Introduction to Battery, Electric
Battery, Electric, a device that produces electric current without the use of moving parts. Strictly speaking, a battery consists of two or more electric cells connected electrically to provide a single source of electricity. However, in common usage, the term battery is also applied to single, self-contained cells such as those used in flashlights and electronic watches.
Batteries are a source of direct current (DC). They are widely used to supply electricity for equipment ranging in size from hearing aids to automobiles, and to provide power for portable equipment and equipment at remote locations. Batteries are generally impractical, however, for large-scale uses, such as lighting streets and houses.
Cells that provide electricity by transforming chemical energy into electrical energy are called galvanic, or voltaic, cells. There are two major types: primary cells and secondary cells. A primary cell is one that requires replacement once the materials it contains are used by the chemical reactions that take place in the cell. With a secondary cell, the chemical reactions can be readily reversed to restore the materials used up in the cell. Secondary cells form the basis of storage batteries. A third type, called a fuel cell, uses outside materials that are continuously supplied to the cell.
Cells that convert the energy of visible light into electricity are called photovoltaic, or solar, cells. Thermoelectric cells produce electricity from heat energy; nuclear batteries produce electricity from the radiation emitted by radioactive substances.
The Primary Cell
All galvanic cells consist essentially of a negative electrode and a positive electrode in an electrolytic solution. The solution contains ions (electrically charged atoms or groups of atoms) that promote chemical changes in the electrode materials. When a cell is connected to an electrical circuit, electrons flow from the negative electrode through the circuit into the positive electrode. The flow of electrons, or electric current, is produced by a difference in potential between the electrodes. The difference in potential is measured in volts and is generally referred to as voltage. It is caused by an electromotive force (emf) resulting from the relative strength with which atoms of each electrode attract electrons. The atoms of the positive electrode exert a stronger attraction for electrons than do the atoms of the negative electrode. When a current is established between the two electrodes, chemical reactions at each electrode proceed spontaneously, supplying free electrons to the circuit from the negative electrode and, at the same time, taking up free electrons from the circuit at the positive electrode.
In chemical terms, the type of reaction that occurs at the negative electrode is called oxidation and the type of reaction that occurs at the positive electrode is called reduction. Together, they constitute an oxidation-reduction, or redox, reaction. The oxidized material loses electrons and the material that is reduced gains them. These processes can best be illustrated by using the zinc-mercury cell as an example. In this cell, zinc atoms make up the negative electrode and mercuric oxide molecules the positive electrode. When the two electrodes are connected electrically, the zinc is oxidized and the mercuric oxide reduced.
A simplified description of the cell's operation begins with the oxidation of an atom of zinc, which loses its two outer electrons. The resulting positive zinc ion combines with a negative oxygen ion in the electrolyte. The two free electrons left in the negative electrode enter the external circuit and pass to the positive electrode. There they combine with a molecule of mercuric oxide, reducing it. The mercury breaks away from the oxygen as a neutral metal atom and the oxygen enters the electrolyte as a negative oxygen ion. The overall chemical reaction of the cell during discharge can be expressed as Zn+HgO—ZnO+Hg.
The reactions in a cell continue until the materials in the cell are used up. In general, the larger a particular type of cell is, the more electrical energy it can deliver. However, such effects as the accumulation of waste products from the chemical reactions can decrease a cell's performance. Commercial cells are designed to lessen these effects, which are known collectively as polarization.
Most commercial primary cells use zinc as the negative electrode, a metallic oxide as the positive electrode, and an acidic or alkaline solution formed by water and an electrolyte as the electrolytic solution. Most primary cells today are dry cells—the electrolytic solution is in the form of a moist paste or is held in absorbent materials so that it is not free to flow.
Graphite or carbon black is often mixed with the metallic oxide to improve the conductivity of the positive electrode. The zinc is usually amalgamated—that is, alloyed with mercury. The amalgamation helps prevent any decomposition of water and the associated formation of hydrogen gas. The accumulation of hydrogen gas around the negative electrode is a chief cause of polarization. Between the electrodes there is a porous barrier of paper or other material, called the separator. The separator allows ions in the electrolyte to pass through it but keeps material of one electrode from reacting directly with the material of the other electrode.
Typical voltages for fresh commercial primary cells range from 1.0 to 1.5 volts. Batteries with higher voltages generally contain several cells connected in series—that is, one after the other in a circuit. A 9-volt battery, for example, will contain six cells of 1.5 volts connected in series. The voltage of a cell tends to decrease with amount of use and the strength of current drawn from the cell. It can also be affected by temperature. Over time, the materials in a cell slowly deteriorate, even if the cell is not used. The time during which an unused cell can still perform adequately is referred to as the cell's shelf life.
