{"id":4573,"date":"2026-05-30T06:09:13","date_gmt":"2026-05-30T05:09:13","guid":{"rendered":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/polar-molecules\/"},"modified":"2026-10-25T12:07:53","modified_gmt":"2026-10-25T12:07:53","slug":"polar-molecules","status":"publish","type":"page","link":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/polar-molecules\/","title":{"rendered":"Polar Molecules"},"content":{"rendered":"\n<section class=\"ols-revision-page ols-polar-nonpolar-molecules-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, 36, 75, 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26px 22px; font-weight: 700; color: #7a4b12; text-align: center; line-height: 1.6; }\n    .ols-figure-placeholder .ols-figure-image { background: transparent; }\n    .ols-figure-placeholder { background: #ffffff; border: 1px solid rgba(28, 36, 75, 0.12); border-radius: 22px; padding: 14px; margin: 18px 0 6px; }\n    .ols-figure-placeholder .ols-figure-caption p { margin: 10px 0 0; font-size: 14px; color: #667085; text-align: center; }\n<\/style>\n\n  <aside class=\"ols-sidebar\">\r\n  <div class=\"ols-sidebar-header\">\r\n    <h3>Revision Notes<\/h3>\r\n    <p>A Level Chemistry<\/p>\r\n  <\/div>\r\n\r\n  <div class=\"ols-topic-group\">\r\n    <h4>Topic 2 Bonding and Structure<\/h4>\r\n\r\n    <ul class=\"ols-topic-list\">\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/ionic-bonding\/\">Ionic Bonding<\/a>\r\n\r\n        <ul class=\"ols-subtopic-list\">\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/ionic-bonding\/nature-of-ionic-bonding\/\">Nature of Ionic Bonding<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/ionic-bonding\/polarisation-of-ions\/\">Polarisation of Ions<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/ionic-bonding\/physical-properties-of-ionic-compounds\/\">Physical Properties of Ionic Compounds<\/a>\r\n          <\/li>\r\n        <\/ul>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/covalent-bonding\/\">Covalent Bonding<\/a>\r\n\r\n        <ul class=\"ols-subtopic-list\">\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/covalent-bonding\/nature-of-covalent-bonding\/\">Nature of Covalent Bonding<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/covalent-bonding\/dative-covalent-bonding\/\">Dative Covalent Bonding<\/a>\r\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/covalent-bonding\/giant-covalent-structures\/\">Giant Covalent Structures<\/a>\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/covalent-bonding\/electronegativity\/\">Electronegativity<\/a>\r\n          <\/li>\r\n        <\/ul>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/\">Shapes of Molecules<\/a>\r\n\r\n        <ul class=\"ols-subtopic-list\">\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/linear\/\">Linear<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/trigonal-planar\/\">Trigonal Planar<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/tetrahedral\/\">Tetrahedral<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/trigonal-pyramidal\/\">Trigonal Pyramidal<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/bent\/\">Bent<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/trigonal-bipyramidal\/\">Trigonal Bipyramidal<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/octahedral\/\">Octahedral<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/square-planar\/\">Square Planar<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/square-pyramidal\/\">Square Pyramidal<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/distorted-t\/\">Distorted T<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/seesaw\/\">SeeSaw<\/a>\r\n          <\/li>\r\n        <\/ul>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/polar-molecules\/\">Polar Molecules<\/a>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/\">Metallic Bonding<\/a>\r\n\r\n        <ul