{"id":4596,"date":"2026-05-30T06:13:12","date_gmt":"2026-05-30T05:13:12","guid":{"rendered":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/metallic-bonding-and-structure\/"},"modified":"2026-10-25T12:14:26","modified_gmt":"2026-10-25T12:14:26","slug":"metallic-bonding-and-structure","status":"publish","type":"page","link":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/metallic-bonding-and-structure\/","title":{"rendered":"Metallic Bonding and Structure"},"content":{"rendered":"\n<section class=\"ols-revision-page ols-metallic-bonding-structure-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      --soft-gold: 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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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\/\n        <span>Metallic Bonding &amp; Structure<\/span>\n      <\/nav>\n\n      <header class=\"ols-title-card\">\n        <h1>Metallic Bonding &amp; Structure<\/h1>\n        <p class=\"ols-page-intro\">A concise revision guide to metallic bonding, giant metallic lattice structures, positive metal ions, delocalised electrons and the factors that affect metallic bonding strength.<\/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: metallic-bonding (swapped 26 Sep 2026) -->\n<!-- Copyright (c) 2026 Dr. Mohammed Al-Fatah, onlinelearningsystem.net. 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text-align:center; font-size:11px; font-style:italic; color:#aab0c0;\n}\n.ols-cc-mtlb-001 a{color:#aab0c0; text-decoration:none;}\n.ols-cc-mtlb-001 a:hover{text-decoration:underline;}\n.ols-mtlb-001 .mtlb-seg button{display:inline-flex; align-items:center;}\n.ols-mtlb-001 .mtlb-seg button .mtlb-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-mtlb-001 .mtlb-seg button[aria-pressed=\"true\"] .mtlb-n{background:#ffffff; color:#2563eb;}\n<\/style>\n\n<div class=\"mtlb-head\">\n  <h2 class=\"mtlb-title\">Metallic Bonding: Ions in a Sea of Electrons<\/h2>\n  <p class=\"mtlb-sub\">Choose a step to watch sodium atoms release their outer electrons, the ions sit in a sea of delocalised electrons, and that sea explain strength, conduction and malleability.<\/p>\n<\/div>\n\n<div class=\"mtlb-stage\" id=\"mtlbStage\">\n  <canvas class=\"mtlb-canvas\" id=\"mtlbCanvas\"><\/canvas>\n  <div class=\"mtlb-overlay\" id=\"mtlbOverlay\"><\/div>\n  <div class=\"mtlb-caption\" id=\"mtlbCaption\"><\/div>\n  <div class=\"mtlb-hint\" id=\"mtlbHint\">Drag to rotate<\/div>\n  <div class=\"mtlb-badges\" id=\"mtlbBadges\"><\/div>\n<\/div>\n\n<div class=\"mtlb-controls\">\n  <div class=\"mtlb-row\">\n    <span class=\"mtlb-rowlab\">Step<\/span>\n    <div class=\"mtlb-seg\" role=\"group\" aria-label=\"Step\">\n      <button type=\"button\" data-step=\"1\" aria-pressed=\"true\"><span class=\"mtlb-n\">1<\/span>Atoms release electrons<\/button>\n      <button type=\"button\" data-step=\"2\" aria-pressed=\"false\"><span class=\"mtlb-n\">2<\/span>Ions in an electron sea<\/button>\n      <button type=\"button\" data-step=\"3\" aria-pressed=\"false\"><span class=\"mtlb-n\">3<\/span>Sodium, magnesium, aluminium<\/button>\n      <button type=\"button\" data-step=\"4\" aria-pressed=\"false\"><span class=\"mtlb-n\">4<\/span>Conducting electricity<\/button>\n      <button type=\"button\" data-step=\"5\" aria-pressed=\"false\"><span class=\"mtlb-n\">5<\/span>Layers slide<\/button>\n    <\/div>\n  <\/div>\n\n  <div class=\"mtlb-row\">\n    <span class=\"mtlb-rowlab\">View<\/span>\n    <button type=\"button\" class=\"mtlb-pill\" id=\"mtlbResetV\">Reset view<\/button>\n  <\/div>\n<\/div>\n\n<div class=\"mtlb-info\">\n  <h3 id=\"mtlbInfoTitle\"><\/h3>\n  <p id=\"mtlbInfoText\"><\/p>\n  <div class=\"mtlb-facts\" id=\"mtlbFacts\"><\/div>\n  <div class=\"mtlb-key\">\n    <span><i class=\"k-ball\" style=\"background:#8c52c4\"><\/i>Sodium atom<\/span>\n    <span><i class=\"k-ball\" style=\"background:#b2b8c4\"><\/i>Metal ion<\/span>\n    <span><i class=\"k-ball\" style=\"background:#f2bc1a\"><\/i>Delocalised electron<\/span>\n    <span><i class=\"\" style=\"background:#fff3c8;border-color:rgba(201,150,28,0.5)\"><\/i>Electron sea<\/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\/metallic-bonding.js?v=20261025p\"><\/script>\n<\/section>\n\n<p class=\"ols-cc-mtlb-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: The Model of a Metal<\/h2>\n<p>Before you start, check the GCSE model of a metal that this page builds on.