{"id":8159,"date":"2026-09-16T17:33:33","date_gmt":"2026-09-16T16:33:33","guid":{"rendered":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/choosing-solvents\/"},"modified":"2026-09-18T11:28:53","modified_gmt":"2026-09-18T10:28:53","slug":"choosing-solvents","status":"publish","type":"page","link":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/choosing-solvents\/","title":{"rendered":"Choosing Solvents"},"content":{"rendered":"\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      --soft-red: #fff7f7;\n      --soft-purple: #f7f0ff;\n      --soft-green: #f0f7f1;\n      --soft-orange: #fff7ed;\n      --grey-text: #667085;\n      --body-text: #1f2937;\n      --border: rgba(28, 36, 75, 0.14);\n  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.ols-figure-placeholder .ols-figure-caption p { margin: 10px 0 0; font-size: 14px; color: #667085; text-align: center; }\n<\/style>\n\n  <aside class=\"ols-sidebar\">\r\n  <div class=\"ols-sidebar-header\">\r\n    <h3>Revision Notes<\/h3>\r\n    <p>AQA A Level Chemistry<\/p>\r\n  <\/div>\r\n\r\n  <div class=\"ols-topic-group\">\r\n    <h4>3.1.3 Bonding<\/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\/aqa\/3-1-3-bonding\/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\/aqa\/3-1-3-bonding\/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\/aqa\/3-1-3-bonding\/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\/aqa\/3-1-3-bonding\/ionic-bonding\/physical-properties-of-ionic-compounds\/\">Physical Properties of Ionic Compounds<\/a>\r\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/ionic-bonding\/ions-and-ionic-formulae\/\">Ions and Ionic Formulae<\/a>\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\/aqa\/3-1-3-bonding\/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\/aqa\/3-1-3-bonding\/covalent-bonding\/covalent-bonding\/\">Covalent Bonding<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/covalent-bonding\/dative-covalent-bonding\/\">Dative Covalent Bonding<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/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\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/\">Shapes of Molecules and Ions<\/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\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/linear\/\">Linear<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/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\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/tetrahedral\/\">Tetrahedral<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/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\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/bent\/\">Bent<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/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\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/octahedral\/\">Octahedral<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/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\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/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\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/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\/aqa\/3-1-3-bonding\/shapes-of-molecules-and-ions\/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\/aqa\/3-1-3-bonding\/bond-polarity\/\">Bond Polarity<\/a>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/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\/aqa\/3-1-3-bonding\/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\/aqa\/3-1-3-bonding\/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\/aqa\/3-1-3-bonding\/giant-covalent-structures\/\">Giant Covalent Structures<\/a>\r\n      <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/simple-molecular-structures\/\">Simple Molecular Structures<\/a>\r\n      <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/structure-types\/\">Structure Types<\/a>\n          <\/li>\r\n\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/\">Intermolecular Forces<\/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\/aqa\/3-1-3-bonding\/intermolecular-forces\/london-forces\/\">London