How Do Batteries Work | An Introduction to Batteries

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An efficient method of electrical energy storage uses reduction-oxide reactions, also known as redox reactions." /><link rel="apple-touch-icon" sizes="180x180" href="//www.ossila.com/cdn/shop/t/304/assets/apple-touch-icon.png?v=47689890648139992551732532704"> <link rel="icon" type="image/png" sizes="32x32" href="//www.ossila.com/cdn/shop/t/304/assets/favicon-32x32.png?v=170914528706734454101732532704"> <link rel="icon" type="image/png" sizes="16x16" href="//www.ossila.com/cdn/shop/t/304/assets/favicon-16x16.png?v=162550173345868048431732532704"> <link rel="manifest" href="//www.ossila.com/cdn/shop/t/304/assets/site.webmanifest?v=100969836723433583841732532704"> <link rel="mask-icon" href="//www.ossila.com/cdn/shop/t/304/assets/safari-pinned-tab.svg?v=95647162979764929801732532704" color="#39499c"> <meta name="msapplication-TileColor" content="#418fde"> <meta name="theme-color" content="#ffffff"> <link rel="canonical" href="https://www.ossila.com/pages/how-batteries-work" />  <link rel="stylesheet" href="//www.ossila.com/cdn/shop/t/304/assets/main-style.css?v=39679133822212140421732532704">  <script>var shopifyMoneyFormat = '${{amount}}';</script> <script defer src="//www.ossila.com/cdn/shop/t/304/assets/main.js?v=137866433984839773511732532704"></script>  <meta property="og:type" content="website" /> <meta property="og:title" content="How Do Batteries Work | An Introduction to Batteries" /> <meta property="og:description" content="Batteries store electricity and provide an easily accessible energy supply. An efficient method of electrical energy storage uses reduction-oxide reactions, also known as redox reactions." /> <meta property="og:url" content="https://www.ossila.com/pages/how-batteries-work" /> <meta property="og:site_name" content="Ossila" /> <meta name="twitter:site" content="@ossilascience"> <meta name="twitter:card" content="summary"> <meta name="twitter:title" content="How Do Batteries Work: An Introduction to Batteries"> <meta name="twitter:description" content="A battery is an energy storage device which provides an easily accessible supply of electrical energy. Batteries convert chemical potential energy, from redox reactions, into electrical energy. Redox reactions include both reduction (where electrons are gained) and oxidation (where electrons are lost) reactions. These happen simultaneously as charge is transferred from one species to another. Since the invention of the first battery in 1800, batteries have proven their versatility by powering everything from small consumer goods like toys to large vehicles. Over time, a wide range of battery materials with varying chemistries and properties have been developed to suit different applications. On This Page How do batteries work? Types of battery Measuring the performance of a battery Battery research How Do Batteries Work? A common example of stored electrical energy is when a plastic rod is rubbed with fur. 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Supplies</a> <a href="/collections/spectroscopy"> <svg class="icon icon-navigate_next"><use xlink:href="#icon-navigate_next"></use></svg> Spectroscopy Equipment</a> <a href="/collections/solution-making"> <svg class="icon icon-navigate_next"><use xlink:href="#icon-navigate_next"></use></svg> Solution Making Supplies</a> <a href="/collections/equipment-accessories"> <svg class="icon icon-navigate_next"><use xlink:href="#icon-navigate_next"></use></svg> Equipment Accessories</a> <a href="/collections/general-laboratory-supplies"> <svg class="icon icon-navigate_next"><use xlink:href="#icon-navigate_next"></use></svg> General Laboratory Supplies</a> </div> </div> </ul> </li> </ul> </nav> </div> </div> </div>  <div class="container"> <div id="unsupported-browser-message" class="alert-warning"> <p>It looks like you are using an unsupported browser. You can still place orders by emailing us on <a href="mailto:info@ossila.com">info@ossila.com</a>, but you may experience issues browsing our website. Please consider upgrading to a modern browser for better security and an improved browsing experience.