{"id":4577,"date":"2026-05-30T06:12:25","date_gmt":"2026-05-30T05:12:25","guid":{"rendered":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/ionic-bonding\/nature-of-ionic-bonding\/"},"modified":"2026-10-25T12:14:52","modified_gmt":"2026-10-25T12:14:52","slug":"nature-of-ionic-bonding","status":"publish","type":"page","link":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/ionic-bonding\/nature-of-ionic-bonding\/","title":{"rendered":"Nature of Ionic Bonding"},"content":{"rendered":"\n<section class=\"ols-revision-page ols-nature-of-ionic-bonding-9ch0-page\">\n  <style>\n    .ols-revision-page {\n      --navy: #1C244B;\n      --blue: #2563eb;\n      --soft-blue: #eef4ff;\n      --soft-red: #fff7f7;\n      --soft-purple: #f7f0ff;\n      --soft-green: #f0f7f1;\n      --soft-orange: #fff7ed;\n      --grey-text: #667085;\n      --body-text: 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}\n      .ols-table thead { display: none; }\n      .ols-table tr { margin-bottom: 14px; border: 1px solid var(--border); border-radius: 18px; overflow: hidden; background: #ffffff; box-shadow: var(--inner-shadow); }\n      .ols-table td { border-bottom: 1px solid var(--border); padding: 14px 16px; overflow-wrap: anywhere; }\n      .ols-table td:last-child { border-bottom: none; }\n      .ols-table td::before { content: attr(data-label); display: block; margin-bottom: 6px; font-size: 13px; font-weight: 700; color: var(--blue); }\n      .ols-author { align-items: flex-start; padding: 22px 18px; border-radius: 22px; }\n      .ols-author-avatar-img { width: 72px; height: 72px; }\n      .ols-author-title { font-size: 24px; }\n      .ols-author-description { font-size: 15px; }\n    }\n  \n    .ols-figure-placeholder .ols-placeholder-box { border: 2px dashed #c9973a; background: #fffaf0; border-radius: 16px; padding: 26px 22px; font-weight: 700; color: #7a4b12; text-align: center; line-height: 1.6; }\n    .ols-figure-placeholder .ols-figure-image { background: transparent; }\n    .ols-figure-placeholder { background: #ffffff; border: 1px solid rgba(28, 36, 75, 0.12); border-radius: 22px; padding: 14px; margin: 18px 0 6px; }\n    .ols-figure-placeholder .ols-figure-caption p { margin: 10px 0 0; font-size: 14px; color: #667085; text-align: center; }\n<\/style>\n\n    <aside class=\"ols-sidebar\">\r\n  <div class=\"ols-sidebar-header\">\r\n    <h3>Revision Notes<\/h3>\r\n    <p>A Level Chemistry<\/p>\r\n  <\/div>\r\n\r\n  <div class=\"ols-topic-group\">\r\n    <h4>Topic 2 Bonding and Structure<\/h4>\r\n\r\n    <ul class=\"ols-topic-list\">\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/ionic-bonding\/\">Ionic Bonding<\/a>\r\n\r\n        <ul class=\"ols-subtopic-list\">\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/ionic-bonding\/nature-of-ionic-bonding\/\">Nature of Ionic Bonding<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/ionic-bonding\/polarisation-of-ions\/\">Polarisation of Ions<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/ionic-bonding\/physical-properties-of-ionic-compounds\/\">Physical Properties of Ionic Compounds<\/a>\r\n          <\/li>\r\n        <\/ul>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/covalent-bonding\/\">Covalent Bonding<\/a>\r\n\r\n        <ul class=\"ols-subtopic-list\">\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/covalent-bonding\/nature-of-covalent-bonding\/\">Nature of Covalent Bonding<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/covalent-bonding\/dative-covalent-bonding\/\">Dative Covalent Bonding<\/a>\r\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/covalent-bonding\/giant-covalent-structures\/\">Giant Covalent Structures<\/a>\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/covalent-bonding\/electronegativity\/\">Electronegativity<\/a>\r\n          <\/li>\r\n        <\/ul>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/\">Shapes of Molecules<\/a>\r\n\r\n        <ul class=\"ols-subtopic-list\">\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/linear\/\">Linear<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/trigonal-planar\/\">Trigonal Planar<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/tetrahedral\/\">Tetrahedral<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/trigonal-pyramidal\/\">Trigonal Pyramidal<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/bent\/\">Bent<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/trigonal-bipyramidal\/\">Trigonal