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overflow: hidden; background: #ffffff; box-shadow: var(--inner-shadow); }\n      .ols-table td { border-bottom: 1px solid var(--border); padding: 14px 16px; overflow-wrap: anywhere; }\n      .ols-table td:last-child { border-bottom: none; }\n      .ols-table td::before { content: attr(data-label); display: block; margin-bottom: 6px; font-size: 13px; font-weight: 700; color: var(--blue); }\n      .ols-author { align-items: flex-start; padding: 22px 18px; border-radius: 22px; }\n      .ols-author-avatar-img { width: 72px; height: 72px; }\n      .ols-author-title { font-size: 24px; }\n      .ols-author-description { font-size: 15px; }\n    }\n  <\/style>\n\n  <aside class=\"ols-sidebar\">\r\n  <div class=\"ols-sidebar-header\">\r\n    <h3>Revision Notes<\/h3>\r\n    <p>A Level Chemistry<\/p>\r\n  <\/div>\r\n\r\n  <div class=\"ols-topic-group\">\r\n    <h4>Topic 2 Bonding and Structure<\/h4>\r\n\r\n    <ul class=\"ols-topic-list\">\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/ionic-bonding\/\">Ionic Bonding<\/a>\r\n\r\n        <ul class=\"ols-subtopic-list\">\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/ionic-bonding\/nature-of-ionic-bonding\/\">Nature of Ionic Bonding<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/ionic-bonding\/polarisation-of-ions\/\">Polarisation of Ions<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/ionic-bonding\/physical-properties-of-ionic-compounds\/\">Physical Properties of Ionic Compounds<\/a>\r\n          <\/li>\r\n        <\/ul>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/covalent-bonding\/\">Covalent Bonding<\/a>\r\n\r\n        <ul class=\"ols-subtopic-list\">\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/covalent-bonding\/nature-of-covalent-bonding\/\">Nature of Covalent Bonding<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/covalent-bonding\/dative-covalent-bonding\/\">Dative Covalent Bonding<\/a>\r\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/covalent-bonding\/giant-covalent-structures\/\">Giant Covalent Structures<\/a>\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/covalent-bonding\/electronegativity\/\">Electronegativity<\/a>\r\n          <\/li>\r\n        <\/ul>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/\">Shapes of Molecules<\/a>\r\n\r\n        <ul class=\"ols-subtopic-list\">\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/linear\/\">Linear<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/trigonal-planar\/\">Trigonal Planar<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/tetrahedral\/\">Tetrahedral<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/trigonal-pyramidal\/\">Trigonal Pyramidal<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/bent\/\">Bent<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/trigonal-bipyramidal\/\">Trigonal Bipyramidal<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/octahedral\/\">Octahedral<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/square-planar\/\">Square Planar<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/square-pyramidal\/\">Square Pyramidal<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/distorted-t\/\">Distorted T<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/seesaw\/\">SeeSaw<\/a>\r\n          <\/li>\r\n        <\/ul>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/polar-molecules\/\">Polar Molecules<\/a>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/\">Metallic Bonding<\/a>\r\n\r\n        <ul class=\"ols-subtopic-list\">\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/metallic-bonding-and-structure\/\">Metallic Bonding and Structure<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/metallic-bonding\/physical-properties-of-metals\/\">Physical Properties of Metals<\/a>\r\n          <\/li>\r\n        <\/ul>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/\">Intermolecular Forces<\/a>\n        <ul