<h2>Secondary Batteries</h2>
<p><strong>Secondary batteries</strong> are rechargeable. These are the types of batteries found in devices such as smartphones, electronic tablets, and automobiles.</p>
<p><strong>Nickel-cadmium</strong>, or NiCd, batteries (see the figure below) consist of a nickel-plated cathode, cadmium-plated anode, and a potassium hydroxide electrode. The positive and negative plates, which are prevented from shorting by the separator, are rolled together and put into the case. This is a “jelly-roll” design and allows the NiCd cell to deliver much more current than a similar-sized alkaline battery. The <a data-lesson="reactions-2" data-subject="chemistry" data-tutorial="metals-metalloids-nonmetals" href="https://app.ulearngo.com/chemistry/metals-metalloids-nonmetals/reactions-2">reactions</a> are</p>
<p>\(\begin{array}{l}\underset{¯}{\begin{array}{l}\text{anode:}\phantom{\rule{4.35em}{0ex}}\text{Cd}(s)+{\text{2OH}}^{\text{−}}(aq)\phantom{\rule{0.2em}{0ex}}⟶\phantom{\rule{0.2em}{0ex}}{\text{Cd(OH)}}_{2}(s)+{\text{2e}}^{\text{−}}\\ \text{cathode:}\phantom{\rule{0.28em}{0ex}}{\text{NiO}}_{2}(s)+{\text{2H}}_{2}\text{O}(l)+{\text{2e}}^{\text{−}}\phantom{\rule{0.2em}{0ex}}⟶\phantom{\rule{0.2em}{0ex}}{\text{Ni(OH)}}_{2}(s)+{\text{2OH}}^{\text{−}}(aq)\end{array}}\\ \hline \text{overall: Cd}(s)+{\text{NiO}}_{2}(s)+{\text{2H}}_{2}\text{O}(l)\phantom{\rule{0.2em}{0ex}}⟶\phantom{\rule{0.2em}{0ex}}{\text{Cd(OH)}}_{2}(s)+{\text{Ni(OH)}}_{2}(s)\end{array}\)</p>
<p>The voltage is about 1.2 V to 1.25 V as the battery discharges. When properly treated, a NiCd battery can be recharged about 1000 times. Cadmium is a toxic heavy metal so NiCd batteries should never be opened or put into the regular trash.</p>
<div class="wp-caption alignnone" style="width: 800px"><img alt="A diagram is shown of a cross section of a nickel cadmium battery. This battery is in a cylindrical shape. An outer red layer is labeled “case.” Just inside this layer is a thin, dark grey layer which is labeled at the bottom of the cylinder as “Negative electrode collector.” A silver rod extends upward through the center of the battery, which is surrounded by alternating layers, shown as vertical repeating bands, of yellow, purple, yellow, and blue. A slightly darker grey narrow band extends across the top of these alternating bands, which is labeled “Positive electrode collector.” A thin light grey band appears at the very bottom of the cylinder, which is labeled “Metal bottom cover (negative).” A small grey and white striped rectangular structure is present at the top of the central silver cylinder, which is labeled “Safety valve.” Above this is an orange layer that curves upward over the safety valve, which is labeled “Insulation ring.” Above this is a thin light grey layer that projects upward slightly at the center, which is labeled “Metal top cover (plus).” A light grey arrow points to a rectangle to the right that illustrates the layers at the center of the battery under magnification. From the central silver rod, the layers shown repeat the alternating pattern yellow, blue, yellow, and purple three times, with a final yellow layer covering the last purple layer. The outermost purple layer is labeled “Negative electrode.” The yellow layer beneath it is labeled “Separator.” The blue layer just inside is labeled “Positive electrode.”" height="508" src="https://data.ulearngo.com/assets/62172a66-f67b-4b54-8e01-1c14be136761" width="800"/><p class="wp-caption-text">NiCd batteries use a “jelly-roll” design that significantly increases the amount of current the battery can deliver as compared to a similar-sized alkaline battery.</p></div>
<div class="ns-tutorial">
<div class="ns-school-defn2">
<h3>Resource:</h3>
<p>Visit this <a href="https://en.wikipedia.org/wiki/Nickel–cadmium_battery" rel="nofollow">Wikipedia webpage</a> for more information about nickel cadmium rechargeable batteries.</p>
</div>
<p><strong>Lithium ion batteries</strong> (see the figure below) are among the most popular rechargeable batteries and are used in many portable electronic devices. The reactions are</p>
