Tech Team · Kintek Solution

In an electrolytic cell, the cathode is negatively charged, and the anode is positively charged. This is because the cell operates by using an external voltage source to drive non-spontaneous redox reactions. The cathode attracts cations (positively charged ions) from the electrolyte, where reduction occurs, while the anode attracts anions (negatively charged ions), where oxidation occurs. The electrolyte facilitates the movement of ions between the electrodes, completing the circuit. Understanding the signs and roles of the electrodes is crucial for applications like electroplating, metal refining, and chemical synthesis.

Key Points Explained:

1. Electrode Signs in an Electrolytic Cell:

   • Cathode: Negatively charged.
   • Anode: Positively charged.
   • This is opposite to a galvanic cell, where the cathode is positive and the anode is negative. The external voltage source in an electrolytic cell reverses the natural flow of electrons.

2. Components of an Electrolytic Cell:

   • Electrolyte: A solution or molten salt containing ions that facilitate the flow of electric current. Common examples include aqueous solutions of salts or acids and molten sodium chloride.
   • Cathode: The electrode where reduction occurs. It attracts cations (positively charged ions) from the electrolyte.
   • Anode: The electrode where oxidation occurs. It attracts anions (negatively charged ions) from the electrolyte.

3. Redox Reactions in the Cell:

   • Reduction at the Cathode: Positively charged ions (cations) gain electrons and are reduced. For example, in the electrolysis of molten sodium chloride, Na⁺ ions are reduced to sodium metal at the cathode.
   • Oxidation at the Anode: Negatively charged ions (anions) lose electrons and are oxidized. In the same example, Cl⁻ ions are oxidized to chlorine gas at the anode.

4. Role of the External Voltage Source:

   • The external voltage source provides the energy needed to drive the non-spontaneous redox reactions. It ensures that electrons flow from the anode to the cathode through the external circuit, while ions move through the electrolyte to maintain charge balance.

5. Electrode Materials:

   • Electrodes are typically made of inert materials like graphite or platinum to prevent unwanted reactions with the electrolyte. The choice of material depends on the specific application and the chemicals involved.

6. Discharge Potential:

   • The minimum voltage required to initiate electrolysis and discharge ions at the electrodes. If multiple ions are present, the ion with the higher reduction potential is reduced at the cathode, and the ion with the lower reduction potential is oxidized at the anode.

7. Applications of Electrolytic Cells:

   • Electroplating: Depositing a layer of metal onto a surface.
   • Metal Refining: Purifying metals like copper or aluminum.
   • Chemical Synthesis: Producing substances like chlorine, hydrogen, and sodium hydroxide.

Understanding these key points helps in designing and operating electrolytic cells for various industrial and laboratory applications. The signs of the electrodes and their roles in redox reactions are fundamental to the functioning of these cells.

Summary Table:

Aspect	Details
Cathode	Negatively charged; attracts cations; reduction occurs here.
Anode	Positively charged; attracts anions; oxidation occurs here.
Electrolyte	Facilitates ion movement; examples include molten salts or aqueous solutions.
Redox Reactions	Reduction at cathode, oxidation at anode.
External Voltage Source	Drives non-spontaneous reactions; ensures electron flow.
Applications	Electroplating, metal refining, chemical synthesis.

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