Molly Ayala
Batteries are a source of electric power that can be used to power electrical devices. They are made up of one or more electrochemical cells that convert chemical energy into electricity. The system underpinning a battery is called an electrochemical cell, which consists of two electrodes separated by a chemical substance called an electrolyte. The electrolyte is usually in the form of a liquid or paste. When a battery is connected to an external electric load, electrons flow through the circuit and reach the positive terminal, causing a redox reaction and producing electricity. Batteries can be classified as primary cells (non-rechargeable) or secondary cells (rechargeable). The oldest form of rechargeable battery is the lead-acid battery, widely used in automotive and boating applications.
| Characteristics | Values |
|---|---|
| Definition | A source of electric power consisting of one or more electrochemical cells with external connections for powering electrical devices. |
| Function | Stores chemical energy and converts it to electricity. |
| Parts | Cathode (positive terminal), Anode (negative terminal), Electrolyte (chemical material separating the cathode and anode) |
| Types | Wet cell battery, Dry cell battery, Primary cells (non-rechargeable), Secondary cells (rechargeable), Lead-acid battery, Nickel-cadmium battery, Lithium-ion battery |
| Uses | Commonly used in portable devices with low current drain, intermittently used devices, or devices used away from alternative power sources. |
| Limitations | Prone to leakage, chemical reactions may not be easily reversible, high-rate cycling can lead to reduced efficiency, self-discharge issues in rechargeable batteries. |
| Development | Research aims to improve materials for anodes, cathodes, and electrolytes, enhance energy storage, safety, charging speed, and capacity. |
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What You'll Learn
Wet cell batteries
A battery is a device that stores chemical energy and converts it to electricity through a process known as electrochemistry. This process occurs in a component of the battery called an electrochemical cell. Each electrochemical cell consists of two electrodes separated by a chemical substance called an electrolyte. The electrolyte facilitates a chemical reaction between the two electrodes, which frees up electrons in one electrode, causing it to develop a negative charge, while the other electrode develops a positive charge. The freed electrons flow from the negative end of the battery to the positive end through a wire or circuit, generating electricity.
The process of generating electricity in a wet cell battery is similar to that of a standard battery. However, the liquid electrolyte in a wet cell battery is typically unsealed, meaning that the battery must be kept upright to avoid leakage. Wet cell batteries are also known as lead-acid batteries because both electrodes are lead plates suspended in a tank of sulphuric acid, which acts as the electrolyte.
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Dry cell batteries
A battery is a device that stores chemical energy and converts it to electricity. This process is known as electrochemistry, and the system that underpins a battery is called an electrochemical cell. An electric battery consists of one or more electrochemical cells with external connections for powering electrical devices.
A dry cell is a type of electric battery commonly used for portable electrical devices. Unlike wet cell batteries, which have a liquid electrolyte, dry cells use an electrolyte in the form of a paste, making them less susceptible to leakage. The dry cell was developed in 1886 by the German scientist Carl Gassner, after the development of wet zinc-carbon batteries by Georges Leclanché in 1866. A type of dry cell was also developed by the Japanese inventor Sakizō Yai in 1887.
The first mass-produced model was the Columbia dry cell, first marketed by the National Carbon Company in 1896. The NCC improved Gassner's model by replacing the plaster of Paris with coiled cardboard, an innovation that leaves more space for the cathode and makes the battery easier to assemble. It was the first convenient battery for the masses and made portable electrical devices practical. The zinc-carbon cell (as it came to be known) is still manufactured today.
A standard dry cell comprises a zinc anode, usually in the form of a cylindrical pot, with a carbon cathode in the form of a central rod. The electrolyte is ammonium chloride in the form of a paste next to the zinc anode. The remaining space between the electrolyte and carbon cathode is taken up by a second paste consisting of ammonium chloride and manganese dioxide, the latter acting as a depolariser.
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Rechargeable batteries
Batteries are devices that store chemical energy and convert it into electricity. This process is known as electrochemistry, and the system that underpins a battery is called an electrochemical cell. A battery can be made up of one or several electrochemical cells, each consisting of two electrodes separated by an electrolyte.
The oldest form of rechargeable battery is the lead-acid battery, widely used in automotive and boating applications. This type of battery contains liquid electrolyte in an unsealed container, requiring the battery to be kept upright and the area well-ventilated to ensure safe dispersal of the hydrogen gas produced during overcharging. Lead-acid batteries are relatively heavy for the amount of electrical energy they supply, but their low manufacturing cost and high surge current levels make them common where capacity is more important than weight and handling issues.
