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1 | 3905-3908 | 3
Example 4 3
Example 4 3
Example 4 3
Solution
Solution
Solution
Solution
Solution
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
4 |
1 | 3906-3909 | 3
Example 4 3
Example 4 3
Solution
Solution
Solution
Solution
Solution
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
4 3 Which of the 3d series of the transition metals exhibits the
largest number of oxidation states and why |
1 | 3907-3910 | 3
Example 4 3
Solution
Solution
Solution
Solution
Solution
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
4 3 Which of the 3d series of the transition metals exhibits the
largest number of oxidation states and why Rationalised 2023-24
98
Chemistry
Table 4 |
1 | 3908-3911 | 3
Solution
Solution
Solution
Solution
Solution
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
4 3 Which of the 3d series of the transition metals exhibits the
largest number of oxidation states and why Rationalised 2023-24
98
Chemistry
Table 4 4 contains the thermochemical parameters related to the
transformation of the solid metal atoms to M
2+ ions in solution and their
standard electrode potentials |
1 | 3909-3912 | 3 Which of the 3d series of the transition metals exhibits the
largest number of oxidation states and why Rationalised 2023-24
98
Chemistry
Table 4 4 contains the thermochemical parameters related to the
transformation of the solid metal atoms to M
2+ ions in solution and their
standard electrode potentials The observed values of E
V and those
calculated using the data of Table 4 |
1 | 3910-3913 | Rationalised 2023-24
98
Chemistry
Table 4 4 contains the thermochemical parameters related to the
transformation of the solid metal atoms to M
2+ ions in solution and their
standard electrode potentials The observed values of E
V and those
calculated using the data of Table 4 4 are compared in Fig |
1 | 3911-3914 | 4 contains the thermochemical parameters related to the
transformation of the solid metal atoms to M
2+ ions in solution and their
standard electrode potentials The observed values of E
V and those
calculated using the data of Table 4 4 are compared in Fig 4 |
1 | 3912-3915 | The observed values of E
V and those
calculated using the data of Table 4 4 are compared in Fig 4 4 |
1 | 3913-3916 | 4 are compared in Fig 4 4 The unique behaviour of Cu, having a positive E
V, accounts for its
inability to liberate H2 from acids |
1 | 3914-3917 | 4 4 The unique behaviour of Cu, having a positive E
V, accounts for its
inability to liberate H2 from acids Only oxidising acids (nitric and hot
concentrated sulphuric) react with Cu, the acids being reduced |
1 | 3915-3918 | 4 The unique behaviour of Cu, having a positive E
V, accounts for its
inability to liberate H2 from acids Only oxidising acids (nitric and hot
concentrated sulphuric) react with Cu, the acids being reduced The
high energy to transform Cu(s) to Cu2+(aq) is not balanced by its hydration
enthalpy |
1 | 3916-3919 | The unique behaviour of Cu, having a positive E
V, accounts for its
inability to liberate H2 from acids Only oxidising acids (nitric and hot
concentrated sulphuric) react with Cu, the acids being reduced The
high energy to transform Cu(s) to Cu2+(aq) is not balanced by its hydration
enthalpy The general trend towards less negative E
V values across the
4 |
1 | 3917-3920 | Only oxidising acids (nitric and hot
concentrated sulphuric) react with Cu, the acids being reduced The
high energy to transform Cu(s) to Cu2+(aq) is not balanced by its hydration
enthalpy The general trend towards less negative E
V values across the
4 3 |
1 | 3918-3921 | The
high energy to transform Cu(s) to Cu2+(aq) is not balanced by its hydration
enthalpy The general trend towards less negative E
