{"id":4589,"date":"2026-05-30T06:12:53","date_gmt":"2026-05-30T05:12:53","guid":{"rendered":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/bent\/"},"modified":"2026-10-25T12:11:37","modified_gmt":"2026-10-25T12:11:37","slug":"bent","status":"publish","type":"page","link":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/bent\/","title":{"rendered":"Bent"},"content":{"rendered":"\n<section class=\"ols-revision-page ols-bent-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      --border: rgba(28, 36, 75, 0.14);\n      --shadow: 0 18px 45px rgba(28, 36, 75, 0.10);\n      --inner-shadow: 0 10px 26px rgba(28, 36, 75, 0.08);\n      font-family: Poppins, Arial, sans-serif;\n      color: var(--navy);\n      background: #ffffff;\n    }\n\n    .ols-revision-page * { box-sizing: border-box; }\n    .ols-main { min-width: 0; max-width: 970px; }\n    .ols-breadcrumbs { display: flex; flex-wrap: wrap; gap: 8px; margin: 10px 0 22px; font-size: 15px; color: var(--grey-text); }\n    .ols-breadcrumbs a, .ols-breadcrumbs span { color: var(--grey-text); text-decoration: none; font-weight: 600; }\n    .ols-breadcrumbs a:hover { color: var(--blue); text-decoration: underline; text-underline-offset: 3px; }\n    .ols-title-card, .ols-note-card, .ols-h5p-card, .ols-related-card, .ols-faq-card { background: #ffffff; border: 1px solid var(--border); border-radius: 28px; box-shadow: var(--shadow); padding: 34px; margin-bottom: 24px; overflow: hidden; }\n    .ols-title-card { background: linear-gradient(135deg, #ffffff 0%, #f8fbff 100%); }\n    .ols-title-card h1 { margin: 0 0 18px; font-size: clamp(36px, 5vw, 58px); line-height: 1.08; font-weight: 800; letter-spacing: -0.04em; color: #111827; }\n    .ols-page-intro { font-size: 19px; line-height: 1.7; font-weight: 300; color: var(--body-text); margin: 0 0 22px; }\n    .ols-badges { display: flex; flex-direction: column; align-items: flex-start; gap: 12px; margin-bottom: 22px; }\n    .ols-badge { display: inline-flex; align-items: center; padding: 9px 14px; border-radius: 999px; background: #ffffff; border: 1px solid var(--border); font-size: 15px; font-weight: 600; color: var(--navy); }\n    .ols-author { display: flex; align-items: center; gap: 20px; padding: 28px; border-radius: 28px; background: linear-gradient(135deg, #ffffff 0%, #f8fbff 100%); border: 1px solid rgba(28,36,75,0.12); box-shadow: 0 18px 45px rgba(28,36,75,0.10); margin-top: 22px; }\n    .ols-author-avatar-img { width: 92px; height: 92px; border-radius: 50%; object-fit: cover; object-position: center; flex-shrink: 0; border: 4px solid #ffffff; box-shadow: 0 14px 32px rgba(28,36,75,0.18), 0 0 0 1px rgba(28,36,75,0.10); transition: transform 0.25s ease, box-shadow 0.25s ease; }\n    .ols-author:hover .ols-author-avatar-img { transform: scale(1.04); box-shadow: 0 20px 42px rgba(28,36,75,0.22), 0 0 0 1px rgba(28,36,75,0.10); }\n    .ols-author-content { min-width: 0; }\n    .ols-author-title { margin: 0 0 4px; font-size: clamp(24px,3vw,34px); line-height: 1.15; font-weight: 700; color: var(--navy); letter-spacing: -0.03em; }\n    .ols-author-description { margin: 0; font-size: 17px; line-height: 1.7; font-weight: 300; color: var(--grey-text); }\n    .ols-linkedin-pill { display: inline-flex; align-items: center; justify-content: center; gap: 10px; margin-top: 16px; padding: 11px 18px; border-radius: 999px; background: linear-gradient(135deg,#0A66C2,#004182); color: #ffffff; text-decoration: none; font-size: 14px; line-height: 1; font-weight: 700; letter-spacing: 0.01em; box-shadow: 0 10px 22px rgba(10,102,194,0.24); position: relative; overflow: hidden; transition: transform 0.22s ease, box-shadow 0.22s ease; }\n    .ols-linkedin-pill::before { content: \"\"; position: absolute; top: 0; left: -120%; width: 100%; height: 100%; background: linear-gradient(120deg, rgba(255,255,255,0) 0%, rgba(255,255,255,0.28) 50%, rgba(255,255,255,0) 100%); transition: left 0.7s ease; }\n    .ols-linkedin-pill:hover { transform: translateY(-3px) scale(1.03); box-shadow: 0 16px 34px rgba(10,102,194,0.34), 0 0 0 6px rgba(10,102,194,0.10); color: #ffffff; }\n    .ols-linkedin-pill:hover::before { left: 120%; }\n    .ols-linkedin-icon { width: 18px; height: 18px; display: block; flex-shrink: 0; }\n    .ols-note-card.soft { background: linear-gradient(135deg, #ffffff 0%, var(--soft-red) 100%); }\n    .ols-note-card.purple { background: linear-gradient(135deg, #ffffff 0%, var(--soft-purple) 100%); }\n    .ols-note-card.orange { background: linear-gradient(135deg, #ffffff 0%, var(--soft-orange) 100%); }\n    .ols-note-title { display: flex; align-items: center; gap: 14px; margin-bottom: 20px; }\n    .ols-note-icon { width: 52px; height: 52px; border-radius: 16px; background: var(--navy); color: #ffffff; display: grid; place-items: center; font-size: 24px; font-weight: 800; flex-shrink: 0; }\n    .ols-note-title h2, .ols-h5p-card h2, .ols-related-card h2, .ols-faq-card h2 { margin: 0; font-size: clamp(28px, 3.5vw, 42px); line-height: 1.15; font-weight: 800; color: #111827; letter-spacing: -0.03em; }\n    .ols-h5p-card h2, .ols-related-card h2, .ols-faq-card h2 { margin-bottom: 14px; }\n    .ols-note-card p, .ols-note-card li { font-size: clamp(15px, 1.25vw, 17px); line-height: 1.65; font-weight: 300; color: var(--body-text); }\n    .ols-h5p-card p, .ols-related-card p, .ols-faq-card p { font-size: clamp(15px, 1.3vw, 18px); line-height: 1.65; font-weight: 300; color: var(--body-text); }\n    .ols-note-card strong, .ols-h5p-card strong, .ols-related-card strong, .ols-faq-card strong { font-weight: 700; color: var(--navy); }\n    .ols-note-card ul, .ols-note-card ol { margin: 0; padding-left: 22px; }\n    .ols-key-box { margin-top: 20px; background: var(--soft-green); border: 1px solid rgba(63, 143, 70, 0.25); border-radius: 20px; padding: 18px 20px; }\n    .ols-key-box p { margin: 0; font-weight: 400; color: var(--navy); }\n    .ols-definition-box { background: linear-gradient(135deg, #ffffff, var(--soft-purple)); border: 2px dashed rgba(122, 62, 157, 0.35); border-radius: 24px; padding: 22px 24px; margin-top: 22px; }\n    .ols-definition-box p { margin: 0; color: var(--navy); font-weight: 400; }\n    .ols-rule-list { display: grid; gap: 14px; margin-top: 18px; }\n    .ols-rule-item { background: #ffffff; border: 1px solid var(--border); border-left: 5px solid var(--blue); border-radius: 18px; padding: 18px; box-shadow: var(--inner-shadow); }\n    .ols-rule-item h3 { margin: 0 0 8px; font-size: 20px; line-height: 1.25; color: var(--navy); }\n    .ols-rule-item p { margin: 