Another type of rechargeable battery is the lithium-ion battery, which does not suffer from the "memory effect" that plagues some other battery types, such as nickel-based batteries. The "memory effect" occurs when rechargeable batteries are recharged without being sufficiently discharged first, causing them to 'remember' where they were in earlier discharge cycles and fail to recharge properly.
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Electrochemical cells
An electric battery is a source of electric power that consists of one or more electrochemical cells with external connections for powering electrical devices. Electrochemical cells are devices that convert chemical energy into electrical energy or electrical energy into chemical energy. They are the system underpinning batteries.
There are two primary types of electrochemical cells: galvanic cells and electrolytic cells. A galvanic cell, also known as a voltaic cell, generates electrical energy from spontaneous redox reactions. Alessandro Volta developed the first voltaic cell in 1800, consisting of alternating zinc and silver disks separated by cardboard soaked in brine. A galvanic cell can be used as a battery, and many commercially important batteries, such as the lead-acid battery, are made up of galvanic cells.
Electrolytic cells, on the other hand, induce chemical reactions by applying external electrical energy. They are used in the electrorefining of many non-ferrous metals, such as lead, zinc, aluminium, and copper. Electrolytic cells are also used in the production of high-purity metals. A battery can be made up of one or several electrochemical cells. Each electrochemical cell consists of two half-cells, each with an electrode dipped in an electrolyte. The two half-cells are connected by a salt bridge, which allows for ionic contact without the solutions mixing and causing unwanted side reactions.
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. The oxidation occurs at the anode, and the reduction occurs at the cathode. The anode is negatively charged, and the cathode is positively charged. When a battery is connected to an external electric load, the negatively charged electrons flow through the circuit and reach the positive terminal, causing a redox reaction and converting higher energy reactants to lower energy products. The free-energy difference is delivered to the external circuit as electrical energy.
Wet cell batteries have a liquid electrolyte and are commonly used as a learning tool for electrochemistry. They can be built with common laboratory supplies and are useful for understanding corrosion. Primary cells, or single-use batteries, are an example of a type of wet cell. Secondary cells, or rechargeable batteries, can be recharged by reversing the chemical reaction.
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Electrochemical reactions
A battery is a device that produces electric currents through electrochemical reactions, which are chemical reactions that create electricity. These reactions take place in a battery's electrodes and involve the transfer of electrons between different types of ions. This movement of electrons creates an electric current, which can then be used to power electrical devices.
In a battery, there are two types of electrodes: the anode and the cathode. The anode is the negative electrode, while the cathode is the positive one. Each electrode is made of a different material, which allows for the specific type of electrochemical reaction needed to generate electricity. The electrodes are placed in an electrolyte, which is usually a liquid or gel-like substance that contains ions.
When a battery is connected to a circuit, a reaction occurs at the interface between the electrode and the electrolyte. This reaction involves the exchange of electrons between the electrode and the ions in the electrolyte. For example, at the anode, the electrode may donate electrons to the ions in the electrolyte, while at the cathode, it may accept electrons from the ions. This movement of electrons creates an electric current as the electrons flow from the anode to the cathode through the circuit.
The specific electrochemical reactions that occur depend on the type of battery and the materials used. For example, in a common alkaline battery, the anode is typically made of zinc, while the cathode is made of manganese dioxide. The electrolyte is usually a paste-like substance containing potassium hydroxide. During discharge, the zinc at the anode oxidizes, releasing electrons that flow through the circuit. At the cathode, the electrons combine with manganese dioxide and hydroxyl ions from the electrolyte to form manganese oxide and water. The overall reaction results in the flow of electrons, creating an electric current.
It is important to note that batteries are not a constant source of electricity; the electrochemical reactions that produce electricity are limited by the amount of active material in the battery. Once these materials are depleted, the battery is considered discharged, and it must be replaced or recharged, depending on its design.
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Frequently asked questions
A battery is a device that stores chemical energy and converts it to electricity.
Batteries use chemistry, in the form of chemical potential, to store energy. To accept and release energy, a battery is coupled to an external circuit. Electrons move through the circuit, while ions move through the electrolyte.
An electrochemical cell is an arrangement of electrodes and ionic solutions in which a redox reaction is used to make electricity. Each electrochemical cell consists of two electrodes separated by an electrolyte.
A wet cell battery has a liquid electrolyte. It was the first known type of electrochemical cell to generate electricity. However, they are prone to leaking, so most modern applications use dry cells.
A rechargeable battery can be charged by passing a current through it in the opposite direction. The chemical reactions are reversible, and the battery can be recharged without losing its functionality.
