A Quick Note on Dioxygen Definition

Oxygen is a vital part of the existence of life. It is a highly reactive non-metal that is a member of the chalcogen group on the modern periodic table, which means that it is very reactive. Because oxygen is a diatomic molecule, it can be formed when two atoms of the elements unite to produce the compound dioxygen. It is the third most plentiful element in the universe, after hydrogen and helium. It is estimated that this gas constitutes approximately 21 percent of the earth’s atmosphere in its free condition. Oxygen has the chemical formula O2 (oxygen dioxide). It is the element that is found in the greatest quantity in the earth’s crust.

With the exception of noble gases, oxygen gas reacts with practically all elements. The resulting product is referred to as oxides. Even though it is not combustible on its own, oxygen gas is needed for combustion. It is also a life-giving gas because mammals require oxygen to survive and it helps in the release of energy.

Dioxygen’s Physical Properties

• It is denser than air, weighing 1.429 g/L.
• It is mildly soluble in water, barely enough for aquatic life to survive.
• Oxygen has a melting point of around 54.36 degrees Kelvin and a boiling point of roughly 90.188 degrees Kelvin.
• Oxygen can exist in any of the three states: solid, liquid, or gas, depending on the temperature and pressure.

Dioxygen’s Chemical Properties

• It interacts directly with nearly all metals and nonmetals to generate their oxides

4Na + O2 → 2Na2O (with metal)

C + O2 → CO2 (with non-metal)

• It is paramagnetic.
• Normally, oxygen is inert when it comes into contact with acids and bases

Fuel + O2 → CO2 + H2O

Ex- CH4 + O2 → CO2 + H2O

• Due to the fact that oxygen is an excellent oxidant, it aids in combustion
• Rust is formed on iron when oxygen and moisture combine

Fe + O2 + H2O → Fe2O3n.H2O (hydrated iron oxide)

Laboratory Dioxygen Synthesis

Dioxygen can be synthesised in a variety of ways in the laboratory.

• Dioxygen is created during the thermal decomposition of metal oxides having a relatively low electrode potential, such as Mercury and Silver Oxides

2HgO (s) → 2Hg(l) + O2(g)

2PbO2(s) → 2PbO(s) + O2(g)

• Because the breakdown of hydrogen peroxide also creates oxygen, manganese (IV) oxide is utilized as a catalyst to accelerate the reaction

2H2O2(aq) → 2H2O(l) + O2(g)

When oxygen-rich salts such as nitrates and permanganates are thermally decomposed, Dioxygen is formed.

2KNO3 → 2KNO2 + O2

2KMnO4 → K2MnO4 + MnO2 + O2

2NaNO3 → 2NaNO2 + O2

Industrial Oxygen Production

There are two basic industrial methods for producing O2 from air.

• Fractional distillation of liquified air results in the distillation of N2 as a vapour and the retention of O2 as a liquid. Liquid air is a combination of liquid Nitrogen and liquid Oxygen in this case. Nitrogen is more flammable than oxygen due to its lower boiling point. It first boils away, leaving only pure oxygen remaining.
• Another method involves passing clean, dry air over one bed of zeolite molecular sieves, which absorbs the N2 gas and produces a gas that is 90% to 93% oxygen.

Dioxygen’s Applications

Oxygen is employed in a wide variety of applications. Oxygen is used in the following different ways: 

• It is a component of oxygen cylinders used in hospitals and mountaineering.

• In the form of oxy-acetylene, it is used for welding and cutting metals.
• When oxygen gas is combined with acetylene gas, an oxy-acetylene flame is created. This flame is utilised for the process of cutting and welding metals.
• It is utilised in liquid rocket fuel.
• It is used to make nitric acid.
• It is used in conjunction with carbon dioxide or methane to provide artificial respiration.
• Laser cutting requires the usage of oxygen.
• Combustion reactions require oxygen. Because materials that do not burn readily in air do so readily in oxygen, combining oxygen with air speeds up the combustion process.
• Oxygen is utilised in water treatment operations, such as wastewater purification and sewage treatment.

CONCLUSION- 

Oxygen is a gaseous chemical element with the symbol O and atomic number 8, accounting for 21% of air and 46% of the Earth’s crust, making it the most plentiful element. Dioxygen is a  tasteless gas that occurs naturally in the form of the diatomic molecule O2. Dioxygen is magnetic in its native condition. This form of oxygen is utilised in medicine, breathing, metal cutting and welding, as an oxidant in water treatment, and as rocket fuel, among other purposes.