{"id":4584,"date":"2026-05-30T06:12:40","date_gmt":"2026-05-30T05:12:40","guid":{"rendered":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/covalent-bonding\/electronegativity\/"},"modified":"2026-10-25T12:10:06","modified_gmt":"2026-10-25T12:10:06","slug":"electronegativity","status":"publish","type":"page","link":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/covalent-bonding\/electronegativity\/","title":{"rendered":"Electronegativity"},"content":{"rendered":"\n<section class=\"ols-revision-page ols-electronegativity-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      --body-text: #1f2937;\n      --border: 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700px; }\n    .ols-zoom-card.wide { max-width: 940px; }\n    .ols-zoom-card:hover { z-index: 50 !important; }\n    .ols-zoom-card-image { display: flex !important; align-items: center !important; justify-content: center !important; width: 100% !important; min-height: 240px !important; padding: 20px !important; background: #ffffff !important; overflow: visible !important; border-top-left-radius: 26px !important; border-top-right-radius: 26px !important; position: relative !important; z-index: 2 !important; }\n    .ols-zoom-card img.ols-zoomable-img { display: block !important; max-width: 100% !important; height: auto !important; border-radius: 18px !important; cursor: zoom-in !important; pointer-events: auto !important; user-select: none !important; -webkit-user-drag: none !important; transform: translateZ(0) scale(1) !important; transform-origin: center center !important; transition: transform 0.32s ease, box-shadow 0.32s ease, filter 0.32s ease !important; position: relative !important; z-index: 2 !important; }\n    @media (hover: hover) and (pointer: fine) { .ols-zoom-card img.ols-zoomable-img:hover { transform: translateZ(0) scale(1.35) !important; box-shadow: 0 28px 70px rgba(28, 36, 75, 0.34) !important; filter: saturate(1.02) contrast(1.01) !important; z-index: 100 !important; } }\n    .ols-zoom-card-caption { padding: 18px 22px 20px !important; background: linear-gradient(135deg, #ffffff, #f8fbff) !important; border-bottom-left-radius: 26px !important; border-bottom-right-radius: 26px !important; position: relative !important; z-index: 1 !important; }\n    .ols-zoom-card-caption p { margin: 0 !important; color: #5f6b85 !important; font-size: 15px !important; line-height: 1.65 !important; font-weight: 300 !important; font-style: italic !important; font-family: Poppins, Arial, sans-serif !important; }\n    .ols-image-lightbox { position: fixed; inset: 0; z-index: 999999; display: none; align-items: center; justify-content: center; padding: 34px; background: rgba(10, 15, 35, 0.86); backdrop-filter: blur(8px); -webkit-backdrop-filter: blur(8px); }\n    .ols-image-lightbox.is-open { display: flex; }\n    .ols-image-lightbox-inner { position: relative; width: min(96vw, 1500px); max-height: 92vh; display: flex; align-items: center; justify-content: center; }\n    .ols-image-lightbox-img { display: block; max-width: 100%; max-height: 92vh; height: auto; width: auto; border-radius: 22px; background: #ffffff; box-shadow: 0 32px 90px rgba(0, 0, 0, 0.45); object-fit: contain; }\n    .ols-image-lightbox-close { position: absolute; top: -18px; right: -18px; width: 46px; height: 46px; border: 0; border-radius: 50%; background: #ffffff; color: var(--navy); font-family: Poppins, Arial, sans-serif; font-size: 28px; line-height: 1; font-weight: 700; cursor: pointer; box-shadow: 0 16px 34px rgba(0, 0, 0, 0.28); display: flex; align-items: center; justify-content: center; transition: transform 0.2s ease, background 0.2s ease, color 0.2s ease; }\n    .ols-image-lightbox-close:hover { transform: scale(1.08); background: var(--blue); color: #ffffff; }\n    @media (max-width: 760px) { .ols-zoom-card { border-radius: 22px !important; overflow: hidden !important; } .ols-zoom-card-image { min-height: auto !important; padding: 12px !important; overflow: hidden !important; border-top-left-radius: 22px !important; border-top-right-radius: 22px !important; } .ols-zoom-card img.ols-zoomable-img, .ols-zoom-card img.ols-zoomable-img:hover { transform: none !important; box-shadow: none !important; } .ols-zoom-card-caption { border-bottom-left-radius: 22px !important; border-bottom-right-radius: 22px !important; } .ols-image-lightbox { padding: 16px; } .ols-image-lightbox-inner { width: 100%; max-height: 88vh; } .ols-image-lightbox-img { max-height: 88vh; border-radius: 16px; } .ols-image-lightbox-close { top: 10px; right: 10px; width: 42px; height: 42px; font-size: 26px; } }\n\n    .ols-table-wrap { overflow: hidden; border-radius: 22px; 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.ols-zoom-card, .ols-zoom-card * { box-sizing: border-box; }\n    .ols-zoom-card { display: block !important; margin: 26px auto 34px !important; border: 1px solid rgba(28, 36, 75, 0.14) !important; border-radius: 26px !important; background: #ffffff !important; box-shadow: 0 18px 45px rgba(28, 36, 75, 0.10) !important; overflow: visible !important; position: relative !important; z-index: 1 !important; isolation: isolate !important; }\n    .ols-zoom-card.medium { max-width: 820px; }\n    .ols-zoom-card.compact { max-width: 700px; }\n    .ols-zoom-card.wide { max-width: 940px; }\n    .ols-zoom-card:hover { z-index: 50 !important; }\n    .ols-zoom-card-image { display: flex !important; align-items: center !important; justify-content: center !important; width: 100% !important; min-height: 240px !important; padding: 20px !important; background: #ffffff !important; overflow: visible !important; border-top-left-radius: 26px !important; border-top-right-radius: 26px !important; position: relative !important; z-index: 2 !important; }\n    .ols-zoom-card img.ols-zoomable-img { display: block !important; max-width: 100% !important; height: auto !important; border-radius: 18px !important; cursor: zoom-in !important; pointer-events: auto !important; user-select: none !important; -webkit-user-drag: none !important; transform: translateZ(0) scale(1) !important; transform-origin: center center !important; transition: transform 0.32s ease, box-shadow 0.32s ease, filter 0.32s ease !important; position: relative !important; z-index: 2 !important; }\n    @media (hover: hover) and (pointer: fine) { .ols-zoom-card img.ols-zoomable-img:hover { transform: translateZ(0) scale(1.35) !important; box-shadow: 0 28px 70px rgba(28, 36, 75, 0.34) !important; filter: saturate(1.02) contrast(1.01) !important; z-index: 100 !important; } }\n    .ols-zoom-card-caption { padding: 18px 22px 20px !important; background: linear-gradient(135deg, #ffffff, #f8fbff) !important; border-bottom-left-radius: 26px !important; border-bottom-right-radius: 26px !important; position: relative !important; z-index: 1 !important; }\n    .ols-zoom-card-caption p { margin: 0 !important; color: #5f6b85 !important; font-size: 15px !important; line-height: 1.65 !important; font-weight: 300 !important; font-style: italic !important; font-family: Poppins, Arial, sans-serif !important; }\n    .ols-image-lightbox { position: fixed; inset: 0; z-index: 999999; display: none; align-items: center; justify-content: center; padding: 34px; background: rgba(10, 15, 35, 0.86); backdrop-filter: blur(8px); -webkit-backdrop-filter: blur(8px); }\n    .ols-image-lightbox.is-open { display: flex; }\n    .ols-image-lightbox-inner { position: relative; width: min(96vw, 1500px); max-height: 92vh; display: flex; align-items: center; justify-content: center; }\n    .ols-image-lightbox-img { display: block; max-width: 100%; max-height: 92vh; height: auto; width: auto; border-radius: 22px; background: #ffffff; box-shadow: 0 32px 90px rgba(0, 0, 0, 0.45); object-fit: contain; }\n    .ols-image-lightbox-close { position: absolute; top: -18px; right: -18px; width: 46px; height: 46px; border: 0; border-radius: 50%; background: #ffffff; color: var(--navy); font-family: Poppins, Arial, sans-serif; font-size: 28px; line-height: 1; font-weight: 700; cursor: pointer; box-shadow: 0 16px 34px rgba(0, 0, 0, 0.28); display: flex; align-items: center; justify-content: center; transition: transform 0.2s ease, background 0.2s ease, color 0.2s ease; }\n    .ols-image-lightbox-close:hover { transform: scale(1.08); background: var(--blue); color: #ffffff; }\n    @media (max-width: 760px) { .ols-zoom-card { border-radius: 22px !important; overflow: hidden !important; } .ols-zoom-card-image { min-height: auto !important; padding: 12px !important; overflow: hidden !important; border-top-left-radius: 22px !important; border-top-right-radius: 22px !important; } .ols-zoom-card img.ols-zoomable-img, .ols-zoom-card img.ols-zoomable-img:hover { transform: none !important; box-shadow: none !important; } .ols-zoom-card-caption { border-bottom-left-radius: 22px !important; border-bottom-right-radius: 22px !important; } .ols-image-lightbox { padding: 16px; } .ols-image-lightbox-inner { width: 100%; max-height: 88vh; } .ols-image-lightbox-img { max-height: 88vh; border-radius: 16px; } .ols-image-lightbox-close { top: 10px; right: 10px; width: 42px; height: 42px; font-size: 26px; } }\n\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 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{\n      .ols-electronegativity-9ch0-page .ols-title-card,\n      .ols-electronegativity-9ch0-page .ols-note-card,\n      .ols-electronegativity-9ch0-page .ols-h5p-card,\n      .ols-electronegativity-9ch0-page .ols-related-card,\n      .ols-electronegativity-9ch0-page .ols-faq-card,\n      .ols-electronegativity-9ch0-page .ols-attribution-card {\n        overflow: hidden !important;\n      }\n\n      .ols-electronegativity-9ch0-page .ols-card3-half-size {\n        width: 100% !important;\n        max-width: 100% !important;\n      }\n\n      .ols-electronegativity-9ch0-page .ols-card3-half-size .ols-zoom-card-image {\n        min-height: auto !important;\n        padding: 12px !important;\n      }\n    }\n\n  \n    .ols-figure-placeholder .ols-placeholder-box { border: 2px dashed #c9973a; background: #fffaf0; border-radius: 16px; padding: 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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\/\n        <span>Electronegativity<\/span>\n      <\/nav>\n\n      <header class=\"ols-title-card\">\n        <h1>Electronegativity<\/h1>\n        <p class=\"ols-page-intro\">A concise revision guide to electronegativity, bond polarity, non-polar covalent bonds, polar covalent bonds, permanent dipoles and the link between electronegativity difference and bonding type.<\/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: electron-density (26 Sep 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-eldn-001 .eldn-key i.k-ball{border-radius:50%;}\n\n@media (max-width:760px){\n  .ols-eldn-001{padding:26px; border-radius:22px;}\n  .ols-eldn-001 h2.eldn-title{font-size:20.5px;}\n  .ols-eldn-001 p.eldn-sub{font-size:13.5px;}\n  .ols-eldn-001 .eldn-stage{height:400px;}\n  .ols-eldn-001 .eldn-rowlab{min-width:100%;}\n  .ols-eldn-001 .eldn-seg button{padding:9px 13px; font-size:13px;}\n  .ols-eldn-001 .eldn-lab{font-size:10.5px; padding:4px 8px;}\n  .ols-eldn-001 .eldn-lab.l-part{font-size:9.5px; padding:3px 7px;}\n  .ols-eldn-001 .eldn-lab.l-read{font-size:12px; padding:5px 9px;}\n  .ols-eldn-001 .eldn-caption{font-size:10.5px; padding:5px 9px; max-width:64%;}\n  .ols-eldn-001 .eldn-badge{font-size:10.5px; padding:4px 9px;}\n  .ols-eldn-001 .eldn-badge.b-eq{font-size:11px;}\n  .ols-eldn-001 .eldn-badges{max-width:calc(100% - 28px);}\n  .ols-eldn-001 .eldn-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-eldn-001 .eldn-hint{display:none;}\n  .ols-eldn-001 .eldn-caption{max-width:calc(100% - 28px);}\n}\n@media (prefers-reduced-motion:reduce){\n  .ols-eldn-001 .eldn-seg button,.ols-eldn-001 .eldn-pill{transition:none;}\n}\n\n.ols-cc-eldn-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-eldn-001 a{color:#aab0c0; text-decoration:none;}\n.ols-cc-eldn-001 a:hover{text-decoration:underline;}\n.ols-eldn-001 .eldn-seg button{display:inline-flex; align-items:center;}\n.ols-eldn-001 .eldn-seg button .eldn-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-eldn-001 .eldn-seg button[aria-pressed=\"true\"] .eldn-n{background:#ffffff; color:#2563eb;}\n<\/style>\n\n<div class=\"eldn-head\">\n  <h2 class=\"eldn-title\">Electron Density in Covalent and Ionic Bonds<\/h2>\n  <p class=\"eldn-sub\">Choose a step to watch the electron density in Cl\u2082, HCl and NaCl shift as the electronegativity difference grows, from non-polar to polar to ionic.