Chapter
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1 | 3705-3708 | 1 4 1
4 1
4 |
1 | 3706-3709 | 4 1
4 1
4 1
4 |
1 | 3707-3710 | 1
4 1
4 1
4 1
4 |
1 | 3708-3711 | 1
4 1
4 1
4 1 Position in the
Position in the
Position in the
Position in the
Position in the
Periodic Table
Periodic Table
Periodic Table
Periodic Table
Periodic Table
4 |
1 | 3709-3712 | 1
4 1
4 1 Position in the
Position in the
Position in the
Position in the
Position in the
Periodic Table
Periodic Table
Periodic Table
Periodic Table
Periodic Table
4 2
4 |
1 | 3710-3713 | 1
4 1 Position in the
Position in the
Position in the
Position in the
Position in the
Periodic Table
Periodic Table
Periodic Table
Periodic Table
Periodic Table
4 2
4 2
4 |
1 | 3711-3714 | 1 Position in the
Position in the
Position in the
Position in the
Position in the
Periodic Table
Periodic Table
Periodic Table
Periodic Table
Periodic Table
4 2
4 2
4 2
4 |
1 | 3712-3715 | 2
4 2
4 2
4 2
4 |
1 | 3713-3716 | 2
4 2
4 2
4 2 Electronic
Electronic
Electronic
Electronic
Electronic
Configurations
Configurations
Configurations
Configurations
Configurations
of the d-Block
of the d-Block
of the d-Block
of the d-Block
of the d-Block
Elements
Elements
Elements
Elements
Elements
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Z
21
22
23
24
25
26
27
28
29
30
4s
2
2
2
1
2
2
2
2
1
2
3d
1
2
3
5
5
6
7
8
10
10
1st Series
Table 4 |
1 | 3714-3717 | 2
4 2
4 2 Electronic
Electronic
Electronic
Electronic
Electronic
Configurations
Configurations
Configurations
Configurations
Configurations
of the d-Block
of the d-Block
of the d-Block
of the d-Block
of the d-Block
Elements
Elements
Elements
Elements
Elements
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Z
21
22
23
24
25
26
27
28
29
30
4s
2
2
2
1
2
2
2
2
1
2
3d
1
2
3
5
5
6
7
8
10
10
1st Series
Table 4 1: Electronic Configurations of outer orbitals of the Transition Elements
(ground state)
Rationalised 2023-24
91
The d- and f- Block Elements
The electronic configurations of outer orbitals of Zn, Cd, Hg and Cn
are represented by the general formula (n-1)d
10ns
2 |
1 | 3715-3718 | 2
4 2 Electronic
Electronic
Electronic
Electronic
Electronic
Configurations
Configurations
Configurations
Configurations
Configurations
of the d-Block
of the d-Block
of the d-Block
of the d-Block
of the d-Block
Elements
Elements
Elements
Elements
Elements
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Z
21
22
23
24
25
26
27
28
29
30
4s
2
2
2
1
2
2
2
2
1
2
3d
1
2
3
5
5
6
7
8
10
10
1st Series
Table 4 1: Electronic Configurations of outer orbitals of the Transition Elements
(ground state)
Rationalised 2023-24
91
The d- and f- Block Elements
The electronic configurations of outer orbitals of Zn, Cd, Hg and Cn
are represented by the general formula (n-1)d
10ns
2 The orbitals in
these elements are completely filled in the ground state as well as in
their common oxidation states |
1 | 3716-3719 | 2 Electronic
Electronic
Electronic
Electronic
Electronic
Configurations
Configurations
Configurations
Configurations
Configurations
of the d-Block
of the d-Block
of the d-Block
of the d-Block
of the d-Block
Elements
Elements
Elements
Elements
Elements
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Z
21
22
23
24
25
26
27
28
29
30
4s
2
2
2
1
2
2
2
2
1
2
3d
1
2
3
5
5
6
7
8
10
10
1st Series
Table 4 1: Electronic Configurations of outer orbitals of the Transition Elements
(ground state)
Rationalised 2023-24
91
The d- and f- Block Elements
The electronic configurations of outer orbitals of Zn, Cd, Hg and Cn
are represented by the general formula (n-1)d
10ns
2 The orbitals in
these elements are completely filled in the ground state as well as in
their common oxidation states Therefore, they are not regarded as
transition elements |
1 | 3717-3720 | 1: Electronic Configurations of outer orbitals of the Transition Elements
(ground state)
Rationalised 2023-24
91
The d- and f- Block Elements
The electronic configurations of outer orbitals of Zn, Cd, Hg and Cn
are represented by the general formula (n-1)d
10ns
2 The orbitals in
these elements are completely filled in the ground state as well as in
their common oxidation states Therefore, they are not regarded as
transition elements The d orbitals of the transition elements protrude to the periphery of
an atom more than the other orbitals (i |
1 | 3718-3721 | The orbitals in
these elements are completely filled in the ground state as well as in
their common oxidation states Therefore, they are not regarded as
transition elements The d orbitals of the transition elements protrude to the periphery of
an atom more than the other orbitals (i e |
1 | 3719-3722 | Therefore, they are not regarded as
transition elements The d orbitals of the transition elements protrude to the periphery of
an atom more than the other orbitals (i e , s and p), hence, they are more
influenced by the surroundings as well as affect the atoms or molecules
surrounding them |
1 | 3720-3723 | The d orbitals of the transition elements protrude to the periphery of
an atom more than the other orbitals (i e , s and p), hence, they are more
