What Is Ammonium Nitrite?
Ammonium nitrite is a type of nitrite, a colorless crystal.
It is a highly unstable and reactive compound used in the manufacture of various organic compounds, fertilizers, and explosives. It is highly explosive and decomposes to produce nitrous oxide, water, and nitrogen gas.
It is obtained by reacting nitrogen oxide with ammonia or ammonium carbonate. It is tidally soluble and highly unstable, which means that it decomposes into water and nitrogen even at room temperature.
Ammonium nitrite is obtained by reacting nitrogen oxide with ammonia or ammonium carbonate at low temperature and high pressure.
Uses of Ammonium Nitrite
Ammonium nitrite (NH4NO2) has limited applications due to its instability and is mainly restricted to laboratory use. The primary use of Ammonium Nitrite is as a reagent for the production of nitrogen gas.
It is also used as a source of nitrogen in the manufacture of fertilizers and explosives such as dynamite. However, due to its highly unstable nature, it is not often used in the commercial manufacture of explosives. Additionally, ammonium nitrite has been used as a component of rocket fuel and as an experimental reagent in the synthesis of other compounds.
In addition, ammonium nitrite is often used as a fertilizer, an ingredient in explosives, a raw material for nitrates, and as a coolant. The most familiar example is as a coolant. Like ammonium nitrite, it is mixed with water to create an endothermic reaction that produces a cooling effect.
When used as a fertilizer, the nitrogen separated from ammonium nitrite may be oxidized by microorganisms in the soil and transformed into nitrate-nitrogen, so care must be taken in its use.
Properties of Ammonium Nitrite
Ammonium nitrite is very soluble in water and is hygroscopic. When in contact with metal surfaces, it can form corrosive solutions.
Ammonium nitrite is also a white or slightly yellow crystalline solid. It is a highly unstable and reactive compound that gradually decomposes to water and nitrogen at room temperature.
Other properties include explosive decomposition upon heating, shock, or friction. This is because ammonium nitrite is a strong oxidizer and can readily donate oxygen to other compounds.
Ammonium nitrite solutions are stable at high pH and low temperatures and can explode if the pH drops below 7.0. To maintain a safe pH, ammonia water is commonly added.
Structure of Ammonium Nitrite
Ammonium nitrite is represented by the chemical formula NH4NO2 and has a structure consisting of an ammonium ion (NH4+) ion bonded to an ammonium nitrite ion (NO2-). The molecule has a tetrahedral structure with a nitrogen atom and four hydrogen atoms symmetrically arranged.
The nitrite ion has an asymmetric structure with double bonds in one direction. The molecule is linear and has an N-N-O bond angle of 120°.
Other Information on Ammonium Nitrite
How Ammonium Nitrite Is Produced
Ammonium nitrite is prepared by the absorption of nitrogen dioxide and nitric oxide gases into ammonia water. It can also be obtained by combining barium or lead nitrite with ammonium sulfate, or by reactions using silver nitrite and ammonium chloride, or ammonium perchlorate and potassium nitrite.
When the precipitates produced in these reactions are filtered and the filtrate is concentrated, they form water-soluble, colorless crystals. It can also be synthesized by oxidation of ammonia with ozone or hydrogen peroxide.
Ammonium nitrite produced by these methods must be handled with care because it decomposes easily when exposed to air or moisture to form ammonium nitrate and ammonia.