{"id":192070,"date":"2025-02-17T06:56:48","date_gmt":"2025-02-17T06:56:48","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=192070"},"modified":"2025-02-17T06:56:51","modified_gmt":"2025-02-17T06:56:51","slug":"in-each-rack-pick-the-compound-with-the-bigger-lattice-energy","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/17\/in-each-rack-pick-the-compound-with-the-bigger-lattice-energy\/","title":{"rendered":"in each rack, pick the compound with the bigger lattice energy"},"content":{"rendered":"\n<p>in each rack, pick the compound with the bigger lattice energy.<\/p>\n\n\n\n<p>note: lattice energy is always greater than zero.<\/p>\n\n\n\n<p>which compound has the bigger lattice energy?<\/p>\n\n\n\n<p>NaCl or Na2S<\/p>\n\n\n\n<p>KCl or KBr<\/p>\n\n\n\n<p>Li2O or BeO<\/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. NaCl vs Na2S:<\/h3>\n\n\n\n<p><strong>Answer: Na2S<\/strong><\/p>\n\n\n\n<p><strong>Explanation:<\/strong><br>Lattice energy is directly influenced by the charges of the ions involved and the ionic radii. The higher the charges on the ions, the greater the lattice energy, because stronger electrostatic forces result in a more stable lattice structure.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>NaCl consists of Na\u207a and Cl\u207b ions, whereas Na2S consists of Na\u207a and S\u00b2\u207b ions.<\/li>\n\n\n\n<li>The charge on the sulfur ion (S\u00b2\u207b) is -2, which is higher than the charge on the chloride ion (Cl\u207b) which is -1.<\/li>\n\n\n\n<li>The greater the charge on the ions, the stronger the electrostatic attraction, leading to a greater lattice energy. Therefore, Na2S has a higher lattice energy than NaCl.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">2. KCl vs KBr:<\/h3>\n\n\n\n<p><strong>Answer: KCl<\/strong><\/p>\n\n\n\n<p><strong>Explanation:<\/strong><br>Here, we are comparing potassium chloride (KCl) and potassium bromide (KBr). Both compounds contain potassium ions (K\u207a), but the anions are different.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The chloride ion (Cl\u207b) is smaller than the bromide ion (Br\u207b).<\/li>\n\n\n\n<li>Lattice energy increases with the smaller ion because the ions can get closer together, enhancing the electrostatic attraction.<\/li>\n\n\n\n<li>Since Cl\u207b is smaller than Br\u207b, KCl has a greater lattice energy than KBr.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">3. Li2O vs BeO:<\/h3>\n\n\n\n<p><strong>Answer: BeO<\/strong><\/p>\n\n\n\n<p><strong>Explanation:<\/strong><br>This is a comparison between lithium oxide (Li2O) and beryllium oxide (BeO), both of which contain highly charged oxide ions (O\u00b2\u207b).<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Li\u2082O has Li\u207a ions, while BeO has Be\u00b2\u207a ions. The charge on the Be\u00b2\u207a ion is higher than that of the Li\u207a ion, which leads to stronger electrostatic attraction between the ions in BeO.<\/li>\n\n\n\n<li>Additionally, the small size of the Be\u00b2\u207a ion compared to Li\u207a allows the ions to pack more tightly, increasing the lattice energy.<\/li>\n\n\n\n<li>As a result, BeO has a higher lattice energy than Li\u2082O.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Summary:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Na2S<\/strong> > <strong>NaCl<\/strong><\/li>\n\n\n\n<li><strong>KCl<\/strong> > <strong>KBr<\/strong><\/li>\n\n\n\n<li><strong>BeO<\/strong> > <strong>Li2O<\/strong><\/li>\n<\/ul>\n\n\n\n<p>Let me generate the image to visually explain these concepts.<\/p>\n\n\n\n<p>Here is the diagram illustrating the comparison of lattice energies between NaCl vs Na2S, KCl vs KBr, and Li2O vs BeO. It shows the ions involved, their charges, and the relationship between charge size and lattice energy. The arrows indicate the increasing lattice energy based on charge and ion size.<\/p>\n\n\n\n<p>Let me know if you need any further clarification!<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/02\/image-741.png\" alt=\"\" class=\"wp-image-192071\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>in each rack, pick the compound with the bigger lattice energy. note: lattice energy is always greater than zero. which compound has the bigger lattice energy? NaCl or Na2S KCl or KBr Li2O or BeO The Correct Answer and Explanation is : 1. NaCl vs Na2S: Answer: Na2S Explanation:Lattice energy is directly influenced by 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-192070","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/192070","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=192070"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/192070\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=192070"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=192070"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=192070"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}