<p>\(\begin{array}{l}\underset{¯}{\begin{array}{l}\text{anode:}\phantom{\rule{5.65em}{0ex}}{\text{LiCoO}}_{2}\phantom{\rule{0.2em}{0ex}}⇌\phantom{\rule{0.2em}{0ex}}{\text{Li}}_{1\text{−}x}{\text{CoO}}_{2}+x\phantom{\rule{0.2em}{0ex}}{\text{Li}}^{\text{+}}+x\phantom{\rule{0.2em}{0ex}}{\text{e}}^{\text{−}}\\ \text{cathode:}\phantom{\rule{0.2em}{0ex}}x\phantom{\rule{0.2em}{0ex}}{\text{Li}}^{\text{+}}+x\phantom{\rule{0.2em}{0ex}}{\text{e}}^{\text{−}}+x\phantom{\rule{0.2em}{0ex}}{\text{C}}_{6}\phantom{\rule{0.2em}{0ex}}⇌\phantom{\rule{0.2em}{0ex}}x\phantom{\rule{0.2em}{0ex}}{\text{LiC}}_{6}\end{array}}\\ \hline \text{overall:}\phantom{\rule{2.3em}{0ex}}{\text{LiCoO}}_{2}+x\phantom{\rule{0.2em}{0ex}}{\text{C}}_{6}\phantom{\rule{0.2em}{0ex}}⇌\phantom{\rule{0.2em}{0ex}}{\text{Li}}_{1\text{−}x}{\text{CoO}}_{2}+x\phantom{\rule{0.2em}{0ex}}{\text{LiC}}_{6}\end{array}\)</p>
<p>With the coefficients representing moles, <em>x</em> is no more than about 0.5 moles. The battery voltage is about 3.7 V. Lithium batteries are popular because they can provide a large amount current, are lighter than comparable batteries of other types, produce a nearly constant voltage as they discharge, and only slowly lose their charge when stored.</p>
<div class="wp-caption alignnone" style="width: 800px"><img alt="This figure shows a model of the flow of charge in a lithium ion battery. At the left, an approximately cubic structure formed by alternating red, grey, and purple spheres is labeled below as “Positive electrode.” The purple spheres are identified by the label “lithium.” The grey spheres are identified by the label “Metal.” The red spheres are identified by the label “oxygen.” Above this structure is the label “Charge” followed by a right pointing green arrow. At the right is a figure with layers of black interconnected spheres with purple spheres located in gaps between the layers. The black layers are labeled “Graphite layers.” Below the purple and black structure is the label “Negative electrode.” Above is the label “Discharge,” which is preceded by a blue arrow which points left. At the center of the diagram between the two structures are six purple spheres which are each labeled with a plus symbol. Three curved green arrows extend from the red, purple, and grey structure to each of the three closest purple plus labeled spheres. Green curved arrows extend from the right side of the upper and lower of these three purple plus labeled spheres to the black and purple layered structure. Three blue arrows extend from the purple and black layered structure to the remaining three purple plus labeled spheres at the center of the diagram. The base of each arrow has a circle formed by a dashed curved line in the layered structure. The lowest of the three purple plus marked spheres reached by the blue arrows has a second blue arrow extending from its left side which points to a purple sphere in the purple, green, and grey structure." height="298" src="https://data.ulearngo.com/assets/b169f776-e22e-4e7f-99af-b0ef26d428d0" width="800"/><p class="wp-caption-text">In a lithium ion battery, charge flows between the electrodes as the lithium ions move between the anode and cathode.</p></div>
<h3>Optional Video:</h3>
<p>Watch the video below for more information about lithium ion batteries.</p>
<p><iframe allowfullscreen="allowfullscreen" frameborder="0" height="531" src="https://www.youtube.com/embed/2PjyJhe7Q1g?rel=0&amp;modestbranding=1&amp;cc_lang_pref=en&amp;cc_load_policy=1" width="944"><span class="mce_SELRES_start" data-mce-type="bookmark" style="display: inline-block; width: 0px; overflow: hidden; line-height: 0;">﻿</span></iframe></p>
<p>The <strong>lead acid battery</strong> (see the figure below) is the type of <a data-lesson="summarizing-batteries-and-fuel-cells" data-subject="chemistry" data-tutorial="electrochemistry" href="https://app.ulearngo.com/chemistry/electrochemistry/summarizing-batteries-and-fuel-cells">secondary battery</a> used in your automobile. It is inexpensive and capable of producing the high current required by automobile starter motors. The reactions for a lead acid battery are</p>
