{"id":223716,"date":"2025-06-02T08:19:04","date_gmt":"2025-06-02T08:19:04","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=223716"},"modified":"2025-06-02T08:19:06","modified_gmt":"2025-06-02T08:19:06","slug":"determine-the-molecular-structure-for-the-ph4-molecule-full-credit-you-must-show-your-work-to-get-full-credit","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/02\/determine-the-molecular-structure-for-the-ph4-molecule-full-credit-you-must-show-your-work-to-get-full-credit\/","title":{"rendered":"Determine the molecular structure for the PH4+ molecule (FULL credit) (you must show your work to get full credit)"},"content":{"rendered":"\n<p> Determine the molecular structure for the PH4+ molecule (FULL credit) (you must show your work to get full credit) Select one: &#8211; Name the Bond Angles &#8211; Name the Geometry &#8211; State the amount of Valence electrons &#8211; Draw the Structure &#8211; State the formal charge<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-0-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To determine the molecular structure of <strong>PH\u2084\u207a (phosphonium ion)<\/strong>, we need to analyze its valence electrons, geometry, bond angles, and formal charge. Here is the full answer with calculations, drawing, and explanations.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">\u2714 Final Answer:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Valence Electrons:<\/strong> 8 total valence electrons<\/li>\n\n\n\n<li><strong>Geometry:<\/strong> <strong>Tetrahedral<\/strong><\/li>\n\n\n\n<li><strong>Bond Angles:<\/strong> Approximately <strong>109.5\u00b0<\/strong><\/li>\n\n\n\n<li><strong>Formal Charge on Phosphorus (P):<\/strong> <strong>+1<\/strong><\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">\ud83e\uddee Step-by-Step Work:<\/h3>\n\n\n\n<h4 class=\"wp-block-heading\">1. <strong>Determine Total Valence Electrons:<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Phosphorus (P)<\/strong> has 5 valence electrons.<\/li>\n\n\n\n<li>Each <strong>Hydrogen (H)<\/strong> has 1 valence electron.<\/li>\n\n\n\n<li>There are 4 hydrogen atoms: 4 \u00d7 1 = 4 electrons.<\/li>\n\n\n\n<li>The <strong>positive charge (+1)<\/strong> means one electron is removed.<\/li>\n<\/ul>\n\n\n\n<p><strong>Total:<\/strong><br>5 (P) + 4 (H) = 9<br>9 \u2013 1 (due to +1 charge) = <strong>8 valence electrons<\/strong><\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\">2. <strong>Draw the Lewis Structure:<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Place <strong>P<\/strong> in the center.<\/li>\n\n\n\n<li>Connect 4 H atoms to P using single bonds (each bond uses 2 electrons).<\/li>\n\n\n\n<li>4 bonds \u00d7 2 electrons = 8 electrons \u2192 all valence electrons used.<\/li>\n<\/ul>\n\n\n\n<pre class=\"wp-block-code\"><code>        H\n        |\n    H - P - H\n        |\n        H\n<\/code><\/pre>\n\n\n\n<p>No lone pairs are left on P. Each H has 2 electrons, satisfying its duet rule.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\">3. <strong>Molecular Geometry:<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>P is bonded to 4 atoms, with 0 lone pairs.<\/li>\n\n\n\n<li>This is the <strong>AX\u2084<\/strong> type in VSEPR theory \u2192 <strong>Tetrahedral geometry<\/strong>.<\/li>\n\n\n\n<li><strong>Bond Angles<\/strong> = <strong>109.5\u00b0<\/strong><\/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\">4. <strong>Formal Charge Calculation on P:<\/strong><\/h4>\n\n\n\n<p><strong>Formal Charge (FC) = [Valence e\u207b] \u2013 [Non-bonding e\u207b] \u2013 \u00bd(Bonding e\u207b)<\/strong><br>For P:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Valence electrons = 5<\/li>\n\n\n\n<li>Non-bonding electrons = 0<\/li>\n\n\n\n<li>Bonding electrons = 8 (4 bonds \u00d7 2 e\u207b)<\/li>\n<\/ul>\n\n\n\n<p><strong>FC = 5 \u2013 0 \u2013 (8\/2) = 5 \u2013 4 = +1<\/strong><\/p>\n\n\n\n<p>So, the phosphorus has a <strong>formal charge of +1<\/strong>, matching the overall <strong>PH\u2084\u207a<\/strong> charge.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">\ud83e\udde0 Summary Explanation <\/h3>\n\n\n\n<p>The phosphonium ion, <strong>PH\u2084\u207a<\/strong>, is a positively charged molecule formed when phosphorus bonds with four hydrogen atoms. The first step in understanding its molecular structure is calculating the total number of valence electrons. Phosphorus contributes 5 electrons, and each hydrogen contributes 1, making 9 total. However, because the molecule has a positive charge (+1), one electron is removed, leaving <strong>8 valence electrons<\/strong>.<\/p>\n\n\n\n<p>These 8 electrons are used to form four single covalent bonds between the central phosphorus atom and four hydrogen atoms. Each bond uses two electrons, and no lone pairs remain on the phosphorus atom. Because the phosphorus atom is bonded to four atoms with no lone pairs, the molecule follows the AX\u2084 arrangement in VSEPR (Valence Shell Electron Pair Repulsion) theory. This gives the molecule a <strong>tetrahedral shape<\/strong> with <strong>bond angles of 109.5\u00b0<\/strong>, which is characteristic of tetrahedral molecules.<\/p>\n\n\n\n<p>Next, we calculate the formal charge to ensure the charge on the central atom matches the ion\u2019s overall charge. The formal charge on phosphorus is <strong>+1<\/strong>, which matches the molecular ion\u2019s overall charge of +1. This confirms the accuracy of our Lewis structure and electron configuration.<\/p>\n\n\n\n<p>In summary, <strong>PH\u2084\u207a<\/strong> has a tetrahedral geometry with 109.5\u00b0 bond angles, uses 8 valence electrons for bonding, and has a formal charge of +1 on phosphorus. Understanding this molecular structure is essential for predicting the molecule\u2019s shape, reactivity, and interaction with other chemical species.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner7-69.jpeg\" alt=\"\" class=\"wp-image-223717\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Determine the molecular structure for the PH4+ molecule (FULL credit) (you must show your work to get full credit) Select one: &#8211; Name the Bond Angles &#8211; Name the Geometry &#8211; State the amount of Valence electrons &#8211; Draw the Structure &#8211; State the formal charge The Correct Answer and Explanation is: To determine the [&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-223716","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/223716","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=223716"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/223716\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=223716"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=223716"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=223716"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}