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Batteries - Energy on the Move


Batteries: who doesn't know them, or use them in one way or another? Nowadays, they come in all shapes and sizes, and the electricity they can deliver varies greatly. They power watches, cameras, mobile phones, remote controls, laptops, wireless keyboards and wireless mice, radios, electric toothbrushes, children's toys, torches... and not to forget: cars and car keys. They're so much part of our everyday life that we hardly ever think about them, except when the batteries are flat or we have run out of them altogether and can't take the photo, or listen to Queen on our Discman or, worst case scenario: open the car doors, let alone start the car. But what is a battery, who invented it and when?

A battery is a device usually consisting of two different sorts of metals and one liquid (an acid or a salt solution) as the electrolyte1. There are always two poles on a battery: a negative one, the anode, and a positive one, the cathode. Once the anode corrodes, negatively charged electrons are released from it and flow through the connected consumer load to the cathode (where the electrons combine with the materials in the cathode) thus constituting a useful electric current. Your battery will go flat sooner or later; how long it takes will depend on how much energy your device requires. Even without a connection to a circuit, there is an electrochemical reaction, known as self-discharge. Depending on the type of battery, this can be anything from 1% or more per day, to 5% - 10% per year.

First Experiments

Most people would think that batteries are a relatively recent invention, but apparently, they were invented as early as about 250 BC.

In 1936, in a village near Baghdad, workers found an ancient clay pot, dating back to about 250 BC, which looked very much like a vase. Archaeologists initially thought it was a scroll container, but the German archaeologist Wilhelm König2 identified it as an ancient battery. It contained a cylinder of sheet copper, whose edge was soldered with a tin-lead alloy. The bottom of the cylinder was pleated with a creased copper disk, and sealed with bitumen or asphalt. A corroded iron rod hung down into the centre of the cylinder, and the top of the cylinder was sealed with asphalt as well, keeping the rod in its place at the same time. It is not known what it was used for. Experiments with a replica filled with grape juice as an acid generated a current which would have been strong enough to electroplate one metal onto another, so it may be that this was what the battery was used for. This construction is known as the Baghdad Battery.

In the 18th Century there was a flurry of experimentations with electricity and the first discovery of what was later to become a battery was allegedly made by the Italian professor of anatomy Luigi Galvani (1737 - 1798), who was searching for 'animal' electricity. In 1789, he discovered that frogs' legs moved when they were touched with a metal tool while a nearby static electricity generator produced a spark. He went on to experiment, transfixing frogs' legs between a zinc and a copper wire. The resulting movement of the legs led him to believe that the frogs produced the electricity. However, he was proven wrong by the Italian physician Alessandro Volta (1745 - 1827) only ten years later.

Volta, Volt, Voltage

Volta found out that the connection of two different metals by an electrolyte solution produced the electricity he was searching for. In 1775, Volta had invented an 'Electrophor', a tool which was capable of storing electric energy. He developed it further, hence creating the first plate condenser in 1783. When he read about Galvani's theory, he started his own experiments; one of them was putting a silver coin and some tinfoil on his tongue. The moment the metals touched each other, he noticed a sour tasting liquid building on his tongue. More experiments with different metals led him to the conclusion that an electric current was flowing between the metals. He discovered that the tension between the metals he used varied. The unit of electrical potential, the volt3, is named after him. The first battery Volta created, the Voltaic Pile (1800), consisted of several layers of copper and zinc plates, separated by sulphuric acid-soaked blotting paper4.

Further Developments

All over the world, people started researching electricity, based on Volta's discoveries. The 19th century saw many great inventions as a consequence. Major improvements to the original Voltaic Pile were soon made. Here is an overview of some of the many developments:

  • 1802: Dr William Cruickshank (? - 1810/11), an English chemist, constructed the first battery fit for mass production by soldering copper sheets on one side. He put zinc sheets between the copper layers, placed and fixed this construction in a wooden box and filled it with either a solution of salt electrolytes, or with diluted sulphuric acid. The box was then sealed with cement. This primary cell5 was more powerful than the Voltaic Pile.
  • 1813: Sir Humphry Davy, another English chemist, constructed the biggest Voltaic Pile in the basement of the Royal Society in London. He connected the metals with charcoal electrodes and thus created the very first electric light (this should not be confused with the light bulb, which was invented by Thomas Alva Edison in 1879). His research led to the invention of the field of electrochemistry. He was knighted for his work in 1818. His assistant the physicist Michael Faraday6 (1791 - 1867) was later to be even more renowned than Davy.
  • 1820: André-Marie Ampère (1775 - 1836) discovered that electricity flowed through magnetic fields.
  • 1833: Faraday's Law was announced.
  • 1839: The Welsh Sir William Grove (1811 - 1896) invented the first fuel cell, combining hydrogen and oxygen to produce electricity and water.
  • 1859: the French physicist Gaston Planté invented the first 'secondary cell', or rechargeable battery, based on a lead-acid combination. Because the reaction that produces the electricity is completely reversible when a current at the correct voltage is applied to it, this battery type is used in cars.
  • 1899: Waldemar Jungner, a Swedish engineer and inventor, created the first nickel-cadmium battery, a major improvement to the lead-acid combination. Its high specific energy of up to ten times more than that of the lead-acid accumulator, its high resilience and robustness made it the most popular secondary cell of the last century.
  • 1947: Neumann in France managed to successfully seal the nickel-cadmium batteries. This would lead to mass production of secondary nickel cadmium cells later.

