{"id":185509,"date":"2025-01-22T15:30:11","date_gmt":"2025-01-22T15:30:11","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=185509"},"modified":"2025-01-22T15:30:13","modified_gmt":"2025-01-22T15:30:13","slug":"give-the-electron-configurations-for-the-following-ions","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/22\/give-the-electron-configurations-for-the-following-ions\/","title":{"rendered":"Give the electron configurations for the following ions"},"content":{"rendered":"\n<p>Give the electron configurations for the following ions: P5+, P3-, Sn4+, Se2-, I-, and Ni2+. 2.10 Potassium iodide (KI) exhibits predominantly ionic bonding. The K+ and I\u2013 ions have electron structures that are identical to which two inert gases? 2. With regard to electron configuration, what do all the elements in Group IIA of the periodic table have in common?<\/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<h3 class=\"wp-block-heading\">1. Electron Configurations for Ions:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>P\u2075\u207a<\/strong>: The electron configuration of a neutral phosphorus (P) atom is 1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u00b3. The P\u2075\u207a ion has lost five electrons, so the electron configuration becomes:\n<ul class=\"wp-block-list\">\n<li><strong>P\u2075\u207a<\/strong>: 1s\u00b2 2s\u00b2 2p\u2076<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>P\u00b3\u207b<\/strong>: A neutral phosphorus (P) atom has 15 electrons. The P\u00b3\u207b ion has gained three electrons, so the electron configuration becomes:\n<ul class=\"wp-block-list\">\n<li><strong>P\u00b3\u207b<\/strong>: 1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u2076 (which is the same as Argon)<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Sn\u2074\u207a<\/strong>: The neutral tin (Sn) atom has the electron configuration [Kr] 4d\u00b9\u2070 5s\u00b2 5p\u00b2. The Sn\u2074\u207a ion has lost four electrons, so its electron configuration becomes:\n<ul class=\"wp-block-list\">\n<li><strong>Sn\u2074\u207a<\/strong>: [Kr] 4d\u00b9\u2070<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Se\u00b2\u207b<\/strong>: The neutral selenium (Se) atom has the electron configuration [Ar] 3d\u00b9\u2070 4s\u00b2 4p\u2074. The Se\u00b2\u207b ion has gained two electrons, so its electron configuration becomes:\n<ul class=\"wp-block-list\">\n<li><strong>Se\u00b2\u207b<\/strong>: [Ar] 3d\u00b9\u2070 4s\u00b2 4p\u2076 (which is the same as Krypton)<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>I\u207b<\/strong>: The neutral iodine (I) atom has the electron configuration [Kr] 4d\u00b9\u2070 5s\u00b2 5p\u2075. The I\u207b ion has gained one electron, so its electron configuration becomes:\n<ul class=\"wp-block-list\">\n<li><strong>I\u207b<\/strong>: [Kr] 4d\u00b9\u2070 5s\u00b2 5p\u2076 (which is the same as Xenon)<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Ni\u00b2\u207a<\/strong>: The neutral nickel (Ni) atom has the electron configuration [Ar] 3d\u2078 4s\u00b2. The Ni\u00b2\u207a ion has lost two electrons, so its electron configuration becomes:\n<ul class=\"wp-block-list\">\n<li><strong>Ni\u00b2\u207a<\/strong>: [Ar] 3d\u2078<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">2. Potassium Iodide (KI) and Inert Gases:<\/h3>\n\n\n\n<p>In potassium iodide (KI), K\u207a and I\u207b ions exhibit the electron configuration of <strong>Argon (Ar)<\/strong> and <strong>Xenon (Xe)<\/strong>, respectively.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>K\u207a (Potassium ion)<\/strong>: The electron configuration of the neutral potassium (K) atom is [Ar] 4s\u00b9. When it loses one electron, it attains the electron configuration of <strong>Argon (Ar)<\/strong>, which is [Ar] 3d\u00b9\u2070 4s\u00b2.<\/li>\n\n\n\n<li><strong>I\u207b (Iodide ion)<\/strong>: The electron configuration of a neutral iodine (I) atom is [Kr] 4d\u00b9\u2070 5s\u00b2 5p\u2075. When it gains one electron, it attains the electron configuration of <strong>Xenon (Xe)<\/strong>, which is [Kr] 4d\u00b9\u2070 5s\u00b2 5p\u2076.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">3. Electron Configuration of Group IIA Elements:<\/h3>\n\n\n\n<p>Group IIA elements (alkaline earth metals) share the common characteristic of having <strong>two electrons in their outermost (valence) shell<\/strong>. These elements include beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra).<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The electron configurations of these elements typically end in <strong>s\u00b2<\/strong> for their outermost shell. For example:\n<ul class=\"wp-block-list\">\n<li><strong>Be<\/strong>: 1s\u00b2 2s\u00b2<\/li>\n\n\n\n<li><strong>Mg<\/strong>: 1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2<\/li>\n\n\n\n<li><strong>Ca<\/strong>: 1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u2076 4s\u00b2<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<p>Thus, all elements in Group IIA have their valence electrons in the <strong>s orbital<\/strong> of the outermost shell, with two electrons. This configuration leads to the formation of <strong>2+ ions<\/strong> when they lose these two outermost electrons during chemical reactions. These properties help characterize the alkaline earth metals as being less reactive than alkali metals, but still reactive enough to form stable ionic compounds.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Give the electron configurations for the following ions: P5+, P3-, Sn4+, Se2-, I-, and Ni2+. 2.10 Potassium iodide (KI) exhibits predominantly ionic bonding. The K+ and I\u2013 ions have electron structures that are identical to which two inert gases? 2. With regard to electron configuration, what do all the elements in Group IIA of 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-185509","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185509","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=185509"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185509\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=185509"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=185509"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=185509"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}