<\/p>\n<\/div>\n\n<div class=\"eldn-stage\" id=\"eldnStage\">\n  <canvas class=\"eldn-canvas\" id=\"eldnCanvas\"><\/canvas>\n  <div class=\"eldn-overlay\" id=\"eldnOverlay\"><\/div>\n  <div class=\"eldn-caption\" id=\"eldnCaption\"><\/div>\n  <div class=\"eldn-hint\" id=\"eldnHint\">Drag to rotate<\/div>\n  <div class=\"eldn-badges\" id=\"eldnBadges\"><\/div>\n<\/div>\n\n<div class=\"eldn-controls\">\n  <div class=\"eldn-row\">\n    <span class=\"eldn-rowlab\">Step<\/span>\n    <div class=\"eldn-seg\" role=\"group\" aria-label=\"Step\">\n      <button type=\"button\" data-step=\"1\" aria-pressed=\"true\"><span class=\"eldn-n\">1<\/span>Non-polar: Cl\u2082<\/button>\n      <button type=\"button\" data-step=\"2\" aria-pressed=\"false\"><span class=\"eldn-n\">2<\/span>Polar: HCl<\/button>\n      <button type=\"button\" data-step=\"3\" aria-pressed=\"false\"><span class=\"eldn-n\">3<\/span>Ionic: NaCl<\/button>\n      <button type=\"button\" data-step=\"4\" aria-pressed=\"false\"><span class=\"eldn-n\">4<\/span>Contour map<\/button>\n      <button type=\"button\" data-step=\"5\" aria-pressed=\"false\"><span class=\"eldn-n\">5<\/span>\u0394EN rises<\/button>\n    <\/div>\n  <\/div>\n\n  <div class=\"eldn-row\">\n    <span class=\"eldn-rowlab\">View<\/span>\n    <button type=\"button\" class=\"eldn-pill\" id=\"eldnResetV\">Reset view<\/button>\n  <\/div>\n<\/div>\n\n<div class=\"eldn-info\">\n  <h3 id=\"eldnInfoTitle\"><\/h3>\n  <p id=\"eldnInfoText\"><\/p>\n  <div class=\"eldn-facts\" id=\"eldnFacts\"><\/div>\n  <div class=\"eldn-key\">\n    <span><i class=\"\" style=\"background:rgba(40,70,170,0.45)\"><\/i>Electron density<\/span>\n    <span><i class=\"\" style=\"background:linear-gradient(90deg,#c0392b,#e8a02a,#4aa86a,#4a5ad0)\"><\/i>Contours: high to low<\/span>\n    <span><i class=\"k-ball\" style=\"background:#ececf0\"><\/i>H<\/span>\n    <span><i class=\"k-ball\" style=\"background:#34aa48\"><\/i>Cl<\/span>\n    <span><i class=\"k-ball\" style=\"background:#8c50c8\"><\/i>Na<\/span>\n    <span><i class=\"k-ball\" style=\"background:#facc28\"><\/i>Electron<\/span>\n  <\/div>\n<\/div>\n\n<script src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/JS\/electron-density.js?v=20261025p\"><\/script>\n<\/section>\n\n<p class=\"ols-cc-eldn-001\">&copy; Dr. Mohammed Al-Fatah &#8211; <a href=\"https:\/\/www.onlinelearningsystem.net\" target=\"_blank\" rel=\"noopener\">onlinelearningsystem.net<\/a><\/p>\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: Attraction for Electrons and Bond Type<\/h2>\n<p>Before you start, check the GCSE ideas about attracting electrons that this page builds on.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"674\"><\/div><\/div>\n<\/section>\n<article class=\"ols-note-card soft\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">1<\/div>\n          <h2>What Is Electronegativity?<\/h2>\n        <\/div>\n\n        <p><strong>Electronegativity<\/strong> is the relative tendency of an atom in a covalent bond to attract the shared pair of electrons towards itself.<\/p>\n        <p>The more electronegative atom pulls bonding electron density more strongly. This can make the bonding electrons unevenly distributed between the bonded atoms.<\/p>\n        <p>Electronegativity values are commonly compared using the <strong>Pauling scale<\/strong>. Fluorine is the most electronegative element, with a value of <strong>4.0<\/strong>.<\/p>\n\n        <div class=\"ols-definition-box\">\n          <p><strong>Definition:<\/strong> Electronegativity is the ability of an atom in a covalent bond to attract the shared electrons in that bond towards itself.<\/p>\n<p>Mark schemes accept <strong>ability<\/strong>, <strong>power<\/strong> or <strong>relative tendency<\/strong>, provided you say that the atom is in a covalent bond and that the electrons are the shared pair.<\/p>\n        <\/div>\n\n        <div class=\"ols-key-box\">\n          <p><strong>Key idea:<\/strong> Electronegativity only becomes meaningful when atoms are bonded. It tells you which atom attracts the bonding electrons more strongly.<\/p>\n        <\/div>\n\n        \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: What Does &#039;More Electronegative&#039; Mean?<\/h2>\n<p>Pick the statement that uses the idea of electronegativity correctly.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-173\" class=\"h5p-iframe\" data-content-id=\"173\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Electronegativity MCQ: What &#039;More Electronegative&#039; Means in a C\u2013O Bond\"><\/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>Trends in Electronegativity<\/h2>\n        <\/div>\n\n        <p>Electronegativity generally <strong>increases across a period<\/strong> and <strong>increases up a group<\/strong>, excluding noble gases.<\/p>\n        <p>Across a period, nuclear charge increases and atomic radius decreases, while the <strong>shielding stays about the same<\/strong> because each extra electron is added to the same shell. The bonding electrons are attracted more strongly because the nucleus has a stronger pull on the shared electrons.