What is Nitrogen dioxide?
NO2 is a highly poisonous gas with chemical name Nitrogen dioxide.
It is also called Nitrogen (IV) oxide or Deutoxide of nitrogen. It is one of the major atmospheric pollutants that absorb UV light and stops to reach it to the earth’s surface.
Nitrogen (IV) oxide is a yellowish-brown liquid in its compressed form or reddish-brown gas. Its vapors are heavier when compared to air.
Nitrogen dioxide Structure – NO2
Properties of Nitrogen dioxide – NO2
|Molecular weight/molar mass of NO2||46.006 g/mol|
|Density of Nitrogen dioxide||1.880 g/dm3|
|Boiling Point of Nitrogen dioxide||21.15 °C|
|Melting Point of Nitrogen dioxide||−9.3 °C|
NO2 Uses (Nitrogen dioxide)
- Nitrogen dioxide is used as an intermediate in the production of nitric acid.
- Used in the manufacturing of oxidized cellulose compounds.
- Used as a catalyst.
- Used as an intermediate in the production of sulfuric acid.
- Used as an oxidizer for rocket fuels.
- Used as a nitrating agent.
- Used to bleach flour.
- Used as an oxidizing agent.
- Used in the making of explosives.
Chemical Properties of Nitrogen dioxide – NO2
1. Thermal properties – Exists in equilibrium dinitrogen tetroxide gas:
2 NO2 ⇌ N2O4
2. As an oxidizer – Due to the weakness of the N–O bond, NO2 is a strong oxidizer.
3. Hydrolysis reaction – Hydrolysis reaction produces nitrous acid and nitric acid.
2 NO2 (N2O4) + H2O → HNO2 + HNO3
5. It is a negligibly slow reaction at low concentrations of nitrogen dioxide.
6. Formation of nitrites – corresponding nitrites are formed by alkyl and metal iodides.
2 CH3I + 2 NO2 → 2 CH3NO2 + I2
TiI4 + 4 NO2 → Ti(NO2)4 + 2 I2
Severe exposures of Deutoxide of nitrogen can be fatal. When in contact it causes burning sensation to eyes and skin. When in liquid form it causes frostbite. It is reported to react with the blood to form methemoglobin. When heated to decompose, it releases toxic fumes of nitrogen oxides.
Learn more about the Structure, physical and chemical properties of NO2 from the experts at BYJU’S.