{"id":36109,"date":"2025-06-25T03:07:38","date_gmt":"2025-06-25T03:07:38","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=36109"},"modified":"2025-06-25T03:07:40","modified_gmt":"2025-06-25T03:07:40","slug":"draw-a-lewis-structure-for-so2-in-which-all-atoms-obey-the-octet-rule","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/draw-a-lewis-structure-for-so2-in-which-all-atoms-obey-the-octet-rule\/","title":{"rendered":"Draw a Lewis structure for SO2 in which all atoms obey the octet rule"},"content":{"rendered":"\n

Draw a Lewis structure for SO2
in which all atoms obey the octet rule. Show formal charges. Do not consider ringed structures.<\/p>\n\n\n\n

\"\"<\/figure>\n\n\n\n

To correctly draw a Lewis structure for sulfur dioxide (SO\u2082)<\/strong> in which all atoms obey the octet rule<\/strong> and formal charges are shown<\/strong>, let us analyze the given options in your image. There are three Lewis structures shown. We will evaluate them and select the correct one.<\/p>\n\n\n\n

\n\n\n\n

Step-by-Step Analysis:<\/h3>\n\n\n\n
    \n
  1. Total Valence Electrons<\/strong>:\n
      \n
    • Sulfur (S) has 6 valence electrons.<\/li>\n\n\n\n
    • Oxygen (O) has 6 valence electrons.<\/li>\n\n\n\n
    • SO\u2082 has 1 sulfur and 2 oxygen atoms:
      \u2192 6 (S) + 6\u00d72 (O) = 18 valence electrons<\/strong> total.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
    • Octet Rule<\/strong>:
      Each atom (S and O) should have 8 electrons around it (shared and lone pairs).<\/li>\n\n\n\n
    • Formal Charges<\/strong>:
      We calculate formal charges to find the most stable structure. The formula is: Formal\u00a0charge=Valence\u00a0electrons\u2212(Lone\u00a0pair\u00a0electrons\u00a0+\u00a0\u00bd\u00a0Bonding\u00a0electrons)\\text{Formal charge} = \\text{Valence electrons} – \\text{(Lone pair electrons + \u00bd Bonding electrons)}Formal\u00a0charge=Valence\u00a0electrons\u2212(Lone\u00a0pair\u00a0electrons\u00a0+\u00a0\u00bd\u00a0Bonding\u00a0electrons)<\/li>\n<\/ol>\n\n\n\n
      \n\n\n\n

      Structure Evaluation:<\/h3>\n\n\n\n

      From the three structures shown in the image:<\/p>\n\n\n\n

        \n
      • Left structure<\/strong>: Both S=O bonds with no lone pair on sulfur.\n
          \n
        • Sulfur has 4 bonding pairs (8 electrons total), so octet is satisfied.<\/li>\n\n\n\n
        • But if you calculate formal charges, both O atoms have 0<\/strong> and sulfur has +2<\/strong>, which is less favorable.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
        • Middle structure<\/strong>: One S=O double bond and one S\u2013O single bond with a negative formal charge on one oxygen and a positive charge on sulfur.\n
            \n
          • Formal charges<\/strong>:\n
              \n
            • Sulfur: +1<\/li>\n\n\n\n
            • Single-bonded O: \u20131<\/li>\n\n\n\n
            • Double-bonded O: 0<\/li>\n\n\n\n
            • This adds up to a net formal charge of 0, and all atoms follow the octet rule.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
            • This is the correct and most stable structure<\/strong>.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
            • Right structure<\/strong>: Similar to the middle one but the position of the double bond is switched.\n
                \n
              • This is a resonance structure<\/strong> of the middle one.<\/li>\n\n\n\n
              • It is equally correct<\/strong> and contributes to the resonance hybrid.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n
                \n\n\n\n

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

                \u2705 The middle and right<\/strong> structures are correct Lewis structures for SO\u2082.
                They follow the octet rule and show proper formal charges (\u20131 on one O, +1 on S).<\/p>\n\n\n\n

                These two are resonance structures<\/strong> of SO\u2082, and the true structure is a resonance hybrid<\/strong> of both.<\/p>\n\n\n\n

                \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

                Draw a Lewis structure for SO2in which all atoms obey the octet rule. Show formal charges. Do not consider ringed structures. To correctly draw a Lewis structure for sulfur dioxide (SO\u2082) in which all atoms obey the octet rule and formal charges are shown, let us analyze the given options in your image. There are […]<\/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-36109","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/36109","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=36109"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/36109\/revisions"}],"predecessor-version":[{"id":36112,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/36109\/revisions\/36112"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=36109"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=36109"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=36109"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}