Batteries

Extracted Attributes

• Mechanism

  Chemical reactions involve the flow of electrons from one electrode to another through an external circuit, balanced by the flow of charged ions through an electrolyte solution.

• Components

  Two electrical terminals (cathode and anode) separated by an electrolyte.

• Definition

  A device that stores chemical energy and converts it to electrical energy.

• Scientific Field

  Electrochemistry

• Types (Secondary/Rechargeable)

  Lead-acid, Lithium-ion, Nickel-metal hydride

• Types (Primary/Non-rechargeable)

  Alkaline, Lithium metal, Zinc-carbon

Timeline

• Batteries were invented. (Source: web_search_results)

  1800

• Scientists are continuously exploring and improving complex chemical processes to develop new generations of highly efficient electrical energy storage systems. (Source: web_search_results)

  Ongoing

• At the All-In Summit, U.S. Secretary of Energy Chris Wright expressed skepticism towards batteries and solar energy, labeling them 'parasites' on the electricity grid. In contrast, Chamath Palihapitiya advocated for batteries as part of a distributed utility model. (Source: related_documents)

  2025

Web Search Results

• How a battery works - Curious - Australian Academy of Science

  A battery is a device that stores chemical energy and converts it to electrical energy. The chemical reactions in a battery involve the flow of electrons from one material (electrode) to another, through an external circuit. The flow of electrons provides an electric current that can be used to do work. To balance the flow of electrons, charged ions also flow through an electrolyte solution that is in contact with both electrodes. [...] A battery is a device that stores chemical energy, and converts it to electricity. This 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 (like in Volta's original pile) electrochemical cells. Each electrochemical cell consists of two electrodes separated by an electrolyte. [...] | Ni2+(aq) + 2e− Ni(s) | –0.257 | | 2SO42−(aq) + 4H+(aq) + 2e− S2O62−(aq) + 2H2O(l) | –0.25 | | Sn2+(aq) + 2e− Sn(s) | −0.14 | | 2H+(aq) + 2e− H2(g) | 0 | | Sn4+(aq) + 2e− Sn2+(aq) | 0.154 | | Cu2+(aq) + e− Cu+(aq) | 0.159 | | AgCl(s) + e− Ag(s) + Cl−(aq) | 0.2223 | | Cu2+(aq) + 2e− Cu(s) | 0.3419 | | O2(g) + 2H2O(l) + 4e− 4OH−(aq) | 0.401 | | H2SO3(aq) + 4H+(aq) + 4e− S(s) + 3H2O(l) | 0.45 | | I2(s) + 2e− 2I−(aq) | 0.5355 |

• Types of Batteries | PNNL

  While there are several types of batteries, at its essence a battery is a device that converts chemical energy into electric energy. This electrochemistry happens through the flow of electrons from one material (electrode) to another, through an external circuit. The flow of electrons provides an electric current that can be used to do work. To balance the flow of electrons, charged ions (atoms or molecules with an electric charge) also flow through an electrolyte solution that is in contact [...] Batteries consist of two electrical terminals called the cathode and the anode, separated by a chemical material called an electrolyte. To accept and release energy, a battery is coupled to an external circuit. Electrons move through the circuit, while ions simultaneously move through the electrolyte. Several materials can be used as battery electrodes. Different materials have different electrochemical properties, so they produce different results when assembled in a battery cell. [...] Batteries were invented in 1800, but their complex chemical processes are still being explored and improved. Scientists are using new tools to better understand the electrical and chemical processes in batteries to produce a new generation of highly efficient, electrical energy storage systems. While we may be more familiar with the rechargeable batteries we use every day in personal electronics, vehicles, and power tools, batteries are also essential for large-scale electricity storage to

• Electric battery - Wikipedia

  A battery consists of some number of voltaic cells. Each cell consists of two half-cells connected in series by a conductive electrolyte containing metal \_cations\_. One half-cell includes electrolyte and the negative electrode, the electrode to which anions (negatively charged ions) migrate; the other half-cell includes electrolyte and the positive electrode, to which cations (positively charged ions) migrate. Cations are reduced (electrons are added) at the cathode, while metal atoms are [...] Batteries convert chemical energy directly to electrical energy. In many cases, the electrical energy released is the difference in the cohesive( or bond energies of the metals, oxides, or molecules undergoing the electrochemical reaction. For instance, energy can be stored in Zn or Li, which are high-energy metals because they are not stabilized by d-electron bonding, unlike transition metals. Batteries are designed so that the energetically favorable redox reaction can occur only when [...] \ \_Primary\_ batteries are designed to be used until exhausted of energy then discarded. Their chemical reactions are generally not reversible, so they cannot be recharged. When the supply of reactants in the battery is exhausted, the battery stops producing current and is useless.(

• List of battery types

  | Primary cell (non-rechargeable) | Alkaline Aluminium–air Bunsen Chromic acid Clark Daniell Dry Edison–Lalande Grove Leclanché Lithium metal Lithium organic Lithium–air Mercury Metal–air electrochemical Nickel oxyhydroxide Silicon–air Silver oxide Weston Zamboni Zinc–air Zinc–carbon | [...] | Secondary cell (rechargeable) | Automotive Lead–acid + gel–VRLA Lithium–air Lithium ion + Dual carbon + Lithium–iron–phosphate + Lithium–polymer + Lithium–sulfur + Lithium–titanate Metal–air Molten salt Nanopore Nanowire Nickel–cadmium Nickel–hydrogen Nickel–iron Nickel–lithium Nickel–metal hydride Nickel–zinc Polysulfide–bromide Potassium ion Rechargeable alkaline Silver–cadmium Silver–zinc Sodium ion Sodium–sulfur Solid state Vanadium redox Zinc–bromine [...] Nickel–iron battery (NiFe battery) Nickel–lithium battery Nickel–metal hydride battery + Low self-discharge NiMH battery Nickel–zinc battery Organic radical battery Polymer-based battery Polysulfide–bromide battery Rechargeable alkaline battery Rechargeable fuel battery Sand battery "Sand battery (electrochemical)") Silver–zinc battery Silver–calcium battery Silver–cadmium battery Sodium-ion battery Sodium–sulfur battery Solid-state battery Super iron battery Wet cell Zinc

• DOE Explains...Batteries - Department of Energy

  Batteries and similar devices accept, store, and release electricity on demand. Batteries use chemistry, in the form of chemical potential, to store energy, just like many other everyday energy sources. For example, logs and oxygen both store energy in their chemical bonds until burning converts some of that chemical energy to heat. Gasoline and oxygen mixtures have stored chemical potential energy until it is converted to mechanical energy in a car engine. Similarly, for batteries to work, [...] electricity must be converted into a chemical potential form before it can be readily stored. Batteries consist of two electrical terminals called the cathode and the anode, separated by a chemical material called an electrolyte. To accept and release energy, a battery is coupled to an external circuit. Electrons move through the circuit, while simultaneously ions (atoms or molecules with an electric charge) move through the electrolyte. In a rechargeable battery, electrons and ions can move

• Award

  DOAJ seal

• Country

  Switzerland

• Instance Of

  Q737498