{"id":4591,"date":"2026-05-30T06:12:58","date_gmt":"2026-05-30T05:12:58","guid":{"rendered":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/octahedral\/"},"modified":"2026-10-25T12:17:12","modified_gmt":"2026-10-25T12:17:12","slug":"octahedral","status":"publish","type":"page","link":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/octahedral\/","title":{"rendered":"Octahedral"},"content":{"rendered":"\n<section class=\"ols-revision-page ols-octahedral-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      --gold: #c9973a;\n      --grey-text: #667085;\n      --body-text: #1f2937;\n      --border: rgba(28, 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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 { 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 { 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: 210px; padding: 14px; }\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    }\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    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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\/shapes-of-molecules\/\">Shapes of Molecules<\/a> \/\n        <span>Octahedral<\/span>\n      <\/nav>\n\n      <header class=\"ols-title-card\">\n        <h1>Octahedral Molecular Shape<\/h1>\n        <p class=\"ols-page-intro\">A focused revision guide to the octahedral molecular shape, using SF<sub>6<\/sub> as the key example. This page explains why six bonding pairs and no lone pairs around a central atom produce a symmetrical arrangement with bond angles of 90&deg; and 180&deg;.<\/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: sf6-octahedral (swapped 26 Sep 2026) -->\n<!-- Copyright (c) 2026 Dr. Mohammed Al-Fatah, onlinelearningsystem.net. All rights reserved. -->\n<!-- 3D card: sf6-octahedral (rebuilt Oct 2026) -->\n<!-- Copyright (c) 2026 Dr. Mohammed Al-Fatah, onlinelearningsystem.net. 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border:1px solid rgba(28,36,75,0.18);\n}\n.ols-soct-001 .soct-key i.k-ball{border-radius:50%;}\n\n@media (max-width:760px){\n  .ols-soct-001{padding:26px; border-radius:22px;}\n  .ols-soct-001 h2.soct-title{font-size:20.5px;}\n  .ols-soct-001 p.soct-sub{font-size:13.5px;}\n  .ols-soct-001 .soct-stage{height:400px;}\n  .ols-soct-001 .soct-rowlab{min-width:100%;}\n  .ols-soct-001 .soct-seg button{padding:9px 13px; font-size:13px;}\n  .ols-soct-001 .soct-lab{font-size:10.5px; padding:4px 8px;}\n  .ols-soct-001 .soct-lab.l-part{font-size:9.5px; padding:3px 7px;}\n  .ols-soct-001 .soct-lab.l-read{font-size:12px; padding:5px 9px;}\n  .ols-soct-001 .soct-caption{font-size:10.5px; padding:5px 9px; max-width:64%;}\n  .ols-soct-001 .soct-badge{font-size:10.5px; padding:4px 9px;}\n  .ols-soct-001 .soct-badge.b-eq{font-size:11px;}\n  .ols-soct-001 .soct-badges{max-width:calc(100% - 28px);}\n  .ols-soct-001 .soct-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-soct-001 .soct-hint{display:none;}\n  .ols-soct-001 .soct-caption{max-width:calc(100% - 28px);}\n}\n@media (prefers-reduced-motion:reduce){\n  .ols-soct-001 .soct-seg button,.ols-soct-001 .soct-pill{transition:none;}\n}\n\n.ols-cc-soct-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-soct-001 a{color:#aab0c0; text-decoration:none;}\n.ols-cc-soct-001 a:hover{text-decoration:underline;}\n.ols-soct-001 .soct-seg button{display:inline-flex; align-items:center;}\n.ols-soct-001 .soct-seg button .soct-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-soct-001 .soct-seg button[aria-pressed=\"true\"] .soct-n{background:#ffffff; color:#2563eb;}\n<\/style>\n\n<div class=\"soct-head\">\n  <h2 class=\"soct-title\">Octahedral Shape of SF\u2086<\/h2>\n  <p class=\"soct-sub\">Choose a step to watch six electron pairs spread out round sulfur and to find the square plane, the 180\u00b0 axial pair and all twelve 90\u00b0 angles.