(c) What process occurs at the anode in the electrolysis of molten NaCl?

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Identify the components involved in the electrolysis of molten NaCl: sodium ions (Na^+) and chloride ions (Cl^-).

Understand that electrolysis involves the movement of ions towards electrodes: cations move to the cathode and anions move to the anode.

Recognize that at the anode, oxidation occurs, which involves the loss of electrons by anions.

Write the half-reaction for the oxidation of chloride ions at the anode: \( 2\text{Cl}^- \rightarrow \text{Cl}_2 + 2e^- \).

Conclude that chlorine gas (Cl_2) is produced at the anode as a result of the oxidation of chloride ions.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Electrolysis

Electrolysis is a chemical process that uses electrical energy to drive a non-spontaneous reaction. In this process, an electric current is passed through an electrolyte, causing the decomposition of the compound into its constituent elements. This is commonly used in the extraction of metals and the production of chemical compounds.

Anode Reaction

The anode is the electrode where oxidation occurs during electrolysis. In the case of molten NaCl, chloride ions (Cl-) are oxidized at the anode, releasing chlorine gas (Cl2). This reaction is crucial as it illustrates the transfer of electrons and the conversion of ions into neutral atoms or molecules.

Ionic Compounds in Electrolysis

Ionic compounds, like sodium chloride (NaCl), dissociate into their respective ions when melted or dissolved in water. During electrolysis, these ions migrate towards the electrodes, where they undergo oxidation or reduction. Understanding the behavior of these ions is essential for predicting the products formed during the electrolysis process.

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