{"id":29974,"date":"2025-06-21T13:50:50","date_gmt":"2025-06-21T13:50:50","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=29974"},"modified":"2025-06-21T13:50:51","modified_gmt":"2025-06-21T13:50:51","slug":"draw-the-lewis-structure-for-xenon-tetrafluoride-please-include-the-following-what-is-the-formula","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/draw-the-lewis-structure-for-xenon-tetrafluoride-please-include-the-following-what-is-the-formula\/","title":{"rendered":"Draw the Lewis structure for xenon tetrafluoride, please include the following: What is the formula"},"content":{"rendered":"\n

Draw the Lewis structure for xenon tetrafluoride, please include the following: What is the formula? How many valence electrons are available? Place the Xe in the center and make 4 bonds to F Complete the octets on the F atoms How many electrons remain? Place lone pairs of electrons on Xe. How many lone pairs are on Xe?<\/p>\n\n\n\n

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

Formula:<\/strong> The chemical formula is XeF\u2084<\/strong> (xenon tetrafluoride).<\/p>\n\n\n\n

\n\n\n\n

Step-by-Step Lewis Structure:<\/h3>\n\n\n\n
    \n
  1. Count Valence Electrons:<\/strong>\n
      \n
    • Xenon (Xe) is in group 18, so it has 8 valence electrons<\/strong>.<\/li>\n\n\n\n
    • Each fluorine (F) atom is in group 17 and has 7 valence electrons<\/strong>.<\/li>\n\n\n\n
    • There are 4 fluorine atoms, so total from fluorine = 4 \u00d7 7 = 28 electrons<\/strong>.<\/li>\n\n\n\n
    • Total valence electrons = 8 (Xe) + 28 (F) = 36 electrons.<\/strong><\/li>\n<\/ul>\n<\/li>\n\n\n\n
    • Structure Setup:<\/strong>\n
        \n
      • Place Xe<\/strong> in the center since it is the least electronegative.<\/li>\n\n\n\n
      • Attach 4 fluorine atoms to Xe with single bonds<\/strong> (each bond uses 2 electrons).<\/li>\n\n\n\n
      • 4 bonds \u00d7 2 electrons = 8 electrons<\/strong> used.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
      • Complete the Octets on Fluorine:<\/strong>
        • Each fluorine needs 6 more electrons to complete its octet.<\/li>
        • 4 fluorines \u00d7 6 electrons = 24 electrons<\/strong>.<\/li><\/ul>So far, 8 (bonds) + 24 (F lone pairs) = 32 electrons<\/strong> used.<\/li>\n\n\n\n
        • Electrons Remaining:<\/strong>\n
            \n
          • Total available: 36 electrons<\/li>\n\n\n\n
          • Used so far: 32 electrons<\/li>\n\n\n\n
          • Remaining: 36 \u2212 32 = 4 electrons<\/strong><\/li>\n<\/ul>\n<\/li>\n\n\n\n
          • Place Lone Pairs on Xe:<\/strong>\n
              \n
            • Place the remaining 4 electrons (or 2 lone pairs) on Xe.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n
              \n\n\n\n

              Final Structure:<\/h3>\n\n\n\n
                \n
              • Xe is bonded to four F atoms.<\/li>\n\n\n\n
              • Each F has 3 lone pairs (6 electrons) to complete its octet.<\/li>\n\n\n\n
              • Xe has 2 lone pairs<\/strong> on it.<\/li>\n\n\n\n
              • Total regions of electron density around Xe = 4 bonding + 2 lone pairs = 6 regions \u2192 square planar<\/strong> geometry.<\/li>\n<\/ul>\n\n\n\n
                \n\n\n\n

                Summary:<\/h3>\n\n\n\n
                  \n
                • Formula:<\/strong> XeF\u2084<\/li>\n\n\n\n
                • Total valence electrons:<\/strong> 36<\/li>\n\n\n\n
                • Electrons used in bonds:<\/strong> 8<\/li>\n\n\n\n
                • Electrons used on F atoms:<\/strong> 24<\/li>\n\n\n\n
                • Remaining electrons on Xe:<\/strong> 4<\/li>\n\n\n\n
                • Lone pairs on Xe:<\/strong> 2<\/li>\n<\/ul>\n\n\n\n

                  Xenon expands its octet and holds more than 8 electrons, which is allowed for elements in period 3 and beyond.<\/p>\n\n\n\n

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

                  Draw the Lewis structure for xenon tetrafluoride, please include the following: What is the formula? How many valence electrons are available? Place the Xe in the center and make 4 bonds to F Complete the octets on the F atoms How many electrons remain? Place lone pairs of electrons on Xe. How many lone pairs […]<\/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-29974","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/29974","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=29974"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/29974\/revisions"}],"predecessor-version":[{"id":29976,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/29974\/revisions\/29976"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=29974"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=29974"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=29974"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}