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In the NO − 3 anion, the oxidation state of the central nitrogen atom is V (+5). This corresponds to the highest possible oxidation number of nitrogen. Nitrate is a potentially powerful oxidizer as evidenced by its explosive behaviour at high temperature when it is detonated in ammonium nitrate (NH 4 NO 3), or black powder, ignited by the shock wave of a primary explosive.
H 2 N 2 O 2 + 2 H + + 2 e − ⇌ N 2 + 2 H 2 O; E 0 = +2.65 V. Oxidation reactions usually result in the formation of the nitrate ion, with nitrogen in oxidation state +5. For example, oxidation with permanganate ion can be used for quantitative analysis of nitrite (by titration): 5 NO − 2 + 2 MnO − 4 + 6 H + → 5 NO − 3 + 2 Mn 2+ + 3 H 2 O
Due to relatively weak N–O bonding, all nitrogen oxides are unstable with respect to N 2 and O 2, which is the principle behind the catalytic converter, and prevents the oxygen and nitrogen in the atmosphere from combusting.
Nitrogen cycle. Denitrification is a microbially facilitated process where nitrate (NO 3 −) is reduced and ultimately produces molecular nitrogen (N 2) through a series of intermediate gaseous nitrogen oxide products.
Nitrogen trioxide or nitrate radical is an oxide of nitrogen with formula NO 3, consisting of three oxygen atoms covalently bound to a nitrogen atom. This highly unstable blue compound has not been isolated in pure form, but can be generated and observed as a short-lived component of gas, liquid, or solid systems.
[12] [13] Complete nitrification, the conversion of ammonia to nitrate in a single step known as comammox, has an energy yield (∆G°′) of −349 kJ mol −1 NH 3, while the energy yields for the ammonia-oxidation and nitrite-oxidation steps of the observed two-step reaction are −275 kJ mol −1 NH 3, and −74 kJ mol −1 NO 2 − ...
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A nitrate nitrite, or nitrite nitrate, is a coordination complex or other chemical compound that contains both nitrite (NO − 2) and nitrate (NO − 3) anions.They are mixed-anion compounds, and they are mixed-valence compounds.