Forces<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/permanent-dipole-dipole-forces\/\">Permanent Dipole-Dipole Forces<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/hydrogen-bonding\/\">Hydrogen Bonding<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/anomalous-properties-of-water\/\">Anomalous Properties of Water<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/boiling-temperature-trends\/\">Boiling Point Trends<\/a>\r\n          <\/li>\r\n          <li>\r\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/choosing-solvents\/\">Choosing Solvents<\/a>\r\n          <\/li>\r\n        <\/ul>\r\n      <\/li>\r\n    <\/ul>\r\n  <\/div>\r\n\r\n  <div class=\"ols-topic-group\">\r\n    <h4>Adjacent 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\/aqa\/3-1-1-atomicstructure\/\">3.1.1 Atomic Structure<\/a>\r\n      <\/li>\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-2-amount-of-substance\/\">3.1.2 Amount of Substance<\/a>\r\n      <\/li>\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-4-energetics\/\">3.1.4 Energetics<\/a>\r\n      <\/li>\r\n      <li>\r\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-2-1-periodicity\/\">3.2.1 Periodicity<\/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\"], 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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\/aqa\/\">AQA<\/a> \/\n<a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/\">3.1.3 Bonding<\/a> \/\n<a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/\">Intermolecular Forces<\/a> \/\n<span>Choosing Solvents<\/span>\n<\/nav>\n\n      <header class=\"ols-title-card\">\n        <h1>Choosing Solvents<\/h1>\n        <p class=\"ols-page-intro\">A concise revision guide to how intermolecular forces decide the choice of solvent: hydration of ions, alcohols dissolving in water by hydrogen bonding, why water is a poor solvent for halogenoalkanes, and like-dissolves-like for non-aqueous solvents, for AQA A Level Chemistry.<\/p>\n\n        <div class=\"ols-badges\">\n<div class=\"ols-badge\">Paper 1 and 2 AQA<\/div>\n<div class=\"ols-badge\">3.1.3 Bonding<\/div>\n<div class=\"ols-badge\">7405\/1 and 7405\/2<\/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 soft\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">1<\/div>\n<h2>What Decides Whether Something Dissolves<\/h2>\n<\/div>\n<p>A substance dissolves in a solvent when the attractions <strong>formed<\/strong> between solute and solvent particles are strong enough to compensate for the attractions <strong>broken<\/strong> within the solute and within the solvent. Dissolving is therefore a balance of intermolecular forces, and the rule of thumb &#8220;like dissolves like&#8221; simply means that the new solute-solvent attractions must be of a similar kind and strength to the ones being lost.<\/p>\n<p>Three questions decide the outcome: what holds the solute together (ionic lattice, hydrogen bonds, permanent dipoles or induced dipole-dipole forces), what holds the solvent together, and what the two can form with each other.<\/p>\n<div class=\"ols-key-box\">\n<p><strong>Key idea:<\/strong> Energy is needed to break solute-solute and solvent-solvent attractions; energy is released when solute-solvent attractions form. Dissolving happens when the two roughly balance.<\/p>\n<\/div>\n<\/article>\n<article class=\"ols-note-card\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">2<\/div>\n<h2>Water Dissolving Ionic Compounds: Hydration of Ions<\/h2>\n<\/div>\n<p>Water is polar: its oxygen is \u03b4- and its hydrogens \u03b4+. When an ionic solid such as sodium chloride is placed in water, the \u03b4- oxygen atoms of water molecules are attracted to the Na\u207a ions and the \u03b4+ hydrogen atoms to the Cl\u207b ions. Each ion that leaves the lattice becomes surrounded by a shell of correctly oriented water molecules; this is <strong>hydration<\/strong>, and the attractions formed are called <strong>ion-dipole attractions<\/strong>.<\/p>\n<p>The energy released by hydrating the ions is comparable to the energy needed to break up the lattice, so sodium chloride dissolves. Ionic compounds with very strongly bonded lattices, such as magnesium oxide, do not dissolve appreciably because the hydration energy cannot match the lattice energy.