0; font-size: 15px; line-height: 1.6; }\n    .ols-zoom-card, .ols-zoom-card * { box-sizing: border-box; }\n    .ols-zoom-card { display: block !important; margin: 26px 0 34px !important; border: 1px solid rgba(28, 36, 75, 0.14) !important; border-radius: 26px !important; background: #ffffff !important; box-shadow: 0 18px 45px rgba(28, 36, 75, 0.10) !important; overflow: visible !important; position: relative !important; z-index: 1 !important; isolation: isolate !important; }\n    .ols-zoom-card.medium { max-width: 820px; margin-left: auto !important; margin-right: auto !important; }\n    .ols-zoom-card.compact { max-width: 700px; margin-left: auto !important; margin-right: auto !important; }\n    .ols-zoom-card:hover { z-index: 50 !important; }\n    .ols-zoom-card-image { display: flex !important; align-items: center !important; justify-content: center !important; width: 100% !important; min-height: 330px !important; padding: 20px !important; background: #ffffff !important; overflow: visible !important; border-top-left-radius: 26px !important; border-top-right-radius: 26px !important; position: relative !important; z-index: 2 !important; }\n    .ols-zoom-card img.ols-zoomable-img { display: block !important; width: 100% !important; max-width: 100% !important; height: auto !important; border-radius: 18px !important; cursor: default !important; pointer-events: auto !important; user-select: none !important; -webkit-user-drag: none !important; transform: translateZ(0) scale(1) !important; transform-origin: center center !important; transition: transform 0.32s ease, box-shadow 0.32s ease, filter 0.32s ease !important; position: relative !important; z-index: 2 !important; }\n    @media (hover: hover) and (pointer: fine) { .ols-zoom-card img.ols-zoomable-img:hover { transform: translateZ(0) scale(1.45) !important; box-shadow: 0 28px 70px rgba(28, 36, 75, 0.34) !important; filter: saturate(1.02) contrast(1.01) !important; z-index: 100 !important; } }\n    .ols-zoom-card-caption { padding: 18px 22px 20px !important; background: linear-gradient(135deg, #ffffff, #f8fbff) !important; border-bottom-left-radius: 26px !important; border-bottom-right-radius: 26px !important; position: relative !important; z-index: 1 !important; }\n    .ols-zoom-card-caption p { margin: 0 !important; color: #5f6b85 !important; font-size: 15px !important; line-height: 1.65 !important; font-weight: 300 !important; font-style: italic !important; font-family: Poppins, Arial, sans-serif !important; }\n    .ols-image-lightbox { position: fixed; inset: 0; z-index: 999999; display: none; align-items: center; justify-content: center; padding: 34px; background: rgba(10, 15, 35, 0.86); backdrop-filter: blur(8px); -webkit-backdrop-filter: blur(8px); }\n    .ols-image-lightbox.is-open { display: flex; }\n    .ols-image-lightbox-inner { position: relative; width: min(96vw, 1500px); max-height: 92vh; display: flex; align-items: center; justify-content: center; }\n    .ols-image-lightbox-img { display: block; max-width: 100%; max-height: 92vh; height: auto; width: auto; border-radius: 22px; background: #ffffff; box-shadow: 0 32px 90px rgba(0, 0, 0, 0.45); object-fit: contain; }\n    .ols-image-lightbox-close { position: absolute; top: -18px; right: -18px; width: 46px; height: 46px; border: 0; border-radius: 50%; background: #ffffff; color: var(--navy); font-family: Poppins, Arial, sans-serif; font-size: 28px; line-height: 1; font-weight: 700; cursor: pointer; box-shadow: 0 16px 34px rgba(0, 0, 0, 0.28); display: flex; align-items: center; justify-content: center; transition: transform 0.2s ease, background 0.2s ease, color 0.2s ease; }\n    .ols-image-lightbox-close:hover { transform: scale(1.08); background: var(--blue); color: #ffffff; }\n    .ols-zoom-card img.ols-lightbox-target { cursor: zoom-in !important; }\n    @media (max-width: 760px) { .ols-zoom-card { border-radius: 22px !important; overflow: hidden !important; } .ols-zoom-card-image { min-height: auto !important; padding: 12px !important; overflow: hidden !important; border-top-left-radius: 22px !important; border-top-right-radius: 22px !important; } .ols-zoom-card img.ols-zoomable-img, .ols-zoom-card img.ols-zoomable-img:hover { transform: none !important; box-shadow: none !important; } .ols-zoom-card-caption { border-bottom-left-radius: 22px !important; border-bottom-right-radius: 22px !important; } .ols-image-lightbox { padding: 16px; } .ols-image-lightbox-inner { width: 100%; max-height: 88vh; } .ols-image-lightbox-img { max-height: 88vh; border-radius: 16px; } .ols-image-lightbox-close { top: 10px; right: 10px; width: 42px; height: 42px; font-size: 26px; } }\n    .ols-table-wrap { overflow: hidden; border-radius: 22px; border: 1px solid var(--border); background: #ffffff; margin-top: 18px; }\n    .ols-table { width: 100%; border-collapse: collapse; table-layout: fixed; }\n    .ols-table th { background: var(--navy); color: #ffffff; padding: 16px; text-align: left; font-size: clamp(14px, 1.2vw, 17px); font-weight: 600; overflow-wrap: anywhere; }\n    .ols-table td { padding: 16px; border-bottom: 1px solid var(--border); font-size: clamp(14px, 1.15vw, 16px); line-height: 1.45; color: var(--body-text); vertical-align: top; overflow-wrap: anywhere; }\n    .ols-table tr:last-child td { border-bottom: none; }\n    .ols-h5p-card { background: linear-gradient(135deg, #ffffff 0%, #f7f0ff 100%); }\n    .ols-h5p-frame { margin-top: 22px; padding: 18px; border-radius: 24px; background: #ffffff; border: 1px solid var(--border); box-shadow: inset 0 0 0 1px rgba(28, 36, 75, 0.03); }\n    .ols-faq-list { display: grid; gap: 14px; margin-top: 18px; }\n    .ols-faq-item { background: #ffffff; border: 1px solid var(--border); border-radius: 18px; padding: 18px 20px; box-shadow: var(--inner-shadow); }\n    .ols-faq-item h3 { margin: 0 0 8px; font-size: 20px; line-height: 1.3; color: var(--navy); }\n    .ols-faq-item p { margin: 0; font-size: 16px; line-height: 1.65; color: var(--body-text); }\n    .ols-related-grid { display: grid; grid-template-columns: repeat(3, minmax(0, 1fr)); gap: 16px; margin-top: 18px; }\n    .ols-related-item { border: 1px solid var(--border); border-radius: 18px; padding: 18px; background: #ffffff; color: var(--navy); text-decoration: none; font-weight: 600; line-height: 1.5; transition: transform 0.2s ease, box-shadow 0.2s ease; }\n    .ols-related-item:hover { transform: translateY(-2px); box-shadow: 0 10px 22px rgba(28, 36, 75, 0.08); }\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-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    });\r\n\r\n    links.forEach(function(a) {\r\n      try {\r\n        var href = a.getAttribute('href');\r\n        if (!href || href === '#' || href.charAt(0) === '#') return;\r\n        var linkPath = normalisePath(new URL(href, window.location.origin).pathname);\r\n        if (!linkPath) return;\r\n        if (currentPath === linkPath || currentPath.indexOf(linkPath + '\/') === 0) {\r\n          if (linkPath.length > matchedLength) {\r\n            matched = a;\r\n            matchedLength = linkPath.length;\r\n          }\r\n        }\r\n      } catch(e) {}\r\n    });\r\n\r\n    if (matched) {\r\n      var matchedLi = matched.closest('li');\r\n      var parentSub = matched.closest('.ols-subtopic-list');\r\n\r\n      if (parentSub) {\r\n        if (matchedLi) {\r\n          matchedLi.classList.add('active');\r\n          matched.setAttribute('aria-current', 'page');\r\n        }\r\n        var parentLi = parentSub.closest('li');\r\n        if (parentLi) {\r\n          parentLi.classList.add('parent-active', 'active-main');\r\n          var parentLink = parentLi.querySelector(':scope > a');\r\n          if (parentLink) {\r\n            parentLink.setAttribute('aria-current', 'true');\r\n            parentLink.setAttribute('tabindex', '-1');\r\n            parentLink.setAttribute('data-ols-disabled-parent', '1');\r\n          }\r\n        }\r\n      } else {\r\n        if (matchedLi) {\r\n          matchedLi.classList.add('parent-active', 'active-main');\r\n          matched.setAttribute('aria-current', 'page');\r\n          matched.setAttribute('tabindex', '-1');\r\n          matched.setAttribute('data-ols-disabled-parent', '1');\r\n        }\r\n      }\r\n    }\r\n\r\n    return true;\r\n  }\r\n\r\n  if (!highlightActive()) {\r\n    document.addEventListener('DOMContentLoaded', highlightActive);\r\n  }\r\n})();\r\n<\/script>\n\n  <main class=\"ols-main\">\n      <nav class=\"ols-breadcrumbs\" aria-label=\"Breadcrumb\">\n        <a 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>Bent<\/span>\n      <\/nav>\n\n      <header class=\"ols-title-card\">\n        <h1>Bent Molecular Shape<\/h1>\n        <p class=\"ols-page-intro\">A focused revision guide to the bent molecular shape, using H<sub>2<\/sub>O as the key example. This page explains why two bonding pairs and two lone pairs around a central atom give a non-linear arrangement with a bond angle of about 104.5&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: h2o-bent (swapped 26 Sep 2026) -->\n<!-- Copyright (c) 2026 Dr. Mohammed Al-Fatah, onlinelearningsystem.net. All rights reserved. -->\n<!-- 3D card: h2o-bent (rebuilt Oct 2026) -->\n<!-- Copyright (c) 2026 Dr. Mohammed Al-Fatah, onlinelearningsystem.net. All rights reserved. -->\n<section class=\"ols-wbnt-001\" id=\"olsWbnt001\">\n<style>\n@import url('https:\/\/fonts.googleapis.com\/css2?family=Poppins:wght@300;400;500;600&display=swap');\n\n.ols-wbnt-001{\n  font-family:'Poppins',system-ui,-apple-system,'Segoe UI',Roboto,Helvetica,Arial,sans-serif;\n  color:#1C244B; background:#ffffff;\n  border:1px solid rgba(28,36,75,0.14);\n  border-radius:28px;\n  box-shadow:0 18px 45px rgba(28,36,75,0.10);\n  padding:44px; margin:26px auto; max-width:980px;\n  box-sizing:border-box; -webkit-font-smoothing:antialiased;\n}\n.ols-wbnt-001 *{box-sizing:border-box;}\n\n.ols-wbnt-001 .wbnt-head{margin:0 0 22px;}\n.ols-wbnt-001 h2.wbnt-title{\n  font-size:26px; line-height:1.25; font-weight:600; letter-spacing:-0.012em;\n  margin:0 0 9px; color:#1C244B;\n}\n.ols-wbnt-001 p.wbnt-sub{\n  font-size:14.5px; line-height:1.62; font-weight:300; color:#4a5270;\n  margin:0; max-width:66ch;\n}\n\n.ols-wbnt-001 .wbnt-stage{\n  position:relative; width:100%; height:540px;\n  background:#ffffff; border:1px solid rgba(28,36,75,0.12);\n  border-radius:18px; overflow:hidden;\n}\n.ols-wbnt-001 .wbnt-canvas{\n  display:block; width:100%; height:100%;\n  touch-action:none; cursor:grab; background:#ffffff;\n}\n.ols-wbnt-001 .wbnt-canvas.is-drag{cursor:grabbing;}\n.ols-wbnt-001 .wbnt-overlay{position:absolute; inset:0; pointer-events:none; overflow:hidden;}\n\n.ols-wbnt-001 .wbnt-lab{\n  position:absolute; left:0; top:0; transform:translate(-50%,-50%);\n  white-space:nowrap; font-size:12.5px; font-weight:500; line-height:1;\n  padding:5px 10px; background:rgba(255,255,255,0.93);\n  border:1px solid rgba(28,36,75,0.16); border-radius:999px;\n  color:#1C244B; will-change:transform;\n}\n.ols-wbnt-001 .wbnt-lab.l-part{font-size:11.5px; color:#3c4463;}\n.ols-wbnt-001 .wbnt-lab.l-msg{font-weight:600; border-color:rgba(28,36,75,0.32);}\n.ols-wbnt-001 .wbnt-lab.l-ok{font-weight:600; border-color:rgba(47,158,87,0.8); color:#1f7a3a;}\n.ols-wbnt-001 .wbnt-lab.l-bad{font-weight:600; border-color:rgba(212,58,50,0.7); color:#b02a24;}\n.ols-wbnt-001 .wbnt-lab.l-hi{font-weight:600; border-color:rgba(201,150,28,0.75); color:#8a6410;}\n.ols-wbnt-001 .wbnt-lab.l-blue{font-weight:600; border-color:rgba(70,125,190,0.55); color:#2f5f9a;}\n.ols-wbnt-001 .wbnt-lab.l-read{font-size:14px; font-weight:600; border-color:rgba(28,36,75,0.45); padding:6px 12px;}\n\n.ols-wbnt-001 .wbnt-caption .c-ok{color:#1f7a3a;}\n.ols-wbnt-001 .wbnt-caption .c-bad{color:#b02a24;}\n.ols-wbnt-001 .wbnt-caption .c-hi{color:#8a6410;}\n.ols-wbnt-001 .wbnt-caption{\n  position:absolute; left:14px; top:14px; max-width:60%;\n  font-size:12px; font-weight:500; color:#4a5270; line-height:1.35;\n  background:rgba(255,255,255,0.92); padding:6px 12px;\n  border-radius:14px; border:1px solid rgba(28,36,75,0.12);\n}\n.ols-wbnt-001 .wbnt-hint{\n  position:absolute; right:14px; top:14px;\n  font-size:11.5px; font-weight:400; color:#8b92a8;\n  background:rgba(255,255,255,0.9); padding:5px 11px;\n  border-radius:999px; border:1px solid rgba(28,36,75,0.10);\n}\n.ols-wbnt-001 .wbnt-badges{\n  position:absolute; right:14px; bottom:14px; max-width:58%;\n  display:flex; flex-direction:column; align-items:flex-end; gap:6px;\n}\n.ols-wbnt-001 .wbnt-badge{\n  font-size:12px; font-weight:500; color:#1C244B; line-height:1.35; text-align:right;\n  background:rgba(255,255,255,0.95); padding:5px 12px;\n  border-radius:14px; border:1px solid rgba(28,36,75,0.22);\n}\n.ols-wbnt-001 .wbnt-badge.b-eq{font-size:13.5px; font-weight:600; border-color:rgba(201,150,28,0.75);}\n\n.ols-wbnt-001 .wbnt-controls{margin-top:20px; display:flex; flex-direction:column; gap:12px;}\n.ols-wbnt-001 .wbnt-row{display:flex; align-items:center; gap:10px; flex-wrap:wrap;}\n.ols-wbnt-001 .wbnt-rowlab{font-size:12px; font-weight:500; color:#6b7290; min-width:100px; flex:0 