{"id":4594,"date":"2026-05-30T06:13:07","date_gmt":"2026-05-30T05:13:07","guid":{"rendered":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/distorted-t\/"},"modified":"2026-10-25T12:08:54","modified_gmt":"2026-10-25T12:08:54","slug":"distorted-t","status":"publish","type":"page","link":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/distorted-t\/","title":{"rendered":"Distorted T"},"content":{"rendered":"\n<section class=\"ols-revision-page ols-distorted-t-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: 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}\n      .ols-figure-caption { padding: 16px; }\n      .ols-table-wrap { border: none; background: transparent; }\n      .ols-table, .ols-table thead, .ols-table tbody, .ols-table th, .ols-table td, .ols-table tr { display: block; width: 100%; }\n      .ols-table { border-collapse: separate; border-spacing: 0; }\n      .ols-table thead { display: none; }\n      .ols-table tr { margin-bottom: 14px; border: 1px solid var(--border); border-radius: 18px; overflow: hidden; background: #ffffff; box-shadow: var(--inner-shadow); }\n      .ols-table td { border-bottom: 1px solid var(--border); padding: 14px 16px; overflow-wrap: anywhere; }\n      .ols-table td:last-child { border-bottom: none; }\n      .ols-table td::before { content: attr(data-label); display: block; margin-bottom: 6px; font-size: 13px; font-weight: 700; color: var(--blue); }\n      .ols-author { align-items: flex-start; padding: 22px 18px; border-radius: 22px; }\n      .ols-author-avatar-img { width: 72px; height: 72px; }\n      .ols-author-title { font-size: 24px; }\n      .ols-author-description { font-size: 15px; }\n    }\n  \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) 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href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/\">Topic 2 Bonding and Structure<\/a> \/\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/\">Shapes of Molecules<\/a> \/\n        <span>Distorted T<\/span>\n      <\/nav>\n\n      <header class=\"ols-title-card\">\n        <h1>Distorted T Molecular Shape<\/h1>\n        <p class=\"ols-page-intro\">A focused revision guide to the distorted T molecular shape, using ClF<sub>3<\/sub> as the key example. This page explains why three bonding pairs and two lone pairs around a central atom give a T-shaped arrangement with bond angles slightly less than 90&deg;.<\/p>\n\n        <div class=\"ols-badges\">\n          <div class=\"ols-badge\">Unit: Paper 1<\/div>\n          <div class=\"ols-badge\">Topic 2: Bonding and Structure<\/div>\n          <div class=\"ols-badge\">9CH0\/01<\/div>\n        <\/div>\n      <\/header>\n<!-- 3D card: clf3-distorted-t (swapped 26 Sep 2026) -->\n<!-- Copyright (c) 2026 Dr. Mohammed Al-Fatah, onlinelearningsystem.net. All rights reserved. -->\n<!-- 3D card: clf3-distorted-t (rebuilt Oct 2026) -->\n<!-- Copyright (c) 2026 Dr. Mohammed Al-Fatah, onlinelearningsystem.net. 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border:1px solid rgba(28,36,75,0.18);\n}\n.ols-cltt-001 .cltt-key i.k-ball{border-radius:50%;}\n\n@media (max-width:760px){\n  .ols-cltt-001{padding:26px; border-radius:22px;}\n  .ols-cltt-001 h2.cltt-title{font-size:20.5px;}\n  .ols-cltt-001 p.cltt-sub{font-size:13.5px;}\n  .ols-cltt-001 .cltt-stage{height:400px;}\n  .ols-cltt-001 .cltt-rowlab{min-width:100%;}\n  .ols-cltt-001 .cltt-seg button{padding:9px 13px; font-size:13px;}\n  .ols-cltt-001 .cltt-lab{font-size:10.5px; padding:4px 8px;}\n  .ols-cltt-001 .cltt-lab.l-part{font-size:9.5px; padding:3px 7px;}\n  .ols-cltt-001 .cltt-lab.l-read{font-size:12px; padding:5px 9px;}\n  .ols-cltt-001 .cltt-caption{font-size:10.5px; padding:5px 9px; max-width:64%;}\n  .ols-cltt-001 .cltt-badge{font-size:10.5px; padding:4px 9px;}\n  .ols-cltt-001 .cltt-badge.b-eq{font-size:11px;}\n  .ols-cltt-001 .cltt-badges{max-width:calc(100% - 28px);}\n  .ols-cltt-001 .cltt-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-cltt-001 .cltt-hint{display:none;}\n  .ols-cltt-001 .cltt-caption{max-width:calc(100% - 28px);}\n}\n@media (prefers-reduced-motion:reduce){\n  .ols-cltt-001 .cltt-seg button,.ols-cltt-001 .cltt-pill{transition:none;}\n}\n\n.ols-cc-cltt-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-cltt-001 a{color:#aab0c0; text-decoration:none;}\n.ols-cc-cltt-001 a:hover{text-decoration:underline;}\n.ols-cltt-001 .cltt-seg button{display:inline-flex; align-items:center;}\n.ols-cltt-001 .cltt-seg button .cltt-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-cltt-001 .cltt-seg button[aria-pressed=\"true\"] .cltt-n{background:#ffffff; color:#2563eb;}\n<\/style>\n\n<div class=\"cltt-head\">\n  <h2 class=\"cltt-title\">Distorted T Shape of ClF\u2083<\/h2>\n  <p class=\"cltt-sub\">Choose a step to watch five electron pairs spread out round chlorine, two lone pairs take equatorial positions, and the T bend to about 87.5\u00b0.<\/p>\n<\/div>\n\n<div class=\"cltt-stage\" id=\"clttStage\">\n  <canvas class=\"cltt-canvas\" id=\"clttCanvas\"><\/canvas>\n  <div class=\"cltt-overlay\" id=\"clttOverlay\"><\/div>\n  <div class=\"cltt-caption\" id=\"clttCaption\"><\/div>\n  <div class=\"cltt-hint\" id=\"clttHint\">Drag to rotate<\/div>\n  <div class=\"cltt-badges\" id=\"clttBadges\"><\/div>\n<\/div>\n\n<div class=\"cltt-controls\">\n  <div class=\"cltt-row\">\n    <span class=\"cltt-rowlab\">Step<\/span>\n    <div class=\"cltt-seg\" role=\"group\" aria-label=\"Step\">\n      <button type=\"button\" data-step=\"1\" aria-pressed=\"true\"><span class=\"cltt-n\">1<\/span>Five electron pairs<\/button>\n      <button type=\"button\" data-step=\"2\" aria-pressed=\"false\"><span class=\"cltt-n\">2<\/span>Two lone pairs equatorial<\/button>\n      <button type=\"button\" data-step=\"3\" aria-pressed=\"false\"><span class=\"cltt-n\">3<\/span>Bent to 87.5\u00b0<\/button>\n      <button type=\"button\" data-step=\"4\" aria-pressed=\"false\"><span class=\"cltt-n\">4<\/span>Why equatorial?<\/button>\n    <\/div>\n  <\/div>\n\n  <div class=\"cltt-row\">\n    <span class=\"cltt-rowlab\">View<\/span>\n    <button type=\"button\" class=\"cltt-pill\" id=\"clttResetV\">Reset view<\/button>\n  <\/div>\n<\/div>\n\n<div class=\"cltt-info\">\n  <h3 id=\"clttInfoTitle\"><\/h3>\n  <p id=\"clttInfoText\"><\/p>\n  <div class=\"cltt-facts\" id=\"clttFacts\"><\/div>\n  <div class=\"cltt-key\">\n    <span><i class=\"k-ball\" style=\"background:#2ea040\"><\/i>Chlorine<\/span>\n    <span><i class=\"k-ball\" style=\"background:#b8de6e\"><\/i>Fluorine<\/span>\n    <span><i class=\"\" style=\"background:rgba(70,128,220,0.45)\"><\/i>Electron pair (bonding)<\/span>\n    <span><i class=\"\" style=\"background:rgba(128,92,214,0.5)\"><\/i>Lone pair<\/span>\n    <span><i class=\"k-ball\" style=\"background:#fac828\"><\/i>Electron<\/span>\n    <span><i class=\"\" style=\"background:#c9961c\"><\/i>Bond angle<\/span>\n    <span><i class=\"\" style=\"background:#d43a32\"><\/i>Lone pair\u2013bond clash at 90\u00b0<\/span>\n  <\/div>\n<\/div>\n\n<script src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/JS\/clf3-distorted-t.js?v=20261025p\"><\/script>\n<\/section>\n\n<p class=\"ols-cc-cltt-001\">&copy; Dr. Mohammed Al-Fatah &#8211; <a href=\"https:\/\/www.onlinelearningsystem.net\" target=\"_blank\" rel=\"noopener\">onlinelearningsystem.net<\/a><\/p>\n\n\n<style>\n  .ols-distorted-t-9ch0-page .ols-spec-grid {\n    display: grid;\n    grid-template-columns: repeat(3, minmax(0, 1fr));\n    gap: 14px;\n    margin-top: 18px;\n  }\n  .ols-distorted-t-9ch0-page .ols-spec-box {\n    background: #ffffff;\n    border: 1px solid var(--border);\n    border-radius: 18px;\n    padding: 18px;\n    box-shadow: var(--inner-shadow);\n  }\n  .ols-distorted-t-9ch0-page .ols-spec-box strong {\n    display: block;\n    font-size: 15px;\n    color: var(--blue);\n    margin-bottom: 6px;\n  }\n  .ols-distorted-t-9ch0-page .ols-spec-box span {\n    display: block;\n    font-size: 17px;\n    line-height: 1.55;\n    color: var(--body-text);\n    font-weight: 300;\n    overflow-wrap: anywhere;\n  }\n  .ols-distorted-t-9ch0-page .ols-h5p-grid {\n    display: grid;\n    gap: 18px;\n    margin-top: 22px;\n  }\n  .ols-distorted-t-9ch0-page .ols-h5p-frame {\n    margin-top: 0;\n  }\n  .ols-distorted-t-9ch0-page .ols-formula {\n    white-space: nowrap;\n  }\n  @media (max-width: 760px) {\n    .ols-distorted-t-9ch0-page .ols-spec-grid {\n      grid-template-columns: 1fr;\n    }\n  }\n<\/style>\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: Halogen Atoms and Their Electron Pairs<\/h2>\n<p>Before you start, check that you can count the shared pairs and lone pairs on a halogen atom.