MCQ Detailed View

Transition elements are d-block elements in the periodic table, characterized by partially filled d-orbitals. They exhibit several common properties that distinguish them from s- and p-block elements. One important property is variable oxidation states. Because electrons in the (n–1)d and ns orbitals have similar energies, transition metals can lose different numbers of electrons, forming multiple oxidation states.

Another characteristic property is the tendency to form complexes. Transition metals have vacant d-orbitals that can accept electron pairs from ligands, allowing them to form coordination compounds with various geometries. This property is extensively utilized in analytical chemistry and industrial catalysis.

Transition elements also have a strong tendency for alloy formation. Metals like iron, copper, and nickel readily combine with other metals to produce alloys with improved strength, corrosion resistance, or other mechanical properties. For example, steel is an alloy of iron with carbon, and brass is an alloy of copper and zinc.

The property that is not common among transition elements is natural radioactivity. While a few elements at the end of the d-block (like technetium and promethium) or actinides may be radioactive, most transition metals are stable and do not exhibit natural radioactivity. Natural radioactivity is not a defining or general property of transition elements.

Other features of transition metals include forming colored ions, paramagnetism, and catalytic activity, all of which are linked to their partially filled d-orbitals. By understanding these properties, students can distinguish common traits of transition elements from exceptions such as radioactive behavior.