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"603\"><\/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 Metallic Bonding?<\/h2>\n        <\/div>\n\n        <p><strong>Metallic bonding<\/strong> is the electrostatic force of attraction between <strong>positive metal ions<\/strong> and <strong>delocalised electrons<\/strong>.<\/p>\n        <p>When metal atoms form a metallic lattice, their outer-shell electrons become delocalised. These electrons are not attached to one particular atom and can move through the structure.<\/p>\n        <p>The metal atoms are left as positive ions. The attraction between these positive ions and the delocalised electrons holds the metal lattice together.<\/p>\n\n        <div class=\"ols-definition-box\">\n          <p><strong>Definition:<\/strong> Metallic bonding is the strong electrostatic attraction between a regular lattice of positive metal ions and a sea of delocalised electrons.<\/p>\n        <\/div>\n\n        <div class=\"ols-key-box\">\n          <p><strong>Key idea:<\/strong> A metal is not made from separate molecules. It is a giant metallic lattice held together by attraction between positive ions and delocalised electrons.<\/p>\n        <\/div>\n      <\/article>\n\n      <article class=\"ols-note-card\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">2<\/div>\n          <h2>Giant Metallic Lattice Structure<\/h2>\n        <\/div>\n\n        <p>Metals exist as <strong>giant metallic lattice structures<\/strong>. The positive metal ions are arranged in a <strong>regular, closely packed lattice<\/strong>.<\/p>\n        <p>The outer-shell electrons are <strong>delocalised<\/strong>, meaning they are free to move through the lattice. This leaves behind positive metal ions such as <strong>Na<sup>+<\/sup><\/strong>, <strong>Mg<sup>2+<\/sup><\/strong> and <strong>Al<sup>3+<\/sup><\/strong>.<\/p>\n        <p>The structure can be described as <strong>layers of positive metal ions surrounded by delocalised electrons<\/strong>.<\/p>\n\n        <div class=\"ols-zoom-card wide\">\n          <div class=\"ols-zoom-card-image\">\n            <img decoding=\"async\" class=\"ols-zoomable-img ols-lightbox-target\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-03-metallattice.jpg\" alt=\"Rows of Mg\u00b2\u207a ions surrounded by a sea of delocalised electrons, labelled with the lattice, the free electrons and the attraction\">\n          <\/div>\n          <div class=\"ols-zoom-card-caption\">\n            <p>The diagram shows positive metal ions in fixed lattice positions surrounded by delocalised electrons.<\/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: Ions and Electrons in New Metals<\/h2>\n<p>Answer each quick question on the ions and delocalised electrons in a metal.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-225\" class=\"h5p-iframe\" data-content-id=\"225\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Metallic Bonding Quick Fire: Ions and Delocalised Electrons in New Metals\"><\/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>Why Delocalised Electrons Matter<\/h2>\n        <\/div>\n\n        <p>In a metal, delocalised electrons can move through the lattice. They are sometimes described as a <strong>sea of delocalised electrons<\/strong>.<\/p>\n        <p>This electron sea is attracted to many positive ions at the same time, helping to hold the whole giant lattice together rather than forming a small separate molecule.<\/p>\n        <p>The delocalised electrons also explain why metals can conduct electricity. When a potential difference is applied, the mobile electrons can move and carry charge through the structure.<\/p>\n\n        <div class=\"ols-equation-box\">\n          <p><strong>Metallic lattice model:<\/strong> positive metal ions + delocalised electrons &rarr; giant metallic lattice held by electrostatic attraction.<\/p>\n        <\/div>\n\n        <div class=\"ols-key-box\">\n          <p><strong>Exam focus:<\/strong> Use the phrase <strong>delocalised electrons<\/strong>, not free electrons by itself. The electrons are free to move through the metallic lattice, but they are still part of the metal structure.<\/p>\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: Metal or Ionic Solid?