Bipyramidal<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/octahedral\/\">Octahedral<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/square-planar\/\">Square Planar<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/square-pyramidal\/\">Square Pyramidal<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/distorted-t\/\">Distorted T<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/seesaw\/\">SeeSaw<\/a>\r\n          <\/li>\r\n        <\/ul>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/polar-molecules\/\">Polar Molecules<\/a>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/\">Metallic Bonding<\/a>\r\n\r\n        <ul class=\"ols-subtopic-list\">\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/metallic-bonding-and-structure\/\">Metallic Bonding and Structure<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/physical-properties-of-metals\/\">Physical Properties of Metals<\/a>\r\n          <\/li>\r\n        <\/ul>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/\">Intermolecular Forces<\/a>\n        <ul class=\"ols-subtopic-list\">\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/london-forces\/\">London Forces<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/permanent-dipole-dipole-forces\/\">Permanent Dipole-Dipole Forces<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/hydrogen-bonding\/\">Hydrogen Bonding<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/anomalous-properties-of-water\/\">Anomalous Properties of Water<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/boiling-temperature-trends\/\">Boiling Temperature Trends<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/choosing-solvents\/\">Choosing Solvents<\/a>\n          <\/li>\n        <\/ul>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/structure-types\/\">Structure Types<\/a>\r\n      <\/li>\r\n\r\n    <\/ul>\r\n  <\/div>\r\n\r\n  <div class=\"ols-topic-group\">\r\n    <h4>Next Topics<\/h4>\r\n\r\n    <ul class=\"ols-topic-list\">\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-3-redox-i\/\">Redox I<\/a>\r\n      <\/li>\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-4-inorganic-chemistry-and-the-periodic-table\/\">Inorganic Chemistry &amp; The Periodic Table<\/a>\r\n      <\/li>\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-5-formulae-equations-and-amounts-of-substance\/\">Formulae, Equations &amp; Amounts<\/a>\r\n      <\/li>\r\n    <\/ul>\r\n  <\/div>\r\n<\/aside>\r\n\r\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', 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   }\r\n    }\r\n\r\n    return true;\r\n  }\r\n\r\n  if (!highlightActive()) {\r\n    document.addEventListener('DOMContentLoaded', highlightActive);\r\n  }\r\n})();\r\n<\/script>\n\n  <main class=\"ols-main\">\n      <nav class=\"ols-breadcrumbs\" aria-label=\"Breadcrumb\">\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/\">Revision Notes<\/a> \/\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/\">A Level Chemistry<\/a> \/\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/\">Edexcel<\/a> \/\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/\">Topic 2 Bonding and Structure<\/a> \/\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/ionic-bonding\/\">Ionic Bonding<\/a> \/\n        <span>Nature of Ionic Bonding<\/span>\n      <\/nav>\n\n      <header class=\"ols-title-card\">\n        <h1>Nature of Ionic Bonding<\/h1>\n        <p class=\"ols-page-intro\">A concise revision guide to ionic bonding, electron transfer, giant ionic lattice structure, ionic bonding strength and ionic radii for Edexcel A Level Chemistry.<\/p>\n\n        <div class=\"ols-badges\">\n          <div class=\"ols-badge\">Unit: Paper 1<\/div>\n          <div class=\"ols-badge\">Topic 2: Bonding and Structure<\/div>\n          <div class=\"ols-badge\">9CH0\/01<\/div>\n        <\/div>\n      <\/header>\n<!-- 3D card: nacl-lattice (swapped 26 Sep 2026) -->\n<!-- Copyright (c) 2026 Dr. Mohammed Al-Fatah, onlinelearningsystem.net. 