{"id":166648,"date":"2024-11-13T23:33:04","date_gmt":"2024-11-13T23:33:04","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=166648"},"modified":"2024-11-13T23:33:07","modified_gmt":"2024-11-13T23:33:07","slug":"what-molecular-geometry-would-be-expected-for-f2-and-hf","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/13\/what-molecular-geometry-would-be-expected-for-f2-and-hf\/","title":{"rendered":"What molecular geometry would be expected for f2 and hf"},"content":{"rendered":"\n

What molecular geometry would be expected for f2 and hf?<\/p>\n\n\n\n

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

The molecular geometries of F\u2082 (fluorine gas)<\/strong> and HF (hydrogen fluoride)<\/strong> can be determined based on their Lewis structures, the number of electron pairs around the central atoms, and the application of the Valence Shell Electron Pair Repulsion (VSEPR) theory.<\/p>\n\n\n\n

F\u2082 (Fluorine Gas):<\/h3>\n\n\n\n
    \n
  • Molecular formula<\/strong>: F\u2082<\/li>\n\n\n\n
  • Lewis structure<\/strong>: Each fluorine atom has seven valence electrons and shares one electron with the other fluorine atom to form a single covalent bond.<\/li>\n\n\n\n
  • Electron regions<\/strong>: There are no lone pairs on the central atoms (the fluorine atoms). Since each fluorine atom is bonded to another fluorine atom with a single bond, and there are no lone pairs, the structure is relatively simple.<\/li>\n\n\n\n
  • VSEPR geometry<\/strong>: According to VSEPR theory, the two fluorine atoms are repelling each other with a single bonding pair. The optimal molecular geometry for two atoms with no lone pairs around the central atom is linear<\/strong>. The bond angle between the two fluorine atoms is 180\u00b0<\/strong>.<\/li>\n<\/ul>\n\n\n\n

    Thus, the molecular geometry of F\u2082<\/strong> is linear<\/strong>.<\/p>\n\n\n\n

    HF (Hydrogen Fluoride):<\/h3>\n\n\n\n
      \n
    • Molecular formula<\/strong>: HF<\/li>\n\n\n\n
    • Lewis structure<\/strong>: In HF, hydrogen (which only has one valence electron) bonds with fluorine (which has seven valence electrons). The bond between them is a single covalent bond. Fluorine will have three lone pairs of electrons.<\/li>\n\n\n\n
    • Electron regions<\/strong>: There are two regions of electron density around fluorine \u2014 one bonding pair and three lone pairs. The electron geometry would be based on the total regions of electron density around the fluorine atom, which is tetrahedral<\/strong>. However, since the lone pairs are not involved in bonding, they are not counted in the molecular geometry.<\/li>\n\n\n\n
    • VSEPR geometry<\/strong>: The molecular geometry is determined by the positions of the atoms only. With one bonding pair and three lone pairs, the molecular geometry is linear<\/strong>, with a bond angle of approximately 180\u00b0<\/strong>.<\/li>\n<\/ul>\n\n\n\n

      Thus, the molecular geometry of HF<\/strong> is also linear<\/strong>, even though the electron geometry is tetrahedral.<\/p>\n\n\n\n

      Conclusion:<\/h3>\n\n\n\n
        \n
      • The molecular geometry of F\u2082<\/strong> is linear<\/strong>.<\/li>\n\n\n\n
      • The molecular geometry of HF<\/strong> is also linear<\/strong>, despite having lone pairs on the fluorine atom, because the geometry concerns the arrangement of atoms, not electron pairs.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"

        What molecular geometry would be expected for f2 and hf? The Correct Answer and Explanation is: The molecular geometries of F\u2082 (fluorine gas) and HF (hydrogen fluoride) can be determined based on their Lewis structures, the number of electron pairs around the central atoms, and the application of the Valence Shell Electron Pair Repulsion (VSEPR) […]<\/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-166648","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/166648","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=166648"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/166648\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=166648"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=166648"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=166648"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}