{"id":10967,"date":"2026-09-26T22:00:21","date_gmt":"2026-09-26T21:00:21","guid":{"rendered":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-2-2-haloalkanes\/halogenoalkanes-naming-classification-and-bonding\/"},"modified":"2026-09-27T10:01:35","modified_gmt":"2026-09-27T09:01:35","slug":"halogenoalkanes-naming-classification-and-bonding","status":"publish","type":"page","link":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-2-2-haloalkanes\/halogenoalkanes-naming-classification-and-bonding\/","title":{"rendered":"Haloalkanes: Naming, Classification and the C\u2013X Bond"},"content":{"rendered":"<script src=\"https:\/\/cdnjs.cloudflare.com\/ajax\/libs\/three.js\/r128\/three.min.js\"><\/script>\n\n<section class=\"ols-revision-page ols-nature-of-covalent-bonding-9ch0-page\">\n  <style>\n    .ols-revision-page {\n      --navy: #1C244B;\n      --blue: #2563eb;\n      --soft-blue: #eef4ff;\n      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!important; min-height: 240px !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; max-width: 100% !important; height: auto !important; border-radius: 18px !important; cursor: zoom-in !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(1.35) !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    @media (max-width: 760px) { .ols-zoom-card { border-radius: 22px !important; overflow: hidden !important; } .ols-zoom-card-image { 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.ols-course-cta-image-link:hover .ols-course-cta-image img { transform: scale(1.03); }\n    .ols-course-cta-header-row { display: flex; flex-wrap: wrap; align-items: center; justify-content: space-between; gap: 14px; margin-bottom: 18px; }\n    .ols-course-cta-kicker { display: inline-flex; align-items: center; padding: 8px 14px; border-radius: 999px; background: #ffffff; border: 1px solid rgba(37, 99, 235, 0.18); color: var(--blue); font-size: 14px; line-height: 1.2; font-weight: 700; box-shadow: var(--inner-shadow); }\n    .ols-course-cta-covalent h2 { margin: 0 0 14px; font-size: clamp(28px, 3.5vw, 42px); line-height: 1.15; font-weight: 800; letter-spacing: -0.03em; color: #111827; }\n    .ols-course-cta-intro { margin: 0 0 24px; color: var(--body-text); font-size: clamp(16px, 1.4vw, 18px); line-height: 1.7; font-weight: 300; }\n    .ols-course-cta-features { display: grid; grid-template-columns: repeat(2, minmax(0, 1fr)); gap: 14px; margin: 0 0 30px; }\n    .ols-course-feature { 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99, 235, 0.24); }\n    .ols-course-button-top { flex-shrink: 0; padding: 12px 22px; font-size: 15px; }\n\n    .ols-attribution-card {\n      background: linear-gradient(135deg, #ffffff, #f8fbff);\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: 34px;\n      margin-bottom: 24px;\n      overflow: hidden;\n      font-family: Poppins, Arial, sans-serif;\n      box-sizing: border-box;\n    }\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      .ols-course-cta-top { grid-template-columns: 1fr; }\n      .ols-course-cta-image-link { max-width: 520px; margin: 0 auto; }\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-related-grid, .ols-course-cta-features { grid-template-columns: 1fr; }\n      .ols-figure-card { border-radius: 22px; }\n      .ols-figure-image { min-height: 210px; padding: 14px; }\n      .ols-figure-caption { padding: 16px; }\n      .ols-table-wrap { border: none; background: transparent; }\n      .ols-table, .ols-table thead, .ols-table tbody, .ols-table th, .ols-table td, .ols-table tr { display: block; width: 100%; }\n      .ols-table { border-collapse: separate; border-spacing: 0; }\n      .ols-table thead { display: none; }\n      .ols-table tr { margin-bottom: 14px; border: 1px solid var(--border); border-radius: 18px; overflow: hidden; background: #ffffff; box-shadow: 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text-transform: uppercase; }\n    .ols-h5p-card.ols-h5p-recap { border-left-color: #c9973a; background: linear-gradient(135deg, #ffffff 0%, #fff8e8 100%); }\n    .ols-h5p-recap .ols-h5p-kicker { background: #fdf0d2; color: #8a5a00; }\n    @media (max-width: 760px) { .ols-h5p-card.ols-h5p-inline { padding: 20px 16px; } }\n<\/style>\n\n  <aside class=\"ols-sidebar\">\n  <div class=\"ols-sidebar-header\">\n    <h3>Revision Notes<\/h3>\n    <p>A Level Chemistry<\/p>\n  <\/div>\n\n  <div class=\"ols-topic-group\">\n    <h4>4.2.2 Haloalkanes<\/h4>\n\n    <ul class=\"ols-topic-list\">\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-2-2-haloalkanes\/\">4.2.2 Overview<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-2-2-haloalkanes\/reaction-types-mechanisms-and-nucleophiles\/\">Reaction Types, Mechanisms and Nucleophiles<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-2-2-haloalkanes\/halogenoalkanes-naming-classification-and-bonding\/\">Haloalkanes: Naming, Classification and the C\u2013X Bond<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-2-2-haloalkanes\/nucleophilic-substitution-reactions\/\">Nucleophilic Substitution Reactions<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-2-2-haloalkanes\/rates-of-hydrolysis-and-bond-enthalpy\/\">Rates of Hydrolysis and Bond Enthalpy<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-2-2-haloalkanes\/cfcs-and-the-ozone-layer\/\">CFCs and the Ozone Layer<\/a>\n      <\/li>\n    <\/ul>\n  <\/div>\n\n  <div class=\"ols-topic-group\">\n    <h4>Other Sections<\/h4>\n\n    <ul class=\"ols-topic-list\">\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-2-1-alcohols\/\">4.2.1 Alcohols<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-2-4-analytical-techniques\/\">4.2.4 Analytical Techniques<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-1-3-alkenes\/\">4.1.3 Alkenes<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-1-2-alkanes\/\">4.1.2 Alkanes<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-1-1-basic-concepts-of-organic-chemistry\/\">4.1.1 Basic Concepts of Organic 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{\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\/ocr-a\/\">OCR<\/a> \/\n<a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-2-2-haloalkanes\/\">4.2.2 Haloalkanes<\/a> \/\n<span>Haloalkanes: Naming, Classification and the C\u2013X Bond<\/span>\n<\/nav>\n\n      <header class=\"ols-title-card\">\n        <h1>Haloalkanes: Naming, Classification and the C\u2013X Bond<\/h1>\n        <p class=\"ols-page-intro\">A concise revision guide to haloalkanes: naming and drawing them, classifying them as primary, secondary or tertiary, the polarity and strength of the carbon\u2013halogen bond, and their properties and uses.<\/p>\n\n        <div class=\"ols-badges\">\n<div class=\"ols-badge\">Paper 2 and 3<\/div>\n<div class=\"ols-badge\">4.2.2: Haloalkanes<\/div>\n<div class=\"ols-badge\">H432\/02 and H432\/03<\/div>\n<\/div>\n\n        <div class=\"ols-author\">\n\n    <img decoding=\"async\"\n      class=\"ols-author-avatar-img\"\n      src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/05\/Author-Profile.jpeg\"\n      alt=\"Dr. Mohammed Al-Fatah\"\n    >\n\n    <div class=\"ols-author-content\">\n\n      <h2 class=\"ols-author-title\">\n        Written by:<br><span>Dr. Mohammed Al-Fatah<\/span>\n      <\/h2>\n\n      <p class=\"ols-author-description\">\n        Chemistry specialist revision notes for A Level Chemistry.