0 auto;}\n\n.ols-wbnt-001 .wbnt-seg{\n  display:inline-flex; border:1px solid rgba(28,36,75,0.16);\n  border-radius:12px; overflow:hidden; background:#fbfbfd; flex-wrap:wrap;\n}\n.ols-wbnt-001 .wbnt-seg button{\n  font-family:inherit; font-size:14px; font-weight:500; color:#3c4463;\n  background:transparent; border:0; border-right:1px solid rgba(28,36,75,0.12);\n  padding:9px 18px; cursor:pointer; transition:background .15s, color .15s;\n}\n.ols-wbnt-001 .wbnt-seg button:last-child{border-right:0;}\n.ols-wbnt-001 .wbnt-seg button:hover{background:rgba(37,99,235,0.06);}\n.ols-wbnt-001 .wbnt-seg button[aria-pressed=\"true\"]{background:#2563eb; color:#fff;}\n.ols-wbnt-001 .wbnt-seg button:focus-visible{outline:2px solid #2563eb; outline-offset:-2px;}\n\n.ols-wbnt-001 .wbnt-pill{\n  font-family:inherit; font-size:13px; font-weight:500; color:#3c4463;\n  background:#fbfbfd; border:1px solid rgba(28,36,75,0.16);\n  border-radius:999px; padding:8px 16px; cursor:pointer;\n  display:inline-flex; align-items:center; gap:8px;\n  transition:background .15s, border-color .15s, color .15s;\n}\n.ols-wbnt-001 .wbnt-pill:hover{border-color:rgba(37,99,235,0.4);}\n.ols-wbnt-001 .wbnt-pill:focus-visible{outline:2px solid #2563eb; outline-offset:2px;}\n\n.ols-wbnt-001 .wbnt-info{\n  margin-top:22px; padding:22px 24px;\n  border:1px solid rgba(28,36,75,0.12); border-radius:16px; background:#fbfbfd;\n}\n.ols-wbnt-001 .wbnt-info h3{margin:0 0 8px; font-size:15.5px; font-weight:600; color:#1C244B;}\n.ols-wbnt-001 .wbnt-info p{margin:0; font-size:14px; line-height:1.68; font-weight:300; color:#41496a; max-width:74ch;}\n.ols-wbnt-001 .wbnt-facts{\n  margin-top:16px; display:flex; gap:26px; flex-wrap:wrap;\n  padding-top:16px; border-top:1px solid rgba(28,36,75,0.10);\n}\n.ols-wbnt-001 .wbnt-fact{min-width:110px;}\n.ols-wbnt-001 .wbnt-fact span{display:block; font-size:11.5px; color:#7d8399; font-weight:400; margin-bottom:3px;}\n.ols-wbnt-001 .wbnt-fact strong{display:block; font-size:15px; font-weight:600; color:#1C244B;}\n\n.ols-wbnt-001 .wbnt-key{\n  margin-top:16px; display:flex; gap:20px; flex-wrap:wrap;\n  font-size:12.5px; font-weight:400; color:#5a6180;\n}\n.ols-wbnt-001 .wbnt-key i{\n  display:inline-block; width:13px; height:13px; border-radius:3px;\n  margin-right:7px; vertical-align:-2px; border:1px solid rgba(28,36,75,0.18);\n}\n.ols-wbnt-001 .wbnt-key i.k-ball{border-radius:50%;}\n\n@media (max-width:760px){\n  .ols-wbnt-001{padding:26px; border-radius:22px;}\n  .ols-wbnt-001 h2.wbnt-title{font-size:20.5px;}\n  .ols-wbnt-001 p.wbnt-sub{font-size:13.5px;}\n  .ols-wbnt-001 .wbnt-stage{height:400px;}\n  .ols-wbnt-001 .wbnt-rowlab{min-width:100%;}\n  .ols-wbnt-001 .wbnt-seg button{padding:9px 13px; font-size:13px;}\n  .ols-wbnt-001 .wbnt-lab{font-size:10.5px; padding:4px 8px;}\n  .ols-wbnt-001 .wbnt-lab.l-part{font-size:9.5px; padding:3px 7px;}\n  .ols-wbnt-001 .wbnt-lab.l-read{font-size:12px; padding:5px 9px;}\n  .ols-wbnt-001 .wbnt-caption{font-size:10.5px; padding:5px 9px; max-width:64%;}\n  .ols-wbnt-001 .wbnt-badge{font-size:10.5px; padding:4px 9px;}\n  .ols-wbnt-001 .wbnt-badge.b-eq{font-size:11px;}\n  .ols-wbnt-001 .wbnt-badges{max-width:calc(100% - 28px);}\n  .ols-wbnt-001 .wbnt-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-wbnt-001 .wbnt-hint{display:none;}\n  .ols-wbnt-001 .wbnt-caption{max-width:calc(100% - 28px);}\n}\n@media (prefers-reduced-motion:reduce){\n  .ols-wbnt-001 .wbnt-seg button,.ols-wbnt-001 .wbnt-pill{transition:none;}\n}\n\n.ols-cc-wbnt-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-wbnt-001 a{color:#aab0c0; text-decoration:none;}\n.ols-cc-wbnt-001 a:hover{text-decoration:underline;}\n.ols-wbnt-001 .wbnt-seg button{display:inline-flex; align-items:center;}\n.ols-wbnt-001 .wbnt-seg button .wbnt-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-wbnt-001 .wbnt-seg button[aria-pressed=\"true\"] .wbnt-n{background:#ffffff; color:#2563eb;}\n<\/style>\n\n<div class=\"wbnt-head\">\n  <h2 class=\"wbnt-title\">Bent Shape of H\u2082O<\/h2>\n  <p class=\"wbnt-sub\">Choose a step to watch four electron pairs form a tetrahedron, two stay as lone pairs and close the bond angle to 104.5\u00b0.<\/p>\n<\/div>\n\n<div class=\"wbnt-stage\" id=\"wbntStage\">\n  <canvas class=\"wbnt-canvas\" id=\"wbntCanvas\"><\/canvas>\n  <div class=\"wbnt-overlay\" id=\"wbntOverlay\"><\/div>\n  <div class=\"wbnt-caption\" id=\"wbntCaption\"><\/div>\n  <div class=\"wbnt-hint\" id=\"wbntHint\">Drag to rotate<\/div>\n  <div class=\"wbnt-badges\" id=\"wbntBadges\"><\/div>\n<\/div>\n\n<div class=\"wbnt-controls\">\n  <div class=\"wbnt-row\">\n    <span class=\"wbnt-rowlab\">Step<\/span>\n    <div class=\"wbnt-seg\" role=\"group\" aria-label=\"Step\">\n      <button type=\"button\" data-step=\"1\" aria-pressed=\"true\"><span class=\"wbnt-n\">1<\/span>Four electron pairs<\/button>\n      <button type=\"button\" data-step=\"2\" aria-pressed=\"false\"><span class=\"wbnt-n\">2<\/span>Two lone pairs<\/button>\n      <button type=\"button\" data-step=\"3\" aria-pressed=\"false\"><span class=\"wbnt-n\">3<\/span>Squeezed to 104.5\u00b0<\/button>\n      <button type=\"button\" data-step=\"4\" aria-pressed=\"false\"><span class=\"wbnt-n\">4<\/span>Compare CH\u2084, NH\u2083, H\u2082O<\/button>\n    <\/div>\n  <\/div>\n\n  <div class=\"wbnt-row\">\n    <span class=\"wbnt-rowlab\">View<\/span>\n    <button type=\"button\" class=\"wbnt-pill\" id=\"wbntResetV\">Reset view<\/button>\n  <\/div>\n<\/div>\n\n<div class=\"wbnt-info\">\n  <h3 id=\"wbntInfoTitle\"><\/h3>\n  <p id=\"wbntInfoText\"><\/p>\n  <div class=\"wbnt-facts\" id=\"wbntFacts\"><\/div>\n  <div class=\"wbnt-key\">\n    <span><i class=\"k-ball\" style=\"background:#d6342c\"><\/i>Oxygen<\/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=\"\" style=\"background:rgba(128,92,214,0.5)\"><\/i>Lone pair<\/span>\n    <span><i class=\"k-ball\" style=\"background:#fac828\"><\/i>Electron<\/span>\n    <span><i class=\"\" style=\"background:#c9961c\"><\/i>Bond angle<\/span>\n  <\/div>\n<\/div>\n\n<script src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/JS\/h2o-bent.js?v=20261025p\"><\/script>\n<\/section>\n\n<p class=\"ols-cc-wbnt-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-bent-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-bent-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-bent-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-bent-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-bent-molecular-shape-9ch0-page .ols-h5p-grid {\n    display: grid;\n    gap: 18px;\n    margin-top: 22px;\n  }\n  .ols-bent-molecular-shape-9ch0-page .ols-h5p-frame {\n    margin-top: 0;\n  }\n  .ols-bent-molecular-shape-9ch0-page .ols-formula {\n    white-space: nowrap;\n  }\n  @media (max-width: 760px) {\n    .ols-bent-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: Shared Pairs and Lone Pairs<\/h2>\n<p>Before you start, check that you can count shared pairs and lone pairs in a dot-and-cross diagram.