{"id":36092,"date":"2025-06-25T02:51:58","date_gmt":"2025-06-25T02:51:58","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=36092"},"modified":"2025-06-25T02:51:59","modified_gmt":"2025-06-25T02:51:59","slug":"for-pbr5-in-part-2-which-of-the-following-options-correctly-describe-the-overall-polarity","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/for-pbr5-in-part-2-which-of-the-following-options-correctly-describe-the-overall-polarity\/","title":{"rendered":"for PBr5 in Part 2, which of the following options correctly describe the overall polarity"},"content":{"rendered":"\n

for PBr5 in Part 2, which of the following options correctly describe the overall polarity? Choose one or more: Each Br bond is polar. Two bond dipoles can cancel, as they are at 180\u00c2\u00b0 to each other. The lone pair contributes to the overall polarity of the molecule. None of the bond dipoles cancel. Gor17CUSTIONS COMPLETED 06\/17 View Solution SUBMLAN Aenfch
Given the table of electronegativities provided and the shape predicted for PBr5 in Part 2, which of the following options correctly describe the overall polarity? Choose one or more: Each Br bond is polar. Two bond dipoles can cancel, as they are at 180\u00c2\u00b0 to each other. The lone pair contributes to the overall polarity of the molecule. None of the bond dipoles cancel. Gor17CUSTIONS COMPLETED 06\/17 View Solution SUBMLAN Aenfch<\/p>\n\n\n\n

\"\"<\/figure>\n\n\n\n

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

To determine the correct options about the polarity of PBr\u2085 (phosphorus pentabromide)<\/strong>, we need to evaluate both its molecular shape<\/strong> and bond polarity<\/strong>, using the electronegativity table provided.<\/p>\n\n\n\n

Step 1: Electronegativity Difference<\/h3>\n\n\n\n

From the chart:<\/p>\n\n\n\n

    \n
  • Electronegativity of P (Phosphorus)<\/strong> = 2.1<\/li>\n\n\n\n
  • Electronegativity of Br (Bromine)<\/strong> = 2.8
    The difference = 2.8 – 2.1 = 0.7<\/strong>, which indicates polar covalent bonds<\/strong>.<\/li>\n<\/ul>\n\n\n\n

    So, each P\u2013Br bond is polar<\/strong>.<\/p>\n\n\n\n

    Step 2: Molecular Geometry of PBr\u2085<\/h3>\n\n\n\n

    PBr\u2085 has:<\/p>\n\n\n\n

      \n
    • 5 bonding pairs<\/li>\n\n\n\n
    • 0 lone pairs on phosphorus<\/li>\n<\/ul>\n\n\n\n

      This gives it a trigonal bipyramidal<\/strong> shape:<\/p>\n\n\n\n

        \n
      • Three Br atoms in the equatorial positions (120\u00b0 apart)<\/li>\n\n\n\n
      • Two Br atoms in the axial positions (180\u00b0 apart from each other and 90\u00b0 from equatorial atoms)<\/li>\n<\/ul>\n\n\n\n

        Step 3: Polarity of the Molecule<\/h3>\n\n\n\n

        Even though the P\u2013Br bonds are polar<\/strong>, the molecule’s symmetrical trigonal bipyramidal shape<\/strong> allows the dipole moments to cancel out. The vector sum of the dipoles results in a nonpolar molecule<\/strong>.<\/p>\n\n\n\n

        Also:<\/p>\n\n\n\n

          \n
        • There is no lone pair<\/strong> on the central atom, so no lone-pair-induced asymmetry.<\/li>\n\n\n\n
        • The equatorial and axial dipoles<\/strong> are balanced and distributed symmetrically.<\/li>\n<\/ul>\n\n\n\n

          Correct Options:<\/h3>\n\n\n\n

          \u2705 Each P\u2013Br bond is polar<\/strong>
          \u274c Two bond dipoles can cancel, as they are at 180\u00b0 to each other<\/strong> \u2192 Partially true for axial bonds, but oversimplified
          \u274c The lone pair contributes to the overall polarity of the molecule<\/strong> \u2192 Incorrect because there is no lone pair<\/strong>
          \u274c None of the bond dipoles cancel<\/strong> \u2192 Incorrect, they do cancel<\/strong> due to symmetry<\/p>\n\n\n\n

          Final Answer:<\/h3>\n\n\n\n
            \n
          • \u2705 Each P\u2013Br bond is polar<\/strong><\/li>\n<\/ul>\n\n\n\n
            \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

            for PBr5 in Part 2, which of the following options correctly describe the overall polarity? Choose one or more: Each Br bond is polar. Two bond dipoles can cancel, as they are at 180\u00c2\u00b0 to each other. The lone pair contributes to the overall polarity of the molecule. None of the bond dipoles cancel. Gor17CUSTIONS […]<\/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-36092","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/36092","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=36092"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/36092\/revisions"}],"predecessor-version":[{"id":36095,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/36092\/revisions\/36095"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=36092"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=36092"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=36092"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}