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  • How is the Nitrate Ion (NO3) formed? - Chemistry Stack Exchange
    5 I understand how the nitrite $\ce {NO2}$ ion can be formed and have a negative charge, but the nitrate $\ce {NO3}$ ion is confusing me I made some simple drawings to try to explain what I don't understand: Does the "electron from outside" that the oxygen receives, as indicated in the drawing, comes from the nitrogen atom?
  • Which has the greater N–O bond length, NO₂⁻ or NO₃⁻?
    For the nitrate ion (NO3-), there is one double bond that leads to resonance amongst all three of the nitrogen-oxygen bonds This effectively gives each bond the characteristic of 1 3 bonds, and slightly longer than in the nitrite ion
  • Are all NO3- salts soluble in water? If so, why?
    All the examples of $\\ce{NO3-}$ salts are soluble in water (all that I know about) Is it always so or there is some salt which doesn't dissolve in water? If so what is the reason behind it?
  • Bond length in NO3- - Chemistry Stack Exchange
    I am doing a multiple choice question for which one of the possible answers is, for the Lewis structure of NO3- (one of the oxygens is double bonded to the nitrogen and the other two are single bon
  • inorganic chemistry - Delocalization of π-electrons in nitrate ion . . .
    Benzene and nitrate ion are given in my textbook as examples for the delocalization of π-electrons Benzene, due to symmetry of its resonating structures, is simple enough We assume that σ-electro
  • inorganic chemistry - Why is it wrong to draw the Lewis structure of a . . .
    0 When drawing for example the Lewis structure of nitrate ion (NO3)^-1 whould it be wrong to draw nitrogen and oxygen separately and then try to figure out the structure of the ion? In that case does the nitrogen give one of its electrons to the oxygen? cause a nitrogen atom does have a lone pair of electons but in the nitrate ion they are gone
  • inorganic chemistry - Brown ring from the anion detection of NO3 . . .
    The brown ring formed in the confirmatory test for the nitrate ion is due to the complex called nitroso ferrous sulphate, or pentaaqua nitrosyl iron (II) sulfate with the formula $\ce { [Fe (H2O)5NO]SO4}$ The concentrated sulfuric acid decomposes this complex and brown ring disappers in a few seconds when $\ce {H2SO4}$ moves to the upper layer This is why slow addition of the acid (through
  • Why do we have to prevent the hydrolysis of iron(III) nitrate?
    I want to make particular concentration of ferric ions from $\\ce{Fe(NO3)3 9H2O}$, and then I found this video It says that we have to add nitric acid to prevent iron from hydrolysis, what does it m
  • Ammonia (NH3) vs Ammonia Nitrogen (NH3-N) - Chemistry Stack Exchange
    I've been looking into chloramination (chlorine amp; nitrogen reactions) and noticed many papers either reference Ammonia (NH3) or Ammonia-Nitrogen (NH3-N), seemingly interchangeably Is the hyphe
  • Why is nitric acid such a strong oxidizing agent?
    ManishEarth did a good job explaining already Perhaps I could point out one more you could think of to understand why nitric acid has such a high reduction potential The nitrogen centre in nitric acid is in +5 oxidation state, which is also the highest known oxidation state of nitrogen As a result, the acid exists in high energy state to begin with as it is really unstable





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