Half-Cell
Definition and meaning of Half-Cell in chemistry.
A half-cell is an electrode sitting in a solution of ions, making up one half of a complete electrochemical cell. In this single compartment, either a chemical oxidation or a chemical reduction reaction takes place.
In more detail
A half-cell by itself cannot do any useful electrical work. The electrons have nowhere to go and no full circuit to travel. To make a working battery, you must connect two different half-cells together.
One half-cell acts as the anode, where molecules lose electrons through oxidation. The other half-cell acts as the cathode, where different molecules gain those electrons through reduction. You connect the two metal electrodes with a wire to let the electrons flow.
You also connect the two liquids with a salt bridge. The salt bridge lets ions move back and forth to keep the electrical charge balanced. Chemists assign a specific voltage number to every possible half-cell.
This number is called the standard reduction potential. We measure this value by comparing the half-cell to a standard hydrogen electrode. The hydrogen electrode is officially assigned a voltage of exactly zero.
A common student mistake is trying to measure a half-cell voltage all alone. You always need two half-cells connected to measure any voltage at all. By knowing the potential of each separate half-cell, you can predict the total voltage of a newly built battery.
Key facts
| Field | Physical Chemistry |
|---|---|
| Anode function | The half-cell where oxidation happens (loses electrons) |
| Cathode function | The half-cell where reduction happens (gains electrons) |
| Reference baseline | Standard hydrogen electrode (SHE) is exactly 0 V |
| Key connection piece | Salt bridge keeps charges balanced |
A classic Daniell cell uses two common half-cells to make a battery. The first half-cell contains a zinc metal strip sitting in a zinc sulfate solution. The second half-cell holds a copper metal strip sitting in a copper sulfate solution. The zinc side loses electrons, acting as the anode. The copper side gains electrons, acting as the cathode. The zinc half-cell has a potential of -0.76 volts. The copper half-cell has a potential of +0.34 volts. Connecting these two specific half-cells produces a total battery voltage of 1.10 volts.
Frequently asked questions
Can a single half-cell generate an electrical current?
No. A single half-cell cannot push electrons on its own. It needs a partner half-cell and a completed circuit for electrons to flow.
What is the purpose of the salt bridge between half-cells?
The salt bridge allows positive and negative ions to move between the solutions. This prevents charge buildup and keeps the battery running safely.
How do chemists measure the voltage of just one half-cell?
You cannot measure it alone. Chemists measure every half-cell against a standard hydrogen half-cell, which acts as the official zero point.