{"id":214437,"date":"2025-05-14T10:47:41","date_gmt":"2025-05-14T10:47:41","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=214437"},"modified":"2025-05-14T10:47:44","modified_gmt":"2025-05-14T10:47:44","slug":"draw-a-louis-dot-diagram-for-magnesium-phosphide-and-phosphorus-try-hydride","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/14\/draw-a-louis-dot-diagram-for-magnesium-phosphide-and-phosphorus-try-hydride\/","title":{"rendered":"Draw a Louis dot diagram for magnesium phosphide and phosphorus try hydride"},"content":{"rendered":"\n<p class=\"wp-block-paragraph\">draw a Louis dot diagram for magnesium phosphide and phosphorus try hydride<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Draw Lewis Dot diagrams for: explain briefly all 2 and explain it<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">a) Magnesium phosphide<br>b) Phosphorus trihydride.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-1-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Let&#8217;s draw the <strong>Lewis Dot Diagrams<\/strong> for the following compounds and explain the bonding:<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>a) Magnesium Phosphide (Mg\u2083P\u2082)<\/strong><\/h3>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Lewis Dot Diagram:<\/strong><\/h4>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Mg has 2 valence electrons<\/strong>, and <strong>P has 5 valence electrons<\/strong>.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Each <strong>P\u00b3\u207b<\/strong> ion needs <strong>3 electrons<\/strong> to complete its octet.<br>Each <strong>Mg atom loses 2 electrons<\/strong> to become <strong>Mg\u00b2\u207a<\/strong>.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Thus:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>3 Mg atoms lose a total of <strong>6 electrons (3 \u00d7 2 = 6)<\/strong><\/li>\n\n\n\n<li>2 P atoms gain a total of <strong>6 electrons (2 \u00d7 3 = 6)<\/strong><\/li>\n<\/ul>\n\n\n\n<p class=\"wp-block-paragraph\">This satisfies the charge balance:<br><strong>3 Mg\u00b2\u207a + 2 P\u00b3\u207b \u2192 Mg\u2083P\u2082<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">We show this by:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Writing <strong>Mg<\/strong> with no dots (they lose electrons).<\/li>\n\n\n\n<li>Writing <strong>P<\/strong> surrounded by <strong>8 electrons<\/strong>, showing the gained 3 extra electrons from Mg.<\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\">Diagram:<\/h4>\n\n\n\n<pre class=\"wp-block-code\"><code>Mg   Mg   Mg         &#91;\u2022\u2022P\u2022\u2022]\u00b3\u207b   &#91;\u2022\u2022P\u2022\u2022]\u00b3\u207b\n(no dots)            (8 electrons around each P)\n(Mg\u00b2\u207a)               (P\u00b3\u207b with octet completed)\n<\/code><\/pre>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>b) Phosphorus Trihydride (PH\u2083)<\/strong><\/h3>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Lewis Dot Diagram:<\/strong><\/h4>\n\n\n\n<p class=\"wp-block-paragraph\">Phosphorus (P) = 5 valence electrons<br>Hydrogen (H) = 1 valence electron \u00d7 3 = 3 electrons<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Phosphorus needs 3 electrons to form bonds with 3 H atoms and keeps one <strong>lone pair<\/strong>.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">Diagram:<\/h4>\n\n\n\n<pre class=\"wp-block-code\"><code>       ..\n      :P:\n     \/ | \\\n   H  H  H\n<\/code><\/pre>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The <strong>&#8220;:&#8221;<\/strong> on top represents the <strong>lone pair<\/strong> of electrons on phosphorus.<\/li>\n\n\n\n<li>Each line (<strong>\u2013<\/strong>) between P and H represents a <strong>single covalent bond<\/strong> (shared pair of electrons).<\/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\"><strong>Explanation (300+ words):<\/strong><\/h3>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Lewis Dot Structures<\/strong> are diagrams that represent the valence electrons of atoms and show how these electrons are involved in bonding. These diagrams help visualize how atoms come together to form molecules or ionic compounds by sharing or transferring electrons.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">a) <strong>Magnesium Phosphide (Mg\u2083P\u2082):<\/strong><\/h4>\n\n\n\n<p class=\"wp-block-paragraph\">This is an <strong>ionic compound<\/strong>, formed between <strong>magnesium (a metal)<\/strong> and <strong>phosphorus (a nonmetal)<\/strong>. Magnesium atoms each lose <strong>two electrons<\/strong>, becoming Mg\u00b2\u207a ions. Phosphorus atoms each need to <strong>gain three electrons<\/strong> to achieve a stable octet, becoming P\u00b3\u207b ions. To balance charges:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>3 Mg atoms lose 6 electrons (3 \u00d7 2 = 6),<\/li>\n\n\n\n<li>2 P atoms gain 6 electrons (2 \u00d7 3 = 6),<br>making the formula <strong>Mg\u2083P\u2082<\/strong> electrically neutral. In Lewis notation, we don\u2019t show the lost electrons on Mg because metals donate them, and we draw full octets around P, with brackets and a charge of 3\u207b.<\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\">b) <strong>Phosphorus Trihydride (PH\u2083):<\/strong><\/h4>\n\n\n\n<p class=\"wp-block-paragraph\">This is a <strong>covalent compound<\/strong>, where phosphorus shares electrons with hydrogen. Phosphorus has 5 valence electrons and needs 3 more to complete its octet. Each hydrogen has 1 electron and needs 1 more. Phosphorus forms <strong>three single bonds<\/strong> with three hydrogen atoms, sharing a pair of electrons with each. The remaining two electrons on phosphorus remain as a <strong>lone pair<\/strong>, which affects the molecule\u2019s geometry (trigonal pyramidal). The resulting molecule is neutral and stable. This type of bonding is typical for covalent molecules, where atoms achieve stability through <strong>electron sharing<\/strong> rather than transfer.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">In conclusion, <strong>Mg\u2083P\u2082 is ionic<\/strong> with complete electron transfer, while <strong>PH\u2083 is covalent<\/strong> with electron sharing. Lewis Dot Diagrams are key to visualizing how these compounds form and help predict structure and behavior.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>draw a Louis dot diagram for magnesium phosphide and phosphorus try hydride Draw Lewis Dot diagrams for: explain briefly all 2 and explain it a) Magnesium phosphideb) Phosphorus trihydride. The Correct Answer and Explanation is: Let&#8217;s draw the Lewis Dot Diagrams for the following compounds and explain the bonding: a) Magnesium Phosphide (Mg\u2083P\u2082) Lewis Dot [&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-214437","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/214437","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=214437"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/214437\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=214437"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=214437"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=214437"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}