AP Chemistry Redox Rx
Name___________________________
1)
What occurs during reduction of an atom? Why? Please write a reduction reaction for X.
2)
What occurs during oxidation of an atom? Why? Please write an oxidation reaction for X.
3)
What is an oxidizing agent? What happens to the oxidizing agent during a redox reaction?
4)
What is a reducing agent? What happens to the reducing agent during a redox reaction?
Please identify the species oxidized, the species reduced, the oxidizing agent & the reducing agent.
5)
2 Ag+ (aq) + Cu (s) → Cu+2 (aq) + 2 Ag (s)
6)
4 KClO3 (s) →
7)
4 Fe (s) + 3 O2 (g)
8)
Zn + 4 H+ + 2 NO3- →
KCl (s)
+
KClO4 (s)
→ 2 Fe2O3 (s)
Zn+2 + 2 NO2
+
2 H2O
Please write a redox reaction for each one. Then identify the element and species that are oxidized,
the element and species that are reduced, the oxidizing agent and the reducing agent.
9)
I2 oxidizes S2O3-2 ions to S4O6-2 and is reduced to I- ions in an acidic solution.
10)
Permanganate ions oxidize iron (II) to iron (III) in a sulfuric acid solution. Permanganate
ions are reduced to manganese (II) ions.
11)
In a basic solution, hypochlorite ions oxidize CrO2- ions to chromate ions and are reduced to
chloride ions.
12)
In an acidic solution, hypochlorite ions oxidize chloride ions to elemental chlorine gas and
are reduced to elemental chlorine gas.
13)
In an acidic solution, sulfite ions reduce dichromate ions to chromium (III) ions and are
oxidized to sulfate ions.
14)
Drano drain cleaner is solid NaOH that contains some Al chips. When Drano is added to
water, the NaOH dissolves rapidly with the evolution of a lot of heat. The Al reduces H2O
in the basic solution to produce [Al(OH)4]- ions and H2 gas, which gives the bubbling action.
15)
In an acidic solution, P4 + NO3- → H3PO4 + NO
16)
In an acidic solution, H2O2 + MnO4- → Mn2+ + O2
17)
In an acidic solution, HgS + Cl- + NO3- → HgCl42- + NO2 + S
18)
In a basic solution, CrO42- + HSnO2- → CrO2- + HSnO3-
19)
In an acidic solution, AsH3 (g) + ClO3- (aq)  H3AsO4 (aq) + Cl- (aq)
20)
In an acidic solution, HNO2 (aq) + I- (aq)  NO (g) + I2 (g)
21)
In a basic solution, MnO2 (s) + ClO3- (aq)  MnO4- (aq) + Cl- (aq)
22)
In a basic solution, Br2 (l)  Br- (aq) + BrO3- (aq)
23)
In a basic solution, N2O4 (aq) + Br- (aq)  NO2- (aq) + BrO3- (aq)
24)
In a basic solution, H2PO2- (aq) + SbO2- (aq)  HPO32- (aq) + Sb (s)
25)
In an acidic solution, Cu(OH)2 (s) + HPO32- (aq)  Cu2O (s) + PO43- (aq)
26)
In an acidic solution, HS- (aq) + IO3- (aq)  I- (aq) + S (s)
27)
In a basic solution, N2O (g) + ClO- (aq)  Cl- (aq) + NO2- (aq)
28)
In an acidic solution, H2SO3 (aq) + MnO2 (s)  SO42- (aq) + Mn2+ (aq)
29)
In an acidic solution, IO4- (aq) + I- (aq)  I2 (g)
30)
CrO42- (aq) + I- (aq)  Cr3+ (aq) + I2 (g)
Redox Common Reactants and Products
Common Reducing Agents
Halide ions
Free metals
SO32- or SO2
NO2Free halogens (dilute basic solution)
Free halogens (concentrated basic solution)
Metallous ions (lower oxidation numbers)
Common Oxidizing Agents
MnO4 (acidic solution)
MnO2 (acidic solution)
MnO4- (neutral or basic solution)
Cr2O72- (acidic solution)
HNO3 (concentrated)
HNO3 (dilute)
H2SO4 (hot, concentrated)
Metallic ions (higher oxidation numbers)
Free halogens
Na2O2
HClO4
C2O42H2O2
-
Products Formed
Free halogen
Metal ions
SO42NO3Hypohalite ions
Halate ions
Metallic ions (higher oxidation numbers)
Products Formed
2+
Mn
Mn2+
MnO2 (s)
Cr3+
NO2 (g)
NO (g)
SO2 (g)
Metallous ions (lower oxidation numbers)
Halide ions
NaOH
ClCO2 (g)
O2 (g)