A Short Note on What Is Dioxygen

In the modern periodic table, oxygen is part of the chalcogen group, a group of highly reactive non-metals. Oxygen is also an oxidising agent that can quickly form oxides with other compounds. The classification of oxides into groups is based on the acid-base properties of the compounds. These are neutral, amphoteric, and basic or acidic. Besides helium and hydrogen, oxygen has been the most common element on Earth. Diatomic oxygen makes up 20.95 percent of the Earth’s atmosphere.

What is Dioxygen?

The lightest members of group 16 have the maximum inclination for bond formation. Thus, elemental Oxygen occurs naturally as a diatomic gas with a net double bond: O=O. Dioxygen refers to the usual allotrope of oxygen, which has two oxygen atoms in the molecule.

With the chemical formula O2, dioxygen is one of the most prevalent allotropes of elemental oxygen. Although it is often referred to as oxygen, other names, such as molecular oxygen or oxygen gas, help differentiate this from elemental oxygen.

The Physical Characteristics of Dioxygen

• It is an odourless, tasteless, and colourless gas.
• Its density is 1.4289 g/L, making it more dense than the air.
• It has negligible solubility in water. This small amount of dissolved oxygen is sufficient to maintain marine and aquatic life.
• Oxygen has melting and boiling points of approximately 54.36 degrees Kelvin and 90.188 degrees Kelvin, respectively.
• All three states of oxygen can exist simultaneously, based on the changes in temperature and pressure.

The Chemical Characteristics of Dioxygen

Oxygen is a highly reactive element that reacts with virtually all metals and non-metals. However, some metals, including gold and platinum, and noble gases, like helium, argon, and neon, do not react.

• It interacts directly with nearly all metals and non-metals to generate their oxides.

Example: 

Si + O2 → SiO2

S + O2 → SiO2

• It is paramagnetic.
• Usually, oxygen is inert when it comes into contact with acids or bases.
• Since oxygen is an excellent oxidant, it assists in combustion.
• Rust is formed on iron when oxygen and moisture combine.
• Hydrogen peroxide in the presence of finely divided metals and manganese dioxide decomposes to give water and dioxygen.

2H2O2 →  2H2O + O2

Oxygen Preparation in the Laboratory

Laboratory Preparation of Oxygen can be done by various methods:

Catalytic breakdown of solid potassium chlorate is the most popular and convenient method for producing dioxygen in the laboratory. This process is catalysed by manganese dioxide.

2KClO3 → 2KCl + 3O2

Another laboratory procedure is the thermal breakdown of metal oxides from the lower electrochemical series. For example, the decomposition of silver or mercury oxides produces dioxygen.

2HgO (s) → 2Hg (l) + O2 (g)

2PbO2 (s) → 2PbO (s) + O2 (g)

Lead, barium, and manganese’s higher oxides can also be heated in the laboratory to produce dioxygen.

2PbO2→ 2PbO + O2

2MnO2 + 2H2SO4 → 2MnSO4 + 2H2O + O2 

2BaO2 → 2BaO + O2

Thermal decomposition of oxygen-rich salts like permanganates and nitrates generate oxygen. It can also be broken down with heat and form oxygen.

2KNO3 → 2KNO2+ O2

2KMnO4 → K2MnO4 + MnO2 + O2

2NaNO3 → 2NaNO2 + O2

Dioxygen’s Reaction with Metals:

Majority of metals are fueled by dioxygen and frame oxides, which are, for the most part, common in nature.

2M + O2 →    2MO

Δ

4M + O2 →    2M2O

Δ

4M + 3O2 →    2M2O3

Δ

A high proportion of non-metals combusting in the presence of acidic oxides are formed by dioxygen complexes. For instance, sulphur ignites in atmospheric oxygen, producing sulphur dioxide.

Δ

S + O2 →   SO2

Dioxygen Reaction with Several Compounds:

Sulphur dioxide is catalytically oxidised to form sulphur trioxide in presence of vanadium pentoxide. These are crucial steps in sulphuric acid synthesis via the contact method.

V2O5

2SO2 + O2 → 2SO3

At high temperatures or upon combustion, dioxygen interacts with various organic molecules, including carbohydrates and hydrocarbons, forming carbon dioxide and water.

High temperature

CH4 + 2O2 → CO2 + 2H2O

Uses of Dioxygen:

Dioxygen is crucial in several important processes. Respiration and combustion are two examples of dioxygen uses. Other applications are listed below.

• Respiration is dependent on the availability of dioxygen.
• It can be found in hospital oxygen cylinders and mountaineering equipment.
• Artificial respiration uses dioxygen and then either carbon dioxide or helium.
• It is used in the production of many different metals.
• If you want to weld or cut metal, you can use this.
• It is used to oxidise ammonia while preparing nitric acid.
• Laser cutting necessitates oxygen utilisation.
• Oxygen is essential in wastewater treatment and sewage treatment.
• Oxygen barrels are widely used in medical facilities, high-altitude flights, and mountaineering.
• Liquid oxygen is necessary as a component of the rocket fuel.

Conclusion

In nature, elemental oxygen exists like a diatomic gas with a net double-fold bonding: O=O. Dioxygen is the common allotrope of oxygen that contains two oxygen atoms. Except for noble gases, oxygen reacts with practically every element. Oxides are the resultant compounds. O2 gas is inflammable, but it is essential for combustion. Additionally, it is a life-sustaining gas. Mammals, like humans, depend on it for survival, and it also helps them burn calories.