{"id":225949,"date":"2025-06-04T18:51:37","date_gmt":"2025-06-04T18:51:37","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=225949"},"modified":"2025-06-04T18:51:39","modified_gmt":"2025-06-04T18:51:39","slug":"which-molecule-is-most-polar","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/04\/which-molecule-is-most-polar\/","title":{"rendered":"Which molecule is most polar"},"content":{"rendered":"\n

Which molecule is most polar? CHF3, CF4, CClF3, CCl4<\/p>\n\n\n\n

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

The most polar molecule among CHF\u2083, CF\u2084, CClF\u2083, and CCl\u2084<\/strong> is CHF\u2083 (fluoroform)<\/strong>.<\/p>\n\n\n\n

\n\n\n\n

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

To determine which molecule is most polar, we need to understand molecular polarity<\/strong>, which is influenced by two main factors:<\/p>\n\n\n\n

    \n
  1. Electronegativity differences<\/strong> between atoms in a bond.<\/li>\n\n\n\n
  2. Molecular geometry<\/strong>, which affects how individual bond dipoles add or cancel out.<\/li>\n<\/ol>\n\n\n\n
    \n\n\n\n

    1. Molecular Shapes and Symmetry<\/strong><\/h3>\n\n\n\n

    All four molecules are tetrahedral<\/strong> in geometry since the central atom (carbon) forms four single bonds with surrounding atoms.<\/p>\n\n\n\n

      \n
    • CF\u2084 (carbon tetrafluoride)<\/strong> and CCl\u2084 (carbon tetrachloride)<\/strong> are symmetrical<\/strong> molecules. All four substituents are the same, so the individual bond dipoles cancel out. Thus, both are non-polar<\/strong>.<\/li>\n\n\n\n
    • CHF\u2083<\/strong> and CClF\u2083<\/strong> are asymmetrical<\/strong>, with one different atom among the four substituents. This asymmetry leads to a net dipole moment<\/strong>, making them polar molecules<\/strong>.<\/li>\n<\/ul>\n\n\n\n
      \n\n\n\n

      2. Electronegativity Considerations<\/strong><\/h3>\n\n\n\n

      Electronegativity values:<\/p>\n\n\n\n

        \n
      • F (fluorine): 3.98<\/li>\n\n\n\n
      • Cl (chlorine): 3.16<\/li>\n\n\n\n
      • H (hydrogen): 2.20<\/li>\n\n\n\n
      • C (carbon): 2.55<\/li>\n<\/ul>\n\n\n\n

        In CHF\u2083<\/strong>, the C\u2013F bonds are highly polar due to the large electronegativity difference. The single C\u2013H bond is much less polar and does not cancel<\/strong> the strong C\u2013F dipoles, resulting in a strong net dipole<\/strong>.<\/p>\n\n\n\n

        In CClF\u2083<\/strong>, the dipole of the lone C\u2013Cl bond partially cancels the dipoles from the three C\u2013F bonds, but because Cl is more electronegative than H, the cancellation is more effective compared to CHF\u2083, making CClF\u2083 less polar<\/strong> than CHF\u2083.<\/p>\n\n\n\n

        \n\n\n\n

        Conclusion<\/strong><\/h3>\n\n\n\n
          \n
        • Most polar<\/strong>: CHF\u2083<\/strong>, due to its strong C\u2013F dipoles and the low polarity of the C\u2013H bond, which fails to cancel out the fluorine’s pull.<\/li>\n\n\n\n
        • Least polar (non-polar)<\/strong>: CF\u2084<\/strong> and CCl\u2084<\/strong>, due to their perfect symmetry.<\/li>\n\n\n\n
        • Intermediate<\/strong>: CClF\u2083<\/strong>, polar but less than CHF\u2083.<\/li>\n<\/ul>\n\n\n\n

          Thus, CHF\u2083 is the most polar molecule<\/strong> among the four.<\/p>\n\n\n\n

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

          Which molecule is most polar? CHF3, CF4, CClF3, CCl4 The Correct Answer and Explanation is: The most polar molecule among CHF\u2083, CF\u2084, CClF\u2083, and CCl\u2084 is CHF\u2083 (fluoroform). Explanation To determine which molecule is most polar, we need to understand molecular polarity, which is influenced by two main factors: 1. Molecular Shapes and Symmetry All […]<\/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-225949","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/225949","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=225949"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/225949\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=225949"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=225949"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=225949"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}