Electrolysis of Ionic Compounds
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Questions and Answers

What occurs at the cathode during a redox reaction?

  • Decrease in temperature
  • Formation of gas
  • Reduction of ions (correct)
  • Oxidation of ions

    • Oxidation occurs when a substance gains electrons.

    False

    What ion is produced at the anode when bromide ions are oxidized?

    Bromine

    If a metal is below hydrogen in the reactivity series, it will be formed at the ______.

    <p>cathode</p> Signup and view all the answers

    Match the following processes with their corresponding electrodes:

    <p>Reduction = Cathode Oxidation = Anode Electron gain = Cathode Electron loss = Anode</p> Signup and view all the answers

    Which ion will more likely be discharged at the anode along with common negative ions?

    <p>Copper (Cu2+)</p> Signup and view all the answers

    Hydroxide ions are more likely to be discharged than sulfate ions.

    <p>False</p> Signup and view all the answers

    List one example of a common negative ion that obtains oxygen at the anode during electrolysis.

    <p>Sulfate</p> Signup and view all the answers

    The order of cation discharge is as follows: Na+, _____, Al3+, H+, Cu2+.

    <p>Mg2+</p> Signup and view all the answers

    Match the following negative ions with their discharge likelihood:

    <p>SO4^2− = Less likely to be discharged Cl− = More likely to be discharged NO3− = Less likely to be discharged Br− = More likely to be discharged</p> Signup and view all the answers

    What products are formed at the cathode during the electrolysis of sodium chloride solution?

    <p>Hydrogen gas</p> Signup and view all the answers

    Chlorine gas is a safe product that can be inhaled without precautions during electrolysis.

    <p>False</p> Signup and view all the answers

    What is left behind in the solution after the electrolysis of sodium chloride?

    <p>Sodium hydroxide solution</p> Signup and view all the answers

    Sodium chloride (NaCl) dissociates in solution to form ___, ___, ___, and ___ ions.

    <p>Na+, Cl-, H+, OH-</p> Signup and view all the answers

    Match the products with their respective locations during the electrolysis of sodium chloride solution:

    <p>Hydrogen gas = Cathode Chlorine gas = Anode Sodium hydroxide solution = Remaining in solution after electrolysis Na+ and OH- = Left behind after electrolysis</p> Signup and view all the answers

    What is formed at the cathode during the electrolysis of molten lead (II) bromide?

    <p>Lead</p> Signup and view all the answers

    Bromine gas is formed at the anode during electrolysis of molten lead (II) bromide.

    <p>True</p> Signup and view all the answers

    What is the half-reaction for the cathode during the electrolysis of aluminum oxide?

    <p>Al3+(aq) + 3e- → Al(s)</p> Signup and view all the answers

    During electrolysis, the electrode where reduction occurs is called the ______.

    <p>cathode</p> Signup and view all the answers

    Which of the following is a product of the anode during the electrolysis of sodium chloride?

    <p>Chlorine gas</p> Signup and view all the answers

    Match the following ionic compounds with their correct anode products:

    <p>Lead (II) bromide = Bromine gas Zinc chloride = Chlorine gas Sodium chloride = Chlorine gas Aluminum oxide = Oxygen gas</p> Signup and view all the answers

    Reduction involves the loss of electrons.

    <p>False</p> Signup and view all the answers

    What type of electrodes are used during the electrolysis of aluminum oxide?

    <p>Platinum electrodes</p> Signup and view all the answers

    The cathode product of copper bromide during electrolysis is ______.

    <p>Copper</p> Signup and view all the answers

    What is the overall reaction at the anode for the electrolysis of zinc chloride?

    <p>2Cl- → Cl2(g) + 2e-</p> Signup and view all the answers

    What gas is produced at the cathode during the electrolysis of potassium iodide (KI) solution?

    <p>Hydrogen gas</p> Signup and view all the answers

    The electrolysis of magnesium bromide (MgBr2) solution produces bromine gas at the anode.

    <p>True</p> Signup and view all the answers

    What happens to the blue color of the solution during the electrolysis of copper (II) sulfate using inert electrodes?

