Science, Tech, Math › Science Find the Anode and Cathode of a Galvanic Cell Electrodes of a Battery Share Flipboard Email Print Erik Dreyer / Getty Images Science Chemistry Basics Chemical Laws Molecules Periodic Table Projects & Experiments Scientific Method Biochemistry Physical Chemistry Medical Chemistry Chemistry In Everyday Life Famous Chemists Activities for Kids Abbreviations & Acronyms Biology Physics Geology Astronomy Weather & Climate By Todd Helmenstine Todd Helmenstine is a science writer and illustrator who has taught physics and math at the college level. He holds bachelor's degrees in both physics and mathematics. our editorial process Todd Helmenstine Updated May 07, 2019 Anodes and cathodes are the endpoints or terminals of a device that produces electrical current. Electrical current runs from the positively charged terminal to the negatively charged terminal. The cathode is the terminal that attracts cations, or positive ions. To attract the cations, the terminal must be negatively charged. Electrical current is the amount of charge that passes a fixed point per unit time. The direction of the current flow is the direction in which a positive charge flows. Electrons are negatively charged and move in the opposite direction of the current. In a galvanic cell, the current is produced by connecting an oxidation reaction to a reduction reaction in an electrolyte solution. Oxidation and reduction reactions or redox reactions are chemical reactions involving a transfer of electrons from one atom in the reaction to another. When two different oxidation or reduction reactions are connected electrically, a current is formed. The direction depends on the type of reaction taking place at the terminal.Reduction reactions involve the gain of electrons. Electrons are needed to fuel the reaction and pull these electrons from the electrolyte. Since electrons are attracted to the reduction site and current flows opposite the flow of electrons, current flows away from the reduction site. Since current flows from the cathode to the anode, the reduction site is the cathode.Oxidation reactions involve the loss of electrons. As the reaction progresses, the oxidation terminal loses electrons to the electrolyte. The negative charge moves away from the oxidation site. The positive current moves towards the oxidation site, against the flow of electrons. Since current flows to the anode, the oxidation site is the anode of the cell. Keeping Anode and Cathode Straight On a commercial battery, the anode and cathode are clearly marked (- for anode and + for cathode). Sometimes only the (+) terminal is marked. On a battery, the bumpy side is (+) and the smooth side is (-). If you're setting up a galvanic cell, you'll need to keep the redox reaction in mind to identify the electrodes. Anode: positively charged terminal - oxidation reactionCathode: negatively charged terminal - reduction reactionThere are a couple mnemonics that can help you remember the details.To remember the charge: Ca+ions are attracted to the Ca+hode (the t is a plus sign)To remember which reaction occurs at which terminal: An Ox and Red Cat - Anode Oxidation, Reduction Cathode Remember, the concept of electrical current was defined back before scientists understood the nature of positive and negative charges, so it was set up for the direction a (+) charge would move. In metals and other conductive materials, it's actually the electrons or (-) charges that move. You can think of it as holes of positive charge. In an electrochemical cell, it's just as likely cations will move as anions (in fact, both are probably moving at the same time).