class=\"ols-subtopic-list\">\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/london-forces\/\">London Forces<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/permanent-dipole-dipole-forces\/\">Permanent Dipole-Dipole Forces<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/hydrogen-bonding\/\">Hydrogen Bonding<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/anomalous-properties-of-water\/\">Anomalous Properties of Water<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/boiling-temperature-trends\/\">Boiling Temperature Trends<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/intermolecular-forces\/choosing-solvents\/\">Choosing Solvents<\/a>\n          <\/li>\n        <\/ul>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/structure-types\/\">Structure Types<\/a>\r\n      <\/li>\r\n\r\n    <\/ul>\r\n  <\/div>\r\n\r\n  <div class=\"ols-topic-group\">\r\n    <h4>Next Topics<\/h4>\r\n\r\n    <ul class=\"ols-topic-list\">\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-3-redox-i\/\">Redox I<\/a>\r\n      <\/li>\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-4-inorganic-chemistry-and-the-periodic-table\/\">Inorganic Chemistry &amp; The Periodic Table<\/a>\r\n      <\/li>\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-5-formulae-equations-and-amounts-of-substance\/\">Formulae, Equations &amp; Amounts<\/a>\r\n      <\/li>\r\n    <\/ul>\r\n  <\/div>\r\n<\/aside>\r\n\r\n<script>\r\n(function() {\r\n  function normalisePath(path) {\r\n    return String(path || '')\r\n      .split('?')[0]\r\n      .split('#')[0]\r\n      .replace(\/\\\/+$\/, '')\r\n      .toLowerCase();\r\n  }\r\n\r\n  function highlightActive() {\r\n    var sidebar = document.querySelector('.ols-sidebar');\r\n    if (!sidebar) 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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>Linear<\/span>\n      <\/nav>\n\n      <header class=\"ols-title-card\">\n        <h1>Linear Molecular Shape<\/h1>\n        <p class=\"ols-page-intro\">A focused revision guide to the linear molecular shape, using BeCl<sub>2<\/sub> as the key example. This page explains why two bonding regions and no lone pairs around a central atom give a 180\u00b0 bond angle.<\/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: linear-shape (swapped 26 Sep 2026) -->\n<!-- Copyright (c) 2026 Dr. Mohammed Al-Fatah, onlinelearningsystem.net. All rights reserved. -->\n<!-- 3D card: linear-shape (rebuilt Oct 2026) -->\n<!-- Copyright (c) 2026 Dr. Mohammed Al-Fatah, onlinelearningsystem.net. 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text-align:center; font-size:11px; font-style:italic; color:#aab0c0;\n}\n.ols-cc-lnsh-001 a{color:#aab0c0; text-decoration:none;}\n.ols-cc-lnsh-001 a:hover{text-decoration:underline;}\n.ols-lnsh-001 .lnsh-seg button{display:inline-flex; align-items:center;}\n.ols-lnsh-001 .lnsh-seg button .lnsh-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-lnsh-001 .lnsh-seg button[aria-pressed=\"true\"] .lnsh-n{background:#ffffff; color:#2563eb;}\n<\/style>\n\n<div class=\"lnsh-head\">\n  <h2 class=\"lnsh-title\">Electron Domains and the Linear Shape<\/h2>\n  <p class=\"lnsh-sub\">Choose a step to watch two electron domains repel to 180\u00b0, then see the same linear shape in BeCl\u2082, CO\u2082 and XeF\u2082.<\/p>\n<\/div>\n\n<div class=\"lnsh-stage\" id=\"lnshStage\">\n  <canvas class=\"lnsh-canvas\" id=\"lnshCanvas\"><\/canvas>\n  <div class=\"lnsh-overlay\" id=\"lnshOverlay\"><\/div>\n  <div class=\"lnsh-caption\" id=\"lnshCaption\"><\/div>\n  <div class=\"lnsh-hint\" id=\"lnshHint\">Drag to rotate<\/div>\n  <div class=\"lnsh-badges\" id=\"lnshBadges\"><\/div>\n<\/div>\n\n<div class=\"lnsh-controls\">\n  <div class=\"lnsh-row\">\n    <span class=\"lnsh-rowlab\">Step<\/span>\n    <div class=\"lnsh-seg\" role=\"group\" aria-label=\"Step\">\n      <button type=\"button\" data-step=\"1\" aria-pressed=\"true\"><span class=\"lnsh-n\">1<\/span>Two domains repel<\/button>\n      <button type=\"button\" data-step=\"2\" aria-pressed=\"false\"><span