<\/p>\n<\/div>\n\n<div class=\"soct-stage\" id=\"soctStage\">\n  <canvas class=\"soct-canvas\" id=\"soctCanvas\"><\/canvas>\n  <div class=\"soct-overlay\" id=\"soctOverlay\"><\/div>\n  <div class=\"soct-caption\" id=\"soctCaption\"><\/div>\n  <div class=\"soct-hint\" id=\"soctHint\">Drag to rotate<\/div>\n  <div class=\"soct-badges\" id=\"soctBadges\"><\/div>\n<\/div>\n\n<div class=\"soct-controls\">\n  <div class=\"soct-row\">\n    <span class=\"soct-rowlab\">Step<\/span>\n    <div class=\"soct-seg\" role=\"group\" aria-label=\"Step\">\n      <button type=\"button\" data-step=\"1\" aria-pressed=\"true\"><span class=\"soct-n\">1<\/span>Six pairs repel<\/button>\n      <button type=\"button\" data-step=\"2\" aria-pressed=\"false\"><span class=\"soct-n\">2<\/span>Square plane, 90\u00b0<\/button>\n      <button type=\"button\" data-step=\"3\" aria-pressed=\"false\"><span class=\"soct-n\">3<\/span>Axial pair, 180\u00b0<\/button>\n      <button type=\"button\" data-step=\"4\" aria-pressed=\"false\"><span class=\"soct-n\">4<\/span>All twelve 90\u00b0 angles<\/button>\n    <\/div>\n  <\/div>\n\n  <div class=\"soct-row\">\n    <span class=\"soct-rowlab\">View<\/span>\n    <button type=\"button\" class=\"soct-pill\" id=\"soctResetV\">Reset view<\/button>\n  <\/div>\n<\/div>\n\n<div class=\"soct-info\">\n  <h3 id=\"soctInfoTitle\"><\/h3>\n  <p id=\"soctInfoText\"><\/p>\n  <div class=\"soct-facts\" id=\"soctFacts\"><\/div>\n  <div class=\"soct-key\">\n    <span><i class=\"k-ball\" style=\"background:#e2c230\"><\/i>Sulfur<\/span>\n    <span><i class=\"k-ball\" style=\"background:#b8de6e\"><\/i>Fluorine<\/span>\n    <span><i class=\"\" style=\"background:rgba(70,128,220,0.45)\"><\/i>Electron pair (bonding)<\/span>\n    <span><i class=\"k-ball\" style=\"background:#fac828\"><\/i>Electron<\/span>\n    <span><i class=\"\" style=\"background:#c9961c\"><\/i>Bond angle \/ highlighted position<\/span>\n  <\/div>\n<\/div>\n\n<script src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/JS\/sf6-octahedral.js?v=20261025p\"><\/script>\n<\/section>\n\n<p class=\"ols-cc-soct-001\">&copy; Dr. Mohammed Al-Fatah &#8211; <a href=\"https:\/\/www.onlinelearningsystem.net\" target=\"_blank\" rel=\"noopener\">onlinelearningsystem.net<\/a><\/p>\n\n\n<style>\n  .ols-octahedral-9ch0-page .ols-spec-grid {\n    display: grid;\n    grid-template-columns: repeat(3, minmax(0, 1fr));\n    gap: 14px;\n    margin-top: 18px;\n  }\n  .ols-octahedral-9ch0-page .ols-spec-box {\n    background: #ffffff;\n    border: 1px solid var(--border);\n    border-radius: 18px;\n    padding: 18px;\n    box-shadow: var(--inner-shadow);\n  }\n  .ols-octahedral-9ch0-page .ols-spec-box strong {\n    display: block;\n    font-size: 15px;\n    color: var(--blue);\n    margin-bottom: 6px;\n  }\n  .ols-octahedral-9ch0-page .ols-spec-box span {\n    display: block;\n    font-size: 17px;\n    line-height: 1.55;\n    color: var(--body-text);\n    font-weight: 300;\n    overflow-wrap: anywhere;\n  }\n  .ols-octahedral-9ch0-page .ols-h5p-grid {\n    display: grid;\n    gap: 18px;\n    margin-top: 22px;\n  }\n  .ols-octahedral-9ch0-page .ols-h5p-frame {\n    margin-top: 0;\n  }\n  .ols-octahedral-9ch0-page .ols-formula {\n    white-space: nowrap;\n  }\n  @media (max-width: 760px) {\n    .ols-octahedral-9ch0-page .ols-spec-grid {\n      grid-template-columns: 1fr;\n    }\n  }\n<\/style>\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: Outer Electrons from the Group Number<\/h2>\n<p>Before you start, check that you can find an atom&#039;s outer-shell electrons and work out how many are left over as lone pairs.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"654\"><\/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 Octahedral Means<\/h2>\n        <\/div>\n        <p>An <strong>octahedral<\/strong> molecule has six atoms bonded to a central atom and no lone pairs on that central atom. The six bonding regions repel and arrange themselves as far apart as possible in three-dimensional space.