Transition elements are elements whose atoms have incomplete d sub-shells or whose ions have incompletely filled d orbitals. They lie between the highly electropositive s-block elements and highly electronegative p-block elements in the periodic table. While all transition elements are d-block elements, not all d-block elements are transition elements as some like zinc, cadmium, and mercury have completely filled d orbitals. Transition elements are divided into four series based on their electronic configurations.

1. d f Block Elements
d Block elements
A transition element may be defined as an element
whose atom in the ground state or ion in common
oxidation state has incomplete sub-shell, has electron 1 to
9. It is called transition element due to fact that it is lying
between most electropositive (s-block) and most
electronegative (p-block) elements and represents a
transition from them. The general electronic configuration
of this element is (n-1)1 to 10 ns
0 to 2.
The definition of transition metal excludes Zn, Cd and
Hg because they have complete d- orbital. Their common
oxidation state is Zn++, Cd++, Hg++. They also do not show

2. the characteristics of transition element. Element of group
3 (Sc, Y, La and Ac) and group 12 (Zn, Cd, Hg) are called
non typical transition element.
First transition or 3d series
Second transition or 4d-series:

3. Third transition or 5d-series

4. Fourth transition or 6d-series:
Elements marked with asterisk have anomalous
configurations. These are attributed to factors like nuclearelectron and electron-electron forces and stability of half
filled and full filled orbital.
All transition elements are d block elements but all d
block elements are not transition elements.

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