influenced by the surroundings as well as affect the atoms or molecules
surrounding them In some respects, ions of a given d
n configuration
(n = 1 β 9) have similar magnetic and electronic properties |
1 | 3721-3724 | e , s and p), hence, they are more
influenced by the surroundings as well as affect the atoms or molecules
surrounding them In some respects, ions of a given d
n configuration
(n = 1 β 9) have similar magnetic and electronic properties With partly
filled d orbitals these elements exhibit certain characteristic properties
such as display of a variety of oxidation states, formation of coloured
ions and entering into complex formation with a variety of ligands |
1 | 3722-3725 | , s and p), hence, they are more
influenced by the surroundings as well as affect the atoms or molecules
surrounding them In some respects, ions of a given d
n configuration
(n = 1 β 9) have similar magnetic and electronic properties With partly
filled d orbitals these elements exhibit certain characteristic properties
such as display of a variety of oxidation states, formation of coloured
ions and entering into complex formation with a variety of ligands The transition metals and their compounds also exhibit catalytic
property and paramagnetic behaviour |
1 | 3723-3726 | In some respects, ions of a given d
n configuration
(n = 1 β 9) have similar magnetic and electronic properties With partly
filled d orbitals these elements exhibit certain characteristic properties
such as display of a variety of oxidation states, formation of coloured
ions and entering into complex formation with a variety of ligands The transition metals and their compounds also exhibit catalytic
property and paramagnetic behaviour All these characteristics have
been discussed in detail later in this Unit |
1 | 3724-3727 | With partly
filled d orbitals these elements exhibit certain characteristic properties
such as display of a variety of oxidation states, formation of coloured
ions and entering into complex formation with a variety of ligands The transition metals and their compounds also exhibit catalytic
property and paramagnetic behaviour All these characteristics have
been discussed in detail later in this Unit There are greater similarities in the properties of the transition
elements of a horizontal row in contrast to the non-transition elements |
1 | 3725-3728 | The transition metals and their compounds also exhibit catalytic
property and paramagnetic behaviour All these characteristics have
been discussed in detail later in this Unit There are greater similarities in the properties of the transition
elements of a horizontal row in contrast to the non-transition elements However, some group similarities also exist |
1 | 3726-3729 | All these characteristics have
been discussed in detail later in this Unit There are greater similarities in the properties of the transition
elements of a horizontal row in contrast to the non-transition elements However, some group similarities also exist We shall first study the
general characteristics and their trends in the horizontal rows
(particularly 3d row) and then consider some group similarities |
1 | 3727-3730 | There are greater similarities in the properties of the transition
elements of a horizontal row in contrast to the non-transition elements However, some group similarities also exist We shall first study the
general characteristics and their trends in the horizontal rows
(particularly 3d row) and then consider some group similarities 2nd Series
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
Z
39
40
41
42
43
44
45
46
47
48
5s
2
2
1
1
1
1
1
0
1
2
4d
1
2
4
5
6
7
8
10
10
10
3rd Series
La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Z
57
72
73
74
75
76
77
78
79
80
6s
2
2
2
2
2
2
2
1
1
2
5d
1
2
3
4
5
6
7
9
10
10
Ac
Rf
Db
Sg
Bh
Hs
Mt
Ds
Rg
Cn
Z
89
104
105
106
107
108
109
110
111
112
7s
2
2
2
2
2
2
2
2
1
2
6d
1
2
3
4
5
6
7
8
10
10
4th Series
On what ground can you say that scandium (Z = 21) is a transition
element but zinc (Z = 30) is not |
1 | 3728-3731 | However, some group similarities also exist We shall first study the
general characteristics and their trends in the horizontal rows
(particularly 3d row) and then consider some group similarities 2nd Series
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
Z
39
40
41
42
43
44
45
46
47
48
5s
2
2
1
1
1
1
1
0
1
2
4d
1
2
4
5
6
7
8
10
10
10
3rd Series
La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Z
57
72
73
74
75
76
77
78
79
80
6s
2
2
2
2
2
2
2
1
1
2
5d
1
2
3
4
5
6
7
9
10
10
Ac
Rf
Db
Sg
Bh
Hs
Mt
Ds
Rg
Cn
Z
89
104
105
106
107
108
109
110
111
112
7s
2
2
2
2
2
2
2
2
1
2
6d
1
2
3
4
5
6
7
8
10
10
4th Series
On what ground can you say that scandium (Z = 21) is a transition
element but zinc (Z = 30) is not On the basis of incompletely filled 3d orbitals in case of scandium atom
in its ground state (3d
1), it is regarded as a transition element |
1 | 3729-3732 | We shall first study the
general characteristics and their trends in the horizontal rows