<\/p>\n        <p>The key example for this page is <strong>SF<sub>6<\/sub><\/strong>. Sulfur is the central atom and forms six S-F bonds to six fluorine atoms.<\/p>\n\n        <div class=\"ols-spec-grid\">\n          <div class=\"ols-spec-box\">\n            <strong>Bonding pairs<\/strong>\n            <span>6 bonding pairs around the central atom<\/span>\n          <\/div>\n          <div class=\"ols-spec-box\">\n            <strong>Lone pairs<\/strong>\n            <span>0 lone pairs on the central atom<\/span>\n          <\/div>\n          <div class=\"ols-spec-box\">\n            <strong>Bond angles<\/strong>\n            <span>90&deg; between adjacent bonds and 180&deg; between opposite bonds<\/span>\n          <\/div>\n        <\/div>\n\n        <div class=\"ols-key-box\"><p><strong>Key idea:<\/strong> six bonding pairs and no lone pairs around a central atom give an octahedral shape.<\/p><\/div>\n      <\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Count the Electron Pairs in an Ion<\/h2>\n<p>Type the numbers to work out the bonding pairs and lone pairs around silicon in an ion you have not met on this page.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-200\" class=\"h5p-iframe\" data-content-id=\"200\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Octahedral Shape Fill in the Blanks: Counting the Electron Pairs in SiF\u2086\u00b2\u207b\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">2<\/div>\n          <h2>Why SF<sub>6<\/sub> Is Octahedral<\/h2>\n        <\/div>\n        <p>In SF<sub>6<\/sub>, the central sulfur atom is surrounded by six S-F bonding pairs. There are no lone pairs on the sulfur atom, so the six bonding regions arrange to minimise bonding pair-bonding pair repulsion.<\/p>\n        <p>Sulfur therefore has <strong>12 electrons<\/strong> in its outer shell. An atom in Period 3 or below can hold more than eight electrons in this way, which is why SF<sub>6<\/sub> exists.<\/p>\n<p>Oxygen is in Period 2 and is limited to eight, so there is no OF<sub>6<\/sub>.<\/p>\n        <p>The octahedral arrangement can be visualised as <strong>four fluorine atoms in a square plane<\/strong>, with one fluorine atom above the plane and one fluorine atom below the plane. This produces a symmetrical three-dimensional shape.<\/p>\n        <div class=\"ols-key-box\"><p><strong>How to count:<\/strong><\/p>\n<ol>\n<li>Start with the <strong>outer-shell electrons<\/strong> of the central atom.<\/li>\n<li>Add one electron for each negative charge and take one away for each positive charge.<\/li>\n<li>Each single bond uses one of those electrons and each double bond uses two. A double or triple bond still counts as <strong>one bonding region<\/strong>.<\/li>\n<li>Divide the electrons left over by two to get the lone pairs.<\/li>\n<\/ol>\n<p>In SF<sub>6<\/sub>: sulfur has <strong>6 outer-shell electrons<\/strong>, the molecule has no charge, and the six S-F single bonds use all six. None are left over, so there are no lone pairs. Six bonding regions and no lone pairs give an octahedral shape.<\/p><\/div>\n\n        <div class=\"ols-figure-card compact ols-zoom-figure\">\n          <button class=\"ols-figure-image ols-lightbox-trigger\" type=\"button\" data-ols-lightbox-src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/skel-P148-sf6-octahedral.svg\" data-ols-lightbox-alt=\"SF6 is octahedral: six bonding pairs, no lone pairs, bond angle 90\u00b0\" aria-label=\"Open SF6 octahedral diagram in full screen\">\n            <img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-cd-15-sf6-octahedral.svg\" alt=\"Octahedral SF\u2086 with two axial and four equatorial F atoms, a 90\u00b0 angle and the opposite 180\u00b0 pair marked\" width=\"980\" height=\"486\">\n          <\/button>\n          <div class=\"ols-figure-caption\">\n            <p>SF<sub>6<\/sub> has six bonding regions around sulfur. Four fluorine atoms lie in a square plane, with one fluorine above and one below the plane.