{"id":4586,"date":"2026-05-30T06:12:46","date_gmt":"2026-05-30T05:12:46","guid":{"rendered":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/trigonal-planar\/"},"modified":"2026-10-25T12:07:31","modified_gmt":"2026-10-25T12:07:31","slug":"trigonal-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\/trigonal-planar\/","title":{"rendered":"Trigonal Planar"},"content":{"rendered":"\n<section class=\"ols-revision-page ols-trigonal-planar-molecular-shape-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      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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      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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>Trigonal Planar<\/span>\n      <\/nav>\n\n      <header class=\"ols-title-card\">\n        <h1>Trigonal Planar Molecular Shape<\/h1>\n        <p class=\"ols-page-intro\">A focused revision guide to the trigonal planar molecular shape, using BCl<sub>3<\/sub> as the key example. This page explains why three bonding pairs and no lone pairs around a central atom give 120&deg; bond angles in one flat plane.<\/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: bcl3-trigonal-planar (swapped 26 Sep 2026) -->\n<!-- Copyright (c) 2026 Dr. Mohammed Al-Fatah, onlinelearningsystem.net. All rights reserved. -->\n<!-- 3D card: bcl3-trigonal-planar (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-bctp-001 .bctp-key i.k-ball{border-radius:50%;}\n\n@media (max-width:760px){\n  .ols-bctp-001{padding:26px; border-radius:22px;}\n  .ols-bctp-001 h2.bctp-title{font-size:20.5px;}\n  .ols-bctp-001 p.bctp-sub{font-size:13.5px;}\n  .ols-bctp-001 .bctp-stage{height:400px;}\n  .ols-bctp-001 .bctp-rowlab{min-width:100%;}\n  .ols-bctp-001 .bctp-seg button{padding:9px 13px; font-size:13px;}\n  .ols-bctp-001 .bctp-lab{font-size:10.5px; padding:4px 8px;}\n  .ols-bctp-001 .bctp-lab.l-part{font-size:9.5px; padding:3px 7px;}\n  .ols-bctp-001 .bctp-lab.l-read{font-size:12px; padding:5px 9px;}\n  .ols-bctp-001 .bctp-caption{font-size:10.5px; padding:5px 9px; max-width:64%;}\n  .ols-bctp-001 .bctp-badge{font-size:10.5px; padding:4px 9px;}\n  .ols-bctp-001 .bctp-badge.b-eq{font-size:11px;}\n  .ols-bctp-001 .bctp-badges{max-width:calc(100% - 28px);}\n  .ols-bctp-001 .bctp-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-bctp-001 .bctp-hint{display:none;}\n  .ols-bctp-001 .bctp-caption{max-width:calc(100% - 28px);}\n}\n@media (prefers-reduced-motion:reduce){\n  .ols-bctp-001 .bctp-seg button,.ols-bctp-001 .bctp-pill{transition:none;}\n}\n\n.ols-cc-bctp-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-bctp-001 a{color:#aab0c0; text-decoration:none;}\n.ols-cc-bctp-001 a:hover{text-decoration:underline;}\n.ols-bctp-001 .bctp-seg button{display:inline-flex; align-items:center;}\n.ols-bctp-001 .bctp-seg button .bctp-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-bctp-001 .bctp-seg button[aria-pressed=\"true\"] .bctp-n{background:#ffffff; color:#2563eb;}\n<\/style>\n\n<div class=\"bctp-head\">\n  <h2 class=\"bctp-title\">Trigonal Planar Shape of BCl\u2083<\/h2>\n  <p class=\"bctp-sub\">Choose a step to watch three electron pairs repel into a flat triangle, bond to chlorine, read the 120\u00b0 angles and turn edge-on to see the molecule is flat.<\/p>\n<\/div>\n\n<div class=\"bctp-stage\" id=\"bctpStage\">\n  <canvas class=\"bctp-canvas\" id=\"bctpCanvas\"><\/canvas>\n  <div class=\"bctp-overlay\" id=\"bctpOverlay\"><\/div>\n  <div class=\"bctp-caption\" id=\"bctpCaption\"><\/div>\n  <div class=\"bctp-hint\" id=\"bctpHint\">Drag to rotate<\/div>\n  <div class=\"bctp-badges\" id=\"bctpBadges\"><\/div>\n<\/div>\n\n<div class=\"bctp-controls\">\n  <div class=\"bctp-row\">\n    <span class=\"bctp-rowlab\">Step<\/span>\n    <div class=\"bctp-seg\" role=\"group\" aria-label=\"Step\">\n      <button type=\"button\" data-step=\"1\" aria-pressed=\"true\"><span class=\"bctp-n\">1<\/span>Pairs repel<\/button>\n      <button type=\"button\" data-step=\"2\" aria-pressed=\"false\"><span class=\"bctp-n\">2<\/span>Bonds to chlorine<\/button>\n      <button type=\"button\" data-step=\"3\" aria-pressed=\"false\"><span class=\"bctp-n\">3<\/span>120\u00b0 bond angles<\/button>\n      <button type=\"button\" data-step=\"4\" aria-pressed=\"false\"><span class=\"bctp-n\">4<\/span>Turn edge-on<\/button>\n    <\/div>\n  <\/div>\n\n  <div class=\"bctp-row\">\n    <span class=\"bctp-rowlab\">View<\/span>\n    <button type=\"button\" class=\"bctp-pill\" id=\"bctpResetV\">Reset view<\/button>\n  <\/div>\n<\/div>\n\n<div class=\"bctp-info\">\n  <h3 id=\"bctpInfoTitle\"><\/h3>\n  <p id=\"bctpInfoText\"><\/p>\n  <div