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border:1px solid rgba(28,36,75,0.18);\n}\n.ols-nacl-001 .nacl-key i.k-ball{border-radius:50%;}\n\n@media (max-width:760px){\n  .ols-nacl-001{padding:26px; border-radius:22px;}\n  .ols-nacl-001 h2.nacl-title{font-size:20.5px;}\n  .ols-nacl-001 p.nacl-sub{font-size:13.5px;}\n  .ols-nacl-001 .nacl-stage{height:400px;}\n  .ols-nacl-001 .nacl-rowlab{min-width:100%;}\n  .ols-nacl-001 .nacl-seg button{padding:9px 13px; font-size:13px;}\n  .ols-nacl-001 .nacl-lab{font-size:10.5px; padding:4px 8px;}\n  .ols-nacl-001 .nacl-lab.l-part{font-size:9.5px; padding:3px 7px;}\n  .ols-nacl-001 .nacl-lab.l-read{font-size:12px; padding:5px 9px;}\n  .ols-nacl-001 .nacl-caption{font-size:10.5px; padding:5px 9px; max-width:64%;}\n  .ols-nacl-001 .nacl-badge{font-size:10.5px; padding:4px 9px;}\n  .ols-nacl-001 .nacl-badge.b-eq{font-size:11px;}\n  .ols-nacl-001 .nacl-badges{max-width:calc(100% - 28px);}\n  .ols-nacl-001 .nacl-info{padding:18px;}\n}\n\/* on a phone the caption needs the full top row, so the drag hint goes *\/\n@media (max-width:480px){\n  .ols-nacl-001 .nacl-hint{display:none;}\n  .ols-nacl-001 .nacl-caption{max-width:calc(100% - 28px);}\n}\n@media (prefers-reduced-motion:reduce){\n  .ols-nacl-001 .nacl-seg button,.ols-nacl-001 .nacl-pill{transition:none;}\n}\n\n.ols-cc-nacl-001{\n  font-family:'Poppins',system-ui,-apple-system,'Segoe UI',Roboto,Helvetica,Arial,sans-serif;\n  margin:10px auto 0; text-align:center; font-size:11px; font-style:italic; color:#aab0c0;\n}\n.ols-cc-nacl-001 a{color:#aab0c0; text-decoration:none;}\n.ols-cc-nacl-001 a:hover{text-decoration:underline;}\n.ols-nacl-001 .nacl-seg button{display:inline-flex; align-items:center;}\n.ols-nacl-001 .nacl-seg button .nacl-n{display:inline-flex; align-items:center; justify-content:center; width:20px; height:20px; margin-right:9px; border-radius:50%; font-size:11px; font-weight:600; background:rgba(37,99,235,0.10); color:#2563eb; flex:0 0 auto;}\n.ols-nacl-001 .nacl-seg button[aria-pressed=\"true\"] .nacl-n{background:#ffffff; color:#2563eb;}\n<\/style>\n\n<div class=\"nacl-head\">\n  <h2 class=\"nacl-title\">The Sodium Chloride Giant Ionic Lattice<\/h2>\n  <p class=\"nacl-sub\">Choose a step to watch sodium and chloride ions build the cubic lattice, see each ion&#8217;s six neighbours, extend the lattice and melt it.<\/p>\n<\/div>\n\n<div class=\"nacl-stage\" id=\"naclStage\">\n  <canvas class=\"nacl-canvas\" id=\"naclCanvas\"><\/canvas>\n  <div class=\"nacl-overlay\" id=\"naclOverlay\"><\/div>\n  <div class=\"nacl-caption\" id=\"naclCaption\"><\/div>\n  <div class=\"nacl-hint\" id=\"naclHint\">Drag to rotate<\/div>\n  <div class=\"nacl-badges\" id=\"naclBadges\"><\/div>\n<\/div>\n\n<div class=\"nacl-controls\">\n  <div class=\"nacl-row\">\n    <span class=\"nacl-rowlab\">Step<\/span>\n    <div class=\"nacl-seg\" role=\"group\" aria-label=\"Step\">\n      <button type=\"button\" data-step=\"1\" aria-pressed=\"true\"><span class=\"nacl-n\">1<\/span>Build the lattice<\/button>\n      <button type=\"button\" data-step=\"2\" aria-pressed=\"false\"><span class=\"nacl-n\">2<\/span>Na\u207a and Cl\u207b<\/button>\n      <button type=\"button\" data-step=\"3\" aria-pressed=\"false\"><span class=\"nacl-n\">3<\/span>6:6 coordination<\/button>\n      <button type=\"button\" data-step=\"4\" aria-pressed=\"false\"><span class=\"nacl-n\">4<\/span>Extend the lattice<\/button>\n      <button type=\"button\" data-step=\"5\" aria-pressed=\"false\"><span class=\"nacl-n\">5<\/span>Melting<\/button>\n    <\/div>\n  <\/div>\n\n  <div class=\"nacl-row\">\n    <span class=\"nacl-rowlab\">View<\/span>\n    <button type=\"button\" class=\"nacl-pill\" id=\"naclResetV\">Reset view<\/button>\n  <\/div>\n<\/div>\n\n<div class=\"nacl-info\">\n  <h3 id=\"naclInfoTitle\"><\/h3>\n  <p id=\"naclInfoText\"><\/p>\n  <div class=\"nacl-facts\" id=\"naclFacts\"><\/div>\n  <div class=\"nacl-key\">\n    <span><i class=\"k-ball\" style=\"background:#8c52c4\"><\/i>Sodium ion, Na\u207a<\/span>\n    <span><i class=\"k-ball\" style=\"background:#34aa48\"><\/i>Chloride ion, Cl\u207b<\/span>\n    <span><i class=\"\" style=\"background:#ffffff;border-color:rgba(212,168,20,0.95)\"><\/i>Electrostatic attraction<\/span>\n    <span><i class=\"\" style=\"background:#ffffff;border-color:rgba(28,36,75,0.6)\"><\/i>Unit cell edge<\/span>\n  <\/div>\n<\/div>\n\n<script src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/JS\/nacl-lattice.js?v=20261025p\"><\/script>\n<\/section>\n\n<p class=\"ols-cc-nacl-001\">&copy; Dr. Mohammed Al-Fatah &#8211; <a href=\"https:\/\/www.onlinelearningsystem.net\" target=\"_blank\" rel=\"noopener\">onlinelearningsystem.net<\/a><\/p>\n\n\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 and Electron Transfer<\/h2>\n<p>Before you start, check the GCSE ideas about ions and electron transfer that this page builds on.