class=\"ols-subtopic-list\">\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/metallic-bonding-and-structure\/\">Metallic Bonding and Structure<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/physical-properties-of-metals\/\">Physical Properties of Metals<\/a>\r\n          <\/li>\r\n        <\/ul>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/\">Intermolecular Forces<\/a>\n        <ul class=\"ols-subtopic-list\">\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/london-forces\/\">London Forces<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/permanent-dipole-dipole-forces\/\">Permanent Dipole-Dipole Forces<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/hydrogen-bonding\/\">Hydrogen Bonding<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/anomalous-properties-of-water\/\">Anomalous Properties of Water<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/boiling-temperature-trends\/\">Boiling Temperature Trends<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/choosing-solvents\/\">Choosing Solvents<\/a>\n          <\/li>\n        <\/ul>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/structure-types\/\">Structure Types<\/a>\r\n      <\/li>\r\n\r\n    <\/ul>\r\n  <\/div>\r\n\r\n  <div class=\"ols-topic-group\">\r\n    <h4>Next Topics<\/h4>\r\n\r\n    <ul class=\"ols-topic-list\">\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-3-redox-i\/\">Redox I<\/a>\r\n      <\/li>\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-4-inorganic-chemistry-and-the-periodic-table\/\">Inorganic Chemistry &amp; The Periodic Table<\/a>\r\n      <\/li>\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-5-formulae-equations-and-amounts-of-substance\/\">Formulae, Equations &amp; Amounts<\/a>\r\n      <\/li>\r\n    <\/ul>\r\n  <\/div>\r\n<\/aside>\r\n\r\n<script>\r\n(function() {\r\n  function normalisePath(path) {\r\n    return String(path || '')\r\n      .split('?')[0]\r\n      .split('#')[0]\r\n      .replace(\/\\\/+$\/, '')\r\n      .toLowerCase();\r\n  }\r\n\r\n  function highlightActive() {\r\n    var sidebar = document.querySelector('.ols-sidebar');\r\n    if (!sidebar) return false;\r\n\r\n    var currentPath = normalisePath(window.location.pathname);\r\n    var links = sidebar.querySelectorAll('a[href]');\r\n    var matched = null;\r\n    var matchedLength = 0;\r\n\r\n    sidebar.querySelectorAll('.active, .active-main, .parent-active').forEach(function(item) {\r\n      item.classList.remove('active', 'active-main', 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class=\"ols-page-intro\">A concise revision guide to molecular polarity, bond dipole cancellation, symmetrical molecules, lone pair effects and the charged rod experiment used to test polar liquids.<\/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: bond-dipoles (swapped 26 Sep 2026) -->\n<!-- Copyright (c) 2026 Dr. Mohammed Al-Fatah, onlinelearningsystem.net. 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text-align:center; font-size:11px; font-style:italic; color:#aab0c0;\n}\n.ols-cc-bdip-001 a{color:#aab0c0; text-decoration:none;}\n.ols-cc-bdip-001 a:hover{text-decoration:underline;}\n.ols-bdip-001 .bdip-seg button{display:inline-flex; align-items:center;}\n.ols-bdip-001 .bdip-seg button .bdip-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-bdip-001 .bdip-seg button[aria-pressed=\"true\"] .bdip-n{background:#ffffff; color:#2563eb;}\n<\/style>\n\n<div class=\"bdip-head\">\n  <h2 class=\"bdip-title\">Bond Dipoles and Polar Molecules<\/h2>\n  <p class=\"bdip-sub\">Choose a step to watch a bond become polar, then join the bond dipoles head to tail to see whether the whole molecule is polar.