Transition Metals

Transition Metals

Basics

• Transition metals are located in the centre of the Periodic table, between Groups 2 and 3.
• They include common metals such as iron, copper, and nickel.
• Generally, they are lustrous, conductive, malleable, and ductile.

Electron Configuration and Behaviour

• Transition metals have a unique electron configuration. They have up to ten d-electrons which can be lost, resulting in multiple oxidation states.
• The ability to exhibit varying oxidation states allows transition metals to partake in a range of chemical reactions and form many different compounds.

Colour Properties

• Transition metals and their compounds are often associated with vivid colours.
• The colours arise due to the presence of unpaired electrons in the d-orbitals of the metal ions which absorb particular wavelengths of light.
• This light absorption shifts electrons between energy levels, producing the striking colours characteristic of these compounds.

Catalytic Activity

• Transition metals often function as effective catalysts in chemical reactions, aiding in reaction rate increase without being consumed in the process.
• Transition metals like Platinum and Iron are commonly used in industry for their catalytic properties.

Magnetism

• The presence of unpaired electrons in the d-orbitals can give transition metals, such as iron, cobalt and nickel, magnetic properties.

Real World Applications

• Transition metals and their compounds have numerous applications, from serving as catalysts in industry to being used in the production of coloured pigments and electronic components.
• High densities and melting points make transition metals suitable for construction materials and tools.