{"id":8055,"date":"2026-09-15T08:23:41","date_gmt":"2026-09-15T07:23:41","guid":{"rendered":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-2-compounds-formulae-and-equations\/equations-and-reaction-types\/ionic-and-full-equations\/"},"modified":"2026-09-19T20:35:49","modified_gmt":"2026-09-19T19:35:49","slug":"ionic-and-full-equations","status":"publish","type":"page","link":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-2-compounds-formulae-and-equations\/equations-and-reaction-types\/ionic-and-full-equations\/","title":{"rendered":"Ionic and Full Equations"},"content":{"rendered":"\n<!--\n===============================================================================\nONLINE LEARNING SYSTEM COPYRIGHT NOTICE\n\u00a9 Online Learning System. 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href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-2-compounds-formulae-and-equations\/\">Section overview<\/a><\/li>\n<li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-2-compounds-formulae-and-equations\/ions-and-ionic-formulae\/\">Ions and Ionic Formulae<\/a><\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-2-compounds-formulae-and-equations\/equations-and-reaction-types\/\">Equations and Reaction Types<\/a>\n        <ul class=\"ols-subtopic-list\">\n          <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-2-compounds-formulae-and-equations\/equations-and-reaction-types\/writing-chemical-equations\/\">Writing Chemical Equations<\/a><\/li>\n          <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-2-compounds-formulae-and-equations\/equations-and-reaction-types\/ionic-and-full-equations\/\">Ionic and Full Equations<\/a><\/li>\n          <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-4-acids\/typical-reactions-of-acids\/\">Typical Reactions of Acids<\/a><\/li>\n        <\/ul>\n      <\/li>\n    <\/ul>\n  <\/div>\n  <div class=\"ols-topic-group\">\n    <h4>Other OCR Sections<\/h4>\n    <ul class=\"ols-topic-list\">\n      <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-1-atomic-structure-and-isotopes\/\">2.1.1 Atomic Structure and Isotopes<\/a><\/li>\n      <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-3-amount-of-substance\/\">2.1.3 Amount of Substance<\/a><\/li>\n      <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-4-acids\/\">2.1.4 Acids<\/a><\/li>\n      <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-2-1-electron-structure\/\">2.2.1 Electron Structure<\/a><\/li>\n      <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-2-2-bonding-and-structure\/\">2.2.2 Bonding and Structure<\/a><\/li>\n      <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/3-1-1-periodicity\/\">3.1.1 Periodicity<\/a><\/li>\n      <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-1-1-basic-concepts-of-organic-chemistry\/\">4.1.1 Basic Concepts of Organic Chemistry<\/a><\/li>\n      <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-1-2-alkanes\/\">4.1.2 Alkanes<\/a><\/li>\n      <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-1-3-alkenes\/\">4.1.3 Alkenes<\/a><\/li>\n    <\/ul>\n  <\/div>\n<\/aside>\n<script>\r\n(function() {\r\n  function normalisePath(path) {\r\n    return String(path || '')\r\n      .split('?')[0]\r\n      .split('#')[0]\r\n      .replace(\/\\\/+$\/, '')\r\n      .toLowerCase();\r\n  }\r\n\r\n  function highlightActive() {\r\n    var sidebar = document.querySelector('.ols-sidebar');\r\n    if (!sidebar) return false;\r\n\r\n    var currentPath = normalisePath(window.location.pathname);\r\n    var links = sidebar.querySelectorAll('a[href]');\r\n    var matched = null;\r\n    var matchedLength = 0;\r\n\r\n    sidebar.querySelectorAll('.active, .active-main, .parent-active').forEach(function(item) {\r\n      item.classList.remove('active', 'active-main', 'parent-active');\r\n    });\r\n\r\n    sidebar.querySelectorAll('a[data-ols-disabled-parent=\"1\"], 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href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-2-compounds-formulae-and-equations\/equations-and-reaction-types\/\">Equations and Reaction Types<\/a> \/\n<span>Ionic and Full Equations<\/span>\n<\/nav>\n\n      <header class=\"ols-title-card\">\n        <h1>Ionic Equations<\/h1>\n        <p class=\"ols-page-intro\">A focused revision guide to ionic equations, spectator ions and precipitation reactions. Ionic equations look difficult at first, but they often make reactions easier because they show only the particles that actually change.