V values across the
4 3 5 Trends in the
M
2+/M
Standard
Electrode
Potentials
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
4 |
1 | 3919-3922 | The general trend towards less negative E
V values across the
4 3 5 Trends in the
M
2+/M
Standard
Electrode
Potentials
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
4 4 The E
o(M
2+/M) value for copper is positive (+0 |
1 | 3920-3923 | 3 5 Trends in the
M
2+/M
Standard
Electrode
Potentials
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
4 4 The E
o(M
2+/M) value for copper is positive (+0 34V) |
1 | 3921-3924 | 5 Trends in the
M
2+/M
Standard
Electrode
Potentials
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
4 4 The E
o(M
2+/M) value for copper is positive (+0 34V) What is possible
reason for this |
1 | 3922-3925 | 4 The E
o(M
2+/M) value for copper is positive (+0 34V) What is possible
reason for this (Hint: consider its high DaH
o and low DhydH
o)
Why is Cr
2+ reducing and Mn
3+ oxidising when both have d
4 configuration |
1 | 3923-3926 | 34V) What is possible
reason for this (Hint: consider its high DaH
o and low DhydH
o)
Why is Cr
2+ reducing and Mn
3+ oxidising when both have d
4 configuration Cr
2+ is reducing as its configuration changes from d
4 to d
3, the latter
having a half-filled t2g level (see Unit 5) |
1 | 3924-3927 | What is possible
reason for this (Hint: consider its high DaH
o and low DhydH
o)
Why is Cr
2+ reducing and Mn
3+ oxidising when both have d
4 configuration Cr
2+ is reducing as its configuration changes from d
4 to d
3, the latter
having a half-filled t2g level (see Unit 5) On the other hand, the change
from Mn
3+ to Mn
2+ results in the half-filled (d
5) configuration which has
extra stability |
1 | 3925-3928 | (Hint: consider its high DaH
o and low DhydH
o)
Why is Cr
2+ reducing and Mn
3+ oxidising when both have d
4 configuration Cr
2+ is reducing as its configuration changes from d
4 to d
3, the latter
having a half-filled t2g level (see Unit 5) On the other hand, the change
from Mn
3+ to Mn
2+ results in the half-filled (d
5) configuration which has
extra stability Example 4 |
1 | 3926-3929 | Cr
2+ is reducing as its configuration changes from d
4 to d
3, the latter
having a half-filled t2g level (see Unit 5) On the other hand, the change
from Mn
3+ to Mn
2+ results in the half-filled (d
5) configuration which has
extra stability Example 4 4
Example 4 |
1 | 3927-3930 | On the other hand, the change
from Mn
3+ to Mn
2+ results in the half-filled (d
5) configuration which has
extra stability Example 4 4
Example 4 4
Example 4 |
1 | 3928-3931 | Example 4 4
Example 4 4
Example 4 4
Example 4 |
1 | 3929-3932 | 4
Example 4 4
Example 4 4
Example 4 4
Example 4 |
1 | 3930-3933 | 4
Example 4 4
Example 4 4
Example 4 4
Solution
Solution
Solution
Solution
Solution
Fig |
1 | 3931-3934 | 4
Example 4 4
Example 4 4
Solution
Solution
Solution
Solution
Solution
Fig 4 |
1 | 3932-3935 | 4
Example 4 4
Solution
Solution
Solution
Solution
Solution
Fig 4 4: Observed and calculated values for the standard
electrode potentials
(M2+ ® M°) of the elements Ti to Zn
series is related to the general increase in the sum of the first and second
ionisation enthalpies |
1 | 3933-3936 | 4
Solution
Solution
Solution
Solution
Solution
Fig 4 4: Observed and calculated values for the standard
electrode potentials
(M2+ ® M°) of the elements Ti to Zn
series is related to the general increase in the sum of the first and second
ionisation enthalpies It is interesting to note that the value of E
V for Mn,
Ni and Zn are more negative than expected from the trend |
1 | 3934-3937 | 4 4: Observed and calculated values for the standard
electrode potentials
(M2+ ® M°) of the elements Ti to Zn