<\/p>\n<\/div>\n\n<div class=\"bdip-stage\" id=\"bdipStage\">\n  <canvas class=\"bdip-canvas\" id=\"bdipCanvas\"><\/canvas>\n  <div class=\"bdip-overlay\" id=\"bdipOverlay\"><\/div>\n  <div class=\"bdip-caption\" id=\"bdipCaption\"><\/div>\n  <div class=\"bdip-hint\" id=\"bdipHint\">Drag to rotate<\/div>\n  <div class=\"bdip-badges\" id=\"bdipBadges\"><\/div>\n<\/div>\n\n<div class=\"bdip-controls\">\n  <div class=\"bdip-row\">\n    <span class=\"bdip-rowlab\">Step<\/span>\n    <div class=\"bdip-seg\" role=\"group\" aria-label=\"Step\">\n      <button type=\"button\" data-step=\"1\" aria-pressed=\"true\"><span class=\"bdip-n\">1<\/span>One polar bond: HCl<\/button>\n      <button type=\"button\" data-step=\"2\" aria-pressed=\"false\"><span class=\"bdip-n\">2<\/span>CO\u2082: dipoles cancel<\/button>\n      <button type=\"button\" data-step=\"3\" aria-pressed=\"false\"><span class=\"bdip-n\">3<\/span>H\u2082O: dipoles add<\/button>\n      <button type=\"button\" data-step=\"4\" aria-pressed=\"false\"><span class=\"bdip-n\">4<\/span>CCl\u2084 and CHCl\u2083<\/button>\n      <button type=\"button\" data-step=\"5\" aria-pressed=\"false\"><span class=\"bdip-n\">5<\/span>BF\u2083 and NH\u2083<\/button>\n    <\/div>\n  <\/div>\n\n  <div class=\"bdip-row\">\n    <span class=\"bdip-rowlab\">View<\/span>\n    <button type=\"button\" class=\"bdip-pill\" id=\"bdipResetV\">Reset view<\/button>\n  <\/div>\n<\/div>\n\n<div class=\"bdip-info\">\n  <h3 id=\"bdipInfoTitle\"><\/h3>\n  <p id=\"bdipInfoText\"><\/p>\n  <div class=\"bdip-facts\" id=\"bdipFacts\"><\/div>\n  <div class=\"bdip-key\">\n    <span><i class=\"k-ball\" style=\"background:#d6342c\"><\/i>Oxygen<\/span>\n    <span><i class=\"k-ball\" style=\"background:#2ea040\"><\/i>Chlorine<\/span>\n    <span><i class=\"k-ball\" style=\"background:#464a54\"><\/i>Carbon<\/span>\n    <span><i class=\"k-ball\" style=\"background:#ececf0\"><\/i>Hydrogen<\/span>\n    <span><i class=\"k-ball\" style=\"background:#3060d0\"><\/i>Nitrogen<\/span>\n    <span><i class=\"k-ball\" style=\"background:#f0a096\"><\/i>Boron<\/span>\n    <span><i class=\"k-ball\" style=\"background:#b8de6e\"><\/i>Fluorine<\/span>\n    <span><i class=\"\" style=\"background:#2f6fd0\"><\/i>Bond dipole (\u03b4+ \u2192 \u03b4\u2212)<\/span>\n    <span><i class=\"\" style=\"background:#b02a74\"><\/i>Overall dipole<\/span>\n    <span><i class=\"k-ball\" style=\"background:#fac828\"><\/i>Electron<\/span>\n  <\/div>\n<\/div>\n\n<script src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/JS\/bond-dipoles.js?v=20261025p\"><\/script>\n<\/section>\n\n<p class=\"ols-cc-bdip-001\">&copy; Dr. Mohammed Al-Fatah &#8211; <a href=\"https:\/\/www.onlinelearningsystem.net\" target=\"_blank\" rel=\"noopener\">onlinelearningsystem.net<\/a><\/p>\n\n\n      \n<section class=\"ols-h5p-card ols-h5p-inline ols-h5p-recap\">\n<span class=\"ols-h5p-kicker\">Before you start<\/span>\n<h2>GCSE Recap: Shared Pairs and Charges<\/h2>\n<p>Before you start, check the GCSE ideas about shared pairs and charges that this page builds on.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"661\"><\/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 Makes a Molecule Polar?<\/h2>\n        <\/div>\n\n        <p>A <strong>polar molecule<\/strong> has an <strong>overall dipole<\/strong>. This means there is a permanent separation of charge across the whole molecule.<\/p>\n        <p>Molecular polarity depends on two linked ideas: the polarity of the individual bonds and the <strong>3D shape<\/strong> of the molecule.<\/p>\n        <p>A molecule can contain polar bonds but still be non-polar overall if the bond dipoles cancel out.<\/p>\n\n        <div class=\"ols-definition-box\">\n          <p><strong>Definition:<\/strong> A polar molecule has an uneven distribution of electron density, giving one side of the molecule a partial negative character and another side a partial positive character.<\/p>\n        <\/div>\n\n        <div class=\"ols-key-box\">\n          <p><strong>Key idea:<\/strong> Do not decide molecular polarity from bond polarity alone. Always check the 3D shape and whether the bond dipoles cancel.