    <p>The blue color fades as copper ions are discharged.</p> Signup and view all the answers

    Match the following half-reactions with their corresponding reactions:

    <p>2I- → I2(g) + 2e = Electrolysis of KI solution (Anode) Cu2+ + 2e → Cu(s) = Electrolysis of copper (II) sulfate (Cathode) 2Br- → Br2(g) + 2e = Electrolysis of MgBr2 solution (Anode) 2H+ + 2e → H2(g) = Electrolysis of both KI and MgBr2 solutions (Cathode)</p> Signup and view all the answers

    The half-reaction at the anode for the electrolysis of copper (II) sulfate solution using copper electrodes is: Cu (s) ______ Cu2+(aq) + 2e.

    <p>→</p> Signup and view all the answers

    Study Notes

    Electrolysis of Molten Ionic Compounds

    • Electrolysis is the process of using electricity to decompose a compound.
    • In molten ionic compounds, the ions are free to move and conduct electricity.
    • At the cathode (negative electrode), positive ions gain electrons and are reduced.
    • At the anode (positive electrode), negative ions lose electrons and are oxidized.
    • The products of electrolysis can be predicted based on the reactivity series.

    Electrolysis of Lead (II) Bromide (PbBr2)

    • Molten PbBr2 decomposes into Pb2+ and Br- ions
    • At the cathode, Pb2+ ions gain electrons to form lead metal (Pb).
    • At the anode, Br- ions lose electrons to form bromine gas (Br2).

    Products of Electrolysis of Molten Compounds

    • Aluminum Oxide (Al2O3):
      • Cathode: Aluminum metal (Al) is formed.
      • Anode: Oxygen gas (O2) is evolved.
    • Copper Bromide (CuBr):
      • Cathode: Copper metal (Cu) is formed.
      • Anode: Bromine gas (Br2) is evolved.
    • Zinc Chloride (ZnCl2):
      • Cathode: Zinc metal (Zn) is formed.
      • Anode: Chlorine gas (Cl2) is evolved.
    • Sodium Chloride (NaCl):
      • Cathode: Sodium metal (Na) is formed.
      • Anode: Chlorine gas (Cl2) is evolved.

    Electrolysis and Redox Reactions

    • Reduction: Gain of electrons. This process occurs at the cathode.
    • Oxidation: Loss of electrons. This process occurs at the anode.
    • Redox Reactions: Oxidation and reduction always occur simultaneously.
    • Cathode: Reduction (RED CAT)
    • Anode: Oxidation (AN OX)

    Reactivity Series and Electrolysis

    • Metals above hydrogen in the reactivity series: Hydrogen gas is produced at the cathode instead of the metal.
    • Metals below hydrogen in the reactivity series: The metal is produced at the cathode.
    • Halides (chlorides, bromides, iodides): The corresponding halogen is produced at the anode.
    • Other common negative ions (sulfate, nitrate, hydroxide): Oxygen gas is produced at the anode.

    Electrolysis of Sodium Chloride Solution (NaCl)

    • Ions in solution: Na+, Cl-, H+, OH-
    • Cathode: Hydrogen gas (H2) is produced.
    • Anode: Chlorine gas (Cl2) is produced.
    • Result: The solution becomes alkaline due to the formation of sodium hydroxide (NaOH).
    • Safety: Chlorine gas is poisonous. Electrolysis of NaCl should be performed in a fume hood or well-ventilated area.

    Electrolysis of Potassium Iodide Solution (KI)

    • Ions in solution: K+, I-, H+, OH-
    • Cathode: Hydrogen gas (H2) is produced.
    • Anode: Iodine gas (I2) is produced.

    Electrolysis of Magnesium Bromide Solution (MgBr2)

    • Ions in solution: Mg2+, Br-, H+, OH-
    • Cathode: Hydrogen gas (H2) is produced.
    • Anode: Bromine gas (Br2) is produced.

    Electrolysis of Aqueous Copper (II) Sulphate Solution

    • Ions in solution: H+, OH-, Cu2+, SO42-
    • Using Inert Electrodes:
      • Cathode: Copper metal (Cu) is deposited, resulting in a fading blue color of the solution.
      • Anode: Oxygen gas (O2) is produced.
    • Using Copper Electrodes:
      • Cathode: Copper metal (Cu) is deposited.
      • Anode: Copper metal (Cu) dissolves, releasing Cu2+ ions, maintaining the deep blue color of the solution.

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