{"id":198919,"date":"2025-03-10T14:43:45","date_gmt":"2025-03-10T14:43:45","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=198919"},"modified":"2025-03-10T14:43:47","modified_gmt":"2025-03-10T14:43:47","slug":"is-brf4-polar-or-nonpolar","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/10\/is-brf4-polar-or-nonpolar\/","title":{"rendered":"Is BrF4 – polar or nonpolar"},"content":{"rendered":"\n

Is BrF4 – polar or nonpolar<\/p>\n\n\n\n

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

BrF\u2084\u207b (Bromine Tetrafluoride) – Polar or Nonpolar?<\/strong>
Answer:<\/strong> BrF\u2084\u207b is nonpolar<\/strong>.<\/p>\n\n\n\n

Explanation:<\/strong><\/h3>\n\n\n\n
    \n
  1. Lewis Structure and Electron Arrangement:<\/strong><\/li>\n<\/ol>\n\n\n\n
      \n
    • Bromine (Br) has 7 valence electrons<\/strong>.<\/li>\n\n\n\n
    • Each fluorine (F) atom contributes 1 valence electron<\/strong>, and there are four fluorine atoms<\/strong>, adding 4 electrons<\/strong>.<\/li>\n\n\n\n
    • The negative charge (-1)<\/strong> adds one more electron<\/strong>.<\/li>\n\n\n\n
    • The total number of valence electrons = 7 + 4(7) + 1 = 36<\/strong> electrons.<\/li>\n<\/ul>\n\n\n\n
        \n
      1. Molecular Geometry and Hybridization:<\/strong><\/li>\n<\/ol>\n\n\n\n
          \n
        • The bromine atom is the central atom<\/strong> with four bonding pairs<\/strong> (Br\u2013F bonds).<\/li>\n\n\n\n
        • There are two lone pairs<\/strong> on the bromine atom.<\/li>\n\n\n\n
        • Using VSEPR (Valence Shell Electron Pair Repulsion) theory<\/strong>, the molecular shape is square planar<\/strong>, which is derived from the octahedral electron geometry.<\/li>\n<\/ul>\n\n\n\n
            \n
          1. Symmetry and Dipole Moments:<\/strong><\/li>\n<\/ol>\n\n\n\n
              \n
            • The square planar geometry<\/strong> (with lone pairs positioned 180\u00b0 apart) makes the molecule highly symmetrical<\/strong>.<\/li>\n\n\n\n
            • Although Br\u2013F bonds are polar<\/strong> due to the electronegativity difference<\/strong> (Fluorine = 3.98, Bromine = 2.96), the dipole moments cancel out<\/strong> because of the symmetric arrangement.<\/li>\n\n\n\n
            • As a result, the net dipole moment is zero<\/strong>, making BrF\u2084\u207b nonpolar<\/strong>.<\/li>\n<\/ul>\n\n\n\n
                \n
              1. Conclusion:<\/strong>
                Even though individual Br\u2013F bonds are polar, the overall molecular symmetry cancels out<\/strong> the dipole moments, making BrF\u2084\u207b a nonpolar ion<\/strong>.<\/li>\n<\/ol>\n","protected":false},"excerpt":{"rendered":"

                Is BrF4 – polar or nonpolar The correct answer and explanation is : BrF\u2084\u207b (Bromine Tetrafluoride) – Polar or Nonpolar?Answer: BrF\u2084\u207b is nonpolar. Explanation:<\/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-198919","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198919","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=198919"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198919\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=198919"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=198919"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=198919"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}