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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
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Identify the substance oxidised, reduced, oxidising agent and reducing agent for the following reaction:
\[\ce{HCHO(l) + 2[Ag (NH3)2]+(aq) + 3OH–(aq) → 2Ag(s) + HCOO–(aq) + 4NH3(aq) + 2H2O(l)}\]
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\[\ce{HCHO (l) + 2Cu^{2+}(aq) + 5 OH–(aq) → Cu2O(s) + HCOO–(aq) + 3H2O(l)}\]
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\[\ce{Pb(s) + PbO2(s) + 2H2SO4(aq) → 2PbSO4(s) + 2H2O(l)}\]
Why does the following reaction occur?
\[\ce{XeO^{4-}_6 (aq) + 2F- (aq) + 6H+ (aq) -> XeO3(g) + F_2(g) + 3H_2O(l)}\]
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(ii) Chlorine is undergoing oxidation.
(iii) Oxygen is reduced.
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