<\/p>\n        <p>Down a group, atoms have more electron shells. The bonding electrons are further from the nucleus and more shielded, so the attraction is weaker.<\/p>\n\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Most electronegative common elements<\/h3>\n            <p>Fluorine, oxygen, nitrogen and chlorine are key electronegative elements to recognise in A Level bonding questions.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Fluorine is highest<\/h3>\n            <p>Fluorine has the strongest attraction for bonding electrons on the Pauling scale.<\/p>\n          <\/div>\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-10-entrends.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-10-entrends.jpg\" alt=\"Heat-map outline of the main-group elements with Pauling electronegativity values, arrows for the trends and the reasons\">\n<\/a>\n<\/div>\n<div class=\"ols-zoom-card-caption\"><p>Electronegativity rises across a period and falls down a group, so fluorine at the top right is the most electronegative element.<\/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: Rank by Electronegativity<\/h2>\n<p>Use the two trends to put six elements in order, least electronegative first.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-675\" class=\"h5p-iframe\" data-content-id=\"675\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Electronegativity Sort: Ranking Six Elements from the Trends\"><\/iframe><\/div><\/div>\n<\/section>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Explain a Group Trend<\/h2>\n<p>Write a short explanation, then compare it with the mark points and the model answer.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-676\" class=\"h5p-iframe\" data-content-id=\"676\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Electronegativity Explain: Oxygen Compared with Sulfur\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card purple\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">3<\/div>\n          <h2>Electronegativity Difference and Bond Type<\/h2>\n        <\/div>\n\n        <p>The <strong>electronegativity difference<\/strong>, often written as &Delta;EN, helps predict whether a bond is best described as non-polar covalent, polar covalent or ionic.<\/p>\n        <p>As a rough guide, a difference below about <strong>0.4<\/strong> leaves a bond essentially non-polar covalent, a difference from about 0.4 up to about <strong>1.7 to 2.0<\/strong> gives a polar covalent bond, and a difference larger than that is usually described as mainly ionic.<\/p>\n        <p>These boundaries are useful revision guides, not rules, and different boards and textbooks draw the lines in slightly different places.<\/p>\n<p>Real bonding exists on a continuum, so increasing &Delta;EN usually means increasing ionic character. Quote the value of &Delta;EN and compare the ionic character rather than declaring a bond simply ionic or simply covalent.<\/p>\n        <p>These are the Pauling values used most often at A Level. Some data booklets print an older set (H 2.1, C 2.5, O 3.5, Cl 3.0), so always work from the values printed in the question.<\/p>\n\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Element<\/th>\n                <th>Pauling electronegativity<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Element\"><strong>Na<\/strong><\/td>\n                <td data-label=\"Pauling electronegativity\">0.9<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Element\"><strong>Mg<\/strong><\/td>\n                <td data-label=\"Pauling electronegativity\">1.3<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Element\"><strong>H<\/strong><\/td>\n                <td data-label=\"Pauling electronegativity\">2.2<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Element\"><strong>C<\/strong><\/td>\n                <td data-label=\"Pauling electronegativity\">2.6<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Element\"><strong>N<\/strong><\/td>\n                <td data-label=\"Pauling electronegativity\">3.0<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Element\"><strong>Cl<\/strong><\/td>\n                <td data-label=\"Pauling electronegativity\">3.2<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Element\"><strong>O<\/strong><\/td>\n                <td data-label=\"Pauling electronegativity\">3.4<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Element\"><strong>F<\/strong><\/td>\n                <td data-label=\"Pauling electronegativity\">4.0<\/td>\n              <\/tr>\n            <\/tbody>\n          <\/table>\n        <\/div>\n\n        <div class=\"ols-figure-card ols-zoom-card wide ols-card3-half-size\">\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-img-40-enbondtype.jpg\" alt=\"Table linking electronegativity difference below 0.4, 0.4 to 1.7 and above 1.7 to non-polar, polar and ionic bonding\">\n          <\/div>\n          <div class=\"ols-figure-caption ols-zoom-card-caption\">\n            <p>As the difference in electronegativity increases, the bond shows more ionic character.<\/p>\n          <\/div>\n        <\/div>\n\n        <div class=\"ols-figure-card ols-zoom-card wide ols-card3-half-size\">\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-img-02-ioniccharacter.jpg\" alt=\"S-shaped curve of percentage ionic character against electronegativity difference, with HCl, NaCl and CsF marked and the 50 % line at 1.7\">\n          <\/div>\n          <div class=\"ols-figure-caption ols-zoom-card-caption\">\n            <p>The percentage ionic character increases as the electronegativity difference becomes larger.<\/p>\n          <\/div>\n        <\/div>\n      <\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Calculating \u0394EN<\/h2>\n<p>Calculate electronegativity differences from Pauling values and use them to compare ionic character.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"175\"><\/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>Non-Polar Covalent Bonds<\/h2>\n        <\/div>\n\n        <p>A <strong>non-polar covalent bond<\/strong> forms when the bonded atoms have identical or very similar electronegativities.<\/p>\n        <p>The shared pair of electrons is attracted equally by both nuclei. There is no charge separation, so the bond has <strong>no permanent dipole<\/strong>.<\/p>\n        <p>Examples include bonds in <strong>Cl<sub>2<\/sub><\/strong>, <strong>H<sub>2<\/sub><\/strong> and <strong>N<sub>2<\/sub><\/strong>, because each bond is between identical atoms.<\/p>\n        <p>The two atoms do not have to be identical. The <strong>C-H<\/strong> bond has an electronegativity difference of only about 0.4, so it is treated as essentially non-polar all the way through organic chemistry.<\/p>\n<p>Any bond between two atoms of similar electronegativity behaves in the same way.<\/p>\n\n        <div class=\"ols-key-box\">\n          <p><strong>Exam focus:<\/strong> Non-polar covalent bonds have electron density distributed symmetrically, so there is no &delta;+ end and no &delta;- end.<\/p>\n        <\/div>\n\n        <div class=\"ols-nonpolar-density-grid\">\n          \n\n          \n        <\/div>\n      <\/article>\n\n      <article class=\"ols-note-card orange\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">5<\/div>\n          <h2>Polar Covalent Bonds and Permanent Dipoles<\/h2>\n        <\/div>\n\n        <p>A <strong>polar covalent bond<\/strong> forms when one bonded atom is more electronegative than the other.<\/p>\n        <p>The more electronegative atom pulls the bonding electrons closer. This creates <strong>charge separation<\/strong>, with a partial negative charge on the more electronegative atom and a partial positive charge on the less electronegative atom.<\/p>\n        <p>Partial charges are written using delta symbols: <strong>&delta;+<\/strong> means slightly positive and <strong>&delta;-<\/strong> means slightly negative.<\/p>\n        <p>Always compare the two atoms in the bond you are given. &delta;- is not a fixed property of an element: an atom is &delta;- only when its partner in that bond is less electronegative than it is.<\/p>\n<p>Hydrogen is usually &delta;+, but it is &delta;- when it is bonded to an atom of lower electronegativity, and even an atom you expect to be &delta;-, such as oxygen, is &delta;+ if its partner is more electronegative still.<\/p>\n\n        <div class=\"ols-definition-box\">\n          <p><strong>Permanent dipole:<\/strong> A permanent separation of charge across a bond or molecule, caused by unequal sharing of bonding electrons.