class=\"lnsh-n\">2<\/span>BeCl\u2082<\/button>\n      <button type=\"button\" data-step=\"3\" aria-pressed=\"false\"><span class=\"lnsh-n\">3<\/span>CO\u2082<\/button>\n      <button type=\"button\" data-step=\"4\" aria-pressed=\"false\"><span class=\"lnsh-n\">4<\/span>XeF\u2082<\/button>\n      <button type=\"button\" data-step=\"5\" aria-pressed=\"false\"><span class=\"lnsh-n\">5<\/span>Angle read-out<\/button>\n    <\/div>\n  <\/div>\n\n  <div class=\"lnsh-row\">\n    <span class=\"lnsh-rowlab\">View<\/span>\n    <button type=\"button\" class=\"lnsh-pill\" id=\"lnshResetV\">Reset view<\/button>\n  <\/div>\n<\/div>\n\n<div class=\"lnsh-info\">\n  <h3 id=\"lnshInfoTitle\"><\/h3>\n  <p id=\"lnshInfoText\"><\/p>\n  <div class=\"lnsh-facts\" id=\"lnshFacts\"><\/div>\n  <div class=\"lnsh-key\">\n    <span><i class=\"\" style=\"background:rgba(59,120,220,0.45)\"><\/i>Electron domain (bonding region)<\/span>\n    <span><i class=\"\" style=\"background:rgba(60,170,110,0.5)\"><\/i>Lone pair (non-bonding)<\/span>\n    <span><i class=\"k-ball\" style=\"background:#facc28\"><\/i>Electron<\/span>\n    <span><i class=\"k-ball\" style=\"background:#a8ae78\"><\/i>Beryllium<\/span>\n    <span><i class=\"k-ball\" style=\"background:#464a54\"><\/i>Carbon<\/span>\n    <span><i class=\"k-ball\" style=\"background:#d6342c\"><\/i>Oxygen<\/span>\n    <span><i class=\"k-ball\" style=\"background:#34aa48\"><\/i>Chlorine<\/span>\n    <span><i class=\"k-ball\" style=\"background:#429eb4\"><\/i>Xenon<\/span>\n    <span><i class=\"k-ball\" style=\"background:#c4e278\"><\/i>Fluorine<\/span>\n    <span><i class=\"\" style=\"background:#d6302a\"><\/i>Repulsion<\/span>\n    <span><i class=\"\" style=\"background:#c9961c\"><\/i>Bond angle<\/span>\n  <\/div>\n<\/div>\n\n<script src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/JS\/linear-shape.js?v=20261025p\"><\/script>\n<\/section>\n\n<p class=\"ols-cc-lnsh-001\">&copy; Dr. Mohammed Al-Fatah &#8211; <a href=\"https:\/\/www.onlinelearningsystem.net\" target=\"_blank\" rel=\"noopener\">onlinelearningsystem.net<\/a><\/p>\n\n\n      \n<section class=\"ols-h5p-card ols-h5p-inline ols-h5p-recap\">\n<span class=\"ols-h5p-kicker\">Before you start<\/span>\n<h2>GCSE Recap: Shared Pairs and Lone Pairs<\/h2>\n<p>Before you start, check the GCSE ideas about shared and lone pairs that this page builds on.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"653\"><\/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>Why Electron Pairs Repel<\/h2>\n        <\/div>\n        <p>All electrons carry a <strong>negative charge<\/strong>. Electron pairs therefore repel one another and arrange themselves as far apart as possible around a central atom.<\/p>\n        <p>This is the basis of the electron-pair repulsion model used to explain molecular shapes. The shape depends on how many <strong>bonding pairs<\/strong> and <strong>lone pairs<\/strong> of electrons surround the central atom.<\/p>\n        <div class=\"ols-key-box\"><p><strong>Key idea:<\/strong> molecular shape is controlled by electron-pair repulsion. Electron pairs move to positions of minimum repulsion.<\/p><\/div>\n      <\/article>\n\n      \n\n      <article class=\"ols-note-card\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">2<\/div>\n          <h2>From Electron Domains to Molecular Shape<\/h2>\n        <\/div>\n        <p>A simple two-dimensional circle helps show why two electron domains become opposite each other. Real molecules, however, exist in three-dimensional space.<\/p>\n        <p>When electron domains are allowed to arrange themselves in three dimensions, they spread out around an imaginary sphere centred on the central atom. With only two electron domains, the furthest-apart arrangement is still opposite sides of the central atom.<\/p>\n        <div class=\"ols-definition-box\"><p><strong>Electron domain:<\/strong> a region of electron density around a central atom. A single bond, double bond, triple bond or lone pair each counts as one electron domain for shape prediction.