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"596\"><\/div><\/div>\n<\/section>\n<article class=\"ols-note-card soft\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">1<\/div>\n          <h2>What Is Ionic Bonding?<\/h2>\n        <\/div>\n\n        <p><strong>Ionic bonding<\/strong> is the strong electrostatic force of attraction between oppositely charged ions formed by electron transfer.<\/p>\n        <p>In sodium chloride, a sodium atom transfers one electron to a chlorine atom. Sodium becomes a positive ion, <strong>Na<sup>+<\/sup><\/strong>, and chlorine becomes a negative ion, <strong>Cl<sup>&#8211;<\/sup><\/strong>.<\/p>\n        <p>The attraction between the <strong>Na<sup>+<\/sup><\/strong> cation and the <strong>Cl<sup>&#8211;<\/sup><\/strong> anion is an ionic bond.<\/p>\n\n        <div class=\"ols-key-box\">\n          <p><strong>Key idea:<\/strong> Ionic bonding is not the transfer of electrons itself. The bond is the electrostatic attraction between the oppositely charged ions after transfer has occurred.<\/p>\n        <\/div>\n\n        <div class=\"ols-zoom-card wide\">\n          <div class=\"ols-figure-card\">\n<div class=\"ols-figure-image\"><img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-cd-01-dotcross-nacl.svg\" alt=\"Dot-and-cross diagram of a sodium atom transferring its 3s electron to a chlorine atom, forming [Na]\u207a (2,8) and [Cl]\u207b (2,8,8)\"><\/div>\n<div class=\"ols-figure-caption\"><p>Formation of sodium and chloride ions by electron transfer<\/p><\/div>\n<\/div>\n          <div class=\"ols-zoom-card-caption\">\n            <p>Sodium loses one outer electron to form Na<sup>+<\/sup>, while chlorine gains one electron to form Cl<sup>&#8211;<\/sup>.<\/p>\n          <\/div>\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: Predicting the Ions Formed<\/h2>\n<p>Answer each quick question on the ions formed and what the ionic bond is.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-153\" class=\"h5p-iframe\" data-content-id=\"153\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Ionic Bonding Quick Fire: Predicting the Ions Formed\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">2<\/div>\n          <h2>Giant Ionic Lattice Structure<\/h2>\n        <\/div>\n\n        <p>Ionic solids, such as sodium chloride, contain a <strong>giant ionic lattice<\/strong>. This means the ions are arranged in a repeating, ordered three-dimensional structure.<\/p>\n        <p>In sodium chloride, <strong>Na<sup>+<\/sup><\/strong> and <strong>Cl<sup>&#8211;<\/sup><\/strong> ions alternate in a regular pattern. Each ion is attracted to neighbouring ions with the opposite charge.<\/p>\n        <p>The electrostatic forces act in <strong>all possible directions<\/strong> through the lattice, so ionic bonding is not limited to one isolated pair of ions.<\/p>\n\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Term<\/th>\n                <th>Meaning<\/th>\n                <th>Exam focus<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Term\">Giant<\/td>\n                <td data-label=\"Meaning\">A very large repeating structure containing many ions.<\/td>\n                <td data-label=\"Exam focus\">Avoid describing NaCl as a small molecule.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Term\">Lattice<\/td>\n                <td data-label=\"Meaning\">A regular, repeating arrangement of particles.<\/td>\n                <td data-label=\"Exam focus\">Refer to a three-dimensional ionic lattice.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Term\">Ionic bond<\/td>\n                <td data-label=\"Meaning\">Electrostatic attraction between oppositely charged ions.<\/td>\n                <td data-label=\"Exam focus\">Attractions act in all directions.<\/td>\n              <\/tr>\n            <\/tbody>\n          <\/table>\n        <\/div>\n\n        <div class=\"ols-zoom-card wide\">\n          <div class=\"ols-figure-card\">\n<div class=\"ols-figure-image\"><img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/fix-17.jpg\" alt=\"Three-dimensional cubic lattice of sodium chloride with alternating Na+ and Cl- ions.\"><\/div>\n<div class=\"ols-figure-caption\"><p>Giant ionic lattice structure of sodium chloride<\/p><\/div>\n<\/div>\n          <div class=\"ols-zoom-card-caption\">\n            <p>The alternating arrangement of Na<sup>+<\/sup> and Cl<sup>&#8211;<\/sup> ions produces a regular cubic lattice in sodium chloride.<\/p>\n          <\/div>\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: Lattice or Molecule?