{"id":21045,"date":"2025-06-14T21:57:48","date_gmt":"2025-06-14T21:57:48","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=21045"},"modified":"2025-06-14T21:57:50","modified_gmt":"2025-06-14T21:57:50","slug":"show-that-brf4-is-a-non-polar-molecule","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/show-that-brf4-is-a-non-polar-molecule\/","title":{"rendered":"Show that [BrF4] – is a non-polar molecule"},"content":{"rendered":"\n

Show that [BrF4] – is a non-polar molecule.<\/p>\n\n\n\n

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

Answer:<\/h3>\n\n\n\n

The BrF4\u2212\\text{BrF}_4^- ion is a non-polar molecule<\/strong>.<\/p>\n\n\n\n

\n\n\n\n

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

To understand why BrF4\u2212\\text{BrF}_4^- is non-polar, we need to analyze its molecular geometry, the distribution of electron density, and the symmetry of the molecule.<\/p>\n\n\n\n

1. Lewis Structure and Electron Count:<\/strong><\/p>\n\n\n\n

    \n
  • Bromine (Br) is the central atom.<\/li>\n\n\n\n
  • Fluorine (F) atoms: 4 atoms bonded to Br.<\/li>\n\n\n\n
  • Charge: \u22121-1 (extra electron).<\/li>\n<\/ul>\n\n\n\n

    Bromine has 7 valence electrons, each fluorine has 7, and there’s one extra electron due to the negative charge.<\/p>\n\n\n\n

    Total valence electrons = 7+(4\u00d77)+1=7+28+1=367 + (4 \\times 7) + 1 = 7 + 28 + 1 = 36 electrons.<\/p>\n\n\n\n

    2. Electron Pair Arrangement:<\/strong><\/p>\n\n\n\n

      \n
    • Br forms 4 single bonds with F atoms.<\/li>\n\n\n\n
    • Remaining electrons form lone pairs on Br.<\/li>\n\n\n\n
    • Bromine uses 8 electrons for bonding (4 bonds \u00d7 2 electrons).<\/li>\n\n\n\n
    • Leftover electrons: 36 total – 8 bonding = 28 electrons.<\/li>\n\n\n\n
    • These 28 electrons are placed as lone pairs: 3 lone pairs on Br (6 electrons) and the rest on fluorines (which complete their octet).<\/li>\n<\/ul>\n\n\n\n

      So, Br has 4 bonding pairs and 2 lone pairs.<\/p>\n\n\n\n

      3. Molecular Geometry:<\/strong><\/p>\n\n\n\n

      With 4 bonded atoms and 2 lone pairs, the electron geometry is octahedral<\/strong> (6 electron pairs around Br), but the molecular shape<\/strong> (considering only atoms) is square planar<\/strong> because the two lone pairs occupy positions opposite each other to minimize repulsion.<\/p>\n\n\n\n

      4. Symmetry and Polarity:<\/strong><\/p>\n\n\n\n

        \n
      • The square planar shape is highly symmetrical.<\/li>\n\n\n\n
      • The four fluorine atoms are arranged evenly around bromine in a plane.<\/li>\n\n\n\n
      • The lone pairs are above and below the plane, cancelling any dipole moment they might create.<\/li>\n\n\n\n
      • The dipole moments of the Br\u2013F bonds cancel out due to the symmetry.<\/li>\n<\/ul>\n\n\n\n

        Hence, the net dipole moment is zero.<\/p>\n\n\n\n

        5. Conclusion:<\/strong><\/p>\n\n\n\n

        Since the BrF4\u2212\\text{BrF}_4^- ion has a symmetric square planar shape with opposing lone pairs cancelling dipoles, it is non-polar<\/strong>.<\/p>\n\n\n\n

        \n\n\n\n

        Summary:<\/h3>\n\n\n\n
          \n
        • BrF4\u2212\\text{BrF}_4^- has 4 bonding pairs and 2 lone pairs on Br.<\/li>\n\n\n\n
        • Electron geometry is octahedral; molecular shape is square planar.<\/li>\n\n\n\n
        • The symmetry causes the bond dipoles to cancel out.<\/li>\n\n\n\n
        • Therefore, BrF4\u2212\\text{BrF}_4^- is a non-polar<\/strong> molecule despite having polar Br\u2013F bonds.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"

          Show that [BrF4] – is a non-polar molecule. The correct answer and explanation is: Answer: The BrF4\u2212\\text{BrF}_4^- ion is a non-polar molecule. Explanation: To understand why BrF4\u2212\\text{BrF}_4^- is non-polar, we need to analyze its molecular geometry, the distribution of electron density, and the symmetry of the molecule. 1. Lewis Structure and Electron Count: Bromine has […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1],"tags":[],"class_list":["post-21045","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/21045","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/comments?post=21045"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/21045\/revisions"}],"predecessor-version":[{"id":21046,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/21045\/revisions\/21046"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=21045"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=21045"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=21045"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}