In a corrosion cell, electrons flow in the direction of:

In a corrosion cell, electrons flow from the anode to the cathode through the metallic path. The anode is the site where oxidation occurs, leading to the loss of electrons. These electrons are then conducted through the metal or metallic components of the corrosion cell to the cathode, where a reduction reaction takes place.

This flow of electrons is fundamental to the operation of electrochemical cells. The metallic path provides a conductive route for the electrons to travel, allowing the electrochemical reactions at both the anode and cathode to occur effectively. If the pathway for electron flow were to be interrupted or altered, the efficiency of the corrosion process would be compromised.

In contrast, the other options either confuse the direction of electron flow or state incorrect pathways. The electrolyte typically facilitates ion movement within the cell, not electron flow, which exclusively happens through the metal in this context. Therefore, the understanding of electron flow from the anode to the cathode via the metallic path is essential for grasping the principles of corrosion processes.