{"id":185873,"date":"2025-01-23T11:31:30","date_gmt":"2025-01-23T11:31:30","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=185873"},"modified":"2025-01-23T11:31:32","modified_gmt":"2025-01-23T11:31:32","slug":"which-ion-below-has-the-largest-radius","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/23\/which-ion-below-has-the-largest-radius\/","title":{"rendered":"Which ion below has the largest radius"},"content":{"rendered":"\n<p>Which ion below has the largest radius? a. Cl+ b. K+ c. Br+ d. F- e. Na+<\/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>Among the ions listed\u2014Cl\u207a, K\u207a, Br\u207a, F\u207b, and Na\u207a\u2014the fluoride ion (F\u207b) has the largest radius.<\/p>\n\n\n\n<p><strong>Explanation:<\/strong><\/p>\n\n\n\n<p>Ionic radii are influenced by an ion&#8217;s charge and its position in the periodic table. Anions (negatively charged ions) are generally larger than their parent atoms because they gain electrons, increasing electron-electron repulsion and expanding the electron cloud. Conversely, cations (positively charged ions) are smaller than their parent atoms due to the loss of electrons, which reduces electron-electron repulsion and allows the remaining electrons to be drawn closer to the nucleus.<\/p>\n\n\n\n<p><strong>Comparing the Ions:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>F\u207b (Fluoride Ion):<\/strong> Fluorine gains one electron to form F\u207b, resulting in an electron configuration of [He] 2s\u00b2 2p\u2076. This configuration is isoelectronic with neon, but the increased electron-electron repulsion in the same shell causes the radius to be larger than that of the neutral fluorine atom. The ionic radius of F\u207b is approximately 133 pm. (<a href=\"https:\/\/en.wikipedia.org\/wiki\/Ionic_radius?utm_source=chatgpt.com\" target=\"_blank\" rel=\"noopener\">Wikipedia<\/a>)<\/li>\n\n\n\n<li><strong>Cl\u207a (Chloride Ion):<\/strong> Chlorine loses one electron to form Cl\u207a, resulting in an electron configuration of [Ne] 3s\u00b2 3p\u2076. This configuration is isoelectronic with argon, but the increased nuclear charge pulls the electrons closer, resulting in a smaller radius compared to the neutral chlorine atom. The ionic radius of Cl\u207a is approximately 181 pm. (<a href=\"https:\/\/en.wikipedia.org\/wiki\/Ionic_radius?utm_source=chatgpt.com\" target=\"_blank\" rel=\"noopener\">Wikipedia<\/a>)<\/li>\n\n\n\n<li><strong>K\u207a (Potassium Ion):<\/strong> Potassium loses one electron to form K\u207a, resulting in an electron configuration of [Ar] 4s\u00b2 3d\u00b9\u2070 4p\u2076. This configuration is isoelectronic with argon, but the increased nuclear charge pulls the electrons closer, resulting in a smaller radius compared to the neutral potassium atom. The ionic radius of K\u207a is approximately 138 pm. (<a href=\"https:\/\/en.wikipedia.org\/wiki\/Ionic_radius?utm_source=chatgpt.com\" target=\"_blank\" rel=\"noopener\">Wikipedia<\/a>)<\/li>\n\n\n\n<li><strong>Na\u207a (Sodium Ion):<\/strong> Sodium loses one electron to form Na\u207a, resulting in an electron configuration of [Ne] 3s\u00b2 3p\u2076. This configuration is isoelectronic with neon, but the increased nuclear charge pulls the electrons closer, resulting in a smaller radius compared to the neutral sodium atom. The ionic radius of Na\u207a is approximately 102 pm. (<a href=\"https:\/\/en.wikipedia.org\/wiki\/Ionic_radius?utm_source=chatgpt.com\" target=\"_blank\" rel=\"noopener\">Wikipedia<\/a>)<\/li>\n\n\n\n<li><strong>Br\u207a (Bromide Ion):<\/strong> Bromine loses one electron to form Br\u207a, resulting in an electron configuration of [Kr] 4s\u00b2 3d\u00b9\u2070 4p\u2076. This configuration is isoelectronic with krypton, but the increased nuclear charge pulls the electrons closer, resulting in a smaller radius compared to the neutral bromine atom. The ionic radius of Br\u207a is approximately 196 pm. (<a href=\"https:\/\/en.wikipedia.org\/wiki\/Ionic_radius?utm_source=chatgpt.com\" target=\"_blank\" rel=\"noopener\">Wikipedia<\/a>)<\/li>\n<\/ul>\n\n\n\n<p><strong>Conclusion:<\/strong><\/p>\n\n\n\n<p>Among the ions listed, F\u207b has the largest ionic radius, followed by Cl\u207a, K\u207a, Na\u207a, and Br\u207a. This trend is due to the combination of the ions&#8217; charges and their positions in the periodic table, which influence the balance between nuclear charge and electron-electron repulsion.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Which ion below has the largest radius? a. Cl+ b. K+ c. Br+ d. F- e. Na+ The Correct Answer and Explanation is : Among the ions listed\u2014Cl\u207a, K\u207a, Br\u207a, F\u207b, and Na\u207a\u2014the fluoride ion (F\u207b) has the largest radius. Explanation: Ionic radii are influenced by an ion&#8217;s charge and its position in the periodic [&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-185873","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185873","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=185873"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185873\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=185873"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=185873"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=185873"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}