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Exp 19A: Oxidation-Reduction Reactions

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Exp 19A: Oxidation-Reduction Reactions Oxidation-Reduction (Redox) reactions Net movement of electrons from one reactant to the other Movement from reactant with less ... – PowerPoint PPT presentation

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Title: Exp 19A: Oxidation-Reduction Reactions


1
Exp 19A Oxidation-Reduction Reactions
  • Oxidation-Reduction (Redox) reactions
  • Net movement of electrons from one reactant to
    the other
  • Movement from reactant with less attraction to
    reactant with more attraction for electrons
    (larger electron affinity)
  • Occurs in both ionic and covalent bond formation
  • Examples
  • 2 Mg(s) O2(g) ? 2 MgO (s) ionic bond formation
  • transfer of electrons (formation of
    cations and anions)
  • H2(g) Cl2(g) ? 2 HCl(g) covalent bond
    formation
  • shift in electron charge (dipole,
    polarity)

2
Exp 19A Oxidation-Reduction Reactions
Oxidation loss of electrons Mg ? Mg2
2e- Reduction gain in electrons ½ O2 2e-
? O2-
transfer or shift of electrons
X looses electron(s)
Y gains electron(s)
X is oxidized
Y is reduced
X is the reducing agent
Y is the oxidizing agent
X increases its oxidation number
Y decreases its oxidation number
  • reducing agents loose electrons while oxidizing
    agents gain electrons simultaneously
  • a chemical change cannot be an oxidation
    reaction or just a reduction reaction
  • it is always an oxidation-reduction reaction

3
Exp 19A Oxidation-Reduction Reactions
  • Goal of the Experiment (I)
  • Observe redox reactions between halogens
    (oxidizers) and halogen ions (halides, reducers)
    in cyclohexane
  • Halide ions (polar!) are insoluble in non-polar
    cyclohexane
  • Halogens (non-polar!) are soluble in cyclohexane
  • If a reaction takes place, the color in the
    cyclohexane may be different from the color in
    water, but ..
  • You have to make very careful observations and
    THINK about the results

4
Redox Activity of Halogens
  • F2 gt Cl2 gt Br2 gt I2
  • Redox potential and reactivity decreases down
    Group 7A
  • A halogen higher in the periodic system oxidizes
    one that is lower in the periodic system
  • Chlorine can oxidize bromide
  • -1 0 0 -1
  • 2 Br- (aq) Cl2 (aq) ? Br2 (aq) 2 Cl- (aq)
  • Bromine cannot oxidize chloride
  • 2 Cl- (aq) Br2 (aq) ? no reaction

5
Exp 19A Oxidation-Reduction Reactions
  • Goal of the Experiment (II)
  • Observe redox reactions with permanganate and
    iron(III) ions
  • Reduction of
  • MnO4- (permanganate, purple) to MnO42-
    (manganate, green)
  • MnO4- (permanganate, purple) to MnO2 (manganese
    oxide, black solid)
  • MnO4- (permanganate, purple) to Mn2
    (manganese(II) ion, pink)
  • Fe3 (iron(III), reddish brown) to Fe2(iron(II),
    pale green)

6
Exp 19A Oxidation-Reduction Reactions
  • Cl2 Solution
  • Reaction
  • 2OCl- 4H3O 2e- ? Cl2 6H2O
  • 2Cl- ? Cl2 2e-
  • 2OCl- 2Cl- 4 H3O ? 2Cl2 6H2O
  • or
  • OCl- Cl- 2 H3O ? Cl2 3H2O
  • Preparation of 12 mL 0.050 M chlorine water (add
    in this order and in the fume hood and leave it
    there!)
  • 1.70 mL bleach (NaOCl)
  • 1.2 ml 0.50 M H2SO4
  • 6.0 mL 0.20 M NaCl
  • 3.1 mL H2O
  • Put in large test tube

7
Exp 19A Oxidation-Reduction Reactions
  • Br2 Solution
  • Reaction
  • 2BrO3- 12 H3O 10e- ? Br2 18H2O
  • 10 Br- ? 5 Br2 10e-
  • 2BrO3- 10 Br- 12 H3O ? 6 Br2 18H2O
  • or
  • BrO3- 5 Br- 6 H3O ? 3 Br2 9H2O
  • Preparation of 12 mL 0.050 M bromine water
  • 1.0 mL 0.2 M KBrO3
  • 5.0 mL 0.20 M NaBr
  • 1.2 ml 0.50 M H2SO4
  • Wait 15 minutes before adding
  • 4.8 mL H2O
  • Put in large test tube

8
Exp 19A Oxidation-Reduction Reactions
  • I2 Solution
  • Reaction
  • 2Cu2 2I- 2e- ? 2CuI
  • 2I- ? I2 2e-
  • 2Cu2 4I- ? 2CuI I2
  • Preparation of 12 mL 0.050 M iodine water
  • 6.0 mL 0.20 M CuSO4
  • 6.0 mL 0.40 M NaI
  • Filter over double filter paper to remove
    insoluble CuI
  • Put solution in large test tube

9
Exp 19A Oxidation-Reduction Reactions
  • Exp 1
  • Put 15 drops of Cl2 solution in small test tube
  • Put 15 drops of Br2 solution in 2nd small test
    tube
  • Put 15 drops of I2 solution in 3rd small test
    tube
  • Add 1 mL cyclohexane to each tube
  • Shake or swirl solution gently
  • Record colors (if any) in cyclohexane layer
  • Keep these tubes as reference colors

