General Properties of Transition Metals

Transition metals are a group of metals, located in the d-block of the periodic table.

Metallic Structures and Characteristics

Transition metals typically form colourful compounds due to d-d transitions.
These metals have high melting and boiling points due to strong metallic bonding, caused by a large number of delocalized electrons in their metal lattice.
Transition metals are highly conductive, again due to the sea of delocalized electrons that they possess.
They generally have high densities when compared to other elements.

Transition metals are known for their ability to form a number of stable oxidation states.
Transition metals show variable oxidation states and have a strong tendency to form complex ions.
The incomplete d orbitals in transition metals allow them to act as good catalysts.
Many transition metals are often involved in redox reactions and often show high reactivity with oxygen and acids.

Iron, copper, zinc, nickel, chromium, platinum, and gold are examples of transition metals.
Iron is used for construction and making tools, due to it being hard and tough.
Copper is used for electrical wiring due to its excellent ability to conduct electricity.
Zinc is often used as a protective coating for iron, to prevent rusting.
Chromium is used in stainless steel to prevent rusting, while platinum and gold are prized for their corrosion resistance and are used in jewellery.