{"id":167710,"date":"2024-11-16T06:13:13","date_gmt":"2024-11-16T06:13:13","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=167710"},"modified":"2024-11-16T06:13:17","modified_gmt":"2024-11-16T06:13:17","slug":"the-molecular-geometry-of-pf3-is-trigonal-planar","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/16\/the-molecular-geometry-of-pf3-is-trigonal-planar\/","title":{"rendered":"The molecular geometry of PF3 is trigonal planar."},"content":{"rendered":"\n<p>The molecular geometry of PF3 is trigonal planar.<br>a. true<br>b. false<\/p>\n\n\n\n<p class=\"has-text-align-left\"><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Correct Answer: <strong>b. False<\/strong><\/h3>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>The molecular geometry of <strong>phosphorus trifluoride (PF\u2083)<\/strong> is <strong>trigonal pyramidal<\/strong>, not trigonal planar. This distinction arises from the electron geometry and the molecular shape determined by the VSEPR (Valence Shell Electron Pair Repulsion) theory.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>1. Electron Configuration and Bonding:<\/strong><\/h4>\n\n\n\n<p>Phosphorus (P) has five valence electrons, and each fluorine (F) atom contributes one electron for bonding. In PF\u2083:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Phosphorus forms three single covalent bonds with fluorine atoms, using three of its valence electrons.<\/li>\n\n\n\n<li>The remaining two electrons form a <strong>lone pair<\/strong> on the phosphorus atom.<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>2. Electron Geometry:<\/strong><\/h4>\n\n\n\n<p>The total number of regions of electron density (bonds and lone pairs) around the central phosphorus atom is <strong>four<\/strong>:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Three bonding pairs (P-F bonds).<\/li>\n\n\n\n<li>One lone pair.<\/li>\n<\/ul>\n\n\n\n<p>According to the VSEPR theory, four regions of electron density arrange themselves in a <strong>tetrahedral electron geometry<\/strong> to minimize repulsion.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>3. Molecular Geometry:<\/strong><\/h4>\n\n\n\n<p>While the electron geometry is tetrahedral, the molecular geometry is determined by the positions of the <strong>atoms<\/strong>, not the lone pairs. The lone pair on phosphorus pushes the three P-F bonds downward, creating a <strong>trigonal pyramidal<\/strong> shape.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>4. Key Differences Between Trigonal Planar and Trigonal Pyramidal:<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Trigonal planar<\/strong> geometry involves three bonded atoms with no lone pairs on the central atom, resulting in bond angles of <strong>120\u00b0<\/strong>. Example: BF\u2083.<\/li>\n\n\n\n<li><strong>Trigonal pyramidal<\/strong> geometry involves three bonded atoms and one lone pair on the central atom, resulting in bond angles slightly less than <strong>109.5\u00b0<\/strong> due to lone-pair repulsion. Example: PF\u2083.<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>5. Conclusion:<\/strong><\/h4>\n\n\n\n<p>The molecular geometry of PF\u2083 is <strong>trigonal pyramidal<\/strong>, not trigonal planar, due to the lone pair on phosphorus, which distorts the structure. This distinction highlights the influence of lone pairs in shaping molecular geometry.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>The molecular geometry of PF3 is trigonal planar.a. trueb. false The Correct Answer and Explanation is: Correct Answer: b. False Explanation: The molecular geometry of phosphorus trifluoride (PF\u2083) is trigonal pyramidal, not trigonal planar. This distinction arises from the electron geometry and the molecular shape determined by the VSEPR (Valence Shell Electron Pair Repulsion) theory. [&hellip;]<\/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-167710","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/167710","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=167710"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/167710\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=167710"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=167710"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=167710"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}