<\/p><\/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-19-twothreepairs.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-19-twothreepairs.jpg\" alt=\"Balloon analogy and ball-and-stick sketches for linear (180\u00b0) and trigonal planar (120\u00b0) shapes, with a summary table\">\n<\/a>\n<\/div>\n<div class=\"ols-zoom-card-caption\"><p>Two regions get as far apart as possible at 180\u00b0, three regions at 120\u00b0 in one plane.<\/p><\/div>\n<\/div>\n<\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Count the Electron Domains<\/h2>\n<p>Count the electron domains around the central atom in each molecule.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-176\" class=\"h5p-iframe\" data-content-id=\"176\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Linear Shape Single Choice: Counting Electron Domains\"><\/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>The Linear Shape<\/h2>\n        <\/div>\n        <p>A molecule is <strong>linear<\/strong> when there are <strong>two bonding regions<\/strong> and <strong>no lone pairs<\/strong> around the central atom.<\/p>\n<p>A double bond or a triple bond counts as <strong>one bonding region<\/strong>, which is why CO<sub>2<\/sub> and HCN are linear even though the central atom holds four bonding pairs.<\/p>\n        <p>The two bonding regions repel equally. The lowest-repulsion arrangement places them in opposite directions, giving a bond angle of <strong>180\u00b0<\/strong>.<\/p>\n\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Shape<\/th>\n                <th>Bonding pairs<\/th>\n                <th>Lone pairs<\/th>\n                <th>Bond angle<\/th>\n                <th>Examples<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Shape\"><strong>Linear<\/strong><\/td>\n                <td data-label=\"Bonding pairs\">2<\/td>\n                <td data-label=\"Lone pairs\">0<\/td>\n                <td data-label=\"Bond angle\"><strong>180\u00b0<\/strong><\/td>\n                <td data-label=\"Examples\">CO<sub>2<\/sub>, CS<sub>2<\/sub>, HCN, BeF<sub>2<\/sub>, BeCl<sub>2<\/sub><\/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: Which Species Are Linear?<\/h2>\n<p>Click every species that is linear.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-178\" class=\"h5p-iframe\" data-content-id=\"178\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Linear Shape Mark the Words: Which Species Are Linear?\"><\/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\">4<\/div>\n          <h2>Linear Shape in BeCl<sub>2<\/sub><\/h2>\n        <\/div>\n        <p>In BeCl<sub>2<\/sub>, beryllium is the central atom and chlorine atoms are bonded on either side. The central beryllium atom has <strong>two bonding pairs<\/strong> and <strong>no lone pairs<\/strong> in the shape model.<\/p>\n        <p>Beryllium has only <strong>2 outer-shell electrons<\/strong>, so it finishes with four electrons around it and never reaches an octet.<\/p>\n<p>That does not change the method: the shape follows from the number of electron regions around the central atom. These notes describe <strong>gaseous<\/strong> BeCl<sub>2<\/sub>, which is the form used in shape questions.<\/p>\n        <p>The two Be-Cl bonding pairs repel equally and move as far apart as possible. This gives a <strong>linear molecule<\/strong> with a <strong>Cl-Be-Cl bond angle of 180\u00b0<\/strong>.<\/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 BeCl<sub>2<\/sub>: beryllium has <strong>2 outer-shell electrons<\/strong>, the molecule has no charge, and the two Be-Cl single bonds use both electrons. None are left over, so there are no lone pairs. Two bonding regions and no lone pairs give a linear molecule.<\/p><\/div>\n        <div class=\"ols-key-box\"><p><strong>Exam sentence:<\/strong> BeCl<sub>2<\/sub> has two bonding pairs and no lone pairs around Be. The bonding pairs repel equally and move as far apart as possible, so the molecule is linear with a 180\u00b0 bond angle.