{"id":4590,"date":"2026-05-30T06:12:56","date_gmt":"2026-05-30T05:12:56","guid":{"rendered":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/trigonal-bipyramidal\/"},"modified":"2026-10-25T12:15:29","modified_gmt":"2026-10-25T12:15:29","slug":"trigonal-bipyramidal","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-bipyramidal\/","title":{"rendered":"Trigonal Bipyramidal"},"content":{"rendered":"\n<section class=\"ols-revision-page ols-trigonal-bipyramidal-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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}\n    .ols-attribution-card { 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-bottom: 24px; overflow: hidden; font-family: Poppins, Arial, sans-serif; box-sizing: border-box; }\n    .ols-attribution-card, .ols-attribution-card * { box-sizing: border-box; }\n    .ols-attribution-card p { margin: 0; font-size: 14px; line-height: 1.65; font-weight: 300; color: #667085; }\n    .ols-attribution-card strong { font-weight: 700; color: #1C244B; }\n\n    @media (max-width: 1050px) {\n.ols-main { max-width: none; }\n      .ols-related-grid { grid-template-columns: repeat(2, minmax(0, 1fr)); }\n    }\n\n    @media (max-width: 760px) {\n.ols-title-card, .ols-note-card, .ols-h5p-card, .ols-related-card, .ols-faq-card, .ols-attribution-card { padding: 24px 18px; border-radius: 22px; }\n      .ols-note-title { align-items: flex-start; }\n.ols-figure-card { border-radius: 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>Trigonal Bipyramidal<\/span>\n      <\/nav>\n\n      <header class=\"ols-title-card\">\n        <h1>Trigonal Bipyramidal Molecular Shape<\/h1>\n        <p class=\"ols-page-intro\">A focused revision guide to the trigonal bipyramidal molecular shape, using PF<sub>5<\/sub> as the key example. This page explains why five bonding pairs and no lone pairs around a central atom produce axial and equatorial positions with bond angles of 90&deg;, 120&deg; and 180&deg;.<\/p>\n\n        <div class=\"ols-badges\">\n          <div class=\"ols-badge\">Unit: Paper 1<\/div>\n          <div class=\"ols-badge\">Topic 2: Bonding and Structure<\/div>\n          <div class=\"ols-badge\">9CH0\/01<\/div>\n        <\/div>\n      <\/header>\n<!-- 3D card: pf5-trigonal-bipyramidal (swapped 26 Sep 2026) -->\n<!-- Copyright (c) 2026 Dr. Mohammed Al-Fatah, onlinelearningsystem.net. All rights reserved. -->\n<!-- 3D card: pf5-trigonal-bipyramidal (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-ptbp-001 a{color:#aab0c0; text-decoration:none;}\n.ols-cc-ptbp-001 a:hover{text-decoration:underline;}\n.ols-ptbp-001 .ptbp-seg button{display:inline-flex; align-items:center;}\n.ols-ptbp-001 .ptbp-seg button .ptbp-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-ptbp-001 .ptbp-seg button[aria-pressed=\"true\"] .ptbp-n{background:#ffffff; color:#2563eb;}\n<\/style>\n\n<div class=\"ptbp-head\">\n  <h2 class=\"ptbp-title\">Trigonal Bipyramidal Shape of PF\u2085<\/h2>\n  <p class=\"ptbp-sub\">Choose a step to watch five electron pairs spread out round phosphorus and to read the axial 180\u00b0, equatorial 120\u00b0 and axial\u2013equatorial 90\u00b0 angles.<\/p>\n<\/div>\n\n<div class=\"ptbp-stage\" id=\"ptbpStage\">\n  <canvas class=\"ptbp-canvas\" id=\"ptbpCanvas\"><\/canvas>\n  <div class=\"ptbp-overlay\" id=\"ptbpOverlay\"><\/div>\n  <div class=\"ptbp-caption\" id=\"ptbpCaption\"><\/div>\n  <div class=\"ptbp-hint\" id=\"ptbpHint\">Drag to rotate<\/div>\n  <div class=\"ptbp-badges\" id=\"ptbpBadges\"><\/div>\n<\/div>\n\n<div class=\"ptbp-controls\">\n  <div class=\"ptbp-row\">\n    <span class=\"ptbp-rowlab\">Step<\/span>\n    <div class=\"ptbp-seg\" role=\"group\" aria-label=\"Step\">\n      <button type=\"button\" data-step=\"1\" aria-pressed=\"true\"><span class=\"ptbp-n\">1<\/span>Five pairs repel<\/button>\n      <button type=\"button\" data-step=\"2\" aria-pressed=\"false\"><span class=\"ptbp-n\">2<\/span>Axial pair, 180\u00b0<\/button>\n      <button type=\"button\" data-step=\"3\" aria-pressed=\"false\"><span class=\"ptbp-n\">3<\/span>Equatorial trio, 120\u00b0<\/button>\n      <button type=\"button\" data-step=\"4\" aria-pressed=\"false\"><span class=\"ptbp-n\">4<\/span>Axial\u2013equatorial, 90\u00b0<\/button>\n    <\/div>\n  <\/div>\n\n  <div class=\"ptbp-row\">\n    <span class=\"ptbp-rowlab\">View<\/span>\n    <button type=\"button\" class=\"ptbp-pill\" id=\"ptbpResetV\">Reset view<\/button>\n  <\/div>\n<\/div>\n\n<div class=\"ptbp-info\">\n  <h3 id=\"ptbpInfoTitle\"><\/h3>\n  <p id=\"ptbpInfoText\"><\/p>\n  <div class=\"ptbp-facts\" id=\"ptbpFacts\"><\/div>\n  <div class=\"ptbp-key\">\n    <span><i class=\"k-ball\" style=\"background:#ec8a28\"><\/i>Phosphorus<\/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=\"k-ball\" style=\"background:#fac828\"><\/i>Electron<\/span>\n    <span><i