{"id":4592,"date":"2026-05-30T06:13:01","date_gmt":"2026-05-30T05:13:01","guid":{"rendered":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/square-planar\/"},"modified":"2026-10-25T12:18:28","modified_gmt":"2026-10-25T12:18:28","slug":"square-planar","status":"publish","type":"page","link":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/square-planar\/","title":{"rendered":"Square Planar"},"content":{"rendered":"\n<section class=\"ols-revision-page ols-square-planar-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      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22px; }\n      .ols-figure-image { min-height: 210px; padding: 14px; }\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  <\/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', 'parent-active');\r\n    });\r\n\r\n    sidebar.querySelectorAll('a[data-ols-disabled-parent=\"1\"], a[aria-current]').forEach(function(a) {\r\n      a.removeAttribute('aria-current');\r\n      a.removeAttribute('tabindex');\r\n      a.removeAttribute('data-ols-disabled-parent');\r\n    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href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/\">Revision Notes<\/a> \/\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/\">A Level Chemistry<\/a> \/\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/\">Edexcel<\/a> \/\n        <a 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>Square Planar<\/span>\n      <\/nav>\n\n      <header class=\"ols-title-card\">\n        <h1>Square Planar Molecular Shape<\/h1>\n        <p class=\"ols-page-intro\">A focused revision guide to the square planar molecular shape, using XeF<sub>4<\/sub> as the key example. This page explains why four bonding pairs and two lone pairs around a central atom give a flat square arrangement with 90&deg; bond angles.<\/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: xef4-square-planar (swapped 26 Sep 2026) -->\n<!-- Copyright (c) 2026 Dr. Mohammed Al-Fatah, onlinelearningsystem.net. All rights reserved. -->\n<!-- 3D card: xef4-square-planar (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-xsqp-001 a{color:#aab0c0; text-decoration:none;}\n.ols-cc-xsqp-001 a:hover{text-decoration:underline;}\n.ols-xsqp-001 .xsqp-seg button{display:inline-flex; align-items:center;}\n.ols-xsqp-001 .xsqp-seg button .xsqp-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-xsqp-001 .xsqp-seg button[aria-pressed=\"true\"] .xsqp-n{background:#ffffff; color:#2563eb;}\n<\/style>\n\n<div class=\"xsqp-head\">\n  <h2 class=\"xsqp-title\">Square Planar Shape of XeF\u2084<\/h2>\n  <p class=\"xsqp-sub\">Choose a step to watch six electron pairs spread out round xenon, two become lone pairs on opposite sides, and four fluorines stay in a flat square.<\/p>\n<\/div>\n\n<div class=\"xsqp-stage\" id=\"xsqpStage\">\n  <canvas class=\"xsqp-canvas\" id=\"xsqpCanvas\"><\/canvas>\n  <div class=\"xsqp-overlay\" id=\"xsqpOverlay\"><\/div>\n  <div class=\"xsqp-caption\" id=\"xsqpCaption\"><\/div>\n  <div class=\"xsqp-hint\" id=\"xsqpHint\">Drag to rotate<\/div>\n  <div class=\"xsqp-badges\" id=\"xsqpBadges\"><\/div>\n<\/div>\n\n<div class=\"xsqp-controls\">\n  <div class=\"xsqp-row\">\n    <span class=\"xsqp-rowlab\">Step<\/span>\n    <div class=\"xsqp-seg\" role=\"group\" aria-label=\"Step\">\n      <button type=\"button\" data-step=\"1\" aria-pressed=\"true\"><span class=\"xsqp-n\">1<\/span>Six electron pairs<\/button>\n      <button type=\"button\" data-step=\"2\" aria-pressed=\"false\"><span class=\"xsqp-n\">2<\/span>First lone pair<\/button>\n      <button type=\"button\" data-step=\"3\" aria-pressed=\"false\"><span class=\"xsqp-n\">3<\/span>Second lone pair opposite<\/button>\n      <button type=\"button\" data-step=\"4\" aria-pressed=\"false\"><span class=\"xsqp-n\">4<\/span>Square plane, 90\u00b0<\/button>\n    <\/div>\n  <\/div>\n\n  <div class=\"xsqp-row\">\n    <span class=\"xsqp-rowlab\">View<\/span>\n    <button type=\"button\" class=\"xsqp-pill\" id=\"xsqpResetV\">Reset view<\/button>\n  <\/div>\n<\/div>\n\n<div class=\"xsqp-info\">\n  <h3 id=\"xsqpInfoTitle\"><\/h3>\n  <p id=\"xsqpInfoText\"><\/p>\n  <div class=\"xsqp-facts\" id=\"xsqpFacts\"><\/div>\n  <div class=\"xsqp-key\">\n    <span><i class=\"k-ball\" style=\"background:#3e98ac\"><\/i>Xenon<\/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>Too close (strong repulsion)<\/span>\n  <\/div>\n<\/div>\n\n<script src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/JS\/xef4-square-planar.js?v=20261025p\"><\/script>\n<\/section>\n\n<p class=\"ols-cc-xsqp-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-square-planar-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-square-planar-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-square-planar-9ch0-page .ols-spec-box strong {\n    display: block;\n    font-size: 15px;\n    color: var(--blue);\n    margin-bottom: 6px;\n  }\n  .ols-square-planar-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-square-planar-9ch0-page .ols-h5p-grid {\n    display: grid;\n    gap: 18px;\n    margin-top: 22px;\n  }\n  .ols-square-planar-9ch0-page .ols-h5p-frame {\n    margin-top: 0;\n  }\n  .ols-square-planar-9ch0-page .ols-formula {\n    white-space: nowrap;\n  }\n  @media (max-width: 760px) {\n    .ols-square-planar-9ch0-page .ols-spec-grid {\n      grid-template-columns: 1fr;\n    }\n  }\n<\/style>\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: Charges and Electron Counts<\/h2>\n<p>Before you start, check the GCSE ideas about ion charges and electron counts that this page builds on.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"656\"><\/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 Square Planar Means<\/h2>\n        <\/div>\n        <p>A <strong>square planar<\/strong> molecule has four atoms bonded to a central atom in one flat plane. The four bonded atoms form the corners of a square, so adjacent bond angles are <strong>90&deg;<\/strong>.<\/p>\n        <p>The key example for this page is <strong>XeF<sub>4<\/sub><\/strong>. Xenon is the central atom, four fluorine atoms are bonded to xenon, and xenon 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>4 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>90&deg; between adjacent bonds<\/span>\n          <\/div>\n        <\/div>\n\n        <div class=\"ols-key-box\"><p><strong>Key idea:<\/strong> four bonding pairs and two lone pairs around a central atom give a square planar shape when the two lone pairs occupy opposite positions.<\/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 XeF<sub>4<\/sub> Is Square Planar<\/h2>\n        <\/div>\n        <p>In XeF<sub>4<\/sub>, the central xenon atom is surrounded by four Xe-F bonding pairs and two lone pairs. This gives six regions of negative charge around xenon.<\/p>\n        <p>Six electron regions arrange themselves octahedrally to minimise repulsion. The two lone pairs occupy opposite positions, above and below the plane, leaving the four Xe-F bonds in a flat square arrangement.<\/p>\n        <p>The <strong>molecular shape<\/strong> only describes the positions of the atoms. Therefore, XeF<sub>4<\/sub> is described as <strong>square planar<\/strong>, even though its electron-pair arrangement is octahedral.<\/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 XeF<sub>4<\/sub>: xenon has <strong>8 outer-shell electrons<\/strong>, the molecule has no charge, and the four Xe-F single bonds use four of them.<\/p>\n<p>Four are left over, which is two lone pairs. Four bonding regions and two lone pairs give six regions, so the arrangement is octahedral and the shape is square planar.<\/p>\n<p>For the ion ICl<sub>4<\/sub><sup>&#8211;<\/sup>: iodine has 7 outer-shell electrons and the negative charge adds one to make 8, so the count then runs exactly as it does for XeF<sub>4<\/sub>.<\/p><\/div>\n\n        <div class=\"ols-figure-card compact ols-zoom-figure\">\n          <button class=\"ols-figure-image ols-lightbox-trigger\" type=\"button\" data-ols-lightbox-src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/skel-63-xef4-square-planar.svg\" data-ols-lightbox-alt=\"Square planar XeF\u2084 with two lone pairs and a 90\u00b0 bond angle\" aria-label=\"Open square planar diagram in full screen\">\n            <img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-cd-16-xef4-squareplanar.svg\" alt=\"Square planar XeF\u2084 with four F atoms in one plane, lone pairs above and below xenon and a 90\u00b0 angle marked\" width=\"1520\" height=\"892\">\n          <\/button>\n          <div class=\"ols-figure-caption\">\n            <p>A square planar species has four bonding regions and two lone pairs around the central atom. XeF<sub>4<\/sub> is the standard example, with adjacent bond angles of 90&deg;.<\/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-30-countxef4.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-30-countxef4.jpg\" alt=\"Five-step electron-pair count for XeF\u2084 giving four bonding pairs, two lone pairs and a square planar 90\u00b0 shape\" data-fullscreen-src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-30-countxef4.jpg\">\n<\/a>\n<\/div>\n<div class=\"ols-figure-caption\"><p>Xenon keeps 4 of its 8 outer electrons as two lone pairs, which sit opposite each other: the four F atoms form a square 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: Arrangement or Shape?<\/h2>\n<p>Choose the species with the same electron-pair arrangement as BrF\u2084\u207b but a different shape.