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"665\"><\/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 Distorted T Means<\/h2>\n        <\/div>\n        <p>A <strong>distorted T<\/strong> molecule has three atoms bonded to a central atom in a T-shaped arrangement. It is called distorted because the bond angles are slightly compressed by lone pair repulsion.<\/p>\n        <p>The key example for this page is <strong>ClF<sub>3<\/sub><\/strong>. Chlorine is the central atom, three fluorine atoms are bonded to chlorine, and chlorine also has two lone pairs.<\/p>\n\n        <div class=\"ols-spec-grid\">\n          <div class=\"ols-spec-box\">\n            <strong>Bonding pairs<\/strong>\n            <span>3 bonding pairs around the central atom<\/span>\n          <\/div>\n          <div class=\"ols-spec-box\">\n            <strong>Lone pairs<\/strong>\n            <span>2 lone pairs on the central atom<\/span>\n          <\/div>\n          <div class=\"ols-spec-box\">\n            <strong>Bond angle<\/strong>\n            <span>Slightly less than 90&deg;, about 87.5&deg; in ClF<sub>3<\/sub><\/span>\n          <\/div>\n        <\/div>\n\n        <div class=\"ols-key-box\"><p><strong>Key idea:<\/strong> three bonding pairs and two lone pairs around a central atom give a distorted T shape when the two lone pairs occupy equatorial positions in a trigonal bipyramidal electron-pair arrangement.<\/p><\/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>Why ClF<sub>3<\/sub> Is Distorted T-Shaped<\/h2>\n        <\/div>\n        <p>In ClF<sub>3<\/sub>, the central chlorine atom is surrounded by three Cl-F bonding pairs and two lone pairs. This gives five regions of negative charge around chlorine.<\/p>\n        <p>Chlorine therefore has <strong>10 electrons<\/strong> in its outer shell. An atom in Period 3 or below can hold more than eight electrons in this way, so ClF<sub>3<\/sub> exists.<\/p>\n<p>Fluorine is in Period 2 and is limited to eight, which is why it is always the outer atom here.<\/p>\n        <p>Five electron regions arrange themselves as a <strong>trigonal bipyramidal electron-pair arrangement<\/strong> to minimise repulsion. The two lone pairs occupy equatorial positions, where they are approximately 120&deg; apart from each other.<\/p>\n        <p>The <strong>molecular shape<\/strong> only describes the positions of the atoms. Therefore, ClF<sub>3<\/sub> is described as <strong>distorted T-shaped<\/strong>, even though its electron-pair arrangement is trigonal bipyramidal.<\/p>\n        <div class=\"ols-key-box\"><p><strong>How to count:<\/strong><\/p>\n<ol>\n<li>Start with the <strong>outer-shell electrons<\/strong> of the central atom.<\/li>\n<li>Add one electron for each negative charge and take one away for each positive charge.<\/li>\n<li>Each single bond uses one of those electrons and each double bond uses two. A double or triple bond still counts as <strong>one bonding region<\/strong>.<\/li>\n<li>Divide the electrons left over by two to get the lone pairs.<\/li>\n<\/ol>\n<p>In ClF<sub>3<\/sub>: chlorine has <strong>7 outer-shell electrons<\/strong>, the molecule has no charge, and the three Cl-F single bonds use three of them.<\/p>\n<p>Four are left over, which is two lone pairs. Three bonding regions and two lone pairs give five regions, so the arrangement is trigonal bipyramidal and the shape is a distorted T.<\/p><\/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\/10\/t3-cd-18-clf3-distortedt.svg\" alt=\"Distorted T-shaped ClF\u2083 with two equatorial lone pairs on chlorine and an F\u2013Cl\u2013F angle of about 87.5\u00b0\" width=\"1516\" height=\"906\"><\/div>\n<div class=\"ols-figure-caption\"><p>A distorted T species has three bonding regions and two lone pairs around the central atom. ClF3 is the standard example, with bond angles close to 89&deg;.