<\/p>\n\n        <div class=\"ols-badges\">\n<div class=\"ols-badge\">Paper 1 and 2<\/div>\n<div class=\"ols-badge\">2.1.2 Compounds, Formulae and Equations<\/div>\n<div class=\"ols-badge\">H432\/01 and H432\/02<\/div>\n<\/div>\n\n        <div class=\"ols-author\">\n          <img decoding=\"async\" class=\"ols-author-avatar-img\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/05\/Author-Profile.jpeg\" alt=\"Dr. Mohammed Al-Fatah\">\n          <div class=\"ols-author-content\">\n            <h2 class=\"ols-author-title\">Written by:<br><span>Dr. Mohammed Al-Fatah<\/span><\/h2>\n            <p class=\"ols-author-description\">Chemistry specialist revision notes for A Level Chemistry.<\/p>\n            <a class=\"ols-linkedin-pill\" href=\"https:\/\/www.linkedin.com\/in\/doctormohammedfatah\/\" target=\"_blank\" rel=\"noopener noreferrer\">\n              <svg class=\"ols-linkedin-icon\" viewBox=\"0 0 24 24\" fill=\"currentColor\" aria-hidden=\"true\"><path d=\"M4.98 3.5C4.98 4.88 3.86 6 2.48 6S0 4.88 0 3.5 1.12 1 2.48 1s2.5 1.12 2.5 2.5zM.5 8h4V24h-4V8zm7 0h3.8v2.2h.1c.5-.9 1.8-2.2 3.9-2.2 4.2 0 5 2.8 5 6.4V24h-4v-7.6c0-1.8 0-4.2-2.6-4.2s-3 2-3 4v7.8h-4V8z\"><\/path><\/svg>\n              View LinkedIn Profile\n            <\/a>\n          <\/div>\n        <\/div>\n      <\/header>\n\n      <section class=\"ols-h5p-card ols-h5p-inline ols-h5p-recap\">\n<span class=\"ols-h5p-kicker\">Before you start<\/span>\n<h2>GCSE Recap: Ions, Formulae and State Symbols<\/h2>\n<p>Before you start, check that you can build a formula from its ions and use state symbols.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"288\"><\/div><\/div>\n<\/section>\n<article class=\"ols-note-card soft\">\n        <div class=\"ols-note-title\"><div class=\"ols-note-icon\">1<\/div><h2>Why Ionic Equations Are Useful<\/h2><\/div>\n        <p>An <strong>ionic equation<\/strong> shows the ions and particles that actually take part in a reaction. It leaves out ions that remain unchanged in solution.<\/p>\n        <p>This is why ionic equations are often shorter than full chemical equations. They remove the chemical detail that is present in the mixture but not directly involved in the reaction.<\/p>\n        <div class=\"ols-definition-box\"><p><strong>Ionic equation:<\/strong> an equation that represents a reaction using the reacting ions or particles, with spectator ions removed.<\/p><\/div>\n        <div class=\"ols-key-box\"><p><strong>Key idea:<\/strong> full equations show every formula in the reaction mixture, while ionic equations show the actual chemical change.<\/p><\/div>\n      <\/article>\n\n      <div class=\"ols-zoom-card\">\n        <div class=\"ols-zoom-card-image\">\n          <img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/05\/Understanding-ionic-equations-in-chemistry.webp\" alt=\"Understanding ionic equations in chemistry with reacting ions and spectator ions\" class=\"ols-zoomable-img ols-lightbox-target\" draggable=\"false\">\n        <\/div>\n        <div class=\"ols-zoom-card-caption\">\n          <p>Ionic equations focus attention on the particles that react, rather than every ion present in the solution.<\/p>\n        <\/div>\n      <\/div>\n\n      <article class=\"ols-note-card\">\n        <div class=\"ols-note-title\"><div class=\"ols-note-icon\">2<\/div><h2>Ions in Aqueous Solution<\/h2><\/div>\n        <p>When a soluble ionic compound dissolves in water, its ions separate and move around in solution. For example, sodium chloride solution contains <strong>Na<sup>+<\/sup>(aq)<\/strong> ions and <strong>Cl<sup>&#8211;<\/sup>(aq)<\/strong> ions.