\n      <\/p>\n\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\">\n          <path d=\"M4.98 3.5C4.98 4.88 3.86 6 2.48 6S0 4.88 0 3.5 1.12 1 2.48 1s2.5 1.12 2.5 2.5zM.5 8h4V24h-4V8zm7 0h3.8v2.2h.1c.5-.9 1.8-2.2 3.9-2.2 4.2 0 5 2.8 5 6.4V24h-4v-7.6c0-1.8 0-4.2-2.6-4.2s-3 2-3 4v7.8h-4V8z\"\/>\n        <\/svg>\n        View LinkedIn Profile\n      <\/a>\n\n    <\/div>\n\n  <\/div>\n      <\/header>\n\n      <article class=\"ols-note-card\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">1<\/div>\n<h2>Naming Haloalkanes<\/h2>\n<\/div>\n<p>A <strong>haloalkane<\/strong> is an alkane in which one or more hydrogen atoms have been replaced by halogen atoms, so the general formula of a mono-substituted compound is C\u2099H\u2082\u2099\u208a\u2081X. They are named as substituted alkanes: the halogen is a prefix, fluoro-, chloro-, bromo- or iodo-, with a number giving its position, and prefixes are listed in alphabetical order. CH\u2083CH\u2082CH\u2082Br is 1-bromopropane, CH\u2083CHBrCH\u2083 is 2-bromopropane, and CH\u2083CHClCH\u2082CH\u2083 is 2-chlorobutane. Two of the same halogen use di-: CH\u2082BrCH\u2082Br is 1,2-dibromoethane.<\/p>\n<p>The same three representations are needed as for alcohols: structural, displayed and skeletal formulae. In a skeletal formula the halogen is written at the end of the line, Br or Cl, and the carbon carrying it is the vertex.<\/p>\n<div class=\"ols-table-wrap\">\n<table class=\"ols-table\">\n<thead>\n<tr><th>Structural formula<\/th><th>Name<\/th><th>Class<\/th><\/tr>\n<\/thead>\n<tbody>\n<tr><td><strong>CH\u2083CH\u2082CH\u2082Cl<\/strong><\/td><td>1-chloropropane<\/td><td>primary<\/td><\/tr>\n<tr><td><strong>CH\u2083CHBrCH\u2083<\/strong><\/td><td>2-bromopropane<\/td><td>secondary<\/td><\/tr>\n<tr><td><strong>(CH\u2083)\u2083CCl<\/strong><\/td><td>2-chloro-2-methylpropane<\/td><td>tertiary<\/td><\/tr>\n<tr><td><strong>CH\u2083CH\u2082CH\u2082CH\u2082I<\/strong><\/td><td>1-iodobutane<\/td><td>primary<\/td><\/tr>\n<tr><td><strong>CH\u2082ClCH\u2082Cl<\/strong><\/td><td>1,2-dichloroethane<\/td><td>primary (both carbons)<\/td><\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n<div class=\"ols-key-box\">\n<p><strong>Exam focus:<\/strong> Number from the end that gives the halogen the lowest number, and put the prefixes in alphabetical order: 1-bromo-2-chloropropane, not 2-chloro-1-bromopropane.<\/p>\n<\/div>\n<\/article>\n<article class=\"ols-note-card soft\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">2<\/div>\n<h2>Primary, Secondary and Tertiary<\/h2>\n<\/div>\n<p>Like alcohols, haloalkanes are classified by the number of carbon atoms bonded to the carbon that carries the halogen. In a <strong>primary haloalkane<\/strong> that carbon is bonded to one other carbon (1-bromopropane); in a <strong>secondary<\/strong> compound to two (2-bromopropane); in a <strong>tertiary<\/strong> compound to three (2-bromo-2-methylpropane). The class affects both the rate of hydrolysis and the balance between substitution and elimination, which is why examiners keep asking for it.<\/p>\n\n<div class=\"ols-key-box\">\n<p><strong>Key idea:<\/strong> Find the carbon bonded to the halogen and count its carbon neighbours: one primary, two secondary, three tertiary.<\/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>Check: Naming and Classifying<\/h2>\n<p>Name and classify haloalkanes not shown on this page.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"950\"><\/div><\/div>\n<\/section>\n<article class=\"ols-note-card\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">3<\/div>\n<h2>The Polar C\u2013X Bond<\/h2>\n<\/div>\n<p>Every halogen is more electronegative than carbon, so the <strong>carbon\u2013halogen bond is polar<\/strong>: the carbon is \u03b4+ and the halogen is \u03b4\u2212. The \u03b4+ carbon is electron-deficient and is the site attacked by nucleophiles. The polarity is greatest for C\u2013F and least for C\u2013I, because electronegativity falls down Group 17: fluorine 4.0, chlorine 3.0, bromine 2.8, iodine 2.5, against carbon 2.5. On that basis chloroalkanes should be the most reactive, but they are not.<\/p>\n<p>The rate of a nucleophilic substitution depends on how easily the C\u2013X bond breaks, that is on the <strong>bond enthalpy<\/strong>. Going down the group the halogen atom gets larger, the bond gets longer, and the bond enthalpy falls: C\u2013F 467, C\u2013Cl 346, C\u2013Br 290, C\u2013I 228 kJ mol\u207b\u00b9. The C\u2013I bond is the weakest and breaks most easily, so iodoalkanes are hydrolysed fastest; fluoroalkanes are so unreactive that they are used in non-stick coatings and refrigerants. Bond strength, not bond polarity, controls the rate.