<\/p>\n        <\/div>\n\n        <div class=\"ols-figure-card ols-zoom-card wide\">\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\/10\/t3-cd-20-polar-nonpolar.svg\" alt=\"CCl\u2084 with cancelling bond dipoles beside CH\u2082F\u2082 and CHCl\u2083, whose bond dipoles leave an overall dipole\" width=\"1520\" height=\"1094\">\n          <\/div>\n          <div class=\"ols-figure-caption ols-zoom-card-caption\">\n            <p>Overall polarity depends on whether the bond dipoles cancel in the 3D structure.<\/p>\n          <\/div>\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>When Polar Bonds Cancel Out<\/h2>\n        <\/div>\n\n        <p>Some molecules contain polar covalent bonds but are <strong>non-polar molecules<\/strong> overall.<\/p>\n        <p>This happens when the molecule is symmetrical, the same atoms or groups are arranged evenly around the central atom, and there are no lone pairs causing an uneven shape.<\/p>\n        <p>The bond dipoles point in different directions and cancel, leaving <strong>no overall dipole moment<\/strong>.<\/p>\n\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Symmetry cancels equal dipoles<\/h3>\n            <p>If equal polar bonds are arranged symmetrically in 3D, the molecule has no net dipole.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Shape matters<\/h3>\n            <p>Dipoles cancel in three dimensions, not just on a flat paper diagram.<\/p>\n          <\/div>\n        <\/div>\n\n        <div class=\"ols-molecule-grid\">\n          <div class=\"ols-figure-card\">\n<div class=\"ols-figure-image\"><img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-cd-21-ccl4-dipoles.svg\" alt=\"Tetrahedral CCl\u2084 with \u03b4+ on carbon, \u03b4\u2212 on each chlorine and four equal bond dipoles that cancel\" width=\"1520\" height=\"988\"><\/div>\n<div class=\"ols-figure-caption\"><p>CCl4 has four polar C-Cl bonds, but the tetrahedral arrangement makes the dipoles cancel.<\/p><\/div>\n<\/div>\n\n          <div class=\"ols-figure-card 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\/10\/t3-cd-22-bf3-dipoles.svg\" alt=\"Trigonal planar BF\u2083 with \u03b4+ on boron, \u03b4\u2212 on each fluorine and three equal bond dipoles at 120\u00b0 that cancel\" width=\"1520\" height=\"891\">\n            <\/div>\n            <div class=\"ols-figure-caption ols-zoom-card-caption\">\n              <p>BF<sub>3<\/sub> is trigonal planar and symmetrical, so the B-F bond dipoles cancel.<\/p>\n            <\/div>\n          <\/div>\n        <\/div>\n      <\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Where Do the Dipoles Cancel?<\/h2>\n<p>Choose the molecule in which the bond dipoles cancel.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-221\" class=\"h5p-iframe\" data-content-id=\"221\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Polar Molecules MCQ: In Which Molecule Do the Dipoles Cancel?\"><\/iframe><\/div><\/div>\n<\/section>\n\n      \n\n      <article class=\"ols-note-card orange\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">3<\/div>\n          <h2>When a Molecule Is Polar Overall<\/h2>\n        <\/div>\n\n        <p>A molecule becomes polar when the individual bond dipoles do <strong>not<\/strong> cancel out.<\/p>\n        <p>This commonly happens when the molecule is not symmetrical, or when lone pairs create an uneven distribution of electron density.<\/p>\n        <p>If the polar bonds point roughly towards the same side of a molecule, there will be a net dipole across the molecule.<\/p>\n        <p>Partial charges are written as <strong>\u03b4+<\/strong> and <strong>\u03b4\u2212<\/strong>. In H-Cl, chlorine is the more electronegative atom, so chlorine is \u03b4\u2212 and hydrogen is \u03b4+. A dipole arrow points from the \u03b4+ end towards the \u03b4\u2212 end.