<\/p>\n        <p>The state symbol <strong>(aq)<\/strong> means <strong>aqueous<\/strong>, which means dissolved in water. It is important because ionic equations often involve dissolved ions.<\/p>\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>State symbol<\/th>\n                <th>Meaning<\/th>\n                <th>Use in ionic equations<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"State symbol\">(s)<\/td>\n                <td data-label=\"Meaning\">Solid<\/td>\n                <td data-label=\"Use in ionic equations\">Used for precipitates and insoluble substances.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"State symbol\">(l)<\/td>\n                <td data-label=\"Meaning\">Liquid<\/td>\n                <td data-label=\"Use in ionic equations\">Used for pure liquids, such as water.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"State symbol\">(g)<\/td>\n                <td data-label=\"Meaning\">Gas<\/td>\n                <td data-label=\"Use in ionic equations\">Used when a gaseous product forms.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"State symbol\">(aq)<\/td>\n                <td data-label=\"Meaning\">Aqueous solution<\/td>\n                <td data-label=\"Use in ionic equations\">Used for ions dissolved in water.<\/td>\n              <\/tr>\n            <\/tbody>\n          <\/table>\n        <\/div>\n        <div class=\"ols-key-box\"><p><strong>Exam focus:<\/strong> state symbols should be included in ionic equations when requested, especially for precipitates and aqueous ions.<\/p><\/div>\n      <\/article>\n\n      <article class=\"ols-note-card purple\">\n        <div class=\"ols-note-title\"><div class=\"ols-note-icon\">3<\/div><h2>Spectator Ions<\/h2><\/div>\n        <p>A <strong>spectator ion<\/strong> is an ion that is present in the reaction mixture but does not change during the reaction. It appears unchanged on both sides of the full ionic equation.<\/p>\n        <p>For example, in the reaction between sodium chloride solution and silver nitrate solution, sodium ions and nitrate ions remain dissolved in solution. They do not form the precipitate.<\/p>\n        <div class=\"ols-definition-box\"><p><strong>Spectator ion:<\/strong> an ion that is present during a reaction but is not chemically changed.<\/p><\/div>\n        <div class=\"ols-key-box\"><p><strong>How to spot one:<\/strong> if the same ion appears with the same charge and state symbol on both sides of the equation, it can be cancelled.<\/p><\/div>\n      <\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Spot the Spectator Ions<\/h2>\n<p>In each round, pick the one accurate statement about the ions in the reaction.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-289\" class=\"h5p-iframe\" data-content-id=\"289\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Spectator Ions Summary: Which Ions Do Not Change?\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card orange\">\n        <div class=\"ols-note-title\"><div class=\"ols-note-icon\">4<\/div><h2>Precipitation Reactions<\/h2><\/div>\n        <p>A <strong>precipitation reaction<\/strong> occurs when two solutions are mixed and an insoluble solid forms. The solid product is called a <strong>precipitate<\/strong>.<\/p>\n        <p>Precipitation reactions are a common context for ionic equations because the useful equation often shows only the two ions that join together to form the insoluble solid.<\/p>\n        <div class=\"ols-definition-box\"><p><strong>Precipitate:<\/strong> an insoluble solid formed when two solutions react.