{"id":192786,"date":"2025-02-18T08:42:38","date_gmt":"2025-02-18T08:42:38","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=192786"},"modified":"2025-02-18T08:43:03","modified_gmt":"2025-02-18T08:43:03","slug":"use-vsepr-theory-to-predict-the-electron-pair-geometry-and-the-molecular-geometry-ofaa-xef5","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/18\/use-vsepr-theory-to-predict-the-electron-pair-geometry-and-the-molecular-geometry-ofaa-xef5\/","title":{"rendered":"Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of XeF5+"},"content":{"rendered":"\n

Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of\u00c3\u201a\u00c2 XeF5+.
Electron-pair geometry =\u00c3\u201a\u00c2 square pyramidal; molecular geometry =\u00c3\u201a\u00c2 trigonal bipyramidal
Electron-pair geometry =\u00c3\u201a\u00c2 trigonal bipyramidal; molecular geometry =\u00c3\u201a\u00c2 see-saw
Electron-pair geometry =\u00c3\u201a\u00c2 trigonal bipyramidal; molecular geometry =\u00c3\u201a\u00c2 trigonal bipyramidal
Electron-pair geometry =\u00c3\u201a\u00c2 octahedral; molecular geometry =\u00c3\u201a\u00c2 trigonal bipyramidal
Electron-pair geometry =\u00c3\u201a\u00c2 octahedral; molecular geometry =\u00c3\u201a\u00c2 square pyramidal<\/p>\n\n\n\n

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

The correct answer is:<\/p>\n\n\n\n

Electron-pair geometry = octahedral; molecular geometry = square pyramidal.<\/strong><\/p>\n\n\n\n

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

The VSEPR (Valence Shell Electron Pair Repulsion) theory helps predict the shapes of molecules by considering electron pairs around a central atom. In this case, the molecule is XeF\u2085\u207a<\/strong>, which is a xenon pentafluoride cation.<\/p>\n\n\n\n

    \n
  1. Determine the electron pairs around the central atom<\/strong>:<\/li>\n<\/ol>\n\n\n\n
      \n
    • Xenon (Xe) is in Group 18 and thus has 8 valence electrons.<\/li>\n\n\n\n
    • Each fluorine atom contributes 1 electron, and since there are 5 fluorine atoms, this adds 5 electrons to the valence shell of xenon.<\/li>\n\n\n\n
    • The cation (XeF\u2085\u207a) means it has lost one electron, so the total electron count around xenon is:\n
        \n
      • 8 (from Xe) + 5 (from F atoms) – 1 (due to the +1 charge) = 12 electrons.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
      • These 12 electrons will be arranged into pairs, and the xenon will have 6 electron pairs (since 12 \u00f7 2 = 6).<\/li>\n<\/ul>\n\n\n\n
          \n
        1. Electron-pair geometry<\/strong>:<\/li>\n<\/ol>\n\n\n\n
            \n
          • With 6 electron pairs, the ideal arrangement is octahedral, as this minimizes the repulsion between electron pairs.<\/li>\n<\/ul>\n\n\n\n
              \n
            1. Molecular geometry<\/strong>:<\/li>\n<\/ol>\n\n\n\n
                \n
              • In the case of the molecular geometry, we focus on the positions of the atoms, not the electron pairs.<\/li>\n\n\n\n
              • Since there are 5 fluorine atoms and 1 lone pair (from the remaining electron), the molecular geometry will be square pyramidal<\/strong>. The 5 fluorine atoms occupy the corners of the square base, and the lone pair occupies the apical position, distorting the geometry from a perfect octahedron to a square pyramid.<\/li>\n<\/ul>\n\n\n\n

                The electron-pair geometry is octahedral, and the molecular geometry, due to the lone pair, is square pyramidal.<\/p>\n\n\n\n

                I will now generate an image illustrating this structure.<\/p>\n\n\n\n

                Here is an image representing the octahedral structure of XeF\u2085\u207a, showing the square pyramidal molecular geometry. You can see how the 5 fluorine atoms are arranged in a square base, with one lone pair occupying the apical position, resulting in this particular molecular geometry.<\/p>\n\n\n\n

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

                Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of\u00c3\u201a\u00c2 XeF5+.Electron-pair geometry =\u00c3\u201a\u00c2 square pyramidal; molecular geometry =\u00c3\u201a\u00c2 trigonal bipyramidalElectron-pair geometry =\u00c3\u201a\u00c2 trigonal bipyramidal; molecular geometry =\u00c3\u201a\u00c2 see-sawElectron-pair geometry =\u00c3\u201a\u00c2 trigonal bipyramidal; molecular geometry =\u00c3\u201a\u00c2 trigonal bipyramidalElectron-pair geometry =\u00c3\u201a\u00c2 octahedral; molecular geometry =\u00c3\u201a\u00c2 trigonal bipyramidalElectron-pair geometry =\u00c3\u201a\u00c2 octahedral; molecular geometry =\u00c3\u201a\u00c2 square […]<\/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-192786","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/192786","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=192786"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/192786\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=192786"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=192786"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=192786"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}