<\/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\/dissolving-sodium-chloride-hydration-and-ion-dipole-attractions.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\/dissolving-sodium-chloride-hydration-and-ion-dipole-attractions.jpg\" alt=\"Sodium chloride dissolving: water molecules orient their oxygen atoms towards sodium ions and their hydrogen atoms towards chloride ions\">\n<\/a>\n<\/div>\n<div class=\"ols-zoom-card-caption\"><p>Hydration: water molecules orient their \u03b4- oxygens towards cations and their \u03b4+ hydrogens towards anions, and the attractions formed pay for breaking the lattice.<\/p><\/div>\n<\/div>\n<div class=\"ols-key-box\">\n<p><strong>Exam sentence:<\/strong> Sodium chloride dissolves in water because the \u03b4- oxygen atoms of water molecules attract the Na\u207a ions and the \u03b4+ hydrogen atoms attract the Cl\u207b ions; the energy released when the ions are hydrated compensates for the energy needed to break the ionic lattice.<\/p>\n<\/div>\n<\/article>\n<article class=\"ols-note-card purple\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">3<\/div>\n<h2>Water Dissolving Alcohols: Hydrogen Bonding<\/h2>\n<\/div>\n<p>Methanol, ethanol and propan-1-ol mix with water in all proportions because the O-H group of the alcohol forms hydrogen bonds with water molecules. The hydrogen bonds formed between alcohol and water are similar in strength to the hydrogen bonds broken within the water and within the alcohol, so there is no barrier to mixing.<\/p>\n<p>As the carbon chain grows the alcohol becomes less soluble: butan-1-ol dissolves only to about 7 g per 100 g of water and hexan-1-ol barely at all. The long non-polar chain can only form induced dipole-dipole forces with water, and to make room for it water must break hydrogen bonds that the chain cannot replace. The hydrocarbon part outweighs the single O-H group.<\/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\/hydrogen-bonding-and-solubility-ethanol-and-chloroethane-in-water.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\/hydrogen-bonding-and-solubility-ethanol-and-chloroethane-in-water.jpg\" alt=\"Ethanol forming hydrogen bonds with water beside chloroethane, which cannot hydrogen bond and so does not dissolve\">\n<\/a>\n<\/div>\n<div class=\"ols-zoom-card-caption\"><p>Ethanol dissolves because its O-H group replaces the water hydrogen bonds it disrupts; chloroethane cannot form hydrogen bonds with water, so it does not dissolve.<\/p><\/div>\n<\/div>\n<div class=\"ols-key-box\">\n<p><strong>Key idea:<\/strong> Small alcohols are miscible with water because they hydrogen bond with it; solubility falls as the non-polar chain lengthens.<\/p>\n<\/div>\n<\/article>\n<article class=\"ols-note-card\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">4<\/div>\n<h2>Why Water Is a Poor Solvent for Halogenoalkanes<\/h2>\n<\/div>\n<p>Halogenoalkanes such as chloroethane are polar molecules: the C-Cl bond has a permanent dipole. Yet they are almost insoluble in water. <strong>The reason is that a halogenoalkane cannot form hydrogen bonds with water: it has no hydrogen bonded to N, O or F, and the halogen atom is a poor acceptor of hydrogen bonds.<\/strong> To dissolve, the halogenoalkane would have to break hydrogen bonds between water molecules to make space for itself, and the weak permanent dipole-dipole forces it could form with water would not pay back that energy.<\/p>\n<p>The same argument applies to many polar molecules without an O-H or N-H group, and it explains why &#8220;polar&#8221; does not automatically mean &#8220;soluble in water&#8221;. The question is always whether the solute can form hydrogen bonds with water, or at least attractions comparable to the ones it disrupts.<\/p>\n<div class=\"ols-table-wrap\">\n<table class=\"ols-table\">\n<thead>\n<tr><th>Solute<\/th><th>Polar?<\/th><th>Can hydrogen bond with water?<\/th><th>Soluble in water?