<\/p><\/div>\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Reaction mixture<\/th>\n                <th>Observation<\/th>\n                <th>Ionic change<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Reaction mixture\">Sodium chloride solution and silver nitrate solution<\/td>\n                <td data-label=\"Observation\">A white precipitate forms.<\/td>\n                <td data-label=\"Ionic change\">Ag<sup>+<\/sup>(aq) and Cl<sup>&#8211;<\/sup>(aq) form AgCl(s).<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Reaction mixture\">Barium chloride solution and sulfate ions<\/td>\n                <td data-label=\"Observation\">A white precipitate forms.<\/td>\n                <td data-label=\"Ionic change\">Ba<sup>2+<\/sup>(aq) and SO<sub>4<\/sub><sup>2-<\/sup>(aq) form BaSO<sub>4<\/sub>(s).<\/td>\n              <\/tr>\n            <\/tbody>\n          <\/table>\n        <\/div>\n      <\/article>\n\n      <div class=\"ols-zoom-card\">\n        <div class=\"ols-zoom-card-image\">\n          <img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/05\/precipitation-reaction.webp\" alt=\"Precipitation reaction showing ions joining to form an insoluble solid\" class=\"ols-zoomable-img ols-lightbox-target\" draggable=\"false\">\n        <\/div>\n        <div class=\"ols-zoom-card-caption\">\n          <p>A precipitate forms when ions in solution are strongly attracted and produce an insoluble solid.<\/p>\n        <\/div>\n      <\/div>\n\n      <article class=\"ols-note-card soft\">\n        <div class=\"ols-note-title\"><div class=\"ols-note-icon\">5<\/div><h2>Example: Silver Chloride Precipitation<\/h2><\/div>\n        <p>When sodium chloride solution is mixed with silver nitrate solution, a white precipitate of <strong>silver chloride<\/strong> forms.<\/p>\n        <div class=\"ols-definition-box\"><p><strong>Full equation:<\/strong> NaCl(aq) + AgNO<sub>3<\/sub>(aq) \u2192 AgCl(s) + NaNO<sub>3<\/sub>(aq)<\/p><\/div>\n        <p>In solution, the dissolved ionic compounds can be shown as ions:<\/p>\n        <div class=\"ols-definition-box\"><p>Na<sup>+<\/sup>(aq) + Cl<sup>&#8211;<\/sup>(aq) + Ag<sup>+<\/sup>(aq) + NO<sub>3<\/sub><sup>&#8211;<\/sup>(aq) \u2192 AgCl(s) + Na<sup>+<\/sup>(aq) + NO<sub>3<\/sub><sup>&#8211;<\/sup>(aq)<\/p><\/div>\n        <p>The <strong>Na<sup>+<\/sup><\/strong> and <strong>NO<sub>3<\/sub><sup>&#8211;<\/sup><\/strong> ions are spectator ions. Once they are removed, the ionic equation is:<\/p>\n        <div class=\"ols-key-box\"><p><strong>Ionic equation:<\/strong> Ag<sup>+<\/sup>(aq) + Cl<sup>&#8211;<\/sup>(aq) \u2192 AgCl(s)<\/p><\/div>\n      <\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Ionic Equation for a Precipitate<\/h2>\n<p>Choose the ionic equation that has the right ions, balanced charges and the right state symbol.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-636\" class=\"h5p-iframe\" data-content-id=\"636\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Ionic Equations MCQ: Iron(III) Hydroxide Precipitate\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card purple\">\n        <div class=\"ols-note-title\"><div class=\"ols-note-icon\">6<\/div><h2>How to Write Ionic Equations<\/h2><\/div>\n        <p>Start with the balanced full equation, then separate aqueous ionic substances into ions. Substances with state symbols <strong>(s)<\/strong>, <strong>(l)<\/strong> and <strong>(g)<\/strong> normally stay together.<\/p>\n        <ol>\n          <li>Write a correct balanced full equation.<\/li>\n          <li>Split aqueous ionic substances into their ions.<\/li>\n          <li>Keep solids, liquids, gases and covalent molecules together.<\/li>\n          <li>Cancel spectator ions that appear unchanged on both sides.<\/li>\n          <li>Check that atoms and charges are balanced.<\/li>\n        <\/ol>\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Substance type<\/th>\n                <th>What to do<\/th>\n                <th>Example<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Substance type\">Aqueous ionic compound<\/td>\n                <td data-label=\"What to do\">Split into ions.