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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.
Ammonium nitrate is an important fertilizer with NPK rating 34-0-0 (34% nitrogen). [17] It is less concentrated than urea (46-0-0), giving ammonium nitrate a slight transportation disadvantage. Ammonium nitrate's advantage over urea is that it is more stable and does not rapidly lose nitrogen to the atmosphere.
[1]: 217 Here the nitrogen oxidation numbers change from (+4 and +4) to (+3 and +5). + + [1]: 224 These solvents all possess atoms with odd atomic numbers, either nitrogen or a halogen.
The oxidation states are also maintained in articles of the elements (of course), and systematically in the table {{Infobox element/symbol-to-oxidation-state}} See also [ edit ]
2 at higher temperatures. Nitrogen forms nine molecular oxides, some of which were the first gases to be identified: N 2 O (nitrous oxide), NO (nitric oxide), N 2 O 3 (dinitrogen trioxide), NO 2 (nitrogen dioxide), N 2 O 4 (dinitrogen tetroxide), N 2 O 5 (dinitrogen pentoxide), N 4 O (nitrosyl azide), [15] and N(NO 2) 3 (trinitramide). [16]
NO y (or NOy) refers to the sum of NO x and all oxidized atmospheric odd-nitrogen species (e.g. the sum of NO x, HNO 3, HNO 2, etc.) NO z (or NO z ) = NO y − NO x Mixed Oxides of Nitrogen ("MON"): solutions of nitric oxide in dinitrogen tetroxide/nitrogen dioxide.
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5, the oxidation state of C is −1 + − 1 / 5 = − 6 / 5 . The −1 occurs because each carbon is bonded to one hydrogen atom (a less electronegative element), and the − 1 / 5 because the total ionic charge of −1 is divided among five equivalent carbons.