{"id":187346,"date":"2025-02-04T08:15:17","date_gmt":"2025-02-04T08:15:17","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=187346"},"modified":"2025-02-04T08:15:20","modified_gmt":"2025-02-04T08:15:20","slug":"rank-these-compounds-in-order-of-increasing-boiling","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/04\/rank-these-compounds-in-order-of-increasing-boiling\/","title":{"rendered":"Rank these compounds in order of increasing boiling"},"content":{"rendered":"\n<p>1.Rank these compounds in order of increasing boiling<\/p>\n\n\n\n<p>point:<\/p>\n\n\n\n<p>(a) fluorine, F2;<\/p>\n\n\n\n<p>(b) hydrogen fluoride, HF;<\/p>\n\n\n\n<p>(c) hydrogen chloride, HCl.<\/p>\n\n\n\n<ol start=\"2\" class=\"wp-block-list\">\n<li>Rank these compounds in order of increasing symmetry:<\/li>\n<\/ol>\n\n\n\n<p>(a) CH4,<\/p>\n\n\n\n<p>(b) NH3,<\/p>\n\n\n\n<p>(c) H2O.<\/p>\n\n\n\n<ol start=\"3\" class=\"wp-block-list\">\n<li>Rank these compounds in order of increasing boiling point:<\/li>\n<\/ol>\n\n\n\n<p>(a) CH4,<\/p>\n\n\n\n<p>(b) NH3,<\/p>\n\n\n\n<p>(c) H2O.<\/p>\n\n\n\n<ol start=\"4\" class=\"wp-block-list\">\n<li>How do the electron-dot structures of elements in the same group in the periodic table compare with one another?<\/li>\n\n\n\n<li>How many more electrons can fit within the valence shell of a fluorine atom?<\/li>\n\n\n\n<li>How many more electrons can fit within the valence shell of a hydrogen atom?<\/li>\n\n\n\n<li>How is the number of unpaired valence electrons in an atom related to the number of bonds that the atom can form? 8. What happens when hydrogen\u2019s electron gets close to the<\/li>\n<\/ol>\n\n\n\n<p>valence shell of a fluorine atom?<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Answers and Explanation<\/h3>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>1. Ranking Compounds by Boiling Point (Increasing Order)<\/strong><\/h4>\n\n\n\n<p>Boiling point is influenced by intermolecular forces (London dispersion, dipole-dipole, and hydrogen bonding).<\/p>\n\n\n\n<p><strong>Ranking:<\/strong><br><strong>Fluorine (F\u2082) &lt; Hydrogen chloride (HCl) &lt; Hydrogen fluoride (HF)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Fluorine (F\u2082)<\/strong> has weak London dispersion forces, leading to a very low boiling point (~\u2212188\u00b0C).<\/li>\n\n\n\n<li><strong>Hydrogen chloride (HCl)<\/strong> exhibits dipole-dipole interactions, increasing its boiling point (~\u221285\u00b0C).<\/li>\n\n\n\n<li><strong>Hydrogen fluoride (HF)<\/strong> has hydrogen bonding, the strongest intermolecular force, leading to the highest boiling point (~19.5\u00b0C).<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>2. Ranking Compounds by Symmetry (Increasing Order)<\/strong><\/h4>\n\n\n\n<p>Molecular symmetry is influenced by shape and bond angles.<\/p>\n\n\n\n<p><strong>Ranking:<\/strong><br><strong>H\u2082O &lt; NH\u2083 &lt; CH\u2084<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Water (H\u2082O)<\/strong> has a bent shape due to two lone pairs, making it the least symmetrical.<\/li>\n\n\n\n<li><strong>Ammonia (NH\u2083)<\/strong> has a trigonal pyramidal shape with one lone pair, giving it intermediate symmetry.<\/li>\n\n\n\n<li><strong>Methane (CH\u2084)<\/strong> is tetrahedral, the most symmetrical structure.<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>3. Ranking Compounds by Boiling Point (Increasing Order)<\/strong><\/h4>\n\n\n\n<p><strong>CH\u2084 &lt; NH\u2083 &lt; H\u2082O<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Methane (CH\u2084)<\/strong> has weak London dispersion forces, leading to a very low boiling point (~\u2212161\u00b0C).<\/li>\n\n\n\n<li><strong>Ammonia (NH\u2083)<\/strong> exhibits hydrogen bonding, but only one hydrogen bond per molecule (~\u221233\u00b0C).<\/li>\n\n\n\n<li><strong>Water (H\u2082O)<\/strong> has extensive hydrogen bonding, leading to the highest boiling point (~100\u00b0C).<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>4. Electron-Dot Structures in the Same Group<\/strong><\/h4>\n\n\n\n<p>Elements in the same group have <strong>the same number of valence electrons<\/strong>, which determines their chemical behavior. For example, all Group 17 (halogens) have 7 valence electrons, forming similar electron-dot structures.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>5. Additional Electrons in Fluorine\u2019s Valence Shell<\/strong><\/h4>\n\n\n\n<p>Fluorine has <strong>7 valence electrons<\/strong> and can hold <strong>8<\/strong> in total. Thus, it can accommodate <strong>1 more electron<\/strong> to complete its octet.