(particularly 3d row) and then consider some group similarities 2nd Series
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
Z
39
40
41
42
43
44
45
46
47
48
5s
2
2
1
1
1
1
1
0
1
2
4d
1
2
4
5
6
7
8
10
10
10
3rd Series
La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Z
57
72
73
74
75
76
77
78
79
80
6s
2
2
2
2
2
2
2
1
1
2
5d
1
2
3
4
5
6
7
9
10
10
Ac
Rf
Db
Sg
Bh
Hs
Mt
Ds
Rg
Cn
Z
89
104
105
106
107
108
109
110
111
112
7s
2
2
2
2
2
2
2
2
1
2
6d
1
2
3
4
5
6
7
8
10
10
4th Series
On what ground can you say that scandium (Z = 21) is a transition
element but zinc (Z = 30) is not On the basis of incompletely filled 3d orbitals in case of scandium atom
in its ground state (3d
1), it is regarded as a transition element On the
other hand, zinc atom has completely filled d orbitals (3d
10) in its
ground state as well as in its oxidised state, hence it is not regarded
as a transition element |
1 | 3730-3733 | 2nd Series
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
Z
39
40
41
42
43
44
45
46
47
48
5s
2
2
1
1
1
1
1
0
1
2
4d
1
2
4
5
6
7
8
10
10
10
3rd Series
La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Z
57
72
73
74
75
76
77
78
79
80
6s
2
2
2
2
2
2
2
1
1
2
5d
1
2
3
4
5
6
7
9
10
10
Ac
Rf
Db
Sg
Bh
Hs
Mt
Ds
Rg
Cn
Z
89
104
105
106
107
108
109
110
111
112
7s
2
2
2
2
2
2
2
2
1
2
6d
1
2
3
4
5
6
7
8
10
10
4th Series
On what ground can you say that scandium (Z = 21) is a transition
element but zinc (Z = 30) is not On the basis of incompletely filled 3d orbitals in case of scandium atom
in its ground state (3d
1), it is regarded as a transition element On the
other hand, zinc atom has completely filled d orbitals (3d
10) in its
ground state as well as in its oxidised state, hence it is not regarded
as a transition element Example 4 |
1 | 3731-3734 | On the basis of incompletely filled 3d orbitals in case of scandium atom
in its ground state (3d
1), it is regarded as a transition element On the
other hand, zinc atom has completely filled d orbitals (3d
10) in its
ground state as well as in its oxidised state, hence it is not regarded
as a transition element Example 4 1
Example 4 |
1 | 3732-3735 | On the
other hand, zinc atom has completely filled d orbitals (3d
10) in its
ground state as well as in its oxidised state, hence it is not regarded
as a transition element Example 4 1
Example 4 1
Example 4 |
1 | 3733-3736 | Example 4 1
Example 4 1
Example 4 1
Example 4 |
1 | 3734-3737 | 1
Example 4 1
Example 4 1
Example 4 1
Example 4 |
1 | 3735-3738 | 1
Example 4 1
Example 4 1
Example 4 1
Solution
Solution
Solution
Solution
Solution
Rationalised 2023-24
92
Chemistry
1
2
3
4
M |
1 | 3736-3739 | 1
Example 4 1
Example 4 1
Solution
Solution
Solution
Solution
Solution
Rationalised 2023-24
92
Chemistry
1
2
3
4
M p |
1 | 3737-3740 | 1
Example 4 1
Solution
Solution
Solution
Solution
Solution
Rationalised 2023-24
92
Chemistry
1
2
3
4
M p /10 K
3
Ti
Zr
Hf
W
Re
Ta
Os
Ir
Ru
Mo
Nb
Tc
Rh
Cr
V
Mn
Fe
Co
Ni
Pd
Pt
Cu
Au
Ag
Atomic number
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
4 |
1 | 3738-3741 | 1
Solution
Solution
Solution
Solution
Solution
Rationalised 2023-24
92
Chemistry
1
2
3
4
M p /10 K
3
Ti
Zr
Hf
W
Re
Ta
Os
Ir
Ru
Mo
Nb
Tc
Rh
Cr
V
Mn
Fe
Co
Ni
Pd
Pt
Cu
Au
Ag
Atomic number
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
4 1 Silver atom has completely filled d orbitals (4d
10) in its ground state |
1 | 3739-3742 | p /10 K
3
Ti
Zr
Hf
W
Re
Ta
Os
Ir
Ru
Mo
Nb
Tc
Rh
Cr
V
Mn
Fe
Co
Ni
Pd
Pt
Cu
Au
Ag
Atomic number
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
4 1 Silver atom has completely filled d orbitals (4d
10) in its ground state How can you say that it is a transition element |
1 | 3740-3743 | /10 K
3
Ti
Zr
Hf
W
Re
Ta
Os
Ir
Ru
Mo
Nb
Tc
Rh
Cr
V
Mn
Fe
Co
Ni
Pd
Pt
Cu
Au
Ag
Atomic number
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
4 1 Silver atom has completely filled d orbitals (4d
10) in its ground state How can you say that it is a transition element We will discuss the properties of elements of first transition series
only in the following sections |
1 | 3741-3744 | 1 Silver atom has completely filled d orbitals (4d
10) in its ground state How can you say that it is a transition element We will discuss the properties of elements of first transition series
only in the following sections 4 |
1 | 3742-3745 | How can you say that it is a transition element We will discuss the properties of elements of first transition series
only in the following sections 4 3 |
1 | 3743-3746 | We will discuss the properties of elements of first transition series
only in the following sections 4 3 1 Physical Properties
Nearly all the transition elements display typical metallic properties
such as high tensile strength, ductility, malleability, high thermal and
electrical conductivity and metallic lustre |
1 | 3744-3747 | 4 3 1 Physical Properties
Nearly all the transition elements display typical metallic properties
such as high tensile strength, ductility, malleability, high thermal and
electrical conductivity and metallic lustre With the exceptions of Zn,
Cd, Hg and Mn, they have one or more typical metallic structures at