<\/p>\n        <p><strong>Worked example:<\/strong> in ammonia, NH<sub>3<\/sub>, each N-H bond is polar, with nitrogen \u03b4\u2212 and hydrogen \u03b4+. The molecule is trigonal pyramidal, so the three bond dipoles do not cancel.<\/p>\n<p>The overall dipole points from the hydrogen atoms towards the nitrogen atom and its lone pair, so NH<sub>3<\/sub> is polar.<\/p>\n\n        <div class=\"ols-key-box\">\n          <p><strong>Exam focus:<\/strong> Explain both parts: the molecule has polar bonds, and the shape means the dipoles do not cancel.<\/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: Polar or Non-Polar Tetrahedral Molecules<\/h2>\n<p>Click every tetrahedral molecule that is polar.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-222\" class=\"h5p-iframe\" data-content-id=\"222\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Polar Molecules Mark the Words: Polar and Non-Polar Tetrahedral Molecules\"><\/iframe><\/div><\/div>\n<\/section>\n\n      \n\n      <article class=\"ols-note-card purple\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">4<\/div>\n          <h2>Lone Pairs Can Make Polarity Trickier<\/h2>\n        <\/div>\n\n        <p>Some molecules are polar even when their bonds are weakly polar or treated as essentially non-polar at this level.<\/p>\n        <p>The reason is that lone pairs occupy regions of electron density and can make the overall electron distribution uneven.<\/p>\n        <p>PH<sub>3<\/sub> is a useful tricky example: the P-H electronegativity difference is very small, but the molecule is trigonal pyramidal with a lone pair on phosphorus, so it has a small overall dipole.<\/p>\n\n        <div class=\"ols-definition-box\">\n          <p><strong>Important distinction:<\/strong> Bond polarity is about individual bonds. Molecular polarity is about the overall electron distribution across the entire molecule.<\/p>\n        <\/div>\n      <div class=\"ols-zoom-card\">\n<div class=\"ols-zoom-card-image\">\n<a class=\"ols-lightbox-link\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-cd-23-lonepair-polarity.svg\" aria-label=\"Open image full screen\">\n<img decoding=\"async\" class=\"ols-zoomable-img ols-lightbox-target\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-cd-23-lonepair-polarity.svg\" alt=\"CO\u2082 (dipoles cancel) beside bent SO\u2082, H\u2082O, NH\u2083 and PH\u2083, whose lone pairs leave an overall dipole\">\n<\/a>\n<\/div>\n<div class=\"ols-zoom-card-caption\"><p>CO\u2082 is linear and non-polar, but a lone pair bends SO\u2082 and makes it polar; H\u2082O, NH\u2083 and even PH\u2083 are polar for the same reason.<\/p><\/div>\n<\/div>\n<\/article>\n\n      \n\n      <article class=\"ols-note-card\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">5<\/div>\n          <h2>How to Decide if a Molecule Is Polar<\/h2>\n        <\/div>\n\n        <p>Use a step-by-step approach rather than guessing from the formula.<\/p>\n\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Step<\/th>\n                <th>What to check<\/th>\n                <th>Exam conclusion<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Step\"><strong>1<\/strong><\/td>\n                <td data-label=\"What to check\">Decide whether the individual bonds are polar using electronegativity differences.<\/td>\n                <td data-label=\"Exam conclusion\">More electronegative atoms attract bonding electrons more strongly.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Step\"><strong>2<\/strong><\/td>\n                <td data-label=\"What to check\">Work out the 3D shape of the molecule, including lone pairs.<\/td>\n                <td data-label=\"Exam conclusion\">The same formula drawn flat can hide the real direction of the dipoles.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Step\"><strong>3<\/strong><\/td>\n                <td data-label=\"What to check\">Check whether the dipoles cancel due to symmetry.