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>6. Additional Electrons in Hydrogen\u2019s Valence Shell<\/strong><\/h4>\n\n\n\n<p>Hydrogen has <strong>1 valence electron<\/strong> and follows the <strong>duet rule<\/strong> (maximum of 2 electrons). It can hold <strong>1 more electron<\/strong> to be stable.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>7. Unpaired Valence Electrons and Bonding<\/strong><\/h4>\n\n\n\n<p>The number of <strong>unpaired valence electrons<\/strong> determines an atom\u2019s <strong>bonding capacity<\/strong>:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Carbon (C) has 4 unpaired electrons \u2192 forms 4 bonds<\/strong><\/li>\n\n\n\n<li><strong>Nitrogen (N) has 3 unpaired electrons \u2192 forms 3 bonds<\/strong><\/li>\n\n\n\n<li><strong>Oxygen (O) has 2 unpaired electrons \u2192 forms 2 bonds<\/strong><\/li>\n<\/ul>\n\n\n\n<p>This principle helps predict molecular structures.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>8. Interaction of Hydrogen\u2019s Electron with Fluorine<\/strong><\/h4>\n\n\n\n<p>When hydrogen\u2019s electron approaches fluorine, a <strong>covalent bond<\/strong> forms. Fluorine\u2019s high electronegativity <strong>attracts hydrogen\u2019s electron<\/strong>, completing its octet. This results in <strong>hydrogen fluoride (HF),<\/strong> where hydrogen achieves stability by sharing its electron.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Detailed Explanation (300 Words)<\/strong><\/h3>\n\n\n\n<p>Boiling points of substances are determined by intermolecular forces. Fluorine (F\u2082) has weak London dispersion forces and the lowest boiling point. Hydrogen chloride (HCl) has stronger dipole-dipole interactions due to its polarity. Hydrogen fluoride (HF) exhibits hydrogen bonding, the strongest force, giving it the highest boiling point.<\/p>\n\n\n\n<p>Symmetry depends on molecular shape. Water (H\u2082O) is <strong>bent<\/strong> due to lone pairs, making it the least symmetrical. Ammonia (NH\u2083) is <strong>trigonal pyramidal<\/strong> with one lone pair. Methane (CH\u2084) is <strong>tetrahedral<\/strong>, making it the most symmetrical.<\/p>\n\n\n\n<p>Boiling points of CH\u2084, NH\u2083, and H\u2082O follow the same intermolecular force pattern: CH\u2084 (London dispersion) has the lowest, NH\u2083 (hydrogen bonding) is intermediate, and H\u2082O (strong hydrogen bonding) is the highest.<\/p>\n\n\n\n<p>Elements in the same periodic group have the same <strong>valence electron configuration<\/strong>, affecting their reactivity. Fluorine, for instance, has <strong>7 valence electrons<\/strong> and needs <strong>1 more<\/strong> for stability. Hydrogen, following the <strong>duet rule<\/strong>, can hold <strong>only one more electron<\/strong>.<\/p>\n\n\n\n<p>The number of unpaired valence electrons dictates how many bonds an atom can form. Carbon has <strong>four<\/strong>, allowing it to form <strong>four covalent bonds<\/strong>, while oxygen forms <strong>two<\/strong>.<\/p>\n\n\n\n<p>When hydrogen\u2019s electron nears fluorine, a <strong>highly polar<\/strong> bond forms, as fluorine strongly attracts electrons. This results in <strong>HF<\/strong>, where fluorine\u2019s <strong>electronegativity<\/strong> causes a <strong>partial negative charge<\/strong>, while hydrogen becomes <strong>partially positive<\/strong>. This explains HF\u2019s high boiling point and strong intermolecular forces.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>1.Rank these compounds in order of increasing boiling point: (a) fluorine, F2; (b) hydrogen fluoride, HF; (c) hydrogen chloride, HCl. (a) CH4, (b) NH3, (c) H2O. (a) CH4, (b) NH3, (c) H2O. valence shell of a fluorine atom? The Correct Answer and Explanation is : Answers and Explanation 1. Ranking Compounds by Boiling Point (Increasing [&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-187346","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187346","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=187346"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187346\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=187346"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=187346"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=187346"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}