</p> </div> </div>  <main> <div id="informational-page"> <h1>How Do Batteries Work: An Introduction to Batteries</h1> <div class="container"> <img alt="An Introduction to Batteries" class="featured-image" height="280" loading="lazy" src="https://www.ossila.com/cdn/shop/files/Battery-Materials.jpg?crop=center&width=1340&height=280" width="1340"> <p>A battery is an energy storage device which provides an easily accessible supply of electrical energy. Batteries convert chemical potential energy, from redox reactions, into electrical energy.</p> <p>Redox reactions include both reduction (where electrons are gained) and oxidation (where electrons are lost) reactions. These happen simultaneously as charge is transferred from one species to another.</p> <p>Since the invention of the first battery in 1800, batteries have proven their versatility by powering everything from small consumer goods like toys to large vehicles. Over time, a wide range of <a title="battery materials" href="https://www.ossila.com/collections/battery-materials">battery materials</a> with varying chemistries and properties have been developed to suit different applications.</p> <div class="panel panel-default"> <div class="panel-body"> <p class="h3" style="margin-top: 10px;" data-mce-style="margin-top: 10px;">On This Page</p> <hr> <ul> <li><a href="#How-do-batteries-work">How do batteries work?</a></li> <li><a href="#Types-of-battery">Types of battery</a></li> <li><a href="#Measuring-the-performance-of-a-battery">Measuring the performance of a battery</a></li> <li><a href="#Battery-research">Battery research</a></li> </ul> </div> </div> <div style="text-align: left;"> <h2 id="How-do-batteries-work">How Do Batteries Work?</h2> <hr> <p><span data-mce-fragment="1"> A common example of stored electrical energy is when a plastic rod is rubbed with fur. The rod becomes negatively charged as the electrons are transferred from the fur. Batteries use a more efficient method to transfer charge: redox reactions. </span>Batteries convert chemical potential energy, from the redox reactions, into electrical energy and consist of four key components:</p> <table> <tbody> <tr> <th width="189"> <p><strong>Component </strong></p> </th> <th width="412"> <p><strong>Role</strong></p> </th> </tr> <tr> <td width="189"> <p>Electrode</p> <p>(cathode and anode)</p> </td> <td width="412"> <p>Enable output and input of electrical energy, these are where the redox reactions occur.</p> </td> </tr> <tr> <td width="189"> <p>Electrolyte</p> </td> <td width="412"> <p>Transfers ions and facilitates a controlled electron flow through the circuit.</p> </td> </tr> <tr> <td width="189"> <p>Separator</p> </td> <td width="412"> <p>Creates mechanical stability and prevents immediate discharge.</p> </td> </tr> <tr> <td width="189"> <p>Battery management system</p> </td> <td width="412"> <p>Maintains a safe voltage region to prevent overheating.</p> </td> </tr> </tbody> </table> <p> </p> <figure><video alt="How Do Batteries Work - charging and discharging cycle" autoplay="autoplay" loop="loop" muted="muted" src="https://cdn.ossila.com/videos/How-do-Batterys-Work-1080p.mp4" type="video/mp4"></video> <figcaption>Charge movement within a battery during battery charging and discharging cycles.</figcaption> </figure> <p>Redox reactions involve the transfer of electrons from one species to another. Therefore, some species lose electrons (oxidation) and some species gain electrons (reduction). Whether the oxidation or reduction reaction takes places at the anode or cathode depends on whether the battery is charging or discharging, this also dictates the direction of ions between the electrodes. A typical set of redox reactions for a Li-ion (Li<sup>+</sup>) battery is shown below:</p> <div style="text-align: center;"><em><strong>Reduction:</strong> CoO<sub>2</sub> + Li<sup>+</sup> + e<sup>- </sup> → LiCoO<sub>2</sub></em></div> <div style="text-align: center;"><em><strong>Oxidation:</strong> LiC<sub>6</sub> → C<sub>6 </sub>+ Li<sup>+</sup> + e<sup>-</sup></em></div> <p style="text-align: center;"><em><strong>Full redox reaction:</strong> LiC<sub>6</sub>+ CoO<sub>2</sub> ↔ C<sub>6 </sub> + LiCoO<sub>2</sub> </em></p> <p