<\/p><\/div>\n<\/div>\n      <div class=\"ols-figure-card ols-zoom-pop\">\n<div class=\"ols-figure-image\">\n<a class=\"ols-image-fullscreen-link\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-32-countclf3.jpg\" target=\"_blank\" rel=\"noopener\" aria-label=\"Open image fullscreen\">\n<img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-32-countclf3.jpg\" alt=\"Five-step electron-pair count for ClF\u2083 giving three bonding pairs, two lone pairs and a distorted T shape\" data-fullscreen-src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-32-countclf3.jpg\">\n<\/a>\n<\/div>\n<div class=\"ols-figure-caption\"><p>Chlorine keeps 4 of its 7 outer electrons as two equatorial lone pairs: the three F atoms form a distorted T.<\/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: Count the Pairs in Three Tribromides<\/h2>\n<p>Work out the lone pairs and electron pairs for three molecules that are not on this page, then type each number.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-213\" class=\"h5p-iframe\" data-content-id=\"213\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Distorted T Flashcards: Counting Electron Pairs in Three Tribromides\"><\/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\">3<\/div>\n          <h2>Electron-Pair Arrangement vs Molecular Shape<\/h2>\n        <\/div>\n        <p>The electron-pair arrangement in ClF<sub>3<\/sub> is based on a <strong>trigonal bipyramidal arrangement<\/strong> because there are five electron regions around chlorine.<\/p>\n        <p>The molecular shape is different. Lone pairs are not counted as atoms when naming the shape, so the visible arrangement of the three fluorine atoms is <strong>distorted T-shaped<\/strong>.<\/p>\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Five electron regions<\/h3>\n            <p>Three bonding pairs and two lone pairs arrange themselves as far apart as possible around chlorine.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Equatorial lone pairs<\/h3>\n            <p>The two lone pairs occupy equatorial positions in the trigonal bipyramidal arrangement. This keeps the lone pairs approximately 120&deg; apart and reduces lone pair-lone pair repulsion.<\/p>\n<p>Count the close neighbours: an <strong>equatorial<\/strong> position has only two at 90&deg;, while an <strong>axial<\/strong> position has three, so a lone pair always takes an equatorial position.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>T-shaped bonded atoms<\/h3>\n            <p>The remaining three bonding pairs form two axial bonds and one equatorial bond, producing a distorted T shape.<\/p>\n          <\/div>\n        <\/div>\n      <div class=\"ols-figure-card ols-zoom-pop\">\n<div class=\"ols-figure-image\">\n<a class=\"ols-image-fullscreen-link\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-21-fivepairs.jpg\" target=\"_blank\" rel=\"noopener\" aria-label=\"Open image fullscreen\">\n<img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-21-fivepairs.jpg\" alt=\"Trigonal bipyramid key with PF\u2085, SF\u2084 and ClF\u2083 sketches showing lone pairs in equatorial positions and their bond angles\" data-fullscreen-src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-21-fivepairs.jpg\">\n<\/a>\n<\/div>\n<div class=\"ols-figure-caption\"><p>Five regions form a trigonal bipyramid; lone pairs take equatorial positions to give the see-saw and distorted T shapes.<\/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: Place the Lone Pairs in Xenon Difluoride<\/h2>\n<p>Use the rule for placing lone pairs to predict the shape of a molecule with three lone pairs.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-214\" class=\"h5p-iframe\" data-content-id=\"214\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Distorted T MCQ: Where Do the Lone Pairs Go in Xenon Difluoride?\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">4<\/div>\n          <h2>Distorted T Shape Examples<\/h2>\n        <\/div>\n        <p>The distorted T shape is found when the central atom has three bonding pairs and two lone pairs. The common exam examples are usually interhalogen species.