Different Oxides of Nitrogen with Formula

Nitrogen forms various oxides with unique properties and formulas. Explore the different oxides of nitrogen, including their chemical structures and uses.

Nitrogen Definition

Nitrogen is the seventh element in the periodic table, following carbon and oxygen. It is an essential component of amino acids. 

• Nitrogen gas accounts for approximately 80% of the Earth’s atmosphere. It is a colourless, primarily diatomic nonmetal gas that is odourless and colourless in nature.
• Most of its compounds are trivalent because it contains five electrons in their outer shell. It is found in all living tissues. It is a necessary component of life since it is a component of DNA and a part of a genetic code. It can be found in soil and water as nitrates and nitrites.
• All of these chemicals are linked and part of the nitrogen cycle.
• Industrial enterprises generate a lot of nitrogen, which increases the nitrite and nitrate levels in the ground and water as a result of nitrogen cycle processes.
• Important chemicals found in nitric acid salts include potassium nitrate, ammonium nitrate, and nitric acid. Nitro glycerine and other nitrated organic compounds are frequently used as explosives.
• Liquid nitrogen is used as a refrigerant in food transportation and freezing. Liquid nitrogen is also used in the preservation of bodies and reproductive cells, as well as the stable storage of biological materials.
• Nitrogen reacts with oxygen under various conditions to generate a multitude of binary oxides that differ depending on the oxidation state of the nitrogen atom. They vary from N2O (N =+1 oxidation state) through NO (+2), N2O3 (+3), N2O4 (+4), and N2O5 (+5). The propensity of oxides to generate pπ- pπ multiple bonds determines their structures.

Nitrous Oxide (N2O)

• Ammonium nitrate is heated to make nitrous oxide.

NH₄NO₃→N₂O+2H₂O

• It is a colourless, unreactive gas with a pleasant odour. It is also known as laughing gas because, when inhaled in little amounts, it generates uncontrollable laughter.
• It’s a neutral oxide that combines with sodamide to generate sodium azide.

N₂O+2NaNH₂→NAN₃+NH₃+NaOHer

• It functions as an anaesthetic in short doses for minor surgeries.
• At 873K, it decomposes into nitrogen and oxygen. As a result, it aids combustion by functioning as an oxygen source.

2N₂O→2N₂ + O₂

Also Check: Nitrogen Dioxide Formula

Nitric Oxide (NO)

• It is produced by the catalytic oxidation of ammonia in the presence of platinum at 1100 K.

4NH₃ + 5O₂ → 4NO + 6H₂O

• It can also be made by reacting nitric acid with copper as follows:

3Cu(NO₃)₂ + 2NO + 4H₂O →3Cu(NO₃)₂ + 2NO + 4H₂O

• It can also be synthesized by reducing sodium nitrite with ferrous sulfate in the presence of sulfuric acid.

Fe₂(SO4)₃ + 2NaHSO₄ + 2H₂O + 2NO → 2NaNO₂ + 2FeSO₄ + 3H₂SO₄

• It is an oxide that is neutral.
• It is an odourless, colourless gas. Because it possesses an odd number of electrons (11 valence electrons), it is paramagnetic in the gaseous form. However, in the liquid and solid stages, it forms a loose dimer that cancels the magnetic effects of two unpaired electrons. It has diamagnetic properties.
• Nitric oxide quickly combines with oxygen to produce brown nitrogen dioxide emissions.

2NO (g) + O₂ (g) →2NO₂ (g)

Dinitrogen Trioxide (N₂O3)

• It is made by chilling equimolar amounts of nitric oxide and nitrogen dioxide to temperatures below 253 K.

NO(g) + NO₂ (g) → N₂O₃ 

• It may also be made by reacting nitric oxide and dinitrogen tetraoxide at 250 degrees Celsius.

2NO + N₂O₄ →2N₂O₃

Dinitrogen Trioxide Properties

• It is a blue solid with acidic chemistry. It is nitrous acid anhydride (HNO2).

N₂O₃ + H₂O →2HNO₂

• It only exists in its pure form as a solid at extremely low temperatures. It dissociates into NO and NO2 above its melting point (273 K). NO + NO₂ →N₂O₃ 

_{Nitrogen Dioxide (NO2)}

• It is made by heating dried lead nitrate in a stainless steel reaction tank.

2Pb(NO₃)₂→2PbO+4NO₂+O₂

• It is also an odd electron molecule that occurs in gas phase equilibrium with N 2O4 as:

N₂O₄⇔2NO₂

• Above 415 K, it is mostly NO, while below 250 K, it is mostly N2O4.

2NO₂⇔N₂O₄

Dinitrogen Pentaoxide (N2O5)

It is made by combining strong nitric acid with phosphorus pentoxide and dehydrating it.

2N₂O₅+ HPO₃ →4HNO₃ + P₄O₁₀.

Below 273K, N₂O₅ occurs as a colourless solid. The colour changes to yellow as the temperature rises due to the partial breakdown of colourless N2O5 to brown NO2.

2 N₂O₅ →4NO₂ + O₂

At 303 K, the crystals melt, releasing a yellow liquid that decomposes at 313 K to produce NO2.

N₂O₅ is a powerful oxidizing agent that oxidizes iodine to I₂O₅.

The elements NO and NO2 are utilized in the production of nitric acid and nitrate fertilizers. Liquid N2O4 is also utilized as an oxidizer in rocket fuels used in missiles and space vehicles. Because of its toxic nature, NO produces pollution in the atmosphere. Its vapours are discharged into the atmosphere when oil and coal are burned.