Other battery types were invented, such as the mercury cells which are powerful, very tiny, and very problematic for the environment as they are not rechargeable. The first small alkaline batteries were invented in 1949, and sold in an improved version (in the new AAA size) in 1954. This was the very year when Gerald Pearson, Daryl Chapin, and Calvin Fuller from the USA allegedly invented the first solar battery or solar cell - experiments with solar power had been made a good hundred years earlier, with Antoine César Becquerel observing photovoltaic effects while experimenting with electrodes in an electrolyte solution in 1839. Solar cells are commonly used in calculators, and as collectors on house roofs. They power satellites, too.

Rechargeable Batteries

The 1970s saw the development from unstable nickel-metal-hydride alloys to their commercial use (of an improved, stable version) in the 1990s. It was the same period of time it took to get from the first primary lithium-metal batteries, to the rechargeable lithium-ion batteries we have now. Rechargeable lithium metal batteries proved to be dangerous, which led people to try non-metallic lithium, a lithium-ion battery. Although these still need to be treated with extreme care while charging or discharging, they are very popular with people who fly model airplanes, because of their small size and weight and are most commonly used in laptops. Faulty lithium-ion batteries causing the accumulators to overheat or even explode, led to a temporary banning of certain laptops on airplanes in 2006.

Environmental Issues...

However, this is not the end to the research of batteries and environmentally friendly energy sources. A copper and a zinc wire stuck into a potato produces enough energy to power a digital watch. Renewable energy sources such as wind, water, and solar power are slowly increasing in importance as the ecologic conscience of people grows. During the 1990s, industry started research on an improvement of the fuel cell. Ideally, this will replace batteries and especially fossil fuel to power cars, hence reducing pollution and noise. First results are promising, but there are some problems to be overcome first, for instance hydrogen can't be stored in large quantities and is not easily available, along with a few other drawbacks like an overall efficiency of only about 24 to 32% at the time of writing. Methanol on the other hand is easy to transport and distribute, and has similar properties to gasoline, which makes it a likely candidate for a fuel cell powering a car. Still, the overall efficiency is relatively low, so the development still has a long way to go before any of these will replace the common fuels.

...And a Word of Warning

All common battery types are potentially dangerous and toxic to humans and the environment, especially when ending up in landfill (about 20,000 tonnes/year in the UK alone). Batteries containing either Mercury or NICad or Lead -Acid are classified as 'Hazardous Waste' and recycling laws are afoot. Here are a few things to consider:

  • Reduce the use of batteries if possible. Use rechargeable batteries if you have the choice, or connect the appliance to the mains if possible.
  • Before using new rechargeable batteries for the first time, charge them according to the instructions that come with them. Don't leave them unattended while charging, and don't overcharge them. Make sure to use the correct charger for your type of batteries.
  • Don't try to recharge primary cells! They'll leak into the charger in the best case scenario, or overheat and cause a fire in the worst case.
  • Don't let batteries lie around, especially not when there are small children in the house.
  • Don't ever swallow a battery!
  • Don't leave batteries in the car in summer, and generally keep them out of direct sunlight or close to an open fire - don't even think about throwing them into a fire!7
  • Don't mix old and new batteries as the voltage will be different. The same goes for different brands and/or types of batteries (eg, NiCad and LiIon) as different metals have different reactions and so each reaction has a specific voltage. Don't mix primary and secondary cells.
  • If you don't use a battery-powered item frequently, check the batteries for leakage from time to time, or, even better, remove the batteries from the appliance. A battery that's not in use but yet warm, is dangerous and should be correctly disposed of immediately.
  • Don't dispose of empty batteries in your normal waste; bring them to a designated place if possible. Contact your council or local supermarket about their disposal offers, some producers may offer a recycling scheme for their products.

1 This is known as a 'wet' cell. In a so-called 'dry' cell, the electrolyte is immobilised, such as through gelling or an absorbent paper.
2 Wilhelm König, German archaeologist and director of the National Museum of Iraq where he conducted the first thorough examination of the Baghdad Battery in 1938.
3 One volt (V) is the equivalent of the electric tension between two points of a homogeneous, evenly tempered electric conductor, where a time-invariant current of one Ampàre (A) produces the power of 1 Watt (W) between the two points: 1V = 1 W/A .
4 Or maybe cardboard or tissue, depending on what source you believe.
5 A term for a non-rechargeable battery. Two or more primary cells connected as a source of electric current is what we commonly call a battery.
6 Faraday cages are named after Michael Faraday, who built such a cage in 1836 and explained how it worked. A Faraday cage or Faraday shield is an enclosure or mesh formed by conducting material which blocks out external static electrical fields.
7 However, the current that is produced when you connect the two poles of a battery with some wire wool is enough to inflame said wire wool and can be used to light a campfire.

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Entry Data
Entry ID: A20600849 (Edited)

Edited by:

Date: 09   May   2007

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Referenced Guide Entries
Remote Controls
Mobile Phones
Classic Children's Toys
Rechargeable Batteries
Tips on How to be Planet Friendly
Shower Radios
The Inventions of Thomas Alva Edison
A Beginner's Guide To Digital Cameras
The History of the Digital Watch
Metals, their Properties and Reactivity - a Beginners' Guide
Queen - the Music
Static Electric Discharges and How To Prevent Them Zapping You
Atmospheric Pollution from the Internal Combustion Engine in the Urban Environment
Sir Humphry Davy FRS (1778 - 1829)

Related BBC Pages
Exploding Li-Ion batteries
EU Battery Recycling Laws

Referenced Sites
Batteries Guide
Baghdad Battery
Michael Faraday
Faraday's Law
William Grove
fuel cell
Battery Disposal/UK
European Portable Battery Association
Battery Recycling

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