{"id":189653,"date":"2025-02-10T06:52:01","date_gmt":"2025-02-10T06:52:01","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=189653"},"modified":"2025-02-10T06:52:03","modified_gmt":"2025-02-10T06:52:03","slug":"which-of-the-following-is-the-correct-condensed-electron-configuration-for-the-atom-or-ion-indicated","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/10\/which-of-the-following-is-the-correct-condensed-electron-configuration-for-the-atom-or-ion-indicated\/","title":{"rendered":"Which of the following is the correct condensed electron configuration for the atom or ion indicated"},"content":{"rendered":"\n<p>Which of the following is the correct condensed electron configuration for the atom or ion indicated? <\/p>\n\n\n\n<p>a) The electron configuration of Ba2+ is [Xe]. <\/p>\n\n\n\n<p>b) The electron configuration of In3+ is [Kr]5s24d8. <\/p>\n\n\n\n<p>c) The electron configuration of Co2+ is [Ar]4s23d5. <\/p>\n\n\n\n<p>d) The electron configuration of p3-is (Ne]3s? <\/p>\n\n\n\n<p>e) The electron configuration of s2 is [Ne]3s23p2.<\/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>The correct electron configuration for each atom or ion is based on the principle that electrons fill orbitals in order of increasing energy levels, which is described by the Aufbau principle. The electron configuration takes into account the element&#8217;s atomic number, and for ions, the loss or gain of electrons is accounted for.<\/p>\n\n\n\n<p>Let&#8217;s review each option:<\/p>\n\n\n\n<p>a) <strong>The electron configuration of Ba\u00b2\u207a is [Xe].<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Correct<\/strong>. Barium (Ba) has an atomic number of 56, so its neutral electron configuration is [Xe] 6s\u00b2. When it forms the Ba\u00b2\u207a ion, it loses two electrons, typically from the 6s orbital. After the loss of these two electrons, the electron configuration becomes [Xe], which is the correct configuration for Ba\u00b2\u207a.<\/li>\n<\/ul>\n\n\n\n<p>b) <strong>The electron configuration of In\u00b3\u207a is [Kr] 5s\u00b2 4d\u2078.<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Incorrect<\/strong>. Indium (In) has an atomic number of 49, and its neutral electron configuration is [Kr] 5s\u00b2 4d\u00b9\u2070 5p\u00b9. When it forms the In\u00b3\u207a ion, it loses three electrons. The first two electrons are removed from the 5p orbital, and the third electron is removed from the 5s orbital. The correct electron configuration for In\u00b3\u207a is [Kr] 4d\u00b9\u2070, not [Kr] 5s\u00b2 4d\u2078.<\/li>\n<\/ul>\n\n\n\n<p>c) <strong>The electron configuration of Co\u00b2\u207a is [Ar] 4s\u00b2 3d\u2075.<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Incorrect<\/strong>. Cobalt (Co) has an atomic number of 27, so its neutral electron configuration is [Ar] 4s\u00b2 3d\u2077. When Co forms the Co\u00b2\u207a ion, it loses two electrons, which are typically removed from the 4s orbital. Therefore, the correct electron configuration for Co\u00b2\u207a is [Ar] 3d\u2077, not [Ar] 4s\u00b2 3d\u2075.<\/li>\n<\/ul>\n\n\n\n<p>d) <strong>The electron configuration of P\u00b3\u207b is [Ne] 3s\u00b2.<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Incorrect<\/strong>. Phosphorus (P) has an atomic number of 15, so its neutral electron configuration is [Ne] 3s\u00b2 3p\u00b3. When it forms the P\u00b3\u207b ion, it gains three electrons, filling the 3p orbital. The correct electron configuration for P\u00b3\u207b is [Ne] 3s\u00b2 3p\u2076, not [Ne] 3s\u00b2.<\/li>\n<\/ul>\n\n\n\n<p>e) <strong>The electron configuration of Si\u00b2\u207a is [Ne] 3s\u00b2 3p\u00b2.<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Incorrect<\/strong>. Silicon (Si) has an atomic number of 14, and its neutral electron configuration is [Ne] 3s\u00b2 3p\u00b2. When it forms the Si\u00b2\u207a ion, it loses two electrons, which are typically removed from the 3p orbital. Therefore, the correct electron configuration for Si\u00b2\u207a is [Ne] 3s\u00b2.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Conclusion:<\/h3>\n\n\n\n<p>The correct answer is <strong>(a)<\/strong>: The electron configuration of Ba\u00b2\u207a is [Xe].<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Which of the following is the correct condensed electron configuration for the atom or ion indicated? a) The electron configuration of Ba2+ is [Xe]. b) The electron configuration of In3+ is [Kr]5s24d8. c) The electron configuration of Co2+ is [Ar]4s23d5. d) The electron configuration of p3-is (Ne]3s? e) The electron configuration of s2 is [Ne]3s23p2. [&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-189653","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/189653","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=189653"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/189653\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=189653"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=189653"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=189653"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}