series is related to the general increase in the sum of the first and second
ionisation enthalpies It is interesting to note that the value of E
V for Mn,
Ni and Zn are more negative than expected from the trend Rationalised 2023-24
99
The d- and f- Block Elements
Element (M)
DDDDDaH
o (M)
DDDDDiH1
o
DDDDD1H2
o
DDDDDhydH
o(M
2+)
E
o/V
Ti
469
656
1309
-1866
-1 |
1 | 3935-3938 | 4: Observed and calculated values for the standard
electrode potentials
(M2+ ® M°) of the elements Ti to Zn
series is related to the general increase in the sum of the first and second
ionisation enthalpies It is interesting to note that the value of E
V for Mn,
Ni and Zn are more negative than expected from the trend Rationalised 2023-24
99
The d- and f- Block Elements
Element (M)
DDDDDaH
o (M)
DDDDDiH1
o
DDDDD1H2
o
DDDDDhydH
o(M
2+)
E
o/V
Ti
469
656
1309
-1866
-1 63
V
515
650
1414
-1895
-1 |
1 | 3936-3939 | It is interesting to note that the value of E
V for Mn,
Ni and Zn are more negative than expected from the trend Rationalised 2023-24
99
The d- and f- Block Elements
Element (M)
DDDDDaH
o (M)
DDDDDiH1
o
DDDDD1H2
o
DDDDDhydH
o(M
2+)
E
o/V
Ti
469
656
1309
-1866
-1 63
V
515
650
1414
-1895
-1 18
Cr
398
653
1592
-1925
-0 |
1 | 3937-3940 | Rationalised 2023-24
99
The d- and f- Block Elements
Element (M)
DDDDDaH
o (M)
DDDDDiH1
o
DDDDD1H2
o
DDDDDhydH
o(M
2+)
E
o/V
Ti
469
656
1309
-1866
-1 63
V
515
650
1414
-1895
-1 18
Cr
398
653
1592
-1925
-0 90
Mn
279
717
1509
-1862
-1 |
1 | 3938-3941 | 63
V
515
650
1414
-1895
-1 18
Cr
398
653
1592
-1925
-0 90
Mn
279
717
1509
-1862
-1 18
Fe
418
762
1561
-1998
-0 |
1 | 3939-3942 | 18
Cr
398
653
1592
-1925
-0 90
Mn
279
717
1509
-1862
-1 18
Fe
418
762
1561
-1998
-0 44
Co
427
758
1644
-2079
-0 |
1 | 3940-3943 | 90
Mn
279
717
1509
-1862
-1 18
Fe
418
762
1561
-1998
-0 44
Co
427
758
1644
-2079
-0 28
Ni
431
736
1752
-2121
-0 |
1 | 3941-3944 | 18
Fe
418
762
1561
-1998
-0 44
Co
427
758
1644
-2079
-0 28
Ni
431
736
1752
-2121
-0 25
Cu
339
745
1958
-2121
0 |
1 | 3942-3945 | 44
Co
427
758
1644
-2079
-0 28
Ni
431
736
1752
-2121
-0 25
Cu
339
745
1958
-2121
0 34
Zn
130
906
1734
-2059
-0 |
1 | 3943-3946 | 28
Ni
431
736
1752
-2121
-0 25
Cu
339
745
1958
-2121
0 34
Zn
130
906
1734
-2059
-0 76
Table 4 |
1 | 3944-3947 | 25
Cu
339
745
1958
-2121
0 34
Zn
130
906
1734
-2059
-0 76
Table 4 4: Thermochemical data (kJ mol
-1) for the first row Transition
Elements and the Standard Electrode Potentials for the
Reduction of M
II to M |
1 | 3945-3948 | 34
Zn
130
906
1734
-2059
-0 76
Table 4 4: Thermochemical data (kJ mol
-1) for the first row Transition
Elements and the Standard Electrode Potentials for the
Reduction of M
II to M The stability of the half-filled d sub-shell in Mn
2+ and the completely
filled d
10 configuration in Zn
2+ are related to their E
o values, whereas E
o
for Ni is related to the highest negative DhydH
o |
1 | 3946-3949 | 76
Table 4 4: Thermochemical data (kJ mol
-1) for the first row Transition
Elements and the Standard Electrode Potentials for the
Reduction of M
II to M The stability of the half-filled d sub-shell in Mn
2+ and the completely
filled d
10 configuration in Zn
2+ are related to their E
o values, whereas E
o
for Ni is related to the highest negative DhydH
o An examination of the E
o(M
3+/M
2+) values (Table 4 |
1 | 3947-3950 | 4: Thermochemical data (kJ mol
-1) for the first row Transition
Elements and the Standard Electrode Potentials for the
Reduction of M
II to M The stability of the half-filled d sub-shell in Mn
2+ and the completely
filled d
10 configuration in Zn
2+ are related to their E
o values, whereas E
o
for Ni is related to the highest negative DhydH
o An examination of the E
o(M
3+/M
2+) values (Table 4 2) shows the varying
trends |