normal temperatures |
1 | 3745-3748 | 3 1 Physical Properties
Nearly all the transition elements display typical metallic properties
such as high tensile strength, ductility, malleability, high thermal and
electrical conductivity and metallic lustre With the exceptions of Zn,
Cd, Hg and Mn, they have one or more typical metallic structures at
normal temperatures 4 |
1 | 3746-3749 | 1 Physical Properties
Nearly all the transition elements display typical metallic properties
such as high tensile strength, ductility, malleability, high thermal and
electrical conductivity and metallic lustre With the exceptions of Zn,
Cd, Hg and Mn, they have one or more typical metallic structures at
normal temperatures 4 3
4 |
1 | 3747-3750 | With the exceptions of Zn,
Cd, Hg and Mn, they have one or more typical metallic structures at
normal temperatures 4 3
4 3
4 |
1 | 3748-3751 | 4 3
4 3
4 3
4 |
1 | 3749-3752 | 3
4 3
4 3
4 3
4 |
1 | 3750-3753 | 3
4 3
4 3
4 3 General
General
General
General
General
Properties of
Properties of
Properties of
Properties of
Properties of
the Transition
the Transition
the Transition
the Transition
the Transition
Elements
Elements
Elements
Elements
Elements
(d-Block)
(d-Block)
(d-Block)
(d-Block)
(d-Block)
(bcc = body centred cubic; hcp = hexagonal close packed;
ccp = cubic close packed; X = a typical metal structure) |
1 | 3751-3754 | 3
4 3
4 3 General
General
General
General
General
Properties of
Properties of
Properties of
Properties of
Properties of
the Transition
the Transition
the Transition
the Transition
the Transition
Elements
Elements
Elements
Elements
Elements
(d-Block)
(d-Block)
(d-Block)
(d-Block)
(d-Block)
(bcc = body centred cubic; hcp = hexagonal close packed;
ccp = cubic close packed; X = a typical metal structure) Fig |
1 | 3752-3755 | 3
4 3 General
General
General
General
General
Properties of
Properties of
Properties of
Properties of
Properties of
the Transition
the Transition
the Transition
the Transition
the Transition
Elements
Elements
Elements
Elements
Elements
(d-Block)
(d-Block)
(d-Block)
(d-Block)
(d-Block)
(bcc = body centred cubic; hcp = hexagonal close packed;
ccp = cubic close packed; X = a typical metal structure) Fig 4 |
1 | 3753-3756 | 3 General
General
General
General
General
Properties of
Properties of
Properties of
Properties of
Properties of
the Transition
the Transition
the Transition
the Transition
the Transition
Elements
Elements
Elements
Elements
Elements
(d-Block)
(d-Block)
(d-Block)
(d-Block)
(d-Block)
(bcc = body centred cubic; hcp = hexagonal close packed;
ccp = cubic close packed; X = a typical metal structure) Fig 4 1: Trends in melting points of
transition elements
The transition metals (with the exception
of Zn, Cd and Hg) are very hard and have low
volatility |
1 | 3754-3757 | Fig 4 1: Trends in melting points of
transition elements
The transition metals (with the exception
of Zn, Cd and Hg) are very hard and have low
volatility Their melting and boiling points are
high |
1 | 3755-3758 | 4 1: Trends in melting points of
transition elements
The transition metals (with the exception
of Zn, Cd and Hg) are very hard and have low
volatility Their melting and boiling points are
high Fig |
1 | 3756-3759 | 1: Trends in melting points of
transition elements
The transition metals (with the exception
of Zn, Cd and Hg) are very hard and have low
volatility Their melting and boiling points are
high Fig 4 |
1 | 3757-3760 | Their melting and boiling points are
high Fig 4 1 depicts the melting points of
transition metals belonging to 3d, 4d and 5d
series |
1 | 3758-3761 | Fig 4 1 depicts the melting points of
transition metals belonging to 3d, 4d and 5d
series The high melting points of these metals
are attributed to the involvement of greater
number of electrons from (n-1)d in addition to
the ns electrons in the interatomic metallic
bonding |
1 | 3759-3762 | 4 1 depicts the melting points of
transition metals belonging to 3d, 4d and 5d
series The high melting points of these metals
are attributed to the involvement of greater
number of electrons from (n-1)d in addition to
the ns electrons in the interatomic metallic
bonding In any row the melting points of these
metals rise to a maximum at d
5 except for
anomalous values of Mn and Tc and fall
regularly as the atomic number increases |
1 | 3760-3763 | 1 depicts the melting points of
transition metals belonging to 3d, 4d and 5d
series The high melting points of these metals
are attributed to the involvement of greater
number of electrons from (n-1)d in addition to
the ns electrons in the interatomic metallic
bonding In any row the melting points of these
metals rise to a maximum at d
5 except for
anomalous values of Mn and Tc and fall
regularly as the atomic number increases They have high enthalpies of atomisation which
are shown in Fig |
1 | 3761-3764 | The high melting points of these metals
are attributed to the involvement of greater
number of electrons from (n-1)d in addition to
the ns electrons in the interatomic metallic
bonding In any row the melting points of these