<\/p>\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\/09\/alcohols-halogenoalkanes-spectra-cxbonds.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\/09\/alcohols-halogenoalkanes-spectra-cxbonds.jpg\" alt=\"Primary, secondary and tertiary chloroalkanes with the polar C\u2013Cl bond, and a bar chart of carbon\u2013halogen bond enthalpies\">\n<\/a>\n<\/div>\n<div class=\"ols-zoom-card-caption\"><p>Primary, secondary and tertiary chloroalkanes with the polar C\u2013Cl bond, and the bond enthalpies of the four carbon\u2013halogen bonds.<\/p><\/div>\n<\/div>\n<!-- 3D card: carbon-halogen-bond (26 Sep 2026) -->\n<section class=\"ols-chx-001\" id=\"olsChx001\">\n<style>\n@import url('https:\/\/fonts.googleapis.com\/css2?family=Poppins:wght@300;400;500;600&display=swap');\n\n.ols-chx-001{\n  font-family:'Poppins',system-ui,-apple-system,'Segoe UI',Roboto,Helvetica,Arial,sans-serif;\n  color:#1C244B; 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padding:1px 5px;}\n  .ols-chx-001 .chx-badge.b-eq{font-size:11px;}\n  .ols-chx-001 .chx-read{padding:5px 9px;}\n  .ols-chx-001 .chx-panel{left:auto; right:14px; transform:none; font-size:11px; padding:6px 10px;}\n}\n@media (prefers-reduced-motion:reduce){\n  .ols-chx-001 .chx-seg button,.ols-chx-001 .chx-pill{transition:none;}\n}\n\n.ols-cc-chx-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-chx-001 a{color:#aab0c0; text-decoration:none;}\n.ols-cc-chx-001 a:hover{text-decoration:underline;}\n<\/style>\n\n<div class=\"chx-head\">\n  <h2 class=\"chx-title\">The Carbon\u2013Halogen Bond: Polarity and Strength<\/h2>\n  <p class=\"chx-sub\">Compare the C\u2013Cl, C\u2013Br and C\u2013I bonds in the halogenoethanes, drawn to scale, and see why the weakest bond, not the most polar one, reacts fastest with a nucleophile.<\/p>\n<\/div>\n\n<div class=\"chx-stage\" id=\"chxStage\">\n  <canvas class=\"chx-canvas\" id=\"chxCanvas\"><\/canvas>\n  <div class=\"chx-overlay\" id=\"chxOverlay\"><\/div>\n  <div class=\"chx-caption\" id=\"chxCaption\"><\/div>\n  <div class=\"chx-hint\" id=\"chxHint\">Drag to rotate<\/div>\n  <div class=\"chx-badges\" id=\"chxBadges\"><\/div>\n<\/div>\n\n<div class=\"chx-readbar\" id=\"chxRead\" aria-live=\"polite\"><\/div>\n\n<div class=\"chx-controls\">\n  <div class=\"chx-row\">\n    <span class=\"chx-rowlab\">Molecule<\/span>\n    <div class=\"chx-seg\" role=\"group\" aria-label=\"Molecule\">\n      <button type=\"button\" data-m=\"Cl\" aria-pressed=\"true\">CH<sub>3<\/sub>CH<sub>2<\/sub>Cl<\/button>\n      <button type=\"button\" data-m=\"Br\" aria-pressed=\"false\">CH<sub>3<\/sub>CH<sub>2<\/sub>Br<\/button>\n      <button type=\"button\" data-m=\"I\" aria-pressed=\"false\">CH<sub>3<\/sub>CH<sub>2<\/sub>I<\/button>\n    <\/div>\n  <\/div>\n\n  <div class=\"chx-row\">\n    <span class=\"chx-rowlab\">Step<\/span>\n    <div class=\"chx-seg\" role=\"group\" aria-label=\"Step\">\n      <button type=\"button\" data-step=\"1\" aria-pressed=\"true\">Shape<\/button>\n      <button type=\"button\" data-step=\"2\" aria-pressed=\"false\">Polarity<\/button>\n      <button type=\"button\" data-step=\"3\" aria-pressed=\"false\">Strength<\/button>\n      <button type=\"button\" data-step=\"4\" aria-pressed=\"false\">Attack<\/button>\n    <\/div>\n  <\/div>\n\n  <div class=\"chx-row\">\n    <span class=\"chx-rowlab\">View<\/span>\n    <div class=\"chx-seg\" role=\"group\" aria-label=\"Camera view\">\n      <button type=\"button\" data-v=\"front\" aria-pressed=\"false\">Front<\/button>\n      <button type=\"button\" data-v=\"side\" aria-pressed=\"false\">Side<\/button>\n      <button type=\"button\" data-v=\"top\" aria-pressed=\"false\">Top<\/button>\n    <\/div>\n  <\/div>\n\n  <div class=\"chx-row\">\n    <span