{"id":169424,"date":"2024-11-19T08:42:31","date_gmt":"2024-11-19T08:42:31","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=169424"},"modified":"2024-11-19T08:42:34","modified_gmt":"2024-11-19T08:42:34","slug":"according-to-vsepr-theory","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/19\/according-to-vsepr-theory\/","title":{"rendered":"According to VSEPR theory"},"content":{"rendered":"\n

According to VSEPR theory, what is the shape of the PH3 molecule best described as?<\/p>\n\n\n\n

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

According to VSEPR (Valence Shell Electron Pair Repulsion) theory, the shape of the PH\u2083<\/strong> (phosphine) molecule is best described as trigonal pyramidal<\/strong>.<\/p>\n\n\n\n

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

VSEPR theory predicts the shape of a molecule based on the repulsion between electron pairs around the central atom. In the case of PH\u2083, phosphorus (P) is the central atom, and it is bonded to three hydrogen (H) atoms. Here’s a breakdown of how we arrive at the shape:<\/p>\n\n\n\n

    \n
  1. Electron Domain Count<\/strong>: Phosphorus has five valence electrons, and each hydrogen atom contributes one electron, making a total of eight electrons around phosphorus (5 from phosphorus and 3 from hydrogen). These electrons will form bonding pairs with hydrogen atoms and potentially lone pairs on the central phosphorus atom.<\/li>\n\n\n\n
  2. Electron Pairs and Geometry<\/strong>:<\/li>\n<\/ol>\n\n\n\n
      \n
    • There are three bonding pairs<\/strong> (from the three P-H bonds).<\/li>\n\n\n\n
    • Phosphorus also has one lone pair<\/strong> of electrons.<\/li>\n\n\n\n
    • According to VSEPR theory, the three bonding pairs and one lone pair on phosphorus will repel each other to minimize electron-electron repulsion.<\/li>\n<\/ul>\n\n\n\n
        \n
      1. Shape Determination<\/strong>:<\/li>\n<\/ol>\n\n\n\n
          \n
        • The ideal geometry<\/strong> for four electron pairs (3 bonding pairs + 1 lone pair) around a central atom is tetrahedral<\/strong>.<\/li>\n\n\n\n
        • However, lone pairs of electrons exert more repulsion than bonding pairs, so the presence of a lone pair pushes the bonding pairs closer together, creating a trigonal pyramidal<\/strong> shape rather than a perfect tetrahedral geometry.<\/li>\n\n\n\n
        • The bond angles in PH\u2083 are approximately 93.5\u00b0<\/strong>, which is less than the ideal tetrahedral angle of 109.5\u00b0 because of the lone pair’s repulsive effect.<\/li>\n<\/ul>\n\n\n\n
            \n
          1. Electron Pair Geometry vs. Molecular Geometry<\/strong>:<\/li>\n<\/ol>\n\n\n\n
              \n
            • The electron pair geometry (which includes both bonding and lone pairs) is tetrahedral<\/strong>.<\/li>\n\n\n\n
            • The molecular geometry (considering only the positions of atoms) is trigonal pyramidal<\/strong>.<\/li>\n<\/ul>\n\n\n\n

              In conclusion, the PH\u2083 molecule adopts a trigonal pyramidal shape due to the presence of a lone pair on the phosphorus atom that repels the bonding pairs, distorting the molecule from a tetrahedral configuration.<\/p>\n","protected":false},"excerpt":{"rendered":"

              According to VSEPR theory, what is the shape of the PH3 molecule best described as? The Correct Answer and Explanation is : According to VSEPR (Valence Shell Electron Pair Repulsion) theory, the shape of the PH\u2083 (phosphine) molecule is best described as trigonal pyramidal. Explanation: VSEPR theory predicts the shape of a molecule based on […]<\/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-169424","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/169424","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=169424"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/169424\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=169424"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=169424"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=169424"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}