<\/td>\n                <td data-label=\"Exam conclusion\">If the dipoles cancel, the molecule is non-polar overall.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Step\"><strong>4<\/strong><\/td>\n                <td data-label=\"What to check\">If the dipoles do not cancel, identify the direction of the overall dipole.<\/td>\n                <td data-label=\"Exam conclusion\">If there is a net dipole, the molecule is polar.<\/td>\n              <\/tr>\n            <\/tbody>\n          <\/table>\n        <\/div>\n      <div class=\"ols-zoom-card\">\n<div class=\"ols-zoom-card-image\">\n<a class=\"ols-lightbox-link\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-11-polarflow.jpg\" aria-label=\"Open image full screen\">\n<img decoding=\"async\" class=\"ols-zoomable-img ols-lightbox-target\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-11-polarflow.jpg\" alt=\"Three-step flowchart deciding molecular polarity from polar bonds, 3D shape and symmetry, with example molecules at each outcome\">\n<\/a>\n<\/div>\n<div class=\"ols-zoom-card-caption\"><p>Work through bonds, then shape, then symmetry: only a molecule whose bond dipoles do not cancel is polar.<\/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: Carbon Dioxide and Sulfur Dioxide<\/h2>\n<p>Drag the words into place to compare the two molecules.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-220\" class=\"h5p-iframe\" data-content-id=\"220\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Polar Molecules Drag: Carbon Dioxide Compared with Sulfur Dioxide\"><\/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>Experiment: Charged Rod and Polar Liquids<\/h2>\n        <\/div>\n\n        <p>A simple demonstration of molecular polarity uses a charged rod brought close to a thin jet of liquid flowing from a burette.<\/p>\n        <p>If the liquid is polar, its molecules contain permanent dipoles. These dipoles align in the electric field from the charged rod, causing the jet of liquid to be attracted and deflected. Water is the liquid shown here.<\/p>\n        <p>The jet is attracted <strong>whichever charge<\/strong> the rod carries. The molecules in a liquid are free to rotate, so each one turns until its oppositely charged end faces the rod: the \u03b4+ end faces a negative rod and the \u03b4\u2212 end faces a positive rod.<\/p>\n<p>The jet bends towards the rod in both cases and is never repelled.<\/p>\n        <p>The stronger the overall dipole in the liquid molecules, the greater the deflection of the liquid jet. Non-polar liquids show little or no significant deflection.<\/p>\n\n        <div class=\"ols-figure-card\">\n<div class=\"ols-figure-image\"><img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/fix-25.jpg\" alt=\"Charged rod deflecting a thin jet of polar liquid from a burette into a beaker\"><\/div>\n<div class=\"ols-figure-caption\"><p>A polar liquid can be attracted towards a charged rod because its molecular dipoles align with the electric field.<\/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: Predict the Charged Rod Test<\/h2>\n<p>Predict what each liquid does near a charged rod.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"662\"><\/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: Pick the Accurate Statement<\/h2>\n<p>In each round, choose the one accurate statement to review the whole page.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-223\" class=\"h5p-iframe\" data-content-id=\"223\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Polar Molecules Summary: Lone Pairs, Symmetry and Overall Dipoles\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">7<\/div>\n          <h2>Common Exam Points<\/h2>\n        <\/div>\n\n        <p>Strong answers use the words <strong>polar bonds<\/strong>, <strong>3D shape<\/strong>, <strong>symmetrical<\/strong>, <strong>dipoles cancel<\/strong> and <strong>overall dipole<\/strong> accurately.