{"id":246991,"date":"2025-07-07T14:10:16","date_gmt":"2025-07-07T14:10:16","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=246991"},"modified":"2025-07-07T14:10:18","modified_gmt":"2025-07-07T14:10:18","slug":"potassium-iodide-ki-exhibits-predominantly-ionic-bonding","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/07\/potassium-iodide-ki-exhibits-predominantly-ionic-bonding\/","title":{"rendered":"Potassium iodide (KI) exhibits predominantly ionic bonding."},"content":{"rendered":"\n<p>Potassium iodide (KI) exhibits predominantly ionic bonding. The<br>and<br>ions have electron structures that are identical to which two inert gases?<\/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>Potassium iodide (KI) exhibits predominantly ionic bonding, where potassium (K) donates an electron to become a positively charged ion (K\u207a), and iodine (I) accepts that electron to become a negatively charged ion (I\u207b). These ions each have electron structures that resemble the electron configurations of the nearest inert gases.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Potassium ion (K\u207a):<\/strong> When potassium loses one electron to become K\u207a, it achieves an electron configuration similar to <strong>argon (Ar)<\/strong>, which has an atomic number of 18. Potassium (K) originally has 19 electrons, but after losing one electron, K\u207a has 18 electrons, matching the electron configuration of argon, which is [Ne]3s\u00b23p\u2076.<\/li>\n\n\n\n<li><strong>Iodide ion (I\u207b):<\/strong> When iodine gains an electron to form I\u207b, its electron configuration resembles that of <strong>xenon (Xe)<\/strong>, which has an atomic number of 54. Iodine (I) has 53 electrons, and by gaining one additional electron, I\u207b has 54 electrons, mirroring the electron configuration of xenon, which is [Kr]4d\u00b9\u20705s\u00b25p\u2076.<\/li>\n<\/ul>\n\n\n\n<p>The reason KI forms ionic bonds is due to the significant difference in electronegativity between potassium and iodine. Potassium, being a metal with low electronegativity, readily loses its outer electron, while iodine, a non-metal with higher electronegativity, readily accepts the electron. This results in the formation of oppositely charged ions, K\u207a and I\u207b, which are held together by strong electrostatic forces of attraction, characteristic of ionic bonds.<\/p>\n\n\n\n<p>The tendency of these ions to achieve electron configurations resembling those of inert gases is a driving force behind the formation of ionic compounds like KI. This process allows both ions to reach a stable, low-energy state akin to that of noble gases, which are chemically inert due to their full outer electron shells.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner5-970.jpeg\" alt=\"\" class=\"wp-image-246995\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Potassium iodide (KI) exhibits predominantly ionic bonding. Theandions have electron structures that are identical to which two inert gases? The Correct Answer and Explanation is: Potassium iodide (KI) exhibits predominantly ionic bonding, where potassium (K) donates an electron to become a positively charged ion (K\u207a), and iodine (I) accepts that electron to become a negatively [&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-246991","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246991","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=246991"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246991\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=246991"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=246991"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=246991"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}