A Quick Note on Oxides of Nitrogen

NOx gases are formed by the interaction between nitrogen and oxygen during the burning of fuels, such as hydrocarbons, in air, especially at high temperatures, such as those found in automobile engines. The nitrogen oxides released in high-traffic regions, such as large cities, can be a substantial cause of air pollution. Lightning can also produce NOx gases naturally.

Oxides of Nitrogen 

Nitrogen reacts with oxygen to form a number of Nitrogen oxides. Two of the most toxicologically relevant chemicals are nitric oxide (NO) and nitrogen dioxide (NO2). Nitrogen monoxide (or N2O) and nitrogen pentoxide are two more gases in this category (NO5). Nitrogen reacts with oxygen to produce a multitude of nitrogen oxides.

It has a wide range of oxidation states in its oxide forms, ranging from +1 to +5. Oxides of nitrogen having nitrogen in the higher oxidation state are acidic compared to those with a lower level of oxidation. Nitrogen dioxide is created during the nitric acid manufacturing process. The majority of nitric acid is used in the production of fertilisers, although it is also utilised in the production of explosives for military and mining purposes. Let us delve more into the topic of nitrogen oxides.

Lists of Oxides of Nitrogen 

Let us look at the oxides of Nitrogen are enlisted –

1. Dinitrogen oxide

Dinitrogen oxide is a gaseous chemical that is colourless and non-flammable. It is a neutral substance. Laughing gas is the most common name for it. The breakdown of ammonium nitrate at high temperatures produces dinitrogen oxide.

                   NH4NO3 → 2H2O + N2O

1. Dinitrogen trioxide 

Dinitrogen trioxide is an acidic, deep blue solid. Only at low temperatures, i.e. in liquid and solid phases, may it be insoluble. As the temperature rises, the equilibrium causes the constituent gases to form. Dinitrogen trioxide is made by mixing equal volumes of nitric oxide and nitrogen dioxide and cooling the mixture to below 21 degrees Celsius.  

NO + NO2 → N2O3

1. Nitrogen Monoxide

Nitrogen monoxide is a colourless gas with a strong odour. It belongs to a class of diatomic compounds with a valence electron in its bond structure. By reducing dilute nitric acid with copper, nitrogen monoxide is produced. 

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

1. Nitrogen Dioxide 

Nitrogen dioxide is a harmful reddish-brown gas with a distinctive odour that contributes significantly to global air pollution. It has a +4 nitrogen oxidation state and is acidic in nature. The heat breakdown of metal nitrate produces nitrogen dioxide.  

2Pb(NO3)2 →  4NO2 + 2PbO  + O2

1. Dinitrogen Tetroxide 

Dinitrogen tetroxide is a colourless substance that reacts with nitrogen dioxide to produce nitrogen dioxide. It’s a powerful oxidizer that’s also employed as a solvent in the manufacture of a variety of chemicals. 

N2O4 ⇌ 2NO2

1. Dinitrogen Pentoxide

The solid form of dinitrogen pentoxide is colourless. Sublimation occurs at a temperature slightly higher than room temperature. It’s an unpredictable and potentially deadly oxidizer. It’s been utilised for nitration as a diluted solvent in chloroform. When nitric acid (HNO3) is dehydrated with phosphorus (V) oxide, dinitrogen pentoxide is formed.

P4O10 + 12HNO3 → 4H3PO4 + 6N2O5

Conclusion 

This is the complete list of nitrogen oxides and their formulae. Concentrate on the formulas and chemical properties of all of these nitrogen oxides to distinguish them. Nitrogen reacts with oxygen to form a number of Nitrogen oxides. Two of the most toxicologically relevant chemicals are nitric oxide (NO) and nitrogen dioxide (NO2). Nitrogen monoxide (or N2O) and nitrogen pentoxide are two more gases in this category (NO5). Nitrogen reacts with oxygen to produce a multitude of nitrogen oxides. Oxides of nitrogen having nitrogen in the higher oxidation state are acidic compared to those with a lower level of oxidation.