<\/h2>\n<p>In each round, choose the one accurate statement about ionic lattices.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-154\" class=\"h5p-iframe\" data-content-id=\"154\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Ionic Lattice Summary: Spot the Accurate Statement\"><\/iframe><\/div><\/div>\n<\/section>\n\n      \n\n      <article class=\"ols-note-card purple\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">3<\/div>\n          <h2>Ionic Bonding Strength<\/h2>\n        <\/div>\n\n        <p>Ionic bonds become stronger when the ions are <strong>smaller<\/strong> and\/or carry <strong>greater charges<\/strong>.<\/p>\n        <p>Smaller ions allow oppositely charged ions to get closer together, increasing electrostatic attraction. Higher ionic charges also increase the attraction between ions.<\/p>\n        <p>This is why magnesium oxide, <strong>MgO<\/strong>, has a much higher melting temperature than sodium chloride, <strong>NaCl<\/strong>. The ions in MgO, <strong>Mg<sup>2+<\/sup><\/strong> and <strong>O<sup>2-<\/sup><\/strong>, are smaller and more highly charged than <strong>Na<sup>+<\/sup><\/strong> and <strong>Cl<sup>&#8211;<\/sup><\/strong>.<\/p>\n\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Compound<\/th>\n                <th>Ions involved<\/th>\n                <th>Ion size<\/th>\n                <th>Ion charge<\/th>\n                <th>Relative melting temperature<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Compound\"><strong>NaCl<\/strong><\/td>\n                <td data-label=\"Ions involved\">Na<sup>+<\/sup> and Cl<sup>&#8211;<\/sup><\/td>\n                <td data-label=\"Ion size\">Larger<\/td>\n                <td data-label=\"Ion charge\">\u00b11<\/td>\n                <td data-label=\"Relative melting point\">801 \u00b0C<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Compound\"><strong>MgO<\/strong><\/td>\n                <td data-label=\"Ions involved\">Mg<sup>2+<\/sup> and O<sup>2-<\/sup><\/td>\n                <td data-label=\"Ion size\">Smaller<\/td>\n                <td data-label=\"Ion charge\">\u00b12<\/td>\n                <td data-label=\"Relative melting point\">2852 \u00b0C<\/td>\n              <\/tr>\n            <\/tbody>\n          <\/table>\n        <\/div>\n\n        <div class=\"ols-key-box\">\n          <p><strong>Exam focus:<\/strong> When comparing ionic bonding strength, refer to both <strong>charge<\/strong> and <strong>ionic radius<\/strong> where relevant.<\/p>\n        <\/div>\n      <div class=\"ols-zoom-card\">\n<div class=\"ols-zoom-card-image\">\n<a class=\"ols-lightbox-link\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-05-ionicstrength.jpg\" aria-label=\"Open image full screen\">\n<img decoding=\"async\" class=\"ols-zoomable-img ols-lightbox-target\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-05-ionicstrength.jpg\" alt=\"NaCl, MgO and CaO ion pairs drawn to scale with ionic radii, charges and melting values, showing the effects of charge and size\">\n<\/a>\n<\/div>\n<div class=\"ols-zoom-card-caption\"><p>Higher charges and smaller ions give stronger ionic bonding: MgO melts far above NaCl, and above CaO because Mg\u00b2\u207a is smaller than Ca\u00b2\u207a.<\/p><\/div>\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: Explain a Melting Temperature Difference<\/h2>\n<p>Write a short explanation, then compare it with the mark points and the model answer.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-597\" class=\"h5p-iframe\" data-content-id=\"597\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Ionic Bonding Explain: Calcium Oxide and Potassium Chloride Melting Temperatures\"><\/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: Rank the Melting Temperatures<\/h2>\n<p>Put the six compounds in order of melting temperature, highest first.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-155\" class=\"h5p-iframe\" data-content-id=\"155\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Ionic Bonding Sort: Ranking Six Compounds by Melting Temperature\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card orange\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">4<\/div>\n          <h2>Ionic Radii<\/h2>\n        <\/div>\n\n        <p><strong>Positive ions<\/strong>, called cations, are smaller than their parent atoms. This is often because an entire outer electron shell is lost and the remaining electrons are pulled in more strongly by the nucleus.