{"id":5385,"date":"2026-06-24T09:25:47","date_gmt":"2026-06-24T08:25:47","guid":{"rendered":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/permanent-dipole-dipole-forces-2\/"},"modified":"2026-09-18T11:28:22","modified_gmt":"2026-09-18T10:28:22","slug":"permanent-dipole-dipole-forces","status":"publish","type":"page","link":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/permanent-dipole-dipole-forces\/","title":{"rendered":"Permanent Dipole-Dipole Forces"},"content":{"rendered":"\n<section class=\"ols-revision-page ols-nature-of-covalent-bonding-9ch0-page\">\n  <style>\n    .ols-revision-page {\n      --navy: #1C244B;\n      --blue: #2563eb;\n      --soft-blue: #eef4ff;\n      --soft-red: #fff7f7;\n      --soft-purple: #f7f0ff;\n      --soft-green: #f0f7f1;\n      --soft-orange: #fff7ed;\n      --grey-text: #667085;\n      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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>AQA A Level Chemistry<\/p>\r\n  <\/div>\r\n\r\n  <div class=\"ols-topic-group\">\r\n    <h4>3.1.3 Bonding<\/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\/aqa\/3-1-3-bonding\/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\/aqa\/3-1-3-bonding\/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\/aqa\/3-1-3-bonding\/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\/aqa\/3-1-3-bonding\/ionic-bonding\/physical-properties-of-ionic-compounds\/\">Physical Properties of Ionic Compounds<\/a>\r\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/ionic-bonding\/ions-and-ionic-formulae\/\">Ions and Ionic Formulae<\/a>\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\/aqa\/3-1-3-bonding\/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\/aqa\/3-1-3-bonding\/covalent-bonding\/covalent-bonding\/\">Covalent Bonding<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/covalent-bonding\/dative-covalent-bonding\/\">Dative Covalent Bonding<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/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\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/\">Shapes of Molecules and Ions<\/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\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/linear\/\">Linear<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/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\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/tetrahedral\/\">Tetrahedral<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/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\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/bent\/\">Bent<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/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\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/octahedral\/\">Octahedral<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/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\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/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\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/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\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/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\/aqa\/3-1-3-bonding\/bond-polarity\/\">Bond Polarity<\/a>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/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\/aqa\/3-1-3-bonding\/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\/aqa\/3-1-3-bonding\/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\/aqa\/3-1-3-bonding\/giant-covalent-structures\/\">Giant Covalent Structures<\/a>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/simple-molecular-structures\/\">Simple Molecular Structures<\/a>\r\n      <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/structure-types\/\">Structure Types<\/a>\n          <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/\">Intermolecular Forces<\/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\/aqa\/3-1-3-bonding\/intermolecular-forces\/london-forces\/\">London Forces<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/permanent-dipole-dipole-forces\/\">Permanent