<\/th><\/tr>\n<\/thead>\n<tbody>\n<tr><td><strong>Ethanol, C\u2082H\u2085OH<\/strong><\/td><td>yes<\/td><td>yes, O-H<\/td><td>miscible<\/td><\/tr>\n<tr><td><strong>Propanone, CH\u2083COCH\u2083<\/strong><\/td><td>yes<\/td><td>yes, C=O accepts from water<\/td><td>miscible<\/td><\/tr>\n<tr><td><strong>Chloroethane, C\u2082H\u2085Cl<\/strong><\/td><td>yes<\/td><td>no<\/td><td>almost insoluble<\/td><\/tr>\n<tr><td><strong>Hexane, C\u2086H\u2081\u2084<\/strong><\/td><td>no<\/td><td>no<\/td><td>insoluble<\/td><\/tr>\n<tr><td><strong>Sodium chloride<\/strong><\/td><td>ionic<\/td><td>ions are hydrated<\/td><td>soluble<\/td><\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n<div class=\"ols-key-box\">\n<p><strong>Exam sentence:<\/strong> Chloroethane does not dissolve in water because chloroethane molecules cannot form hydrogen bonds with water molecules; the hydrogen bonds between water molecules that would have to be broken are not replaced by attractions of similar strength.<\/p>\n<\/div>\n<\/article>\n<article class=\"ols-note-card soft\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">5<\/div>\n<h2>Non-Aqueous Solvents: Like Dissolves Like<\/h2>\n<\/div>\n<p>Substances that water cannot dissolve usually dissolve in a solvent whose intermolecular forces match their own. <strong>A non-polar solute dissolves in a non-polar solvent because the induced dipole-dipole forces broken between solute molecules and between solvent molecules are replaced by induced dipole-dipole forces of similar strength between solute and solvent.<\/strong> Iodine dissolves readily in hexane or cyclohexane but only slightly in water; grease and candle wax dissolve in hexane; halogenoalkanes dissolve in hexane and in ethanol.<\/p>\n<div class=\"ols-table-wrap\">\n<table class=\"ols-table\">\n<thead>\n<tr><th>Solute<\/th><th>Forces within the solute<\/th><th>Good solvent<\/th><th>Poor solvent<\/th><\/tr>\n<\/thead>\n<tbody>\n<tr><td><strong>Iodine, I\u2082<\/strong><\/td><td>induced dipole-dipole forces<\/td><td>hexane, cyclohexane<\/td><td>water<\/td><\/tr>\n<tr><td><strong>Candle wax (long alkanes)<\/strong><\/td><td>induced dipole-dipole forces<\/td><td>hexane, white spirit<\/td><td>water<\/td><\/tr>\n<tr><td><strong>Chloroethane<\/strong><\/td><td>permanent dipole-dipole forces and induced dipole-dipole forces<\/td><td>hexane, ethanol<\/td><td>water<\/td><\/tr>\n<tr><td><strong>Sodium chloride<\/strong><\/td><td>ionic lattice<\/td><td>water<\/td><td>hexane<\/td><\/tr>\n<tr><td><strong>Sugar (sucrose)<\/strong><\/td><td>hydrogen bonds (many O-H)<\/td><td>water<\/td><td>hexane<\/td><\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n<p>The choice of solvent matters in practical chemistry: an organic product is extracted from an aqueous mixture with a non-polar solvent in a separating funnel because the product dissolves in the organic layer and the ionic impurities stay in the water.<\/p>\n<div class=\"ols-key-box\">\n<p><strong>Exam focus:<\/strong> When asked to choose or justify a solvent, name the strongest force in the solute, name the strongest force in the candidate solvent, and say whether the solute-solvent attractions formed can replace those broken.<\/p>\n<\/div>\n<\/article>\n<article class=\"ols-note-card\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">6<\/div>\n<h2>Common Exam Points<\/h2>\n<\/div>\n<h3>Explain why sodium chloride dissolves in water<\/h3><p>\u03b4- oxygen of water attracts Na\u207a, \u03b4+ hydrogen attracts Cl\u207b; hydration energy compensates for lattice energy.<\/p>\n<h3>Explain why ethanol mixes with water but hexane does not<\/h3><p>Ethanol forms hydrogen bonds with water; hexane can only form induced dipole-dipole forces, which cannot replace the hydrogen bonds broken in water.<\/p>\n<h3>Explain why a polar halogenoalkane is insoluble in water<\/h3><p>It cannot hydrogen bond with water; the attractions it forms do not compensate for the water hydrogen bonds broken.<\/p>\n<h3>Suggest a solvent for iodine<\/h3><p>A non-polar solvent such as hexane, because both are held by induced dipole-dipole forces only.<\/p>\n<\/article>\n<section class=\"ols-h5p-card\">\n<h2>Check Your Understanding<\/h2>\n<p>Predict solubility for substances that are not in the tables above.