<\/p>\n        <p><strong>Negative ions<\/strong>, called anions, are larger than their parent atoms. Extra electrons are added while the number of protons stays the same, so the nuclear attraction is spread over more electrons.<\/p>\n\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Ion<\/th>\n                <th>Li<sup>+<\/sup><\/th>\n                <th>Na<sup>+<\/sup><\/th>\n                <th>K<sup>+<\/sup><\/th>\n                <th>Rb<sup>+<\/sup><\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Ion\"><strong>Ionic radius \/ nm<\/strong><\/td>\n                <td data-label=\"Li+\">0.060<\/td>\n                <td data-label=\"Na+\">0.095<\/td>\n                <td data-label=\"K+\">0.133<\/td>\n                <td data-label=\"Rb+\">0.148<\/td>\n              <\/tr>\n            <\/tbody>\n          <\/table>\n        <\/div>\n\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Ion<\/th>\n                <th>N<sup>3-<\/sup><\/th>\n                <th>O<sup>2-<\/sup><\/th>\n                <th>F<sup>&#8211;<\/sup><\/th>\n                <th>Na<sup>+<\/sup><\/th>\n                <th>Mg<sup>2+<\/sup><\/th>\n                <th>Al<sup>3+<\/sup><\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Ion\"><strong>No. of electrons<\/strong><\/td>\n                <td data-label=\"N3-\">10<\/td>\n                <td data-label=\"O2-\">10<\/td>\n                <td data-label=\"F-\">10<\/td>\n                <td data-label=\"Na+\">10<\/td>\n                <td data-label=\"Mg2+\">10<\/td>\n                <td data-label=\"Al3+\">10<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Ion\"><strong>No. of protons<\/strong><\/td>\n                <td data-label=\"N3-\">7<\/td>\n                <td data-label=\"O2-\">8<\/td>\n                <td data-label=\"F-\">9<\/td>\n                <td data-label=\"Na+\">11<\/td>\n                <td data-label=\"Mg2+\">12<\/td>\n                <td data-label=\"Al3+\">13<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Ion\"><strong>Ionic radius \/ nm<\/strong><\/td>\n                <td data-label=\"N3-\">0.171<\/td>\n                <td data-label=\"O2-\">0.140<\/td>\n                <td data-label=\"F-\">0.136<\/td>\n                <td data-label=\"Na+\">0.095<\/td>\n                <td data-label=\"Mg2+\">0.065<\/td>\n                <td data-label=\"Al3+\">0.050<\/td>\n              <\/tr>\n            <\/tbody>\n          <\/table>\n        <\/div>\n\n        <div class=\"ols-key-box\">\n          <p><strong>Key idea:<\/strong> In an isoelectronic series, the ions have the same number of electrons. As the number of protons increases, the attraction for those electrons increases and the ionic radius decreases.<\/p>\n        <\/div>\n      <div class=\"ols-zoom-card\">\n<div class=\"ols-zoom-card-image\">\n<a class=\"ols-lightbox-link\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-06-ionicradii.jpg\" aria-label=\"Open image full screen\">\n<img decoding=\"async\" class=\"ols-zoomable-img ols-lightbox-target\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-06-ionicradii.jpg\" alt=\"Circles to scale for N\u00b3\u207b to Al\u00b3\u207a (10 electrons each), Li\u207a to Rb\u207a down a group, and Na\/Na\u207a and Cl\/Cl\u207b atom-to-ion comparisons\">\n<\/a>\n<\/div>\n<div class=\"ols-zoom-card-caption\"><p>In an isoelectronic series the radius falls as the proton number rises; down a group the radius grows as shells are added.<\/p><\/div>\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: Ions with 18 Electrons<\/h2>\n<p>Count the protons and electrons in each ion, then drag the terms into place.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-152\" class=\"h5p-iframe\" data-content-id=\"152\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Ionic Radii Drag: An Isoelectronic Series with 18 Electrons\"><\/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: The Whole Page in Five Statements<\/h2>\n<p>In each round, pick the one accurate statement to review everything on this page.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-1292\" class=\"h5p-iframe\" data-content-id=\"1292\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Nature of Ionic Bonding Summary: Lattice, Bond Strength and Ion Size Reviewed\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">5<\/div>\n          <h2>Common Exam Points<\/h2>\n        <\/div>\n\n        <p>For ionic bonding and structure questions, exam answers usually need precise language. The most important phrases are <strong>oppositely charged ions<\/strong>, <strong>strong electrostatic attraction<\/strong>, <strong>giant ionic lattice<\/strong> and <strong>attraction in all directions<\/strong>.