Dipole-Dipole Forces<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/hydrogen-bonding\/\">Hydrogen Bonding<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/anomalous-properties-of-water\/\">Anomalous Properties of Water<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/boiling-temperature-trends\/\">Boiling Point Trends<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/choosing-solvents\/\">Choosing Solvents<\/a>\r\n          <\/li>\r\n        <\/ul>\r\n      <\/li>\r\n    <\/ul>\r\n  <\/div>\r\n\r\n  <div class=\"ols-topic-group\">\r\n    <h4>Adjacent 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\/aqa\/3-1-1-atomicstructure\/\">3.1.1 Atomic Structure<\/a>\r\n      <\/li>\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-2-amount-of-substance\/\">3.1.2 Amount of Substance<\/a>\r\n      <\/li>\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-4-energetics\/\">3.1.4 Energetics<\/a>\r\n      <\/li>\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-2-1-periodicity\/\">3.2.1 Periodicity<\/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\"], 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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\/aqa\/\">AQA<\/a> \/\n<a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/\">3.1.3 Bonding<\/a> \/\n<a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/\">Intermolecular Forces<\/a> \/\n<span>Permanent Dipole-Dipole Forces<\/span>\n<\/nav>\n\n      <header class=\"ols-title-card\">\n        <h1>Permanent Dipole-Dipole Forces<\/h1>\n        <p class=\"ols-page-intro\">A concise revision guide to permanent dipole-dipole forces: which molecules have a permanent dipole, how polar molecules attract each other, why the attraction adds to induced dipole-dipole forces, and how to decide the forces in an unfamiliar molecule, for AQA A Level Chemistry.<\/p>\n\n        <div class=\"ols-badges\">\n<div class=\"ols-badge\">Paper 1 and 2 AQA<\/div>\n<div class=\"ols-badge\">3.1.3 Bonding<\/div>\n<div class=\"ols-badge\">7405\/1 and 7405\/2<\/div>\n<\/div>\n\n        <div class=\"ols-author\">\n\n    <img decoding=\"async\"\n      class=\"ols-author-avatar-img\"\n      src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/05\/Author-Profile.jpeg\"\n      alt=\"Dr. Mohammed Al-Fatah\"\n    >\n\n    <div class=\"ols-author-content\">\n\n      <h2 class=\"ols-author-title\">\n        Written by:<br><span>Dr. Mohammed Al-Fatah<\/span>\n      <\/h2>\n\n      <p class=\"ols-author-description\">\n        Chemistry specialist revision notes for A Level Chemistry.\n      <\/p>\n\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\"\/>\n        <\/svg>\n        View LinkedIn Profile\n      <\/a>\n\n    <\/div>\n\n  <\/div>\n      <\/header>\n\n      <article class=\"ols-note-card soft\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">1<\/div>\n<h2>Polar Molecules and Permanent Dipoles<\/h2>\n<\/div>\n<p>A <strong>permanent dipole<\/strong> exists in a molecule that contains polar bonds whose dipoles do not cancel, so one end of the molecule is always \u03b4+ and the other always \u03b4-. Permanent dipole-dipole forces are the attractions between the \u03b4+ end of one such molecule and the \u03b4- end of a neighbour.<\/p>\n<p>Two conditions must both hold. First, the molecule must contain a bond between atoms of different electronegativity, such as H-Cl, C-Cl, C-F or C=O. Second, the shape of the molecule must leave an overall dipole. CO\u2082 has two very polar C=O bonds, but the molecule is linear and the two bond dipoles cancel, so CO\u2082 has no permanent dipole and only induced dipole-dipole forces act between its molecules. The same applies to CCl\u2084 and BF\u2083.<\/p>\n<div class=\"ols-table-wrap\">\n<table class=\"ols-table\">\n<thead>\n<tr><th>Molecule<\/th><th>Polar bonds?<\/th><th>Shape<\/th><th>Overall dipole?