Periodic table of 118 elements

1. d & f block elements
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2. 1
- 2
1-
10ns
2n
-
d
3d 15T.S
4d 2ndTS
sa 30d4.5
6d 2MTs
(n-
2)f(
-
14(n-
1)d0ns

3. Elements of groups 3-12 in the periodic table
Also called transition metals
Last electron enters in the penultimate d - orbital

4. Electronic configuration of the d-Block elements
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amfar
-

5. 2
aVYrYa
i.
v
.
& 525nd
M
sat4s2 said
sat
s
36545
3d145/

6. Scandium, Sc
Titanium, Ti
Vanadium, V
Chromium, Cr
Manganese, Mn
Iron, Fe
Cobalt, Co
Nickel, Ni
Copper, Cu
Zinc, Zn
[Ar] 3d 4s
1 2
[Ar] 3d 4s
2 2
[Ar] 3d 4s
3 2
[Ar] 3d 4s
5 1
[Ar] 3d 4s
5 2
[Ar] 3d 4s
6 2
[Ar] 3d 4s
7 2
[Ar] 3d 4s
8 2
[Ar] 3d 4s
10 1
[Ar] 3d 4s
10 2

7. Exceptional Electronic Configuration
Chromium :
Copper :
“Half filled and fully filled configuration is more stable than
partially filled configuration”.
36545'
3d9451

8. Q.
Cr, (n.

9. All transition elelments are d- block
elements, but all d - block elements are
not transition elements ?
Fe
=
3d"as
23a+ =
3d"
Fe

10. Transition metals
A transition metal is defined as the one which has incompletely filled
d orbital in its ground state or in any one of its oxidation states
Zinc, cadmium and mercury are not regarded as transition metals
General electronic configuration is
♻
♻
( n-1)d ns
1-10 1-2
r
I
⑩

11. Zn (atomic number = 30) is not a transition element, though it
is a d block element. Why?
Q.
32 =
361452
2n2
+
=
3d10

12. Q.
zn,
cd,
Ag.

13. General Characteristics
Atomic and ionic radii
Melting point and boiling point
lonisation enthalpy
Oxidation states
Magnetic properties

14. Formation of complexes
Formation of coloured compounds
Catalytic properties
Interstitial compounds formation
Alloy formation
Electrode potential
♻

15. Atomic and ionic radii
In a given transition series, the atomic and ionic radii first
decreases, then become constant and increases towards the end
of the series.
The atomic and ionic radii of 2nd and 3rd row transition metals
are quite similar. This is due to the Lanthanide contraction.
1
·
x.
⑨

16. F block
d block
T.S
1st
and
3od
4th.

17. Q.
h.c.

18. Melting point and boiling point
In a given transition series the melting and boiling points 1st
increases up to the middle and then decreases.
As the number of unpaired electron increases, the metallic bond
strength increases. Hence the melting point also increases.
In a given transition series, the number of unpaired electrons
increases up to the middle and then decreases.
♻
♻
♻
⑩
X

19. High enthalpy of atomisation
_

20. Why do the transition elements exhibit higher enthalpies
of atomisation?
Due to the presence of unpaired electrons, they have strong interatomic
interaction. Thus they have high enthalpy of atomisation.

21. Ionisation enthalpy
The ionisation enthalpy of transition elements generally increases
from left to right. This is due to increase in nuclear charge. But the
increase is not regular.
The first ionisation enthalpies of Cr and Cu are low. This is because
the removal of one electron does not change their d configuration.
♻

22. l
Cr =
3d545' 1st1.E = loue.
(n =
3d104512nd1.E=hish
1st I.E
=lush.
Mr =
3d5452
2
2nd1.7-lare.
24
=
3d1045

23. The 2nd ionisation energy of Cr and Cu are very high.
This is because the removal of one more electron from these metals
disrupted their stable configuration (d or d )
The 2nd ionisation enthalpies of Mn and Zn are lower than the
1st Ionisation enthalpies, this is because after the removal of one
more electron, they attain the stable half filled or completely filled
electronic configuration.
5 10
♻

24. Oxidation State
Transition metals show variable oxidation states. This is because
in chemical reactions along with s-electrons, d-electrons also
participate.
3dkS
②
o o
②

25. Common on state (d block)s =
+
2 -

26. Magnetic Properties
Spin Magnetic moment :
Paramagnetism is due to the presence of unpaired electrons.
As the number of unpaired electrons increases paramagnetism
increases.
->
paramagnetic
->
piamagnetic.
BM.
Iwoympaised is

27. n(n +
2
m
=
aS n =
r 3
M. =
3d5452
=
⑤(5
+
a)
2+
=
365450
M =
55Bm
-
⑭
1
(1/7 -
15
n
=
5.

28. Formation of coloured ions or compounds
Due to the presence of unpaired electrons in d orbitals.
When an electron from a lower energy d orbital is excited
to a higher energy d orbital, (d-d transition) the energy of
excitation corresponds to the frequency of light absorbed.

29. .IT

30. d10or do
-
- -
-
2n =
3d'4S
2
30
2n2+ =
3d10. ->
HiL
T fulyhiled
dd tons
asovi
=
3d5452
Niat =
3d8.
↑k
n
=
2,1 coloured.

31. Ti2+ =
32482n=
21
-
4i =
362452
414+ =
3d045
o
d colonless
= =

32. Formation of Complexes
Transition metals form a large no. of complexes.
This is due to:
1. Comparatively smaller size
2. High ionic charge
3. Presence of partially filled d orbitals
4. Ability to show variable oxidation state
⑤
2
⑨
v

33. Catalytic Property
Transition metals act as catalysts in a large no. of chemical reactions.
This is due to their large surface area and their ability to show
variable oxidation state.
haber =
Fe.
Conduct
=
v205

34. n

35. B.

36. Interstitial Compound Formation
These are formed when smaller atoms like H, N, C, B etc. are
trapped inside the crystal lattice of the metal.
They are usually non-stoichiometric and neither typically ionic nor
covalent.
Examples: Fe3H, Mn4N, TiC, VH0.56, TiH1.7 etc
♻
♻
♻

37. 1) They have high melting point.
2) They are very hard.
3) They retain metallic conductivity.
4) They are chemically inert.
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38. Alloy Formation
Alloys are homogeneous solid solutions of elements in which at
least one element is a metal.
Because of similar radii and other characteristics of Transition
metals, they readily form alloys.
The alloys formed are hard and have high m.p.
Examples: Bronze (Cu, Zn), Stainless steel (Fe, C, Ni, Mn and Cr).
♻
Reason

39. M /M Electrode Potential
Copper has positive potential - The high energy to transform
Cu(s) to Cu (aq) is not balanced by its hydration enthalpy
2+
2+
(u2+/cn = 0.34
cu -> (ya+
2
Snydeation
1123z-

40. ⑭
cu2t stable.
-
cut
in (as) sain unstable.
Reason, lane hydration enthalpy ofcution.
-
hydratin a stability.
hydration I range
enthalpy. Siz

41. thank goin