1 | 3948-3951 | The stability of the half-filled d sub-shell in Mn
2+ and the completely
filled d
10 configuration in Zn
2+ are related to their E
o values, whereas E
o
for Ni is related to the highest negative DhydH
o An examination of the E
o(M
3+/M
2+) values (Table 4 2) shows the varying
trends The low value for Sc reflects the stability of Sc
3+ which has a
noble gas configuration |
1 | 3949-3952 | An examination of the E
o(M
3+/M
2+) values (Table 4 2) shows the varying
trends The low value for Sc reflects the stability of Sc
3+ which has a
noble gas configuration The highest value for Zn is due to the removal
of an electron from the stable d
10 configuration of Zn
2+ |
1 | 3950-3953 | 2) shows the varying
trends The low value for Sc reflects the stability of Sc
3+ which has a
noble gas configuration The highest value for Zn is due to the removal
of an electron from the stable d
10 configuration of Zn
2+ The
comparatively high value for Mn shows that Mn
2+(d
5) is particularly
stable, whereas comparatively low value for Fe shows the extra stability
of Fe
3+ (d
5) |
1 | 3951-3954 | The low value for Sc reflects the stability of Sc
3+ which has a
noble gas configuration The highest value for Zn is due to the removal
of an electron from the stable d
10 configuration of Zn
2+ The
comparatively high value for Mn shows that Mn
2+(d
5) is particularly
stable, whereas comparatively low value for Fe shows the extra stability
of Fe
3+ (d
5) The comparatively low value for V is related to the stability
of V
2+ (half-filled t2g level, Unit 5) |
1 | 3952-3955 | The highest value for Zn is due to the removal
of an electron from the stable d
10 configuration of Zn
2+ The
comparatively high value for Mn shows that Mn
2+(d
5) is particularly
stable, whereas comparatively low value for Fe shows the extra stability
of Fe
3+ (d
5) The comparatively low value for V is related to the stability
of V
2+ (half-filled t2g level, Unit 5) Table 4 |
1 | 3953-3956 | The
comparatively high value for Mn shows that Mn
2+(d
5) is particularly
stable, whereas comparatively low value for Fe shows the extra stability
of Fe
3+ (d
5) The comparatively low value for V is related to the stability
of V
2+ (half-filled t2g level, Unit 5) Table 4 5 shows the stable halides of the 3d series of transition metals |
1 | 3954-3957 | The comparatively low value for V is related to the stability
of V
2+ (half-filled t2g level, Unit 5) Table 4 5 shows the stable halides of the 3d series of transition metals The highest oxidation numbers are achieved in TiX4 (tetrahalides), VF5
and CrF6 |
1 | 3955-3958 | Table 4 5 shows the stable halides of the 3d series of transition metals The highest oxidation numbers are achieved in TiX4 (tetrahalides), VF5
and CrF6 The +7 state for Mn is not represented in simple halides but
MnO3F is known, and beyond Mn no metal has a trihalide except FeX3
and CoF3 |
1 | 3956-3959 | 5 shows the stable halides of the 3d series of transition metals The highest oxidation numbers are achieved in TiX4 (tetrahalides), VF5
and CrF6 The +7 state for Mn is not represented in simple halides but
MnO3F is known, and beyond Mn no metal has a trihalide except FeX3
and CoF3 The ability of fluorine to stabilise the highest oxidation state is
due to either higher lattice energy as in the case of CoF3, or higher bond
enthalpy terms for the higher covalent compounds, e |
1 | 3957-3960 | The highest oxidation numbers are achieved in TiX4 (tetrahalides), VF5
and CrF6 The +7 state for Mn is not represented in simple halides but
MnO3F is known, and beyond Mn no metal has a trihalide except FeX3
and CoF3 The ability of fluorine to stabilise the highest oxidation state is
due to either higher lattice energy as in the case of CoF3, or higher bond
