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प्रश्न
Suggest a list of the substances where carbon can exhibit oxidation states from –4 to +4 and nitrogen from –3 to +5.
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उत्तर
The substances where carbon can exhibit oxidation states from –4 to +4 are listed in the following table.
| Substance | O.N. of carbon |
| CH2Cl2 | 0 |
| ClC≡CCl | +1 |
| HC≡CH | –1 |
| CHCl3, CO | +2 |
| CH3Cl | –2 |
| Cl3C – CCl3 | +3 |
| H3C – CH3 | –3 |
| CCl4, CO2 | +4 |
| CH4 | –4 |
The substances where nitrogen can exhibit oxidation states from –3 to +5 are listed in the following table
| Substance | O.N. of nitrogen |
| N2 | 0 |
| N2O | +1 |
| N2H2 | –1 |
| NO | +2 |
| N2H4 | –2 |
| N2O3 | +3 |
| NH3 | –3 |
| NO2 | +4 |
| N2O5 | +5 |
संबंधित प्रश्न
Justify that the following reaction is redox reaction:
\[\ce{CuO(s) + H2(g) → Cu(s) + H2O(g)}\]
Justify that the following reaction is redox reaction:
\[\ce{Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)}\]
Justify that the following reaction is redox reaction:
\[\ce{4BCl3(g) + 3LiAlH4(s) → 2B2H6(g) + 3LiCl(s) + 3 AlCl3(s)}\]
While sulphur dioxide and hydrogen peroxide can act as oxidising as well as reducing agents in their reactions, ozone and nitric acid act only as oxidants. Why?
Identify the substance oxidised, reduced, oxidising agent and reducing agent for the following reaction:
\[\ce{HCHO(l) + 2[Ag (NH3)2]+(aq) + 3OH–(aq) → 2Ag(s) + HCOO–(aq) + 4NH3(aq) + 2H2O(l)}\]
Consider the reactions:
\[\ce{2S_2O_3^{(2-)}(aq) + l_2(S) -> S_4O_6^{(2-)}(aq) + 2l-(aq)}\]
\[\ce{S_2O_3^{(2-)}(aq) + 2Br_2(l) + 5H_2O(l) -> 2SO_4^{2-} (aq) + 4Br-(aq) + 10H+ (aq)}\]
Why does the same reductant, thiosulphate react differently with iodine and bromine?
Why does the following reaction occur?
\[\ce{XeO^{4-}_6 (aq) + 2F- (aq) + 6H+ (aq) -> XeO3(g) + F_2(g) + 3H_2O(l)}\]
What conclusion about the compound Na4XeO6 (of which `"XeO"_6^(4+)` is a part) can be drawn from the reaction.
What sorts of informations can you draw from the following reaction ?
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Al, Cu, Fe, Mg and Zn.
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\[\ce{2KClO3 -> 2KCl + 3O2}\]
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(ii) Chlorine is undergoing oxidation.
(iii) Oxygen is reduced.
(iv) None of the species are undergoing oxidation or reduction.
Identify the correct statements with reference to the given reaction.
\[\ce{P4 + 3OH- + 3H2O -> PH3 + 3H2PO^{-}2}\]
(i) Phosphorus is undergoing reduction only.
(ii) Phosphorus is undergoing oxidation only.
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(iv) Hydrogen is undergoing neither oxidation nor reduction.
\[\ce{MnO^{2-}4}\] undergoes disproportionation reaction in acidic medium but \[\ce{MnO^{-}4}\] does not. Give reason.
Assertion (A): Redox couple is the combination of oxidised and reduced form of a substance involved in an oxidation or reduction half cell.
Reason (R): In the representation \[\ce{E^Θ_{Fe^{3+}/Fe^{2+}}}\] and \[\ce{E^Θ_{Cu^{2+}/Cu}, Fe^{3+}/Fe^{2+}}\] and \[\ce{Cu^{2+}/Cu}\] are redox couples.
Why does fluorine not show disporportionation reaction?
Which of the following reactions is the metal displacement reaction? Choose the right option.
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