{"id":199055,"date":"2025-03-10T17:18:19","date_gmt":"2025-03-10T17:18:19","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=199055"},"modified":"2025-03-10T17:18:21","modified_gmt":"2025-03-10T17:18:21","slug":"determine-the-molecular-geometry-of-brf5","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/10\/determine-the-molecular-geometry-of-brf5\/","title":{"rendered":"Determine the molecular geometry of BrF5"},"content":{"rendered":"\n

Determine the molecular geometry of BrF5.<\/p>\n\n\n\n

seesaw<\/p>\n\n\n\n

trigonal bipyramidal<\/p>\n\n\n\n

square pyramidal<\/p>\n\n\n\n

octahedral<\/p>\n\n\n\n

The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n

The correct molecular geometry of BrF\u2085 (Bromine Pentafluoride)<\/strong> is square pyramidal<\/strong>.<\/p>\n\n\n\n

Explanation (300 words)<\/strong><\/h3>\n\n\n\n

1. Determining Electron Geometry Using VSEPR Theory<\/strong><\/h4>\n\n\n\n

The molecular geometry of BrF\u2085<\/strong> can be determined using the Valence Shell Electron Pair Repulsion (VSEPR) theory<\/strong>, which helps predict molecular shapes based on electron pair repulsions.<\/p>\n\n\n\n

    \n
  • Step 1: Count the Valence Electrons of Bromine<\/strong>
    Bromine (Br<\/strong>) belongs to Group 17<\/strong> in the periodic table, so it has 7 valence electrons<\/strong>.<\/li>\n\n\n\n
  • Step 2: Count the Valence Electrons from Fluorine Atoms<\/strong>
    Each fluorine (F)<\/strong> contributes 1 valence electron<\/strong>, and since there are five fluorine atoms<\/strong>, the total electrons from fluorine are 5 \u00d7 1 = 5 electrons<\/strong>.<\/li>\n\n\n\n
  • Step 3: Determine the Total Valence Electrons<\/strong><\/li>\n\n\n\n
  • Br = 7 electrons<\/strong><\/li>\n\n\n\n
  • F\u2085 = 5 \u00d7 1 = 5 electrons<\/strong><\/li>\n\n\n\n
  • Total = 7 + 5 = 12 electrons (6 electron pairs)<\/strong><\/li>\n<\/ul>\n\n\n\n

    2. Predicting the Electron Pair Arrangement<\/strong><\/h4>\n\n\n\n
      \n
    • The central Br atom<\/strong> has six electron pairs<\/strong> (five bonding pairs from Br\u2013F bonds and one lone pair).<\/li>\n\n\n\n
    • The electron geometry<\/strong> is based on six electron pairs, which corresponds to an octahedral arrangement<\/strong>.<\/li>\n<\/ul>\n\n\n\n

      3. Determining the Molecular Geometry<\/strong><\/h4>\n\n\n\n
        \n
      • Since one of the six electron pairs is a lone pair<\/strong>, the molecular geometry deviates from the octahedral shape<\/strong>.<\/li>\n\n\n\n
      • The lone pair repels the bonded atoms, distorting the shape into a square pyramidal geometry<\/strong>.<\/li>\n<\/ul>\n\n\n\n

        4. Confirming Square Pyramidal Shape<\/strong><\/h4>\n\n\n\n
          \n
        • In square pyramidal geometry<\/strong>, five fluorine atoms form a square base, and the lone pair is positioned at the axial position.<\/li>\n\n\n\n
        • The bond angles are slightly less than 90\u00b0<\/strong> due to lone pair repulsion.<\/li>\n<\/ul>\n\n\n\n

          Final Answer:<\/strong> Square Pyramidal<\/strong><\/h3>\n","protected":false},"excerpt":{"rendered":"

          Determine the molecular geometry of BrF5. seesaw trigonal bipyramidal square pyramidal octahedral The correct answer and explanation is : The correct molecular geometry of BrF\u2085 (Bromine Pentafluoride) is square pyramidal. Explanation (300 words) 1. Determining Electron Geometry Using VSEPR Theory The molecular geometry of BrF\u2085 can be determined using the Valence Shell Electron Pair Repulsion […]<\/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-199055","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/199055","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=199055"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/199055\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=199055"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=199055"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=199055"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}