Order Balancing Oxidation Reduction Reactions Assignment

Order Balancing Oxidation-Reduction Reactions Assignment
17.1 Arrange the following species in order of
increasing oxidation number of the sulfur atom:
(a) H2S, (b) S8, (c) H2SO4, (d) S2−, (e) HS−,
(f) SO2, (g) SO3.
17.2 Phosphorus forms many oxoacids. Indicate the
oxidation number of phosphorus in each of the
following acids: (a) HPO3, (b) H3PO2, (c) H3PO3,
(d) H3PO4, (e) H4P2O7, (f) H5P3O10.
17.3 Give the oxidation numbers for the underlined
atoms in the following molecules and ions:
(a) ClF, (b) IF7, (c) CH4, (d) C2H2, (e) C2H4,
(f) K2CrO4, (g) K2Cr2O7, (h) KMnO4, (i) NaHCO3,
(j) Li2, (k) NaIO3, (l) KO2, (m) PF6
−, (n) KAuCl4.
17.4 Give the oxidation numbers for the underlined atoms
in the following molecules and ions: (a) Cs2O,
(b) CaI2, (c) Al2O3, (d) H3AsO3, (e) TiO2, (f) MoO4
2−,
(g) PtCl4
2−, (h) PCl6
−, (i) SnF2, (j) ClF3, (k) SbF6
−.
17.5 Assign oxidation states to each element and use
this information to identify the substance
undergoing oxidation and the substance
undergoing reduction in each reaction.
(a) 2AlCl3(s) ⟶ 2Al(s) 3Cl2(g)
(b) Zn(s) S(s) ⟶ ZnS(s)
17.6 Assign oxidation states to each element and use
this information to identify the substance
undergoing oxidation and the substance
undergoing reduction in each reaction.
(a) Ni(s) Cu(NO3)2(aq) ⟶
Ni(NO3)2(aq) Cu(s)
(b) 2C2H4(g) 5O2(g) ⟶ 4CO2(g) 2H2O(g)
17.7 Identify the oxidizing agent and the reducing
agent in each reaction.
(a) 2Sr O2 ⟶ 2SrO
(b) 2Li H2 ⟶ 2LiH
(c) 2Cs Br2 ⟶ 2CsBr
(d) 3Mg N2 ⟶ Mg3N2
17.8 Identify the oxidizing agent and the reducing
agent in each reaction.
(a) 4Fe 3O2 ⟶ 2Fe2O3
(b) Cl2 2NaBr ⟶ 2NaCl Br2
(c) Si 2F2 ⟶ SiF4
(d) H2 Cl2 ⟶ 2HCl
Order Balancing Oxidation Reduction Reactions Assignment
17.9 Identify the oxidizing agent and the reducing
agent in each reaction.
(a) 2H2O2 ⟶ 2H2O O2
(b) Mg 2AgNO3 ⟶ Mg(NO3)2 2Ag
(c) NH4NO2 ⟶ N2 2H2O
(d) H2 Br2 ⟶ 2HBr
17.10 Identify the oxidizing agent and the reducing
agent in each reaction.
(a) P4 10Cl2 ⟶ 4PCl5
(b) 2NO ⟶ N2 O2
(c) Cl2 2KI ⟶ 2KCl I2
(d) 3HNO2 ⟶ HNO3 H2O 2NO
17.11 Balance the following redox equations by the
half-reaction method:
(a) H2O2 Fe2 ⟶ Fe3 H2O
(in acidic solution)
(b) Cu HNO3 ⟶ Cu2 NO H2O
(in acidic solution)
(c) CN− MnO4
− ⟶ CNO− MnO2
(in basic solution)
(d) Br2 ⟶ BrO3
− Br− (in basic solution)
(e) S2O3
2− I2 ⟶ I− S4O6
2−
(in acidic solution)
17.12 Balance the following redox equations by the
half-reaction method:
(a) Mn2 H2O2 ⟶ M