4.3.3 Using electrolysis to extract metals

• Electrolysis requires ionic compounds to be either molten or dissolved in solution.


  True
• The cathode in electrolysis has a negative charge and is where reduction occurs.


  True
• Reduction at the cathode results in the gain of electrons and the formation of neutral atoms or molecules.

  True
• What is electrolysis used for in chemistry?

  Decomposing ionic compounds
• At the anode, the process of oxidation occurs, where electrons are lost.
• Match the electrode with its process and charge:

  Anode ↔️ Oxidation, Positive (+)

  Cathode ↔️ Reduction, Negative (-)
• What is the reaction at the anode during the electrolysis of molten sodium chloride?

  2Cl^- → Cl₂ + 2e^-
• What is the purpose of heating sodium chloride in its electrolysis to extract sodium metal?

  To make it molten
• At the anode during electrolysis of molten NaCl, chlorine gas is produced, represented by the reaction 2Cl^- → Cl₂ + 2e^-.
• Ionic compounds used as electrolytes must be molten or dissolved in water.


  True
• Metals suitable for electrolysis extraction are highly reactive.
• Electrolysis is the preferred extraction method for highly reactive metals like potassium and calcium.


  True
• The cathode is where oxidation occurs and loses electrons.

  False
• At the cathode, the process that occurs is reduction
• During electrolysis, negative ions lose electrons at the anode


  True
• Why are electrolytes essential in electrolysis?

  Conduct electricity
• Where does reduction occur in electrolysis?

  Cathode
• Highly reactive metals are suitable for electrolysis extraction because they require a significant amount of energy to be reduced.


  True
• Sodium is an example of a reactive metal extracted using electrolysis.


  True
• Electrolytes in electrolysis must be either molten or dissolved in water.

  True
• The anode is the electrode where oxidation occurs.
• The cathode carries a negative (-) charge.
• At the cathode, reduction occurs as ions gain electrons.


  True
• An electrolyte contains free ions to conduct electricity.
• Order the steps in the electrolysis of molten NaCl:

  1️⃣ Chlorine ions are oxidized at the anode

  2️⃣ Sodium ions are reduced at the cathode

  3️⃣ Chlorine gas forms at the anode

  4️⃣ Sodium metal forms at the cathode
• Sodium is a reactive metal extracted using electrolysis.
• Electrolysis uses an electric current to break down ionic compounds.
• At the anode, the process that occurs is oxidation
• During electrolysis, positive ions gain electrons at the cathode

  True
• An electrolyte contains free ions
• Where does oxidation occur in electrolysis?

  Anode
• Reduction is the gain of electrons
• What type of reduction is used for less reactive metals like iron and copper?

  Chemical
• Electrolysis is especially useful for extracting metals that are highly reactive
• During electrolysis, the key reaction at the anode is oxidation, which involves the loss of electrons.
• An electrolyte contains free ions, which can conduct electricity
• The extraction of sodium metal from sodium chloride involves heating NaCl until molten.
• The anode carries a positive (+) charge.

  True
• Match the electrode with its process and charge:

  Anode ↔️ Oxidation, Positive (+)

  Cathode ↔️ Reduction, Negative (-)
• At the cathode during electrolysis of molten NaCl, sodium metal is formed.


  True