Wiktor Wise
Electric cells, also known as electrochemical cells, are devices that can generate electrical energy from chemical reactions or use electrical energy to induce chemical reactions. These cells are made up of two half-cells, each consisting of an electrode and an electrolyte. The chemical reactions in the cell involve the electrolyte, electrodes, and/or an external substance. In a full electrochemical cell, one half-cell loses electrons (oxidation) while the other gains electrons (reduction). The type of electrochemical cell that generates electrical energy from chemical reactions is called a galvanic or voltaic cell, while those that induce chemical reactions are called electrolytic cells. The chemicals stored in an electric cell depend on the type of cell and its application. For example, lead-acid batteries in automobiles use the chemical reactions of lead and acid to store electricity, while fuel cells use hydrogen fuel and oxygen.
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What You'll Learn
Electrochemical cells
An electrochemical cell is a device that either generates electrical energy from chemical reactions or induces chemical reactions (electrolysis) by applying external electrical energy. The two modes an electrochemical cell operates in are the spontaneous redox reaction and the electrolytic mode. The former can be used to provide energy to do work, while the latter will not occur unless an external energy source is added to drive it.
A galvanic cell (or voltaic cell) is an electrochemical cell that generates electrical energy from spontaneous redox reactions. It is named after Luigi Galvani and Alessandro Volta. A galvanic cell consists of two half-cells, each consisting of an electrode and an electrolyte. The chemical reactions in the cell involve the electrolyte, electrodes, and/or an external substance. In a full electrochemical cell, species from one half-cell lose electrons (oxidation) to their electrode, while species from the other half-cell gain electrons (reduction) from their electrode.
An electrolytic cell is an electrochemical cell in which applied electrical energy drives a non-spontaneous redox reaction. They are often used to decompose chemical compounds in a process called electrolysis. Electrolysis is a technique that uses a direct electric current (DC). A primary cell produces current by irreversible chemical reactions and is not rechargeable. They are used for their portability, low cost, and short lifetime. A secondary cell, on the other hand, produces current by reversible chemical reactions and is rechargeable.
Fuel cells are electrochemical cells that react hydrogen fuel with oxygen or another oxidizing agent to convert chemical energy to electricity. Fuel cells are different from batteries in that they require a continuous source of fuel and oxygen to sustain the chemical reaction, while batteries contain the necessary chemicals. Fuel cells can produce electricity continuously as long as they are supplied with fuel and oxygen. They are used for primary and backup power in various settings and to power fuel cell vehicles.
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Galvanic cells
A galvanic cell, also known as a voltaic cell, is an electrochemical device that produces electricity through spontaneous redox (reduction-oxidation) reactions. These reactions occur when electrons are transferred between different chemical species, releasing energy that can be harnessed as electrical power.
In its simplest form, a galvanic cell consists of a solid metal (called an electrode) that is submerged in a solution; the solution contains cations (+) of the electrode metal and anions (−) to balance the charge of the cations. The full cell consists of two half-cells, usually connected by a semi-permeable membrane or by a salt bridge that prevents the ions of the more noble metal from plating out at the other electrode.
The electrode where oxidation occurs is termed the anode, while the electrode where reduction takes place is called the cathode. A positive cell potential indicates a spontaneous reaction and that the electrons are flowing from the left to the right—from the anode to the cathode.
The underlying scientific principles of galvanic cells have been identified in much greater detail since their invention, and their function has been optimized to produce efficient batteries capable of generating significant amounts of electricity for extended periods.
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Electrolytic cells
An electrolytic cell is an electrochemical cell that uses an external source of electrical energy to drive a non-spontaneous chemical reaction, a process known as electrolysis. Electrolytic cells are composed of two half-cells, one being a reduction half-cell and the other an oxidation half-cell. The two half-cells are separated by a salt bridge.
The two half-cells consist of separate oxidation and reduction reactions. In the reduction half-cell, the cathode, there is a gain of electrons. In the oxidation half-cell, the anode, there is a loss of electrons. The cathode is the electrode to which cations (positively charged ions) flow within the cell, to be reduced by reacting with electrons (negatively charged) from that electrode. The anode is the electrode to which anions (negatively charged ions) flow within the cell, to be oxidised by depositing electrons on the electrode.
