{"id":170580,"date":"2024-11-19T21:26:31","date_gmt":"2024-11-19T21:26:31","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=170580"},"modified":"2024-11-19T21:26:33","modified_gmt":"2024-11-19T21:26:33","slug":"draw-the-best-lewis-structure-of-no%e2%82%83cl","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/19\/draw-the-best-lewis-structure-of-no%e2%82%83cl\/","title":{"rendered":"draw the best lewis structure of NO\u2083Cl"},"content":{"rendered":"\n

draw the best lewis structure of NO\u2083Cl. if applicable, include lone pairs of electrons and formal charges (minimized) in the lewis structure.<\/p>\n\n\n\n

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

To draw the best Lewis structure of NO\u2083Cl<\/strong>, we need to consider the following steps:<\/p>\n\n\n\n

Step 1: Determine the total number of valence electrons.<\/h3>\n\n\n\n
    \n
  • Nitrogen (N) is in Group 15, so it has 5 valence electrons.<\/li>\n\n\n\n
  • Oxygen (O) is in Group 16, so each oxygen atom has 6 valence electrons, and there are three oxygens, contributing ( 3 \\times 6 = 18 ) electrons.<\/li>\n\n\n\n
  • Chlorine (Cl) is in Group 17, so it has 7 valence electrons.<\/li>\n\n\n\n
  • Total valence electrons = ( 5 + 18 + 7 = 30 ) valence electrons.<\/li>\n<\/ul>\n\n\n\n

    Step 2: Determine the central atom.<\/h3>\n\n\n\n
      \n
    • The least electronegative atom (other than hydrogen) is typically the central atom. In this case, nitrogen (N) will be the central atom.<\/li>\n<\/ul>\n\n\n\n

      Step 3: Connect the atoms with single bonds.<\/h3>\n\n\n\n
        \n
      • Connect nitrogen to the three oxygen atoms with single bonds. Chlorine will be attached to one of the oxygens through a single bond. This accounts for ( 4 ) bonds, which use up ( 4 \\times 2 = 8 ) electrons.<\/li>\n<\/ul>\n\n\n\n

        Step 4: Distribute the remaining electrons.<\/h3>\n\n\n\n
          \n
        • After using 8 electrons for bonding, ( 30 – 8 = 22 ) electrons remain.<\/li>\n\n\n\n
        • Place lone pairs around the oxygen atoms and chlorine. Chlorine typically forms only one bond and has three lone pairs, while oxygen atoms will get lone pairs as well.<\/li>\n<\/ul>\n\n\n\n

          Step 5: Check formal charges and adjust if necessary.<\/h3>\n\n\n\n
            \n
          • The formal charge on an atom is calculated using the formula:
            [ \\text{Formal charge} = \\text{Valence electrons} – (\\text{Lone electrons} + \\frac{1}{2} \\text{Bonding electrons}) ]<\/li>\n\n\n\n
          • Aim to minimize formal charges by adjusting bonds. Typically, a double bond between nitrogen and one oxygen will reduce formal charges.<\/li>\n<\/ul>\n\n\n\n

            Final Lewis Structure:<\/h3>\n\n\n\n

            The final structure shows:<\/p>\n\n\n\n

              \n
            • Nitrogen (N) at the center, with a double bond to one oxygen, single bonds to the other two oxygens.<\/li>\n\n\n\n
            • The chlorine atom is bonded to one oxygen atom.<\/li>\n\n\n\n
            • Each oxygen atom (except the doubly bonded one) will have lone pairs to complete their octet.<\/li>\n\n\n\n
            • The formal charge on nitrogen is 0, on oxygen (double-bonded) is 0, on oxygens (single-bonded) is -1, and on chlorine is 0.<\/li>\n<\/ul>\n\n\n\n

              This structure minimizes formal charges and satisfies the octet rule for most atoms.<\/p>\n","protected":false},"excerpt":{"rendered":"

              draw the best lewis structure of NO\u2083Cl. if applicable, include lone pairs of electrons and formal charges (minimized) in the lewis structure. The Correct Answer and Explanation is : To draw the best Lewis structure of NO\u2083Cl, we need to consider the following steps: Step 1: Determine the total number of valence electrons. Step 2: […]<\/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-170580","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/170580","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=170580"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/170580\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=170580"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=170580"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=170580"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}