{"id":207280,"date":"2025-04-21T09:31:53","date_gmt":"2025-04-21T09:31:53","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=207280"},"modified":"2025-04-21T09:31:55","modified_gmt":"2025-04-21T09:31:55","slug":"which-of-the-following-ionic-compounds-has-the-largest-lattice-energy-i-e-the-lattice-energy-most-favorable-to-a-stable-lattice","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/04\/21\/which-of-the-following-ionic-compounds-has-the-largest-lattice-energy-i-e-the-lattice-energy-most-favorable-to-a-stable-lattice\/","title":{"rendered":"Which of the following ionic compounds has the largest lattice energy (i.e., the lattice energy most favorable to a stable lattice)"},"content":{"rendered":"\n<p>Which of the following ionic compounds has the largest lattice energy (i.e., the lattice energy most favorable to a stable lattice)?<\/p>\n\n\n\n<p>a) BaO<br>b) BeO<br>c) CsI<br>d) NaBr<br>e) BaS<\/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 answer is <strong>b) BeO<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>Lattice energy refers to the energy released when ions in the gas phase combine to form an ionic solid. The lattice energy is influenced by two key factors:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Charge of the ions<\/strong>: The higher the charge on the ions, the greater the lattice energy. This is because the electrostatic force between ions increases with the magnitude of their charges.<\/li>\n\n\n\n<li><strong>Size of the ions<\/strong>: Smaller ions have higher lattice energies because the distance between the ion centers is smaller, resulting in a stronger Coulomb attraction between the oppositely charged ions.<\/li>\n<\/ol>\n\n\n\n<p>To determine which compound has the largest lattice energy, we need to evaluate these two factors for each ionic compound:<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">1. <strong>BaO<\/strong>:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Ba\u00b2\u207a<\/strong> (charge 2) and <strong>O\u00b2\u207b<\/strong> (charge 2).<\/li>\n\n\n\n<li>Ba\u00b2\u207a is relatively large, and the ionic size of Ba\u00b2\u207a is considerably bigger than that of smaller ions like Be\u00b2\u207a. The large size of Ba\u00b2\u207a reduces the lattice energy despite the high charge on both ions.<\/li>\n\n\n\n<li><strong>Result<\/strong>: Lower lattice energy compared to BeO.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">2. <strong>BeO<\/strong>:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Be\u00b2\u207a<\/strong> (charge 2) and <strong>O\u00b2\u207b<\/strong> (charge 2).<\/li>\n\n\n\n<li>Be\u00b2\u207a is much smaller than Ba\u00b2\u207a, and O\u00b2\u207b is the same size in both cases. The small size of Be\u00b2\u207a leads to a much stronger Coulomb attraction between Be\u00b2\u207a and O\u00b2\u207b, resulting in a very high lattice energy.<\/li>\n\n\n\n<li><strong>Result<\/strong>: BeO has the largest lattice energy.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">3. <strong>CsI<\/strong>:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Cs\u207a<\/strong> (charge 1) and <strong>I\u207b<\/strong> (charge 1).<\/li>\n\n\n\n<li>Both ions are relatively large (Cs\u207a is much larger than Be\u00b2\u207a), and the charge on both ions is only \u00b11. This significantly reduces the lattice energy compared to compounds with higher charges.<\/li>\n\n\n\n<li><strong>Result<\/strong>: Lower lattice energy.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">4. <strong>NaBr<\/strong>:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Na\u207a<\/strong> (charge 1) and <strong>Br\u207b<\/strong> (charge 1).<\/li>\n\n\n\n<li>Similar reasoning as CsI applies here, with the ions being large and the charges low.<\/li>\n\n\n\n<li><strong>Result<\/strong>: Lower lattice energy.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">5. <strong>BaS<\/strong>:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Ba\u00b2\u207a<\/strong> (charge 2) and <strong>S\u00b2\u207b<\/strong> (charge 2).<\/li>\n\n\n\n<li>While both ions have a high charge, Ba\u00b2\u207a is large, which lowers the lattice energy compared to smaller ions.<\/li>\n\n\n\n<li><strong>Result<\/strong>: Lower lattice energy than BeO.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Conclusion:<\/h3>\n\n\n\n<p>BeO has the smallest ionic radii for its divalent cation (Be\u00b2\u207a), and both ions carry a high charge, leading to the largest lattice energy, which corresponds to a more stable lattice.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/04\/image-203.png\" alt=\"\" class=\"wp-image-207281\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Which of the following ionic compounds has the largest lattice energy (i.e., the lattice energy most favorable to a stable lattice)? a) BaOb) BeOc) CsId) NaBre) BaS The correct answer and explanation is : The correct answer is b) BeO. Explanation: Lattice energy refers to the energy released when ions in the gas phase combine [&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-207280","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/207280","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=207280"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/207280\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=207280"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=207280"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=207280"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}