class=\"\" style=\"background:#c9961c\"><\/i>Bond angle \/ highlighted position<\/span>\n  <\/div>\n<\/div>\n\n<script src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/JS\/pf5-trigonal-bipyramidal.js?v=20261025p\"><\/script>\n<\/section>\n\n<p class=\"ols-cc-ptbp-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-bipyramidal-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-bipyramidal-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-bipyramidal-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-bipyramidal-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-bipyramidal-9ch0-page .ols-h5p-grid {\n    display: grid;\n    gap: 18px;\n    margin-top: 22px;\n  }\n  .ols-trigonal-bipyramidal-9ch0-page .ols-h5p-frame {\n    margin-top: 0;\n  }\n  .ols-trigonal-bipyramidal-9ch0-page .ols-formula {\n    white-space: nowrap;\n  }\n  @media (max-width: 760px) {\n    .ols-trigonal-bipyramidal-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: Angles and Pyramids<\/h2>\n<p>Before you start, check the GCSE ideas about angles and 3D shapes that this page builds on.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"680\"><\/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 Bipyramidal Means<\/h2>\n        <\/div>\n        <p>A <strong>trigonal bipyramidal<\/strong> molecule has five atoms bonded to a central atom and no lone pairs on that central atom. The five bonding regions repel and arrange themselves as far apart as possible.<\/p>\n        <p>The key example for this page is <strong>PF<sub>5<\/sub><\/strong>. Phosphorus is the central atom and forms five P-F bonds to five fluorine atoms.<\/p>\n\n        <div class=\"ols-spec-grid\">\n          <div class=\"ols-spec-box\">\n            <strong>Bonding pairs<\/strong>\n            <span>5 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 angles<\/strong>\n            <span>120&deg; equatorial, 90&deg; axial-equatorial, 180&deg; axial-axial<\/span>\n          <\/div>\n        <\/div>\n\n        <div class=\"ols-key-box\"><p><strong>Key idea:<\/strong> five bonding pairs and no lone pairs around a central atom give a trigonal bipyramidal shape.<\/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 PF<sub>5<\/sub> Is Trigonal Bipyramidal<\/h2>\n        <\/div>\n        <p>In PF<sub>5<\/sub>, the central phosphorus atom is surrounded by five P-F bonding pairs. There are no lone pairs on the phosphorus atom, so the five bonding regions arrange to minimise bonding pair-bonding pair repulsion.<\/p>\n        <p>The shape has <strong>three equatorial positions<\/strong> in a trigonal plane and <strong>two axial positions<\/strong> above and below this plane. The molecular shape is therefore described as trigonal bipyramidal.<\/p>\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-P147-pf5-trigonal-bipyramidal.svg\" data-ols-lightbox-alt=\"PF5 is trigonal bipyramidal: five bonding pairs, no lone pairs, bond angles 90\u00b0 (axial) and 120\u00b0 (equatorial)\" aria-label=\"Open PF5 trigonal bipyramidal diagram in full screen\">\n            <img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-cd-14-pf5-tbp.svg\" alt=\"Trigonal bipyramidal PF\u2085 with axial and equatorial F atoms labelled and 90\u00b0 and 120\u00b0 angles marked\" width=\"1023\" height=\"474\">\n          <\/button>\n          <div class=\"ols-figure-caption\">\n            <p>PF<sub>5<\/sub> has five bonding regions around phosphorus. Three fluorine atoms occupy equatorial positions and two fluorine atoms occupy axial positions.<\/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-28-countpf5.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-28-countpf5.jpg\" alt=\"Five-step electron-pair count for PF\u2085 giving five bonding regions and a trigonal bipyramidal shape with 90\u00b0 and 120\u00b0 angles\" data-fullscreen-src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-28-countpf5.jpg\">\n<\/a>\n<\/div>\n<div class=\"ols-figure-caption\"><p>Phosphorus uses all 5 outer electrons in bonds: five regions and no lone pairs give a trigonal bipyramid.<\/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: Five Bonds, No Lone Pair?<\/h2>\n<p>Choose the pentafluoride that has no lone pair on its central atom.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-197\" class=\"h5p-iframe\" data-content-id=\"197\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Trigonal Bipyramidal MCQ: The Pentafluoride with No Lone Pair\"><\/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>Axial and Equatorial Positions<\/h2>\n        <\/div>\n        <p>The trigonal bipyramidal shape has two different types of position around the central atom. The <strong>equatorial positions<\/strong> lie in the central triangular plane. The <strong>axial positions<\/strong> point above and below this plane.