{"id":219336,"date":"2025-05-26T04:00:17","date_gmt":"2025-05-26T04:00:17","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=219336"},"modified":"2025-05-26T04:00:20","modified_gmt":"2025-05-26T04:00:20","slug":"arrange-these-ions-according-to-ionic-radius-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/26\/arrange-these-ions-according-to-ionic-radius-2\/","title":{"rendered":"Arrange these ions according to ionic radius."},"content":{"rendered":"\n<p>Arrange these ions according to ionic radius. Largest radius Smallest radius Answer Bank S2- K+ Ca2+ p3- CI-<br>Arrange these ions according to ionic\u00c3\u201a\u00c2 radius.<\/p>\n\n\n\n<p><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><strong>Correct Order (from Largest Radius to Smallest Radius):<\/strong><br><strong>P\u00b3\u207b &gt; S\u00b2\u207b &gt; Cl\u207b &gt; K\u207a &gt; Ca\u00b2\u207a<\/strong><\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Explanation <\/strong><\/h3>\n\n\n\n<p>Ionic radius refers to the size of an ion, which depends on the number of electrons, the nuclear charge (number of protons), and the electron-electron repulsion within an atom or ion.<\/p>\n\n\n\n<p>To arrange the given ions (<strong>S\u00b2\u207b, K\u207a, Ca\u00b2\u207a, P\u00b3\u207b, Cl\u207b<\/strong>) by <strong>ionic radius<\/strong>, we consider two main factors:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Electron gain or loss (charge of the ion)<\/strong><\/li>\n\n\n\n<li><strong>Number of protons (nuclear charge)<\/strong><\/li>\n<\/ol>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Step 1: Determine electron configurations<\/strong><\/h4>\n\n\n\n<p>All of these ions are <strong>isoelectronic<\/strong>\u2014they have the same number of electrons (18 electrons, like Argon) but different numbers of protons.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>P\u00b3\u207b<\/strong>: 15 protons, 18 electrons<\/li>\n\n\n\n<li><strong>S\u00b2\u207b<\/strong>: 16 protons, 18 electrons<\/li>\n\n\n\n<li><strong>Cl\u207b<\/strong>: 17 protons, 18 electrons<\/li>\n\n\n\n<li><strong>K\u207a<\/strong>: 19 protons, 18 electrons<\/li>\n\n\n\n<li><strong>Ca\u00b2\u207a<\/strong>: 20 protons, 18 electrons<\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Step 2: Compare nuclear charge<\/strong><\/h4>\n\n\n\n<p>All ions have the same number of electrons, so the <strong>number of protons<\/strong> will determine how strongly the nucleus pulls those electrons inward.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Fewer protons = weaker pull = larger radius<\/strong><\/li>\n\n\n\n<li><strong>More protons = stronger pull = smaller radius<\/strong><\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Step 3: Arrange by size<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>P\u00b3\u207b<\/strong> has the <strong>fewest protons (15)<\/strong> \u2192 <strong>largest ionic radius<\/strong><\/li>\n\n\n\n<li><strong>S\u00b2\u207b<\/strong> (16 protons) \u2192 slightly smaller<\/li>\n\n\n\n<li><strong>Cl\u207b<\/strong> (17 protons) \u2192 smaller<\/li>\n\n\n\n<li><strong>K\u207a<\/strong> (19 protons) \u2192 smaller still<\/li>\n\n\n\n<li><strong>Ca\u00b2\u207a<\/strong> has the <strong>most protons (20)<\/strong> \u2192 <strong>smallest ionic radius<\/strong><\/li>\n<\/ul>\n\n\n\n<p>Also, cations (positive ions like K\u207a, Ca\u00b2\u207a) are smaller than their parent atoms because they lose electrons, reducing electron repulsion and allowing the nucleus to pull remaining electrons in closer. Anions (negative ions like P\u00b3\u207b, S\u00b2\u207b) are larger because they gain electrons, increasing electron repulsion and expanding the cloud.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>Final Order:<\/strong><br>\u27a1\ufe0f <strong>P\u00b3\u207b &gt; S\u00b2\u207b &gt; Cl\u207b &gt; K\u207a &gt; Ca\u00b2\u207a<\/strong><br>From <strong>largest<\/strong> to <strong>smallest<\/strong> ionic radius.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/05\/learnexams-banner7-11.jpeg\" alt=\"\" class=\"wp-image-219337\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Arrange these ions according to ionic radius. Largest radius Smallest radius Answer Bank S2- K+ Ca2+ p3- CI-Arrange these ions according to ionic\u00c3\u201a\u00c2 radius. The Correct Answer and Explanation is: Correct Order (from Largest Radius to Smallest Radius):P\u00b3\u207b &gt; S\u00b2\u207b &gt; Cl\u207b &gt; K\u207a &gt; Ca\u00b2\u207a Explanation Ionic radius refers to the size of an [&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-219336","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/219336","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=219336"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/219336\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=219336"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=219336"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=219336"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}