{"id":265477,"date":"2025-07-22T06:44:41","date_gmt":"2025-07-22T06:44:41","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=265477"},"modified":"2025-07-22T06:44:43","modified_gmt":"2025-07-22T06:44:43","slug":"draw-the-lewis-structures-of-s22-ions-giving-all-the-steps","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/22\/draw-the-lewis-structures-of-s22-ions-giving-all-the-steps\/","title":{"rendered":"Draw the Lewis structures of S2^2- ions giving all the steps."},"content":{"rendered":"\n

Draw the Lewis structures of S2^2- ions giving all the steps.<\/p>\n\n\n\n

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

To draw the Lewis structure of the S22\u2212S_2^{2-}S22\u2212\u200b ion (a di-sulfide anion with a charge of -2), we follow these steps:<\/p>\n\n\n\n

Step 1: Determine the total number of valence electrons<\/h3>\n\n\n\n

Sulfur (S) is in group 16 of the periodic table, so each sulfur atom has 6 valence electrons. For the S22\u2212S_2^{2-}S22\u2212\u200b ion, the total number of electrons is: 6(from each sulfur)\u00d72(atoms)+2(extra electrons from the -2 charge)=14\u2009electrons6 (\\text{from each sulfur}) \\times 2 (\\text{atoms}) + 2 (\\text{extra electrons from the -2 charge}) = 14 \\, \\text{electrons}6(from each sulfur)\u00d72(atoms)+2(extra electrons from the -2 charge)=14electrons<\/p>\n\n\n\n

Step 2: Sketch the basic structure<\/h3>\n\n\n\n

Start by placing the two sulfur atoms next to each other, as they are bonded in the ion. Each sulfur atom will form a bond with the other sulfur atom.<\/p>\n\n\n\n

Step 3: Distribute the electrons<\/h3>\n\n\n\n
    \n
  • Place a single bond (which consists of two electrons) between the two sulfur atoms.<\/li>\n\n\n\n
  • This leaves 12 electrons (14 – 2 = 12) to be distributed as lone pairs around the atoms.<\/li>\n<\/ul>\n\n\n\n

    Step 4: Complete the octets<\/h3>\n\n\n\n
      \n
    • Give each sulfur atom 3 lone pairs of electrons (6 electrons per sulfur atom), which accounts for 12 electrons (6 electrons per sulfur \u00d7 2 atoms).<\/li>\n\n\n\n
    • After placing the lone pairs, each sulfur atom will have 8 electrons, satisfying the octet rule.<\/li>\n<\/ul>\n\n\n\n

      Step 5: Check for formal charges<\/h3>\n\n\n\n
        \n
      • In the structure, each sulfur atom has 6 valence electrons in lone pairs and 2 electrons in the bond with the other sulfur. This means each sulfur atom has 7 electrons, which leads to a formal charge of -1 on each sulfur.<\/li>\n\n\n\n
      • The total charge on the ion is -2, so the formal charges are correct.<\/li>\n<\/ul>\n\n\n\n

        Final structure:<\/h3>\n\n\n\n

        The structure consists of a single bond between two sulfur atoms, each surrounded by 3 lone pairs. The overall charge of the ion is -2.<\/p>\n\n\n\n

        Lewis Structure:<\/h4>\n\n\n\n
        ruby:S:S:
        <\/code><\/pre>\n\n\n\n
        Each sulfur atom has three lone pairs of electrons, and there is a single bond between them, with the overall charge being -2.<\/p>\n\n\n\n
        \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"
        Draw the Lewis structures of S2^2- ions giving all the steps. The Correct Answer and Explanation is: To draw the Lewis structure of the S22\u2212S_2^{2-}S22\u2212\u200b ion (a di-sulfide anion with a charge of -2), we follow these steps: Step 1: Determine the total number of valence electrons Sulfur (S) is in group 16 of the […]<\/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-265477","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/265477","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=265477"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/265477\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=265477"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=265477"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=265477"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}