{"id":4597,"date":"2026-05-30T06:13:15","date_gmt":"2026-05-30T05:13:15","guid":{"rendered":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/physical-properties-of-metals\/"},"modified":"2026-10-25T12:13:46","modified_gmt":"2026-10-25T12:13:46","slug":"physical-properties-of-metals","status":"publish","type":"page","link":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/physical-properties-of-metals\/","title":{"rendered":"Physical Properties of Metals"},"content":{"rendered":"\n<section class=\"ols-revision-page ols-physical-properties-metals-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: #fff8e8;\n      --gold: #c9973a;\n      --grey-text: #667085;\n      --body-text: #1f2937;\n      --border: rgba(28, 36, 75, 0.14);\n      --shadow: 0 18px 45px rgba(28, 36, 75, 0.10);\n      --inner-shadow: 0 10px 26px rgba(28, 36, 75, 0.08);\n      font-family: Poppins, Arial, sans-serif;\n      color: var(--navy);\n      background: #ffffff;\n    }\n\n    .ols-revision-page * { box-sizing: border-box; }\n\n    .ols-physical-properties-metals-9ch0-page,\n    .ols-physical-properties-metals-9ch0-page .ols-main,\n    .ols-physical-properties-metals-9ch0-page .ols-note-card,\n    .ols-physical-properties-metals-9ch0-page .ols-zoom-card,\n    .ols-physical-properties-metals-9ch0-page .ols-zoom-card-image {\n      overflow: visible !important;\n    }\n\n    .ols-zoom-card {\n      position: relative;\n      z-index: 1;\n    }\n\n    .ols-zoom-card-image {\n      position: relative;\n      z-index: 2;\n    }\n\n    .ols-zoomable-img {\n      position: relative;\n      z-index: 3;\n      cursor: zoom-in;\n      transition: transform 0.28s ease, box-shadow 0.28s ease;\n      transform-origin: center center;\n    }\n\n    .ols-zoomable-img:hover {\n      transform: scale(1.08);\n      z-index: 80;\n      box-shadow: 0 24px 60px rgba(28,36,75,0.20);\n      border-radius: 18px;\n    }\n\n    .ols-lightbox-overlay {\n      display: none;\n      position: fixed;\n      inset: 0;\n      z-index: 99999;\n      background: rgba(0,0,0,0.88);\n      align-items: center;\n      justify-content: center;\n      padding: 24px;\n    }\n\n    .ols-lightbox-overlay.is-open {\n      display: flex;\n    }\n\n    .ols-lightbox-img {\n      max-width: 92vw;\n      max-height: 88vh;\n      border-radius: 12px;\n      box-shadow: 0 24px 60px rgba(0,0,0,0.5);\n      background: #ffffff;\n    }\n\n    .ols-lightbox-close {\n      position: absolute;\n      top: 20px;\n      right: 24px;\n      background: none;\n      border: none;\n      color: #ffffff;\n      font-size: 36px;\n      cursor: pointer;\n      line-height: 1;\n    }\n\n\n    .ols-main { min-width: 0; max-width: 970px; }\n    .ols-breadcrumbs { display: flex; flex-wrap: wrap; gap: 8px; margin: 10px 0 22px; font-size: 15px; color: var(--grey-text); }\n    .ols-breadcrumbs a, .ols-breadcrumbs span { color: var(--grey-text); text-decoration: none; font-weight: 600; }\n    .ols-breadcrumbs a:hover { color: var(--blue); text-decoration: underline; text-underline-offset: 3px; }\n\n    .ols-title-card, .ols-note-card, .ols-h5p-card, .ols-related-card, .ols-faq-card, .ols-quicksnap-card { background: #ffffff; border: 1px solid var(--border); border-radius: 28px; box-shadow: var(--shadow); padding: 34px; margin-bottom: 24px; overflow: hidden; }\n    .ols-title-card { background: linear-gradient(135deg, #ffffff 0%, #f8fbff 100%); }\n    .ols-title-card h1 { margin: 0 0 18px; font-size: clamp(36px, 5vw, 58px); line-height: 1.08; font-weight: 800; letter-spacing: -0.04em; color: #111827; }\n    .ols-page-intro { font-size: 19px; line-height: 1.7; font-weight: 300; color: var(--body-text); margin: 0 0 22px; }\n    .ols-badges { display: flex; flex-wrap: wrap; gap: 12px; margin-bottom: 22px; }\n    .ols-badge { display: inline-flex; align-items: center; padding: 9px 14px; border-radius: 999px; background: #ffffff; border: 1px solid var(--border); font-size: 15px; font-weight: 600; color: var(--navy); }\n\n    .ols-author { display: flex; align-items: center; gap: 20px; padding: 28px; border-radius: 28px; background: linear-gradient(135deg, #ffffff 0%, #f8fbff 100%); border: 1px solid rgba(28,36,75,0.12); box-shadow: 0 18px 45px rgba(28,36,75,0.10); margin-top: 22px; }\n    .ols-author-avatar-img { width: 92px; height: 92px; border-radius: 50%; object-fit: cover; object-position: center; flex-shrink: 0; border: 4px solid #ffffff; box-shadow: 0 14px 32px rgba(28,36,75,0.18), 0 0 0 1px rgba(28,36,75,0.10); transition: transform 0.25s ease, box-shadow 0.25s ease; }\n    .ols-author:hover .ols-author-avatar-img { transform: scale(1.04); box-shadow: 0 20px 42px rgba(28,36,75,0.22), 0 0 0 1px rgba(28,36,75,0.10); }\n    .ols-author-content { min-width: 0; }\n    .ols-author-title { margin: 0 0 4px; font-size: clamp(24px,3vw,34px); line-height: 1.15; font-weight: 700; color: var(--navy); letter-spacing: -0.03em; }\n    .ols-author-description { margin: 0; font-size: 17px; line-height: 1.7; font-weight: 300; color: var(--grey-text); }\n    .ols-linkedin-pill { display: inline-flex; align-items: center; justify-content: center; gap: 10px; margin-top: 16px; padding: 11px 18px; border-radius: 999px; background: linear-gradient(135deg,#0A66C2,#004182); color: #ffffff; text-decoration: none; font-size: 14px; line-height: 1; font-weight: 700; letter-spacing: 0.01em; box-shadow: 0 10px 22px rgba(10,102,194,0.24); position: relative; overflow: hidden; transition: transform 0.22s ease, box-shadow 0.22s ease; }\n    .ols-linkedin-pill::before { content: \"\"; position: absolute; top: 0; left: -120%; width: 100%; height: 100%; background: linear-gradient(120deg, rgba(255,255,255,0) 0%, rgba(255,255,255,0.28) 50%, rgba(255,255,255,0) 100%); transition: left 0.7s ease; }\n    .ols-linkedin-pill:hover { transform: translateY(-3px) scale(1.03); box-shadow: 0 16px 34px rgba(10,102,194,0.34), 0 0 0 6px rgba(10,102,194,0.10); color: #ffffff; }\n    .ols-linkedin-pill:hover::before { left: 120%; }\n    .ols-linkedin-icon { width: 18px; height: 18px; display: block; flex-shrink: 0; }\n\n    .ols-note-card.soft { background: linear-gradient(135deg, #ffffff 0%, var(--soft-red) 100%); }\n    .ols-note-card.purple { background: linear-gradient(135deg, #ffffff 0%, var(--soft-purple) 100%); }\n    .ols-note-card.orange { background: linear-gradient(135deg, #ffffff 0%, var(--soft-orange) 100%); }\n    .ols-note-card.gold { background: linear-gradient(135deg, #ffffff 0%, var(--soft-gold) 100%); }\n    .ols-note-title { display: flex; align-items: center; gap: 14px; margin-bottom: 20px; }\n    .ols-note-icon { width: 52px; height: 52px; border-radius: 16px; background: var(--navy); color: #ffffff; display: grid; place-items: center; font-size: 24px; font-weight: 800; flex-shrink: 0; }\n    .ols-note-title h2, .ols-h5p-card h2, .ols-related-card h2, .ols-faq-card h2, .ols-quicksnap-card h2 { margin: 0; font-size: clamp(28px, 3.5vw, 42px); line-height: 1.15; font-weight: 800; color: #111827; letter-spacing: -0.03em; }\n    .ols-h5p-card h2, .ols-related-card h2, .ols-faq-card h2, .ols-quicksnap-card h2 { margin-bottom: 14px; }\n    .ols-note-card p, .ols-note-card li { font-size: clamp(15px, 1.25vw, 17px); line-height: 1.65; font-weight: 300; color: var(--body-text); }\n    .ols-h5p-card p, .ols-related-card p, .ols-faq-card p, .ols-quicksnap-card p, .ols-quicksnap-card li { font-size: clamp(15px, 1.3vw, 18px); line-height: 1.65; font-weight: 300; color: var(--body-text); }\n    .ols-note-card strong, .ols-h5p-card strong, .ols-related-card strong, .ols-faq-card strong, .ols-quicksnap-card strong { font-weight: 700; color: var(--navy); }\n    .ols-note-card ul, .ols-note-card ol, .ols-quicksnap-card ul { margin: 0; padding-left: 22px; }\n\n    .ols-key-box { margin-top: 20px; background: var(--soft-green); border: 1px solid rgba(63, 143, 70, 0.25); border-radius: 20px; padding: 18px 20px; }\n    .ols-key-box p { margin: 0; font-weight: 400; color: var(--navy); }\n    .ols-definition-box { background: linear-gradient(135deg, #ffffff, var(--soft-purple)); border: 2px dashed rgba(122, 62, 157, 0.35); border-radius: 24px; padding: 22px 24px; margin-top: 22px; }\n    .ols-definition-box p { margin: 0; color: var(--navy); font-weight: 400; }\n    .ols-equation-box { background: #ffffff; border: 1px solid rgba(201,151,58,0.35); border-left: 5px solid var(--gold); border-radius: 20px; padding: 18px 20px; margin-top: 20px; box-shadow: var(--inner-shadow); }\n    .ols-equation-box p { margin: 0; font-size: 17px; line-height: 1.7; }\n\n    .ols-rule-list { display: grid; gap: 14px; margin-top: 18px; }\n    .ols-rule-item { background: #ffffff; border: 1px solid var(--border); border-left: 5px solid var(--blue); border-radius: 18px; padding: 18px; box-shadow: var(--inner-shadow); }\n    .ols-rule-item h3 { margin: 0 0 8px; font-size: 20px; line-height: 1.25; color: var(--navy); }\n    .ols-rule-item p { margin: 0; font-size: 15px; line-height: 1.6; }\n\n    .ols-property-grid { display: grid; grid-template-columns: repeat(2, minmax(0, 1fr)); gap: 16px; margin-top: 18px; }\n    .ols-property-box { background: #ffffff; border: 1px solid var(--border); border-radius: 20px; padding: 18px; box-shadow: var(--inner-shadow); }\n    .ols-property-box h3 { margin: 0 0 10px; color: var(--navy); font-size: 20px; line-height: 1.25; font-weight: 800; }\n    .ols-property-box p, .ols-property-box li { margin: 0; font-size: 15px; line-height: 1.6; color: var(--body-text); font-weight: 300; }\n\n    .ols-figure-card { margin: 26px auto 4px; border: 1px solid var(--border); border-radius: 26px; overflow: hidden; background: #ffffff; box-shadow: var(--inner-shadow); max-width: 100%; }\n    .ols-figure-card.medium { max-width: 820px; }\n    .ols-figure-card.compact { max-width: 700px; }\n    .ols-figure-card.wide { max-width: 940px; }\n    .ols-figure-image { width: 100%; min-height: 240px; display: flex; align-items: center; justify-content: center; background: #ffffff; padding: 20px; }\n    .ols-figure-image img { max-width: 100%; height: auto; display: block; }\n    .ols-figure-caption { padding: 18px 24px 22px; background: linear-gradient(135deg, #ffffff, #f8fbff); border-top: 1px solid var(--border); }\n    .ols-figure-caption p { margin: 0; color: #5f6b85; font-size: clamp(15px, 1.3vw, 17px); line-height: 1.6; font-weight: 300; font-style: italic; }\n\n    .ols-table-wrap { overflow: hidden; border-radius: 22px; border: 1px solid var(--border); background: #ffffff; margin-top: 18px; }\n    .ols-table { width: 100%; border-collapse: collapse; table-layout: fixed; }\n    .ols-table th { background: var(--navy); color: #ffffff; padding: 16px; text-align: left; font-size: clamp(14px, 1.2vw, 17px); font-weight: 600; overflow-wrap: anywhere; }\n    .ols-table td { padding: 16px; border-bottom: 1px solid var(--border); font-size: clamp(14px, 1.15vw, 16px); line-height: 1.45; color: var(--body-text); vertical-align: top; overflow-wrap: anywhere; }\n    .ols-table tr:last-child td { border-bottom: none; }\n\n    .ols-h5p-card { background: linear-gradient(135deg, #ffffff 0%, #f7f0ff 100%); }\n    .ols-h5p-frame { margin-top: 22px; padding: 18px; border-radius: 24px; background: #ffffff; border: 1px solid var(--border); box-shadow: inset 0 0 0 1px rgba(28, 36, 75, 0.03); }\n    .ols-h5p-stack { display: grid; gap: 18px; margin-top: 22px; }\n\n    .ols-quicksnap-card { background: linear-gradient(135deg, #ffffff 0%, #fff8e8 100%); }\n    .ols-quicksnap-grid { display: grid; grid-template-columns: repeat(2, minmax(0, 1fr)); gap: 14px; margin-top: 18px; }\n    .ols-quicksnap-item { background: #ffffff; border: 1px solid var(--border); border-left: 5px solid var(--gold); border-radius: 18px; padding: 18px; box-shadow: var(--inner-shadow); }\n    .ols-quicksnap-item h3 { margin: 0 0 8px; color: var(--navy); font-size: 18px; line-height: 1.25; font-weight: 800; }\n    .ols-quicksnap-item p { margin: 0; font-size: 15px; line-height: 1.6; }\n\n    .ols-faq-list { display: grid; gap: 14px; margin-top: 18px; }\n    .ols-faq-item { background: #ffffff; border: 1px solid var(--border); border-radius: 18px; padding: 18px 20px; box-shadow: var(--inner-shadow); }\n    .ols-faq-item h3 { margin: 0 0 8px; font-size: 20px; line-height: 1.3; color: var(--navy); }\n    .ols-faq-item p { margin: 0; font-size: 16px; line-height: 1.65; color: var(--body-text); }\n\n    .ols-related-grid { display: grid; grid-template-columns: repeat(3, minmax(0, 1fr)); gap: 16px; margin-top: 18px; }\n    .ols-related-item { border: 1px solid var(--border); border-radius: 18px; padding: 18px; background: #ffffff; color: var(--navy); text-decoration: none; font-weight: 600; line-height: 1.5; transition: transform 0.2s ease, box-shadow 0.2s ease; }\n    .ols-related-item:hover { transform: translateY(-2px); box-shadow: 0 10px 22px rgba(28, 36, 75, 0.08); }\n\n    .ols-attribution-card { 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-bottom: 24px; overflow: hidden; font-family: Poppins, Arial, sans-serif; box-sizing: border-box; }\n    .ols-attribution-card, .ols-attribution-card * { box-sizing: border-box; }\n    .ols-attribution-card p { margin: 0; font-size: 14px; line-height: 1.65; font-weight: 300; color: #667085; }\n    .ols-attribution-card strong { font-weight: 700; color: #1C244B; }\n\n    @media (max-width: 1050px) {\n      .ols-main { max-width: none; }\n      .ols-related-grid, .ols-property-grid, .ols-quicksnap-grid { grid-template-columns: repeat(2, minmax(0, 1fr)); }\n    }\n\n    @media (max-width: 760px) {\n      .ols-title-card, .ols-note-card, .ols-h5p-card, .ols-related-card, .ols-faq-card, .ols-attribution-card, .ols-quicksnap-card { padding: 24px 18px; border-radius: 22px; }\n      .ols-note-title { align-items: flex-start; }\n      .ols-figure-card { border-radius: 22px; }\n      .ols-figure-image { min-height: 190px; padding: 12px; }\n      .ols-figure-caption { padding: 16px; }\n      .ols-table-wrap { border: none; background: transparent; }\n      .ols-table, .ols-table thead, .ols-table tbody, .ols-table th, .ols-table td, .ols-table tr { display: block; width: 100%; }\n      .ols-table { border-collapse: separate; border-spacing: 0; }\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      .ols-zoomable-img:hover { transform: none; box-shadow: none; }\n    }\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', 'parent-active');\r\n    });\r\n\r\n    sidebar.querySelectorAll('a[data-ols-disabled-parent=\"1\"], a[aria-current]').forEach(function(a) {\r\n      a.removeAttribute('aria-current');\r\n      a.removeAttribute('tabindex');\r\n      a.removeAttribute('data-ols-disabled-parent');\r\n    });\r\n\r\n    links.forEach(function(a) {\r\n      try {\r\n        var href = a.getAttribute('href');\r\n        if (!href || href === '#' || href.charAt(0) === '#') return;\r\n        var linkPath = normalisePath(new URL(href, window.location.origin).pathname);\r\n        if (!linkPath) return;\r\n        if (currentPath === linkPath || currentPath.indexOf(linkPath + '\/') === 0) {\r\n          if (linkPath.length > matchedLength) {\r\n            matched = a;\r\n            matchedLength = linkPath.length;\r\n          }\r\n        }\r\n      } catch(e) {}\r\n    });\r\n\r\n    if (matched) {\r\n      var matchedLi = matched.closest('li');\r\n      var parentSub = matched.closest('.ols-subtopic-list');\r\n\r\n      if (parentSub) {\r\n        if (matchedLi) {\r\n          matchedLi.classList.add('active');\r\n          matched.setAttribute('aria-current', 'page');\r\n        }\r\n        var parentLi = parentSub.closest('li');\r\n        if (parentLi) {\r\n          parentLi.classList.add('parent-active', 'active-main');\r\n          var parentLink = parentLi.querySelector(':scope > a');\r\n          if (parentLink) {\r\n            parentLink.setAttribute('aria-current', 'true');\r\n            parentLink.setAttribute('tabindex', '-1');\r\n            parentLink.setAttribute('data-ols-disabled-parent', '1');\r\n          }\r\n        }\r\n      } else {\r\n        if (matchedLi) {\r\n          matchedLi.classList.add('parent-active', 'active-main');\r\n          matched.setAttribute('aria-current', 'page');\r\n          matched.setAttribute('tabindex', '-1');\r\n          matched.setAttribute('data-ols-disabled-parent', '1');\r\n        }\r\n      }\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\/metallic-bonding\/\">Metallic Bonding<\/a> \/\n        <span>Physical Properties of Metals<\/span>\n      <\/nav>\n\n      <header class=\"ols-title-card\">\n        <h1>Physical Properties of Metals<\/h1>\n        <p class=\"ols-page-intro\">A concise revision guide to the physical properties of metals, including high melting temperatures, electrical conductivity, thermal conductivity, malleability and ductility.<\/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\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: Spotting a Metal from Its Properties<\/h2>\n<p>Before you start, check that you can still recognise a metal from its GCSE properties.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"667\"><\/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>Why Metallic Bonding Explains Metal Properties<\/h2>\n        <\/div>\n\n        <p>Most physical properties of metals can be explained using the same model: a <strong>giant metallic lattice<\/strong> of <strong>positive metal ions<\/strong> surrounded by <strong>delocalised electrons<\/strong>.<\/p>\n        <p>The positive metal ions are arranged in regular layers. The delocalised electrons are mobile and spread throughout the structure, producing strong electrostatic attractions between the ions and the electron cloud.<\/p>\n\n        <div class=\"ols-definition-box\">\n          <p><strong>Key definition:<\/strong> Metallic bonding is the strong electrostatic attraction between positive metal ions and delocalised electrons.<\/p>\n        <\/div>\n\n        <div class=\"ols-key-box\">\n          <p><strong>Exam link:<\/strong> When explaining a metal property, always connect the property to either strong electrostatic attractions, mobile delocalised electrons, or layers of metal ions that can slide.<\/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>High Melting Temperatures<\/h2>\n        <\/div>\n\n        <p>Metals usually have <strong>high melting temperatures<\/strong> because there are strong electrostatic attractions between positive metal ions and delocalised electrons.<\/p>\n        <p>To melt a metal, these attractions must be partially overcome so that the metal ions can move out of their fixed lattice positions. Since metals have giant lattice structures, many strong attractions must be overcome.<\/p>\n\n        <div class=\"ols-property-grid\">\n          <div class=\"ols-property-box\">\n            <h3>Factors affecting melting temperature<\/h3>\n            <ul>\n              <li><strong>More delocalised electrons per ion<\/strong> usually produce stronger metallic bonding.<\/li>\n              <li>A <strong>higher charge-to-radius ratio<\/strong> gives stronger attraction between metal ions and delocalised electrons.<\/li>\n            <\/ul>\n          <\/div>\n          <div class=\"ols-property-box\">\n            <h3>Trends to remember<\/h3>\n            <ul>\n              <li><strong>Group 1 metals<\/strong> have relatively low melting temperatures.<\/li>\n              <li><strong>Group 2 metals<\/strong> usually have higher melting temperatures than Group 1 metals.<\/li>\n              <li><strong>Transition metals<\/strong> often have high melting temperatures because of strong metallic bonding.<\/li>\n            <\/ul>\n          <\/div>\n        <\/div>\n\n        <div class=\"ols-equation-box\">\n          <p><strong>Comparison:<\/strong> Magnesium has a higher melting temperature than sodium because Mg<sup>2+<\/sup> ions have a greater charge than Na<sup>+<\/sup> ions and magnesium contributes more delocalised electrons.