<\/td>\n                <td data-label=\"Example\">NaCl(aq) becomes Na<sup>+<\/sup>(aq) + Cl<sup>&#8211;<\/sup>(aq)<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Substance type\">Solid precipitate<\/td>\n                <td data-label=\"What to do\">Keep as a formula.<\/td>\n                <td data-label=\"Example\">AgCl(s) stays as AgCl(s)<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Substance type\">Liquid water<\/td>\n                <td data-label=\"What to do\">Keep as a molecule.<\/td>\n                <td data-label=\"Example\">H<sub>2<\/sub>O(l) stays as H<sub>2<\/sub>O(l)<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Substance type\">Gas<\/td>\n                <td data-label=\"What to do\">Keep as a formula.<\/td>\n                <td data-label=\"Example\">H<sub>2<\/sub>(g) stays as H<sub>2<\/sub>(g)<\/td>\n              <\/tr>\n            <\/tbody>\n          <\/table>\n        <\/div>\n      <\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Split or Keep Together?<\/h2>\n<p>Click every substance that is written as separate ions in an ionic equation.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-637\" class=\"h5p-iframe\" data-content-id=\"637\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Ionic Equations Mark the Words: Which Substances Are Split into Ions?\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card orange\">\n        <div class=\"ols-note-title\"><div class=\"ols-note-icon\">7<\/div><h2>Example: Barium Sulfate Precipitation<\/h2><\/div>\n        <p>When barium chloride solution is added to a solution containing sulfate ions, a white precipitate of <strong>barium sulfate<\/strong> forms.<\/p>\n        <div class=\"ols-definition-box\"><p><strong>Full equation:<\/strong> BaCl<sub>2<\/sub>(aq) + MgSO<sub>4<\/sub>(aq) \u2192 BaSO<sub>4<\/sub>(s) + MgCl<sub>2<\/sub>(aq)<\/p><\/div>\n        <p>The ions that form the insoluble precipitate are <strong>Ba<sup>2+<\/sup><\/strong> and <strong>SO<sub>4<\/sub><sup>2-<\/sup><\/strong>.<\/p>\n        <div class=\"ols-key-box\"><p><strong>Ionic equation:<\/strong> Ba<sup>2+<\/sup>(aq) + SO<sub>4<\/sub><sup>2-<\/sup>(aq) \u2192 BaSO<sub>4<\/sub>(s)<\/p><\/div>\n        <p>This reaction is used as a chemical test for sulfate ions. The sample is usually acidified before barium chloride solution is added.<\/p>\n      <\/article>\n\n      <article class=\"ols-note-card\">\n        <div class=\"ols-note-title\"><div class=\"ols-note-icon\">8<\/div><h2>Ionic Equations Beyond Precipitation<\/h2><\/div>\n        <p>Ionic equations are also useful for displacement reactions because they show the species that gain or lose electrons, or the ions that are displaced.<\/p>\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Reaction type<\/th>\n                <th>Example full equation<\/th>\n                <th>Useful ionic equation<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Reaction type\">Metal displacement<\/td>\n                <td data-label=\"Example full equation\">Mg(s) + CuSO<sub>4<\/sub>(aq) \u2192 MgSO<sub>4<\/sub>(aq) + Cu(s)<\/td>\n                <td data-label=\"Useful ionic equation\">Mg(s) + Cu<sup>2+<\/sup>(aq) \u2192 Mg<sup>2+<\/sup>(aq) + Cu(s)<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Reaction type\">Halogen displacement<\/td>\n                <td data-label=\"Example full equation\">Cl<sub>2<\/sub>(aq) + 2KBr(aq) \u2192 2KCl(aq) + Br<sub>2<\/sub>(aq)<\/td>\n                <td data-label=\"Useful ionic equation\">Cl<sub>2<\/sub>(aq) + 2Br<sup>&#8211;<\/sup>(aq) \u2192 2Cl<sup>&#8211;<\/sup>(aq) + Br<sub>2<\/sub>(aq)<\/td>\n              <\/tr>\n            <\/tbody>\n          <\/table>\n        <\/div>\n        <div class=\"ols-key-box\"><p><strong>Exam focus:<\/strong> spectator ions are not always sodium, potassium or nitrate ions, but these are very common because their compounds are usually soluble.