10
Exp 19A Oxidation-Reduction Reactions
  • Exp 2 Reactions of Halogens with Halides (I)
  • Put 10 drops of 0.2 M NaCl in 2 clean and dry
    test tubes
  • Add 10 drops of Br2 solution to tube 1
  • Add 10 drops of I2 solution to tube 2
  • Add 1 mL cyclohexane to each tube
  • Shake or swirl
  • Record color change for both the aqueous and the
    organic layer
  • NO reaction cyclohexane will have color of
    aqueous layer
  • Reaction color change in cyclohexane

11
Exp 19A Oxidation-Reduction Reactions
  • Exp 2 Reactions of Halogens with Halides (II)
  • Clean test tubes
  • Put 10 drops of 0.2 M NaBr in 2 clean and dry
    test tubes
  • Add 10 drops of Cl2 solution to tube 1
  • Add 10 drops of I2 solution to tube 2
  • Add 1 mL cyclohexane to each tube
  • Shake or swirl
  • Record color change for both the aqueous and the
    organic layer

12
Exp 19A Oxidation-Reduction Reactions
  • Exp 2 Reactions of Halogens with Halides (III)
  • Clean test tubes
  • Put 5 drops of 0.4 M NaI in 2 clean and dry test
    tubes
  • Add 10 drops of Cl2 solution to tube 1
  • Add 10 drops of Br2 solution to tube 2
  • Add 1 mL cyclohexane to each tube
  • Shake or swirl
  • Record color change for both the aqueous and the
    organic layer

13
Exp 19A Oxidation-Reduction Reactions
  • Exp 3 Reactions of Permanganate and Iron (I)
  • Clean test tubes
  • Put 15 drops of 0.2 M NaBr in two test tubes
  • Add 1 drop of 0.1 M KMnO4 solution to tube 1
  • Add 5 drops of 0.1 M FeCl3 solution to tube 2
  • Add 5 drops of 3 M H2SO4 to each tube
  • Add 1 mL cyclohexane to each tube
  • Shake or swirl
  • Record color change/observations for both the
    aqueous and the organic layer

14
Exp 19A Oxidation-Reduction Reactions
  • Exp 3 Reactions of Permanganate and Iron (II)
  • Clean test tubes
  • Put 8 drops of 0.4 M NaI in two test tubes
  • Add 1 drop of 0.1 M KMnO4 solution to tube 1
  • Add 5 drops of 0.1 M FeCl3 solution to tube 2
  • Add 5 drops of 3 M H2SO4 to each tube
  • Add 1 mL cyclohexane to each tube
  • Shake or swirl
  • Record color change/observations for both the
    aqueous and the organic layer

15
Exp 19A Oxidation-Reduction Reactions
  • Exp 3 Reactions of Permanganate and Iron (III)
  • Clean test tubes
  • Put 8 drops of 0.4 M NaI in one test tube
  • Add 5 drop of 6.0 M NaOH solution to tube
  • Add 1 drop of 0.1 M KMnO4 solution to tube
  • Add 1 mL cyclohexane to tube
  • Shake or swirl
  • Record color change/observations for both the
    aqueous and the organic layer

16
Exp 19A Oxidation-Reduction Reactions
  • Exp 3 Reactions of Halogens and Halides
  • Cl- Br2 NR Br2 is still present
    (yellow-orange color)
  • Cl- I2 NR I2 is still present (violet color)
  • Cl2 2Br- ? 2Cl- Br2 (yellow-orange color)
  • I2 2Br- NR I2 is still present (violet
    color)
  • Cl2 2I- ? 2Cl- I2 (violet color)
  • Br2 2I- ? 2Br- I2 (violet color)

17
Exp 19A Oxidation-Reduction Reactions
  • Exp 3 Reactions of Permanganate and Iron
  • (7) 2MnO4- 16H3O 10e- ? 2Mn2 8H2O
  • 10Br- ? 5Br2 10e-
  • 2MnO4- 10Br- 16H3O ? 2Mn2 5Br2 8H2O
    (yellow-orange color)
  • (9) 2MnO4- 16H3O 10e- ? 2Mn2 8H2O
  • 10I- ? 5I2 10e-
  • 2MnO4- 10I- 16H3O ? 2Mn2 5I2 8H2O
    (violet color)
  • (8) Fe3 Br- ? No color, No Reaction
  • (10) 2Fe3 2 e- ? 2Fe2
  • 2I- ? I2 2e-
  • 2Fe3 2I- ? 2Fe2 I2 (violet color)

18
Exp 19A Oxidation-Reduction Reactions
  • Exp 3 Reactions of Permanganate and Iron
  • (11) 6MnO4- 6e- ? 6MnO42-
  • I- 3H2O ? IO3- 6H3O 6e-
  • 6H3O 6OH- ? 6H2O
  • 6MnO4- I- 6OH- ? 6MnO42- IO3- 3H2O
  • green color in aqueous layer
  • no color in cyclohexane
  • no formation of a nonpolar halogen

19
Exp 19A Oxidation-Reduction Reactions
  • Post Lab
  • Results sheets (p. 351-352)
  • Post lab questions 1, 2a-d, 3a-c
  • Give balanced equations for every reaction that
    happened
  • If there was no reaction, write NR and indicate
    how you reached that conclusion
  • Answer the questions
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