<\/p><\/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-23-countbecl2.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-23-countbecl2.jpg\" alt=\"Five-step electron-pair count for BeCl\u2082 giving two bonding regions, no lone pairs and a linear 180\u00b0 shape, with CO\u2082 as a second example\">\n<\/a>\n<\/div>\n<div class=\"ols-zoom-card-caption\"><p>Beryllium has 2 outer electrons, both used in bonds: two regions and no lone pairs give a linear molecule.<\/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: Who Has Predicted NO\u2082\u207a Correctly?<\/h2>\n<p>Choose the student with the correct shape and the correct reasoning.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-177\" class=\"h5p-iframe\" data-content-id=\"177\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Linear Shape MCQ: Four Students Predict the Shape of NO\u2082\u207a\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <div class=\"ols-zoom-card compact\">\n        <div class=\"ols-zoom-card-image\">\n          <img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-cd-09-becl2-linear.svg\" alt=\"Linear BeCl\u2082 with a 180\u00b0 angle and its dot-and-cross diagram, beside linear O=C=O\" class=\"ols-zoomable-img ols-lightbox-target\" draggable=\"false\" width=\"1042\" height=\"377\">\n        <\/div>\n        <div class=\"ols-zoom-card-caption\">\n          <p>BeCl<sub>2<\/sub> is linear because the two bonding pairs around the central Be atom repel equally and sit opposite one another.<\/p>\n        <\/div>\n      <\/div>\n\n      \n\n      <article class=\"ols-note-card\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">5<\/div>\n          <h2>How to Explain Shape in an Exam<\/h2>\n        <\/div>\n        <p>Shape explanations need a clear sequence. State the number of electron pairs first, then explain repulsion, then give the shape and bond angle.<\/p>\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\"><h3>1. Count electron pairs<\/h3><p>State the number of bonding pairs and lone pairs around the central atom.<\/p><\/div>\n          <div class=\"ols-rule-item\"><h3>2. Use repulsion language<\/h3><p>State that electron pairs repel and arrange themselves as far apart as possible.<\/p><\/div>\n          <div class=\"ols-rule-item\"><h3>3. Compare pair types where needed<\/h3><p>If there are no lone pairs, state that the bonding pairs repel equally. If there are lone pairs, state that lone pairs repel more strongly than bonding pairs.<\/p><\/div>\n          <div class=\"ols-rule-item\"><h3>4. Give the final shape and angle<\/h3><p>For BeCl<sub>2<\/sub>, the final answer is linear, 180\u00b0.<\/p><\/div>\n        <\/div>\n      <\/article>\n\n      <article class=\"ols-note-card purple\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">6<\/div>\n          <h2>BeCl<sub>2<\/sub> Exam Answer Model<\/h2>\n        <\/div>\n        <p>Use the exam-answer structure from Part 5, then change only the molecule-specific information. The black wording is the reusable sentence frame. The coloured wording is the part that changes for each molecule.<\/p>\n\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Model answer for BeCl<sub>2<\/sub><\/h3>\n            <p>There are <span style=\"color:#2563eb;font-weight:800;\">two bonding pairs<\/span> and <span style=\"color:#c81e1e;font-weight:800;\">no lone pairs<\/span> around the central <span style=\"color:#c9973a;font-weight:800;\">beryllium atom<\/span>.<\/p>\n            <p>Electron pairs repel each other and arrange themselves as far apart as possible to minimise repulsion.<\/p>\n            <p>Because there are <span style=\"color:#c81e1e;font-weight:800;\">no lone pairs<\/span>, the <span style=\"color:#2563eb;font-weight:800;\">two bonding pairs<\/span> repel equally.<\/p>\n            <p>The molecule is therefore <span style=\"color:#31a36a;font-weight:800;\">linear<\/span> with a bond angle of <span style=\"color:#31a36a;font-weight:800;\">180\u00b0<\/span>.