{"id":4587,"date":"2026-05-30T06:12:48","date_gmt":"2026-05-30T05:12:48","guid":{"rendered":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/tetrahedral\/"},"modified":"2026-10-25T12:08:37","modified_gmt":"2026-10-25T12:08:37","slug":"tetrahedral","status":"publish","type":"page","link":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/tetrahedral\/","title":{"rendered":"Tetrahedral"},"content":{"rendered":"\n<section class=\"ols-revision-page ols-tetrahedral-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      --body-text: #1f2937;\n      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 .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-zoom-card { border-radius: 22px; }\n      .ols-zoom-card-image { min-height: 210px; padding: 14px; }\n      .ols-zoom-card-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      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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>Tetrahedral<\/span>\n      <\/nav>\n\n      <header class=\"ols-title-card\">\n        <h1>Tetrahedral Molecular Shape<\/h1>\n        <p class=\"ols-page-intro\">A focused revision guide to the tetrahedral molecular shape, using CH<sub>4<\/sub> as the key example. This page explains why four bonding pairs and no lone pairs around a central atom give a three-dimensional tetrahedral arrangement with bond angles of 109.5&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: ch4-tetrahedral (swapped 26 Sep 2026) -->\n<!-- Copyright (c) 2026 Dr. Mohammed Al-Fatah, onlinelearningsystem.net. All rights reserved. -->\n<!-- 3D card: ch4-tetrahedral (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-ctet-001 .ctet-key i.k-ball{border-radius:50%;}\n\n@media (max-width:760px){\n  .ols-ctet-001{padding:26px; border-radius:22px;}\n  .ols-ctet-001 h2.ctet-title{font-size:20.5px;}\n  .ols-ctet-001 p.ctet-sub{font-size:13.5px;}\n  .ols-ctet-001 .ctet-stage{height:400px;}\n  .ols-ctet-001 .ctet-rowlab{min-width:100%;}\n  .ols-ctet-001 .ctet-seg button{padding:9px 13px; font-size:13px;}\n  .ols-ctet-001 .ctet-lab{font-size:10.5px; padding:4px 8px;}\n  .ols-ctet-001 .ctet-lab.l-part{font-size:9.5px; padding:3px 7px;}\n  .ols-ctet-001 .ctet-lab.l-read{font-size:12px; padding:5px 9px;}\n  .ols-ctet-001 .ctet-caption{font-size:10.5px; padding:5px 9px; max-width:64%;}\n  .ols-ctet-001 .ctet-badge{font-size:10.5px; padding:4px 9px;}\n  .ols-ctet-001 .ctet-badge.b-eq{font-size:11px;}\n  .ols-ctet-001 .ctet-badges{max-width:calc(100% - 28px);}\n  .ols-ctet-001 .ctet-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-ctet-001 .ctet-hint{display:none;}\n  .ols-ctet-001 .ctet-caption{max-width:calc(100% - 28px);}\n}\n@media (prefers-reduced-motion:reduce){\n  .ols-ctet-001 .ctet-seg button,.ols-ctet-001 .ctet-pill{transition:none;}\n}\n\n.ols-cc-ctet-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-ctet-001 a{color:#aab0c0; text-decoration:none;}\n.ols-cc-ctet-001 a:hover{text-decoration:underline;}\n.ols-ctet-001 .ctet-seg button{display:inline-flex; align-items:center;}\n.ols-ctet-001 .ctet-seg button .ctet-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-ctet-001 .ctet-seg button[aria-pressed=\"true\"] .ctet-n{background:#ffffff; color:#2563eb;}\n<\/style>\n\n<div class=\"ctet-head\">\n  <h2 class=\"ctet-title\">Tetrahedral Shape of CH\u2084<\/h2>\n  <p class=\"ctet-sub\">Choose a step to watch four electron pairs push apart into a tetrahedron, become C\u2013H bonds at 109.5\u00b0 and turn into a wedge-and-dash drawing.<\/p>\n<\/div>\n\n<div class=\"ctet-stage\" id=\"ctetStage\">\n  <canvas class=\"ctet-canvas\" id=\"ctetCanvas\"><\/canvas>\n  <div class=\"ctet-overlay\" id=\"ctetOverlay\"><\/div>\n  <div class=\"ctet-caption\" id=\"ctetCaption\"><\/div>\n  <div class=\"ctet-hint\" id=\"ctetHint\">Drag to rotate<\/div>\n  <div class=\"ctet-badges\" id=\"ctetBadges\"><\/div>\n<\/div>\n\n<div class=\"ctet-controls\">\n  <div class=\"ctet-row\">\n    <span class=\"ctet-rowlab\">Step<\/span>\n    <div class=\"ctet-seg\" role=\"group\" aria-label=\"Step\">\n      <button type=\"button\" data-step=\"1\" aria-pressed=\"true\"><span class=\"ctet-n\">1<\/span>Flat square to tetrahedron<\/button>\n      <button type=\"button\" data-step=\"2\" aria-pressed=\"false\"><span class=\"ctet-n\">2<\/span>Four C\u2013H bonds<\/button>\n      <button type=\"button\" data-step=\"3\" aria-pressed=\"false\"><span class=\"ctet-n\">3<\/span>109.5\u00b0 bond angles<\/button>\n      <button type=\"button\" data-step=\"4\" aria-pressed=\"false\"><span class=\"ctet-n\">4<\/span>Wedge and dash<\/button>\n    <\/div>\n  <\/div>\n\n  <div class=\"ctet-row\">\n    <span class=\"ctet-rowlab\">View<\/span>\n    <button type=\"button\" class=\"ctet-pill\" id=\"ctetResetV\">Reset