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-205\" class=\"h5p-iframe\" data-content-id=\"205\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Square Planar MCQ: Same Electron-Pair Arrangement, Different Shape\"><\/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 XeF<sub>4<\/sub> is based on an <strong>octahedral arrangement<\/strong> because there are six electron regions around xenon.<\/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 four fluorine atoms is <strong>square planar<\/strong>.<\/p>\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Six electron regions<\/h3>\n            <p>Four bonding pairs and two lone pairs arrange themselves as far apart as possible around xenon.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Opposite lone pairs<\/h3>\n            <p><strong>Lone pairs repel more strongly<\/strong> than bonding pairs, so the two lone pairs take opposite positions, as far from each other as possible.<\/p>\n<p>One sits above the square plane and one below it, so they push on the four Xe-F bonds equally. The extra repulsion cancels out and the bond angle stays at exactly 90&deg; instead of being squeezed.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Flat square of bonded atoms<\/h3>\n            <p>The four Xe-F bonds remain in one plane, giving 90&deg; angles between adjacent bonds and 180&deg; across the square.<\/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-22-sixpairs.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-22-sixpairs.jpg\" alt=\"Octahedron key with SF\u2086, IF\u2085 and XeF\u2084 sketches: no, one and two opposite lone pairs, with bond angles\" data-fullscreen-src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-22-sixpairs.jpg\">\n<\/a>\n<\/div>\n<div class=\"ols-figure-caption\"><p>Six regions form an octahedron; one lone pair gives a square pyramid and two opposite lone pairs give a square 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: Explain the 90\u00b0 Angle<\/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-206\" class=\"h5p-iframe\" data-content-id=\"206\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Square Planar Explain: Why Two Lone Pairs Leave the Angle at 90\u00b0\"><\/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>Square Planar Shape Examples<\/h2>\n        <\/div>\n        <p>The square planar shape is found when the central atom has four bonding pairs and two lone pairs. The common exam examples usually include xenon tetrafluoride and square planar halogen-containing ions.<\/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>Typical exam angle<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Species\">XeF<sub>4<\/sub><\/td>\n                <td data-label=\"Central atom\">Xe<\/td>\n                <td data-label=\"Electron regions\">4 bonding regions, 2 lone pairs<\/td>\n                <td data-label=\"Shape\">Square planar<\/td>\n                <td data-label=\"Typical exam angle\">90&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">ICl<sub>4<\/sub><sup>&#8211;<\/sup><\/td>\n                <td data-label=\"Central atom\">I<\/td>\n                <td data-label=\"Electron regions\">4 bonding regions, 2 lone pairs<\/td>\n                <td data-label=\"Shape\">Square planar<\/td>\n                <td data-label=\"Typical exam angle\">90&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">BrCl<sub>4<\/sub><sup>&#8211;<\/sup><\/td>\n                <td data-label=\"Central atom\">Br<\/td>\n                <td data-label=\"Electron regions\">4 bonding regions, 2 lone pairs<\/td>\n                <td data-label=\"Shape\">Square planar<\/td>\n                <td data-label=\"Typical exam angle\">90&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">IF<sub>4<\/sub><sup>&#8211;<\/sup><\/td>\n                <td data-label=\"Central atom\">I<\/td>\n                <td data-label=\"Electron regions\">4 bonding regions, 2 lone pairs<\/td>\n                <td data-label=\"Shape\">Square planar<\/td>\n                <td data-label=\"Typical exam angle\">90&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: Square Planar or Not?<\/h2>\n<p>Work out each species on paper, then flip the card to check.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-204\" class=\"h5p-iframe\" data-content-id=\"204\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Square Planar Flip Cards: Is This Species Square Planar?\"><\/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 Square Planar 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 opposite and why the atoms form a square plane.<\/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 XeF<sub>4<\/sub>, the central atom is xenon.