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-542\" class=\"h5p-iframe\" data-content-id=\"542\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"IMF Solvents Drag: potassium bromide and bromoethane\"><\/iframe><\/div><\/div>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-543\" class=\"h5p-iframe\" data-content-id=\"543\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"IMF Solvents MCQ: cyclohexanol and cyclohexane\"><\/iframe><\/div><\/div>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-544\" class=\"h5p-iframe\" data-content-id=\"544\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"IMF Solvents MCQ: removing a grease stain\"><\/iframe><\/div><\/div>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-545\" class=\"h5p-iframe\" data-content-id=\"545\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"IMF Solvents MCQ: sucrose and iodine\"><\/iframe><\/div><\/div>\n<\/section>\n<section class=\"ols-faq-card\">\n<h2>FAQs<\/h2>\n<p>Use these quick answers to check how intermolecular forces decide what dissolves in what.<\/p>\n\n<div class=\"ols-faq-list\">\n<div class=\"ols-faq-item\">\n<h3>Why does sodium chloride dissolve in water?<\/h3>\n<p>The \u03b4- oxygen atoms of water molecules are attracted to the Na\u207a ions and the \u03b4+ hydrogen atoms to the Cl\u207b ions, so the ions become hydrated. The energy released by hydration compensates for the energy needed to break up the ionic lattice.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>Why do small alcohols mix with water?<\/h3>\n<p>The O-H group of the alcohol forms hydrogen bonds with water molecules that are similar in strength to the ones being broken, so there is no barrier to mixing. Solubility falls as the carbon chain lengthens.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>Why does a polar halogenoalkane not dissolve in water?<\/h3>\n<p>It has no hydrogen bonded to N, O or F, so it cannot form hydrogen bonds with water. The water-water hydrogen bonds that must be broken to make room for it are not replaced by attractions of similar strength.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>What does &#8220;like dissolves like&#8221; actually mean?<\/h3>\n<p>It means the solute-solvent attractions formed must be of the same kind and strength as the solute-solute and solvent-solvent attractions broken. Iodine dissolves in hexane because both are held only by induced dipole-dipole forces.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>Does polar always mean water-soluble?<\/h3>\n<p>No. Chloroethane is polar but almost insoluble in water, because its dipole is not enough to replace the hydrogen bonds it disrupts. The question to ask is whether the solute can hydrogen bond with water.<\/p>\n<\/div>\n<\/div>\n<\/section>\n<section class=\"ols-related-card\">\n<h2>Related Intermolecular Forces Pages<\/h2>\n<p>Use these pages to connect the three intermolecular forces with the physical properties they explain.<\/p>\n<div class=\"ols-related-grid\">\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/london-forces\/\">London Forces<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/permanent-dipole-dipole-forces\/\">Permanent Dipole-Dipole Forces<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/hydrogen-bonding\/\">Hydrogen Bonding<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/anomalous-properties-of-water\/\">Anomalous Properties of Water<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/intermolecular-forces\/boiling-temperature-trends\/\">Boiling Point Trends<\/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>. It is designed for A Level Chemistry revision and should not be copied or redistributed without permission.<\/p>\n      <\/section>\n\n      <div class=\"ols-image-lightbox\" id=\"olsImageLightboxNatureCovalentBonding9ch0\" 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-nature-of-covalent-bonding-9ch0-page\");\n          if (!page) { return; }\n          var lightbox = page.querySelector(\"#olsImageLightboxNatureCovalentBonding9ch0\");\n          if (!lightbox) { return; }\n          var lightboxImage = lightbox.querySelector(\".ols-image-lightbox-img\");\n    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