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"663\"><\/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 Bent Means<\/h2>\n        <\/div>\n        <p>A <strong>bent<\/strong> molecule has two atoms bonded to a central atom, with two lone pairs also present on the central atom. The bonded atoms are not arranged in a straight line because the lone pairs repel the bonding pairs and compress the bond angle.<\/p>\n        <p>The key example for this page is <strong>H<sub>2<\/sub>O<\/strong>. Oxygen is the central atom, each hydrogen atom is bonded to oxygen, and oxygen also has two lone pairs.<\/p>\n\n        <div class=\"ols-spec-grid\">\n          <div class=\"ols-spec-box\">\n            <strong>Bonding pairs<\/strong>\n            <span>2 bonding pairs around the central atom<\/span>\n          <\/div>\n          <div class=\"ols-spec-box\">\n            <strong>Lone pairs<\/strong>\n            <span>2 lone pairs on the central atom<\/span>\n          <\/div>\n          <div class=\"ols-spec-box\">\n            <strong>Bond angle<\/strong>\n            <span>about 104.5&deg; between the bonds<\/span>\n          <\/div>\n        <\/div>\n\n        <div class=\"ols-key-box\"><p><strong>Key idea:<\/strong> two bonding pairs and two lone pairs around a central atom give a bent shape with a bond angle of about 104.5&deg;.<\/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 H<sub>2<\/sub>O Is Bent<\/h2>\n        <\/div>\n        <p>In H<sub>2<\/sub>O, the central oxygen atom is surrounded by two O-H bonding pairs and two lone pairs. These four regions of negative charge repel one another and are based on a tetrahedral electron-pair arrangement.<\/p>\n        <div class=\"ols-key-box\"><p><strong>How to count:<\/strong><\/p>\n<ol>\n<li>Start with the <strong>outer-shell electrons<\/strong> of the central atom.<\/li>\n<li>Add one electron for each negative charge and take one away for each positive charge.<\/li>\n<li>Each single bond uses one of those electrons and each double bond uses two. A double or triple bond still counts as <strong>one bonding region<\/strong>.<\/li>\n<li>Divide the electrons left over by two to get the lone pairs.<\/li>\n<\/ol>\n<p>In H<sub>2<\/sub>O: oxygen has <strong>6 outer-shell electrons<\/strong>, the molecule has no charge, and the two O-H single bonds use two of them. Four are left over, which is two lone pairs.<\/p>\n<p>Two bonding regions and two lone pairs give four regions, so the arrangement is tetrahedral and the shape is bent. The same count works for an ion once the charge has been added or taken away.<\/p><\/div>\n        <p>The <strong>molecular shape<\/strong> only considers the positions of the atoms, not the invisible lone pairs. Therefore, H<sub>2<\/sub>O is described as <strong>bent<\/strong>, not tetrahedral.<\/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-13-h2o-bent.svg\" alt=\"Bent H\u2082O with two lone-pair lobes and a 104.5\u00b0 angle, beside its dot-and-cross diagram\" class=\"ols-zoomable-img ols-lightbox-target\" draggable=\"false\" width=\"1520\" height=\"918\">\n          <\/div>\n          <div class=\"ols-zoom-card-caption\">\n            <p>A bent species has two bonding regions and two lone pairs around the central atom. H<sub>2<\/sub>O is the key model example, with a bond angle of about 104.5&deg;.<\/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-27-counth2o.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-27-counth2o.jpg\" alt=\"Five-step electron-pair count for H\u2082O giving two bonding pairs, two lone pairs and a bent 104.5\u00b0 shape\">\n<\/a>\n<\/div>\n<div class=\"ols-zoom-card-caption\"><p>Oxygen keeps 4 of its 6 outer electrons as two lone pairs: two bonding regions and two lone pairs give a bent 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: Count the Pairs in Hydrogen Selenide<\/h2>\n<p>Apply the same reasoning to a molecule that is not on this page, answering each question as quickly as you can.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-193\" class=\"h5p-iframe\" data-content-id=\"193\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Bent Shape Quick Fire: Counting the Electron Pairs in Hydrogen Selenide\"><\/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 four electron regions around oxygen in H<sub>2<\/sub>O are arranged to minimise repulsion. If all four regions were bonding pairs, the bond angle would be close to the tetrahedral angle of 109.5&deg;.<\/p>\n        <p>However, H<sub>2<\/sub>O has two lone pairs. Lone pair-lone pair repulsion is stronger than lone pair-bonding pair repulsion, which is stronger than bonding pair-bonding pair repulsion. This stronger repulsion compresses the H-O-H bond angle to about 104.5&deg;.<\/p>\n        <div class=\"ols-rule-list\">\n          <div class=\"ols-rule-item\">\n            <h3>Bonding pair-bonding pair<\/h3>\n            <p>Weakest repulsion of the three common repulsion types.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Lone pair-bonding pair<\/h3>\n            <p>Stronger repulsion, so bond angles are compressed.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Lone pair-lone pair<\/h3>\n            <p>Strongest repulsion. NH<sub>3<\/sub> has one lone pair and a bond angle of <strong>107&deg;<\/strong>, while H<sub>2<\/sub>O has two and closes to about <strong>104.5&deg;<\/strong>. As a rule of thumb, each lone pair takes about 2.5&deg; off the tetrahedral angle of 109.5&deg;.<\/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-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: Rank the Bond Angles<\/h2>\n<p>Drag the four fluorides into order of bond angle, largest at the top.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-194\" class=\"h5p-iframe\" data-content-id=\"194\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Bent Shape Sort: Ranking Four Fluorides by Bond Angle\"><\/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>Bent Shape Examples<\/h2>\n        <\/div>\n        <p>The bent shape is found when the central atom has two bonding pairs and two lone pairs. H<sub>2<\/sub>O is the standard example used to explain the 104.5&deg; bond angle.