metals rise to a maximum at d
5 except for
anomalous values of Mn and Tc and fall
regularly as the atomic number increases They have high enthalpies of atomisation which
are shown in Fig 4 |
1 | 3762-3765 | In any row the melting points of these
metals rise to a maximum at d
5 except for
anomalous values of Mn and Tc and fall
regularly as the atomic number increases They have high enthalpies of atomisation which
are shown in Fig 4 2 |
1 | 3763-3766 | They have high enthalpies of atomisation which
are shown in Fig 4 2 The maxima at about
the middle of each series indicate that one
unpaired electron per d orbital is particularly
Lattice Structures of Transition Metals
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
hcp
hcp
bcc
bcc
X
bcc
ccp
ccp
ccp
X
(bcc)
(bcc)
(bcc, ccp)
(hcp)
(hcp)
(hcp)
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
hcp
hcp
bcc
bcc
hcp
hcp
ccp
ccp
ccp
X
(bcc)
(bcc)
(hcp)
La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
hcp
hcp
bcc
bcc
hcp
hcp
ccp
ccp
ccp
X
(ccp,bcc)
(bcc)
Rationalised 2023-24
93
The d- and f- Block Elements
favourable for strong interatomic interaction |
1 | 3764-3767 | 4 2 The maxima at about
the middle of each series indicate that one
unpaired electron per d orbital is particularly
Lattice Structures of Transition Metals
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
hcp
hcp
bcc
bcc
X
bcc
ccp
ccp
ccp
X
(bcc)
(bcc)
(bcc, ccp)
(hcp)
(hcp)
(hcp)
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
hcp
hcp
bcc
bcc
hcp
hcp
ccp
ccp
ccp
X
(bcc)
(bcc)
(hcp)
La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
hcp
hcp
bcc
bcc
hcp
hcp
ccp
ccp
ccp
X
(ccp,bcc)
(bcc)
Rationalised 2023-24
93
The d- and f- Block Elements
favourable for strong interatomic interaction In general, greater the
number of valence electrons, stronger is the resultant bonding |
1 | 3765-3768 | 2 The maxima at about
the middle of each series indicate that one
unpaired electron per d orbital is particularly
Lattice Structures of Transition Metals
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
hcp
hcp
bcc
bcc
X
bcc
ccp
ccp
ccp
X
(bcc)
(bcc)
(bcc, ccp)
(hcp)
(hcp)
(hcp)
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
hcp
hcp
bcc
bcc
hcp
hcp
ccp
ccp
ccp
X
(bcc)
(bcc)
(hcp)
La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
hcp
hcp
bcc
bcc
hcp
hcp
ccp
ccp
ccp
X
(ccp,bcc)
(bcc)
Rationalised 2023-24
93
The d- and f- Block Elements
favourable for strong interatomic interaction In general, greater the
number of valence electrons, stronger is the resultant bonding Since
the enthalpy of atomisation is an important factor in determining the
standard electrode potential of a metal, metals with very high enthalpy
of atomisation (i |
1 | 3766-3769 | The maxima at about
the middle of each series indicate that one
unpaired electron per d orbital is particularly
Lattice Structures of Transition Metals
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
hcp
hcp
bcc
bcc
X
bcc
ccp
ccp
ccp
X
(bcc)
(bcc)
(bcc, ccp)
(hcp)
(hcp)
(hcp)
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
hcp
hcp
bcc
bcc
hcp
hcp
ccp
ccp
ccp
X
(bcc)
(bcc)
(hcp)
La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
hcp
hcp
bcc
bcc
hcp
hcp
ccp
ccp
ccp
X
(ccp,bcc)
(bcc)
Rationalised 2023-24
93
The d- and f- Block Elements
favourable for strong interatomic interaction In general, greater the
number of valence electrons, stronger is the resultant bonding Since
the enthalpy of atomisation is an important factor in determining the
standard electrode potential of a metal, metals with very high enthalpy
of atomisation (i e |
1 | 3767-3770 | In general, greater the
number of valence electrons, stronger is the resultant bonding Since
the enthalpy of atomisation is an important factor in determining the
standard electrode potential of a metal, metals with very high enthalpy
of atomisation (i e , very high boiling point) tend to be noble in their
reactions (see later for electrode potentials) |
1 | 3768-3771 | Since
the enthalpy of atomisation is an important factor in determining the
standard electrode potential of a metal, metals with very high enthalpy
of atomisation (i e , very high boiling point) tend to be noble in their
reactions (see later for electrode potentials) Another generalisation that may be drawn from Fig |
1 | 3769-3772 | e , very high boiling point) tend to be noble in their
reactions (see later for electrode potentials) Another generalisation that may be drawn from Fig 4 |
1 | 3770-3773 | , very high boiling point) tend to be noble in their
reactions (see later for electrode potentials) Another generalisation that may be drawn from Fig 4 2 is that the
metals of the second and third series have greater enthalpies of
atomisation than the corresponding elements of the first series; this is an
important factor in accounting for the occurrence of much more frequent
metal β metal bonding in compounds of the heavy transition metals |
1 | 3771-3774 | Another generalisation that may be drawn from Fig 4 2 is that the
metals of the second and third series have greater enthalpies of