enthalpy terms for the higher covalent compounds, e g |
1 | 3958-3961 | The +7 state for Mn is not represented in simple halides but
MnO3F is known, and beyond Mn no metal has a trihalide except FeX3
and CoF3 The ability of fluorine to stabilise the highest oxidation state is
due to either higher lattice energy as in the case of CoF3, or higher bond
enthalpy terms for the higher covalent compounds, e g , VF5 and CrF6 |
1 | 3959-3962 | The ability of fluorine to stabilise the highest oxidation state is
due to either higher lattice energy as in the case of CoF3, or higher bond
enthalpy terms for the higher covalent compounds, e g , VF5 and CrF6 Although V
+5 is represented only by VF5, the other halides, however,
undergo hydrolysis to give oxohalides, VOX3 |
1 | 3960-3963 | g , VF5 and CrF6 Although V
+5 is represented only by VF5, the other halides, however,
undergo hydrolysis to give oxohalides, VOX3 Another feature of fluorides
is their instability in the low oxidation states e |
1 | 3961-3964 | , VF5 and CrF6 Although V
+5 is represented only by VF5, the other halides, however,
undergo hydrolysis to give oxohalides, VOX3 Another feature of fluorides
is their instability in the low oxidation states e g |
1 | 3962-3965 | Although V
+5 is represented only by VF5, the other halides, however,
undergo hydrolysis to give oxohalides, VOX3 Another feature of fluorides
is their instability in the low oxidation states e g , VX2 (X = CI, Br or I)
4 |
1 | 3963-3966 | Another feature of fluorides
is their instability in the low oxidation states e g , VX2 (X = CI, Br or I)
4 3 |
1 | 3964-3967 | g , VX2 (X = CI, Br or I)
4 3 6 Trends in
the M
3+/M
2+
Standard
Electrode
Potentials
4 |
1 | 3965-3968 | , VX2 (X = CI, Br or I)
4 3 6 Trends in
the M
3+/M
2+
Standard
Electrode
Potentials
4 3 |
1 | 3966-3969 | 3 6 Trends in
the M
3+/M
2+
Standard
Electrode
Potentials
4 3 7 Trends in
Stability of
Higher
Oxidation
States
+ 6
CrF6
+ 5
VF5
CrF5
+ 4
TiX4
VX
I
4
CrX4
MnF4
+ 3
TiX3
VX3
CrX3
MnF3
FeX
I
3
CoF3
+ 2
TiX2
III
VX2
CrX2
MnX2
FeX2
CoX2
NiX2
CuX2
II
ZnX2
+ 1
CuX
III
Oxidation
Number
Table 4 |
1 | 3967-3970 | 6 Trends in
the M
3+/M
2+
Standard
Electrode
Potentials
4 3 7 Trends in
Stability of
Higher
Oxidation
States
+ 6
CrF6
+ 5
VF5
CrF5
+ 4
TiX4
VX
I
4
CrX4
MnF4
+ 3
TiX3
VX3
CrX3
MnF3
FeX
I
3
CoF3
+ 2
TiX2
III
VX2
CrX2
MnX2
FeX2
CoX2
NiX2
CuX2
II
ZnX2
+ 1
CuX
III
Oxidation
Number
Table 4 5: Formulas of Halides of 3d Metals
Key: X = F ® I; XI = F ® Br; XII = F, CI; XIII = CI ® I
Rationalised 2023-24
100
Chemistry
and the same applies to CuX |
1 | 3968-3971 | 3 7 Trends in
Stability of
Higher
Oxidation
States
+ 6
CrF6
+ 5
VF5
CrF5
+ 4
TiX4
VX
I
4
CrX4
MnF4
+ 3
TiX3
VX3
CrX3
MnF3
FeX
I
3
CoF3
+ 2
TiX2
III
VX2
CrX2
MnX2
FeX2
CoX2
NiX2
CuX2
II
ZnX2
+ 1
CuX
III
Oxidation
Number
Table 4 5: Formulas of Halides of 3d Metals
Key: X = F ® I; XI = F ® Br; XII = F, CI; XIII = CI ® I
Rationalised 2023-24
100
Chemistry
and the same applies to CuX On the other hand, all Cu
II halides are
known except the iodide |
1 | 3969-3972 | 7 Trends in
Stability of
Higher
Oxidation
States
+ 6
CrF6
+ 5
VF5
CrF5
+ 4
TiX4
VX
I
4
CrX4
MnF4
+ 3
TiX3
VX3
CrX3
MnF3
FeX
I
3
CoF3
+ 2
TiX2
III
VX2
CrX2
MnX2
FeX2
CoX2
NiX2
CuX2
II
ZnX2
+ 1
CuX
III
Oxidation
Number
Table 4 5: Formulas of Halides of 3d Metals
Key: X = F ® I; XI = F ® Br; XII = F, CI; XIII = CI ® I
Rationalised 2023-24
100
Chemistry
and the same applies to CuX On the other hand, all Cu
II halides are
known except the iodide In this case, Cu
2+ oxidises I
– to I2:
2
2 2
2
2Cu
4I
Cu I
I
s
However, many copper (I) compounds are unstable in aqueous
solution and undergo disproportionation |
1 | 3970-3973 | 5: Formulas of Halides of 3d Metals
Key: X = F ® I; XI = F ® Br; XII = F, CI; XIII = CI ® I
