{"id":203741,"date":"2025-03-20T14:42:48","date_gmt":"2025-03-20T14:42:48","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=203741"},"modified":"2025-03-20T14:42:50","modified_gmt":"2025-03-20T14:42:50","slug":"select-the-correct-electron-configurations-from-the-list-below","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/20\/select-the-correct-electron-configurations-from-the-list-below\/","title":{"rendered":"select the correct electron configurations from the list below"},"content":{"rendered":"\n<p>select the correct electron configurations from the list below. You can refer to the periodic table for atomic numbers.<\/p>\n\n\n\n<p>The electron configuration of Cu+ is [Ar]4s13d9.<\/p>\n\n\n\n<p>The electron configuration of S2\u2212 is [Ne]3s23p6.<\/p>\n\n\n\n<p>The electron configuration of Fe is [Ar]4s23d6.<\/p>\n\n\n\n<p>The electron configuration of Si is [Ne]3s23p2.<\/p>\n\n\n\n<p>The electron configuration of Rb is [Kr]5s04d1.<\/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>Let&#8217;s analyze each given electron configuration and determine its correctness.<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Cu\u207a (Copper ion, +1 charge)<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Given: <strong>[Ar]4s\u00b93d\u2079<\/strong><\/li>\n\n\n\n<li>Correct Configuration: <strong>[Ar]3d\u00b9\u2070<\/strong><\/li>\n\n\n\n<li>Explanation: Copper (Cu) has an atomic number of 29, with a neutral configuration of <strong>[Ar]4s\u00b93d\u00b9\u2070<\/strong> (due to stability considerations). When Cu loses one electron to form Cu\u207a, it loses the 4s electron first, resulting in <strong>[Ar]3d\u00b9\u2070<\/strong>. Thus, the given configuration is incorrect.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>S\u00b2\u207b (Sulfide ion, -2 charge)<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Given: <strong>[Ne]3s\u00b23p\u2076<\/strong><\/li>\n\n\n\n<li>Correct Configuration: <strong>[Ne]3s\u00b23p\u2076<\/strong><\/li>\n\n\n\n<li>Explanation: Sulfur (S) has an atomic number of 16, with a neutral configuration of <strong>[Ne]3s\u00b23p\u2074<\/strong>. When it gains two electrons to form S\u00b2\u207b, it achieves the noble gas configuration of argon, <strong>[Ne]3s\u00b23p\u2076<\/strong>. Thus, this configuration is correct.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Fe (Iron, neutral atom)<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Given: <strong>[Ar]4s\u00b23d\u2076<\/strong><\/li>\n\n\n\n<li>Correct Configuration: <strong>[Ar]4s\u00b23d\u2076<\/strong><\/li>\n\n\n\n<li>Explanation: Iron (Fe) has an atomic number of 26, with a neutral configuration of <strong>[Ar]4s\u00b23d\u2076<\/strong>. The given configuration is correct.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Si (Silicon, neutral atom)<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Given: <strong>[Ne]3s\u00b23p\u00b2<\/strong><\/li>\n\n\n\n<li>Correct Configuration: <strong>[Ne]3s\u00b23p\u00b2<\/strong><\/li>\n\n\n\n<li>Explanation: Silicon (Si) has an atomic number of 14, with a neutral configuration of <strong>[Ne]3s\u00b23p\u00b2<\/strong>. The given configuration is correct.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Rb (Rubidium, neutral atom)<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Given: <strong>[Kr]5s\u20704d\u00b9<\/strong><\/li>\n\n\n\n<li>Correct Configuration: <strong>[Kr]5s\u00b9<\/strong><\/li>\n\n\n\n<li>Explanation: Rubidium (Rb) has an atomic number of 37, with a neutral configuration of <strong>[Kr]5s\u00b9<\/strong>. The given configuration is incorrect. The electron should be in the 5s orbital, not in the 4d orbital.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Final Evaluation:<\/strong><\/h3>\n\n\n\n<p>\u2705 <strong>Correct Configurations:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>S\u00b2\u207b: [Ne]3s\u00b23p\u2076<\/strong><\/li>\n\n\n\n<li><strong>Fe: [Ar]4s\u00b23d\u2076<\/strong><\/li>\n\n\n\n<li><strong>Si: [Ne]3s\u00b23p\u00b2<\/strong><\/li>\n<\/ul>\n\n\n\n<p>\u274c <strong>Incorrect Configurations:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Cu\u207a: Should be [Ar]3d\u00b9\u2070<\/strong><\/li>\n\n\n\n<li><strong>Rb: Should be [Kr]5s\u00b9<\/strong><\/li>\n<\/ul>\n\n\n\n<p>This analysis follows the Aufbau principle, Hund\u2019s rule, and the order of orbital filling.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>select the correct electron configurations from the list below. You can refer to the periodic table for atomic numbers. The electron configuration of Cu+ is [Ar]4s13d9. The electron configuration of S2\u2212 is [Ne]3s23p6. The electron configuration of Fe is [Ar]4s23d6. The electron configuration of Si is [Ne]3s23p2. The electron configuration of Rb is [Kr]5s04d1. 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-203741","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/203741","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=203741"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/203741\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=203741"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=203741"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=203741"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}