style="text-align: center;"><em>left to right is discharging (→), right to left is charging (←)</em></p> <h3>Storing Electricity</h3> <p>Batteries store electrical energy by converting it into chemical potential energy. This is defined as ‘charging’ the battery. An applied voltage drives ions stored in the cathode towards the anode via the electrolyte. When the ions reach the anode, they are positioned within the anode material’s layers. This process is called intercalation. At the same time, electrons move from the cathode to the anode through the circuit. The non-conductive nature of the electrolyte and the separator prevent the electrons travelling back towards the cathode, known as internal short circuiting. Therefore these electrons are held at the anode, ready for discharge.</p> <p>The type of ion depends on the type of battery, for example <a href="/pages/lithium-ion-batteries" title="How Lithium-Batteries Work">lithium-ion batteries</a> have cathode materials that supply lithium ions (Li<sup>+</sup>).</p> </div> <figure><img alt="Battery charging involves the cathode (left) releasing lithium ions through an electrolyte and separator towards the anode (right)." src="https://www.ossila.com/cdn/shop/files/Graphine-Battery-Setup.svg?v=1721743504" width="636"> <figcaption>Charging of a battery</figcaption> </figure> <h3></h3> <h3>Releasing Electricity</h3> <p>Connecting the battery to a circuit causes the battery to release electricity, this is known as discharging. The circuit allows for a flow of electrons from the anode back towards the cathode without an applied voltage. This releases the stored electrical energy.</p> <figure><img alt="Battery discharging involves the anode (right) releasing lithium ions through an electrolyte and separator towards the cathode(left) while electrons flow from the anode through a circuit to power it." src="https://www.ossila.com/cdn/shop/files/How_fo_Batterys_Work_Discharging.svg?v=1695895194" width="636"> <figcaption>Discharging of a battery</figcaption> </figure> <h2 id="Types-of-battery">Types of Battery</h2> <hr> <p>Batteries have been under development since 1800 and therefore there is a wide range of variations. The different chemistry used in batteries each offer unique benefits and applications.</p> <h3>Primary and Secondary Batteries</h3> <p>Batteries can be organized into two main categories: primary and secondary. Primary batteries are single use, while secondary batteries are rechargeable. Both can be further divided into subcategories depending on the <a href="https://www.ossila.com/collections/battery-materials" data-mce-href="https://www.ossila.com/collections/battery-materials"><strong>battery material</strong></a>.</p> <p>Primary batteries are typically assembled charged and the lifespan depends on the amount of chemically reactive material used. Secondary batteries still have a limited lifespan, known as the lifecycle. The lifecycle of a secondary battery is based on how many times the battery can be fully recharged until the capacity of the battery drops to below 80% of the original capacity. The rechargeability of a secondary battery stem from the reversibility of its redox reactions.</p> <p>While primary and secondary batteries have their differences, most consist of the same components.</p> <table> <tbody width="100%"> <tr> <th width="15%">Battery Type</th> <th width="15%">Usage</th> <th width="25%">Lifespan</th> <th width="15%">Examples</th> <th width="30%">Applications</th> </tr> <tr> <td> <p><em><strong>Primary</strong></em></p> </td> <td> <p>Single use</p> </td> <td> <p>Finite, depends on amount of chemically reactive material</p> </td> <td> <p>Alkaline</p> </td> <td> <p>Consumer electronics, such as smoke detectors, flashlights and toys.</p> </td> </tr> <tr> <td><em><strong>Secondary</strong></em></td> <td>Rechargeable</td> <td> <p>Limited, known as the lifecycle. This is how many charge cycles can occur before capacity drops below 80%</p> </td> <td width="126"> <p>Lithium-ion</p> <p>Lead-acid</p> <p>Nickel-cadmium</p> </td> <td width="126"> <p>Consumer goods and electric vehicles</p> <p>Car batteries</p> <p>Emergency power source</p> </td> </tr> </tbody> </table> <h3>Battery Applications</h3> <p>Battery applications depend on a range of characteristics, including electrical storage capacity, high power, and lifespan. Different batteries are known by their chemistries and research is highly focused on optimizing and discovering further applications.