Electric battery

Battery
	Various cells and batteries (top left to bottom right): two AA, one D, one handheld ham radio battery, two 9-volt (PP3), two AAA, one C, one camcorder battery, one cordless phone battery
Type	Power source
Working principle‍	Electrochemical reactions, Electromotive force
First production	1800s
Electronic symbol
	; The symbol for a battery in a circuit diagram. It originated as a schematic drawing of the earliest type of battery, a voltaic pile.

An electric battery is a source of electric power consisting of one or more electrochemical cells with external connections^[1] for powering electrical devices. When a battery is supplying power, its positive terminal is the cathode and its negative terminal is the anode.^[2] The terminal marked negative is the source of electrons. When a battery is connected to an external electric load, those negatively charged electrons flow through the circuit and reach to the positive terminal, thus cause a redox reaction by attracting positively charged ions, cations. Thus converts high-energy reactants to lower-energy products, and the free-energy difference is delivered to the external circuit as electrical energy. Historically the term "battery" specifically referred to a device composed of multiple cells; however, the usage has evolved to include devices composed of a single cell.^[3]

Primary (single-use or "disposable") batteries are used once and discarded, as the electrode materials are irreversibly changed during discharge; a common example is the alkaline battery used for flashlights and a multitude of portable electronic devices. Secondary (rechargeable) batteries can be discharged and recharged multiple times using an applied electric current; the original composition of the electrodes can be restored by reverse current. Examples include the lead–acid batteries used in vehicles and lithium-ion batteries used for portable electronics such as laptops and mobile phones.

Batteries come in many shapes and sizes, from miniature cells used to power hearing aids and wristwatches to, at the largest extreme, huge battery banks the size of rooms that provide standby or emergency power for telephone exchanges and computer data centers. Batteries have much lower specific energy (energy per unit mass) than common fuels such as gasoline. In automobiles, this is somewhat offset by the higher efficiency of electric motors in converting electrical energy to mechanical work, compared to combustion engines.

^ Crompton, T. R. (20 March 2000). Battery Reference Book (third ed.). Newnes. p. Glossary 3. ISBN 978-0-08-049995-6. Retrieved 18 March 2016.
^ Pauling, Linus (1988). "15: Oxidation-Reduction Reactions; Electrolysis". General Chemistry. New York: Dover Publications, Inc. p. 539. ISBN 978-0-486-65622-9.
^ Pistoia, Gianfranco (25 January 2005). Batteries for Portable Devices. Elsevier. p. 1. ISBN 978-0-08-045556-3. Retrieved 18 March 2016.

[1] Crompton, T. R. (20 March 2000). Battery Reference Book (third ed.). Newnes. p. Glossary 3. ISBN 978-0-08-049995-6. Retrieved 18 March 2016.

[Pauling1988-2] Pauling, Linus (1988). "15: Oxidation-Reduction Reactions; Electrolysis". General Chemistry. New York: Dover Publications, Inc. p. 539. ISBN 978-0-486-65622-9.

[3] Pistoia, Gianfranco (25 January 2005). Batteries for Portable Devices. Elsevier. p. 1. ISBN 978-0-08-045556-3. Retrieved 18 March 2016.

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