<\/p>\n\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Do not stop at \u201cthe bonds are polar\u201d<\/h3>\n            <p>A molecule with polar bonds may still be non-polar overall if the dipoles cancel.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Use cancellation language<\/h3>\n            <p>For CCl<sub>4<\/sub> and BF<sub>3<\/sub>, state that the bond dipoles cancel because the molecule is symmetrical.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Mention lone pairs where relevant<\/h3>\n            <p>Lone pairs can distort the shape or make electron density uneven, so the molecule may have an overall dipole.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Experimental deflection<\/h3>\n            <p>A polar liquid is attracted to a charged rod because permanent dipoles align with the electric field.<\/p>\n          <\/div>\n        <\/div>\n      <\/article>\n\n      \n\n      <article class=\"ols-note-card purple\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">\u2713<\/div>\n          <h2>QuickSnap<\/h2>\n        <\/div>\n\n        <p>Molecular polarity is decided by both bond polarity and molecular shape. Symmetrical molecules can contain polar bonds but be non-polar overall because the dipoles cancel. Unsymmetrical molecules, or molecules with lone pair effects that create uneven electron density, can be polar overall.<\/p>\n\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Polar molecule<\/h3>\n            <p>Has an overall dipole due to uneven electron density across the molecule.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Non-polar molecule<\/h3>\n            <p>Has no overall dipole because the bond dipoles cancel or the bonds are non-polar.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Symmetry<\/h3>\n            <p>Equal bond dipoles arranged symmetrically cancel in three dimensions.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Charged rod test<\/h3>\n            <p>Polar liquids are deflected because their permanent dipoles align with the charged rod.<\/p>\n          <\/div>\n        <\/div>\n      <\/article>\n\n            <section class=\"ols-faq-card\">\n        <h2>FAQs<\/h2>\n        <p>Use these quick answers to check the common polarity misconceptions that appear in A Level Chemistry questions.<\/p>\n\n        <div class=\"ols-faq-list\">\n          <div class=\"ols-faq-item\">\n            <h3>Can a molecule have polar bonds but be non-polar overall?<\/h3>\n            <p>Yes. If the molecule is symmetrical, the individual bond dipoles can cancel out, leaving no overall dipole. CCl<sub>4<\/sub> and BF<sub>3<\/sub> are common examples.<\/p>\n          <\/div>\n\n          <div class=\"ols-faq-item\">\n            <h3>Why is CHCl<sub>3<\/sub> polar?<\/h3>\n            <p>CHCl<sub>3<\/sub> has three polar C-Cl bonds and one C-H bond arranged tetrahedrally. The molecule is not symmetrical, so the bond dipoles do not cancel and there is an overall dipole towards the chlorine-rich side.<\/p>\n          <\/div>\n\n          <div class=\"ols-faq-item\">\n            <h3>Why is CCl<sub>4<\/sub> non-polar even though C-Cl bonds are polar?<\/h3>\n            <p>CCl<sub>4<\/sub> is tetrahedral and symmetrical. The four equal C-Cl bond dipoles point in different directions and cancel in three dimensions.<\/p>\n          <\/div>\n\n          <div class=\"ols-faq-item\">\n            <h3>How does a charged rod show that a liquid is polar?<\/h3>\n            <p>A polar liquid contains molecules with permanent dipoles. These dipoles align with the electric field from the charged rod, so the liquid jet is attracted and bends towards the rod.<\/p>\n          <\/div>\n\n          <div class=\"ols-faq-item\">\n            <h3>Why can lone pairs affect molecular polarity?