Primary cells are manufactured in a large variety of shapes and sizes. For consumer use, common shapes and sizes include cylindrical D (flashlight) and AA (penlight) cells and smaller button-shaped cells of various sizes. A discussion of typical examples of major kinds of primary cells follows.
was the original dry cell and is the most common type of primary battery used today. In the typical carbon-zinc cell, a small can made of zinc serves as both the cell's container and the negative electrode. The inside of the zinc can is lined with the separator and filled with a mixture of manganese dioxide, which serves as the positive electrode. The separator and manganese dioxide are saturated with the electrolytic solution—ammonium chloride, zinc chloride, and water. This solution is slightly acidic. A carbon rod is placed in the center of the cell within the manganese dioxide to improve the electrical conductivity of the cell. The rod makes electrical contact with a metal plate that is insulated from the zinc can and forms the positive terminal. The voltage of a carbon-zinc cell tends to drop as the cell is being used and to recover between periods of use.
Cell is very similar to the ordinary carbon-zinc cell. The major difference is that its electrolyte consists chiefly of zinc chloride.
Cell contains electrode materials similar to those used in the carbon-zinc cell. Unlike the carbon-zinc cell, it uses an alkaline electrolyte—potassium hydroxide. In a typical alkaline cell, the zinc is in the form of a fine powder and lies in the center of the cell surrounded by a layer of manganese dioxide. The separator lies between the materials. The entire cell is encased in a steel container.
Cell provides a relatively large amount of energy per unit volume. For this reason small cells, such as button cells, are commonly mercury cells. In mercury button cells, the positive electrode, consisting of mercuric oxide, forms a layer at the bottom of the cell. The negative electrode, consisting of powdered zinc, forms a layer at the top. The electrode materials and the separator are infused with an alkaline electrolyte.
Cell is ordinarily in the form of a button cell that is very similar to the mercury button cell. However, the positive electrode is composed of silver oxide instead of mercuric oxide.
Lithium cells produce voltages higher than other primary cells, but they are relatively difficult and expensive to manufacture because lithium is very reactive chemically. The electrolyte usually consists of organic salts in a nonaqueous solution.
All lithium cells contain a negative electrode composed of lithium, but the composition of the positive electrode varies with different types. The most common lithium cells used for consumer products have a positive electrode composed of manganese dioxide.
once widely used for telegraphic equipment, is historically important but is little used today. In this cell, the positive electrode is made of copper, the negative electrode of zinc. A separate electrolyte is used for each electrode: copper sulfate for the copper electrode and zinc sulfate for the zinc electrode. The two electrolytes are separated by a porous barrier.
is not used as a source of power, but to provide a standard voltage for calibrating electrical instruments. A Weston Standard Cell uses mercury as the positive electrode and cadmium as the negative electrode with an electrolyte of cadmium sulfate. It produces 1.018636 volts at 68° F. (20° C.).
The Storage Battery
A storage battery is composed of one or more secondary, or storage, cells. This type of cell is rechargeable—that is, the chemical reactions that produce electricity in the cell can be readily reversed to restore the materials in the cell to their original condition. (The chemical reactions in a primary cell either are difficult to reverse or cause irreversible changes in the cell's internal structure.) A secondary cell is recharged by forcing an electric current through the cell in a direction opposite to that of the current produced by the cell itself. Devices called rechargers make it possible to recharge some secondary cells with household electrical current.
For some uses, secondary cells are recharged frequently to keep the battery at full charge. For others, the battery is used essentially like a primary battery and is allowed to run down" before it is recharged. Over time, a storage battery will fail because of deterioration of its parts or decomposition of its materials. Two major kinds of storage batteries are the lead-acid and nickel-cadmium batteries.
is used in most automobiles, trucks, and other vehicles for the starter motor, ignition system, and accessory electrical equipment. Each secondary cell produces approximately 2 volts, and the total voltage of the battery (6 or 12 volts in the case of automobiles) equals the number of cells multiplied by two.
The most common lead-acid cell consists of two types of plates immersed in a solution of sulfuric acid and water. Perforated separators made of fiber glass, wood, or rubber help insulate the plates from each other. The negative plates are made of spongy (porous) lead. The positive plates are a lead grid filled with lead dioxide. As the battery discharges (gives off current), the surfaces of the lead dioxide and spongy lead plates gradually become lead sulfate and the sulfuric acid becomes increasingly diluted with water formed during the process. As these chemical reactions occur, the battery becomes progressively weaker.
An automobile battery is recharged by an electric current produced by an alternator or generator. A device called a voltage regulator controls the charging process and prevents overcharging. Overcharging causes the plates in the battery to deteriorate.
The state of charge of some lead-acid batteries can be checked by testing each cell with either a hydrometer or a voltmeter. The hydrometer measures the specific gravity of the sulfuric acid in a cell. The specific gravity indicates a cell's state of charge. A voltmeter indicates the state of charge of a cell by measuring the cell's voltage. The failure of one or more cells to reach an adequate state of charge may be an indication that the battery needs replacing.