<\/p>\n        <p>This produces different bond angles within the same molecule. Equatorial bonds are 120&deg; apart, axial bonds are 90&deg; from equatorial bonds, and the two axial bonds are 180&deg; apart.<\/p>\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Equatorial positions<\/h3>\n            <p>Three positions in the central plane. The equatorial bond angles are 120&deg;.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Axial positions<\/h3>\n            <p>Two positions above and below the central plane. Each axial bond is 90&deg; from the equatorial plane.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Opposite axial bonds<\/h3>\n            <p>The two axial bonds are opposite each other, giving an axial-axial angle of 180&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-21-fivepairs.jpg\" target=\"_blank\" rel=\"noopener\" aria-label=\"Open image fullscreen\">\n<img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-21-fivepairs.jpg\" alt=\"Trigonal bipyramid key with PF\u2085, SF\u2084 and ClF\u2083 sketches showing lone pairs in equatorial positions and their bond angles\" data-fullscreen-src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/10\/t3-img-21-fivepairs.jpg\">\n<\/a>\n<\/div>\n<div class=\"ols-figure-caption\"><p>Five regions form a trigonal bipyramid; lone pairs take equatorial positions to give the see-saw and distorted T shapes.<\/p><\/div>\n<\/div>\n<\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Count the Angles<\/h2>\n<p>Count the 90\u00b0 and 120\u00b0 angles in SbCl\u2085.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-198\" class=\"h5p-iframe\" data-content-id=\"198\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Trigonal Bipyramidal Single Choice: Counting the Angles in SbCl\u2085\"><\/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>Trigonal Bipyramidal Examples<\/h2>\n        <\/div>\n        <p>The trigonal bipyramidal shape is found when the central atom has five bonding pairs and no lone pairs. PF<sub>5<\/sub> and PCl<sub>5<\/sub> are common examples.<\/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 angles<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Species\">PF<sub>5<\/sub><\/td>\n                <td data-label=\"Central atom\">P<\/td>\n                <td data-label=\"Electron regions\">5 bonding regions, 0 lone pairs<\/td>\n                <td data-label=\"Shape\">Trigonal bipyramidal<\/td>\n                <td data-label=\"Typical exam angles\">90&deg;, 120&deg; and 180&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">PCl<sub>5<\/sub><\/td>\n                <td data-label=\"Central atom\">P<\/td>\n                <td data-label=\"Electron regions\">5 bonding regions, 0 lone pairs<\/td>\n                <td data-label=\"Shape\">Trigonal bipyramidal<\/td>\n                <td data-label=\"Typical exam angles\">90&deg;, 120&deg; and 180&deg;<\/td>\n              <\/tr>\n            <\/tbody>\n          <\/table>\n        <\/div>\n      <\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Explaining a New Pentafluoride<\/h2>\n<p>Decide whether each statement about AsF\u2085 is true or false.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"1062\"><\/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 Bipyramidal Shape in an Exam<\/h2>\n        <\/div>\n        <p>A full exam explanation should connect the number of bonding pairs to electron-pair repulsion, then state the shape and the bond angles.<\/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 PF<sub>5<\/sub>, the central atom is phosphorus.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>2. Count bonding pairs and lone pairs<\/h3>\n            <p>Phosphorus has five 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 five bonding pairs repel and arrange themselves as far apart as possible, giving three equatorial positions and two axial positions.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>4. State the shape and angles<\/h3>\n            <p>The molecule is trigonal bipyramidal with bond angles of 120&deg; between equatorial bonds, 90&deg; between axial and equatorial bonds, and 180&deg; between the axial bonds.<\/p>\n          <\/div>\n        <\/div>\n\n        <div class=\"ols-definition-box\">\n          <p><strong>Exam answer model:<\/strong> PF<sub>5<\/sub> has five bonding pairs and no lone pairs around the central phosphorus atom. The bonding pairs repel and arrange themselves as far apart as possible.<\/p>\n<p>Three fluorine atoms occupy equatorial positions at 120&deg; to each other, while two fluorine atoms occupy axial positions at 90&deg; to the equatorial plane and 180&deg; from each other. Therefore, PF<sub>5<\/sub> is trigonal bipyramidal.<\/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: Spot the Sound Reasoning<\/h2>\n<p>In each round, choose the one fully correct statement to review the whole page.