class=\"bctp-facts\" id=\"bctpFacts\"><\/div>\n  <div class=\"bctp-key\">\n    <span><i class=\"\" style=\"background:rgba(59,120,220,0.45)\"><\/i>Electron pair (bonding region)<\/span>\n    <span><i class=\"k-ball\" style=\"background:#facc28\"><\/i>Electron<\/span>\n    <span><i class=\"k-ball\" style=\"background:#f0b4a0\"><\/i>Boron, central atom<\/span>\n    <span><i class=\"k-ball\" style=\"background:#34aa48\"><\/i>Chlorine<\/span>\n    <span><i class=\"\" style=\"background:#b4b9c6\"><\/i>Bond<\/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\/bcl3-trigonal-planar.js?v=20261025p\"><\/script>\n<\/section>\n\n<p class=\"ols-cc-bctp-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-trigonal-planar-molecular-shape-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-trigonal-planar-molecular-shape-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-trigonal-planar-molecular-shape-9ch0-page .ols-spec-box strong {\n    display: block;\n    font-size: 15px;\n    color: var(--blue);\n    margin-bottom: 6px;\n  }\n  .ols-trigonal-planar-molecular-shape-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-trigonal-planar-molecular-shape-9ch0-page .ols-h5p-grid {\n    display: grid;\n    gap: 18px;\n    margin-top: 22px;\n  }\n  .ols-trigonal-planar-molecular-shape-9ch0-page .ols-h5p-frame {\n    margin-top: 0;\n  }\n  .ols-trigonal-planar-molecular-shape-9ch0-page .ols-formula {\n    white-space: nowrap;\n  }\n  @media (max-width: 760px) {\n    .ols-trigonal-planar-molecular-shape-9ch0-page .ols-spec-grid {\n      grid-template-columns: 1fr;\n    }\n  }\n<\/style>\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: Double Covalent Bonds<\/h2>\n<p>Before you start, check the GCSE ideas about double bonds that this page builds on.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"677\"><\/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 Trigonal Planar Means<\/h2>\n        <\/div>\n        <p>A <strong>trigonal planar<\/strong> molecule has three atoms arranged around a central atom in a flat triangular pattern. The word <strong>trigonal<\/strong> means three positions around the central atom, and <strong>planar<\/strong> means all the atoms lie in the same plane.<\/p>\n        <p>The key example for this page is <strong>BCl<sub>3<\/sub><\/strong>. Boron is the central atom and each chlorine atom is attached to boron by a covalent bond.<\/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>0 lone pairs on the central atom<\/span>\n          <\/div>\n          <div class=\"ols-spec-box\">\n            <strong>Bond angle<\/strong>\n            <span>120&deg; between each bond<\/span>\n          <\/div>\n        <\/div>\n\n        <div class=\"ols-key-box\"><p><strong>Key idea:<\/strong> three bonding regions and no lone pairs around a central atom give a trigonal planar shape with 120&deg; bond angles.<\/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 BCl<sub>3<\/sub> Is Trigonal Planar<\/h2>\n        <\/div>\n        <p>In BCl<sub>3<\/sub>, the central boron atom is surrounded by three B-Cl bonding pairs. These bonding pairs are regions of negative charge, so they repel each other and move as far apart as possible.<\/p>\n        <p>With three equal bonding regions and no lone pairs, the maximum separation is achieved when the bonds are spread evenly in one plane. This places each B-Cl bond <strong>120&deg;<\/strong> from the next.<\/p>\n\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-24-countbcl3.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-24-countbcl3.jpg\" alt=\"Five-step electron-pair count for BCl\u2083 giving three bonding regions, no lone pairs and a trigonal planar 120\u00b0 shape\">\n<\/a>\n<\/div>\n<div class=\"ols-zoom-card-caption\"><p>Boron has 3 outer electrons, all used in bonds: three regions and no lone pairs give a trigonal planar 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: Why Flat?<\/h2>\n<p>Choose the statement that explains why borane is flat.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-181\" class=\"h5p-iframe\" data-content-id=\"181\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Trigonal Planar MCQ: Why Borane Is Flat and Not a Pyramid\"><\/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-10-bcl3-planar.svg\" alt=\"Trigonal planar BCl\u2083 with 120\u00b0 angles and lone pairs on Cl, beside its dot-and-cross diagram with six electrons round boron\" class=\"ols-zoomable-img ols-lightbox-target\" draggable=\"false\" width=\"1006\" height=\"408\">\n        <\/div>\n        <div class=\"ols-zoom-card-caption\">\n          <p>BCl<sub>3<\/sub> has three B-Cl bonds around boron and no lone pairs on the central atom, so the three bonds spread out evenly.