class=\"chx-rowlab\">Show<\/span>\n    <button type=\"button\" class=\"chx-pill\" id=\"chxTogCloud\" aria-pressed=\"true\"><i class=\"dot\"><\/i>Electron cloud<\/button>\n    <button type=\"button\" class=\"chx-pill\" id=\"chxTogDelta\" aria-pressed=\"true\"><i class=\"dot\"><\/i>&delta; labels<\/button>\n    <button type=\"button\" class=\"chx-pill p-gold\" id=\"chxTogRul\" aria-pressed=\"true\"><i class=\"dot\"><\/i>Bond-length ruler<\/button>\n    <button type=\"button\" class=\"chx-pill\" id=\"chxTogLp\" aria-pressed=\"true\"><i class=\"dot\"><\/i>Lone pair<\/button>\n  <\/div>\n\n  <div class=\"chx-row\">\n    <span class=\"chx-rowlab\">Motion<\/span>\n    <button type=\"button\" class=\"chx-pill\" id=\"chxSpin\" aria-pressed=\"false\"><i class=\"dot\"><\/i>Rotation<\/button>\n    <button type=\"button\" class=\"chx-pill\" id=\"chxResetV\">Reset view<\/button>\n  <\/div>\n<\/div>\n\n<div class=\"chx-info\">\n  <h3 id=\"chxInfoTitle\"><\/h3>\n  <p id=\"chxInfoText\"><\/p>\n  <div class=\"chx-facts\" id=\"chxFacts\"><\/div>\n  <div class=\"chx-key\">\n    <span><i style=\"background:#484e5c\"><\/i>Carbon<\/span>\n    <span><i style=\"background:#eef0f5\"><\/i>Hydrogen<\/span>\n    <span><i style=\"background:#3aa048\"><\/i>Chlorine<\/span>\n    <span><i style=\"background:#8c1e1e\"><\/i>Bromine<\/span>\n    <span><i style=\"background:#7832a0\"><\/i>Iodine<\/span>\n    <span><i style=\"background:#cd342c\"><\/i>Oxygen<\/span>\n    <span><i style=\"background:rgba(46,96,210,0.35); border:1.5px dotted rgba(46,96,210,0.9)\"><\/i>Bonding electron density<\/span>\n    <span><i style=\"background:#2563eb\"><\/i>Dipole arrow<\/span>\n    <span><i style=\"background:#c9961c\"><\/i>Bond-length ruler<\/span>\n    <span><i style=\"background:#3b78dc; border-radius:50%\"><\/i>Lone pair<\/span>\n  <\/div>\n<\/div>\n<\/section>\n\n<p class=\"ols-cc-chx-001\">&copy; Dr. Mohammed Al-Fatah &#8211; <a href=\"https:\/\/www.onlinelearningsystem.net\" target=\"_blank\" rel=\"noopener\">onlinelearningsystem.net<\/a><\/p>\n<script src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/JS\/carbon-halogen-bond.js?v=20260926d\"><\/script>\n\n<div class=\"ols-key-box\">\n<p><strong>Exam trap:<\/strong> Polarity predicts the wrong order. Write: &#8220;the C\u2013I bond has the lowest bond enthalpy, so it breaks most easily and iodoalkanes react fastest&#8221;.<\/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>Check: Bond Polarity and Bond Strength<\/h2>\n<p>Apply the polarity and bond enthalpy ideas to compounds not compared above.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-951\" class=\"h5p-iframe\" data-content-id=\"951\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Alcohols, Halogenoalkanes and Spectra Summary: Bond Polarity and Bond Strength\"><\/iframe><\/div><\/div>\n<\/section>\n<article class=\"ols-note-card soft\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">4<\/div>\n<h2>Uses and Properties of Haloalkanes<\/h2>\n<\/div>\n<p>Haloalkanes are useful because the C\u2013X bond can be swapped for other groups, so they are the starting point for making alcohols, amines and nitriles in synthesis. Chloroalkanes and chlorofluoroalkanes were used as solvents, refrigerants, aerosol propellants and anaesthetics, and many of those uses have been stopped because the compounds are toxic or damage the ozone layer.<\/p>\n<p>Their physical properties follow from the polar C\u2013X bond and the size of the halogen. Haloalkanes have permanent dipole\u2013dipole forces as well as London forces, so they boil at higher temperatures than the alkanes of similar size, and boiling temperature rises from chloro- to iodo- as the number of electrons and the London forces increase. They are not soluble in water, because they cannot hydrogen bond, which is why an ethanol solvent is needed when they are reacted with aqueous reagents.