An example of the use of electrolytic cells is the electrolysis of water. Water is a poor conductor of electricity, so an electrolyte is added to the water to provide ions that can flow through the solution, thereby completing the electric circuit. The electrolysis of water produces hydrogen and oxygen. Another example is the electrolysis of sodium chloride, which decomposes the compound into its elements.
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Rechargeable batteries
The chemistry of rechargeable batteries involves the exchange of electrons between two electrodes, the anode (negative electrode) and the cathode (positive electrode). These electrodes are made of different types of metals or other chemical compounds, such as zinc and silver. During charging, the positive active material is oxidized, releasing electrons, while the negative material is reduced, absorbing electrons. These electrons flow between the electrodes, creating an electric current.
There are several types of rechargeable batteries, each with its own unique chemistry and characteristics:
- Lead-acid batteries: Commonly used in automobile engines, they offer high voltage, low cost, and large storage capacity but are heavy and perform poorly in low temperatures.
- Nickel-cadmium (NiCd) batteries: Suited for low-temperature conditions and offer a long shelf life but are more expensive and have lower watt-hour capacity.
- Nickel-zinc batteries: Known for their long lifespan, high voltage, and good energy-to-mass ratio.
- Lithium-ion (Li-ion) batteries: These have a higher output voltage per cell compared to NiCd and alkaline batteries, making them popular in portable electronic devices.
- Lithium-ion polymer (Li-ion polymer) batteries: A variation of Li-ion batteries with a polymer electrolyte.
- Lithium Iron Phosphate (LFP): A type of lithium-ion battery with specific chemistry.
The choice of rechargeable battery depends on the specific requirements of the application, such as long-term use, storage time, remote activation, or harsh weather conditions. While rechargeable batteries have a higher initial cost, they offer a lower total cost of ownership and environmental impact due to their reusability.
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Non-rechargeable batteries
A battery is a galvanic cell or a series of galvanic cells that contain all the reactants required to produce electricity. A primary battery or primary cell is a single-use galvanic cell that is designed to be used once and discarded. It is not rechargeable, and the chemical reactions occurring in the cell are not reversible. As the battery is used, the chemical reactions taking place inside the battery consume the chemicals that generate power. Once these chemicals are exhausted, the battery stops producing electricity.
Primary cells are made in a range of standard sizes to power small household appliances such as flashlights and portable radios. They are used for their portability, low cost, and short lifetime. However, they are considered wasteful and environmentally unfriendly due to the toxic heavy metals and strong acids they contain.
The anode and cathode are the two electrodes in a battery. The anode is the negative electrode, while the cathode is the positive electrode. The anode is where chemical oxidation occurs, as it donates electrons that flow out into the external circuit. The cathode, on the other hand, is where chemical reduction occurs, as it accepts electrons from the circuit.
There are various types of primary batteries, such as the Leclanché cell, zinc-carbon cell, Bunsen cell, and Grove cell. Each of these cells uses different chemicals to facilitate the necessary electrochemical reactions. For example, the Leclanché cell and zinc-carbon cell use manganese dioxide, while the Bunsen cell and Grove cell use nitric acid.
Another type of non-rechargeable battery is the lithium-iodine battery, which consists of two cells separated by a nickel metal mesh that collects charge from the anode. These batteries have a high internal resistance due to the solid electrolyte, limiting the amount of current that can be drawn. However, they are long-lasting and reliable, making them suitable for applications where frequent replacement is challenging or undesirable, such as cardiac pacemakers, medical implants, and computers for memory protection.
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Frequently asked questions
An electric cell is a device that can generate electrical energy from chemical reactions or use electrical energy to cause chemical reactions.
There are two types of electric cells: galvanic cells (or voltaic cells) and electrolytic cells.
Galvanic cells are electric cells that generate electrical energy from chemical reactions. They are named after Luigi Galvani and Alessandro Volta.
Electrolytic cells are a type of electric cell in which electrical energy is converted into chemical energy. They are often used to decompose chemical compounds in a process called electrolysis.