<\/p>\n\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Do not call ionic compounds molecules<\/h3>\n            <p>NaCl is normally described as a giant ionic lattice, not as individual NaCl molecules.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Separate electron transfer from bonding<\/h3>\n            <p>Electron transfer forms ions. The ionic bond is the electrostatic attraction between those ions.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Use charge and radius in explanations<\/h3>\n            <p>Greater charge and smaller ionic radius generally produce stronger ionic attractions and higher melting temperatures.<\/p>\n          <\/div>\n        <\/div>\n      <\/article>\n\n      \n\n      <article class=\"ols-note-card purple\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">\u2713<\/div>\n          <h2>QuickSnap<\/h2>\n        <\/div>\n\n        <p>For this page, the essential idea is that <strong>electron transfer forms ions<\/strong>, but the <strong>ionic bond<\/strong> is the strong electrostatic attraction between those oppositely charged ions.<\/p>\n\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Formation of ions<\/h3>\n            <p>Metals lose electrons to form positive cations, while non-metals gain electrons to form negative anions. For example, sodium forms Na<sup>+<\/sup> and chlorine forms Cl<sup>&#8211;<\/sup>.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Giant ionic lattice<\/h3>\n            <p>Ionic compounds form regular, repeating three-dimensional lattices. The attractions act in all directions between neighbouring oppositely charged ions.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Bond strength<\/h3>\n            <p>Ionic bonding is stronger when ions are smaller and\/or more highly charged. This explains why MgO has a much higher melting temperature than NaCl.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Ionic radius<\/h3>\n            <p>Cations are smaller than their parent atoms because electrons are lost. Anions are larger because extra electrons are added and electron-electron repulsion increases.<\/p>\n          <\/div>\n        <\/div>\n      <\/article>\n\n            <section class=\"ols-faq-card\">\n        <h2>Frequently Asked Questions<\/h2>\n        <p>Use these quick answers to check the core language needed for ionic bonding and structure questions.<\/p>\n\n        <div class=\"ols-faq-list\">\n          <div class=\"ols-faq-item\">\n            <h3>What is ionic bonding?<\/h3>\n            <p>Ionic bonding is the strong electrostatic force of attraction between oppositely charged ions formed by electron transfer.<\/p>\n          <\/div>\n\n          <div class=\"ols-faq-item\">\n            <h3>Is ionic bonding the same as electron transfer?<\/h3>\n            <p>No. Electron transfer forms positive and negative ions. The ionic bond is the electrostatic attraction between those oppositely charged ions.<\/p>\n          <\/div>\n\n          <div class=\"ols-faq-item\">\n            <h3>What is a giant ionic lattice?<\/h3>\n            <p>A giant ionic lattice is a regular, repeating three-dimensional arrangement of ions held together by electrostatic attractions in all directions.<\/p>\n          <\/div>\n\n          <div class=\"ols-faq-item\">\n            <h3>Why does MgO have a higher melting temperature than NaCl?<\/h3>\n            <p>MgO contains Mg<sup>2+<\/sup> and O<sup>2-<\/sup> ions, which are more highly charged and smaller than Na<sup>+<\/sup> and Cl<sup>&#8211;<\/sup> ions. This creates stronger electrostatic attractions, so more energy is needed to melt MgO.<\/p>\n          <\/div>\n\n          <div class=\"ols-faq-item\">\n            <h3>How do the sizes of ions compare with their parent atoms?<\/h3>\n            <p>A cation is smaller than its atom: it loses electrons, often a whole shell, and the remaining electrons are pulled in more strongly. An anion is larger: the added electrons repel each other while the nuclear charge stays the same.<\/p>\n          <\/div>\n        <\/div>\n      <\/section>\n\n      <!