Transition metals, found in the center block (d-block) of the periodic table, are known for their ability to exhibit multiple oxidation states—meaning they can lose different numbers of electrons depending on the chemical environment.

This happens because transition metals have incomplete d-subshells, and both their outermost (s) and inner (d) electrons can participate in bonding. As a result, they can form a variety of ions with different charges.

Examples:

• Iron (Fe) can exist as Fe²⁺ and Fe³⁺
• Copper (Cu) can be Cu⁺ or Cu²⁺
• Manganese (Mn) can show oxidation states from +2 to +7

This versatility in oxidation states allows transition metals to:

• Form a wide range of colored compounds
• Serve as effective catalysts in industrial and biological processes
• Exhibit complex magnetic and conductive properties

These characteristics make transition metals crucial in chemical reactions, materials science, and biochemistry.