{"id":267103,"date":"2025-07-23T09:33:32","date_gmt":"2025-07-23T09:33:32","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=267103"},"modified":"2025-07-23T09:33:34","modified_gmt":"2025-07-23T09:33:34","slug":"draw-the-lewis-dot-structure-for-tellurium-dioxide-teo","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/23\/draw-the-lewis-dot-structure-for-tellurium-dioxide-teo\/","title":{"rendered":"Draw the Lewis dot structure for tellurium dioxide, TeO"},"content":{"rendered":"\n

Draw the Lewis dot structure for tellurium dioxide, TeO
. The bonding can be best described as: A single bond and a triple bond A single bond a double bond Two double bonds Two single bonds<\/p>\n\n\n\n

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

To draw the Lewis dot structure for tellurium dioxide (TeO2), let’s follow these steps:<\/p>\n\n\n\n

    \n
  1. Count the valence electrons:<\/strong>\n
      \n
    • Tellurium (Te) is in Group 16, so it has 6 valence electrons.<\/li>\n\n\n\n
    • Oxygen (O) is also in Group 16, and each oxygen atom has 6 valence electrons.<\/li>\n\n\n\n
    • For TeO2, there are 6 + (2 \u00d7 6) = 18 valence electrons to account for.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
    • Determine the skeleton structure:<\/strong>\n
        \n
      • Since Te is less electronegative than O, Te will be the central atom, and the two O atoms will be bonded to it.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
      • Distribute the electrons:<\/strong>\n
          \n
        • Place single bonds between Te and each O atom. Each single bond uses 2 electrons (1 from Te and 1 from O).<\/li>\n\n\n\n
        • This consumes 4 electrons (2 electrons per bond \u00d7 2 bonds).<\/li>\n<\/ul>\n<\/li>\n\n\n\n
        • Complete the octets for oxygen atoms:<\/strong>\n
            \n
          • Each oxygen atom now has 2 electrons from the single bond. To complete the octet, we need to add 6 more electrons to each oxygen atom. So, each O gets 3 lone pairs (3 \u00d7 2 = 6 electrons).<\/li>\n<\/ul>\n<\/li>\n\n\n\n
          • Allocate remaining electrons to Te:<\/strong>\n
              \n
            • After distributing electrons to the oxygen atoms, there are 18 \u2212 4 \u2212 12 = 2 electrons left. These 2 electrons should be placed as a lone pair on the central tellurium atom.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
            • Check for double bonds:<\/strong>\n
                \n
              • To ensure all atoms have full octets, we recognize that Te can form a double bond with each O atom. The extra lone pair electrons on the O atoms are shared, forming double bonds with Te.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
              • Final structure:<\/strong>\n
                  \n
                • The final structure consists of two double bonds between Te and the two O atoms, with 2 lone pairs on Te and 2 lone pairs on each O.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n

                  So, the correct answer is: Two double bonds.<\/strong><\/p>\n\n\n\n

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

                  Tellurium dioxide (TeO2) has a central Te atom double-bonded to two oxygen atoms. The double bonds help satisfy the octet rule for oxygen, and tellurium can accommodate more than 8 electrons in its valence shell, as it’s in the 4th period of the periodic table. The resulting structure is stable, with all atoms satisfying their<\/p>\n\n\n\n

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

                  Draw the Lewis dot structure for tellurium dioxide, TeO. The bonding can be best described as: A single bond and a triple bond A single bond a double bond Two double bonds Two single bonds The Correct Answer and Explanation is: To draw the Lewis dot structure for tellurium dioxide (TeO2), let’s follow these steps: […]<\/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-267103","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/267103","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=267103"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/267103\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=267103"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=267103"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=267103"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}