{"id":1046,"date":"2010-10-25T16:32:00","date_gmt":"2010-10-25T14:32:00","guid":{"rendered":"https:\/\/www.masterorganicchemistry.com\/?p=1046"},"modified":"2026-05-03T07:32:53","modified_gmt":"2026-05-03T12:32:53","slug":"3-trends-that-affect-boiling-points","status":"publish","type":"post","link":"https:\/\/www.masterorganicchemistry.com\/2010\/10\/25\/3-trends-that-affect-boiling-points\/","title":{"rendered":"3 Trends That Affect Boiling Points"},"content":{"rendered":"<p>Figuring out the order of boiling points is all about <strong>understanding trends<\/strong>. The key thing to consider here is that boiling points reflect the strength of forces between molecules. The more they stick together, the more energy it will take to blast them into the atmosphere as gases.<\/p>\n<p>There are 3 important trends to consider.<\/p>\n<ul>\n<li>The relative strength of the <a title=\"For forces that affect boiling points\" href=\"https:\/\/www.masterorganicchemistry.com\/2010\/10\/01\/how-intermolecular-forces-affect-boiling-points\/\">four intermolecular forces<\/a> is: <strong>Ionic<\/strong> &gt; <strong>Hydrogen bonding<\/strong> &gt; <strong>dipole dipole<\/strong> &gt; <strong>Van der Waals dispersion<\/strong> forces. The influence of each of these attractive forces will depend on the functional groups present.<\/li>\n<li>Boiling points increase as the number of carbons is increased.<\/li>\n<li>Branching decreases boiling point.<\/li>\n<\/ul>\n<p>Let&#8217;s have a closer look.<\/p>\n<p><img fetchpriority=\"high\" decoding=\"async\" class=\"alignnone wp-image-37378\" src=\"https:\/\/www.masterorganicchemistry.com\/wp-content\/uploads\/2024\/09\/0-3-important-trends-that-affect-boiling-points-include-intermolecular-forces-molecular-weight-and-branching.gif\" alt=\"3 important trends that affect boiling points include intermolecular forces molecular weight and branching\" width=\"640\" height=\"558\" \/><\/a><\/p>\n<p><strong>Table of Contents<\/strong><\/p>\n<ol>\n<li><a href=\"#one\">Trend #1: The Relative Strength Of The Four Intermolecular Forces<\/a><\/li>\n<li><a href=\"#two\">Trend #2 &#8211; For Molecules With A Given Functional Group, Boiling Point Increases With Increasing Molecular Weight<\/a><\/li>\n<li><a href=\"#three\">The Role Of Symmetry (or lack thereof) On Melting And Boiling Points<\/a><\/li>\n<li><a href=\"#notes\">Notes<\/a><\/li>\n<li><a href=\"#quizzes\">Quiz Yourself!\u00a0<\/a><\/li>\n<\/ol>\n<hr \/>\n<h2><strong><a id=\"one\"><\/a>1. Trend #1: The relative strength of the four intermolecular forces .<\/strong><\/h2>\n<p>Compare the different butane alcohol derivatives shown below. Molecules of diethyl ether, C<sub>4<\/sub>H<sub>10<\/sub> O, are held together by <strong>dipole-dipole<\/strong> interactions which arise due to the polarized C-O bonds.<\/p>\n<p>Compare the boiling point of diethyl ether (35 \u00b0C)with that of Its isomer <strong>1-butanol<\/strong> (117 \u00b0C). The greatly <strong>increased<\/strong> boiling point is due to the fact that butanol contains a <strong>hydroxyl<\/strong> group, which is capable of <strong>hydrogen bonding<\/strong>.<\/p>\n<p>Still, the attractive forces in butanol pale in comparison to those of the salt sodium butoxide, which <em>melts <\/em>at an extremely high temperature (well above 260 \u00b0C) and actually <strong><em>decomposes<\/em><\/strong> before it can turn into a liquid and boil.<\/p>\n<p><img decoding=\"async\" class=\"aligncenter wp-image-14040\" src=\"https:\/\/www.masterorganicchemistry.com\/wp-content\/uploads\/2019\/11\/1-boiling-points-reflect-intermolecular-attractive-forces-for-example-diethyl-ether-versus-n-butanol-versus-sodium-n-butoxide.gif\" alt=\"boiling-points-reflect-intermolecular-attractive-forces-for-example-diethyl-ether-versus-n-butanol-versus-sodium-n-butoxide\" width=\"550\" height=\"340\" \/><\/p>\n<p>Then think about butane, C<sub>4<\/sub>H<sub>10<\/sub>, which contains <strong>no<\/strong> polar functional groups. The only attractive forces between individual butane molecules are the relatively weak Van der Waals dispersion forces. The result is that butane boils at the temperature at which water freezes (0\u00b0 C), far below even that of diethyl ether.