view<\/button>\n  <\/div>\n<\/div>\n\n<div class=\"ctet-info\">\n  <h3 id=\"ctetInfoTitle\"><\/h3>\n  <p id=\"ctetInfoText\"><\/p>\n  <div class=\"ctet-facts\" id=\"ctetFacts\"><\/div>\n  <div class=\"ctet-key\">\n    <span><i class=\"k-ball\" style=\"background:#464a54\"><\/i>Carbon<\/span>\n    <span><i class=\"k-ball\" style=\"background:#ececf0\"><\/i>Hydrogen<\/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<\/span>\n  <\/div>\n<\/div>\n\n<script src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/JS\/ch4-tetrahedral.js?v=20261025p\"><\/script>\n<\/section>\n\n<p class=\"ols-cc-ctet-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-tetrahedral-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-tetrahedral-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-tetrahedral-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-tetrahedral-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-tetrahedral-molecular-shape-9ch0-page .ols-h5p-grid {\n    display: grid;\n    gap: 18px;\n    margin-top: 22px;\n  }\n  .ols-tetrahedral-molecular-shape-9ch0-page .ols-h5p-frame {\n    margin-top: 0;\n  }\n  .ols-tetrahedral-molecular-shape-9ch0-page .ols-formula {\n    white-space: nowrap;\n  }\n  @media (max-width: 760px) {\n    .ols-tetrahedral-molecular-shape-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: Flat Drawings and 3D Structures<\/h2>\n<p>Before you start, check what you remember about four bonds on one atom and about what a flat drawing can and cannot show.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"678\"><\/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 Tetrahedral Means<\/h2>\n        <\/div>\n        <p>A <strong>tetrahedral<\/strong> molecule has four atoms or groups arranged around a central atom in a three-dimensional shape. The four bonding regions point towards the corners of a tetrahedron.<\/p>\n        <p>The key example for this page is <strong>CH<sub>4<\/sub><\/strong>. Carbon is the central atom and each hydrogen atom is attached to carbon 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>4 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>109.5&deg; between each bond<\/span>\n          <\/div>\n        <\/div>\n\n        <div class=\"ols-key-box\"><p><strong>Key idea:<\/strong> four bonding regions and no lone pairs around a central atom give a tetrahedral shape with 109.5&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 CH<sub>4<\/sub> Is Tetrahedral<\/h2>\n        <\/div>\n        <p>In CH<sub>4<\/sub>, the central carbon atom is surrounded by four C-H bonding pairs. These bonding pairs are regions of negative charge, so they repel one another and move as far apart as possible.<\/p>\n        <p>With four equal bonding regions and no lone pairs, the maximum separation is achieved in three dimensions. This gives a <strong>tetrahedral<\/strong> arrangement with H-C-H bond angles of <strong>109.5&deg;<\/strong>.<\/p>\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-11-ch4-tetrahedral.svg\" alt=\"Tetrahedral CH\u2084 with wedge and hashed bonds and a 109.5\u00b0 angle, its dot-and-cross diagram, and NH\u2084\u207a drawn the same way\" class=\"ols-zoomable-img ols-lightbox-target\" draggable=\"false\" width=\"1520\" height=\"910\">\n          <\/div>\n          <div class=\"ols-zoom-card-caption\">\n            <p>A tetrahedral species has four bonding regions around the central atom and no lone pairs, giving a 109.5&deg; bond angle.<\/p>\n          <\/div>\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-25-countch4.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-25-countch4.jpg\" alt=\"Five-step electron-pair count for CH\u2084 giving four bonding regions and a tetrahedral 109.5\u00b0 shape, with NH\u2084\u207a as a second example\">\n<\/a>\n<\/div>\n<div class=\"ols-zoom-card-caption\"><p>Carbon has 4 outer electrons, all used in bonds: four regions and no lone pairs give a tetrahedral 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 Not Flat?<\/h2>\n<p>Drag the words and values into the gaps to explain why four bonding pairs do not lie in one plane.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-184\" class=\"h5p-iframe\" data-content-id=\"184\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Tetrahedral Drag: Why Silane Is Not a Flat Square\"><\/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>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 molecular shape question, each single bond counts as one bonding region. CH<sub>4<\/sub> has four bonding regions around carbon and no lone pair regions on carbon.