Rationalised 2023-24
100
Chemistry
and the same applies to CuX On the other hand, all Cu
II halides are
known except the iodide In this case, Cu
2+ oxidises I
– to I2:
2
2 2
2
2Cu
4I
Cu I
I
s
However, many copper (I) compounds are unstable in aqueous
solution and undergo disproportionation 2Cu
+ ® Cu
2+ + Cu
The stability of Cu
2+ (aq) rather than Cu
+(aq) is due to the much
more negative DhydH
o of Cu
2+ (aq) than Cu
+, which more than
compensates for the second ionisation enthalpy of Cu |
1 | 3971-3974 | On the other hand, all Cu
II halides are
known except the iodide In this case, Cu
2+ oxidises I
– to I2:
2
2 2
2
2Cu
4I
Cu I
I
s
However, many copper (I) compounds are unstable in aqueous
solution and undergo disproportionation 2Cu
+ ® Cu
2+ + Cu
The stability of Cu
2+ (aq) rather than Cu
+(aq) is due to the much
more negative DhydH
o of Cu
2+ (aq) than Cu
+, which more than
compensates for the second ionisation enthalpy of Cu The ability of oxygen to stabilise the highest oxidation state is
demonstrated in the oxides |
1 | 3972-3975 | In this case, Cu
2+ oxidises I
– to I2:
2
2 2
2
2Cu
4I
Cu I
I
s
However, many copper (I) compounds are unstable in aqueous
solution and undergo disproportionation 2Cu
+ ® Cu
2+ + Cu
The stability of Cu
2+ (aq) rather than Cu
+(aq) is due to the much
more negative DhydH
o of Cu
2+ (aq) than Cu
+, which more than
compensates for the second ionisation enthalpy of Cu The ability of oxygen to stabilise the highest oxidation state is
demonstrated in the oxides The highest oxidation number in the oxides
(Table 4 |
1 | 3973-3976 | 2Cu
+ ® Cu
2+ + Cu
The stability of Cu
2+ (aq) rather than Cu
+(aq) is due to the much
more negative DhydH
o of Cu
2+ (aq) than Cu
+, which more than
compensates for the second ionisation enthalpy of Cu The ability of oxygen to stabilise the highest oxidation state is
demonstrated in the oxides The highest oxidation number in the oxides
(Table 4 6) coincides with the group number and is attained in Sc2O3
to Mn2O7 |
1 | 3974-3977 | The ability of oxygen to stabilise the highest oxidation state is
demonstrated in the oxides The highest oxidation number in the oxides
(Table 4 6) coincides with the group number and is attained in Sc2O3
to Mn2O7 Beyond Group 7, no higher oxides of Fe above Fe2O3, are
known, although ferrates (VI)(FeO4)
2–, are formed in alkaline media but
they readily decompose to Fe2O3 and O2 |
1 | 3975-3978 | The highest oxidation number in the oxides
(Table 4 6) coincides with the group number and is attained in Sc2O3
to Mn2O7 Beyond Group 7, no higher oxides of Fe above Fe2O3, are
known, although ferrates (VI)(FeO4)
2–, are formed in alkaline media but
they readily decompose to Fe2O3 and O2 Besides the oxides, oxocations
stabilise V
v as VO2
+, V
IV as VO
2+ and Ti
IV as TiO
2+ |
1 | 3976-3979 | 6) coincides with the group number and is attained in Sc2O3
to Mn2O7 Beyond Group 7, no higher oxides of Fe above Fe2O3, are
known, although ferrates (VI)(FeO4)
2–, are formed in alkaline media but
they readily decompose to Fe2O3 and O2 Besides the oxides, oxocations
stabilise V
v as VO2
+, V
IV as VO
2+ and Ti
IV as TiO
2+ The ability of oxygen
to stabilise these high oxidation states exceeds that of fluorine |
1 | 3977-3980 | Beyond Group 7, no higher oxides of Fe above Fe2O3, are
known, although ferrates (VI)(FeO4)
2–, are formed in alkaline media but
they readily decompose to Fe2O3 and O2 Besides the oxides, oxocations
stabilise V
v as VO2
+, V
IV as VO
2+ and Ti
IV as TiO
2+ The ability of oxygen
to stabilise these high oxidation states exceeds that of fluorine Thus
the highest Mn fluoride is MnF4 whereas the highest oxide is Mn2O7 |
1 | 3978-3981 | Besides the oxides, oxocations
stabilise V
v as VO2