<p>\(\begin{array}{l}\underset{¯}{\begin{array}{l}\text{anode:}\phantom{\rule{9.6em}{0ex}}\text{Pb}(s)+{\text{HSO}}_{4}{}^{\text{−}}(aq)\phantom{\rule{0.2em}{0ex}}⟶\phantom{\rule{0.2em}{0ex}}{\text{PbSO}}_{4}(s)+{\text{H}}^{\text{+}}(aq)+{\text{2e}}^{\text{−}}\\ {\text{cathode: PbO}}_{2}(s)+{\text{HSO}}_{4}{}^{\text{−}}(aq)+{\text{3H}}^{\text{+}}(aq)+{\text{2e}}^{\text{−}}\phantom{\rule{0.2em}{0ex}}⟶\phantom{\rule{0.2em}{0ex}}{\text{PbSO}}_{4}(s)+2{\text{H}}_{2}\text{O}(l)\end{array}}\\ \hline \text{overall:}\phantom{\rule{4.43em}{0ex}}\text{Pb}(s)+{\text{PbO}}_{2}(s)+2{\text{H}}_{2}{\text{SO}}_{4}(aq)\phantom{\rule{0.2em}{0ex}}⟶\phantom{\rule{0.2em}{0ex}}{\text{2PbSO}}_{4}(s)+2{\text{H}}_{2}\text{O}(l)\end{array}\)</p>
<p>Each cell produces 2 V, so six cells are connected in series to produce a 12-V car battery. Lead acid batteries are heavy and contain a caustic <a data-lesson="summarizing-properties-of-liquids" data-subject="chemistry" data-tutorial="liquids-and-solids" href="https://app.ulearngo.com/chemistry/liquids-and-solids/summarizing-properties-of-liquids">liquid</a> electrolyte, but are often still the battery of choice because of their high current density. Since these batteries contain a significant amount of lead, they must always be disposed of properly.</p>
<div class="wp-caption alignnone" style="width: 800px"><img alt="A diagram of a lead acid battery is shown. A black outer casing, which is labeled “Protective casing” is in the form of a rectangular prism. Grey cylindrical projections extend upward from the upper surface of the battery in the back left and back right corners. At the back right corner, the projection is labeled “Positive terminal.” At the back right corner, the projection is labeled “Negative terminal.” The bottom layer of the battery diagram is a dark green color, which is labeled “Dilute H subscript 2 S O subscript 4.” A blue outer covering extends upward from this region near the top of the battery. Inside, alternating grey and white vertical “sheets” are packed together in repeating units within the battery. The battery has the sides cut away to show three of these repeating units which are separated by black vertical dividers, which are labeled as “cell dividers.” The grey layers in the repeating units are labeled “Negative electrode (lead).” The white layers are labeled “Postive electrode (lead dioxide).”" height="504" src="https://data.ulearngo.com/assets/ea4ff5fb-c1c7-417c-8d0e-808aa0f70ad1" width="800"/><p class="wp-caption-text">The lead acid battery in your automobile consists of six cells connected in series to give 12 V. Their low cost and high current output makes these excellent candidates for providing power for automobile starter motors.</p></div>
<h3>Optional Video:</h3>
<p>Watch the video below for more information about lead acid batteries.</p>
<p><iframe allowfullscreen="allowfullscreen" frameborder="0" height="531" src="https://www.youtube.com/embed/rhIRD5YVNbs?rel=0&amp;modestbranding=1&amp;cc_lang_pref=en&amp;cc_load_policy=1" width="944"><span class="mce_SELRES_start" data-mce-type="bookmark" style="display: inline-block; width: 0px; overflow: hidden; line-height: 0;">﻿</span></iframe></p>
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Secondary Batteries

Chemistry generally explores the substances of which matter is composed, the investigation of their properties and reactions, and the use of such reactions to form new substances. 

Chemistry

Discover the principles of electrochemistry and learn how to balance oxidation-reduction reactions, analyze galvanic cells, explore standard reduction potentials, understand the Nernst equation, study batteries and fuel cells, discuss corrosion, and investigate electrolysis and electrode potentials.


Secondary Batteries

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