<\/p>\n          <\/div>\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-29-countsf6.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-29-countsf6.jpg\" alt=\"Five-step electron-pair count for SF\u2086 giving six bonding regions and an octahedral 90\u00b0 shape, with PF\u2086\u207b as a second example\" data-fullscreen-src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-29-countsf6.jpg\">\n<\/a>\n<\/div>\n<div class=\"ols-figure-caption\"><p>Sulfur uses all 6 outer electrons in bonds: six regions and no lone pairs give an octahedral molecule.<\/p><\/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\">3<\/div>\n          <h2>Square Plane and Opposite Positions<\/h2>\n        <\/div>\n        <p>The octahedral shape has six positions around the central atom. Four bonding pairs lie in a square plane and two bonding pairs are positioned above and below this plane.<\/p>\n        <p>This produces two important bond angles. Adjacent bonds are <strong>90&deg;<\/strong> apart, while bonds directly opposite each other are <strong>180&deg;<\/strong> apart.<\/p>\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Four bonds in a square plane<\/h3>\n            <p>Four S-F bonds lie around sulfur in one plane. Each adjacent bond in this plane is 90&deg; from the next.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Two bonds above and below<\/h3>\n            <p>One S-F bond points above the square plane and one S-F bond points below it.<\/p>\n<p>All six positions are <strong>equivalent<\/strong>: any four bonds that lie in the same plane can be taken as the square plane. This is unlike a trigonal bipyramid, where the axial and equatorial positions are different.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Opposite bonds<\/h3>\n            <p>Pairs of opposite bonds are 180&deg; apart, giving a highly symmetrical arrangement.<\/p>\n          <\/div>\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-22-sixpairs.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-22-sixpairs.jpg\" alt=\"Octahedron key with SF\u2086, IF\u2085 and XeF\u2084 sketches: no, one and two opposite lone pairs, with bond angles\" data-fullscreen-src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-22-sixpairs.jpg\">\n<\/a>\n<\/div>\n<div class=\"ols-figure-caption\"><p>Six regions form an octahedron; one lone pair gives a square pyramid and two opposite lone pairs give a square plane.<\/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: How Many Angles?<\/h2>\n<p>Picture the octahedron in three dimensions and answer each question as quickly as you can.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-202\" class=\"h5p-iframe\" data-content-id=\"202\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Octahedral Shape Single Choice: Counting the Angles in TeF\u2086\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">4<\/div>\n          <h2>Octahedral Examples<\/h2>\n        <\/div>\n        <p>The octahedral shape is found when the central atom has six bonding pairs and no lone pairs. SF<sub>6<\/sub> is the key A Level Chemistry example.