<\/p>\n<div class=\"ols-key-box\">\n<p><strong>Key idea:<\/strong> Insoluble in water, denser than water for most bromo- and iodo- compounds, and boiling temperature rising down the halogen group with the London forces.<\/p>\n<\/div>\n<\/article>\n<article class=\"ols-note-card\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">5<\/div>\n<h2>Common Exam Points<\/h2>\n<\/div>\n<h3>Say<\/h3><p>&#8220;The C\u2013Br bond is polar because bromine is more electronegative than carbon, so the carbon is \u03b4+.&#8221; &#8220;C\u2013I has the lowest bond enthalpy so it is broken most easily.&#8221;<\/p>\n<h3>Do not say<\/h3><p>&#8220;Iodoalkanes react fastest because the C\u2013I bond is most polar.&#8221; &#8220;Tertiary because there are three carbons in the molecule.&#8221;<\/p>\n<h3>Watch for<\/h3><p>Questions that give bond enthalpy data and ask you to predict a rate: quote the numbers in your answer.<\/p>\n<\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Check: Properties and Uses<\/h2>\n<p>Explain properties of haloalkanes that are not the examples used above.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-952\" class=\"h5p-iframe\" data-content-id=\"952\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Alcohols, Halogenoalkanes and Spectra Quick Choice: Properties and Uses\"><\/iframe><\/div><\/div>\n<\/section>\n<section class=\"ols-faq-card\">\n<h2>FAQs<\/h2>\n<p>Use these quick answers to check the haloalkane basics.<\/p>\n\n<div class=\"ols-faq-list\">\n<div class=\"ols-faq-item\">\n<h3>How do I order two different halogens in a name?<\/h3>\n<p>Alphabetically, ignoring the numbers: 1-bromo-2-chloroethane, because b comes before c.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>Why is the carbon of a C\u2013Br bond \u03b4+?<\/h3>\n<p>Bromine is more electronegative than carbon, so it pulls the bonding electrons towards itself, leaving the carbon slightly positive.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>If C\u2013Cl is the most polar bond, why are chloroalkanes the least reactive?<\/h3>\n<p>Because the rate depends on breaking the C\u2013X bond, and C\u2013Cl is the strongest of the three (346 kJ mol\u207b\u00b9). Bond enthalpy, not polarity, controls the rate.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>Why do haloalkanes not dissolve in water?<\/h3>\n<p>They have no O\u2013H or N\u2013H, so they cannot hydrogen bond to water; the water\u2013water hydrogen bonds are not replaced by anything as strong.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>Why do haloalkanes boil higher than alkanes of similar mass?<\/h3>\n<p>The polar C\u2013X bond gives permanent dipole\u2013dipole forces in addition to London forces, and the large halogen atom adds electrons that strengthen the London forces.<\/p>\n<\/div>\n<\/div>\n<\/section>\n<section class=\"ols-related-card\">\n<h2>Related 4.2.2 Haloalkanes Pages<\/h2>\n<p>Use these pages to connect the ideas across 4.2.2 Haloalkanes and the rest of the course.<\/p>\n<div class=\"ols-related-grid\">\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-2-2-haloalkanes\/reaction-types-mechanisms-and-nucleophiles\/\">Reaction Types, Mechanisms and Nucleophiles<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-2-2-haloalkanes\/nucleophilic-substitution-reactions\/\">Nucleophilic Substitution Reactions<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-2-2-haloalkanes\/rates-of-hydrolysis-and-bond-enthalpy\/\">Rates of Hydrolysis and Bond Enthalpy<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-2-2-haloalkanes\/cfcs-and-the-ozone-layer\/\">CFCs and the Ozone Layer<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-2-2-haloalkanes\/\">4.2.2 Haloalkanes Overview<\/a>\n<\/div>\n<\/section>\n<section class=\"ols-attribution-card\">\n        <p><strong>Copyright and author footprint:<\/strong> This OLS revision page was written for Online Learning System by <strong>Dr. Mohammed Al-Fatah<\/strong>. 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