Difference Between Anode and Cathode

The main difference between anode and cathode is that anode is the terminal where the (conventional) current flows into a device from outside, whereas cathode is the terminal where (conventional) current flows out of the device.

Cathode and anode are terms used to refer to terminals of a polarised electrical device. However, the usage is not strictly followed in some instances because when a device is able to undergo a reversible process, the same terminal that was called the “anode” could be called the “cathode”. Undoubtedly, this may lead to confusion, and it is advisable to adapt to the general usage in the specific field. In this article, we will look at several scenarios where these terms are used and explore their usage in terms of the processes that occur in these devices.

Key Areas Covered

1. What is an Anode
2. What is a Cathode
3. Anode and Cathode in Galvanic/Voltaic Cells
4. Anode and Cathode in Electrolytic Cells
5. Difference Between Anode and Cathode

Key Terms

Electrochemical Cells, Anode, Cathode

Difference Between Anode and Cathode - Comparison Summary

What is an Anode

The anode is the terminal where the (conventional) current flows into a device from outside. This means that electrons flow out of the device at the anode.

What is a Cathode

The cathode is the terminal where the (conventional) current flows out of a device. This means that electrons flow into this terminal from the outside.

Anode and Cathode in Galvanic/Voltaic Cells

The setup of a galvanic cell is shown below:

Difference Between Anode and Cathode - A_Galvanic_Cell

A Galvanic cell

In a Galvanic cell, one of the electrodes is at a higher reduction potential than the other. The electrode with a higher reduction potential has a stronger ability to gain electrons, so electrons flow into it from the other electrode. In the cell drawn above, copper has a higher reduction potential than zinc, so it draws electrons from the zinc electrode. This accompanies two reactions. At the zinc electrode, the zinc dissociates into Zn2+ ions and electrons. In other words, zinc is being oxidised (it loses electrons).

\mathrm{Zn\rightarrow Zn^{2+}+2e^-}

The electrons lost by zinc flow across the wires onto the copper electrode. Here, the incoming electrons combine with Cu2+ ions and form copper atoms. Copper is being reduced (it gains electrons):

\mathrm{Cu^{2+}+2e^-\rightarrow Cu}

Here, electrons flow “out of the device” from the zinc terminal, so the conventional current is flowing into the device here. This makes the zinc terminal the anode. Conventional current flows out of the device at the copper terminal, so it makes copper the cathode. Whenever a device works using redox reactions, the terminal where oxidation happens is the anode, and the electrode where reduction happens is the cathode. This agrees with the description above: zinc (the anode) becomes oxidised, and copper (the cathode) gets reduced.

Anode and Cathode in Electrolytic Cells

In electrolytic cells, a power supply is used to create a current in a liquid containing ions. For instance, we will look at what happens when two electrodes are put into a sample of molten sodium chloride (NaCl or common salt).

Difference Between Anode and Cathode - Electrolysis

Electrolysis of molten sodium chloride

The electrode connected to the positive terminal of the battery attracts the Cl^- anions. Here, these ions give off their electrons, forming chlorine gas.

\mathrm{2Cl^-\rightarrow Cl_2+2e}

At the electrode connected to the negative terminal, the positive sodium ions gain electrons, forming sodium atoms:

\mathrm{Na^++e\rightarrow Na}

Here, the terminal that draws current into the device is the electrode connected to the positive terminal of the battery.  Therefore, this is the anode. Cl^- ions lose their electrons here, so this is consistent with the idea that oxidation happens at the anode. Sodium forms at the other electrode where Na^+ ions are reduced. Current flows out of the device from this terminal. Therefore, this terminal forms the cathode.

The above two examples should clarify that the terms anode and cathode do not refer to a specific potential but rather how current flows in the setup. For example, the “positive” electrode in the Galvanic cell is its “cathode”, but the “positive” electrode in the case of electrolysis is its “anode”.

Difference Between Anode and Cathode

The names “anode” and “cathode” can be given to a terminal depending on whether current flows into that terminal from outside or whether current flows out of the terminal to the outside. However, because the way currents flow in different situations could be radically different, translating the use of these terms from one situation to another could be confusing. Therefore, it may be necessary to first examine the situation in order to use the terminology properly. If possible, alternative, less ambiguous terms should be used (depending on the situation). We have discussed two particular examples from electrochemistry, but the terms “anode” and “cathode” are used in many other fields as well. A few more examples are mentioned in the summary section below.

Current Flow Direction

Generally, current flows into the anode from the outside. The cathode gives current out of the device. This means that outside the device, electrons flow from the anode to the cathode.

Redox Reaction

Moreover, in devices that rely on redox reactions, oxidation takes place at the anodes, whereas reduction takes place at the cathodes.

In Galvanic Cells and Electrolytic Cells

Meanwhile, in Galvanic cells and electrolytic cells, the cathode attracts cations and oxidises them, but the anode attracts anions and reduces them.

In Electrolysis

The anode forms the positive terminal in electrolysis, while the cathode forms the negative terminal in the Galvanic cell.

In Electron Guns and X-ray Tubes

In electron guns and X-ray tubes, the part that emits electrons into the device forms the cathode, while inside the device, the anode collects the electrons. 

Forward Bias

When normal diodes are connected in forward bias, the anode is the p-side, which is the side connected to the positive side of the battery (it draws current from the cell). Similarly, the cathode forms the n-side.

Notable Exceptions

Although the names of the terminals should be reversed when current flows in reverse bias in a Zener diode, the p-side is still referred to as the “anode” even though, technically, it gives current to the outside. This is a notable exception and highlights why the terms “anode” and “cathode” should be avoided when possible (in this case, it is better to refer to the sides as the p-side and the n-side).

Another source of confusion occurs when battery manufacturers label the negative terminal of a rechargeable battery as the “anode“. When the battery is discharging, the terminology works. However, when the battery is being charged, technically, the terminology should be reversed, as well.


Denker, J. (2004). How to Define Anode and Cathode. Retrieved October 1, 2015, from Welcome to Av8n.com

Image Courtesy:

1. “Galvanic cell diagram” by Ohio standard (Transferred from en.wikipedia; transferred to Commons by User:Burpelson AFB using CommonsHelper) [CC BY-SA 3.0], via Wikimedia Commons

About the Author: Hasa

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