atomisation than the corresponding elements of the first series; this is an
important factor in accounting for the occurrence of much more frequent
metal β metal bonding in compounds of the heavy transition metals Fig |
1 | 3772-3775 | 4 2 is that the
metals of the second and third series have greater enthalpies of
atomisation than the corresponding elements of the first series; this is an
important factor in accounting for the occurrence of much more frequent
metal β metal bonding in compounds of the heavy transition metals Fig 4 |
1 | 3773-3776 | 2 is that the
metals of the second and third series have greater enthalpies of
atomisation than the corresponding elements of the first series; this is an
important factor in accounting for the occurrence of much more frequent
metal β metal bonding in compounds of the heavy transition metals Fig 4 2
Trends in enthalpies
of atomisation of
transition elements
In general, ions of the same charge in a given series show progressive
decrease in radius with increasing atomic number |
1 | 3774-3777 | Fig 4 2
Trends in enthalpies
of atomisation of
transition elements
In general, ions of the same charge in a given series show progressive
decrease in radius with increasing atomic number This is because the
new electron enters a d orbital each time the nuclear charge increases
by unity |
1 | 3775-3778 | 4 2
Trends in enthalpies
of atomisation of
transition elements
In general, ions of the same charge in a given series show progressive
decrease in radius with increasing atomic number This is because the
new electron enters a d orbital each time the nuclear charge increases
by unity It may be recalled that the shielding effect of a d electron is
not that effective, hence the net electrostatic attraction between the
nuclear charge and the outermost electron increases and the ionic
radius decreases |
1 | 3776-3779 | 2
Trends in enthalpies
of atomisation of
transition elements
In general, ions of the same charge in a given series show progressive
decrease in radius with increasing atomic number This is because the
new electron enters a d orbital each time the nuclear charge increases
by unity It may be recalled that the shielding effect of a d electron is
not that effective, hence the net electrostatic attraction between the
nuclear charge and the outermost electron increases and the ionic
radius decreases The same trend is observed in the atomic radii of a
given series |
1 | 3777-3780 | This is because the
new electron enters a d orbital each time the nuclear charge increases
by unity It may be recalled that the shielding effect of a d electron is
not that effective, hence the net electrostatic attraction between the
nuclear charge and the outermost electron increases and the ionic
radius decreases The same trend is observed in the atomic radii of a
given series However, the variation within a series is quite small |
1 | 3778-3781 | It may be recalled that the shielding effect of a d electron is
not that effective, hence the net electrostatic attraction between the
nuclear charge and the outermost electron increases and the ionic
radius decreases The same trend is observed in the atomic radii of a
given series However, the variation within a series is quite small An
interesting point emerges when atomic sizes of one series are compared
with those of the corresponding elements in the other series |
1 | 3779-3782 | The same trend is observed in the atomic radii of a
given series However, the variation within a series is quite small An
interesting point emerges when atomic sizes of one series are compared
with those of the corresponding elements in the other series The curves
in Fig |
1 | 3780-3783 | However, the variation within a series is quite small An
interesting point emerges when atomic sizes of one series are compared
with those of the corresponding elements in the other series The curves
in Fig 4 |
1 | 3781-3784 | An
interesting point emerges when atomic sizes of one series are compared
with those of the corresponding elements in the other series The curves
in Fig 4 3 show an increase from the first (3d) to the second (4d) series
of the elements but the radii of the third (5d) series are virtually the
same as those of the corresponding members of the second series |
1 | 3782-3785 | The curves
in Fig 4 3 show an increase from the first (3d) to the second (4d) series
of the elements but the radii of the third (5d) series are virtually the
same as those of the corresponding members of the second series This
phenomenon is associated with the intervention of the 4f orbitals which
must be filled before the 5d series of elements begin |
1 | 3783-3786 | 4 3 show an increase from the first (3d) to the second (4d) series
of the elements but the radii of the third (5d) series are virtually the
same as those of the corresponding members of the second series This
phenomenon is associated with the intervention of the 4f orbitals which
must be filled before the 5d series of elements begin The filling of 4f
