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  • How is the Nitrate Ion (NO3) formed? - Chemistry Stack Exchange
    Does the "electron from outside" that the oxygen receives, as indicated in the drawing, comes from the nitrogen atom? If so, then the N atom would be left with only 4 valence electrons instead of 5, thus being able to form another covalent bond with the extra oxygen, forming $\ce{NO3}$ Is this the correct line of thinking?
  • Are all NO3- salts soluble in water? If so, why?
    $\begingroup$ $\ce{BiO(NO3)}$ could probably be added to the list … to quote a fellow student in the ion lottery practical course 'Found nitrate, didn’t dissolve; only one insoluble nitrate ' (Note: He meant that we wouldn’t have gotten any others ) $\endgroup$
  • Covalent bond in NO3 - Chemistry Stack Exchange
    $\begingroup$ Please, clarify: are you talking about $\ce{NO3-}$ anion or $\ce{NO3}$ neutral radical $\endgroup$ – permeakra Commented Feb 7, 2018 at 12:22
  • Which has the greater N–O bond length, NO₂⁻ or NO₃⁻?
    There are two ways to think of it First: draw out the (major) contributing Lewis structures for both ions Each iin has one pi bond, but it's shared between two linkages in $\ce{NO2^-}$ ion versus three linkages in the $\ce{NO3^-}$ ion So the $\ce{NO3^-}$ ion has less pi bonding in each linkage making those bonds weaker overall
  • What is the oxidation state of nitrogen in nitrate ion and what is its . . .
    The $\ce{NO3-}$ ion cannot be depicted using a single Lewis structure However, its resonance structures are shown below: What this means is that the actual structure of the nitrate ion is somewhere in between the three structures shown below
  • Why do we have to prevent the hydrolysis of iron(III) nitrate?
    Increase the concentration of $\ce{NO3^-}$ in the solution to prevent formation of aqua complexes in accordance with Le Chatelier's Principle, as explained in the section Hydration Isomerism of $\ce{Fe(NO3)3}$ below
  • equilibrium - Which one is nitric Acid, HNO3 by itself, or when it is . . .
    The resulting $\ce{H3O+}$, called hydronium, is the conjugate acid, while the $\ce{NO3-}$, called nitrate, is the conjugate base (this is the molecule of nitric acid, but stripped of its $\ce{H+}$) You could view this as a dilution, in the sense that the resulting solution is less acidic than highly concentrated nitric acid would be, but the
  • Products of electrolysis of Ni (NO3)2 - Chemistry Stack Exchange
    Looking at related metal electrolysis, for example, Cu(NO3)2, per this source with again graphite electrodes: Electrolysis of a copper(II) nitrate solution produces oxygen at the anode and copper at the cathode Lastly, with the transition metal manganese, a source on the electrolysis of Mn(NO3)2, reports, to quote:
  • Reaction of copper with nitric acid - Chemistry Stack Exchange
    $$\ce{Cu + 4HNO3 -> Cu(NO3)2 + 2NO2 + 2H2O}$$ As we see that with dilute acid oxidation state of nitrogen changes from $+5$ to $+2$ and with concentrated acid it changes from $+5$ to $+4$ but shouldn't it be vice- versa because since concentrated nitric acid is a good oxidizing agent and should show a huge change in oxidation number ?
  • Neutralization reaction between ammonia and nitric acid
    $$\ce{NH4+(aq) + NO3-(aq) ->NH4NO3(aq)}$$ The result of #2 would be reasonable if you had not been told that the reaction was occurring in aqueous solution In aqueous solution, the products should have been those of #1, since ammonium nitrate is freely soluble in water





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