<\/h2>\n<p>Drag the words into place to compare calcium metal with calcium oxide.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-224\" class=\"h5p-iframe\" data-content-id=\"224\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Metallic Bonding Drag: Calcium Metal Compared with Calcium Oxide\"><\/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>Metallic Bonding Strength Factors<\/h2>\n        <\/div>\n\n        <p>The strength of metallic bonding depends on how strongly the positive metal ions attract the delocalised electrons.<\/p>\n        <p>Three main factors are used in exam explanations: <strong>nuclear charge<\/strong>, the <strong>number of delocalised electrons per atom<\/strong> and the <strong>size of the metal ion<\/strong>.<\/p>\n\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Factor<\/th>\n                <th>Effect on metallic bonding<\/th>\n                <th>Exam wording<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Factor\"><strong>Number of protons<\/strong><\/td>\n                <td data-label=\"Effect on metallic bonding\">More protons means a higher nuclear charge, giving a stronger attraction to delocalised electrons.<\/td>\n                <td data-label=\"Exam wording\">More protons lead to a stronger attraction between positive ions and delocalised electrons.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Factor\"><strong>Number of delocalised electrons per atom<\/strong><\/td>\n                <td data-label=\"Effect on metallic bonding\">More delocalised electrons means a greater electron density available for attraction to the metal ions.<\/td>\n                <td data-label=\"Exam wording\">More delocalised electrons result in a stronger metallic bond.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Factor\"><strong>Size of the metal ion<\/strong><\/td>\n                <td data-label=\"Effect on metallic bonding\">Smaller ions allow the delocalised electrons to be attracted more strongly because the charge is closer.<\/td>\n                <td data-label=\"Exam wording\">Smaller ions produce a stronger attraction and therefore stronger metallic bonding.<\/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-21.jpg\" alt=\"Three factors that make metallic bonding stronger, compared across sodium, magnesium and aluminium.\"><\/div>\n<div class=\"ols-figure-caption\"><p>Metallic bonding strength factors table showing protons, delocalised electrons and ion size<\/p><\/div>\n<\/div>\n          <div class=\"ols-zoom-card-caption\">\n            <p>Metallic bonding becomes stronger when the attraction between positive ions and delocalised electrons increases.<\/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: Rank the Metallic Bonding<\/h2>\n<p>Put the metals in order of metallic bonding strength.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-227\" class=\"h5p-iframe\" data-content-id=\"227\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Metallic Bonding Sort: Ranking Five Metals by Bond Strength\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card gold\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">5<\/div>\n          <h2>Comparing Metallic Bonding Strength<\/h2>\n        <\/div>\n\n        <p>Metallic bonding is often stronger when a metal atom contributes more outer-shell electrons to the delocalised electron sea.<\/p>\n        <p>For example, magnesium forms <strong>Mg<sup>2+<\/sup><\/strong> ions and contributes more delocalised electrons per atom than sodium, which forms <strong>Na<sup>+<\/sup><\/strong> ions. Aluminium forms <strong>Al<sup>3+<\/sup><\/strong> ions and contributes even more delocalised electrons per atom.<\/p>\n        <p>This is why exam answers often compare the charge on the metal ion, the number of delocalised electrons, and the strength of attraction within the lattice.<\/p>\n\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Metal<\/th>\n                <th>Ion commonly shown<\/th>\n                <th>Delocalised electrons per atom<\/th>\n                <th>Expected bonding strength trend<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Metal\"><strong>Sodium<\/strong><\/td>\n                <td data-label=\"Ion commonly shown\">Na<sup>+<\/sup><\/td>\n                <td data-label=\"Delocalised electrons per atom\">1<\/td>\n                <td data-label=\"Expected bonding strength trend\">Weaker than magnesium and aluminium, because fewer electrons are delocalised per atom.