<\/p>\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Species<\/th>\n                <th>Central atom<\/th>\n                <th>Electron regions<\/th>\n                <th>Shape<\/th>\n                <th>Typical exam angles<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Species\">SF<sub>6<\/sub><\/td>\n                <td data-label=\"Central atom\">S<\/td>\n                <td data-label=\"Electron regions\">6 bonding regions, 0 lone pairs<\/td>\n                <td data-label=\"Shape\">Octahedral<\/td>\n                <td data-label=\"Typical exam angles\">90&deg; and 180&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">PF<sub>6<\/sub><sup>&#8211;<\/sup><\/td>\n                <td data-label=\"Central atom\">P<\/td>\n                <td data-label=\"Electron regions\">6 bonding regions, 0 lone pairs<\/td>\n                <td data-label=\"Shape\">Octahedral<\/td>\n                <td data-label=\"Typical exam angles\">90&deg; and 180&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">SiF<sub>6<\/sub><sup>2-<\/sup><\/td>\n                <td data-label=\"Central atom\">Si<\/td>\n                <td data-label=\"Electron regions\">6 bonding regions, 0 lone pairs<\/td>\n                <td data-label=\"Shape\">Octahedral<\/td>\n                <td data-label=\"Typical exam angles\">90&deg; and 180&deg;<\/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: Six Fluorines, but Is It Octahedral?<\/h2>\n<p>Count the electrons around each central atom to find the species that does not fit.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-201\" class=\"h5p-iframe\" data-content-id=\"201\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Octahedral Shape MCQ: The Hexafluoride That Is Not a Regular Octahedron\"><\/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\">5<\/div>\n          <h2>How to Explain Octahedral Shape in an Exam<\/h2>\n        <\/div>\n        <p>A full exam explanation should connect the number of bonding pairs to electron-pair repulsion, then state the shape and bond angles.<\/p>\n\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>1. Identify the central atom<\/h3>\n            <p>For SF<sub>6<\/sub>, the central atom is sulfur.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>2. Count bonding pairs and lone pairs<\/h3>\n            <p>Sulfur has six bonding pairs and no lone pairs around it.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>3. Apply electron-pair repulsion<\/h3>\n            <p>The six bonding pairs repel and arrange themselves as far apart as possible in three-dimensional space.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>4. State the shape and angles<\/h3>\n            <p>The molecule is octahedral with bond angles of 90&deg; between adjacent bonds and 180&deg; between opposite bonds.<\/p>\n          <\/div>\n        <\/div>\n\n        <div class=\"ols-definition-box\">\n          <p><strong>Exam answer model:<\/strong> SF<sub>6<\/sub> has six bonding pairs and no lone pairs around the central sulfur atom. The bonding pairs repel and arrange themselves as far apart as possible.<\/p>\n<p>Four fluorine atoms lie in a square plane, with one fluorine atom above and one below the plane. Therefore, SF<sub>6<\/sub> is octahedral, with bond angles of 90&deg; between adjacent bonds and 180&deg; between opposite bonds.<\/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: Spot the Sound Reasoning<\/h2>\n<p>In each round, choose the one statement that an examiner would accept.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-203\" class=\"h5p-iframe\" data-content-id=\"203\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Octahedral Shape Summary: Spot the Sound Reasoning\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card soft\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">6<\/div>\n          <h2>Common Exam Points<\/h2>\n        <\/div>\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Do not confuse octahedral with square planar<\/h3>\n            <p>Octahedral molecules have six bonding pairs around the central atom. Square planar molecules have four bonded atoms in one plane because <strong>two lone pairs<\/strong> occupy the other two octahedral positions.