<\/p>\n<p><strong> Moral of the story<\/strong>: among molecules <em>with roughly similar molecular weights<\/em>, the boiling points will be determined by the functional groups present.<\/p>\n<p>You could tell a similar tale for the similar amine and carboxylic acid isomers shown below.<\/p>\n<p><img decoding=\"async\" class=\"aligncenter wp-image-14041\" src=\"https:\/\/www.masterorganicchemistry.com\/wp-content\/uploads\/2019\/11\/2-amine-derivatives-of-similar-molecular-weight-with-compare-boiling-points-dipole-dipole-vs-hydrogen-bonding-vs-ionic.gif\" alt=\"amine-derivatives-of-similar-molecular-weight-with-compare-boiling-points-dipole-dipole-vs-hydrogen-bonding-vs-ionic\" width=\"550\" height=\"759\" \/><\/p>\n<p>For a previous discussion of the 4 intermolecular forces, see the previous article (<a href=\"https:\/\/www.masterorganicchemistry.com\/2010\/10\/01\/how-intermolecular-forces-affect-boiling-points\/\"><span style=\"color: #993366;\"><em>The Four Intermolecular Forces And How They Affect Boiling Points<\/em><\/span><\/a>)<\/p>\n<h2><strong><a id=\"two\"><\/a>2. Trend #2 &#8211; For molecules with a given functional group, boiling point increases with molecular weight.<\/strong><\/h2>\n<p>Look at the dramatic increases in boiling points as you increase molecular weight in all of these series:<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter wp-image-14042\" src=\"https:\/\/www.masterorganicchemistry.com\/wp-content\/uploads\/2019\/11\/3-alkanes-versus-alcohols-versus-carboxylic-acid-vs-ether-boiling-points.gif\" alt=\"alkanes-versus-alcohols-versus-carboxylic-acid-vs-ether-boiling-points\" width=\"575\" height=\"443\" \/><\/p>\n<p>Here&#8217;s the question: <strong>How,<\/strong> exactly do intermolecular forces increase as molecular weight increases?<\/p>\n<p>Well, the key force that is acting here are Van der Waals dispersion forces, which are <strong>proportional to surface area<\/strong>. So as you <strong>increase<\/strong> the <strong>length<\/strong> of the chain, you also increase the <strong>surface area<\/strong>, which means that you increase the ability of individual molecules to attract each other.<\/p>\n<p>On an intuitive level, you could compare these long molecules to strands of spaghetti &#8211;\u00a0 the longer the noodles, the more work it takes to pull them apart. As the chain length increases, there will be regions where they can line up next to each other extremely well.<\/p>\n<p>Individually, each interaction might not be worth very much, but when you add them all up over the length of a chain, Van der Waals dispersion forces can exert tremendous effects.<\/p>\n<h2><strong><a id=\"three\"><\/a>3. The Role Of Symmetry (or lack thereof) On Melting And Boiling Points<\/strong><\/h2>\n<p>This is another byproduct of the surface-area dependence of Van der Waals dispersion forces &#8211; the more rod-like the molecules are, the better able they will be to line up and bond.<\/p>\n<p>To take another intuitive pasta example, what sticks together more: spaghetti or macaroni? The more spherelike the molecule, the lower its surface area will be and the fewer intermolecular Van der Waals interactions will operate. Compare the boiling points of pentane (36\u00b0C) and 2,2-dimethyl propane (9 \u00b0C).<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter wp-image-14043\" title=\"5-bp copy\" src=\"https:\/\/www.masterorganicchemistry.com\/wp-content\/uploads\/2019\/11\/4-branching-decreases-boiling-point-and-polar-functional-groups-most-exposed-will-elevate-boiling-points-to-greatest-extent.gif\" alt=\"branching-decreases-boiling-point-and-polar-functional-groups-most-exposed-will-elevate-boiling-points-to-greatest-extent\" width=\"550\" height=\"224\" \/><\/p>\n<p>It can also apply to hydrogen bonding molecules like alcohols &#8211; compare the boiling points of 1-pentanol to 2-pentanol and 3-pentanol, for instance. The hydroxyl group of 1-pentanol is more &#8220;exposed&#8221; than it is in 3-pentanol (which is flanked by two bulky alkyl groups), so it will be better able to hydrogen bond with its fellows.<\/p>\n<p>In summary, there are three main factors you need to think about when confronted with a question about boiling points. 