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-196\" class=\"h5p-iframe\" data-content-id=\"196\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Trigonal Bipyramidal Summary: Spot the Sound Reasoning\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card soft\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">6<\/div>\n          <h2>Common Exam Points<\/h2>\n        <\/div>\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Do not use only one bond angle<\/h3>\n            <p>Trigonal bipyramidal molecules have more than one relevant angle. State 120&deg; for equatorial-equatorial, 90&deg; for axial-equatorial and 180&deg; for axial-axial when needed.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Separate trigonal planar from trigonal bipyramidal<\/h3>\n            <p>Trigonal planar has three bonding regions and a 120&deg; angle. Trigonal bipyramidal has five bonding regions with axial and equatorial positions.<\/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 bonding pairs and lone pairs around phosphorus in PF<sub>5<\/sub>, not by the total number of atoms in the formula alone.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Use electron-pair repulsion language<\/h3>\n            <p>Explain that bonding pairs repel and arrange as far apart as possible. Since PF<sub>5<\/sub> has no lone pairs on phosphorus, there is no lone pair compression to discuss.<\/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 bipyramidal shape is produced when a central atom has <strong>five bonding pairs<\/strong> and <strong>no lone pairs<\/strong>. PF<sub>5<\/sub> has three equatorial bonds and two axial bonds, giving bond angles of <strong>120&deg;<\/strong>, <strong>90&deg;<\/strong> and <strong>180&deg;<\/strong>.<\/p>\n        <div class=\"ols-key-box\"><p><strong>Memory line:<\/strong> 5 bonding pairs + 0 lone pairs = trigonal bipyramidal = 90&deg;, 120&deg; and 180&deg;.<\/p><\/div>\n      <\/article>\n\n      <section class=\"ols-faq-card\">\n        <h2>FAQs<\/h2>\n        <p>Common questions about trigonal bipyramidal molecular shape.<\/p>\n        <div class=\"ols-faq-list\">\n          <div class=\"ols-faq-item\">\n            <h3>What is a trigonal bipyramidal molecular shape?<\/h3>\n            <p>A trigonal bipyramidal molecular shape forms when a central atom has five bonding pairs and no lone pairs. Three atoms occupy equatorial positions and two atoms occupy axial positions.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Why is PF<sub>5<\/sub> trigonal bipyramidal?<\/h3>\n            <p>PF<sub>5<\/sub> is trigonal bipyramidal because phosphorus has five P-F bonding pairs and no lone pairs around it. The five bonding regions repel and arrange themselves as far apart as possible.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>What are the bond angles in PF<sub>5<\/sub>?<\/h3>\n            <p>PF<sub>5<\/sub> has 120&deg; between equatorial bonds, 90&deg; between axial and equatorial bonds, and 180&deg; between the two axial bonds.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>What is the difference between axial and equatorial positions?<\/h3>\n            <p>Equatorial positions lie in the central triangular plane and are 120&deg; apart. Axial positions are above and below this plane and are 90&deg; from the equatorial positions.<\/p>\n          <\/div>\n        \n<div class=\"ols-faq-item\">\n<h3>Why are the bond angles in PF<sub>5<\/sub> not all the same?<\/h3>\n<p>Five regions cannot be spaced equally in three dimensions. The lowest-repulsion arrangement has three equatorial bonds at 120&deg; to each other and two axial bonds at 90&deg; to them, with 180&deg; between the two axial bonds.<\/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 pages to connect trigonal bipyramidal shape with the rest of Topic 2 bonding and structure.<\/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\/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\/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\/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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The lowest-repulsion arrangement has three equatorial bonds at 120\u00b0 to each other and two axial bonds at 90\u00b0 to them, with 180\u00b0 between the two axial bonds.\"\n                    }\n                }\n            ]\n        }\n    ]\n}\n<\/script>\n    <\/main>\n<\/section>\n\n","protected":false},"excerpt":{"rendered":"<p>Revision Notes \/ A Level Chemistry \/ Edexcel \/ Topic 2 Bonding and Structure \/ Shapes of Molecules \/ Trigonal Bipyramidal Trigonal Bipyramidal Molecular Shape A focused revision guide to the trigonal bipyramidal molecular shape, using PF5 as the key example. 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