<\/p>\n<p>The Mg<sup>2+<\/sup> ion is also smaller. This gives stronger metallic bonding. The melting temperature rises across Period 3 from sodium (98 \u00b0C) to magnesium (650 \u00b0C) to aluminium (660 \u00b0C).<\/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: Find the Error<\/h2>\n<p>Read the student&#039;s four-point explanation and decide which point is wrong.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-229\" class=\"h5p-iframe\" data-content-id=\"229\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Properties of Metals MCQ: Find the Error in a Calcium and Potassium Answer\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card purple\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">3<\/div>\n          <h2>Electrical Conductivity<\/h2>\n        <\/div>\n\n        <p>Metals conduct electricity because they contain <strong>delocalised electrons<\/strong> that are free to move throughout the lattice.<\/p>\n        <p>When a potential difference is applied, these mobile electrons move towards the positive terminal and carry charge through the metal. This movement of charge is an electric current.<\/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 electrical conductivity<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Factor\"><strong>Number of delocalised electrons<\/strong><\/td>\n                <td data-label=\"Effect on electrical conductivity\">Within a period, more delocalised electrons per atom means more mobile charge carriers, so conductivity increases from sodium to magnesium to aluminium. This is a trend within a period, not a rule for comparing any two metals.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Factor\"><strong>Charge density of metal ions<\/strong><\/td>\n                <td data-label=\"Effect on electrical conductivity\">Not a direct factor. The charge and size of the ions decide how strong the metallic bonding is, which affects melting temperature. Conductivity depends on the delocalised electrons and how freely they move.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Factor\"><strong>Impurities<\/strong><\/td>\n                <td data-label=\"Effect on electrical conductivity\">Impurities disrupt the regular lattice and scatter moving electrons, which can lower conductivity.<\/td>\n              <\/tr>\n            <\/tbody>\n          <\/table>\n        <\/div>\n\n        <div class=\"ols-key-box\">\n          <p><strong>Comparison:<\/strong> Across Period 3, electrical conductivity increases from sodium to magnesium to aluminium. Each sodium atom contributes one delocalised electron, magnesium two and aluminium three, so there are more charge carriers.<\/p>\n<p>The difference between sodium and magnesium is small; aluminium is clearly the best conductor of the three.<\/p>\n          <p><strong>Remember:<\/strong> a molten metal still contains delocalised electrons, so a metal conducts electricity as a liquid as well as a solid.<\/p>\n        <\/div>\n      <div class=\"ols-figure-card ols-zoom-pop\">\n<div class=\"ols-figure-image\">\n<a class=\"ols-image-fullscreen-link\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-12-metalconduct.jpg\" target=\"_blank\" rel=\"noopener\" aria-label=\"Open image fullscreen\">\n<img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-12-metalconduct.jpg\" alt=\"Delocalised electrons drifting towards the positive terminal and carrying heat along a metal bar, with melting values for Na, Mg and Al\" data-fullscreen-src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-12-metalconduct.jpg\">\n<\/a>\n<\/div>\n<div class=\"ols-figure-caption\"><p>Delocalised electrons drift towards the positive terminal to carry charge, and carry kinetic energy along the metal to conduct heat.<\/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: A Liquid Metal<\/h2>\n<p>Apply the model of metallic bonding to a metal that is liquid at room temperature.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-230\" class=\"h5p-iframe\" data-content-id=\"230\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Properties of Metals MCQ: What Carries the Current in Liquid Mercury?\"><\/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>Thermal Conductivity<\/h2>\n        <\/div>\n\n        <p>Metals conduct heat well because their delocalised electrons can move through the structure and transfer kinetic energy rapidly.<\/p>\n        <p>When thermal energy is supplied, delocalised electrons gain kinetic energy. They move through the lattice and transfer energy to other electrons and ions.<\/p>\n\n        <div class=\"ols-property-grid\">\n          <div class=\"ols-property-box\">\n            <h3>Main mechanism<\/h3>\n            <p>Delocalised electrons transfer kinetic energy quickly through the metal. Closely packed metal ions can also vibrate and pass energy through the lattice.<\/p>\n          <\/div>\n          <div class=\"ols-property-box\">\n            <h3>Effect of impurities<\/h3>\n            <p>Impurities disrupt both electron movement and lattice vibrations, reducing the efficiency of heat transfer.<\/p>\n          <\/div>\n        <\/div>\n\n        <div class=\"ols-equation-box\">\n          <p><strong>Comparison:<\/strong> Magnesium can transfer heat more effectively than sodium because it provides more delocalised electrons per atom, allowing more rapid transfer of kinetic energy.<\/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: Comparing Two Conductors<\/h2>\n<p>Complete the comparison of aluminium and potassium, two metals this page has not compared.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-228\" class=\"h5p-iframe\" data-content-id=\"228\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Properties of Metals Drag: Conductivity of Aluminium and Potassium\"><\/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>Malleability and Ductility<\/h2>\n        <\/div>\n\n        <p>Metals are <strong>malleable<\/strong>, meaning they can be hammered or shaped, and <strong>ductile<\/strong>, meaning they can be drawn into wires.<\/p>\n        <p>This is because the layers of positive metal ions can slide over each other without breaking the metallic structure. The delocalised electrons continue to attract the positive ions after the layers have moved.<\/p>\n\n        <div class=\"ols-property-grid\">\n          <div class=\"ols-property-box\">\n            <h3>Why layers can slide<\/h3>\n            <p>Metallic bonding is non-directional. There are no fixed individual bonds between specific pairs of ions, so layers can shift while attractions remain.<\/p>\n          <\/div>\n          <div class=\"ols-property-box\">\n            <h3>Why the structure does not shatter<\/h3>\n            <p>The delocalised electrons move with the ions and continue to hold the lattice together, preventing strong repulsion from breaking the structure apart.