<\/p><\/div>\n      <\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Atoms Balance, but Does the Charge?<\/h2>\n<p>Decide whether the ionic equation for this displacement reaction is balanced.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-638\" class=\"h5p-iframe\" data-content-id=\"638\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Ionic Equations True or False: Is the Charge Balanced?\"><\/iframe><\/div><\/div>\n<\/section>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Write the Ionic Equations<\/h2>\n<p>Write the full and ionic equations on paper before you flip each card.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-639\" class=\"h5p-iframe\" data-content-id=\"639\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Ionic Equations Flip Cards: New Precipitation and Displacement Reactions\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card soft\">\n        <div class=\"ols-note-title\"><div class=\"ols-note-icon\">9<\/div><h2>Common Exam Points<\/h2><\/div>\n        <ul>\n          <li>Ionic equations show only the particles that actually change.<\/li>\n          <li>Spectator ions appear unchanged on both sides of the equation and are cancelled.<\/li>\n          <li>The state symbol (aq) means aqueous, which means dissolved in water.<\/li>\n          <li>Precipitation reactions form an insoluble solid from ions in solution.<\/li>\n          <li>For precipitation reactions, the precipitate is written as a solid with the state symbol (s).<\/li>\n          <li>Do not split solids, liquids, gases or covalent molecules into ions.<\/li>\n          <li>Always check that the final ionic equation is balanced for both atoms and charge.<\/li>\n          <li>Ag<sup>+<\/sup>(aq) + Cl<sup>&#8211;<\/sup>(aq) \u2192 AgCl(s) is the ionic equation for forming silver chloride.<\/li>\n          <li>Ba<sup>2+<\/sup>(aq) + SO<sub>4<\/sub><sup>2-<\/sup>(aq) \u2192 BaSO<sub>4<\/sub>(s) is the ionic equation for forming barium sulfate.<\/li>\n        <\/ul>\n      <\/article>\n\n      \n\n      \n\n      <section class=\"ols-quicksnap-card\">\n        <h2>QuickSnap<\/h2>\n        <p>This text summary condenses the page into the essential exam ideas.<\/p>\n        <ul class=\"ols-quicksnap-list\">\n          <li><strong>Ionic equations:<\/strong> show the particles that actually react.<\/li>\n          <li><strong>Spectator ions:<\/strong> ions that appear unchanged on both sides of the equation.<\/li>\n          <li><strong>Aqueous ions:<\/strong> ions in solution are shown using the state symbol (aq).<\/li>\n          <li><strong>Precipitation:<\/strong> two aqueous ions combine to form an insoluble solid.<\/li>\n          <li><strong>Silver chloride:<\/strong> Ag<sup>+<\/sup>(aq) + Cl<sup>&#8211;<\/sup>(aq) \u2192 AgCl(s).<\/li>\n          <li><strong>Barium sulfate:<\/strong> Ba<sup>2+<\/sup>(aq) + SO<sub>4<\/sub><sup>2-<\/sup>(aq) \u2192 BaSO<sub>4<\/sub>(s).<\/li>\n          <li><strong>Final check:<\/strong> atoms and overall charge must both balance.<\/li>\n        <\/ul>\n      <\/section>\n\n      <div class=\"ols-image-lightbox\" id=\"olsImageLightboxIonicEquations001\" aria-hidden=\"true\" role=\"dialog\" aria-modal=\"true\" aria-label=\"Expanded revision image\">\n        <div class=\"ols-image-lightbox-inner\">\n          <button class=\"ols-image-lightbox-close\" type=\"button\" aria-label=\"Close enlarged image\">\u00d7<\/button>\n          <img decoding=\"async\" class=\"ols-image-lightbox-img\" src=\"\" alt=\"\">\n        <\/div>\n      <\/div>\n\n      <script>\n        (function(){\n          var page = document.querySelector(\".ols-ionic-equations-page\");\n          if (!page) {\n            return;\n          }\n\n          var lightbox = 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document.addEventListener(\"keydown\", function(event){\n            if (event.key === \"Escape\" && lightbox.classList.contains(\"is-open\")) {\n              closeLightbox();\n            }\n          });\n        })();\n      <\/script>\n\n      <section class=\"ols-faq-card\">\n        <h2>FAQs<\/h2>\n        <p>These questions address the most common misconceptions students have when learning ionic equations.