<\/th><th>Strongest intermolecular force<\/th><\/tr>\n<\/thead>\n<tbody>\n<tr><td><strong>HCl<\/strong><\/td><td>yes<\/td><td>linear, two atoms<\/td><td>yes<\/td><td>permanent dipole-dipole forces<\/td><\/tr>\n<tr><td><strong>CH\u2083Cl<\/strong><\/td><td>yes<\/td><td>tetrahedral, one Cl<\/td><td>yes<\/td><td>permanent dipole-dipole forces<\/td><\/tr>\n<tr><td><strong>CO\u2082<\/strong><\/td><td>yes<\/td><td>linear, symmetric<\/td><td>no<\/td><td>induced dipole-dipole forces<\/td><\/tr>\n<tr><td><strong>CCl\u2084<\/strong><\/td><td>yes<\/td><td>tetrahedral, symmetric<\/td><td>no<\/td><td>induced dipole-dipole forces<\/td><\/tr>\n<tr><td><strong>SO\u2082<\/strong><\/td><td>yes<\/td><td>bent<\/td><td>yes<\/td><td>permanent dipole-dipole forces<\/td><\/tr>\n<tr><td><strong>N\u2082<\/strong><\/td><td>no<\/td><td>linear<\/td><td>no<\/td><td>induced dipole-dipole forces<\/td><\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n<div class=\"ols-key-box\">\n<p><strong>Key idea:<\/strong> Polar bonds are necessary but not sufficient. Ask whether the bond dipoles cancel in three dimensions before deciding that a molecule is polar.<\/p>\n<\/div>\n<\/article>\n<article class=\"ols-note-card\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">2<\/div>\n<h2>How the Molecules Line Up<\/h2>\n<\/div>\n<p>In a liquid such as hydrogen chloride the molecules tumble constantly, but on average they spend more time with their \u03b4+ hydrogen close to the \u03b4- chlorine of a neighbour than in any other arrangement. This partial alignment produces a net attraction that is stronger than induced dipole-dipole forces alone for molecules of similar size, so more energy is needed to pull the molecules apart.<\/p>\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\/09\/intermolecular-forces-in-hydrogen-chloride-and-fluorine.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\/09\/intermolecular-forces-in-hydrogen-chloride-and-fluorine.jpg\" alt=\"Polar hydrogen chloride molecules aligned by permanent dipole-dipole attractions, beside non-polar fluorine molecules held only by London forces\">\n<\/a>\n<\/div>\n<div class=\"ols-zoom-card-caption\"><p>Polar molecules attract each other by the alignment of their permanent dipoles; this attraction acts in addition to the induced dipole-dipole forces that every molecule has.<\/p><\/div>\n<\/div>\n<p>The alignment is never perfect, because thermal motion keeps disturbing it, which is why permanent dipole-dipole forces are still weak compared with covalent bonds and why polar liquids such as HCl still boil far below room temperature.<\/p>\n<div class=\"ols-key-box\">\n<p><strong>Remember:<\/strong> Permanent dipole-dipole forces act <strong>in addition to<\/strong> induced dipole-dipole forces, never instead of them.<\/p>\n<\/div>\n<\/article>\n<article class=\"ols-note-card purple\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">3<\/div>\n<h2>Comparing Molecules With Similar Numbers of Electrons<\/h2>\n<\/div>\n<p>The fair way to show that a permanent dipole raises the boiling point is to compare two molecules with the same number of electrons, so that their induced dipole-dipole forces are similar. Hydrogen chloride and fluorine both have 18 electrons. F\u2082 is non-polar and boils at -188 \u00b0C; HCl is polar and boils at -85 \u00b0C. The extra 100 \u00b0C comes from the permanent dipole-dipole forces.<\/p>\n<div class=\"ols-table-wrap\">\n<table class=\"ols-table\">\n<thead>\n<tr><th>Pair<\/th><th>Electrons<\/th><th>Polar?<\/th><th>boiling point \/ \u00b0C<\/th><\/tr>\n<\/thead>\n<tbody>\n<tr><td><strong>F\u2082<\/strong><\/td><td>18<\/td><td>no<\/td><td>-188<\/td><\/tr>\n<tr><td><strong>HCl<\/strong><\/td><td>18<\/td><td>yes<\/td><td>-85<\/td><\/tr>\n<tr><td><strong>Butane, C\u2084H\u2081\u2080<\/strong><\/td><td>34<\/td><td>no<\/td><td>-1<\/td><\/tr>\n<tr><td><strong>Propanone, CH\u2083COCH\u2083<\/strong><\/td><td>32<\/td><td>yes (C=O)<\/td><td>56<\/td><\/tr>\n<tr><td><strong>Ethane, C\u2082H\u2086<\/strong><\/td><td>18<\/td><td>no<\/td><td>-89<\/td><\/tr>\n<tr><td><strong>Fluoromethane, CH\u2083F<\/strong><\/td><td>18<\/td><td>yes (C-F)<\/td><td>-78<\/td><\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n<p>Propanone and butane make the same point with organic molecules: almost the same electron count, but the C=O dipole in propanone lifts its boiling point by nearly 60 \u00b0C.