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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    Description

    Test your knowledge on the electrolysis of molten ionic compounds, including lead (II) bromide and aluminum oxide. This quiz covers the movement of ions, electrode reactions, and products formed during the process. Understand the principles behind electrolysis and the reactivity series.

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