{"id":196361,"date":"2025-03-04T18:19:08","date_gmt":"2025-03-04T18:19:08","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=196361"},"modified":"2025-03-04T18:19:11","modified_gmt":"2025-03-04T18:19:11","slug":"write-the-lewis-structure-for-nf3-and-pf5-on-the-basis-of-hybrid-orbitals","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/04\/write-the-lewis-structure-for-nf3-and-pf5-on-the-basis-of-hybrid-orbitals\/","title":{"rendered":"write the lewis structure for NF3 and PF5 on the basis of hybrid orbitals"},"content":{"rendered":"\n

write the lewis structure for NF3 and PF5 on the basis of hybrid orbitals<\/p>\n\n\n\n

explain the fact that NF3, PF3, and PF5 are stable molecules but NF5 does not exist<\/p>\n\n\n\n

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

Lewis Structures of NF\u2083 and PF\u2085 Based on Hybrid Orbitals<\/strong><\/h3>\n\n\n\n
    \n
  1. NF\u2083 (Nitrogen trifluoride)<\/strong>\n
      \n
    • Central Atom:<\/strong> Nitrogen (N)<\/li>\n\n\n\n
    • Valence Electrons:<\/strong> N (5), F (7 \u00d7 3) = 26 electrons<\/li>\n\n\n\n
    • Hybridization:<\/strong> sp\u00b3<\/li>\n\n\n\n
    • Structure:<\/strong> Trigonal pyramidal<\/li>\n\n\n\n
    • Lone Pair on N:<\/strong> 1<\/li>\n<\/ul>\n<\/li>\n\n\n\n
    • PF\u2085 (Phosphorus pentafluoride)<\/strong>\n
        \n
      • Central Atom:<\/strong> Phosphorus (P)<\/li>\n\n\n\n
      • Valence Electrons:<\/strong> P (5), F (7 \u00d7 5) = 40 electrons<\/li>\n\n\n\n
      • Hybridization:<\/strong> sp\u00b3d<\/li>\n\n\n\n
      • Structure:<\/strong> Trigonal bipyramidal<\/li>\n\n\n\n
      • Lone Pairs on P:<\/strong> 0<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n

        Why NF\u2085 Does Not Exist?<\/strong><\/h3>\n\n\n\n
          \n
        • Electron Configuration & Hybridization:<\/strong>\n
            \n
          • Nitrogen (N) belongs to Period 2 and has no available d-orbitals to expand its octet.<\/li>\n\n\n\n
          • Phosphorus (P) is in Period 3 and can use empty 3d orbitals to accommodate five fluorine atoms.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
          • Bonding & Steric Effects:<\/strong>\n
              \n
            • NF\u2083 is stable due to the availability of sp\u00b3 hybridization.<\/li>\n\n\n\n
            • NF\u2085 would require sp\u00b3d hybridization, but nitrogen lacks accessible d orbitals.<\/li>\n\n\n\n
            • The absence of d orbitals in nitrogen prevents it from forming more than four bonds.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
            • Phosphorus Stability in PF\u2085:<\/strong>\n
                \n
              • Phosphorus, being a third-period element, can expand its octet.<\/li>\n\n\n\n
              • PF\u2085 forms a stable trigonal bipyramidal structure using sp\u00b3d hybridization.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
              • Electronegativity & Bond Strength:<\/strong>\n
                  \n
                • Strong lone-pair repulsion and high electronegativity of fluorine make NF\u2085 formation unfavorable.<\/li>\n\n\n\n
                • Phosphorus has a larger atomic size, reducing repulsion in PF\u2085.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n

                  Thus, NF\u2085 does not exist<\/strong>, whereas NF\u2083, PF\u2083, and PF\u2085 are stable<\/strong> due to differences in hybridization and available orbitals.<\/p>\n\n\n\n

                  Now, I’ll generate the Lewis structure image for NF\u2083 and PF\u2085.<\/p>\n\n\n\n

                  I have generated the Lewis structure diagram for NF\u2083 and PF\u2085. Let me know if you need any modifications or further explanations!<\/p>\n","protected":false},"excerpt":{"rendered":"

                  write the lewis structure for NF3 and PF5 on the basis of hybrid orbitals explain the fact that NF3, PF3, and PF5 are stable molecules but NF5 does not exist The correct answer and explanation is: Lewis Structures of NF\u2083 and PF\u2085 Based on Hybrid Orbitals Why NF\u2085 Does Not Exist? Thus, NF\u2085 does not […]<\/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-196361","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/196361","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=196361"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/196361\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=196361"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=196361"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=196361"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}