MCQ Detailed View

Vanadium is a transition metal with the atomic number 23. It exhibits multiple oxidation states, ranging from +2 to +5. The common oxidation states of vanadium are V²⁺, V³⁺, V⁴⁺, and V⁵⁺, each with distinct chemical properties. The stability of an oxidation state depends on electronic configuration, lattice energy, and ligand interactions.

The electronic configuration of vanadium is [Ar] 3d³ 4s². In the +3 oxidation state (V³⁺), vanadium loses its two 4s electrons and one 3d electron, resulting in a 3d² configuration. This partially filled d-orbital provides extra stability due to exchange energy and crystal field stabilization. As a result, V³⁺ is the most stable oxidation state of vanadium under normal conditions.

The +2 oxidation state (V²⁺) is less stable because it has more unpaired electrons, making it more prone to oxidation. The +4 (V⁴⁺) and +5 (V⁵⁺) oxidation states are stabilized in the presence of strong oxidizing agents or in compounds such as vanadyl ions (VO²⁺) and vanadates (VO₄³⁻), but they are generally less stable in aqueous solution compared to V³⁺.

Understanding the stability of vanadium oxidation states is important in inorganic chemistry, particularly in redox reactions, coordination chemistry, and catalysis. V³⁺ is commonly found in compounds like VCl₃ and acts as a reducing agent in many chemical processes.

The stability trend of vanadium’s oxidation states can also be linked to the effective nuclear charge, electronic repulsion, and ligand effects. Among all the oxidation states, V³⁺ provides the best balance between electronic stability and chemical reactivity, making it the most stable form of vanadium in ordinary chemical conditions.