<\/p>\n\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Feature<\/th>\n                <th>Tetrahedral value<\/th>\n                <th>Meaning in CH<sub>4<\/sub><\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Feature\">Number of bonding pairs<\/td>\n                <td data-label=\"Tetrahedral value\">4<\/td>\n                <td data-label=\"Meaning in CH4\">Four C-H 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=\"Tetrahedral value\">0<\/td>\n                <td data-label=\"Meaning in CH4\">No lone pair compression occurs, so the ideal tetrahedral angle is maintained.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Feature\">Bond angle<\/td>\n                <td data-label=\"Tetrahedral value\">109.5&deg;<\/td>\n                <td data-label=\"Meaning in CH4\">The four bonds are arranged as far apart as possible in three-dimensional space.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Feature\">Molecular shape<\/td>\n                <td data-label=\"Tetrahedral value\">Tetrahedral<\/td>\n                <td data-label=\"Meaning in CH4\">The surrounding atoms point towards the corners of a tetrahedron.<\/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-20-fourpairs.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-20-fourpairs.jpg\" alt=\"CH\u2084, NH\u2083 and H\u2082O ball sketches with angles 109.5\u00b0, 107\u00b0 and 104.5\u00b0, and the order of electron-pair repulsion\">\n<\/a>\n<\/div>\n<div class=\"ols-zoom-card-caption\"><p>Swapping a bonding pair for a lone pair closes the angle by about 2.5\u00b0 each time: 109.5\u00b0, 107\u00b0, 104.5\u00b0.<\/p><\/div>\n<\/div>\n<\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Count the Pairs<\/h2>\n<p>Work out the electron count for two species with four bonded atoms and type each answer.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-186\" class=\"h5p-iframe\" data-content-id=\"186\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Tetrahedral Flashcards: Counting Electron Pairs in BH\u2084\u207b and TeBr\u2084\"><\/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 Tetrahedral Species<\/h2>\n        <\/div>\n        <p>Several molecules and ions use the same four-region arrangement around the central atom. Other examples are <strong>SiCl<sub>4<\/sub><\/strong>, <strong>SO<sub>4<\/sub><sup>2-<\/sup><\/strong>, <strong>ClO<sub>4<\/sub><sup>&#8211;<\/sup><\/strong> and <strong>NH<sub>4<\/sub><sup>+<\/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\">CH<sub>4<\/sub><\/td>\n                <td data-label=\"Central atom\">C<\/td>\n                <td data-label=\"Electron regions\">4 bonding regions, 0 lone pairs<\/td>\n                <td data-label=\"Shape\">Tetrahedral<\/td>\n                <td data-label=\"Bond angle\">109.5&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">SiCl<sub>4<\/sub><\/td>\n                <td data-label=\"Central atom\">Si<\/td>\n                <td data-label=\"Electron regions\">4 bonding regions, 0 lone pairs<\/td>\n                <td data-label=\"Shape\">Tetrahedral<\/td>\n                <td data-label=\"Bond angle\">109.5&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">SO<sub>4<\/sub><sup>2-<\/sup><\/td>\n                <td data-label=\"Central atom\">S<\/td>\n                <td data-label=\"Electron regions\">4 bonding regions, 0 lone pairs<\/td>\n                <td data-label=\"Shape\">Tetrahedral<\/td>\n                <td data-label=\"Bond angle\">109.5&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">ClO<sub>4<\/sub><sup>&#8211;<\/sup><\/td>\n                <td data-label=\"Central atom\">Cl<\/td>\n                <td data-label=\"Electron regions\">4 bonding regions, 0 lone pairs<\/td>\n                <td data-label=\"Shape\">Tetrahedral<\/td>\n                <td data-label=\"Bond angle\">109.5&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">NH<sub>4<\/sub><sup>+<\/sup><\/td>\n                <td data-label=\"Central atom\">N<\/td>\n                <td data-label=\"Electron regions\">4 bonding regions, 0 lone pairs<\/td>\n                <td data-label=\"Shape\">Tetrahedral<\/td>\n                <td data-label=\"Bond angle\">109.5&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: Which Are Tetrahedral?<\/h2>\n<p>Count the electrons left over on each central atom, then click every species that is tetrahedral.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-185\" class=\"h5p-iframe\" data-content-id=\"185\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Tetrahedral Mark the Words: Which Species Are Tetrahedral?\"><\/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 Tetrahedral 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 CH<sub>4<\/sub>, the central atom is carbon.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>2. Count bonding pairs and lone pairs<\/h3>\n            <p>Carbon has four 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 four 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 tetrahedral with bond angles of 109.5&deg;.