<\/p>\n        <\/div>\n      <\/div>\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>Bonding Pairs, Lone Pairs and Bond Angle<\/h2>\n        <\/div>\n        <p>The shape is decided by the number of electron domains around the central atom. In a simple shape question, each single bond counts as one bonding region. BCl<sub>3<\/sub> has three bonding regions around boron and no lone pair regions on boron.<\/p>\n\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Feature<\/th>\n                <th>Trigonal planar value<\/th>\n                <th>Meaning in BCl<sub>3<\/sub><\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Feature\">Number of bonding pairs<\/td>\n                <td data-label=\"Trigonal planar value\">3<\/td>\n                <td data-label=\"Meaning in BCl3\">Three B-Cl bonding pairs repel each other equally.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Feature\">Number of lone pairs<\/td>\n                <td data-label=\"Trigonal planar value\">0<\/td>\n                <td data-label=\"Meaning in BCl3\">No lone pair compression occurs, so the ideal angle is maintained.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Feature\">Bond angle<\/td>\n                <td data-label=\"Trigonal planar value\">120&deg;<\/td>\n                <td data-label=\"Meaning in BCl3\">The three bonds are evenly spaced in a flat triangular arrangement.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Feature\">Molecular shape<\/td>\n                <td data-label=\"Trigonal planar value\">Trigonal planar<\/td>\n                <td data-label=\"Meaning in BCl3\">All four atoms lie in one plane.<\/td>\n              <\/tr>\n            <\/tbody>\n          <\/table>\n        <\/div>\n      <div class=\"ols-zoom-card\">\n<div class=\"ols-zoom-card-image\">\n<a class=\"ols-lightbox-link\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-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 Regions<\/h2>\n<p>Count the bonding regions and lone pairs, then type the numbers.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-182\" class=\"h5p-iframe\" data-content-id=\"182\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Trigonal Planar Fill in the Blanks: Counting Regions in GaCl\u2083 and COCl\u2082\"><\/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>Examples of Trigonal Planar Species<\/h2>\n        <\/div>\n        <p>Several molecules and ions use the same three-region arrangement around the central atom. Other examples are <strong>BF<sub>3<\/sub><\/strong>, <strong>AlCl<sub>3<\/sub><\/strong>, <strong>SO<sub>3<\/sub><\/strong>, <strong>NO<sub>3<\/sub><sup>&#8211;<\/sup><\/strong> and <strong>CO<sub>3<\/sub><sup>2-<\/sup><\/strong>.<\/p>\n        <p>For exam purposes, focus on the central atom, count the electron domains around it, then state the shape and bond angle.<\/p>\n\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 around central atom<\/th>\n                <th>Shape<\/th>\n                <th>Bond angle<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Species\">BF<sub>3<\/sub><\/td>\n                <td data-label=\"Central atom\">B<\/td>\n                <td data-label=\"Electron regions\">3 bonding regions, 0 lone pairs<\/td>\n                <td data-label=\"Shape\">Trigonal planar<\/td>\n                <td data-label=\"Bond angle\">120&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">AlCl<sub>3<\/sub><\/td>\n                <td data-label=\"Central atom\">Al<\/td>\n                <td data-label=\"Electron regions\">3 bonding regions, 0 lone pairs<\/td>\n                <td data-label=\"Shape\">Trigonal planar<\/td>\n                <td data-label=\"Bond angle\">120&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">SO<sub>3<\/sub><\/td>\n                <td data-label=\"Central atom\">S<\/td>\n                <td data-label=\"Electron regions\">3 bonding regions, 0 lone pairs<\/td>\n                <td data-label=\"Shape\">Trigonal planar<\/td>\n                <td data-label=\"Bond angle\">120&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">NO<sub>3<\/sub><sup>&#8211;<\/sup><\/td>\n                <td data-label=\"Central atom\">N<\/td>\n                <td data-label=\"Electron regions\">3 bonding regions, 0 lone pairs<\/td>\n                <td data-label=\"Shape\">Trigonal planar<\/td>\n                <td data-label=\"Bond angle\">120&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">CO<sub>3<\/sub><sup>2-<\/sup><\/td>\n                <td data-label=\"Central atom\">C<\/td>\n                <td data-label=\"Electron regions\">3 bonding regions, 0 lone pairs<\/td>\n                <td data-label=\"Shape\">Trigonal planar<\/td>\n                <td data-label=\"Bond angle\">120&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: Trigonal Planar or Not?