<\/h3>\n            <p>Lone pairs occupy regions of electron density and can make the electron distribution uneven. This can create an overall dipole even when the bond polarity is weak.<\/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\"\n            class=\"ols-author-avatar-img\"\n            src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/05\/Author-Profile.jpeg\"\n            alt=\"Dr. Mohammed Al-Fatah\"\n          >\n\n          <div class=\"ols-author-content\">\n            <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\n            <a\n              class=\"ols-linkedin-pill\"\n              href=\"https:\/\/www.linkedin.com\/in\/doctormohammedfatah\/\"\n              target=\"_blank\"\n              rel=\"noopener noreferrer\"\n            >\n              <svg class=\"ols-linkedin-icon\" viewBox=\"0 0 24 24\" fill=\"currentColor\" aria-hidden=\"true\">\n                <path d=\"M4.98 3.5C4.98 4.88 3.86 6 2.48 6S0 4.88 0 3.5 1.12 1 2.48 1s2.5 1.12 2.5 2.5zM.5 8h4V24h-4V8zm7 0h3.8v2.2h.1c.5-.9 1.8-2.2 3.9-2.2 4.2 0 5 2.8 5 6.4V24h-4v-7.6c0-1.8 0-4.2-2.6-4.2s-3 2-3 4v7.8h-4V8z\"><\/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>Revise the connected bonding and structure ideas that support molecular polarity questions.<\/p>\n\n        <div class=\"ols-related-grid\">\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/covalent-bonding\/electronegativity\/\">Electronegativity<\/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\/\">Shapes of Molecules<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/covalent-bonding\/\">Covalent Bonding<\/a>\n          <a class=\"ols-related-item\" 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>\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<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/\">Topic 2 Bonding and Structure<\/a>\n        <\/div>\n      <\/section>\n\n      <section class=\"ols-attribution-card ols-attr-std\" aria-label=\"Copyright notice\">\n<style id=\"ols-attribution-card-css\">.ols-attribution-card.ols-attr-std{background:linear-gradient(135deg,#ffffff,#f8fbff);border:1px solid rgba(28,36,75,0.14);border-radius:28px;box-shadow:0 18px 45px rgba(28,36,75,0.10);padding:34px;margin:24px 0;overflow:hidden;font-family:Poppins,Arial,sans-serif;box-sizing:border-box}.ols-attribution-card.ols-attr-std *{box-sizing:border-box}.ols-attribution-card.ols-attr-std p{margin:0;font-size:14px;line-height:1.65;font-weight:300;color:#667085}.ols-attribution-card.ols-attr-std strong{font-weight:700;color:#1C244B}@media (max-width:760px){.ols-attribution-card.ols-attr-std{padding:24px 18px;border-radius:22px}}<\/style>\n<p><strong>Copyright notice:<\/strong> This OLS revision content, including the explanations, layout, diagrams, tables and embedded learning structure, is authored for Online Learning System by Dr. Mohammed Al-Fatah. It may not be copied, reproduced, redistributed or adapted without written permission.<\/p>\n<\/section>\n\n      <div class=\"ols-image-lightbox\" id=\"olsImageLightboxPolarMolecules9ch0\" aria-hidden=\"true\" role=\"dialog\" aria-modal=\"true\" aria-label=\"Expanded revision image\">\n        <div class=\"ols-image-lightbox-inner\">\n          <button class=\"ols-image-lightbox-close\" type=\"button\" aria-label=\"Close enlarged image\">\u00d7<\/button>\n          <img decoding=\"async\" class=\"ols-image-lightbox-img\" src=\"\" alt=\"\">\n        <\/div>\n      <\/div>\n\n      <script>\n        (function(){\n          var page = document.querySelector(\".ols-polar-nonpolar-molecules-9ch0-page\");\n          if (!page) { return; }\n          var lightbox = page.querySelector(\"#olsImageLightboxPolarMolecules9ch0\");\n          if (!lightbox) { return; }\n          var lightboxImage = lightbox.querySelector(\".ols-image-lightbox-img\");\n          var closeButton = 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