before 5d orbital results in a regular decrease in atomic radii called
Lanthanoid contraction which essentially compensates for the expected
4 |
1 | 3784-3787 | 3 show an increase from the first (3d) to the second (4d) series
of the elements but the radii of the third (5d) series are virtually the
same as those of the corresponding members of the second series This
phenomenon is associated with the intervention of the 4f orbitals which
must be filled before the 5d series of elements begin The filling of 4f
before 5d orbital results in a regular decrease in atomic radii called
Lanthanoid contraction which essentially compensates for the expected
4 3 |
1 | 3785-3788 | This
phenomenon is associated with the intervention of the 4f orbitals which
must be filled before the 5d series of elements begin The filling of 4f
before 5d orbital results in a regular decrease in atomic radii called
Lanthanoid contraction which essentially compensates for the expected
4 3 2 Variation in
Atomic and
Ionic Sizes
of
Transition
Metals
οΏ½aH
οΏ½/kJ mol
β1
Rationalised 2023-24
94
Chemistry
increase in atomic size with increasing atomic number |
1 | 3786-3789 | The filling of 4f
before 5d orbital results in a regular decrease in atomic radii called
Lanthanoid contraction which essentially compensates for the expected
4 3 2 Variation in
Atomic and
Ionic Sizes
of
Transition
Metals
οΏ½aH
οΏ½/kJ mol
β1
Rationalised 2023-24
94
Chemistry
increase in atomic size with increasing atomic number The net result
of the lanthanoid contraction is that the second and the third d series
exhibit similar radii (e |
1 | 3787-3790 | 3 2 Variation in
Atomic and
Ionic Sizes
of
Transition
Metals
οΏ½aH
οΏ½/kJ mol
β1
Rationalised 2023-24
94
Chemistry
increase in atomic size with increasing atomic number The net result
of the lanthanoid contraction is that the second and the third d series
exhibit similar radii (e g |
1 | 3788-3791 | 2 Variation in
Atomic and
Ionic Sizes
of
Transition
Metals
οΏ½aH
οΏ½/kJ mol
β1
Rationalised 2023-24
94
Chemistry
increase in atomic size with increasing atomic number The net result
of the lanthanoid contraction is that the second and the third d series
exhibit similar radii (e g , Zr 160 pm, Hf 159 pm) and have very similar
physical and chemical properties much more than that expected on
the basis of usual family relationship |
1 | 3789-3792 | The net result
of the lanthanoid contraction is that the second and the third d series
exhibit similar radii (e g , Zr 160 pm, Hf 159 pm) and have very similar
physical and chemical properties much more than that expected on
the basis of usual family relationship The factor responsible for the lanthanoid
contraction is somewhat similar to that observed
in an ordinary transition series and is attributed
to similar cause, i |
1 | 3790-3793 | g , Zr 160 pm, Hf 159 pm) and have very similar
physical and chemical properties much more than that expected on
the basis of usual family relationship The factor responsible for the lanthanoid
contraction is somewhat similar to that observed
in an ordinary transition series and is attributed
to similar cause, i e |
1 | 3791-3794 | , Zr 160 pm, Hf 159 pm) and have very similar
physical and chemical properties much more than that expected on
the basis of usual family relationship The factor responsible for the lanthanoid
contraction is somewhat similar to that observed
in an ordinary transition series and is attributed
to similar cause, i e , the imperfect shielding of
one electron by another in the same set of orbitals |
1 | 3792-3795 | The factor responsible for the lanthanoid
contraction is somewhat similar to that observed
in an ordinary transition series and is attributed
to similar cause, i e , the imperfect shielding of
one electron by another in the same set of orbitals However, the shielding of one 4f electron by
another is less than that of one d electron by
another, and as the nuclear charge increases
along the series, there is fairly regular decrease
in the size of the entire 4f
n orbitals |
1 | 3793-3796 | e , the imperfect shielding of
one electron by another in the same set of orbitals However, the shielding of one 4f electron by
another is less than that of one d electron by
another, and as the nuclear charge increases
along the series, there is fairly regular decrease
in the size of the entire 4f
n orbitals The decrease in metallic radius coupled with
increase in atomic mass results in a general
increase in the density of these elements |
1 | 3794-3797 | , the imperfect shielding of
one electron by another in the same set of orbitals However, the shielding of one 4f electron by
another is less than that of one d electron by
another, and as the nuclear charge increases
along the series, there is fairly regular decrease
in the size of the entire 4f
n orbitals The decrease in metallic radius coupled with
increase in atomic mass results in a general
increase in the density of these elements Thus,
from titanium (Z = 22) to copper (Z = 29) the
significant increase in the density may be noted
(Table 4 |