<\/p>\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Species<\/th>\n                <th>Central atom<\/th>\n                <th>Electron regions<\/th>\n                <th>Shape<\/th>\n                <th>Bond angles<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Species\">ClF<sub>3<\/sub><\/td>\n                <td data-label=\"Central atom\">Cl<\/td>\n                <td data-label=\"Electron regions\">3 bonding regions, 2 lone pairs<\/td>\n                <td data-label=\"Shape\">Distorted T<\/td>\n                <td data-label=\"Bond angles\">About 87.5&deg; and about 175&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">BrF<sub>3<\/sub><\/td>\n                <td data-label=\"Central atom\">Br<\/td>\n                <td data-label=\"Electron regions\">3 bonding regions, 2 lone pairs<\/td>\n                <td data-label=\"Shape\">Distorted T<\/td>\n                <td data-label=\"Bond angles\">Slightly less than 90&deg; and slightly less than 180&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">IF<sub>3<\/sub><\/td>\n                <td data-label=\"Central atom\">I<\/td>\n                <td data-label=\"Electron regions\">3 bonding regions, 2 lone pairs<\/td>\n                <td data-label=\"Shape\">Distorted T<\/td>\n                <td data-label=\"Bond angles\">Slightly less than 90&deg; and slightly less than 180&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">ICl<sub>3<\/sub><\/td>\n                <td data-label=\"Central atom\">I<\/td>\n                <td data-label=\"Electron regions\">3 bonding regions, 2 lone pairs<\/td>\n                <td data-label=\"Shape\">Distorted T<\/td>\n                <td data-label=\"Bond angles\">Slightly less than 90&deg; and slightly less than 180&deg;<\/td>\n              <\/tr>\n            <\/tbody>\n          <\/table>\n        <\/div>\n      <\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Find the Distorted T Species<\/h2>\n<p>Count the electron pairs around each central atom and click every species with three bonding pairs and two lone pairs.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-212\" class=\"h5p-iframe\" data-content-id=\"212\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Distorted T Mark the Words: Which Species Have Three Bonding Pairs and Two Lone Pairs?\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card orange\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">5<\/div>\n          <h2>How to Explain Distorted T Shape in an Exam<\/h2>\n        <\/div>\n        <p>A full exam explanation should connect the number of electron regions to electron-pair repulsion, then explain why the two lone pairs are equatorial and why the bonded atoms form a T shape.<\/p>\n\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>1. Identify the central atom<\/h3>\n            <p>For ClF<sub>3<\/sub>, the central atom is chlorine.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>2. Count bonding pairs and lone pairs<\/h3>\n            <p>Chlorine has three bonding pairs and two lone pairs around it.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>3. Apply electron-pair repulsion<\/h3>\n            <p>The five electron regions arrange themselves as far apart as possible. The two lone pairs occupy equatorial positions to reduce repulsion.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>4. State the shape and angle<\/h3>\n            <p>The three bonded atoms form a distorted T shape.<\/p>\n<p>The two lone pairs repel more strongly than the bonding pairs, so the bond angles are slightly less than 90&deg;, about 87.5&deg; in ClF<sub>3<\/sub>, and the axial to axial angle is slightly less than 180&deg;.<\/p>\n          <\/div>\n        <\/div>\n\n        <div class=\"ols-definition-box\">\n          <p><strong>Exam answer model:<\/strong> ClF<sub>3<\/sub> has three bonding pairs and two lone pairs around the central chlorine atom. The five electron regions arrange themselves as a trigonal bipyramidal electron-pair arrangement.<\/p>\n<p>The two lone pairs occupy equatorial positions to minimise repulsion. Therefore, ClF<sub>3<\/sub> is distorted T-shaped, with bond angles slightly less than 90&deg;, about 87.5&deg;.