Advertisements
Advertisements
प्रश्न
Suggest a list of the substances where carbon can exhibit oxidation states from –4 to +4 and nitrogen from –3 to +5.
Advertisements
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 |
APPEARS IN
संबंधित प्रश्न
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:
\[\ce{4 NH3(g) + 5 O2(g) → 4NO(g) + 6H2O(g)}\]
Identify the substance oxidised, reduced, oxidising agent and reducing agent for the following reaction:
\[\ce{HCHO(l) + 2[Ag (NH3)2]+(aq) + 3OH–(aq) → 2Ag(s) + HCOO–(aq) + 4NH3(aq) + 2H2O(l)}\]
Identify the substance oxidised, reduced, oxidising agent and reducing agent for the following reaction:
\[\ce{HCHO (l) + 2Cu^{2+}(aq) + 5 OH–(aq) → Cu2O(s) + HCOO–(aq) + 3H2O(l)}\]
Identify the substance oxidised, reduced, oxidising agent and reducing agent for the following reaction:
\[\ce{N2H4(l) + 2H2O2(l) → N2(g) + 4H2O(l)}\]
Identify the substance oxidised, reduced, oxidising agent and reducing agent for the following reaction:
\[\ce{Pb(s) + PbO2(s) + 2H2SO4(aq) → 2PbSO4(s) + 2H2O(l)}\]
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.
Refer to the periodic table given in your book and now answer the following questions:
Select the possible non-metals that can show disproportionation reaction.
Refer to the periodic table given in your book and now answer the following question:
Select three metals that can show disproportionation reaction.
Which of the following elements does not show disproportionation tendency?
Why does fluorine not show disporportionation reaction?
Write redox couples involved in the reactions given.
\[\ce{Cu + Zn^{2+} ->Cu^{2+} + Zn}\]
Write redox couples involved in the reactions given.
\[\ce{Mg + Fe^{2+} -> Mg^{2+} + Fe}\]
Write redox couples involved in the reactions given.
\[\ce{Br2 + 2Cl- -> Cl2 + 2Br-}\]
Write redox couples involved in the reactions given.
\[\ce{Fe + Cd^{2+} -> Cd + Fe^{2+}}\]
An acidified manganate solution undergoes disproportionation reaction. The spin-only magnetic moment value of the product having manganese in a higher oxidation state is ______ B.M. (Nearest integer)
\[\ce{H2O2 -> H2O + O2}\]
This represents ______.
