{"id":187444,"date":"2025-02-04T19:13:03","date_gmt":"2025-02-04T19:13:03","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=187444"},"modified":"2025-02-04T19:13:05","modified_gmt":"2025-02-04T19:13:05","slug":"is-clo2-asf6-sebr3-i3-o3-icl4-and-xebr4-polar-or-non-polar","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/04\/is-clo2-asf6-sebr3-i3-o3-icl4-and-xebr4-polar-or-non-polar\/","title":{"rendered":"is clo2-, asf6-, sebr3+, i3-, o3, icl4+ and xebr4 polar or non polar"},"content":{"rendered":"\n

is clo2-, asf6-, sebr3+, i3-, o3, icl4+ and xebr4 polar or non polar?<\/p>\n\n\n\n

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

To determine whether the given molecules\/ions are polar or nonpolar<\/strong>, we need to analyze their molecular geometry<\/strong> and electronegativity differences<\/strong>. A molecule is polar if it has an asymmetrical shape<\/strong> that creates a net dipole moment<\/strong>. Conversely, if the dipole moments cancel out due to symmetry<\/strong>, the molecule is nonpolar.<\/p>\n\n\n\n

\n\n\n\n

1. ( ClO_2^- ) (Chlorite ion) – Polar<\/strong><\/h3>\n\n\n\n
    \n
  • Lewis Structure<\/strong>: Bent shape due to lone pairs on chlorine.<\/li>\n\n\n\n
  • Electronegativity<\/strong>: Oxygen is more electronegative than chlorine.<\/li>\n\n\n\n
  • Polarity<\/strong>: The bent shape prevents dipoles from canceling, making ( ClO_2^- ) polar.<\/li>\n<\/ul>\n\n\n\n
    \n\n\n\n

    2. ( AsF_6^- ) (Hexafluoroarsenate) – Nonpolar<\/strong><\/h3>\n\n\n\n
      \n
    • Geometry<\/strong>: Octahedral.<\/li>\n\n\n\n
    • Electronegativity<\/strong>: Fluorine pulls electrons evenly in opposite directions.<\/li>\n\n\n\n
    • Polarity<\/strong>: Since the molecule is symmetric, dipoles cancel, making it nonpolar.<\/li>\n<\/ul>\n\n\n\n
      \n\n\n\n

      3. ( SeBr_3^+ ) (Selenium tribromide cation) – Polar<\/strong><\/h3>\n\n\n\n
        \n
      • Geometry<\/strong>: Trigonal pyramidal due to lone pairs on selenium.<\/li>\n\n\n\n
      • Electronegativity<\/strong>: Bromine is more electronegative than selenium.<\/li>\n\n\n\n
      • Polarity<\/strong>: Asymmetry leads to a net dipole moment, making it polar.<\/li>\n<\/ul>\n\n\n\n
        \n\n\n\n

        4. ( I_3^- ) (Triiodide ion) – Nonpolar<\/strong><\/h3>\n\n\n\n
          \n
        • Geometry<\/strong>: Linear (lone pairs on central iodine).<\/li>\n\n\n\n
        • Electronegativity<\/strong>: Iodine atoms share electrons symmetrically.<\/li>\n\n\n\n
        • Polarity<\/strong>: No net dipole moment due to linear shape, making it nonpolar.<\/li>\n<\/ul>\n\n\n\n
          \n\n\n\n

          5. ( O_3 ) (Ozone) – Polar<\/strong><\/h3>\n\n\n\n
            \n
          • Geometry<\/strong>: Bent due to lone pairs on central oxygen.<\/li>\n\n\n\n
          • Electronegativity<\/strong>: Oxygen has a strong dipole.<\/li>\n\n\n\n
          • Polarity<\/strong>: Asymmetrical shape creates a net dipole, making it polar.<\/li>\n<\/ul>\n\n\n\n
            \n\n\n\n

            6. ( ICl_4^+ ) (Tetrachloroiodate cation) – Polar<\/strong><\/h3>\n\n\n\n
              \n
            • Geometry<\/strong>: See-saw shape due to lone pair on iodine.<\/li>\n\n\n\n
            • Electronegativity<\/strong>: Chlorine is more electronegative than iodine.<\/li>\n\n\n\n
            • Polarity<\/strong>: Asymmetrical shape results in a net dipole, making it polar.<\/li>\n<\/ul>\n\n\n\n
              \n\n\n\n

              7. ( XeBr_4 ) (Xenon tetrabromide) – Nonpolar<\/strong><\/h3>\n\n\n\n
                \n
              • Geometry<\/strong>: Square planar due to lone pairs on xenon.<\/li>\n\n\n\n
              • Electronegativity<\/strong>: Bromine pulls symmetrically.<\/li>\n\n\n\n
              • Polarity<\/strong>: Symmetry cancels out dipoles, making it nonpolar.<\/li>\n<\/ul>\n\n\n\n
                \n\n\n\n

                Final Answer:<\/strong><\/h3>\n\n\n\n
                Molecule\/Ion<\/th>Polarity<\/th><\/tr><\/thead>
                ( ClO_2^- )<\/td>Polar<\/strong><\/td><\/tr>
                ( AsF_6^- )<\/td>Nonpolar<\/strong><\/td><\/tr>
                ( SeBr_3^+ )<\/td>Polar<\/strong><\/td><\/tr>
                ( I_3^- )<\/td>Nonpolar<\/strong><\/td><\/tr>
                ( O_3 )<\/td>Polar<\/strong><\/td><\/tr>
                ( ICl_4^+ )<\/td>Polar<\/strong><\/td><\/tr>
                ( XeBr_4 )<\/td>Nonpolar<\/strong><\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

                Conclusion:<\/strong> Polarity depends on both electronegativity and molecular shape. Molecules with symmetrical geometry (e.g., octahedral, square planar, linear) are generally nonpolar<\/strong>, while asymmetrical ones (bent, trigonal pyramidal, see-saw) tend to be polar<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":"

                is clo2-, asf6-, sebr3+, i3-, o3, icl4+ and xebr4 polar or non polar? The Correct Answer and Explanation is : To determine whether the given molecules\/ions are polar or nonpolar, we need to analyze their molecular geometry and electronegativity differences. A molecule is polar if it has an asymmetrical shape that creates a net dipole […]<\/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-187444","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187444","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=187444"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187444\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=187444"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=187444"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=187444"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}