<\/p>\n        <p>The last column gives the angle <strong>predicted<\/strong> at A Level, which is what mark schemes expect. Measured angles vary around it, and H<sub>2<\/sub>S is actually about 92&deg;. Quote about 104.5&deg; unless a question gives you a value to use.<\/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>Angle predicted at A Level<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Species\">H<sub>2<\/sub>O<\/td>\n                <td data-label=\"Central atom\">O<\/td>\n                <td data-label=\"Electron regions\">2 bonding regions, 2 lone pairs<\/td>\n                <td data-label=\"Shape\">Bent<\/td>\n                <td data-label=\"Angle predicted at A Level\">about 104.5&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">OCl<sub>2<\/sub><\/td>\n                <td data-label=\"Central atom\">O<\/td>\n                <td data-label=\"Electron regions\">2 bonding regions, 2 lone pairs<\/td>\n                <td data-label=\"Shape\">Bent<\/td>\n                <td data-label=\"Angle predicted at A Level\">about 104.5&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">H<sub>2<\/sub>S<\/td>\n                <td data-label=\"Central atom\">S<\/td>\n                <td data-label=\"Electron regions\">2 bonding regions, 2 lone pairs<\/td>\n                <td data-label=\"Shape\">Bent<\/td>\n                <td data-label=\"Angle predicted at A Level\">about 104.5&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">OF<sub>2<\/sub><\/td>\n                <td data-label=\"Central atom\">O<\/td>\n                <td data-label=\"Electron regions\">2 bonding regions, 2 lone pairs<\/td>\n                <td data-label=\"Shape\">Bent<\/td>\n                <td data-label=\"Angle predicted at A Level\">about 104.5&deg;<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Species\">SCl<sub>2<\/sub><\/td>\n                <td data-label=\"Central atom\">S<\/td>\n                <td data-label=\"Electron regions\">2 bonding regions, 2 lone pairs<\/td>\n                <td data-label=\"Shape\">Bent<\/td>\n                <td data-label=\"Angle predicted at A Level\">about 104.5&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: Find the Bent Species<\/h2>\n<p>Count the electron pairs around each central atom and click every species with two bonding pairs and two lone pairs.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-192\" class=\"h5p-iframe\" data-content-id=\"192\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Bent Shape Mark the Words: Which Species Have Two Bonding Pairs and Two Lone Pairs?\"><\/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 Bent Shape in an Exam<\/h2>\n        <\/div>\n        <p>A full exam explanation should connect the number of electron pairs to electron-pair repulsion, then explain why the bond angle is smaller than the tetrahedral 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 H<sub>2<\/sub>O, the central atom is oxygen.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>2. Count bonding pairs and lone pairs<\/h3>\n            <p>Oxygen has two bonding pairs and two lone pairs around it.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>3. Apply electron-pair repulsion<\/h3>\n            <p>The electron pairs repel and arrange themselves as far apart as possible, but the two lone pairs repel more strongly than bonding pairs.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>4. State the shape and angle<\/h3>\n            <p>The molecule is bent with a bond angle of about 104.5&deg;.<\/p>\n          <\/div>\n        <\/div>\n\n        <div class=\"ols-definition-box\">\n          <p><strong>Exam answer model:<\/strong> H<sub>2<\/sub>O has two bonding pairs and two lone pairs around the central oxygen atom. The electron pairs repel and arrange themselves as far apart as possible.<\/p>\n<p>The two lone pairs repel the bonding pairs more strongly, compressing the H-O-H bond angle from 109.5&deg; to about 104.5&deg;. Therefore, H<sub>2<\/sub>O is bent.<\/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: Explain the Amide Ion<\/h2>\n<p>Write a short exam-style 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-195\" class=\"h5p-iframe\" data-content-id=\"195\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Bent Shape Explain: Shape and Bond Angle of the Amide Ion\"><\/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: Whose Reasoning Is Sound?<\/h2>\n<p>In each round, choose the one student whose reasoning is correct.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-664\" class=\"h5p-iframe\" data-content-id=\"664\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Bent Shape 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 call H<sub>2<\/sub>O linear<\/h3>\n            <p>Although there are only two bonded atoms, the two lone pairs on oxygen bend the molecule.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Separate electron-pair arrangement from molecular shape<\/h3>\n            <p>The electron-pair arrangement is based on tetrahedral geometry, but the molecular shape is bent because only atoms are used to describe the visible shape.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Use the correct repulsion order<\/h3>\n            <p>Lone pair-lone pair repulsion is strongest, followed by lone pair-bonding pair, then bonding pair-bonding pair.<\/p>\n          <\/div>\n          <div class=\"ols-rule-item\">\n            <h3>Count around the central atom only<\/h3>\n            <p>The shape is determined by the bonding pairs and lone pairs around the central atom, not by the total number of atoms in the whole species.<\/p>\n          <\/div>\n        <\/div>\n      <\/article>\n\n      \n\n      <article class=\"ols-note-card purple\">\n        <div class=\"ols-note-title\">\n          <div class=\"ols-note-icon\">\u2713<\/div>\n          <h2>QuickSnap<\/h2>\n        <\/div>\n        <p>The bent shape is produced when a central atom has <strong>two bonding pairs<\/strong> and <strong>two lone pairs<\/strong>. The lone pairs repel bonding pairs more strongly and compress the bond angle to about <strong>104.5&deg;<\/strong>.<\/p>\n        <div class=\"ols-key-box\"><p><strong>Memory line:<\/strong> 2 bonding pairs + 2 lone pairs = bent = about 104.5&deg;.<\/p><\/div>\n      <\/article>\n\n      <section class=\"ols-faq-card\">\n        <h2>FAQs<\/h2>\n        <p>These are the key questions students often ask when revising the bent molecular shape.