</p> <h4>Lithium-Ion</h4> <p>Lithium-ion (Li-ion) batteries are the most common type of <strong>secondary battery</strong>. Most often these are used in electrical goods and electrical vehicles (EV). <a href="https://www.ossila.com/pages/lithium-ion-batteries" data-mce-href="https://www.ossila.com/pages/lithium-ion-batteries"><strong>Lithium-ion batteries</strong></a> offer a high energy density, long cycle life, and are lightweight.</p> <h4>Alkaline</h4> <p>Alkaline batteries are another common type of <strong>primary batteries </strong>and are often used to power consumer electronics such as smoke detectors, flashlights and toys. Alkaline batteries are reliable and have long shelf lives. As well as their inability to recharge and lower power outputs, they are also commonly made of toxic materials and so leakages can be dangerous if mishandled.</p> <h4>Lead-Acid</h4> <p>Commonly used in the automotive industry, lead-acid batteries are reliable secondary batteries that can provide large currents. The ability to offer a high and sudden charge is required for starting a car engine, especially in colder climates.</p> <h4>Nickel-Cadmium</h4> <p>Nickel-cadmium (Ni-Cd) were once popular; however, these <strong>secondary batteries</strong> have been replaced by safer options due to environmental concerns. While they are not as common, Ni-Cd batteries are still sometimes used as an emergency power source as they deliver reliable power over a long lifecycle.</p> <h2 id="Measuring-the-performance-of-a-battery">Measuring the performance of a battery</h2> <hr> <h3>Discharge rate</h3> <p>Typically referred to as C, the discharge rate affects how quickly charge flows through a circuit. A battery with a discharge rate of 1C can discharge its capacity in 1 hour. The higher the C value the faster the battery can discharge. If a battery holds 2000 mAh but can discharge with a current of 1000mA, then the battery has a C rate of 2C.</p> <p> </p> <figure><img alt="Equation for the discharge rate of a battery" src="https://www.ossila.com/cdn/shop/files/Discharge-Rate-Equashion-01.svg?v=1721826846" width="250"> <figcaption>Equation for the discharge rate of a battery</figcaption> </figure> <p>C is determined by the ion mobility and overall capacity. If the lithium ions in a <a href="https://www.ossila.com/pages/lithium-ion-batteries"><strong>lithium-ion battery</strong></a> can move through the electrolyte faster, the electrons at the anode can discharge through a circuit faster. Similarly, during charging, the lithium ions can be stored in the anode faster.</p> <h3>Charge capacity</h3> <p>The specific capacity of a battery is defined as how much charge can be stored per unit mass: mAh/g. The theoretical capacity can be calculated by:</p> <figure><img alt="Equation to calculate the theoretical capacity of a battery" height="47" loading="lazy" src="https://www.ossila.com/cdn/shop/files/Battery-theoretical-charge-equation.svg?width=150" width="74"> <figcaption>Equation to calculate the theoretical charge capacity of a battery</figcaption> </figure> <p> </p> <p>Where <em>Q</em> is the specific charge, <em>n</em> is the number of electrons transferred per mole of reaction, <em>F</em> is Faraday's constant, and <em>Mr</em> is the molecular mass.</p> <p>The experimental capacities are far inferior to the theoretically calculated. This is due to imperfections and defects in the purity of the material. For example, <a href="https://www.ossila.com/products/lithium-cobalt-oxide-powder"><strong>LiCoO<sub>2</sub></strong></a> has a theoretical capacity of 274 mAh/g but only an experimental capacity of 165 mAh/g.