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>2. Count bonding pairs and lone pairs<\/h3>\n            <p>Xenon has four 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 six electron regions arrange themselves as far apart as possible. The two lone pairs are placed opposite each other to minimise repulsion.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>4. State the shape and angle<\/h3>\n            <p>The four bonded atoms form a square planar shape with 90&deg; angles between adjacent Xe-F bonds.<\/p>\n          <\/div>\n        <\/div>\n\n        <div class=\"ols-definition-box\">\n          <p><strong>Exam answer model:<\/strong> XeF<sub>4<\/sub> has four bonding pairs and two lone pairs around the central xenon atom. The six electron regions arrange themselves octahedrally.<\/p>\n<p>The two lone pairs occupy opposite positions to minimise repulsion, leaving the four Xe-F bonds in one plane. Therefore, XeF<sub>4<\/sub> is square planar with bond angles of 90&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: Which Answer Scores Full Marks?<\/h2>\n<p>Choose the explanation of ClF\u2084\u207b that would score full marks.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-1063\" class=\"h5p-iframe\" data-content-id=\"1063\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Square Planar MCQ: The Explanation That Scores Full Marks for ClF\u2084\u207b\"><\/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 Four 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-1299\" class=\"h5p-iframe\" data-content-id=\"1299\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Square Planar Summary: Six Regions, Two Opposite Lone Pairs\"><\/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 XeF<sub>4<\/sub> octahedral<\/h3>\n            <p>The electron-pair arrangement is octahedral, but the molecular shape is square planar 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 opposite<\/h3>\n            <p>The two lone pairs occupy opposite positions above and below the square plane to minimise repulsion.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Use 90&deg; for adjacent bonds<\/h3>\n            <p>Adjacent bonds in the square plane are separated by 90&deg;. Opposite bonds are 180&deg; apart.<\/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 square planar shape is produced when a central atom has <strong>four bonding pairs<\/strong> and <strong>two lone pairs<\/strong>. The lone pairs occupy opposite positions, leaving the four bonded atoms in one flat square plane with <strong>90&deg;<\/strong> bond angles.<\/p>\n        <div class=\"ols-key-box\"><p><strong>Memory line:<\/strong> 4 bonding pairs + 2 lone pairs = square planar = 90&deg;.<\/p><\/div>\n      <\/article>\n<section class=\"ols-faq-card\">\n        <h2>Square Planar FAQs<\/h2>\n        <p>These questions target the points students most often lose marks on when explaining square planar molecular shape.<\/p>\n        <div class=\"ols-faq-list\">\n          <div class=\"ols-faq-item\">\n            <h3>Why is XeF<sub>4<\/sub> square planar?<\/h3>\n            <p>XeF<sub>4<\/sub> is square planar because xenon has four bonding pairs and two lone pairs. The six electron regions arrange octahedrally, but the two lone pairs occupy opposite positions, leaving the four Xe-F bonds in a flat square plane.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>What is the bond angle in a square planar molecule?<\/h3>\n            <p>The bond angle between adjacent bonds in a square planar molecule is 90&deg;. Opposite bonds across the square are 180&deg; apart.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Is square planar the same as octahedral?<\/h3>\n            <p>No. Square planar is the molecular shape, based on the positions of atoms. Octahedral is the electron-pair arrangement for six regions of negative charge around the central atom.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Why are the two lone pairs opposite in XeF<sub>4<\/sub>?<\/h3>\n            <p>The two lone pairs are opposite because this places them as far apart as possible, reducing lone pair-lone pair repulsion.<\/p>\n          <\/div>\n        \n<div class=\"ols-faq-item\">\n<h3>Does ICl<sub>4<\/sub><sup>&#8211;<\/sup> have the same shape as XeF<sub>4<\/sub>?<\/h3>\n<p>Yes. Iodine has 7 outer-shell electrons and the negative charge adds one, giving 8, as in xenon. Four bonds use four, leaving two lone pairs, so ICl<sub>4<\/sub><sup>&#8211;<\/sup> is also square planar with 90&deg; angles.<\/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\/octahedral\/\">Octahedral<\/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-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\/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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