<\/p>\n        <\/div>\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-35.jpg\" alt=\"A polar H-Cl bond: chlorine pulls the shared pair, giving delta plus on hydrogen and delta minus on chlorine.\"><\/div>\n<div class=\"ols-figure-caption\"><p>In HCl, chlorine attracts the bonding electrons more strongly, so chlorine becomes &delta;- and hydrogen becomes &delta;+.<\/p><\/div>\n<\/div>\n\n        \n\n\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: \u03b4+ or \u03b4\u2212?<\/h2>\n<p>Use the Pauling values given to assign the partial charges in six bonds this page has not used.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-174\" class=\"h5p-iframe\" data-content-id=\"174\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Electronegativity Quick Fire: Assigning \u03b4+ and \u03b4\u2212 in Six New Bonds\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">6<\/div>\n          <h2>Bond Dipoles and Molecular Polarity<\/h2>\n        <\/div>\n\n        <p>A <strong>bond dipole<\/strong> shows the direction of polarity in a bond. In chemistry diagrams, the arrow points towards the more electronegative atom.<\/p>\n        <p>A molecule with polar bonds is not automatically a polar molecule. The overall molecular polarity depends on the shape of the molecule and whether the bond dipoles cancel.<\/p>\n        <p>This becomes especially important in the next subtopic, <strong>polar and non-polar molecules<\/strong>.<\/p>\n\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Term<\/th>\n                <th>Meaning<\/th>\n                <th>Common exam wording<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Term\"><strong>Bond polarity<\/strong><\/td>\n                <td data-label=\"Meaning\">Unequal sharing of electrons in a covalent bond.<\/td>\n                <td data-label=\"Common exam wording\">One atom is more electronegative and attracts the bonding pair more strongly.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Term\"><strong>Bond dipole<\/strong><\/td>\n                <td data-label=\"Meaning\">A partial charge separation across a bond.<\/td>\n                <td data-label=\"Common exam wording\">The less electronegative atom is &delta;+ and the more electronegative atom is &delta;-.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Term\"><strong>Molecular polarity<\/strong><\/td>\n                <td data-label=\"Meaning\">The overall polarity of the molecule after considering all bond dipoles and shape.<\/td>\n                <td data-label=\"Common exam wording\">Dipoles may cancel in symmetrical molecules.<\/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: Spot the Accurate Statement<\/h2>\n<p>In each round, pick the one statement about polar bonds and dipoles that is accurate.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-172\" class=\"h5p-iframe\" data-content-id=\"172\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Electronegativity Summary: Spot the Accurate Statement\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">7<\/div>\n          <h2>Common Exam Points<\/h2>\n        <\/div>\n\n        <p>Strong electronegativity answers link the definition to <strong>bonding electrons<\/strong>, <strong>partial charges<\/strong> and <strong>permanent dipoles<\/strong>.<\/p>\n\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Do not define electronegativity using lone pairs<\/h3>\n            <p>Electronegativity is about attracting the shared pair of electrons in a covalent bond.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Use partial charges for polar covalent bonds<\/h3>\n            <p>The more electronegative atom is &delta;-, while the less electronegative atom is &delta;+.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Non-polar bonds have no charge separation<\/h3>\n            <p>Identical atoms have the same electronegativity, so electrons are shared equally and no dipole forms.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Bond type is a continuum<\/h3>\n            <p>Electronegativity difference is a guide. A larger difference means greater ionic character.<\/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>Electronegativity explains how strongly an atom attracts bonding electrons. When bonded atoms attract the shared electrons equally, the bond is non-polar. When one atom attracts them more strongly, the bond becomes polar and has partial charges.