1 | 4085-4088 | 8
Solution
Solution
Solution
Solution
Solution
Rationalised 2023-24
103
The d- and f- Block Elements
3d
0
Sc
3+
colourless
3d
0
Ti
4+
colourless
3d
1
Ti
3+
purple
3d
1
V
4+
blue
3d
2
V
3+
green
3d
3
V
2+
violet
3d
3
Cr
3+
violet
3d
4
Mn
3+
violet
3d
4
Cr
2+
blue
3d
5
Mn
2+
pink
3d
5
Fe
3+
yellow
3d
6
Fe
2+
green
3d
63d
7
Co
3+Co
2+
bluepink
3d
8
Ni
2+
green
3d
9
Cu
2+
blue
3d
10
Zn
2+
colourless
Configuration
Example
Colour
Table 4 8: Colours of Some of the First Row
(aquated) Transition Metal Ions
4 3 11 Formation
of Complex
Compounds
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
4 |
1 | 4086-4089 | 8: Colours of Some of the First Row
(aquated) Transition Metal Ions
4 3 11 Formation
of Complex
Compounds
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
4 8 Calculate the ‘spin only’ magnetic moment of M
2+
(aq) ion (Z = 27) |
1 | 4087-4090 | 3 11 Formation
of Complex
Compounds
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
4 8 Calculate the ‘spin only’ magnetic moment of M
2+
(aq) ion (Z = 27) When an electron from a lower energy d orbital is excited to a higher
energy d orbital, the energy of excitation corresponds to the frequency
of light absorbed (Unit 5) |
1 | 4088-4091 | 11 Formation
of Complex
Compounds
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
4 8 Calculate the ‘spin only’ magnetic moment of M
2+
(aq) ion (Z = 27) When an electron from a lower energy d orbital is excited to a higher
energy d orbital, the energy of excitation corresponds to the frequency
of light absorbed (Unit 5) This frequency generally lies in the visible
region |
1 | 4089-4092 | 8 Calculate the ‘spin only’ magnetic moment of M
2+
(aq) ion (Z = 27) When an electron from a lower energy d orbital is excited to a higher
energy d orbital, the energy of excitation corresponds to the frequency
of light absorbed (Unit 5) This frequency generally lies in the visible
region The colour observed corresponds to the complementary colour
of the light absorbed |
1 | 4090-4093 | When an electron from a lower energy d orbital is excited to a higher
energy d orbital, the energy of excitation corresponds to the frequency
of light absorbed (Unit 5) This frequency generally lies in the visible
region The colour observed corresponds to the complementary colour
of the light absorbed The
frequency of the light
absorbed is determined by
the nature of the ligand |
1 | 4091-4094 | This frequency generally lies in the visible
region The colour observed corresponds to the complementary colour
of the light absorbed The
frequency of the light
absorbed is determined by
the nature of the ligand In
aqueous
solutions
where water molecules are
the ligands, the colours
of the ions observed are
listed in Table 4 |
1 | 4092-4095 | The colour observed corresponds to the complementary colour
of the light absorbed The
frequency of the light
absorbed is determined by
the nature of the ligand In
aqueous
solutions
where water molecules are
the ligands, the colours
of the ions observed are
listed in Table 4 8 |
1 | 4093-4096 | The
frequency of the light
absorbed is determined by
the nature of the ligand In
aqueous
solutions
where water molecules are
the ligands, the colours
of the ions observed are
listed in Table 4 8 A few
coloured
solutions
of
d–block
elements
are
illustrated in Fig |
1 | 4094-4097 | In
aqueous
solutions
where water molecules are
the ligands, the colours
of the ions observed are
listed in Table 4 8 A few
coloured
solutions
of
d–block
elements
are
illustrated in Fig 4 |
1 | 4095-4098 | 8 A few
coloured
solutions
of
d–block
elements
are
illustrated in Fig 4 5 |
1 | 4096-4099 | A few
coloured
solutions
of
d–block
elements
are
illustrated in Fig 4 5 4 |
1 | 4097-4100 | 4 5 4 3 |
1 | 4098-4101 | 5 4 3 10 Formation
of Coloured
Ions
Fig |
1 | 4099-4102 | 4 3 10 Formation
of Coloured
Ions
Fig 4 |
1 | 4100-4103 | 3 10 Formation
of Coloured
Ions
Fig 4 5: Colours of some of the first row
transition metal ions in aqueous solutions |
1 | 4101-4104 | 10 Formation
of Coloured
Ions
Fig 4 5: Colours of some of the first row
transition metal ions in aqueous solutions From
left to right: V4+,V3+,Mn2+,Fe3+,Co2+,Ni2+and Cu2+ |
1 | 4102-4105 | 4 5: Colours of some of the first row
transition metal ions in aqueous solutions From
left to right: V4+,V3+,Mn2+,Fe3+,Co2+,Ni2+and Cu2+ Complex compounds are those in which the metal ions bind a number
of anions or neutral molecules giving complex species with
characteristic properties |
1 | 4103-4106 | 5: Colours of some of the first row
transition metal ions in aqueous solutions From
left to right: V4+,V3+,Mn2+,Fe3+,Co2+,Ni2+and Cu2+ Complex compounds are those in which the metal ions bind a number
of anions or neutral molecules giving complex species with
characteristic properties A few examples are: [Fe(CN)6]
3–, [Fe(CN)6]
4–,
[Cu(NH3)4]
2+ and [PtCl4]
2– |
1 | 4104-4107 | From
left to right: V4+,V3+,Mn2+,Fe3+,Co2+,Ni2+and Cu2+ Complex compounds are those in which the metal ions bind a number
of anions or neutral molecules giving complex species with
characteristic properties A few examples are: [Fe(CN)6]
3–, [Fe(CN)6]
4–,
[Cu(NH3)4]
2+ and [PtCl4]
2– (The chemistry of complex compounds is
Rationalised 2023-24
104
Chemistry
dealt with in detail in Unit 5) |
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