<\/p>\n        <div class=\"ols-faq-list\">\n          <div class=\"ols-faq-item\">\n            <h3>What makes a molecule bent?<\/h3>\n            <p>A molecule is bent when the central atom has two bonded atoms and lone pairs that repel the bonding pairs. In the standard H<sub>2<\/sub>O example, oxygen has two bonding pairs and two lone pairs.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Why is H<sub>2<\/sub>O bent?<\/h3>\n            <p>H<sub>2<\/sub>O is bent because oxygen has two O-H bonding pairs and two lone pairs. The lone pairs occupy electron regions but are not shown as atoms in the molecular shape.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>What is the bond angle in H<sub>2<\/sub>O?<\/h3>\n            <p>The H-O-H bond angle in H<sub>2<\/sub>O is about 104.5&deg;. It is smaller than 109.5&deg; because the two lone pairs repel bonding pairs more strongly.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Is bent the same as linear?<\/h3>\n            <p>No. A linear molecule has a bond angle of 180&deg;. A bent molecule has a smaller bond angle because lone pairs on the central atom repel the bonding pairs.<\/p>\n          <\/div>\n        \n<div class=\"ols-faq-item\">\n<h3>Why is the bond angle in H<sub>2<\/sub>O smaller than in NH<sub>3<\/sub>?<\/h3>\n<p>H<sub>2<\/sub>O has two lone pairs and NH<sub>3<\/sub> has one. Lone pair-lone pair repulsion is the strongest, so the bonding pairs in water are pushed closer together: about 104.5&deg; against 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          <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 linked revision pages to connect bent 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\/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\/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\/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\/bent\/#webpage\",\n            \"url\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/bent\/\",\n            \"name\": \"Bent Molecular Shape | Edexcel A Level Chemistry\",\n            \"description\": \"Revision notes explaining bent molecular shape using H2O, including two bonding pairs, two lone pairs, lone-pair repulsion and the 104.5 degree bond angle.\",\n            \"isPartOf\": {\n                \"@type\": \"WebSite\",\n                \"@id\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/#website\",\n                \"name\": \"Online Learning System\",\n                \"url\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/\"\n            },\n            \"about\": [\n                {\n                    \"@type\": \"Thing\",\n                    \"name\": \"Bent molecular shape\"\n                },\n                {\n                    \"@type\": \"Thing\",\n                    \"name\": \"Electron-pair repulsion theory\"\n                },\n                {\n                    \"@type\": \"Thing\",\n                    \"name\": \"Water molecular shape\"\n                }\n            ],\n            \"educationalLevel\": \"A Level\",\n            \"learningResourceType\": \"Revision notes\",\n            \"inLanguage\": \"en-GB\"\n        },\n        {\n            \"@type\": \"Person\",\n            \"@id\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/#dr-mohammed-al-fatah\",\n            \"name\": \"Dr. Mohammed Al-Fatah\",\n            \"url\": \"https:\/\/www.linkedin.com\/in\/doctormohammedfatah\/\",\n            \"affiliation\": {\n                \"@type\": \"Organization\",\n                \"name\": \"Online Learning System\",\n                \"url\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/\"\n            }\n        },\n        {\n            \"@type\": \"BreadcrumbList\",\n            \"@id\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/bent\/#breadcrumb\",\n            \"itemListElement\": [\n                {\n                    \"@type\": \"ListItem\",\n                    \"position\": 1,\n                    \"name\": \"Revision Notes\",\n                    \"item\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/\"\n                },\n                {\n                    \"@type\": \"ListItem\",\n                    \"position\": 2,\n                    \"name\": \"A Level Chemistry\",\n                    \"item\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/\"\n                },\n                {\n                    \"@type\": \"ListItem\",\n                    \"position\": 3,\n                    \"name\": \"Edexcel\",\n                    \"item\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/\"\n                },\n                {\n                    \"@type\": \"ListItem\",\n                    \"position\": 4,\n                    \"name\": \"Topic 2 Bonding and Structure\",\n                    \"item\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/\"\n                },\n                {\n                    \"@type\": \"ListItem\",\n                    \"position\": 5,\n                    \"name\": \"Shapes of Molecules\",\n                    \"item\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/\"\n                },\n                {\n                    \"@type\": \"ListItem\",\n                    \"position\": 6,\n                    \"name\": \"Bent\",\n                    \"item\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/bent\/\"\n                }\n            ]\n        },\n        {\n            \"@type\": \"Course\",\n            \"@id\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/product\/covalent-bonding-shapes-of-molecules-edexcel-t2ab\/#course\",\n            \"name\": \"Covalent Bonding, Structure and Shapes of Molecules\",\n            \"description\": \"A paid OLS course covering covalent bonding, structure, molecular shapes, electron-pair repulsion, bond angles and exam-style practice for Edexcel A Level Chemistry.\",\n            \"provider\": {\n                \"@type\": \"Organization\",\n                \"name\": \"Online Learning System\",\n                \"sameAs\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/\"\n            },\n            \"url\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/product\/covalent-bonding-shapes-of-molecules-edexcel-t2ab\/\"\n        },\n        {\n            \"@type\": \"ImageObject\",\n            \"@id\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/skel-54-water-bent.svg#image\",\n            \"url\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/skel-54-water-bent.svg\",\n            \"caption\": \"Bent molecular shape table entry showing two bonding pairs, two lone pairs and a bond angle of about 104.5 degrees.