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Use both relevant bond angles<\/h3>\n            <p>For SF<sub>6<\/sub>, adjacent bonds are 90&deg; apart and opposite bonds are 180&deg; apart.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Count around the central atom only<\/h3>\n            <p>The shape is determined by bonding pairs and lone pairs around sulfur in SF<sub>6<\/sub>, not by the total number of atoms alone.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Use electron-pair repulsion language<\/h3>\n            <p>Explain that bonding pairs repel and arrange as far apart as possible. Since SF<sub>6<\/sub> has no lone pairs on sulfur, there is no lone-pair compression to discuss.<\/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        <p>The octahedral shape is produced when a central atom has <strong>six bonding pairs<\/strong> and <strong>no lone pairs<\/strong>. SF<sub>6<\/sub> has six S-F bonds arranged symmetrically, giving bond angles of <strong>90&deg;<\/strong> and <strong>180&deg;<\/strong>.<\/p>\n        <div class=\"ols-key-box\"><p><strong>Memory line:<\/strong> 6 bonding pairs + 0 lone pairs = octahedral = 90&deg; and 180&deg;.<\/p><\/div>\n      <\/article>\n<section class=\"ols-faq-card\">\n        <h2>FAQs<\/h2>\n        <p>Common questions about octahedral molecular shape.<\/p>\n        <div class=\"ols-faq-list\">\n          <div class=\"ols-faq-item\">\n            <h3>What is an octahedral molecular shape?<\/h3>\n            <p>An octahedral molecular shape forms when a central atom has six bonding pairs and no lone pairs. The bonding pairs arrange symmetrically with adjacent bonds at 90&deg; and opposite bonds at 180&deg;.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Why is SF<sub>6<\/sub> octahedral?<\/h3>\n            <p>SF<sub>6<\/sub> is octahedral because sulfur has six bonding pairs and no lone pairs around it. The six S-F bonding regions repel and arrange as far apart as possible.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>What are the bond angles in an octahedral molecule?<\/h3>\n            <p>The main bond angles are 90&deg; between adjacent bonds and 180&deg; between opposite bonds.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>How do I explain octahedral shape in an exam?<\/h3>\n            <p>State that the central atom has six bonding pairs and no lone pairs, explain that electron pairs repel and arrange as far apart as possible, then give the shape as octahedral with 90&deg; and 180&deg; bond angles.<\/p>\n          <\/div>\n        \n<div class=\"ols-faq-item\">\n<h3>How can sulfur form six bonds when it has only six outer-shell electrons?<\/h3>\n<p>Each S-F bond uses one sulfur electron and one fluorine electron, so six bonds use all six sulfur electrons. Sulfur ends with 12 electrons in its outer shell, which is possible because it is in Period 3.<\/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\"><path d=\"M4.98 3.5C4.98 4.88 3.86 6 2.48 6S0 4.88 0 3.5 1.12 1 2.48 1s2.5 1.12 2.5 2.5zM.5 8h4V24h-4V8zm7 0h3.8v2.2h.1c.5-.9 1.8-2.2 3.9-2.2 4.2 0 5 2.8 5 6.4V24h-4v-7.6c0-1.8 0-4.2-2.6-4.2s-3 2-3 4v7.8h-4V8z\"><\/path><\/svg>\n              View LinkedIn Profile\n            <\/a>\n          <\/div>\n        <\/div>\n\n\n      <section class=\"ols-related-card\">\n        <h2>Related Topics<\/h2>\n        <p>Use these pages to connect octahedral shape with 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\/shapes-of-molecules\/trigonal-bipyramidal\/\">Trigonal Bipyramidal<\/a>\n          <a class=\"ols-related-item\" 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>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/polar-molecules\/\">Polar &amp; Non-Polar Molecules<\/a>\n        <\/div>\n      <\/section>\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. 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