+, V
IV as VO
2+ and Ti
IV as TiO
2+ The ability of oxygen
to stabilise these high oxidation states exceeds that of fluorine Thus
the highest Mn fluoride is MnF4 whereas the highest oxide is Mn2O7 The ability of oxygen to form multiple bonds to metals explains its
superiority |
1 | 3979-3982 | The ability of oxygen
to stabilise these high oxidation states exceeds that of fluorine Thus
the highest Mn fluoride is MnF4 whereas the highest oxide is Mn2O7 The ability of oxygen to form multiple bonds to metals explains its
superiority In the covalent oxide Mn2O7, each Mn is tetrahedrally
surrounded by O’s including a Mn–O–Mn bridge |
1 | 3980-3983 | Thus
the highest Mn fluoride is MnF4 whereas the highest oxide is Mn2O7 The ability of oxygen to form multiple bonds to metals explains its
superiority In the covalent oxide Mn2O7, each Mn is tetrahedrally
surrounded by O’s including a Mn–O–Mn bridge The tetrahedral [MO4]
n-
ions are known for V
V, Cr
Vl, Mn
V, Mn
Vl and Mn
VII |
1 | 3981-3984 | The ability of oxygen to form multiple bonds to metals explains its
superiority In the covalent oxide Mn2O7, each Mn is tetrahedrally
surrounded by O’s including a Mn–O–Mn bridge The tetrahedral [MO4]
n-
ions are known for V
V, Cr
Vl, Mn
V, Mn
Vl and Mn
VII + 7
Mn2O7
+ 6
CrO3
+ 5
V2O5
+ 4
TiO2
V2O4
CrO2
MnO2
+ 3
Sc2O3
Ti2O3
V2O3
Cr2O3
Mn2O3
Fe2O3
Mn3O4
*
Fe3O4
*
Co3O4
*
+ 2
TiO
VO
(CrO)
MnO
FeO
CoO
NiO
CuO
ZnO
+ 1
Cu2O
Table 4 |
1 | 3982-3985 | In the covalent oxide Mn2O7, each Mn is tetrahedrally
surrounded by O’s including a Mn–O–Mn bridge The tetrahedral [MO4]
n-
ions are known for V
V, Cr
Vl, Mn
V, Mn
Vl and Mn
VII + 7
Mn2O7
+ 6
CrO3
+ 5
V2O5
+ 4
TiO2
V2O4
CrO2
MnO2
+ 3
Sc2O3
Ti2O3
V2O3
Cr2O3
Mn2O3
Fe2O3
Mn3O4
*
Fe3O4
*
Co3O4
*
+ 2
TiO
VO
(CrO)
MnO
FeO
CoO
NiO
CuO
ZnO
+ 1
Cu2O
Table 4 6: Oxides of 3d Metals
*
mixed oxides
Groups
3
4
5
6
7
8
9
10
11
12
Oxidation
Number
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
4 |
1 | 3983-3986 | The tetrahedral [MO4]
n-
ions are known for V
V, Cr
Vl, Mn
V, Mn
Vl and Mn
VII + 7
Mn2O7
+ 6
CrO3
+ 5
V2O5
+ 4
TiO2
V2O4
CrO2
MnO2
+ 3
Sc2O3
Ti2O3
V2O3
Cr2O3
Mn2O3
Fe2O3
Mn3O4
*
Fe3O4
*
Co3O4
*
+ 2
TiO
VO
(CrO)
MnO
FeO
CoO
NiO
CuO
ZnO
+ 1
Cu2O
Table 4 6: Oxides of 3d Metals
*
mixed oxides
Groups
3
4
5
6
7
8
9
10
11
12
Oxidation
Number
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
4 5 How would you account for the irregular variation of ionisation
enthalpies (first and second) in the first series of the transition elements |
1 | 3984-3987 | + 7
Mn2O7
+ 6
CrO3
+ 5
V2O5
+ 4
TiO2
V2O4
CrO2
MnO2
+ 3
Sc2O3
Ti2O3
V2O3
Cr2O3
Mn2O3
Fe2O3
Mn3O4
*
Fe3O4
*
Co3O4
*
+ 2
TiO
VO
(CrO)
MnO
FeO
CoO
NiO
CuO
ZnO
+ 1
Cu2O
Table 4 6: Oxides of 3d Metals
*
mixed oxides
Groups
3
4
5
6
7
8
9
10
11
12
Oxidation
Number
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
4 5 How would you account for the irregular variation of ionisation
enthalpies (first and second) in the first series of the transition elements Example 4 |
1 | 3985-3988 | 6: Oxides of 3d Metals
*
mixed oxides
Groups
3
4
5
6
7
8
9
10
11
12
Oxidation
Number
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
4 5 How would you account for the irregular variation of ionisation
enthalpies (first and second) in the first series of the transition elements Example 4 5
Example 4 |
1 | 3986-3989 | 5 How would you account for the irregular variation of ionisation
enthalpies (first and second) in the first series of the transition elements Example 4 5
Example 4 5
Example 4 |
1 | 3987-3990 | Example 4 5
Example 4 5
Example 4 5
Example 4 |
1 | 3988-3991 | 5
Example 4 5
Example 4 5
Example 4 5
How would you account for the increasing oxidising power in theExample 4 |
1 | 3989-3992 | 5
Example 4 5
Example 4 5