<\/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: Explain the Shape of an Ion<\/h2>\n<p>Write a short exam-style 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-215\" class=\"h5p-iframe\" data-content-id=\"215\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Distorted T Explain: Shape and Bond Angle of the XeF\u2083\u207a Ion\"><\/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: Whose Reasoning Is Sound?<\/h2>\n<p>In each round, choose the one student whose reasoning is correct.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-666\" class=\"h5p-iframe\" data-content-id=\"666\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Distorted T Summary: Spot the Sound Reasoning\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card soft\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">6<\/div>\n          <h2>Common Exam Points<\/h2>\n        <\/div>\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Do not call ClF<sub>3<\/sub> trigonal bipyramidal<\/h3>\n            <p>The electron-pair arrangement is trigonal bipyramidal, but the molecular shape is distorted T because the two lone pairs are not counted as atoms.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>State the lone pairs are equatorial<\/h3>\n            <p>The two lone pairs occupy equatorial positions. This gives fewer 90&deg; lone pair interactions than placing a lone pair in an axial position.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Give an angle just under 90&deg;<\/h3>\n            <p>Write slightly less than 90&deg;, or about 87.5&deg; for ClF<sub>3<\/sub>. Mark schemes accept values from about 87&deg; to 90&deg;, and some boards simply expect 90&deg; and 180&deg; for a T shape. The axial to axial angle is slightly less than 180&deg;.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Count around the central atom only<\/h3>\n            <p>The shape is determined by the bonding pairs and lone pairs around the central atom, not by the total number of atoms in the species.<\/p>\n          <\/div>\n        <\/div>\n      <\/article>\n\n      \n\n      <article class=\"ols-note-card purple\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">\u2713<\/div>\n          <h2>QuickSnap<\/h2>\n        <\/div>\n        <p>The distorted T shape is produced when a central atom has <strong>three bonding pairs<\/strong> and <strong>two lone pairs<\/strong>.<\/p>\n<p>The lone pairs occupy equatorial positions in a trigonal bipyramidal electron-pair arrangement, leaving three bonded atoms in a T-shaped arrangement with bond angles <strong>slightly less than 90&deg;<\/strong>, about 87.5&deg; in ClF<sub>3<\/sub>.<\/p>\n        <div class=\"ols-key-box\"><p><strong>Memory line:<\/strong> 3 bonding pairs + 2 lone pairs = distorted T = just under 90&deg;.<\/p><\/div>\n      <\/article>\n<section class=\"ols-faq-card\">\n        <h2>Distorted T FAQs<\/h2>\n        <p>These questions target the points students most often lose marks on when explaining the distorted T molecular shape.<\/p>\n        <div class=\"ols-faq-list\">\n          <div class=\"ols-faq-item\">\n            <h3>Why is ClF<sub>3<\/sub> distorted T-shaped?<\/h3>\n            <p>ClF<sub>3<\/sub> is distorted T-shaped because chlorine has three bonding pairs and two lone pairs. The five electron regions arrange as trigonal bipyramidal, but the two lone pairs occupy equatorial positions, leaving two axial Cl-F bonds and one equatorial Cl-F bond.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>What is the bond angle in a distorted T molecule?<\/h3>\n            <p>The bond angles are slightly less than 90&deg;, about 87.5&deg; in ClF<sub>3<\/sub> and about 86&deg; in BrF<sub>3<\/sub>. Mark schemes accept about 87&deg; to 90&deg;. The axial to axial angle is slightly less than 180&deg;.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Is distorted T the same as trigonal bipyramidal?<\/h3>\n            <p>No. Trigonal bipyramidal is the electron-pair arrangement for five regions of negative charge. Distorted T is the molecular shape after the two lone pairs are ignored when naming the shape.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Why do the lone pairs in ClF<sub>3<\/sub> occupy equatorial positions?