{"id":230751,"date":"2025-06-10T05:20:27","date_gmt":"2025-06-10T05:20:27","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=230751"},"modified":"2025-06-10T05:20:29","modified_gmt":"2025-06-10T05:20:29","slug":"for-each-pair-of-compounds-listed-check-the-box-next-to-the-one-with-the-higher-boiling-point","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/10\/for-each-pair-of-compounds-listed-check-the-box-next-to-the-one-with-the-higher-boiling-point\/","title":{"rendered":"For each pair of compounds listed, check the box next to the one with the higher boiling point."},"content":{"rendered":"\n

For each pair of compounds listed, check the box next to the one with the higher boiling point. compounds higher boiling point SiCl
SiI
SnH
GeH
CCl
CBr
X 5<\/p>\n\n\n\n

The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n

Here are the correct selections for the compounds with the higher boiling points<\/strong>:<\/p>\n\n\n\n

    \n
  1. SiI\u2084<\/strong> (higher boiling point than SiCl\u2084)<\/li>\n\n\n\n
  2. SnH\u2084<\/strong> (higher boiling point than GeH\u2084)<\/li>\n\n\n\n
  3. CBr\u2084<\/strong> (higher boiling point than CCl\u2084)<\/li>\n<\/ol>\n\n\n\n
    \n\n\n\n

    Explanation <\/h3>\n\n\n\n

    Boiling points are influenced by the strength of intermolecular forces, molecular size, and polarizability. Let’s break down each pair:<\/p>\n\n\n\n

    \n\n\n\n

    1. SiCl\u2084 vs. SiI\u2084<\/strong><\/h4>\n\n\n\n
      \n
    • Both are tetrahalides of silicon with similar molecular geometry (tetrahedral, non-polar), and both experience London dispersion forces<\/strong>.<\/li>\n\n\n\n
    • Iodine atoms are larger and more polarizable than chlorine atoms<\/strong>, leading to stronger dispersion forces in SiI\u2084<\/strong>.<\/li>\n\n\n\n
    • Hence, SiI\u2084<\/strong> has a higher boiling point due to stronger van der Waals interactions.<\/li>\n<\/ul>\n\n\n\n
      \n\n\n\n

      2. SnH\u2084 vs. GeH\u2084<\/strong><\/h4>\n\n\n\n
        \n
      • Both are group 14 hydrides, but SnH\u2084 (stannane)<\/strong> is heavier than GeH\u2084 (germane)<\/strong>.<\/li>\n\n\n\n
      • As molecular weight increases down the group, London dispersion forces<\/strong> become stronger.<\/li>\n\n\n\n
      • Despite being gases at room temperature, SnH\u2084<\/strong> has a higher boiling point than GeH\u2084<\/strong> due to increased mass and polarizability.<\/li>\n<\/ul>\n\n\n\n
        \n\n\n\n

        3. CCl\u2084 vs. CBr\u2084<\/strong><\/h4>\n\n\n\n
          \n
        • Both are non-polar, symmetrical tetrahalides of carbon, so dispersion forces dominate<\/strong>.<\/li>\n\n\n\n
        • Bromine is larger and more polarizable than chlorine, making CBr\u2084<\/strong> capable of stronger London dispersion forces.<\/li>\n\n\n\n
        • Thus, CBr\u2084<\/strong> has a higher boiling point than CCl\u2084<\/strong>.<\/li>\n<\/ul>\n\n\n\n
          \n\n\n\n

          Summary Table:<\/h3>\n\n\n\n
          Compounds<\/th>Higher Boiling Point<\/th><\/tr><\/thead>
          SiCl\u2084 \/ SiI\u2084<\/td>\u2705 SiI\u2084<\/td><\/tr>
          SnH\u2084 \/ GeH\u2084<\/td>\u2705 SnH\u2084<\/td><\/tr>
          CCl\u2084 \/ CBr\u2084<\/td>\u2705 CBr\u2084<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

          These trends are consistent with periodic trends in atomic size and intermolecular forces, particularly dispersion forces which are more pronounced in heavier, more polarizable molecules.<\/p>\n\n\n\n

          \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

          For each pair of compounds listed, check the box next to the one with the higher boiling point. compounds higher boiling point SiClSiISnHGeHCClCBrX 5 The Correct Answer and Explanation is: Here are the correct selections for the compounds with the higher boiling points: Explanation Boiling points are influenced by the strength of intermolecular forces, molecular […]<\/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-230751","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/230751","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=230751"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/230751\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=230751"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=230751"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=230751"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}