National education day: e-learning transforming educational landscape. Understanding the importance of education with e-learning transforming. JEE Main may commence the registration in the first week of Dec tentatively. CBSE has released the term-1 admit card Share This Video.
Apne doubts clear karein ab Whatsapp par bhi. Try it now. Ab clear karein apne doubts Whatsapp par bhi. Apna phone number register karein. Ab aap Whatsapp pe solutions paa saktey h, hum aapko message karenge. Ab aap Whatsapp pe solutions paa saktey h, hum aapko ping karenge. Study Materials. Why use Doubtnut? Instant Video Solutions. Request OTP. Much of the chemistry of nitrogen involves oxidation-reduction reactions.
Some active metals such as alkali metals and alkaline earth metals can reduce nitrogen to form metal nitrides. In the remainder of this section, we will examine nitrogen-oxygen chemistry. When ammonium nitrate is carefully heated, nitrous oxide dinitrogen oxide and water vapor form.
Stronger heating generates nitrogen gas, oxygen gas, and water vapor. No one should ever attempt this reaction—it can be very explosive. In , there was a major ammonium nitrate explosion in Texas City, Texas, and, in , there was another major explosion in West, Texas.
In the last years, there were nearly 30 similar disasters worldwide, resulting in the loss of numerous lives. In this oxidation-reduction reaction, the nitrogen in the nitrate ion oxidizes the nitrogen in the ammonium ion.
Low yields of nitric oxide, NO, form when heating nitrogen and oxygen together. NO also forms when lightning passes through air during thunderstorms. Burning ammonia is the commercial method of preparing nitric oxide. In the laboratory, the reduction of nitric acid is the best method for preparing nitric oxide. When copper reacts with dilute nitric acid, nitric oxide is the principal reduction product:. Gaseous nitric oxide is the most thermally stable of the nitrogen oxides and is the simplest known thermally stable molecule with an unpaired electron.
It is one of the air pollutants generated by internal combustion engines, resulting from the reaction of atmospheric nitrogen and oxygen during the combustion process. At room temperature, nitric oxide is a colorless gas consisting of diatomic molecules. As is often the case with molecules that contain an unpaired electron, two molecules combine to form a dimer by pairing their unpaired electrons to form a bond.
Most substances with unpaired electrons exhibit color by absorbing visible light; however, NO is colorless because the absorption of light is not in the visible region of the spectrum. Dinitrogen trioxide exists only in the liquid and solid states. When heated, it reverts to a mixture of NO and NO 2. Commercially, it is possible to prepare nitrogen dioxide by oxidizing nitric oxide with air. It is also responsible for the dimerization of NO 2. At low pressures or at high temperatures, nitrogen dioxide has a deep brown color that is due to the presence of the NO 2 molecule.
At low temperatures, the color almost entirely disappears as dinitrogen tetraoxide, N 2 O 4 , forms. At room temperature, an equilibrium exists:. It is unstable above room temperature, decomposing to N 2 O 4 and O 2. The nitrogen oxides exhibit extensive oxidation-reduction behavior. Nitrous oxide resembles oxygen in its behavior when heated with combustible substances.
N 2 O is a strong oxidizing agent that decomposes when heated to form nitrogen and oxygen. Because one-third of the gas liberated is oxygen, nitrous oxide supports combustion better than air one-fifth oxygen. A glowing splinter bursts into flame when thrust into a bottle of this gas. Nitric oxide acts both as an oxidizing agent and as a reducing agent.
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