Vanadium

Vanadium is a hard, ductile metal with a silvery-grey appearance. It is known for being harder than most metals and offering excellent corrosion resistance to alkalis and acids. It has an atomic number of 23 and is represented by the symbol V. Vanadium belongs to the transition metal category, positioned in period 4 and group 5 of the periodic table.

1.0Introduction

The metallic blue-silvery-grey element vanadium is a member of Group 5 of the periodic table. It was first discovered in 1801 by the Mexican-Spanish scientist Andrés Manuel del Río. Later, in 1830, a Swedish scientist named Nils Gabriel Sefström successfully isolated vanadium. British chemist Henry Enfield Roscoe achieved pure vanadium in 1867.

With a rank of 20th in the Earth's crust, vanadium is one of the most prevalent metallic elements. Additionally, it has been detected in the light that the Sun and a few other stars release. Roughly 65 distinct vanadium compounds occur naturally, while pure vanadium is uncommon. Substances are found in nature. Vanadium is mainly mined from patronite (VS₄) ores for commercial use.

2.0Physical Properties of vanadium 

3.0Chemical properties of Vanadium

It can be found in several oxidation states, the most prevalent of which are +2, +3, +4, and +5.

Due to its diversity in oxidation states, it can be used in various chemical reactions and applications.

Reactivity with Acids:

• Alkalis, hydrochloric acid, and diluted sulfuric acid cannot corrode vanadium.
• On the other hand, vanadium oxides can be created when it reacts with strong acids. 

Formation of Vanadium Oxides:

• The most commonly used vanadium oxide is vanadium pentoxide (V₂O₅), produced when vanadium reacts with oxygen at elevated temperatures.
• The reaction can be represented as:

4V + 5O₂ → 2V₂O₅

Reactions with Halogens: Vanadium reacts with halogens to form halides, such as vanadium(III) iodide (VI₃): 

2V + 3I₂ → 2VI₃

Reactivity with Water: Vanadium does not react with water at room temperature but can react with steam or hot water to produce vanadium oxides.

Hydrogen Reaction: Vanadium can react with hydrogen gas at high temperatures to form vanadium hydrides.

Complex Formation: Vanadium can form complexes with various ligands, important in catalysis and materials science.

4.0Uses of Vanadium

• Ferrovanadium and Steel Additives: The majority of vanadium produced—about 85%—is added to steel to increase its strength significantly.
• Aerospace Applications: Vanadium is combined with aluminium to create titanium alloys for high-speed airframes and jet engines because of its strength and resilience to heat. 
• Steel Alloys: Vanadium steel alloys are used to make axles, crankshafts, gears, and other crucial automotive and industrial components.
• Nuclear Reactors: Vanadium alloys are used in nuclear reactors because they have low neutron absorption and resist deformation under high temperatures.
• Catalysis: Vanadium pentoxide (V₂O₅) is a critical catalyst in producing sulfuric acid and maleic anhydride.
• Glass and Ceramics
• Infrared Radiation Blocking: Glass coated with vanadium dioxide (VO₂) can block infrared radiation at specific temperatures, providing energy-efficient applications in building materials.