{"id":168229,"date":"2024-11-16T21:02:39","date_gmt":"2024-11-16T21:02:39","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=168229"},"modified":"2024-11-16T21:02:41","modified_gmt":"2024-11-16T21:02:41","slug":"which-of-the-following-pairs-would-have-the-greatest-coulombic-attraction-in-a-solid-compound","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/16\/which-of-the-following-pairs-would-have-the-greatest-coulombic-attraction-in-a-solid-compound\/","title":{"rendered":"Which of the following pairs would have the greatest coulombic attraction in a solid compound"},"content":{"rendered":"\n

Which of the following pairs would have the greatest coulombic attraction in a solid compound? 1. mg2+, S2- 2. mg2+, se2- 3.mg2+, O2-<\/p>\n\n\n\n

The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n

The correct answer is Option 3: Mg\u00b2\u207a and O\u00b2\u207b<\/strong>.<\/p>\n\n\n\n

Explanation:<\/h3>\n\n\n\n

Coulombic attraction refers to the electrostatic force between positively and negatively charged ions, which depends on two key factors: the charge<\/strong> of the ions and the distance<\/strong> between them (which is influenced by the size of the ions). The force can be described by Coulomb\u2019s Law:<\/p>\n\n\n\n

[
F = \\frac{{k \\cdot |q_1 \\cdot q_2|}}{{r^2}}
]<\/p>\n\n\n\n

Where:<\/p>\n\n\n\n

    \n
  • (F) is the force of attraction,<\/li>\n\n\n\n
  • (k) is Coulomb\u2019s constant,<\/li>\n\n\n\n
  • (q_1) and (q_2) are the charges of the ions,<\/li>\n\n\n\n
  • (r) is the distance between the ions (related to their ionic radii).<\/li>\n<\/ul>\n\n\n\n

    Analyzing the Options:<\/h3>\n\n\n\n
      \n
    1. Mg\u00b2\u207a and S\u00b2\u207b<\/strong>:
      Magnesium (Mg) has a +2 charge, and sulfur (S) has a -2 charge. While both ions have relatively large charges, sulfur\u2019s ionic radius is relatively larger than that of oxygen or selenium. This means that the distance between the ions will be greater, which results in a weaker Coulombic attraction compared to pairs with smaller ions.<\/li>\n\n\n\n
    2. Mg\u00b2\u207a and Se\u00b2\u207b<\/strong>:
      Selenium (Se) also has a -2 charge, similar to sulfur, but it has a larger ionic radius<\/strong> than sulfur. As a result, the distance between the Mg\u00b2\u207a and Se\u00b2\u207b ions will be even larger, leading to a weaker Coulombic attraction than between Mg\u00b2\u207a and O\u00b2\u207b.<\/li>\n\n\n\n
    3. Mg\u00b2\u207a and O\u00b2\u207b<\/strong>:
      Oxygen (O) has a -2 charge, and it has the smallest ionic radius<\/strong> among the three anions (S\u00b2\u207b, Se\u00b2\u207b, O\u00b2\u207b). Magnesium\u2019s ionic radius is relatively small as well. Because of the smaller size of the ions, the distance between Mg\u00b2\u207a and O\u00b2\u207b ions will be the smallest, resulting in the greatest Coulombic attraction. Additionally, the +2 and -2 charges are strong, further contributing to a stronger attraction.<\/li>\n<\/ol>\n\n\n\n

      Conclusion:<\/h3>\n\n\n\n

      The Coulombic attraction is strongest between Mg\u00b2\u207a and O\u00b2\u207b<\/strong> because the ions are both small in size, leading to a short distance between them and a stronger electrostatic force of attraction. Therefore, Option 3<\/strong> is the correct answer.<\/p>\n","protected":false},"excerpt":{"rendered":"

      Which of the following pairs would have the greatest coulombic attraction in a solid compound? 1. mg2+, S2- 2. mg2+, se2- 3.mg2+, O2- The Correct Answer and Explanation is: The correct answer is Option 3: Mg\u00b2\u207a and O\u00b2\u207b. Explanation: Coulombic attraction refers to the electrostatic force between positively and negatively charged ions, which depends on […]<\/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-168229","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/168229","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=168229"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/168229\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=168229"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=168229"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=168229"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}