<\/p>\n        <div class=\"ols-faq-list\">\n          <div class=\"ols-faq-item\">\n            <h3>What is an ionic equation?<\/h3>\n            <p>An ionic equation is an equation that shows the particles that actually take part in a reaction. Spectator ions are removed because they do not change.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>What is a spectator ion?<\/h3>\n            <p>A spectator ion is an ion that remains unchanged during a reaction. It appears on both sides of the full ionic equation with the same charge and state symbol.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Why do precipitates form?<\/h3>\n            <p>A precipitate forms when ions in solution combine to make an insoluble solid. For example, Ag<sup>+<\/sup>(aq) and Cl<sup>&#8211;<\/sup>(aq) form AgCl(s).<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Do I split every compound into ions?<\/h3>\n            <p>No. Only aqueous ionic substances are split into ions. Solids, liquids, gases and covalent molecules are normally kept together.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>How do I check my ionic equation is correct?<\/h3>\n            <p>Check that the atoms balance and that the total charge on the left equals the total charge on the right. A chemically correct ionic equation must satisfy both checks.<\/p>\n          <\/div>\n        <\/div>\n      <\/section>\n\n      <section class=\"ols-related-card\">\n        <h2>Related Topics<\/h2>\n        <p>Build the surrounding skills needed to write and interpret ionic equations confidently.<\/p>\n        <div class=\"ols-related-grid\">\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-2-compounds-formulae-and-equations\/equations-and-reaction-types\/writing-chemical-equations\/\">Writing Chemical Equations<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-4-acids\/typical-reactions-of-acids\/\">Typical Reactions of Acids<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-2-compounds-formulae-and-equations\/equations-and-reaction-types\/\">Equations and Reaction Types<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-3-amount-of-substance\/atoms-elements-and-molecules\/\">Atoms, Elements and Molecules<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-3-amount-of-substance\/empirical-and-molecular-formulae\/\">Formulae<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-2-compounds-formulae-and-equations\/\">this section Overview<\/a>\n        <\/div>\n      <\/section>\n\n      <section class=\"ols-attribution-card\">\n        <p><strong>Copyright notice:<\/strong> This OLS revision content, including the explanations, layout, diagrams, tables and embedded learning structure, is authored for Online Learning System by Dr. Mohammed Al-Fatah. It may not be copied, reproduced, redistributed or adapted without written permission.<\/p>\n      <\/section>\n\n      <script type=\"application\/ld+json\">\n{\n  \"@context\": \"https:\/\/schema.org\",\n  \"@graph\": [\n    {\n      \"@type\": \"WebPage\",\n      \"@id\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-2-compounds-formulae-and-equations\/equations-and-reaction-types\/ionic-and-full-equations\/#webpage\",\n      \"url\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-2-compounds-formulae-and-equations\/equations-and-reaction-types\/ionic-and-full-equations\/\",\n      \"name\": \"Ionic Equations - OCR A Level Chemistry A\",\n      \"description\": \"Revise ionic equations, spectator ions, state symbols and precipitation reactions for OCR A Level Chemistry A this section.\",\n      \"inLanguage\": \"en-GB\",\n      \"isPartOf\": {\n        \"@type\": \"WebSite\",\n        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