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Practice: Fill in the Blanks Review Activity (Oxidation vs Reduction)

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Wize High School Grade 12 Chemistry Textbook > Electrochemistry

Redox Reactions

7 Activities

Review of Oxidation/Reduction:

  • Redox reaction: involve changes in oxidation states or numbers.
  • Oxidation AND reduction must occur in order for it to be called a redox reaction!

Oxidation

  • Involves losing/gaining electrons:
  • Increases/decreases oxidation #:
  • More/less bonds to O:
  • More/less bonds to H:
  • Oxidizing/reducing agent:
    agent (aka reductant)

Reduction

  • Involves losing/gaining electrons:
  • Increases/decreases oxidation #:
  • More/less bonds to O:
  • More/less bonds to H:
  • Oxidizing/reducing agent:
    agent (aka oxidant)
More Redox Reactions Questions:
Electrochemistry: Reduction potential application
Reduction Potentials Application
Below we see a diagram showing mitochondrial cellular respiration.
If we just consider the electron carrier NADH, NADH molecules gives up their electrons to the first complex, then the electron goes to the 2nd complex, then the 3rd, then the 4th and finally oxygen (O2) is the final electron acceptor.
Electrochemistry: Reduction potential application
Reduction Potentials Application
Below we see a diagram showing mitochondrial cellular respiration.
If we just consider the electron carrier NADH, NADH molecules gives up their electrons to the first complex, then the electron goes to the 2nd complex, then the 3rd, then the 4th and finally oxygen (O2) is the final electron acceptor.
Electrochemistry: Redox
Write the half-reactions for the following redox reaction. Which is the oxidizing agent and which is the reducing agent?
Au2+(aq) + 2I-(aq) <----> Au(s) + I2(s)
Electrochemistry: Reduction potential application
Reduction Potentials Application
Below we see a diagram showing mitochondrial cellular respiration.
If we just consider the electron carrier NADH, NADH molecules gives up their electrons to the first complex, then the electron goes to the 2nd complex, then the 3rd, then the 4th and finally oxygen (O2) is the final electron acceptor.
A voltaic cell is constructed with an Sn/Sn2+ half-cell and a Zn/Zn2+ half-cell. The zinc electrode is negative.
Write a balanced overall reaction for this cell
Draw a diagram of this cell, labeling electrodes with their charges and showing the direction of electron flow in the wire and anion/cation flow in the salt bridge
Consider the following balanced redox equation:
16H(aq)++2MnO4(aq)−+10Cl(aq)−→2Mn(aq)2++5Cl2(g)+8H2O(l)16H^+_{(aq)}+2MnO^-_{4(aq)}+10Cl^-_{(aq)} \to 2Mn^{2+}_{(aq)}+5Cl_{2(g)}+8H_2O_{(l)}
Which species is being oxidized?
Electrochemistry: Standard Reduction Potentials
A galvanic cell is constructed from chromium and copper electrodes immersed in aqueous solutions of Cr3+and Cu2+ respectively (half-reactions shown below).
Cr3+(aq)+3e−⇌Cr(s)Cr^{3+}(aq)+3e^-⇌Cr(s) E°red=−0.74VE°_{red}=-0.74V
Cu2+(aq)+2e−⇌Cu(s)Cu^{2+}(aq)+2e^-⇌Cu(s) E°red=+0.34VE°_{red}=+0.34V
Electrochemistry: Redox
Consider the following balanced redox equation:
16H(aq)++2MnO4(aq)−+10Cl(aq)−→2Mn(aq)2++5Cl2(g)+8H2O(l)16H^+_{(aq)}+2MnO^-_{4(aq)}+10Cl^-_{(aq)} \to 2Mn^{2+}_{(aq)}+5Cl_{2(g)}+8H_2O_{(l)}
Which species is being oxidized?
Electrochemistry: Redox
Consider the following balanced redox equation:
16H(aq)++2MnO4(aq)−+10Cl(aq)−→2Mn(aq)2++5Cl2(g)+8H2O(l)16H^+_{(aq)}+2MnO^-_{4(aq)}+10Cl^-_{(aq)} \to 2Mn^{2+}_{(aq)}+5Cl_{2(g)}+8H_2O_{(l)}
Which species is the reducing agent?
Consider the following balanced redox equation:
16H(aq)++2MnO4(aq)−+10Cl(aq)−→2Mn(aq)2++5Cl2(g)+8H2O(l)16H^+_{(aq)}+2MnO^-_{4(aq)}+10Cl^-_{(aq)} \to 2Mn^{2+}_{(aq)}+5Cl_{2(g)}+8H_2O_{(l)}
Which species is being reduced?