<\/p>\n          <\/div>\n\n          <div class=\"ols-rule-item\">\n            <h3>Reusable sentence frame<\/h3>\n            <p>There are <span style=\"color:#2563eb;font-weight:800;\">[number of bonding pairs]<\/span> and <span style=\"color:#c81e1e;font-weight:800;\">[number of lone pairs]<\/span> around the central <span style=\"color:#c9973a;font-weight:800;\">[central atom]<\/span>.<\/p>\n            <p>Electron pairs repel each other and arrange themselves as far apart as possible to minimise repulsion.<\/p>\n            <p>If there are <span style=\"color:#c81e1e;font-weight:800;\">[no lone pairs]<\/span>, the bonding pairs repel equally. If there are lone pairs, the lone pairs repel more strongly than bonding pairs.<\/p>\n            <p>The molecule is therefore <span style=\"color:#31a36a;font-weight:800;\">[shape]<\/span> with a bond angle of <span style=\"color:#31a36a;font-weight:800;\">[bond angle]<\/span>.<\/p>\n          <\/div>\n\n          <div class=\"ols-rule-item\">\n            <h3>Colour key<\/h3>\n            <p><span style=\"color:#2563eb;font-weight:800;\">Blue<\/span> = bonding-pair information. <span style=\"color:#c81e1e;font-weight:800;\">Red<\/span> = lone-pair information. <span style=\"color:#c9973a;font-weight:800;\">Gold<\/span> = central atom. <span style=\"color:#31a36a;font-weight:800;\">Green<\/span> = final shape and bond angle.<\/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: Explain a New Pair of Molecules<\/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-179\" class=\"h5p-iframe\" data-content-id=\"179\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Linear Shape Explain: Beryllium Hydride Compared with Hydrogen Sulfide\"><\/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: The Whole Page in Five Statements<\/h2>\n<p>In each round, pick the one accurate statement to review everything on this page.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-1296\" class=\"h5p-iframe\" data-content-id=\"1296\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Linear Shape Summary: Electron Domains, Lone Pairs and the 180\u00b0 Angle\"><\/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\">7<\/div>\n          <h2>Common Exam Points<\/h2>\n        <\/div>\n        <p>Linear shape questions are usually straightforward, but marks are often lost when students describe the atoms moving apart instead of the electron pairs repelling.<\/p>\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\"><h3>Focus on electron pairs<\/h3><p>The cause of the shape is repulsion between regions of electron density, not a simple repulsion between atoms.<\/p><\/div>\n          <div class=\"ols-rule-item\"><h3>State no lone pairs clearly<\/h3><p>For BeCl<sub>2<\/sub>, the central Be atom has two bonding pairs and no lone pairs in the molecular shape model.<\/p><\/div>\n          <div class=\"ols-rule-item\"><h3>Use the exact angle<\/h3><p>The bond angle in a linear molecule is 180\u00b0. Do not write approximately 180\u00b0 unless the question specifically allows approximation.<\/p><\/div>\n          <div class=\"ols-rule-item\"><h3>Do not confuse linear with bent<\/h3><p>A bent molecule has lone pairs on the central atom: H<sub>2<\/sub>O has two bonding pairs and two lone pairs, so its bond angle is about 104.5\u00b0.<\/p>\n<p>A linear molecule has two bonding regions and no lone pairs, counting a double or triple bond as one region, so the angle is 180\u00b0.<\/p><\/div>\n        <\/div>\n      <\/article>\n\n      \n\n      <article class=\"ols-note-card purple\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">\u2713<\/div>\n          <h2>QuickSnap<\/h2>\n        <\/div>\n        <p>The linear shape is produced when a central atom has <strong>two bonding regions<\/strong> and <strong>no lone pairs<\/strong>. A double or triple bond counts as one region. The two regions repel equally and move to opposite sides of the central atom.