1 | 3795-3798 | However, the shielding of one 4f electron by
another is less than that of one d electron by
another, and as the nuclear charge increases
along the series, there is fairly regular decrease
in the size of the entire 4f
n orbitals The decrease in metallic radius coupled with
increase in atomic mass results in a general
increase in the density of these elements Thus,
from titanium (Z = 22) to copper (Z = 29) the
significant increase in the density may be noted
(Table 4 2) |
1 | 3796-3799 | The decrease in metallic radius coupled with
increase in atomic mass results in a general
increase in the density of these elements Thus,
from titanium (Z = 22) to copper (Z = 29) the
significant increase in the density may be noted
(Table 4 2) 19
18
16
15
13
12
Sc Ti
V
Cr Mn Fe
Co Ni Cu Zn
Y
Zr Nb Mo Tc Ru
Rh Pd Ag Cd
La Hf Ta
W
Re Os
Ir
Pt
Au Hg
Radius/nm
17
14
Fig |
1 | 3797-3800 | Thus,
from titanium (Z = 22) to copper (Z = 29) the
significant increase in the density may be noted
(Table 4 2) 19
18
16
15
13
12
Sc Ti
V
Cr Mn Fe
Co Ni Cu Zn
Y
Zr Nb Mo Tc Ru
Rh Pd Ag Cd
La Hf Ta
W
Re Os
Ir
Pt
Au Hg
Radius/nm
17
14
Fig 4 |
1 | 3798-3801 | 2) 19
18
16
15
13
12
Sc Ti
V
Cr Mn Fe
Co Ni Cu Zn
Y
Zr Nb Mo Tc Ru
Rh Pd Ag Cd
La Hf Ta
W
Re Os
Ir
Pt
Au Hg
Radius/nm
17
14
Fig 4 3: Trends in atomic radii of
transition elements
Atomic number
21
22
23
24
25
26
27
28
29
30
Electronic configuration
M
3d
14s
2
3d
24s
2
3d
34s
2
3d
54s
1 3d
54s
2
3d
64s
2
3d
74s
2
3d
84s
2
3d
104s
1
3d
104s
2
M
+
3d
14s
1
3d
24s
1
3d
34s
1
3d
5
3d
54s
1
3d
64s
1
3d
74s
1
3d
84s
1
3d
10
3d
104s
1
M
2+
3d
1
3d
2
3d
3
3d
4
3d
5
3d
6
3d
7
3d
8
3d
9
3d
10
M
3+
[Ar]
3d
1
3d
2
3d
3
3d
4
3d
5
3d
6
3d
7
β
β
Enthalpy of atomisation, DaH o/kJ mol
β1
326
473
515
397
281
416
425
430
339
126
Ionisation enthalpy/DDDDDiH o/kJ mol
β1
DiHo
I
631
656
650
653
717
762
758
736
745
906
DiHo
II
1235
1309
1414
1592
1509
1561
1644
1752
1958
1734
DiHo
III
2393
2657
2833
2990
3260
2962
3243
3402
3556
3837
Metallic/ionic
M
164
147
135
129
137
126
125
125
128
137
radii/pm
M
2+
β
β
79
82
82
77
74
70
73
75
M
3+
73
67
64
62
65
65
61
60
β
β
Standard
electrode
M
2+/M
β
β1 |
1 | 3799-3802 | 19
18
16
15
13
12
Sc Ti
V
Cr Mn Fe
Co Ni Cu Zn
Y
Zr Nb Mo Tc Ru
Rh Pd Ag Cd
La Hf Ta
W
Re Os
Ir
Pt
Au Hg
Radius/nm
17
14
Fig 4 3: Trends in atomic radii of
transition elements
Atomic number
21
22
23
24
25
26
27
28
29
30
Electronic configuration
M
3d
14s
2
3d
24s
2
3d
34s
2
3d
54s
1 3d
54s
2
3d
64s
2
3d
74s
2
3d
84s
2
3d
104s
1
3d
104s
2
M
+
3d
14s
1
3d
24s
1
3d
34s
1
3d
5
3d
54s
1
3d
64s
1
3d
74s
1
3d
84s
1
3d
10
3d
104s
1
M
2+
3d
1
3d
2
3d
3
3d
4
3d
5
3d
6
3d
7
3d
8
3d
9
3d
10
M
3+
[Ar]
3d
1
3d
2
3d
3
3d
4
3d
5
3d
6
3d
7
β
β
Enthalpy of atomisation, DaH o/kJ mol
β1
326
473
515
397
281
416
425
430
339
126
Ionisation enthalpy/DDDDDiH o/kJ mol
β1
DiHo
I
631
656
650
653
717
762
758
736
745
906
DiHo
II
1235
1309
1414
1592
1509
1561
1644
1752
1958
1734
DiHo
III
2393
2657
2833
2990
3260
2962
3243
3402
3556
3837
Metallic/ionic
M
164
147
135
129
137
126
125
125
128
137
radii/pm
M
2+
β
β
79
82
82
77
74
70
73
75
M
3+
73
67
64
62
65
65
61
60
β
β
Standard
electrode
M
2+/M
β
β1 63
β1 |
1 | 3800-3803 | 4 3: Trends in atomic radii of
transition elements
Atomic number
21
22
23
24
25
26
27
28
29
30
Electronic configuration
M
3d
14s
2
3d
24s
2
3d
34s
2
3d
54s
1 3d
54s
2
3d
64s
2
3d
74s
2
3d
84s
2
3d
104s
1
3d
104s
2
M
+
3d
14s
1
3d
24s
1
3d
34s
1
3d
5
3d
54s
1
3d
64s
1
3d
74s
1
3d
84s
1
3d
10
3d
104s
1
M
2+
3d
1
3d
2
3d
3
3d
4
3d
5
3d
6
3d
7
3d
8
3d
9
3d
10
M
3+
[Ar]
3d
1
3d
2
3d
3
3d
4
3d
5
3d
6
3d
7
β
β
Enthalpy of atomisation, DaH o/kJ mol
β1
326
473
515
397
281
416
425
430
339
126
Ionisation enthalpy/DDDDDiH o/kJ mol
β1
DiHo
I
631
656
650
653
717
762
758
736
745
906
DiHo
II
1235
1309
1414
1592
1509
1561
1644
1752
1958
1734
DiHo
III
2393
2657
2833
2990
3260
2962
3243
3402
3556
3837
Metallic/ionic
M
164
147
135
129
137
126
125
125
128
137
radii/pm
M
2+
β
β
79
82
82
77
74
70
73
75
M
3+
73
67
64
62
65
65
61
60
β
β
Standard
electrode
M
2+/M
β
β1 63
β1 18
β0 |
1 | 3801-3804 | 3: Trends in atomic radii of
transition elements
Atomic number
21
22
23
24
25
26
27
28
29
30
Electronic configuration
M
3d
14s
2
3d
24s
2
3d
34s
2
3d
54s
1 3d
54s
2
3d
64s
2
3d
74s
2
3d
84s
2
3d
104s
1
3d
104s
2
M
+
3d
14s
1
3d
24s
1
3d
34s
1
3d
5
3d
54s
1
3d
64s
1
3d
74s
1
3d
84s
1
3d
10
3d
104s
1
M
2+
3d
1
3d
2
3d
3
3d
4
3d
5
3d
6
3d
7
3d
8
3d
9
3d
10
M
3+
[Ar]
3d
1
3d
2
3d
3
3d
4
3d
5
3d
6
3d
7
β
β
Enthalpy of atomisation, DaH o/kJ mol
β1
326
473
515
397
281
416
425
430
339
126
Ionisation enthalpy/DDDDDiH o/kJ mol
β1
DiHo
I
631
656
650
653
717
762
758
736
745
906
DiHo
II
1235
1309
1414
1592
1509
1561
1644
1752
1958
1734
DiHo
III
2393
2657
2833
2990
3260
2962
3243
3402
3556
3837
Metallic/ionic
M
164
147
135
129
137
126
125
125
128
137
radii/pm
M
2+
β
β
79
82
82
77
74
70
73
75
M
3+
73
67
64
62
65
65
61
60
β
β
Standard
electrode
M
2+/M
β
β1 63
β1 18
β0 90
β1 |
1 | 3802-3805 | 63
β1 18
β0 90
β1 18
β0 |
1 | 3803-3806 | 18
β0 90
β1 18
β0 44
β0 |
1 | 3804-3807 | 90
β1 18
β0 44
β0 28
β0 |
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