Chemistry 30
Chapter 13
Name:
Oxidation Numbers
Extra Exercises
Section 13.3
1. Assign oxidation numbers to chlorine in each of the following chemicals.
HCl(aq),
Cl2(g),
NaClO(s),
Cl(aq),
ClO3(aq),
KClO2(s),
ClO2(g),
HClO4(aq)
HClO3(aq),
2. Assign oxidation numbers to manganese in each of the following chemicals.
MnO2(s),
KMnO4(s),
Mn2O7(s),
Mn2+(aq)
Mn(s),
MnO42(aq),
MnCl2(s),
For the following reaction equations, use oxidation numbers to identify the oxidation
(the atom oxidized) and the reduction (the atom reduced).
3.
AsO33(aq) + IO3–(aq) AsO43(aq) + I(aq)
4.
CuO(s) + NH3(g) N2(g) + H2O(l) + Cu(s)
5. MnO4(aq) + H2Se(g) + H+(aq) Se(s) + Mn2+(aq) + H2O(l)
6. PbO2(s) + Pb(s) + H2SO4(aq) PbSO4(s) + H2O(l)
7. Cl2(g) + OH–(aq) ClO3–(aq) + Cl–(aq) + H2O(l)
Balance Redox Equations with Oxidation Numbers
Extra Exercises
Section 13.3
Balance the following reaction equations.
1. Sn2+(aq) + Fe3+(aq) → Fe2+(aq) + Sn4+(aq)
(neutral solution)
2. CH3OH(aq) + MnO4–(aq) → Mn2+(aq) + CH2O(aq)
(acidic solution)
3. Fe2+(aq) + Cr2O72–(aq) → Cr3+(aq) + Fe3+(aq)
(acidic solution)
4. CH3OH(aq) + MnO4(aq) → MnO42–(aq) + CO32–(aq)
(basic solution)
5. MnO4(aq) + SO32–(aq) → SO42–(aq) + MnO2(s)
(basic solution)
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