Nitrogen oxides are a mixture of nitrogen and oxygen-composed gases. Nitric oxide (NO) and nitrogen dioxide (NO2) are two of the most significant toxicologically important compounds. Other gases in this group are nitrogen monoxide (or N2O), and nitrogen pentoxide (NO5). A number of nitrogen oxides are formed by nitrogen reacting with oxygen.
It exhibits various oxidation states, ranging from +1 to +5 in its oxide forms. Nitrogen oxides having nitrogen in the higher state of oxidation are more acidic than those in the lower state of oxidation. Nitrogen dioxide is produced for the manufacturing process of nitric acid. Most nitric acid is used in fertiliser manufacturing, while some are used in explosives manufacturing for both military and mining uses. Let us find out more about the oxides of nitrogen in detail.
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Names of Oxides of Nitrogen
Let us now look at nitrogen oxide formula and about the different types of names of oxides of nitrogen: -
Dinitrogen oxide is a colourless, non-flammable gaseous compound. It has neutral properties. It's usually referred to as laughing gas. Dinitrogen oxide is formulated by the decomposition of ammonium nitrate at high temperatures.
NH4NO3 → 2H2O + N2O
Dinitrogen trioxide is a deep blue, acidic solid. It can only be insoluble at low temperatures, i.e. in liquid and solid phases. As temperature rises, the equilibrium leads to the formation of the constituent gases. Dinitrogen trioxide is prepared by mixing equal parts of nitric oxide and nitrogen dioxide and by further cooling the mixture below −21 ° C.
NO + NO2 → N2O3
Nitrogen monoxide is a colourless gas. Its bond structure includes a valence electron, and it belongs to a class of diatomic molecules. Nitrogen monoxide is prepared by reducing the dilute nitric acid with copper.
3H2SO4 + 2NaNO2 + 2FeSO4 → 2NaHSO4 + Fe2(SO4)3 + 2H2O + 2NO
Nitrogen dioxide is a reddish-brown poisonous gas with a pungent smell and contributes greatly to air pollution all around the world. It is acidic in nature with a +4 nitrogen oxidation state. Nitrogen dioxide is formulated by the thermal decomposition of metal nitrate.
2Pb(NO3)2 → 4NO2 + 2PbO + O2
Dinitrogen tetroxide is a colourless solid that is in equilibrium with nitrogen dioxide. It is an efficient oxidising agent which is used as a solvent for the production of many chemical substances.
N2O4 ⇌ 2NO2
Dinitrogen pentoxide is a colourless solid. It undergoes sublimation marginally above room temperature. It is an erratic and potentially dangerous oxidising agent. It has been used as a solvent diluted in chloroform for nitration. Dinitrogen pentoxide is produced by the process of dehydration of nitric acid (HNO3) with phosphorus (V) oxide.
Solved Questions on Nitrogen Oxide
1. What are the Industry and Natural Sources for the Emission of Oxides of Nitrogen?
The industry sources of nitrogen include oil and gas extraction, the supply of electricity, mining, manufacturing industries and petroleum manufacturing.
The natural sources for the emission of nitrogen include: Biological nitrogen recycling involves processes that produce nitric oxide and nitrous oxide as intermediates. Thermal processes in the atmosphere which take place during lightning or wildfires also produce nitrogen oxides.
2. What are the Ways to Reduce Nitrogen Oxide Emissions to Treat the Pollution of Air?
The ways to reduce the emission of nitrogen oxide are:
Using a limited quantity of nitrogen fertilisers
Using catalytic converters in cars to reduce emissions
It can be done in two ways:
Reduction: Removal of oxygen from the nitrogen oxide
Oxidation: Adding oxygen to carbon monoxide to form carbon dioxide, which is less harmful than carbon monoxide.
3. What are some Applications of Nitrous Oxide?
Some applications of Nitrous Oxides are:
Used for sedation in dentistry
Used as analgesic to control pain
It is extremely safe does not react with body fluids
Rapid and onset recovery
This is the explanation of all the oxides of nitrogen and their formulas. Focus on the formula and chemical properties of all these nitrogen oxides and understand their differences. Learn these oxides separately to understand their features properly.