<\/p>\n          <\/div>\n        <\/div>\n\n        <div class=\"ols-figure-card wide ols-zoom-card\">\n          <div class=\"ols-figure-image 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\/09\/wave-51.jpg\" alt=\"Two-panel flat vector of metal layers before and after sliding, with labels for the force, the positive ions, the delocalised electrons and the unbroken structure\">\n          <\/div>\n          <div class=\"ols-figure-caption\">\n            <p>When a force is applied, layers of metal ions can slide while delocalised electrons continue to hold the metallic structure together.<\/p>\n          <\/div>\n        <\/div>\n      <\/article>\n<!-- 3D card: layers-under-stress (5 Oct 2026, Topics 1-5 upgrade) -->\n<!-- Copyright (c) 2026 Dr. Mohammed Al-Fatah, onlinelearningsystem.net. All rights reserved. -->\n<section class=\"ols-lyrs-001\" id=\"olsLyrs001\">\n<style>\n@import url('https:\/\/fonts.googleapis.com\/css2?family=Poppins:wght@300;400;500;600&display=swap');\n\n.ols-lyrs-001{\n  font-family:'Poppins',system-ui,-apple-system,'Segoe UI',Roboto,Helvetica,Arial,sans-serif;\n  color:#1C244B; background:#ffffff;\n  border:1px solid rgba(28,36,75,0.14);\n  border-radius:28px;\n  box-shadow:0 18px 45px rgba(28,36,75,0.10);\n  padding:44px; margin:26px auto; max-width:980px;\n  box-sizing:border-box; -webkit-font-smoothing:antialiased;\n}\n.ols-lyrs-001 *{box-sizing:border-box;}\n\n.ols-lyrs-001 .lyrs-head{margin:0 0 22px;}\n.ols-lyrs-001 h2.lyrs-title{\n  font-size:26px; line-height:1.25; font-weight:600; letter-spacing:-0.012em;\n  margin:0 0 9px; color:#1C244B;\n}\n.ols-lyrs-001 p.lyrs-sub{\n  font-size:14.5px; line-height:1.62; font-weight:300; color:#4a5270;\n  margin:0; max-width:66ch;\n}\n\n.ols-lyrs-001 .lyrs-stage{\n  position:relative; width:100%; height:540px;\n  background:#ffffff; border:1px solid rgba(28,36,75,0.12);\n  border-radius:18px; overflow:hidden;\n}\n.ols-lyrs-001 .lyrs-canvas{\n  display:block; width:100%; height:100%;\n  touch-action:none; cursor:grab; background:#ffffff;\n}\n.ols-lyrs-001 .lyrs-canvas.is-drag{cursor:grabbing;}\n.ols-lyrs-001 .lyrs-overlay{position:absolute; inset:0; pointer-events:none; overflow:hidden;}\n\n.ols-lyrs-001 .lyrs-lab{\n  position:absolute; left:0; top:0; transform:translate(-50%,-50%);\n  white-space:nowrap; font-size:12.5px; font-weight:500; line-height:1;\n  padding:5px 10px; background:rgba(255,255,255,0.93);\n  border:1px solid rgba(28,36,75,0.16); border-radius:999px;\n  color:#1C244B; will-change:transform;\n}\n.ols-lyrs-001 .lyrs-lab.l-sm{font-size:11.5px; color:#2f5f9a; border-color:rgba(70,125,190,0.45);}\n.ols-lyrs-001 .lyrs-lab.l-msg{font-weight:600; border-color:rgba(28,36,75,0.32);}\n.ols-lyrs-001 .lyrs-lab.l-ok{font-weight:600; border-color:rgba(47,158,87,0.8); color:#1f7a3a;}\n.ols-lyrs-001 .lyrs-lab.l-bad{font-weight:600; border-color:rgba(212,58,50,0.7); color:#b02a24;}\n.ols-lyrs-001 .lyrs-lab.l-e{font-size:11.5px; font-weight:600; border-color:rgba(201,150,28,0.75); color:#8a6410;}\n.ols-lyrs-001 .lyrs-lab.l-hot{font-size:11.5px; font-weight:600; border-color:rgba(214,110,40,0.75); color:#a4501a;}\n.ols-lyrs-001 .lyrs-lab.l-cool{font-size:11.5px; font-weight:600; border-color:rgba(60,120,200,0.7); color:#2a5a98;}\n\n.ols-lyrs-001 .lyrs-caption .c-ok{color:#1f7a3a;}\n.ols-lyrs-001 .lyrs-caption .c-bad{color:#b02a24;}\n.ols-lyrs-001 .lyrs-caption{\n  position:absolute; left:14px; top:14px; max-width:60%;\n  font-size:12px; font-weight:500; color:#4a5270; line-height:1.35;\n  background:rgba(255,255,255,0.92); padding:6px 12px;\n  border-radius:14px; border:1px solid rgba(28,36,75,0.12);\n}\n.ols-lyrs-001 .lyrs-hint{\n  position:absolute; right:14px; top:14px;\n  font-size:11.5px; font-weight:400; color:#8b92a8;\n  background:rgba(255,255,255,0.9); padding:5px 11px;\n  border-radius:999px; border:1px solid rgba(28,36,75,0.10);\n}\n.ols-lyrs-001 .lyrs-badges{\n  position:absolute; right:14px; bottom:14px; max-width:58%;\n  display:flex; flex-direction:column; align-items:flex-end; gap:6px;\n}\n.ols-lyrs-001 .lyrs-badge{\n  font-size:12px; font-weight:500; color:#1C244B; line-height:1.35; text-align:right;\n  background:rgba(255,255,255,0.95); padding:5px 12px;\n  border-radius:14px; border:1px solid rgba(28,36,75,0.22);\n}\n.ols-lyrs-001 .lyrs-badge.b-eq{font-size:13.5px; font-weight:600; border-color:rgba(201,150,28,0.75);}\n\n.ols-lyrs-001 .lyrs-controls{margin-top:20px; display:flex; flex-direction:column; gap:12px;}\n.ols-lyrs-001 .lyrs-row{display:flex; align-items:center; gap:10px; flex-wrap:wrap;}\n.ols-lyrs-001 .lyrs-rowlab{font-size:12px; font-weight:500; color:#6b7290; min-width:100px; flex:0 0 auto;}\n\n.ols-lyrs-001 .lyrs-seg{\n  display:inline-flex; border:1px solid rgba(28,36,75,0.16);\n  border-radius:12px; overflow:hidden; background:#fbfbfd; flex-wrap:wrap;\n}\n.ols-lyrs-001 .lyrs-seg button{\n  font-family:inherit; font-size:14px; font-weight:500; color:#3c4463;\n  background:transparent; border:0; border-right:1px solid rgba(28,36,75,0.12);\n  padding:9px 18px; cursor:pointer; transition:background .15s, color .15s;\n}\n.ols-lyrs-001 .lyrs-seg button:last-child{border-right:0;}\n.ols-lyrs-001 .lyrs-seg button:hover{background:rgba(37,99,235,0.06);}\n.ols-lyrs-001 .lyrs-seg button[aria-pressed=\"true\"]{background:#2563eb; color:#fff;}\n.ols-lyrs-001 .lyrs-seg button:focus-visible{outline:2px solid #2563eb; outline-offset:-2px;}\n\n.ols-lyrs-001 .lyrs-pill{\n  font-family:inherit; font-size:13px; font-weight:500; color:#3c4463;\n  background:#fbfbfd; border:1px solid rgba(28,36,75,0.16);\n  border-radius:999px; padding:8px 16px; cursor:pointer;\n  display:inline-flex; align-items:center; gap:8px;\n  transition:background .15s, border-color .15s, color .15s;\n}\n.ols-lyrs-001 .lyrs-pill:hover{border-color:rgba(37,99,235,0.4);}\n.ols-lyrs-001 .lyrs-pill:focus-visible{outline:2px solid #2563eb; outline-offset:2px;}\n\n.ols-lyrs-001 .lyrs-info{\n  margin-top:22px; padding:22px 24px;\n  border:1px solid rgba(28,36,75,0.12); border-radius:16px; background:#fbfbfd;\n}\n.ols-lyrs-001 .lyrs-info h3{margin:0 0 8px; font-size:15.5px; font-weight:600; color:#1C244B;}\n.ols-lyrs-001 .lyrs-info p{margin:0; font-size:14px; line-height:1.68; font-weight:300; color:#41496a; max-width:74ch;}\n.ols-lyrs-001 .lyrs-facts{\n  margin-top:16px; display:flex; gap:26px; flex-wrap:wrap;\n  padding-top:16px; border-top:1px solid rgba(28,36,75,0.10);\n}\n.ols-lyrs-001 .lyrs-fact{min-width:110px;}\n.ols-lyrs-001 .lyrs-fact span{display:block; font-size:11.5px; color:#7d8399; font-weight:400; margin-bottom:3px;}\n.ols-lyrs-001 .lyrs-fact strong{display:block; font-size:15px; font-weight:600; color:#1C244B;}\n\n.ols-lyrs-001 .lyrs-key{\n  margin-top:16px; display:flex; gap:20px; flex-wrap:wrap;\n  font-size:12.5px; font-weight:400; color:#5a6180;\n}\n.ols-lyrs-001 .lyrs-key i{\n  display:inline-block; width:13px; height:13px; border-radius:3px;\n  margin-right:7px; vertical-align:-2px; border:1px solid rgba(28,36,75,0.18);\n}\n\n@media (max-width:760px){\n  .ols-lyrs-001{padding:26px; border-radius:22px;}\n  .ols-lyrs-001 h2.lyrs-title{font-size:20.5px;}\n  .ols-lyrs-001 p.lyrs-sub{font-size:13.5px;}\n  .ols-lyrs-001 .lyrs-stage{height:400px;}\n  .ols-lyrs-001 .lyrs-rowlab{min-width:100%;}\n  .ols-lyrs-001 .lyrs-seg button{padding:9px 13px; font-size:13px;}\n  .ols-lyrs-001 .lyrs-lab{font-size:10.5px; padding:4px 8px;}\n  .ols-lyrs-001 .lyrs-lab.l-sm,.ols-lyrs-001 .lyrs-lab.l-e,.ols-lyrs-001 .lyrs-lab.l-hot,.ols-lyrs-001 .lyrs-lab.l-cool{font-size:9.5px; padding:3px 7px;}\n  .ols-lyrs-001 .lyrs-caption{font-size:10.5px; padding:5px 9px; max-width:64%;}\n  .ols-lyrs-001 .lyrs-badge{font-size:10.5px; padding:4px 9px;}\n  .ols-lyrs-001 .lyrs-badge.b-eq{font-size:11px;}\n  .ols-lyrs-001 .lyrs-badges{max-width:calc(100% - 28px);}\n  .ols-lyrs-001 .lyrs-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-lyrs-001 .lyrs-hint{display:none;}\n  .ols-lyrs-001 .lyrs-caption{max-width:calc(100% - 28px);}\n}\n@media (prefers-reduced-motion:reduce){\n  .ols-lyrs-001 .lyrs-seg button,.ols-lyrs-001 .lyrs-pill{transition:none;}\n}\n\n.ols-cc-lyrs-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-lyrs-001 a{color:#aab0c0; text-decoration:none;}\n.ols-cc-lyrs-001 a:hover{text-decoration:underline;}\n.ols-lyrs-001 .lyrs-seg button{display:inline-flex; align-items:center;}\n.ols-lyrs-001 .lyrs-seg button .lyrs-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-lyrs-001 .lyrs-seg button[aria-pressed=\"true\"] .lyrs-n{background:#ffffff; color:#2563eb;}\n<\/style>\n\n<div class=\"lyrs-head\">\n  <h2 class=\"lyrs-title\">Layers Under Stress: Ionic Crystal v Metal<\/h2>\n  <p class=\"lyrs-sub\">Choose a step to watch the same force push one layer of ions along, first in an ionic crystal and then in a metal.<\/p>\n<\/div>\n\n<div class=\"lyrs-stage\" id=\"lyrsStage\">\n  <canvas class=\"lyrs-canvas\" id=\"lyrsCanvas\"><\/canvas>\n  <div class=\"lyrs-overlay\" id=\"lyrsOverlay\"><\/div>\n  <div class=\"lyrs-caption\" id=\"lyrsCaption\"><\/div>\n  <div class=\"lyrs-hint\" id=\"lyrsHint\">Drag to rotate<\/div>\n  <div class=\"lyrs-badges\" id=\"lyrsBadges\"><\/div>\n<\/div>\n\n<div class=\"lyrs-controls\">\n  <div class=\"lyrs-row\">\n    <span class=\"lyrs-rowlab\">Step<\/span>\n    <div class=\"lyrs-seg\" role=\"group\" aria-label=\"Step\">\n      <button type=\"button\" data-step=\"1\" aria-pressed=\"true\"><span class=\"lyrs-n\">1<\/span>Force on an ionic crystal<\/button>\n      <button type=\"button\" data-step=\"2\" aria-pressed=\"false\"><span class=\"lyrs-n\">2<\/span>A layer slides one ion<\/button>\n      <button type=\"button\" data-step=\"3\" aria-pressed=\"false\"><span class=\"lyrs-n\">3<\/span>Like charges repel: it cleaves<\/button>\n      <button type=\"button\" data-step=\"4\" aria-pressed=\"false\"><span class=\"lyrs-n\">4<\/span>The same force on a metal<\/button>\n      <button type=\"button\" data-step=\"5\" aria-pressed=\"false\"><span class=\"lyrs-n\">5<\/span>Layers slide, metal bends<\/button>\n    <\/div>\n  <\/div>\n\n  <div class=\"lyrs-row\">\n    <span class=\"lyrs-rowlab\">View<\/span>\n    <button type=\"button\" class=\"lyrs-pill\" id=\"lyrsResetV\">Reset view<\/button>\n  <\/div>\n<\/div>\n\n<div class=\"lyrs-info\">\n  <h3 id=\"lyrsInfoTitle\"><\/h3>\n  <p id=\"lyrsInfoText\"><\/p>\n  <div class=\"lyrs-facts\" id=\"lyrsFacts\"><\/div>\n  <div class=\"lyrs-key\">\n    <span><i style=\"background:#8c52c4\"><\/i>Positive ion (Na\u207a)<\/span>\n    <span><i style=\"background:#34aa48\"><\/i>Negative ion (Cl\u207b)<\/span>\n    <span><i style=\"background:#a8adb8\"><\/i>Metal ion<\/span>\n    <span><i style=\"background:#f6c424\"><\/i>Delocalised electron<\/span>\n    <span><i style=\"background:#d43a32\"><\/i>Force<\/span>\n  <\/div>\n<\/div>\n\n<script src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/JS\/layers-under-stress.js?v=20261025p\"><\/script>\n<\/section>\n\n<p class=\"ols-cc-lyrs-001\">&copy; Dr. Mohammed Al-Fatah &#8211; <a href=\"https:\/\/www.onlinelearningsystem.net\" target=\"_blank\" rel=\"noopener\">onlinelearningsystem.net<\/a><\/p>\n\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Explain Foil and an Alloy<\/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-231\" class=\"h5p-iframe\" data-content-id=\"231\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Properties of Metals Explain: Aluminium Foil and a Harder Aluminium Alloy\"><\/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: Which Explanation Is Accurate?<\/h2>\n<p>In each round, pick the one statement that explains the property correctly.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-668\" class=\"h5p-iframe\" data-content-id=\"668\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Properties of Metals Summary: Spot the Accurate Explanation\"><\/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>Exam questions often ask students to explain properties using bonding and structure. The strongest answers use clear cause-and-effect language.<\/p>\n\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Property<\/th>\n                <th>What to mention<\/th>\n                <th>Common mistake<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Property\"><strong>High melting temperature<\/strong><\/td>\n                <td data-label=\"What to mention\">Strong electrostatic attractions between positive metal ions and delocalised electrons require a large amount of energy to overcome.<\/td>\n                <td data-label=\"Common mistake\">Saying metals have strong intermolecular forces. Metals do not exist as simple molecules.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Property\"><strong>Electrical conductivity<\/strong><\/td>\n                <td data-label=\"What to mention\">Delocalised electrons are mobile and can carry charge through the lattice.<\/td>\n                <td data-label=\"Common mistake\">Saying the metal ions move to carry charge. In the solid metal, the ions are fixed in lattice positions.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Property\"><strong>Thermal conductivity<\/strong><\/td>\n                <td data-label=\"What to mention\">Delocalised electrons gain kinetic energy and transfer it rapidly through the lattice.