Some batteries lose water in the electrolytic solution through evaporation or decomposition and have removable caps for their individual cells so that water can be added periodically. Calcium-lead batteries, commonly known as maintenance-free batteries, do not require additional water; the cells usually do not have caps but are permanently sealed.
has a positive electrode composed of nickelic hydroxide, a negative electrode composed of cadmium, and an electrolyte of potassium hydroxide. Nickel-cadmium cells are available in many of the same sizes and shapes as primary cells. In one flashlight nickel-cadmium cell, the positive and negative electrodes are long plates wound in a spiral within the metal cylinder. Wound with the plates is a separator that lies between the plates.
The Fuel Cell
A fuel cell converts the chemical energy of a fuel directly into electrical energy. A typical cell contains two metal screens separated by a layer of material saturated with an alkaline or acid electrolyte. Hydrogen is fed to one side of the electrolyte layer, oxygen to the other side. As the gases react with the electrolyte, a voltage is produced between the screens. The hydrogen and oxygen used by the fuel cell can be supplied to the cell for continuous operation.
Light generates an electric current when it falls on certain substances and releases electrons from their atoms. The electrons are then available to flow through a circuit.
A typical photovoltaic cell is the silicon solar cell. Each silicon cell is formed from a wafer of pure silicon to which selected impurities have been added. The surface that is exposed to light is treated with boron or a similar element. The rest of the silicon is treated with an element such as arsenic. When light strikes the boron-treated surface, it releases electrons which then tend to move into the arsenic-treated layer. The surface is the positive electrode; the arsenic-treated layer is the negative electrode. When the two electrodes are connected by a wire, current flows from the arsenic-treated layer through the wire to the boron-treated surface.
Solar batteries power most artificial satellites. On earth they are used to power communications equipment, navigational buoys, and pumping stations, particularly at remote locations. Because solar batteries operate only when the sun shines, they are usually used with storage batteries if continuous power is needed.
A thermoelectric cell produces an electric current directly from heat through differences in temperature. A simple thermoelectric cell consists of two conductors made of different kinds of metal, joined together in two places (the junctions). One of the junctions is then heated (or cooled) with respect to the other. As the temperatures at the two junctions begin to differ, a current starts to flow through the circuit. The strength of the current depends on the kinds of metals used as conductors, and on how great a difference there is in the temperatures of the two junctions.
The source of energy in nuclear batteries is radiation from radioactive atoms. Several methods are used to convert nuclear energy into electrical energy in batteries.
Beta particles are electrons emitted from the nuclei of atoms. The emitter in a beta-emission battery is a source of pure beta particles, such as hydrogen 3, krypton 85, or strontium 90. As the electrons leave the emitter, they pass through a vacuum or a relatively unreactive material, such as plastic. Some of the electrons strike a collector made of carbon, and enter a circuit. Direct beta-emission batteries produce extremely high voltages (up to 500 volts or more) with extremely low current. They are used to charge capacitors.
use radioactivity to produce light, which in turn produces electric currents in photovoltaic cells. In one type, promethium 147, a radioactive byproduct of nuclear fission, is mixed with a phosphor and encased in transparent plastic. Electrons given off by the promethium cause the phosphor to glow, just as electrons in a television picture tube cause phosphors on the screen to glow. The light strikes a photovoltaic cell, which transforms the light into electrical current.
The first battery was made in about 1800 by Count Alessandro Volta, an Italian scientist. It consisted of a stack of alternating zinc and silver discs with a brine-soaked separating material after every second disc. The voltaic pile, as the battery came to be known, has the disadvantage that its voltage quickly drops because of waste products that accumulate near the discs during discharge.
A cell that overcame this problem was developed by an English scientist, John F. Daniell, in 1836. An improved Daniell cell was a reliable source of electrical energy for telegraphy through the end of the 19th century.
The first storage battery was built by Gaston Plant in 1859. The battery, called an accumulator, used lead plates immersed in a solution of sulfuric acid, basically the same system as that used in the lead-acid batteries of today. Another storage battery system, using plates of iron and nickel in an alkaline solution, was invented by Thomas A. Edison in 1901.
The carbon-zinc cell was developed by Georges Leclanche, a French chemist, in the late 1860's. The original cell was a wet cell—one that used a free-flowing electrolytic solution. The carbon-zinc dry cell, in which the electrolytic solution is confined to a semisolid material, was developed in the 1880's.
In the mid-1900's, several types of cells were developed and improved. The mercury cell was developed during World War II. In 1954 the first practical solar battery was demonstrated. The first nuclear batteries were made in the late 1950's.
During the 1970's, a growing number of battery-powered electronic items for consumer use stimulated the production of numerous types of cells in many shapes and sizes. By the early 1980's lithium cells had been developed for consumer use.