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Metal\"><strong>Magnesium<\/strong><\/td>\n                <td data-label=\"Ion commonly shown\">Mg<sup>2+<\/sup><\/td>\n                <td data-label=\"Delocalised electrons per atom\">2<\/td>\n                <td data-label=\"Expected bonding strength trend\">Stronger than sodium, because Mg<sup>2+<\/sup> attracts more delocalised electrons.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Metal\"><strong>Aluminium<\/strong><\/td>\n                <td data-label=\"Ion commonly shown\">Al<sup>3+<\/sup><\/td>\n                <td data-label=\"Delocalised electrons per atom\">3<\/td>\n                <td data-label=\"Expected bonding strength trend\">Usually stronger again, because Al<sup>3+<\/sup> has a higher charge and more delocalised electrons per atom.<\/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: Explain a Period 5 Contrast<\/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-604\" class=\"h5p-iframe\" data-content-id=\"604\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Metallic Bonding Explain: Strontium Compared with Rubidium\"><\/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: Accurate Statement or Common Mistake?<\/h2>\n<p>In each round, choose the one accurate statement to review the whole page.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-226\" class=\"h5p-iframe\" data-content-id=\"226\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Metallic Bonding Summary: Spot the Accurate Statement\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">6<\/div>\n          <h2>Common Exam Points<\/h2>\n        <\/div>\n\n        <p>Strong answers about metallic bonding must describe the correct particles and the correct force between them.<\/p>\n\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Say positive metal ions, not atoms<\/h3>\n            <p>In the metallic lattice, the particles in fixed positions are positive metal ions, not neutral metal atoms.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Say delocalised electrons<\/h3>\n            <p>The outer-shell electrons are delocalised and can move through the structure. This is central to metallic bonding and electrical conductivity.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Use electrostatic attraction<\/h3>\n            <p>Metallic bonding is an electrostatic force of attraction between oppositely charged particles: positive metal ions and delocalised electrons.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Link strength to attraction<\/h3>\n            <p>Stronger metallic bonding means stronger attraction between the positive ions and the delocalised electron sea.<\/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>Metallic bonding is the strong electrostatic attraction between positive metal ions and delocalised electrons. Metals form giant metallic lattices, not molecules. The stronger the attraction between the ions and electron sea, the stronger the metallic bonding.<\/p>\n\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Metallic bonding<\/h3>\n            <p>Electrostatic attraction between positive metal ions and delocalised electrons.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Giant metallic lattice<\/h3>\n            <p>A regular, closely packed arrangement of positive metal ions surrounded by delocalised electrons.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Delocalised electrons<\/h3>\n            <p>Outer-shell electrons that are free to move through the metal lattice.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Bonding strength<\/h3>\n            <p>Increases with stronger attraction, more delocalised electrons per atom, higher nuclear charge and smaller metal ion size.<\/p>\n          <\/div>\n        <\/div>\n      <\/article>\n\n            <section class=\"ols-faq-card\">\n        <h2>FAQs<\/h2>\n        <p>These are the key points students often confuse when revising metallic bonding.<\/p>\n\n        <div class=\"ols-faq-list\">\n          <div class=\"ols-faq-item\">\n            <h3>What is metallic bonding?<\/h3>\n            <p>Metallic bonding is the electrostatic force of attraction between positive metal ions and delocalised electrons.