<\/td>\n                <td data-label=\"Common mistake\">Only saying particles vibrate. In metals, mobile electrons are a major reason for efficient heat transfer.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Property\"><strong>Malleability and ductility<\/strong><\/td>\n                <td data-label=\"What to mention\">Layers of positive metal ions can slide while delocalised electrons continue to attract them.<\/td>\n                <td data-label=\"Common mistake\">Saying metallic bonds break completely when the metal is bent. The structure can deform without shattering.<\/td>\n              <\/tr>\n            <\/tbody>\n          <\/table>\n        <\/div>\n      <\/article>\n\n      \n\n      <section class=\"ols-quicksnap-card\">\n        <h2>QuickSnap<\/h2>\n        <p>Use this summary to connect each property to the correct metallic bonding explanation.<\/p>\n        <div class=\"ols-quicksnap-grid\">\n          <div class=\"ols-quicksnap-item\">\n            <h3>High melting temperatures<\/h3>\n            <p>Strong electrostatic attractions between positive metal ions and delocalised electrons require a large amount of energy to overcome.<\/p>\n          <\/div>\n          <div class=\"ols-quicksnap-item\">\n            <h3>Electrical conductivity<\/h3>\n            <p>Mobile delocalised electrons carry charge through the metal when a potential difference is applied.<\/p>\n          <\/div>\n          <div class=\"ols-quicksnap-item\">\n            <h3>Thermal conductivity<\/h3>\n            <p>Delocalised electrons transfer kinetic energy rapidly through the lattice.<\/p>\n          <\/div>\n          <div class=\"ols-quicksnap-item\">\n            <h3>Malleability and ductility<\/h3>\n            <p>Layers of metal ions can slide while delocalised electrons continue to hold the structure together.<\/p>\n          <\/div>\n        <\/div>\n      <\/section>\n\n      <section class=\"ols-faq-card\">\n        <h2>FAQs<\/h2>\n        <p>These are the key points students often confuse when revising the physical properties of metals.<\/p>\n\n        <div class=\"ols-faq-list\">\n          <div class=\"ols-faq-item\">\n            <h3>Why do metals have high melting temperatures?<\/h3>\n            <p>Metals have high melting temperatures because strong electrostatic attractions between positive metal ions and delocalised electrons require a large amount of energy to overcome.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Why do metals conduct electricity?<\/h3>\n            <p>Metals conduct electricity because delocalised electrons are mobile and can carry charge through the metallic lattice when a potential difference is applied.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Why do metals conduct heat?<\/h3>\n            <p>Metals conduct heat because delocalised electrons gain kinetic energy and transfer it rapidly through the lattice. Vibrating metal ions can also transfer energy.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Why are metals malleable?<\/h3>\n            <p>Metals are malleable because layers of positive metal ions can slide over each other while delocalised electrons continue to attract the ions and hold the structure together.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Why is magnesium generally stronger in metallic bonding than sodium?<\/h3>\n            <p>Magnesium forms Mg<sup>2+<\/sup> ions and contributes two delocalised electrons per atom, whereas sodium forms Na<sup>+<\/sup> ions and contributes one. This gives magnesium stronger electrostatic attractions in the metallic lattice.<\/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 the physical properties of metals with ionic bonding, metallic bonding and the wider Topic 2 bonding and structure content.<\/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\/metallic-bonding-and-structure\/\">Metallic Bonding and Structure<\/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<div class=\"ols-lightbox-overlay ols-physical-properties-metals-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-physical-properties-metals-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\/physical-properties-of-metals\/#webpage\",\n            \"url\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/physical-properties-of-metals\/\",\n            \"name\": \"Physical Properties of Metals - Edexcel A Level Chemistry\",\n            \"description\": \"Edexcel A Level Chemistry revision notes on the physical properties of metals, including high melting points, electrical conductivity, thermal conductivity, malleability and ductility.\",\n            \"inLanguage\": \"en-GB\",\n            \"isPartOf\": {\n                \"@type\": \"WebSite\",\n                \"@id\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/#website\",\n                \"name\": \"Online Learning System\",\n                \"url\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/\"\n            },\n            \"author\": {\n                \"@type\": \"Person\",\n                \"name\": \"Dr. Mohammed Al-Fatah\",\n                \"url\": \"https:\/\/www.linkedin.com\/in\/doctormohammedfatah\/\"\n            },\n            \"publisher\": {\n                \"@type\": \"Organization\",\n                \"name\": \"Online Learning System\",\n                \"url\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/\"\n            },\n            \"about\": [\n                {\n                    \"@type\": \"Thing\",\n                    \"name\": \"Physical properties of metals\"\n                },\n                {\n                    \"@type\": \"Thing\",\n                    \"name\": \"Metallic bonding\"\n                },\n                {\n                    \"@type\": \"Thing\",\n                    \"name\": \"Delocalised electrons\"\n                },\n                {\n                    \"@type\": \"Thing\",\n                    \"name\": \"Electrical conductivity\"\n                },\n                {\n                    \"@type\": \"Thing\",\n                    \"name\": \"Malleability\"\n                }\n            ]\n        },\n        {\n            \"@type\": \"BreadcrumbList\",\n            \"@id\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/physical-properties-of-metals\/#breadcrumb\",\n            \"itemListElement\": [\n                {\n                    \"@type\": \"ListItem\",\n                    \"position\": 1,\n                    \"name\": \"Revision Notes\",\n                    \"item\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/\"\n                },\n                {\n                    \"@type\": \"ListItem\",\n                    \"position\": 2,\n                    \"name\": \"A Level Chemistry\",\n                    \"item\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/\"\n                },\n                {\n                    \"@type\": \"ListItem\",\n                    \"position\": 3,\n                    \"name\": \"Edexcel\",\n                    \"item\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/\"\n                },\n                {\n                    \"@type\": \"ListItem\",\n                    \"position\": 4,\n                    \"name\": \"Topic 2 Bonding and Structure\",\n                    \"item\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/\"\n                },\n                {\n                    \"@type\": \"ListItem\",\n                    \"position\": 5,\n                    \"name\": \"Metallic Bonding\",\n                    \"item\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/\"\n                },\n                {\n                    \"@type\": \"ListItem\",\n                    \"position\": 6,\n                    \"name\": \"Physical Properties of Metals\",\n                    \"item\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/physical-properties-of-metals\/\"\n                }\n            ]\n        },\n        {\n            \"@type\": \"Course\",\n            \"@id\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/product\/metallic-bonding-edexcel-a-level-chemistry\/#course\",\n            \"name\": \"Metallic Bonding - Edexcel A Level Chemistry Course\",\n            \"description\": \"A guided Edexcel A Level Chemistry course covering metallic bonding, metallic structure, physical properties of metals, exam-style questions and progress tracking.\",\n            \"url\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/product\/metallic-bonding-edexcel-a-level-chemistry\/\",\n            \"provider\": {\n                \"@type\": \"Organization\",\n                \"name\": \"Online Learning System\",\n                \"url\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/\"\n            }\n        },\n        {\n            \"@type\": \"FAQPage\",\n            \"@id\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/physical-properties-of-metals\/#faq\",\n            \"mainEntity\": [\n                {\n                    \"@type\": \"Question\",\n                    \"name\": \"Why do metals have high melting temperatures?\",\n                    \"acceptedAnswer\": {\n                        \"@type\": \"Answer\",\n                        \"text\": \"Metals have high melting temperatures because strong electrostatic attractions between positive metal ions and delocalised electrons require a large amount of energy to overcome.\"\n                    }\n                },\n                {\n                    \"@type\": \"Question\",\n                    \"name\": \"Why do metals conduct electricity?\",\n                    \"acceptedAnswer\": {\n                        \"@type\": \"Answer\",\n                        \"text\": \"Metals conduct electricity because delocalised electrons are mobile and can carry charge through the metallic lattice when a potential difference is applied.\"\n                    }\n                },\n                {\n                    \"@type\": \"Question\",\n                    \"name\": \"Why do metals conduct heat?\",\n                    \"acceptedAnswer\": {\n                        \"@type\": \"Answer\",\n                        \"text\": \"Metals conduct heat because delocalised electrons gain kinetic energy and transfer it rapidly through the lattice. Vibrating metal ions can also transfer energy.\"\n                    }\n                },\n                {\n                    \"@type\": \"Question\",\n                    \"name\": \"Why are metals malleable?\",\n                    \"acceptedAnswer\": {\n                        \"@type\": \"Answer\",\n                        \"text\": \"Metals are malleable because layers of positive metal ions can slide over each other while delocalised electrons continue to attract the ions and hold the structure together.\"\n                    }\n                },\n                {\n                    \"@type\": \"Question\",\n                    \"name\": \"Why is magnesium generally stronger in metallic bonding than sodium?\",\n                    \"acceptedAnswer\": {\n                        \"@type\": \"Answer\",\n                        \"text\": \"Magnesium forms Mg2+ ions and contributes two delocalised electrons per atom, whereas sodium forms Na+ ions and contributes one. This gives magnesium stronger electrostatic attractions in the metallic lattice.\"\n                    }\n                }\n            ]\n        },\n        {\n            \"@type\": \"ImageObject\",\n            \"@id\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/wave-51.jpg#image\",\n            \"url\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/wave-51.jpg\",\n            \"name\": \"Layers of metal ions sliding in a metallic lattice\",\n            \"description\": \"A diagram showing layers of positive metal ions sliding over each other while delocalised electrons hold the metallic structure together.\"\n        }\n    ]\n}\n<\/script>\n    <\/main>\n<\/section>\n\n","protected":false},"excerpt":{"rendered":"<p>Revision Notes \/ A Level Chemistry \/ Edexcel \/ Topic 2 Bonding and Structure \/ Metallic Bonding \/ Physical Properties of Metals Physical Properties of Metals A concise revision guide to the physical properties of metals, including high melting temperatures, electrical conductivity, thermal conductivity, malleability and ductility. Unit: Paper 1 Topic 2: Bonding and Structure [&hellip;]<\/p>\n","protected":false},"author":12,"featured_media":0,"parent":4574,"menu_order":1,"comment_status":"closed","ping_status":"closed","template":"","meta":{"footnotes":""},"class_list":["post-4597","page","type-page","status-publish","hentry"],"_links":{"self":[{"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages\/4597","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=4597"}],"version-history":[{"count":2,"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages\/4597\/revisions"}],"predecessor-version":[{"id":24777,"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages\/4597\/revisions\/24777"}],"up":[{"embeddable":true,"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages\/4574"}],"wp:attachment":[{"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/media?parent=4597"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}