Magnesium metal is produced by the electrolysis of molten magnesium chloride using inert electrodes. (a) Sketch the cell, label the anode and cathode, indicate the sign of the electrodes, and show the direction of electron and ion flow.

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. In the case of magnesium chloride, the electrolysis results in the production of magnesium metal at the cathode and chlorine gas at the anode.

In an electrolysis cell, there are two electrodes: the anode and the cathode. The anode is the positive electrode where oxidation occurs, while the cathode is the negative electrode where reduction takes place. In the electrolysis of magnesium chloride, magnesium ions gain electrons at the cathode to form magnesium metal, while chloride ions lose electrons at the anode to produce chlorine gas.

During electrolysis, ions move towards the electrodes due to the electric field created by the applied voltage. Cations (positively charged ions) migrate towards the cathode, where they gain electrons, while anions (negatively charged ions) move towards the anode, where they lose electrons. Understanding the direction of ion and electron flow is crucial for correctly sketching the electrolysis cell and labeling the electrodes.