{"id":27334,"date":"2025-06-19T22:16:00","date_gmt":"2025-06-19T22:16:00","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=27334"},"modified":"2025-06-19T22:16:03","modified_gmt":"2025-06-19T22:16:03","slug":"which-of-the-following-has-greatest-lattice-energy","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/which-of-the-following-has-greatest-lattice-energy\/","title":{"rendered":"Which of the following has greatest lattice energy"},"content":{"rendered":"\n<p>Which of the following has greatest lattice energy? MgBr2 MgF2 MgCl2 MgI<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-vivid-green-cyan-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>The correct answer is: <strong>MgF\u2082<\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p><strong>Lattice energy<\/strong> is the energy released when one mole of an ionic crystalline compound is formed from its gaseous ions. It is a measure of the strength of the forces holding the ions together in an ionic solid.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">Factors Affecting Lattice Energy:<\/h4>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Charge of the ions<\/strong><br>Greater charges on the ions result in a stronger electrostatic attraction and higher lattice energy.<\/li>\n\n\n\n<li><strong>Size (radius) of the ions<\/strong><br>Smaller ions can pack more closely, resulting in stronger attraction between the oppositely charged ions and thus higher lattice energy.<\/li>\n<\/ol>\n\n\n\n<p>All the compounds listed \u2014 MgF\u2082, MgCl\u2082, MgBr\u2082, and MgI\u2082 \u2014 contain the <strong>same cation<\/strong>, Mg\u00b2\u207a, which has a +2 charge. So, to determine the compound with the <strong>greatest lattice energy<\/strong>, we compare the <strong>anions<\/strong>:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>F\u207b (fluoride):<\/strong> smallest radius<\/li>\n\n\n\n<li><strong>Cl\u207b (chloride):<\/strong> larger than F\u207b<\/li>\n\n\n\n<li><strong>Br\u207b (bromide):<\/strong> larger than Cl\u207b<\/li>\n\n\n\n<li><strong>I\u207b (iodide):<\/strong> largest<\/li>\n<\/ul>\n\n\n\n<p>Because <strong>F\u207b is the smallest anion<\/strong>, it allows the Mg\u00b2\u207a cation to come closer, which increases the electrostatic force and results in a greater lattice energy. As the anion size increases from F\u207b to I\u207b, the distance between the centers of the ions increases, reducing the lattice energy.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">Ranking of lattice energy (from greatest to least):<\/h4>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>MgF\u2082<\/strong> (smallest anion, highest lattice energy)<\/li>\n\n\n\n<li><strong>MgCl\u2082<\/strong><\/li>\n\n\n\n<li><strong>MgBr\u2082<\/strong><\/li>\n\n\n\n<li><strong>MgI\u2082<\/strong> (largest anion, lowest lattice energy)<\/li>\n<\/ol>\n\n\n\n<p>Therefore, <strong>MgF\u2082<\/strong> has the <strong>greatest lattice energy<\/strong> due to the <strong>small size<\/strong> of the fluoride ion and the strong attraction it forms with the Mg\u00b2\u207a ion.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"722\" height=\"1024\" src=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner10-127.jpeg\" alt=\"\" class=\"wp-image-27339\" srcset=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner10-127.jpeg 722w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner10-127-212x300.jpeg 212w\" sizes=\"auto, (max-width: 722px) 100vw, 722px\" \/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Which of the following has greatest lattice energy? MgBr2 MgF2 MgCl2 MgI The Correct Answer and Explanation is: The correct answer is: MgF\u2082 Explanation: Lattice energy is the energy released when one mole of an ionic crystalline compound is formed from its gaseous ions. It is a measure of the strength of the forces holding [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1],"tags":[],"class_list":["post-27334","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/27334","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/comments?post=27334"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/27334\/revisions"}],"predecessor-version":[{"id":27340,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/27334\/revisions\/27340"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=27334"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=27334"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=27334"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}