1) what intermolecular forces will be present in the molecules? 2) how do the molecular weights compare? 3) how do the symmetries compare?<\/p>\n<p>One last quick question for the road (see comments for answer).<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter wp-image-14044\" src=\"https:\/\/www.masterorganicchemistry.com\/wp-content\/uploads\/2019\/11\/5-three-amine-isomers-will-have-highest-boiling-point-butylamine-vs-diethylamine-vs-n-n-dimethyl-ethylamine.gif\" alt=\"three-amine-isomers-will-have-highest-boiling-point-butylamine-vs-diethylamine-vs-n-n-dimethyl-ethylamine\" width=\"550\" height=\"220\" \/><\/p>\n<hr \/>\n<h2><a id=\"notes\"><\/a>Notes<\/h2>\n<div class=\"related-articles\"><p><strong>Related Articles<\/strong><\/p><ul><li><a href=\"https:\/\/www.masterorganicchemistry.com\/2010\/10\/01\/how-intermolecular-forces-affect-boiling-points\/\" class=\"\"><span>The Four Intermolecular Forces and How They Affect Boiling Points<\/span><\/a><\/li><li><a href=\"https:\/\/www.masterorganicchemistry.com\/2010\/07\/09\/branching-melting-boiling-points\/\" class=\"\"><span>Branching, and Its Affect On Melting and Boiling Points<\/span><\/a><\/li><li><a href=\"https:\/\/www.masterorganicchemistry.com\/2011\/11\/15\/how_to_use_electronegativity\/\" class=\"\"><span>How To Use Electronegativity To Determine Electron Density (and why NOT to trust formal charge)<\/span><\/a><\/li><li><a href=\"https:\/\/www.masterorganicchemistry.com\/2011\/11\/23\/introduction-to-resonance\/\" class=\"\"><span>Introduction to Resonance<\/span><\/a><\/li><li><a href=\"https:\/\/www.masterorganicchemistry.com\/2011\/11\/30\/introduction-to-resonance-2-curved-arrows\/\" class=\"\"><span>How To Use Curved Arrows To Interchange Resonance Forms<\/span><\/a><\/li><li><a href=\"https:\/\/www.masterorganicchemistry.com\/2017\/10\/10\/hybrid-orbitals\/\" class=\"\"><span>Hybrid Orbitals and Hybridization<\/span><\/a><\/li><li><a href=\"https:\/\/www.masterorganicchemistry.com\/2025\/10\/17\/dipole-moments-and-dipoles\/\" class=\"\"><span>Dipole Moments and Dipoles<\/span><\/a><\/li><\/ul><\/div>\n<p>P.S.\u00a0<strong>New! Check out this free 3-page handout on solving common boiling point exam problems!\u00a0<\/strong><\/p>\n<p><strong><a href=\"https:\/\/www.masterorganicchemistry.com\/wp-content\/uploads\/2025\/01\/MOC-Boiling-Point-Handout.pdf\">MOC_Boiling_Point_Handout (PDF)<\/a><\/strong><\/p>\n<p><strong>Note 1.\u00a0<\/strong>Some physical properties for alkanes<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-45809\" src=\"https:\/\/www.masterorganicchemistry.com\/wp-content\/uploads\/2026\/05\/T11-Physical-properties-of-the-normal-alkanes-boiling-point-melting-point-molecular-weight-heat-of-combustion-master-organic-chemistry.gif\" alt=\"Physical-properties-of-the-normal-alkanes-boiling-point-melting-point-molecular-weight-heat-of-combustion-master-organic-chemistry\" width=\"640\" height=\"472\" \/><\/a><\/p>\n<p><strong>Note 2.\u00a0<\/strong>Physical properties for higher alkanes (undecane, dodecane, tridecane, tetradecane, pentadecane, hexadecane, heptadecane, octadecane, nonadecane, and eicosane.<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-45808\" src=\"https:\/\/www.masterorganicchemistry.com\/wp-content\/uploads\/2026\/05\/T10-Physical-properties-of-C11-C20-alkanes-undecane-eicosane-boiling-point-melting-point-molecular-weight-heat-of-combustion-master-organic-chemistry-2.gif\" alt=\"Physical properties of C11-C20 alkanes undecane eicosane boiling point melting point molecular weight heat of combustion master organic chemistry 2\" width=\"640\" height=\"486\" \/><\/a><\/p>\n<p>&nbsp;<\/p>\n<hr \/>\n<h2><a id=\"quizzes\"><\/a>Quiz Yourself!