\"\n        },\n        {\n            \"@type\": \"FAQPage\",\n            \"@id\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel\/topic-2-bonding-and-structure\/shapes-of-molecules\/bent\/#faq\",\n            \"mainEntity\": [\n                {\n                    \"@type\": \"Question\",\n                    \"name\": \"What makes a molecule bent?\",\n                    \"acceptedAnswer\": {\n                        \"@type\": \"Answer\",\n                        \"text\": \"A molecule is bent when the central atom has two bonded atoms and lone pairs that repel the bonding pairs. In the standard H2O example, oxygen has two bonding pairs and two lone pairs.\"\n                    }\n                },\n                {\n                    \"@type\": \"Question\",\n                    \"name\": \"Why is H2O bent?\",\n                    \"acceptedAnswer\": {\n                        \"@type\": \"Answer\",\n                        \"text\": \"H2O is bent because oxygen has two O-H bonding pairs and two lone pairs. The lone pairs occupy electron regions but are not shown as atoms in the molecular shape.\"\n                    }\n                },\n                {\n                    \"@type\": \"Question\",\n                    \"name\": \"What is the bond angle in H2O?\",\n                    \"acceptedAnswer\": {\n                        \"@type\": \"Answer\",\n                        \"text\": \"The H-O-H bond angle in H2O is about 104.5\u00b0. It is smaller than 109.5\u00b0 because the two lone pairs repel bonding pairs more strongly.\"\n                    }\n                },\n                {\n                    \"@type\": \"Question\",\n                    \"name\": \"Is bent the same as linear?\",\n                    \"acceptedAnswer\": {\n                        \"@type\": \"Answer\",\n                        \"text\": \"No. A linear molecule has a bond angle of 180\u00b0. A bent molecule has a smaller bond angle because lone pairs on the central atom repel the bonding pairs.\"\n                    }\n                },\n                {\n                    \"@type\": \"Question\",\n                    \"name\": \"Why is the bond angle in H2O smaller than in NH3?\",\n                    \"acceptedAnswer\": {\n                        \"@type\": \"Answer\",\n                        \"text\": \"H2O has two lone pairs and NH3 has one. Lone pair-lone pair repulsion is the strongest, so the bonding pairs in water are pushed closer together: about 104.5\u00b0 against 107\u00b0.\"\n                    }\n                }\n            ]\n        }\n    ]\n}\n<\/script>\n\n      <div class=\"ols-image-lightbox\" id=\"olsImageLightboxBent9ch0\" aria-hidden=\"true\" role=\"dialog\" aria-modal=\"true\" aria-label=\"Expanded revision image\">\n        <div class=\"ols-image-lightbox-inner\">\n          <button class=\"ols-image-lightbox-close\" type=\"button\" aria-label=\"Close enlarged image\">\u00d7<\/button>\n          <img decoding=\"async\" class=\"ols-image-lightbox-img\" src=\"\" alt=\"\">\n        <\/div>\n      <\/div>\n\n      <script>\n        (function(){\n          var page = document.querySelector(\".ols-bent-molecular-shape-9ch0-page\");\n          if (!page) {\n            return;\n          }\n\n          var lightbox = page.querySelector(\"#olsImageLightboxBent9ch0\");\n          if (!lightbox) {\n            return;\n          }\n\n          var lightboxImage = lightbox.querySelector(\".ols-image-lightbox-img\");\n          var closeButton = lightbox.querySelector(\".ols-image-lightbox-close\");\n          var clickableImages = page.querySelectorAll(\"img.ols-lightbox-target\");\n\n          function openLightbox(image) {\n            lightboxImage.src = image.currentSrc || image.src;\n            lightboxImage.alt = image.alt || \"Expanded revision image\";\n            lightbox.classList.add(\"is-open\");\n            lightbox.setAttribute(\"aria-hidden\", \"false\");\n\n            if (!document.body.dataset.olsPreviousOverflow) {\n              document.body.dataset.olsPreviousOverflow = document.body.style.overflow || \"default\";\n            }\n\n            document.body.style.overflow = \"hidden\";\n          }\n\n          function closeLightbox() {\n            lightbox.classList.remove(\"is-open\");\n            lightbox.setAttribute(\"aria-hidden\", \"true\");\n            lightboxImage.src = \"\";\n\n            if (document.body.dataset.olsPreviousOverflow) {\n              document.body.style.overflow = document.body.dataset.olsPreviousOverflow === \"default\" ? \"\" : document.body.dataset.olsPreviousOverflow;\n              delete document.body.dataset.olsPreviousOverflow;\n            }\n          }\n\n          clickableImages.forEach(function(image){\n            image.addEventListener(\"click\", function(event){\n              event.preventDefault();\n              event.stopPropagation();\n              openLightbox(image);\n            });\n          });\n\n          closeButton.addEventListener(\"click\", closeLightbox);\n\n          lightbox.addEventListener(\"click\", function(event){\n            if (event.target === lightbox) {\n              closeLightbox();\n            }\n          });\n\n          document.addEventListener(\"keydown\", function(event){\n            if (event.key === \"Escape\" && lightbox.classList.contains(\"is-open\")) {\n              closeLightbox();\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 \/ Bent Bent Molecular Shape A focused revision guide to the bent molecular shape, using H2O as the key example. This page explains why two bonding pairs and two lone pairs around a central atom give a [&hellip;]<\/p>\n","protected":false},"author":12,"featured_media":0,"parent":4572,"menu_order":4,"comment_status":"closed","ping_status":"closed","template":"","meta":{"footnotes":""},"class_list":["post-4589","page","type-page","status-publish","hentry"],"_links":{"self":[{"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages\/4589","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=4589"}],"version-history":[{"count":2,"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages\/4589\/revisions"}],"predecessor-version":[{"id":24670,"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages\/4589\/revisions\/24670"}],"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=4589"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}