<\/h2>\n<p>Decide quickly whether each species is trigonal planar.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-180\" class=\"h5p-iframe\" data-content-id=\"180\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Trigonal Planar Single Choice: Trigonal Planar or Not?\"><\/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 Trigonal Planar Shape in an Exam<\/h2>\n        <\/div>\n        <p>A full exam explanation should name the electron pairs around the central atom and connect this directly to repulsion and angle.<\/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 BCl<sub>3<\/sub>, the central atom is boron.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>2. Count bonding pairs and lone pairs<\/h3>\n            <p>Boron has three bonding pairs and no lone pairs around it.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>3. Apply electron-pair repulsion<\/h3>\n            <p>The three bonding pairs repel equally and move as far apart as possible.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>4. State the shape and angle<\/h3>\n            <p>The molecule is trigonal planar with bond angles of 120&deg;.<\/p>\n          <\/div>\n        <\/div>\n\n        <div class=\"ols-definition-box\">\n          <p><strong>Exam answer model:<\/strong> BCl<sub>3<\/sub> has three bonding pairs and no lone pairs around the central boron atom. The bonding pairs repel equally and arrange themselves as far apart as possible in one plane. Therefore, BCl<sub>3<\/sub> is trigonal planar with bond angles of 120&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: Write the Exam Answer<\/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-183\" class=\"h5p-iframe\" data-content-id=\"183\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Trigonal Planar Explain: Shape and Bond Angle of the Methyl Cation\"><\/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-1297\" class=\"h5p-iframe\" data-content-id=\"1297\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Trigonal Planar Summary: Three Regions, No Lone Pair, 120\u00b0\"><\/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        <p>Trigonal planar questions often test whether you can distinguish between the number of atoms attached to the central atom and the number of electron domains around the central atom.<\/p>\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Do not write 109.5&deg;<\/h3>\n            <p>109.5&deg; is the tetrahedral angle. Trigonal planar species have three electron regions and an ideal angle of 120&deg;.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Do not add a lone pair to boron in BCl<sub>3<\/sub><\/h3>\n            <p>For this shape model, boron has three bonding pairs and no lone pairs around the central atom.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>State \u201cin one plane\u201d when useful<\/h3>\n            <p>The planar part of trigonal planar means the atoms lie in a flat arrangement.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Use electron-pair repulsion language<\/h3>\n            <p>Marks usually require the idea that bonding pairs repel and arrange themselves as far apart as possible.<\/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 trigonal planar shape is produced when a central atom has <strong>three bonding pairs<\/strong> and <strong>no lone pairs<\/strong>. The bonding pairs repel equally and spread out evenly in one plane, giving <strong>120&deg;<\/strong> bond angles.<\/p>\n        <div class=\"ols-key-box\"><p><strong>Memory line:<\/strong> 3 bonding pairs + 0 lone pairs = trigonal planar = 120&deg;.<\/p><\/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 trigonal planar molecular shape.<\/p>\n        <div class=\"ols-faq-list\">\n          <div class=\"ols-faq-item\">\n            <h3>What makes a molecule trigonal planar?<\/h3>\n            <p>A molecule is trigonal planar when the central atom has three bonding regions and no lone pairs. The bonding pairs repel equally and arrange themselves 120&deg; apart in one plane.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Why is BCl<sub>3<\/sub> trigonal planar?<\/h3>\n            <p>BCl<sub>3<\/sub> has three B-Cl bonding pairs around the central boron atom and no lone pairs on boron in the shape model. The three bonding pairs repel equally, so the molecule is trigonal planar with 120&deg; bond angles.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>What is the bond angle in a trigonal planar molecule?