Short Answer TypeConsider the reactions:
(a) H3PO2(aq) + 4 AgNO3(aq) + 2 H2O(l) → H3PO4(aq) + 4Ag(s) + 4HNO3(aq)
(b) H3PO2(aq) + 2CuSO4(aq) + 2H2O(l) → H3PO4(aq) + 2Cu(s) + H2SO4(aq)
(c) C6H5CHO(l) + 2[Ag (NH3)2]+(aq) + 3OH–(aq) → C6H5COO–(aq)+ 2Ag(s) +4NH3 (aq) + 2H2O(l)
(d) C6H5CHO(l) + 2Cu2+(aq) + 5OH–(aq) → No change observed.
What inference do you draw about the behaviour of Ag+ and Cu2+ from these reactions ?
Long Answer Type(i) Let the oxidation number of Si = x
Writing the oxidation number of each atom at the op of its symbol,
x -1
Si H4
The algebraic sum of oxidation number of various atoms = 0
x + 4 (-1) = 0
x = 4
(ii) Let the oxidation number of B =x
Writing the oxidation number of each atom at the top of its symbol
x -1
B H3
The algebraic sum of the oxidation number of various atoms = 0
x + 3(-1) = 0
x = 3
(iii) Let the oxidation number of B = x
Writing the oxidation number of each atom at the top of its symbol,
x -1
B F3
The algebraic sum of the oxidation number of various atoms = 0
x + 3 (-1) = 0
x = 3
Discuss briefly the types of redox reactions. Give examples.
or
Discuss the following redox reactions.
(a) Combination reactions
(b) Decomposition reactions
(c) Displacement reactions
(d) Disproportionation reactions.
Give one example in each case.
Suggest a scheme of classification of the following redox reactions:
(a) N2(g) + O2(g) → 2 NO (g)
(b) 2Pb(NO3)2(s) → 2PbO(s) + 2 NO2 (g) + ½ O2 (g)
(c) NaH(s) + H2O(l) → NaOH(aq) + H2 (g)
(d)2NO2(g) + 2OH–(aq) → NO2-(aq) +NO3–(aq)+H2O(l)
Short Answer TypeRefer to the periodic table given in your book and now answer the following questions:
(a) Select the possible non-metals that can show disproportionation reaction.
(b) Select three metals that can show disproportionation reaction.
Long Answer TypeShort Answer TypeWhat sorts of informations can you draw from the following reaction?
(CN)2(g) + 2OH– (aq) → CN–(aq) + CNO–(aq) + H2O(l)
Suggest a scheme of classification of the given redox reactions,
N2 (g) + O2 (g) 
2NO (g)
Switch