<\/p>\n<div class=\"ols-key-box\">\n<p><strong>Exam sentence:<\/strong> Propanone has a higher boiling point than butane because propanone molecules have a permanent dipole, so permanent dipole-dipole forces act between them in addition to induced dipole-dipole forces, and more energy is needed to separate the molecules.<\/p>\n<\/div>\n<\/article>\n<article class=\"ols-note-card\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">4<\/div>\n<h2>Deciding the Forces in an Unfamiliar Molecule<\/h2>\n<\/div>\n<p>Exam questions often give a molecule you have never met and ask which intermolecular forces act between its molecules. Use three questions in order.<\/p>\n<ol>\n<li><strong>Does the molecule contain an H atom bonded directly to N, O or F?<\/strong> If yes, hydrogen bonding is present (see the <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/hydrogen-bonding\/\">Hydrogen Bonding<\/a> page), and so are the two forces below.<\/li>\n<li><strong>Does the molecule have an overall permanent dipole?<\/strong> Check for polar bonds and then check that the shape does not cancel them. If yes, permanent dipole-dipole forces are present, plus induced dipole-dipole forces.<\/li>\n<li><strong>Every molecule<\/strong> has induced dipole-dipole forces. If the answers to questions 1 and 2 are no, these are the only forces.<\/li>\n<\/ol>\n<p>For example, chloromethane, CH\u2083Cl, has no H bonded to N, O or F, but it has a polar C-Cl bond in a tetrahedral molecule with only one chlorine, so it has an overall dipole: permanent dipole-dipole forces plus induced dipole-dipole forces. Methanal, HCHO, has a C=O dipole: the same answer. Tetrachloromethane, CCl\u2084, has four polar bonds that cancel: induced dipole-dipole forces only.<\/p>\n<div class=\"ols-key-box\">\n<p><strong>Exam focus:<\/strong> Name every force that is present and say which is the strongest. A list with one force missing loses the mark even if the strongest is right.<\/p>\n<\/div>\n<\/article>\n<article class=\"ols-note-card soft\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">5<\/div>\n<h2>Permanent Dipoles and Solubility<\/h2>\n<\/div>\n<p>Polar molecules tend to dissolve in polar solvents and non-polar molecules in non-polar solvents, because a solute dissolves when the new attractions it makes with solvent molecules are similar in strength to the attractions it loses. Propanone mixes with water in all proportions because its C=O oxygen can accept a hydrogen bond from water, while hexane does not mix with water because the only forces hexane can offer are induced dipole-dipole forces. The <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/choosing-solvents\/\">Choosing Solvents<\/a> page develops this idea.<\/p>\n<div class=\"ols-key-box\">\n<p><strong>Key idea:<\/strong> Like dissolves like: match the strongest intermolecular force in the solute to the strongest force in the solvent.<\/p>\n<\/div>\n<\/article>\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<h3>Explain why HCl boils higher than F\u2082<\/h3><p>Similar electrons, so similar induced dipole-dipole forces; HCl is polar, so permanent dipole-dipole forces act as well; more energy is needed to separate HCl molecules.<\/p>\n<h3>Explain why CO\u2082 is non-polar although C=O bonds are polar<\/h3><p>The molecule is linear and symmetrical, so the two bond dipoles cancel and there is no overall dipole.<\/p>\n<h3>State the intermolecular forces in CH\u2083Br<\/h3><p>Permanent dipole-dipole forces and induced dipole-dipole forces; no hydrogen bonding because no H is bonded to N, O or F.<\/p>\n<h3>Do not say<\/h3><p>&#8220;Polar molecules have no induced dipole-dipole forces&#8221;; &#8220;any molecule with a polar bond is polar&#8221;.<\/p>\n<\/article>\n<section class=\"ols-h5p-card\">\n<h2>Check Your Understanding<\/h2>\n<p>Decide which intermolecular forces act in molecules that do not appear in the notes above.