<\/p>\n\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Electronegativity<\/h3>\n            <p>Relative tendency of an atom in a covalent bond to attract the shared electrons towards itself.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Non-polar covalent bond<\/h3>\n            <p>Bonding electrons are shared equally or almost equally, so there is no permanent dipole.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Polar covalent bond<\/h3>\n            <p>Bonding electrons are shared unequally, giving a &delta;+ end and a &delta;- end.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Ionic character<\/h3>\n            <p>A larger electronegativity difference gives a bond with more ionic character.<\/p>\n          <\/div>\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-img-01-bondspectrum.jpg\" alt=\"Bonding continuum from Cl\u2082 (equal sharing) through HCl (\u03b4+ \u03b4\u2212) to Na\u207aCl\u207b (transfer), with an electronegativity difference scale beneath\">\n          <\/div>\n          <div class=\"ols-figure-caption ols-zoom-card-caption\">\n            <p>Use this visual comparison to connect electron distribution with ionic, polar covalent and non-polar covalent bonding.<\/p>\n          <\/div>\n        <\/div>\n      <\/article>\n\n            <section class=\"ols-faq-card\">\n        <h2>FAQs<\/h2>\n        <p>These answers summarise the key ideas students often confuse when revising electronegativity and bond polarity.<\/p>\n\n        <div class=\"ols-faq-list\">\n          <div class=\"ols-faq-item\">\n            <h3>What is electronegativity?<\/h3>\n            <p>Electronegativity is the relative tendency of an atom in a covalent bond to attract the shared pair of electrons towards itself.<\/p>\n          <\/div>\n\n          <div class=\"ols-faq-item\">\n            <h3>Which element is the most electronegative?<\/h3>\n            <p>Fluorine is the most electronegative element on the Pauling scale, with an electronegativity value of 4.0.<\/p>\n          <\/div>\n\n          <div class=\"ols-faq-item\">\n            <h3>What makes a bond polar?<\/h3>\n            <p>A bond is polar when the bonded atoms have different electronegativities, so the bonding electrons are attracted more strongly by one atom.<\/p>\n          <\/div>\n\n          <div class=\"ols-faq-item\">\n            <h3>What do &delta;+ and &delta;- mean?<\/h3>\n            <p>&delta;+ means slightly positive and &delta;- means slightly negative. These symbols show partial charges in polar covalent bonds.<\/p>\n          <\/div>\n\n          <div class=\"ols-faq-item\">\n            <h3>Is a molecule with polar bonds always polar?<\/h3>\n            <p>No. A molecule can contain polar bonds but still be non-polar overall if the bond dipoles cancel because of the molecular shape.<\/p>\n          <\/div>\n        <\/div>\n      <\/section>\n\n      <!-- author card (moved to the end, 10 Oct 2026) -->\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: Dr. Mohammed Al-Fatah\n      <\/h2>\n\n      <p class=\"ols-author-description\">\n        Chemistry specialist revision notes for A Level Chemistry.\n      <\/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\"\/>\n        <\/svg>\n        View LinkedIn Profile\n      <\/a>\n\n    <\/div>\n\n  <\/div>\n\n\n      <section class=\"ols-related-card\">\n        <h2>Related Topics<\/h2>\n        <p>Continue revising the Edexcel Topic 2 bonding ideas that connect directly to electronegativity and polarity.<\/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\/\">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\/polar-molecules\/\">Polar &amp; Non-Polar 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\/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\/ionic-bonding\/\">Ionic Bonding &amp; Structure<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/metallic-bonding-and-structure\/\">Metallic Bonding &amp; 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=\"olsImageLightboxElectronegativity9ch0\" 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-electronegativity-9ch0-page\");\n          if (!page) { return; }\n          var lightbox = page.querySelector(\"#olsImageLightboxElectronegativity9ch0\");\n          if (!lightbox) { return; }\n          var lightboxImage = lightbox.querySelector(\".ols-image-lightbox-img\");\n          var closeButton = 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