<\/h3>\n            <p>The ideal bond angle in a trigonal planar molecule is 120&deg;.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Are all atoms in a trigonal planar molecule in one plane?<\/h3>\n            <p>Yes. In a trigonal planar molecule such as BCl<sub>3<\/sub>, the central atom and the three surrounding atoms lie in the same plane.<\/p>\n          <\/div>\n        \n<div class=\"ols-faq-item\">\n<h3>Why is NH<sub>3<\/sub> not trigonal planar when BF<sub>3<\/sub> is?<\/h3>\n<p>BF<sub>3<\/sub> has three bonding pairs and no lone pairs, so it is trigonal planar at 120&deg;. NH<sub>3<\/sub> also has a lone pair, giving four regions, so its shape is trigonal pyramidal at about 107&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\"\n      class=\"ols-author-avatar-img\"\n      src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/05\/Author-Profile.jpeg\"\n      alt=\"Dr. Mohammed Al-Fatah\"\n    >\n\n    <div class=\"ols-author-content\">\n\n      <h2 class=\"ols-author-title\">\n        Written by: Dr. Mohammed Al-Fatah\n      <\/h2>\n\n      <p class=\"ols-author-description\">\n        Chemistry specialist revision notes for A Level Chemistry.\n      <\/p>\n\n      <a\n        class=\"ols-linkedin-pill\"\n        href=\"https:\/\/www.linkedin.com\/in\/doctormohammedfatah\/\"\n        target=\"_blank\"\n        rel=\"noopener noreferrer\"\n      >\n        <svg class=\"ols-linkedin-icon\" viewBox=\"0 0 24 24\" fill=\"currentColor\" aria-hidden=\"true\">\n          <path d=\"M4.98 3.5C4.98 4.88 3.86 6 2.48 6S0 4.88 0 3.5 1.12 1 2.48 1s2.5 1.12 2.5 2.5zM.5 8h4V24h-4V8zm7 0h3.8v2.2h.1c.5-.9 1.8-2.2 3.9-2.2 4.2 0 5 2.8 5 6.4V24h-4v-7.6c0-1.8 0-4.2-2.6-4.2s-3 2-3 4v7.8h-4V8z\"\/>\n        <\/svg>\n        View LinkedIn Profile\n      <\/a>\n\n    <\/div>\n\n  <\/div>\n\n\n      <section class=\"ols-related-card\">\n        <h2>Related Topics<\/h2>\n        <p>Use these pages to connect trigonal planar 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\/linear\/\">Linear<\/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<script type=\"application\/ld+json\">\n{\n    \"@context\": \"https:\/\/schema.org\",\n    \"@graph\": [\n        {\n            \"@type\": \"WebPage\",\n            \"@id\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/trigonal-planar\/#webpage\",\n            \"url\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/trigonal-planar\/\",\n            \"name\": \"Trigonal Planar Molecular Shape | Edexcel A Level Chemistry\",\n            \"description\": \"A Level Chemistry revision notes explaining the trigonal planar molecular shape, BCl3, electron-pair repulsion, three bonding pairs, no lone pairs and 120 degree bond angles.\",\n            \"isPartOf\": {\n                \"@type\": 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The bonding pairs repel equally and arrange themselves 120\u00b0 apart in one plane.\"\n                    }\n                },\n                {\n                    \"@type\": \"Question\",\n                    \"name\": \"Why is BCl3 trigonal planar?\",\n                    \"acceptedAnswer\": {\n                        \"@type\": \"Answer\",\n                        \"text\": \"BCl3 has three B-Cl bonding pairs around the central boron atom and no lone pairs on boron in the shape model. 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This page explains why three bonding pairs and no lone pairs around a central [&hellip;]<\/p>\n","protected":false},"author":12,"featured_media":0,"parent":4572,"menu_order":1,"comment_status":"closed","ping_status":"closed","template":"","meta":{"footnotes":""},"class_list":["post-4586","page","type-page","status-publish","hentry"],"_links":{"self":[{"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages\/4586","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages"}],"about":[{"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/types\/page"}],"author":[{"embeddable":true,"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/users\/12"}],"replies":[{"embeddable":true,"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/comments?post=4586"}],"version-history":[{"count":2,"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages\/4586\/revisions"}],"predecessor-version":[{"id":24454,"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages\/4586\/revisions\/24454"}],"up":[{"embeddable":true,"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages\/4572"}],"wp:attachment":[{"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/media?parent=4586"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}