|It commonly refers to any element in the
d-block of the periodic table.
The first definition is simple and has traditionally
been used. However, many interesting properties of the
transition elements as a group are the result of their
partly filled d-subshell. Periodic trends in the d
block (transition metals) are less prevailing than in
the rest of the periodic table. Going across a period,
the valence doesn't change, so the electron being added
to an atom goes to the inner shell, not outer shell,
strengthening the shield.
The (loosely defined) transition metals are the 40
chemical elements 21 to 30, 39 to 48, 71 to 80, and 103
to 112. The name transition comes from their position in
the periodic table of elements. In each of the four
periods in which they occur, these elements represent
the successive addition of electrons to the d atomic
orbitals of the atoms. In this way, the transition
metals represent the transition between group 2 elements
and group 13 elements.
Transition elements tend to have high tensile
strength, density and melting and boiling points. As
with many properties of transition metals, this is due
to d orbital electrons' ability to delocalize within the
metal lattice. In metallic substances, the more
electrons shared between nuclei, the stronger the metal.
are several common characteristic properties of
often form colored compounds.
can have a variety of different oxidation
least one of their compounds has an incomplete
are often good catalysts.
are silvery-blue at room temperature (except copper
are solids at room temperature (except
form complex ions (aqua ions included).
are often paramagnetic.