How would you account for the increasing oxidising power in theExample 4 5
series VO2
+ < Cr2O7
2– < MnO4
– |
1 | 3990-3993 | 5
Example 4 5
How would you account for the increasing oxidising power in theExample 4 5
series VO2
+ < Cr2O7
2– < MnO4
– This is due to the increasing stability of the lower species to which they
are reduced |
1 | 3991-3994 | 5
How would you account for the increasing oxidising power in theExample 4 5
series VO2
+ < Cr2O7
2– < MnO4
– This is due to the increasing stability of the lower species to which they
are reduced Solution
Solution
Solution
Solution
Solution
Rationalised 2023-24
101
The d- and f- Block Elements
EFor the first row transition metals the Eo values are:
o
V
Cr
Mn
Fe
Co
Ni
Cu
(M
2+/M)
–1 |
1 | 3992-3995 | 5
series VO2
+ < Cr2O7
2– < MnO4
– This is due to the increasing stability of the lower species to which they
are reduced Solution
Solution
Solution
Solution
Solution
Rationalised 2023-24
101
The d- and f- Block Elements
EFor the first row transition metals the Eo values are:
o
V
Cr
Mn
Fe
Co
Ni
Cu
(M
2+/M)
–1 18
– 0 |
1 | 3993-3996 | This is due to the increasing stability of the lower species to which they
are reduced Solution
Solution
Solution
Solution
Solution
Rationalised 2023-24
101
The d- and f- Block Elements
EFor the first row transition metals the Eo values are:
o
V
Cr
Mn
Fe
Co
Ni
Cu
(M
2+/M)
–1 18
– 0 91
–1 |
1 | 3994-3997 | Solution
Solution
Solution
Solution
Solution
Rationalised 2023-24
101
The d- and f- Block Elements
EFor the first row transition metals the Eo values are:
o
V
Cr
Mn
Fe
Co
Ni
Cu
(M
2+/M)
–1 18
– 0 91
–1 18
– 0 |
1 | 3995-3998 | 18
– 0 91
–1 18
– 0 44
– 0 |
1 | 3996-3999 | 91
–1 18
– 0 44
– 0 28
– 0 |
1 | 3997-4000 | 18
– 0 44
– 0 28
– 0 25
+0 |
1 | 3998-4001 | 44
– 0 28
– 0 25
+0 34
Explain the irregularity in the above values |
1 | 3999-4002 | 28
– 0 25
+0 34
Explain the irregularity in the above values The E
o (M
2+/M) values are not regular which can be explained from
the irregular variation of ionisation enthalpies (
i
i
1
2
H
H ) and also
the sublimation enthalpies which are relatively much less for
manganese and vanadium |
1 | 4000-4003 | 25
+0 34
Explain the irregularity in the above values The E
o (M
2+/M) values are not regular which can be explained from
the irregular variation of ionisation enthalpies (
i
i
1
2
H
H ) and also
the sublimation enthalpies which are relatively much less for
manganese and vanadium Why is the E
o value for the Mn
3+/Mn
2+ couple much more positive
than that for Cr
3+/Cr
2+ or Fe
3+/Fe
2+ |
1 | 4001-4004 | 34
Explain the irregularity in the above values The E
o (M
2+/M) values are not regular which can be explained from
the irregular variation of ionisation enthalpies (
i
i
1
2
H
H ) and also
the sublimation enthalpies which are relatively much less for
manganese and vanadium Why is the E
o value for the Mn
3+/Mn
2+ couple much more positive
than that for Cr
3+/Cr
2+ or Fe
3+/Fe
2+ Explain |
1 | 4002-4005 | The E
o (M
2+/M) values are not regular which can be explained from
the irregular variation of ionisation enthalpies (
i
i
1
2
H
H ) and also
the sublimation enthalpies which are relatively much less for
manganese and vanadium Why is the E
o value for the Mn
3+/Mn
2+ couple much more positive
than that for Cr
3+/Cr
2+ or Fe
3+/Fe
2+ Explain Much larger third ionisation energy of Mn (where the required change
is d
5 to d
4) is mainly responsible for this |
1 | 4003-4006 | Why is the E
o value for the Mn
3+/Mn
2+ couple much more positive
than that for Cr
3+/Cr
2+ or Fe
3+/Fe
2+ Explain 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 |
1 | 4004-4007 | Explain 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 |
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