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-526\" class=\"h5p-iframe\" data-content-id=\"526\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"IMF Permanent Dipole Drag: iodomethane and ethane\"><\/iframe><\/div><\/div>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-527\" class=\"h5p-iframe\" data-content-id=\"527\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"IMF Permanent Dipole MCQ: which molecule is polar\"><\/iframe><\/div><\/div>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-528\" class=\"h5p-iframe\" data-content-id=\"528\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"IMF Permanent Dipole MCQ: ethanal and propane\"><\/iframe><\/div><\/div>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-529\" class=\"h5p-iframe\" data-content-id=\"529\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"IMF Permanent Dipole MCQ: forces in dichloromethane\"><\/iframe><\/div><\/div>\n<\/section>\n<section class=\"ols-faq-card\">\n<h2>FAQs<\/h2>\n<p>Use these quick answers to check how AQA expects permanent dipoles to be identified and explained.<\/p>\n\n<div class=\"ols-faq-list\">\n<div class=\"ols-faq-item\">\n<h3>What is a permanent dipole?<\/h3>\n<p>It is a separation of charge that is always present in a molecule, because the molecule contains polar bonds whose dipoles do not cancel. One end of the molecule is permanently \u03b4+ and the other permanently \u03b4-.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>Does a polar bond always make a polar molecule?<\/h3>\n<p>No. CO\u2082 and CCl\u2084 both contain very polar bonds, but the molecules are symmetrical, so the bond dipoles cancel and there is no overall dipole. Always check the shape before deciding.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>How do I decide which forces act between molecules of an unfamiliar substance?<\/h3>\n<p>Ask three questions in order: is a hydrogen atom bonded directly to N, O or F (hydrogen bonding); does the molecule have an overall permanent dipole (permanent dipole-dipole forces); and finally, every molecule has induced dipole-dipole forces.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>Which is stronger, a permanent dipole attraction or induced dipole-dipole forces?<\/h3>\n<p>For molecules of a similar size, the permanent dipole-dipole attraction is stronger. For a much larger molecule the induced dipole-dipole forces can be bigger in total, which is why HI boils higher than HCl even though HCl is more polar.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>How should I show this in an answer?<\/h3>\n<p>Compare molecules with a similar number of electrons so the induced dipole-dipole forces are similar, then attribute the difference to the permanent dipole and finish with the energy statement.<\/p>\n<\/div>\n<\/div>\n<\/section>\n<section class=\"ols-related-card\">\n<h2>Related Intermolecular Forces Pages<\/h2>\n<p>Use these pages to connect the three intermolecular forces with the physical properties they explain.<\/p>\n<div class=\"ols-related-grid\">\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/london-forces\/\">London Forces<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/hydrogen-bonding\/\">Hydrogen Bonding<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/anomalous-properties-of-water\/\">Anomalous Properties of Water<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/boiling-temperature-trends\/\">Boiling Point Trends<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/choosing-solvents\/\">Choosing Solvents<\/a>\n<\/div>\n<\/section>\n<section class=\"ols-attribution-card\">\n        <p><strong>Copyright and author footprint:<\/strong> This OLS revision page was written for Online Learning System by <strong>Dr. Mohammed Al-Fatah<\/strong>. It is designed for A Level Chemistry revision and should not be copied or redistributed without permission.<\/p>\n      <\/section>\n\n      <div class=\"ols-image-lightbox\" id=\"olsImageLightboxNatureCovalentBonding9ch0\" 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-nature-of-covalent-bonding-9ch0-page\");\n          if (!page) { return; }\n          var lightbox = page.querySelector(\"#olsImageLightboxNatureCovalentBonding9ch0\");\n          if (!lightbox) { return; }\n          var lightboxImage = lightbox.querySelector(\".ols-image-lightbox-img\");\n    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