<\/p>\n          <\/div>\n        <\/div>\n\n        <div class=\"ols-definition-box\">\n          <p><strong>Exam answer model:<\/strong> CH<sub>4<\/sub> has four bonding pairs and no lone pairs around the central carbon atom. The bonding pairs repel equally and arrange themselves as far apart as possible in three-dimensional space. Therefore, CH<sub>4<\/sub> is tetrahedral with bond angles of 109.5&deg;.<\/p>\n        <\/div>\n      <\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Whose Reasoning Is Right?<\/h2>\n<p>In each round, choose the one student statement that an examiner would accept.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-187\" class=\"h5p-iframe\" data-content-id=\"187\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Tetrahedral Summary: Whose Reasoning Is Right?\"><\/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>Tetrahedral questions often test whether you can distinguish a four-domain arrangement from trigonal planar or shapes affected by lone pairs.<\/p>\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Do not write 120&deg;<\/h3>\n            <p>120&deg; is the trigonal planar angle. Tetrahedral species have four electron regions and an ideal angle of 109.5&deg;.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Do not flatten the shape<\/h3>\n            <p>Tetrahedral molecules are three-dimensional, not planar. Wedge and dashed bonds are often used to show this 3D arrangement.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Check for lone pairs<\/h3>\n            <p>Four bonding pairs and no lone pairs gives tetrahedral. If lone pairs are present, the molecular shape and bond angle may change.<\/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 tetrahedral shape is produced when a central atom has <strong>four bonding pairs<\/strong> and <strong>no lone pairs<\/strong>. The bonding pairs repel equally and spread out in three-dimensional space, giving <strong>109.5&deg;<\/strong> bond angles.<\/p>\n        <div class=\"ols-key-box\"><p><strong>Memory line:<\/strong> 4 bonding pairs + 0 lone pairs = tetrahedral = 109.5&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 tetrahedral molecular shape.<\/p>\n        <div class=\"ols-faq-list\">\n          <div class=\"ols-faq-item\">\n            <h3>What makes a molecule tetrahedral?<\/h3>\n            <p>A molecule is tetrahedral when the central atom has four bonding regions and no lone pairs. The bonding pairs repel equally and arrange themselves as far apart as possible in three-dimensional space.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Why is CH<sub>4<\/sub> tetrahedral?<\/h3>\n            <p>CH<sub>4<\/sub> has four C-H bonding pairs around the central carbon atom and no lone pairs on carbon. The four bonding pairs repel equally, so the molecule is tetrahedral with 109.5&deg; bond angles.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>What is the bond angle in a tetrahedral molecule?<\/h3>\n            <p>The ideal bond angle in a tetrahedral molecule is 109.5&deg;.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Is a tetrahedral molecule flat?<\/h3>\n            <p>No. A tetrahedral molecule is three-dimensional. The bonds point towards the corners of a tetrahedron rather than lying in one flat plane.<\/p>\n          <\/div>\n        \n<div class=\"ols-faq-item\">\n<h3>Is NH<sub>4<\/sub><sup>+<\/sup> tetrahedral even though it is an ion?<\/h3>\n<p>Yes. Nitrogen has 5 outer-shell electrons and the positive charge removes one, leaving 4 for four N-H bonds and no lone pairs. Four bonding pairs repel equally, so NH<sub>4<\/sub><sup>+<\/sup> is tetrahedral at 109.5&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          <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 tetrahedral 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 &amp; Structure<\/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\/trigonal-planar\/\">Trigonal Planar<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/trigonal-pyramidal\/\">Trigonal Pyramidal<\/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\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\/tetrahedral\/#webpage\",\n            \"url\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/tetrahedral\/\",\n            \"name\": \"Tetrahedral Molecular Shape | Edexcel A Level Chemistry\",\n            \"description\": \"A Level Chemistry revision notes explaining the tetrahedral molecular shape, CH4, electron-pair repulsion, four bonding pairs, no lone pairs and 109.5 degree bond angles.\",\n            \"isPartOf\": {\n                \"@type\": 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