{"id":219814,"date":"2025-05-27T04:12:03","date_gmt":"2025-05-27T04:12:03","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=219814"},"modified":"2025-05-27T04:12:05","modified_gmt":"2025-05-27T04:12:05","slug":"mark-each-of-the-following-statement-as-true-or-false","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/27\/mark-each-of-the-following-statement-as-true-or-false\/","title":{"rendered":"Mark each of the following statement as True or False."},"content":{"rendered":"\n<p>Hexane, C6H14 (MW=86 g\/mol) has a boiling point of 68\u00b0C. Ethanol, CH3CH2OH (MW= 46 g\/mol) has a boiling point of 78\u00b0C. Mark each of the following statement as True or False.<\/p>\n\n\n\n<p>a. Ethanol must have stronger IMF, based on its higher boiling point<br>b. Ethanol has a higher boiling point because of greater London dispersion forces<br>c. Both hexane and ethanol have hydrogen bonding<br>d. Ethanol has a higher boiling point due to hydrogen bonding<br>e. Hydrogen bonding and London dispersion forces are at cross purposes here (one favors ethanol, the other favors hexane); in this case the hydrogen bonding evidently \u201cwins\u201d.<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-1-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Correct Answers:<\/h3>\n\n\n\n<p>a. <strong>True<\/strong><br>b. <strong>False<\/strong><br>c. <strong>False<\/strong><br>d. <strong>True<\/strong><br>e. <strong>True<\/strong><\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation <\/h3>\n\n\n\n<p>Boiling point is directly influenced by the strength of <strong>intermolecular forces (IMFs)<\/strong>\u2014stronger IMFs require more energy (heat) to overcome, resulting in a higher boiling point.<\/p>\n\n\n\n<p><strong>(a) True:<\/strong> Ethanol has a higher boiling point (78\u00b0C) than hexane (68\u00b0C), despite its lower molar mass. This suggests that <strong>ethanol has stronger intermolecular forces<\/strong> than hexane. Stronger IMFs correlate with higher boiling points.<\/p>\n\n\n\n<p><strong>(b) False:<\/strong> <strong>London dispersion forces<\/strong> (LDFs) are temporary, weak attractions that increase with molecular size and surface area. Hexane, being larger and more hydrophobic, actually experiences stronger London dispersion forces than ethanol. Therefore, LDFs do not explain ethanol\u2019s higher boiling point.<\/p>\n\n\n\n<p><strong>(c) False:<\/strong> <strong>Hydrogen bonding<\/strong> occurs when a hydrogen atom is directly bonded to a highly electronegative atom (like O, N, or F) and interacts with a lone pair on another electronegative atom. Ethanol (CH\u2083CH\u2082OH) has an \u2013OH group, which allows hydrogen bonding. Hexane (C\u2086H\u2081\u2084), however, is a nonpolar hydrocarbon with only C\u2013H bonds, which <strong>cannot hydrogen bond<\/strong>. Therefore, only ethanol exhibits hydrogen bonding.<\/p>\n\n\n\n<p><strong>(d) True:<\/strong> Ethanol&#8217;s higher boiling point is primarily due to <strong>hydrogen bonding<\/strong>, a much stronger IMF than London dispersion forces. The polar \u2013OH group in ethanol allows molecules to associate through these strong interactions, requiring more energy to break apart during boiling.<\/p>\n\n\n\n<p><strong>(e) True:<\/strong> This statement correctly acknowledges the interplay between two types of IMFs: <strong>London dispersion forces<\/strong> dominate in hexane (a larger, nonpolar molecule), while <strong>hydrogen bonding<\/strong> dominates in ethanol. Despite hexane\u2019s stronger LDFs due to its size, the <strong>hydrogen bonding in ethanol is more significant<\/strong>, leading to its higher boiling point. Thus, \u201chydrogen bonding wins\u201d in determining the boiling point comparison.<\/p>\n\n\n\n<p>In summary, the key factor driving ethanol\u2019s higher boiling point is its ability to hydrogen bond, which outweighs the stronger London dispersion forces present in the larger, nonpolar hexane molecules.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/05\/learnexams-banner4-33.jpeg\" alt=\"\" class=\"wp-image-219815\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Hexane, C6H14 (MW=86 g\/mol) has a boiling point of 68\u00b0C. Ethanol, CH3CH2OH (MW= 46 g\/mol) has a boiling point of 78\u00b0C. Mark each of the following statement as True or False. a. Ethanol must have stronger IMF, based on its higher boiling pointb. Ethanol has a higher boiling point because of greater London dispersion forcesc. [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-219814","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/219814","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=219814"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/219814\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=219814"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=219814"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=219814"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}