<\/p>\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\"><h3>Electron-pair repulsion<\/h3><p>Electron pairs repel because electrons are negatively charged.<\/p><\/div>\n          <div class=\"ols-rule-item\"><h3>Linear condition<\/h3><p>Two bonding regions and no lone pairs around the central atom. A double or triple bond is one region.<\/p><\/div>\n          <div class=\"ols-rule-item\"><h3>Bond angle<\/h3><p>The two bonding regions are furthest apart at 180\u00b0.<\/p><\/div>\n          <div class=\"ols-rule-item\"><h3>Example<\/h3><p>BeCl<sub>2<\/sub> is linear, with a Cl-Be-Cl bond angle of 180\u00b0.<\/p><\/div>\n        <\/div>\n      <\/article>\n\n      <section class=\"ols-faq-card\">\n        <h2>FAQs<\/h2>\n        <p>These questions target the common points students confuse when learning the linear molecular shape.<\/p>\n        <div class=\"ols-faq-list\">\n          <div class=\"ols-faq-item\">\n            <h3>What makes a molecule linear?<\/h3>\n            <p>A molecule is linear when the central atom has two bonding regions and no lone pairs. The bonding pairs repel equally and arrange themselves 180\u00b0 apart.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Why is BeCl<sub>2<\/sub> linear?<\/h3>\n            <p>BeCl<sub>2<\/sub> has two Be-Cl bonding pairs around the central Be atom and no lone pairs in the shape model. The two bonding pairs repel equally, so the Cl-Be-Cl bond angle is 180\u00b0.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Do lone pairs affect the linear shape?<\/h3>\n            <p>Yes. Lone pairs repel more strongly than bonding pairs and can reduce bond angles. BeCl<sub>2<\/sub> is linear because there are no lone pairs on the central atom in the shape model.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>What bond angle should I write for a linear molecule?<\/h3>\n            <p>The bond angle for a linear molecule is 180\u00b0.<\/p>\n          <\/div>\n        \n<div class=\"ols-faq-item\">\n<h3>Can a molecule with lone pairs on the central atom be linear?<\/h3>\n<p>Yes. XeF<sub>2<\/sub> has two bonding pairs and three lone pairs. The five regions take a trigonal bipyramidal arrangement with all three lone pairs equatorial, so the two fluorine atoms sit axially at 180&deg;.<\/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\" 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\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 class=\"ols-linkedin-pill\" href=\"https:\/\/www.linkedin.com\/in\/doctormohammedfatah\/\" target=\"_blank\" rel=\"noopener noreferrer\">\n        <svg class=\"ols-linkedin-icon\" viewBox=\"0 0 24 24\" fill=\"currentColor\" aria-hidden=\"true\">\n          <path d=\"M4.98 3.5C4.98 4.88 3.86 6 2.48 6S0 4.88 0 3.5 1.12 1 2.48 1s2.5 1.12 2.5 2.5zM.5 8h4V24h-4V8zm7 0h3.8v2.2h.1c.5-.9 1.8-2.2 3.9-2.2 4.2 0 5 2.8 5 6.4V24h-4v-7.6c0-1.8 0-4.2-2.6-4.2s-3 2-3 4v7.8h-4V8z\"><\/path>\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>Use these pages to connect linear shape with the wider bonding and structure topic.<\/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\/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\/electronegativity\/\">Electronegativity<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/trigonal-planar\/\">Trigonal Planar<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/tetrahedral\/\">Tetrahedral<\/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\/bent\/\">Bent<\/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 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=\"olsImageLightboxLinear9ch0\" 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-linear-molecular-shape-9ch0-page\");\n          if (!page) {\n            return;\n          }\n\n          var lightbox = page.querySelector(\"#olsImageLightboxLinear9ch0\");\n          if (!lightbox) {\n            return;\n          }\n\n          var lightboxImage = lightbox.querySelector(\".ols-image-lightbox-img\");\n          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