</p> <h3>Energy density</h3> <p>Energy density is the amount of energy a battery can store per unit mass and is measured in watt-hours per kilogram (Wh kg<sup>-1</sup>). Higher energy densities mean more energy can be stored in a smaller energy. More stored energy increases the lifetime of the battery and means it does not need to be replaced as frequently. Moreover, more energy in a smaller area means more compact and lightweight batteries can be fabricated. This is particularly important for the usability of consumer goods such as smartphones and laptops as well as in electric vehicles.</p> <h3>Lifetime</h3> <p>The lifetime of a battery is one of the most important properties to the consumer. A battery ‘s lifetime is defined as the number of times a battery can be fully recharged whilst maintaining at least 80% of its original capacity. Often this is stated as a timeframe, in hours, instead of a number of cycles. Not only do longer lifetimes increase the relative efficiency of a battery, but they also increase user convenience. Long lifetimes mean less replacements and less waste, therefore increasing the sustainability as less energy is required to both produce and recycle the battery.</p> <h2 id="Battery-research">Battery Research</h2> <hr> <p>A vast amount of research is ongoing to determine the best chemistry to boost each aspect of a battery. Specifically, there is a large focus on <a href="https://www.ossila.com/pages/lithium-ion-batteries"><strong>lithium-ion batteries</strong></a> due to their use in EVs. While Li-ion batteries are the dominant rechargeable batteries, there is potential for new battery developments. For example sodium-ion batteries (Na-ion), there is a natural abundance of sodium, making it easier and cheaper to obtain than lithium. Similarly, graphene batteries are advancing due to their high energy density and non-flammable makeup.</p> <a data-track-content="" class="green-banner" href="https://www.ossila.com/collections/battery-materials"> <p data-content-piece="cta-battery-materials" data-content-name="/pages/how-batteries-work">Battery Materials</p> <img loading="lazy" alt="single-walled carbon nanotubes" src="https://www.ossila.com/cdn/shop/files/carbon-nanotubes-bottle.jpg?v=1724162898" height="120" width="600"> <button>Browse now</button> </a> <h2>Learn More</h2> <hr> <div class="row button-row"> <div class="col-xs-12 col-sm-6 button-col"> <div class="card-box card-truncate"> <a href="/pages/lithium-ion-batteries"><img width="160" src="https://www.ossila.com/cdn/shop/files/lithium-ion-battery-work-diagram.png?v=1696343218&crop=center&width=160&height=160" loading="lazy" height="160" alt="How Lithium-Ion Batteries Work"></a> <a href="/pages/lithium-ion-batteries"> How Lithium-Ion Batteries Work</a> <p>Lithium-ion batteries use the reversible lithium intercalation reaction. The battery has several important components to enable this intercalation.</p> <a href="/pages/lithium-ion-batteries">Read more...</a> </div> </div> <div class="col-xs-12 col-sm-6 button-col"> <div class="card-box card-truncate"> <a href="/pages/anode-vs-cathode-batteries"><img width="160" src="https://www.ossila.com/cdn/shop/files/cathode-vs-anode.png?v=1718371020&crop=center&width=160&height=160" loading="lazy" height="160" alt="Cathode vs Anode: What is the Difference?"></a> <a href="/pages/anode-vs-cathode-batteries"> Cathode vs Anode: What is the Difference?</a> <p>Defining a cathode and anode as positive and negative, or as the source and sink of a current, depends on your definition of current itself. Current can describe the flow of positive or negative charge.</p> <a href="/pages/anode-vs-cathode-batteries">Read more...</a> </div> </div> </div> <div class="panel panel-default"> <div class="panel-body"> <h3>Contributing Authors</h3> <hr> <p>Written by</p> <p class="no-margin"><a href="/pages/our-writers#other-authors" title="Contributing Authors">Brett Pasquill</a></p> <p class="text-muted">Scientific Writer</p> </div> </div> <script type="application/ld+json"> { "@context": "https://schema.org", "@type": "Article", "abstract": "Batteries convert chemical potential energy, from redox reactions, into electrical energy. Redox reactions include both reduction (where electrons are gained) and oxidation (where electrons are lost) reactions. 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How Do Batteries Work | An Introduction to Batteries | Ossila