{"id":182606,"date":"2025-01-14T13:06:13","date_gmt":"2025-01-14T13:06:13","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=182606"},"modified":"2025-01-14T13:06:15","modified_gmt":"2025-01-14T13:06:15","slug":"shorthand-electron-configuration-and-orbital-notations-use-noble-gas-shorthand-configurations-to-determine-orbital-notations","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/14\/shorthand-electron-configuration-and-orbital-notations-use-noble-gas-shorthand-configurations-to-determine-orbital-notations\/","title":{"rendered":"Shorthand Electron Configuration and Orbital Notations Use noble gas shorthand configurations to determine orbital notations"},"content":{"rendered":"\n<p>Shorthand Electron Configuration and Orbital Notations Use noble gas shorthand configurations to determine orbital notations. You only need to write out orbital notations for the energy levels and sublevels after the noble gas. Electron configuration (noble gas shortcut) Orbital Notation Symbol # e [Kr] 5s2 7. Sr [Kr] \u00c3\u00a2\u00e2\u20ac \u00e2\u20ac\u02dc4 38 5s 8. Pb 9. Al 10 Pu 11 Au None<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n<p>To write the correct electron configurations and orbital notations for the given elements, we&#8217;ll first recall the noble gas shorthand, which abbreviates electron configurations by using the noble gas preceding an element as a reference point. Then, we expand the electron configuration by filling in the remaining energy levels and orbitals for the element.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">1. <strong>Sr (Strontium)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Electron Configuration:<\/strong> [Kr] 5s\u00b2<\/li>\n\n\n\n<li><strong>Orbital Notation:<\/strong><\/li>\n\n\n\n<li>5s: \u2191\u2193<\/li>\n\n\n\n<li><strong>Explanation:<\/strong> Strontium is in period 5 and group 2, so after [Kr] (which represents the electron configuration of Krypton), it has 2 electrons in the 5s orbital. The orbital notation for the 5s orbital shows two electrons with opposite spins, denoted as \u2191\u2193.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">2. <strong>Pb (Lead)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Electron Configuration:<\/strong> [Xe] 4f\u00b9\u2074 5d\u00b9\u2070 6s\u00b2 6p\u00b2<\/li>\n\n\n\n<li><strong>Orbital Notation:<\/strong><\/li>\n\n\n\n<li>4f: \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193<\/li>\n\n\n\n<li>5d: \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193<\/li>\n\n\n\n<li>6s: \u2191\u2193<\/li>\n\n\n\n<li>6p: \u2191\u2193<\/li>\n\n\n\n<li><strong>Explanation:<\/strong> Lead is in period 6 and group 14. Starting with [Xe], the remaining electrons fill the 4f, 5d, 6s, and 6p orbitals. The 4f orbitals fill first, then the 5d orbitals, and finally, the 6s and 6p orbitals.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">3. <strong>Al (Aluminum)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Electron Configuration:<\/strong> [Ne] 3s\u00b2 3p\u00b9<\/li>\n\n\n\n<li><strong>Orbital Notation:<\/strong><\/li>\n\n\n\n<li>3s: \u2191\u2193<\/li>\n\n\n\n<li>3p: \u2191<\/li>\n\n\n\n<li><strong>Explanation:<\/strong> Aluminum is in period 3 and group 13. After the noble gas [Ne], aluminum has two electrons in the 3s orbital and one electron in the 3p orbital, as indicated by the orbital notation.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">4. <strong>Pu (Plutonium)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Electron Configuration:<\/strong> [Rn] 5f\u2076 6d\u00b9 7s\u00b2<\/li>\n\n\n\n<li><strong>Orbital Notation:<\/strong><\/li>\n\n\n\n<li>5f: \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193<\/li>\n\n\n\n<li>6d: \u2191<\/li>\n\n\n\n<li>7s: \u2191\u2193<\/li>\n\n\n\n<li><strong>Explanation:<\/strong> Plutonium is in period 7, and its electron configuration starts with the noble gas <a href=\"Radon\">Rn<\/a>. The electrons then fill the 5f, 6d, and 7s orbitals, with 6 electrons in the 5f orbital, 1 in the 6d orbital, and 2 in the 7s orbital.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">5. <strong>Au (Gold)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Electron Configuration:<\/strong> [Xe] 4f\u00b9\u2074 5d\u00b9\u2070 6s\u00b2 6p\u00b9<\/li>\n\n\n\n<li><strong>Orbital Notation:<\/strong><\/li>\n\n\n\n<li>4f: \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193<\/li>\n\n\n\n<li>5d: \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193<\/li>\n\n\n\n<li>6s: \u2191\u2193<\/li>\n\n\n\n<li>6p: \u2191<\/li>\n\n\n\n<li><strong>Explanation:<\/strong> Gold is in period 6 and group 11. The electron configuration begins with [Xe], followed by electrons filling the 4f, 5d, 6s, and 6p orbitals. The 5d orbital holds 10 electrons, and the 6p orbital holds 1 electron.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Conclusion:<\/h3>\n\n\n\n<p>Orbital notation involves writing out the energy level and sublevel of each electron, indicating its spin with arrows. This method helps visualize the electron distribution across various orbitals and provides insights into an element\u2019s chemical properties and behavior.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Shorthand Electron Configuration and Orbital Notations Use noble gas shorthand configurations to determine orbital notations. You only need to write out orbital notations for the energy levels and sublevels after the noble gas. Electron configuration (noble gas shortcut) Orbital Notation Symbol # e [Kr] 5s2 7. Sr [Kr] \u00c3\u00a2\u00e2\u20ac \u00e2\u20ac\u02dc4 38 5s 8. Pb 9. [&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-182606","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182606","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=182606"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182606\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=182606"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=182606"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=182606"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}