{"id":190074,"date":"2025-02-11T06:22:01","date_gmt":"2025-02-11T06:22:01","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=190074"},"modified":"2025-02-11T06:22:03","modified_gmt":"2025-02-11T06:22:03","slug":"draw-a-suitable-lewis-structure-for-li2s","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/11\/draw-a-suitable-lewis-structure-for-li2s\/","title":{"rendered":"Draw a suitable Lewis structure for Li2S"},"content":{"rendered":"\n

Draw a suitable Lewis structure for Li2S. In the structure,
A. there are two lithium ions each with a +1 charge and and one sulfide ion with four pairs of electrons and a -2 charge.<\/p>\n\n\n\n

B. there are two sulfide ions and one lithium ion.<\/p>\n\n\n\n

C. there are wto lithium atoms and one sulfur atom with 6 electrons.<\/p>\n\n\n\n

D. each lithium atom makes one bond to sulfur.<\/p>\n\n\n\n

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

The correct answer is A<\/strong>.<\/p>\n\n\n\n

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

Lithium sulfide (Li\u2082S) consists of two lithium (Li) atoms and one sulfur (S) atom. To determine the Lewis structure of Li\u2082S, we need to consider the electronic configuration and bonding behavior of lithium and sulfur.<\/p>\n\n\n\n

    \n
  1. Lithium’s Electron Configuration:<\/strong><\/li>\n<\/ol>\n\n\n\n
      \n
    • Lithium is an alkali metal with the electron configuration ( 1s^2 2s^1 ).<\/li>\n\n\n\n
    • Lithium atoms tend to lose one electron to achieve a stable electron configuration, which results in a lithium ion (( Li^+ )) with a +1 charge.<\/li>\n<\/ul>\n\n\n\n
        \n
      1. Sulfur’s Electron Configuration:<\/strong><\/li>\n<\/ol>\n\n\n\n
          \n
        • Sulfur is a non-metal in Group 16 with an electron configuration of ( [Ne] 3s^2 3p^4 ).<\/li>\n\n\n\n
        • Sulfur needs to gain two electrons to complete its octet and achieve a stable electron configuration. Thus, sulfur tends to form a sulfide ion (( S^{2-} )) with a -2 charge.<\/li>\n<\/ul>\n\n\n\n
            \n
          1. Ionic Bonding in Li\u2082S:<\/strong><\/li>\n<\/ol>\n\n\n\n
              \n
            • Lithium atoms each lose one electron, forming two ( Li^+ ) ions.<\/li>\n\n\n\n
            • The sulfur atom gains two electrons to form one ( S^{2-} ) ion.<\/li>\n\n\n\n
            • The electrostatic attraction between the ( Li^+ ) ions and the ( S^{2-} ) ion holds the compound together.<\/li>\n<\/ul>\n\n\n\n

              Lewis Structure of Li\u2082S:<\/h3>\n\n\n\n
                \n
              • The two lithium ions (( Li^+ )) are each surrounded by a +1 charge.<\/li>\n\n\n\n
              • The sulfide ion (( S^{2-} )) has four pairs of electrons around it, making it negatively charged with a -2 charge.<\/li>\n\n\n\n
              • Since lithium donates one electron and sulfur accepts two electrons, we end up with a formula of ( Li_2S ), where the ionic charges are balanced.<\/li>\n<\/ul>\n\n\n\n

                Thus, option A<\/strong> correctly describes the structure of Li\u2082S with two lithium ions, each with a +1 charge, and one sulfide ion with four pairs of electrons and a -2 charge.<\/p>\n","protected":false},"excerpt":{"rendered":"

                Draw a suitable Lewis structure for Li2S. In the structure,A. there are two lithium ions each with a +1 charge and and one sulfide ion with four pairs of electrons and a -2 charge. B. there are two sulfide ions and one lithium ion. C. there are wto lithium atoms and one sulfur atom with […]<\/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-190074","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/190074","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=190074"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/190074\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=190074"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=190074"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=190074"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}