<\/h2>\n\n<p class=\"p1\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-26714\" src=\"https:\/\/www.masterorganicchemistry.com\/wp-content\/uploads\/quiz-previews\/3688-Front-Image-Only.png\" alt=\"\" width=\"640\" height=\"616\" \/><\/p>\n<p><a href=\"https:\/\/www.masterorganicchemistry.com\/moc-membership\/\"><strong>Become a\u00a0 MOC member<\/strong><\/a> to see the clickable quiz with answers on the back. <\/p>\n\n<p class=\"p1\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-26714\" src=\"https:\/\/www.masterorganicchemistry.com\/wp-content\/uploads\/quiz-previews\/3689-Front-Image-Only.png\" alt=\"\" width=\"640\" height=\"616\" \/><\/p>\n<p><a href=\"https:\/\/www.masterorganicchemistry.com\/moc-membership\/\"><strong>Become a\u00a0 MOC member<\/strong><\/a> to see the clickable quiz with answers on the back. <\/p>\n\n<p class=\"p1\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-26714\" src=\"https:\/\/www.masterorganicchemistry.com\/wp-content\/uploads\/quiz-previews\/3690-Front-Image-Only.png\" alt=\"\" width=\"640\" height=\"616\" \/><\/p>\n<p><a href=\"https:\/\/www.masterorganicchemistry.com\/moc-membership\/\"><strong>Become a\u00a0 MOC member<\/strong><\/a> to see the clickable quiz with answers on the back. <\/p>\n\n<p class=\"p1\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-26714\" src=\"https:\/\/www.masterorganicchemistry.com\/wp-content\/uploads\/quiz-previews\/1246-Front-Image-Only.png\" alt=\"\" width=\"640\" height=\"616\" \/><\/p>\n<p><a href=\"https:\/\/www.masterorganicchemistry.com\/moc-membership\/\"><strong>Become a\u00a0 MOC member<\/strong><\/a> to see the clickable quiz with answers on the back. <br \/>\n<\/p>\n<p class=\"p1\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-26714\" src=\"https:\/\/www.masterorganicchemistry.com\/wp-content\/uploads\/quiz-previews\/1247-Front-Image-Only.png\" alt=\"\" width=\"640\" height=\"616\" \/><\/p>\n<p><a href=\"https:\/\/www.masterorganicchemistry.com\/moc-membership\/\"><strong>Become a\u00a0 MOC member<\/strong><\/a> to see the clickable quiz with answers on the back. <br \/>\n<\/p>\n<p class=\"p1\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-26714\" src=\"https:\/\/www.masterorganicchemistry.com\/wp-content\/uploads\/quiz-previews\/1250-Front-Image-Only.png\" alt=\"\" width=\"640\" height=\"616\" \/><\/p>\n<p><a href=\"https:\/\/www.masterorganicchemistry.com\/moc-membership\/\"><strong>Become a\u00a0 MOC member<\/strong><\/a> to see the clickable quiz with answers on the back. <br \/>\n<\/p>\n<p class=\"p1\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-26714\" src=\"https:\/\/www.masterorganicchemistry.com\/wp-content\/uploads\/quiz-previews\/1242-Front-Image-Only.png\" alt=\"\" width=\"640\" height=\"616\" \/><\/p>\n<p><a href=\"https:\/\/www.masterorganicchemistry.com\/moc-membership\/\"><strong>Become a\u00a0 MOC member<\/strong><\/a> to see the clickable quiz with answers on the back. <br \/>\n<\/p>\n<p class=\"p1\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-26714\" src=\"https:\/\/www.masterorganicchemistry.com\/wp-content\/uploads\/quiz-previews\/1243-Front-Image-Only.png\" alt=\"\" width=\"640\" height=\"616\" \/><\/p>\n<p><a href=\"https:\/\/www.masterorganicchemistry.com\/moc-membership\/\"><strong>Become a\u00a0 MOC member<\/strong><\/a> to see the clickable quiz with answers on the back. <\/p>\n","protected":false},"excerpt":{"rendered":"<p>Figuring out the order of boiling points is all about understanding trends. The key thing to consider here is that boiling points reflect the strength <\/p>\n","protected":false},"author":1,"featured_media":37378,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"footnotes":""},"categories":[1406],"tags":[179,674,495,199,673,496,558,317,675],"post_folder":[],"class_list":["post-1046","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-bonding-structure-resonance","tag-boiling-points","tag-branching","tag-dipoles","tag-electronegativity","tag-electrostatics","tag-hydrogen-bonding","tag-intramolecular","tag-ionic-bonding","tag-van-der-waals"],"acf":[],"yoast_head":"<!-- This site is optimized with the Yoast SEO plugin v27.7 - https:\/\/yoast.com\/product\/yoast-seo-wordpress\/ -->\n<title>3 Trends That Affect Boiling Points &#8211; Master Organic Chemistry<\/title>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/www.masterorganicchemistry.com\/2010\/10\/25\/3-trends-that-affect-boiling-points\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"3 Trends That Affect Boiling Points &#8211; Master Organic Chemistry\" \/>\n<meta property=\"og:description\" content=\"Figuring out the order of boiling points is all about understanding trends. 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