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>What is a giant metallic lattice?<\/h3>\n            <p>A giant metallic lattice is a regular, closely packed arrangement of positive metal ions surrounded by delocalised electrons.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Why are electrons in metals called delocalised?<\/h3>\n            <p>They are called delocalised because they are not fixed to one atom or one bond. They can move through the metallic lattice.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>What makes metallic bonding stronger?<\/h3>\n            <p>Metallic bonding becomes stronger when there is a stronger attraction between positive ions and delocalised electrons. This is affected by nuclear charge, ion size and the number of delocalised electrons per atom.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Why do metals conduct electricity?<\/h3>\n            <p>Metals conduct electricity because their delocalised electrons are mobile and can carry charge through the lattice when a potential difference is applied.<\/p>\n          <\/div>\n        <\/div>\n      <\/section>\n\n      <!-- author card (moved to the end, 10 Oct 2026) -->\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\">\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\"><\/path>\n              <\/svg>\n              View LinkedIn Profile\n            <\/a>\n          <\/div>\n        <\/div>\n\n\n      <section class=\"ols-related-card\">\n        <h2>Related Topics<\/h2>\n        <p>Use these pages to connect metallic bonding with ionic bonding, polarisation and covalent bonding in Topic 2.<\/p>\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\/metallic-bonding\/physical-properties-of-metals\/\">Physical Properties of Metals<\/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\/nature-of-ionic-bonding\/\">Nature of Ionic Bonding<\/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\/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\/nature-of-covalent-bonding\/\">Nature of Covalent Bonding<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/\">Topic 2 Bonding and Structure<\/a>\n        <\/div>\n      <\/section>\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\n      <div class=\"ols-lightbox-overlay ols-metallic-bonding-structure-9ch0-page-lb\" role=\"dialog\" aria-modal=\"true\" aria-label=\"Image lightbox\">\n        <button class=\"ols-lightbox-close\" aria-label=\"Close lightbox\">&times;<\/button>\n        <img decoding=\"async\" class=\"ols-lightbox-img\" src=\"\" alt=\"\">\n      <\/div>\n\n      <script>\n      (function(){\n        var wrap = document.querySelector('.ols-metallic-bonding-structure-9ch0-page');\n        if (!wrap) return;\n\n        var targets = wrap.querySelectorAll('.ols-lightbox-target');\n        var overlay = wrap.querySelector('.ols-lightbox-overlay');\n        var lbImg = wrap.querySelector('.ols-lightbox-img');\n        var closeBtn = wrap.querySelector('.ols-lightbox-close');\n\n        if (!overlay || !lbImg || !closeBtn) return;\n\n        targets.forEach(function(img){\n          img.addEventListener('click', function(){\n            lbImg.src = img.src;\n            lbImg.alt = img.alt || '';\n            overlay.classList.add('is-open');\n            document.body.style.overflow = 'hidden';\n          });\n        });\n\n        function closeLb(){\n          overlay.classList.remove('is-open');\n          document.body.style.overflow = '';\n          lbImg.src = '';\n          lbImg.alt = '';\n        }\n\n        closeBtn.addEventListener('click', closeLb);\n        overlay.addEventListener('click', function(e){\n          if (e.target === overlay) closeLb();\n        });\n        document.addEventListener('keydown', function(e){\n          if (e.key === 'Escape' && overlay.classList.contains('is-open')) closeLb();\n        });\n      })();\n      <\/script>\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\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/metallic-bonding-and-structure\/#webpage\",\n            \"url\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/metallic-bonding-and-structure\/\",\n            \"name\": \"Metallic Bonding and Structure - 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