{"id":267012,"date":"2025-07-23T08:41:54","date_gmt":"2025-07-23T08:41:54","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=267012"},"modified":"2025-07-23T08:41:57","modified_gmt":"2025-07-23T08:41:57","slug":"predict-the-molecular-structure-and-bond-angles-for-each-molecule-or-ion-given-below","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/23\/predict-the-molecular-structure-and-bond-angles-for-each-molecule-or-ion-given-below\/","title":{"rendered":"Predict the molecular structure and bond angles for each molecule or ion given below"},"content":{"rendered":"\n

Predict the molecular structure and bond angles for each molecule or ion given below: PO43-: tetrahedral XeO4: tetrahedral POCl3: trigonal pyramid CIO4: tetrahedral CIO3-: tetrahedral SO3: trigonal pyramid NF3: V-shaped SO42-: tetrahedral molecular structure bond angles<\/p>\n\n\n\n

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

Let’s break down each molecule or ion:<\/p>\n\n\n\n

    \n
  1. PO4^3- (Phosphate ion)<\/strong>:\n
      \n
    • Molecular structure<\/strong>: Tetrahedral.<\/li>\n\n\n\n
    • Bond angles<\/strong>: Approximately 109.5\u00b0.<\/li>\n\n\n\n
    • Explanation: In PO4^3-, the central phosphorus atom is bonded to four oxygen atoms, with each oxygen carrying a negative charge. This leads to a tetrahedral structure due to electron pair repulsion, where the bond angles are close to 109.5\u00b0.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
    • XeO4 (Xenon tetroxide)<\/strong>:\n
        \n
      • Molecular structure<\/strong>: Tetrahedral.<\/li>\n\n\n\n
      • Bond angles<\/strong>: Approximately 109.5\u00b0.<\/li>\n\n\n\n
      • Explanation: Xenon is in the center, bonded to four oxygen atoms. The xenon atom in XeO4 has no lone pairs, so the molecule adopts a tetrahedral geometry, similar to methane, with bond angles of around 109.5\u00b0.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
      • POCl3 (Phosphorus trichloride oxide)<\/strong>:\n
          \n
        • Molecular structure<\/strong>: Trigonal pyramid.<\/li>\n\n\n\n
        • Bond angles<\/strong>: Approximately 107\u00b0.<\/li>\n\n\n\n
        • Explanation: The phosphorus atom is surrounded by three chlorine atoms and one lone pair. This leads to a trigonal pyramidal structure, with bond angles slightly less than 109.5\u00b0, approximately 107\u00b0 due to the lone pair.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
        • ClO4- (Perchlorate ion)<\/strong>:\n
            \n
          • Molecular structure<\/strong>: Tetrahedral.<\/li>\n\n\n\n
          • Bond angles<\/strong>: Approximately 109.5\u00b0.<\/li>\n\n\n\n
          • Explanation: The central chlorine atom is bonded to four oxygen atoms in a tetrahedral arrangement. Since there are no lone pairs on the chlorine atom, the bond angles remain around 109.5\u00b0.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
          • ClO3- (Chlorate ion)<\/strong>:\n
              \n
            • Molecular structure<\/strong>: Tetrahedral.<\/li>\n\n\n\n
            • Bond angles<\/strong>: Approximately 109.5\u00b0.<\/li>\n\n\n\n
            • Explanation: Similar to the perchlorate ion, chlorine is surrounded by three oxygen atoms and a lone pair. Although there\u2019s a lone pair, the overall structure still tends to follow tetrahedral geometry, leading to bond angles near 109.5\u00b0, but slightly distorted.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
            • SO3 (Sulfur trioxide)<\/strong>:\n
                \n
              • Molecular structure<\/strong>: Trigonal planar (Not trigonal pyramidal).<\/li>\n\n\n\n
              • Bond angles<\/strong>: 120\u00b0.<\/li>\n\n\n\n
              • Explanation: The sulfur atom is bonded to three oxygen atoms in a trigonal planar arrangement, and the bond angles are 120\u00b0 due to no lone pairs on the sulfur atom.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
              • NF3 (Nitrogen trifluoride)<\/strong>:\n
                  \n
                • Molecular structure<\/strong>: V-shaped (Bent).<\/li>\n\n\n\n
                • Bond angles<\/strong>: Approximately 102\u00b0.<\/li>\n\n\n\n
                • Explanation: In NF3, nitrogen is bonded to three fluorine atoms, but due to a lone pair on nitrogen, the molecule adopts a V-shaped structure. The bond angles are slightly less than 109.5\u00b0, around 102\u00b0.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
                • SO4^2- (Sulfate ion)<\/strong>:\n
                    \n
                  • Molecular structure<\/strong>: Tetrahedral.<\/li>\n\n\n\n
                  • Bond angles<\/strong>: 109.5\u00b0.<\/li>\n\n\n\n
                  • Explanation: The sulfur atom is surrounded by four oxygen atoms in a tetrahedral geometry, and there are no lone pairs on the sulfur atom. The bond angles are about 109.5\u00b0.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n

                    In summary:<\/p>\n\n\n\n

                      \n
                    • Tetrahedral structures<\/strong>: PO4^3-, XeO4, ClO4-, ClO3-, SO42-.<\/li>\n\n\n\n
                    • Trigonal pyramidal structures<\/strong>: POCl3.<\/li>\n\n\n\n
                    • Trigonal planar<\/strong>: SO3.<\/li>\n\n\n\n
                    • V-shaped (Bent)<\/strong>: NF3.<\/li>\n<\/ul>\n\n\n\n

                      Most of these molecules and ions follow the VSEPR model, where electron pair repulsion determines the molecular geometry and bond angles.<\/p>\n\n\n\n

                      \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

                      Predict the molecular structure and bond angles for each molecule or ion given below: PO43-: tetrahedral XeO4: tetrahedral POCl3: trigonal pyramid CIO4: tetrahedral CIO3-: tetrahedral SO3: trigonal pyramid NF3: V-shaped SO42-: tetrahedral molecular structure bond angles The Correct Answer and Explanation is: Let’s break down each molecule or ion: In summary: Most of these molecules […]<\/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-267012","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/267012","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=267012"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/267012\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=267012"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=267012"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=267012"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}