-- author card (moved to the end, 10 Oct 2026) -->\n      <div class=\"ols-author\">\n\n    <img decoding=\"async\"\n      class=\"ols-author-avatar-img\"\n      src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/05\/Author-Profile.jpeg\"\n      alt=\"Dr. Mohammed Al-Fatah\"\n    >\n\n    <div class=\"ols-author-content\">\n\n      <h2 class=\"ols-author-title\">\n        Written by: Dr. Mohammed Al-Fatah\n      <\/h2>\n\n      <p class=\"ols-author-description\">\n        Chemistry specialist revision notes for A Level Chemistry.\n      <\/p>\n\n      <a\n        class=\"ols-linkedin-pill\"\n        href=\"https:\/\/www.linkedin.com\/in\/doctormohammedfatah\/\"\n        target=\"_blank\"\n        rel=\"noopener noreferrer\"\n      >\n\n        <svg class=\"ols-linkedin-icon\" viewBox=\"0 0 24 24\" fill=\"currentColor\" aria-hidden=\"true\">\n          <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\"\/>\n        <\/svg>\n\n        View LinkedIn Profile\n\n      <\/a>\n\n    <\/div>\n\n  <\/div>\n\n\n      <section class=\"ols-related-card\">\n        <h2>Related Ionic Bonding Revision Notes<\/h2>\n        <p>Continue through Topic 2 by linking ionic bonding to polarisation, ionic properties and covalent bonding.<\/p>\n\n        <div class=\"ols-related-grid\">\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/ionic-bonding\/polarisation-of-ions\/\">Polarisation of Ions<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/ionic-bonding\/physical-properties-of-ionic-compounds\/\">Physical Properties of Ionic Compounds<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/covalent-bonding\/\">Covalent Bonding<\/a>\n        <\/div>\n      <\/section>\n\n    \n\n      <section class=\"ols-attribution-card ols-attr-std\" aria-label=\"Copyright notice\">\n<style id=\"ols-attribution-card-css\">.ols-attribution-card.ols-attr-std{background:linear-gradient(135deg,#ffffff,#f8fbff);border:1px solid rgba(28,36,75,0.14);border-radius:28px;box-shadow:0 18px 45px rgba(28,36,75,0.10);padding:34px;margin:24px 0;overflow:hidden;font-family:Poppins,Arial,sans-serif;box-sizing:border-box}.ols-attribution-card.ols-attr-std *{box-sizing:border-box}.ols-attribution-card.ols-attr-std p{margin:0;font-size:14px;line-height:1.65;font-weight:300;color:#667085}.ols-attribution-card.ols-attr-std strong{font-weight:700;color:#1C244B}@media (max-width:760px){.ols-attribution-card.ols-attr-std{padding:24px 18px;border-radius:22px}}<\/style>\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      <div class=\"ols-image-lightbox\" role=\"dialog\" aria-modal=\"true\" aria-label=\"Image lightbox\">\n        <div class=\"ols-image-lightbox-inner\">\n          <button class=\"ols-image-lightbox-close\" type=\"button\" aria-label=\"Close image lightbox\">&times;<\/button>\n          <img decoding=\"async\" class=\"ols-image-lightbox-img\" src=\"\" alt=\"\">\n        <\/div>\n      <\/div>\n    <\/main>\n<script>\n(function(){\n  var wrap = document.querySelector('.ols-nature-of-ionic-bonding-9ch0-page');\n  if (!wrap) return;\n\n  var targets = wrap.querySelectorAll('.ols-lightbox-target');\n  var overlay = wrap.querySelector('.ols-image-lightbox');\n  var lbImg = wrap.querySelector('.ols-image-lightbox-img');\n  var closeBtn = wrap.querySelector('.ols-image-lightbox-close');\n\n  if (!overlay || !lbImg || !closeBtn || !targets.length) return;\n\n  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Unit: Paper 1 Topic 2: [&hellip;]<\/p>\n","protected":false},"author":12,"featured_media":0,"parent":4570,"menu_order":0,"comment_status":"closed","ping_status":"closed","template":"","meta":{"footnotes":""},"class_list":["post-4577","page","type-page","status-publish","hentry"],"_links":{"self":[{"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages\/4577","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages"}],"about":[{"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/types\/page"}],"author":[{"embeddable":true,"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/users\/12"}],"replies":[{"embeddable":true,"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/comments?post=4577"}],"version-history":[{"count":2,"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages\/4577\/revisions"}],"predecessor-version":[{"id":24835,"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages\/4577\/revisions\/24835"}],"up":[{"embeddable":true,"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages\/4570"}],"wp:attachment":[{"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/media?parent=4577"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}