<\/h3>\n            <p>The lone pairs occupy equatorial positions because this arrangement minimises repulsion. The two lone pairs are approximately 120&deg; apart and avoid unnecessary 90&deg; lone pair-lone pair interactions.<\/p>\n          <\/div>\n        \n<div class=\"ols-faq-item\">\n<h3>Why is ClF<sub>3<\/sub> not trigonal planar?<\/h3>\n<p>Trigonal planar needs three bonding regions and no lone pairs. ClF<sub>3<\/sub> has three bonding pairs and two lone pairs, five regions in all, so the arrangement is trigonal bipyramidal and the three fluorine atoms form a distorted T.<\/p>\n<\/div>\n<\/div>\n      <\/section>\n\n      <!-- author card (moved to the end, 10 Oct 2026) -->\n      <div class=\"ols-author\">\n          <img decoding=\"async\" class=\"ols-author-avatar-img\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/05\/Author-Profile.jpeg\" alt=\"Dr. Mohammed Al-Fatah\">\n          <div class=\"ols-author-content\">\n            <h2 class=\"ols-author-title\">Written by:<br><span>Dr. Mohammed Al-Fatah<\/span><\/h2>\n            <p class=\"ols-author-description\">Chemistry specialist revision notes for A Level Chemistry.<\/p>\n            <a class=\"ols-linkedin-pill\" href=\"https:\/\/www.linkedin.com\/in\/doctormohammedfatah\/\" target=\"_blank\" rel=\"noopener noreferrer\">\n              <svg class=\"ols-linkedin-icon\" viewBox=\"0 0 24 24\" fill=\"currentColor\" aria-hidden=\"true\"><path d=\"M4.98 3.5C4.98 4.88 3.86 6 2.48 6S0 4.88 0 3.5 1.12 1 2.48 1s2.5 1.12 2.5 2.5zM.5 8h4V24h-4V8zm7 0h3.8v2.2h.1c.5-.9 1.8-2.2 3.9-2.2 4.2 0 5 2.8 5 6.4V24h-4v-7.6c0-1.8 0-4.2-2.6-4.2s-3 2-3 4v7.8h-4V8z\"><\/path><\/svg>\n              View LinkedIn Profile\n            <\/a>\n          <\/div>\n        <\/div>\n\n\n      <section class=\"ols-related-card\">\n        <h2>Related Topics<\/h2>\n        <p>Use these related revision notes to strengthen the surrounding bonding and molecular shape ideas.<\/p>\n        <div class=\"ols-related-grid\">\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/trigonal-bipyramidal\/\">Trigonal Bipyramidal<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/seesaw\/\">SeeSaw<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/polar-molecules\/\">Polar &amp; Non-Polar Molecules<\/a>\n        <\/div>\n      <\/section>\n<section class=\"ols-attribution-card ols-attr-std\" aria-label=\"Copyright notice\">\n<style id=\"ols-attribution-card-css\">.ols-attribution-card.ols-attr-std{background:linear-gradient(135deg,#ffffff,#f8fbff);border:1px solid rgba(28,36,75,0.14);border-radius:28px;box-shadow:0 18px 45px rgba(28,36,75,0.10);padding:34px;margin:24px 0;overflow:hidden;font-family:Poppins,Arial,sans-serif;box-sizing:border-box}.ols-attribution-card.ols-attr-std *{box-sizing:border-box}.ols-attribution-card.ols-attr-std p{margin:0;font-size:14px;line-height:1.65;font-weight:300;color:#667085}.ols-attribution-card.ols-attr-std strong{font-weight:700;color:#1C244B}@media (max-width:760px){.ols-attribution-card.ols-attr-std{padding:24px 18px;border-radius:22px}}<\/style>\n<p><strong>Copyright notice:<\/strong> This OLS revision content, including the explanations, layout, diagrams, tables and embedded learning structure, is authored for Online Learning System by Dr. Mohammed Al-Fatah. It may not be copied, reproduced, redistributed or adapted without written permission.<\/p>\n<\/section>\n\n<div class=\"ols-image-lightbox\" id=\"olsImageLightbox\" aria-hidden=\"true\">\n        <button class=\"ols-image-lightbox-close\" type=\"button\" aria-label=\"Close image\">&times;<\/button>\n        <img decoding=\"async\" src=\"\" alt=\"\">\n      <\/div>\n\n      <script>\n        (function(){\n          var lightbox = document.getElementById(\"olsImageLightbox\");\n          if (!lightbox) { return; }\n\n          var lightboxImage = lightbox.querySelector(\"img\");\n          var closeButton = lightbox.querySelector(\".ols-image-lightbox-close\");\n          var triggers = document.querySelectorAll(\".ols-lightbox-trigger\");\n\n          function closeLightbox() {\n            lightbox.classList.remove(\"is-open\");\n            lightbox.setAttribute(\"aria-hidden\", \"true\");\n            lightboxImage.setAttribute(\"src\", \"\");\n            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