{"id":229817,"date":"2025-06-08T13:04:00","date_gmt":"2025-06-08T13:04:00","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=229817"},"modified":"2025-06-08T13:04:03","modified_gmt":"2025-06-08T13:04:03","slug":"question-25-2-5-pts-what-is-the-correct-lewis-structure-for-oxygen-difluoride-molecule-of","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/08\/question-25-2-5-pts-what-is-the-correct-lewis-structure-for-oxygen-difluoride-molecule-of\/","title":{"rendered":"Question 25 2.5 pts What is the correct Lewis structure for oxygen difluoride molecule, OF"},"content":{"rendered":"\n

Question 25 2.5 pts What is the correct Lewis structure for oxygen difluoride molecule, OF
?
F::O::F
F::O::F
F::O::F
F::O::F
:F::O::F:<\/p>\n\n\n\n

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

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

ChatGPT said:<\/h6>\n\n\n\n

The correct Lewis structure for the oxygen difluoride (OF\u2082) molecule is the last option<\/strong> (fifth one):<\/p>\n\n\n\n

:F\u2013O\u2013F:<\/code><\/strong>
Each fluorine (F) atom has three lone pairs<\/strong>, and the oxygen (O) atom has two lone pairs<\/strong>, with single bonds<\/strong> connecting O to each F atom.<\/p>\n\n\n\n

\n\n\n\n

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

Oxygen difluoride (OF\u2082)<\/strong> consists of one oxygen atom bonded to two fluorine atoms. To determine the correct Lewis structure, follow these steps:<\/p>\n\n\n\n

\n\n\n\n

1. Count Valence Electrons:<\/strong><\/h3>\n\n\n\n
    \n
  • Oxygen (O) has 6 valence electrons.<\/li>\n\n\n\n
  • Fluorine (F) has 7 valence electrons, and there are two F atoms.
    Total valence electrons = 6 (O) + 7\u00d72 (F) = 20 electrons<\/strong><\/li>\n<\/ul>\n\n\n\n
    \n\n\n\n

    2. Determine Atom Placement:<\/strong><\/h3>\n\n\n\n

    Oxygen is less electronegative<\/strong> than fluorine, so it is the central atom<\/strong>, with the two fluorines bonded to it.<\/p>\n\n\n\n

    \n\n\n\n

    3. Create Single Bonds:<\/strong><\/h3>\n\n\n\n

    Create single bonds between O and each F:<\/p>\n\n\n\n

      \n
    • 2 single bonds = 2\u00d72 = 4 electrons used<\/li>\n\n\n\n
    • Remaining electrons = 20 \u2013 4 = 16 electrons<\/li>\n<\/ul>\n\n\n\n
      \n\n\n\n

      4. Distribute Remaining Electrons as Lone Pairs:<\/strong><\/h3>\n\n\n\n
        \n
      • Each F needs 3 lone pairs (6 electrons), so 2 Fs = 12 electrons<\/li>\n\n\n\n
      • 4 electrons remain, which go as 2 lone pairs on O<\/strong><\/li>\n<\/ul>\n\n\n\n

        Now, each atom has a full octet:<\/p>\n\n\n\n

          \n
        • Fluorines: 1 bond + 6 electrons = 8 electrons<\/li>\n\n\n\n
        • Oxygen: 2 bonds + 4 electrons (2 lone pairs) = 8 electrons<\/li>\n<\/ul>\n\n\n\n
          \n\n\n\n

          5. Check Formal Charges:<\/strong><\/h3>\n\n\n\n

          All atoms have formal charges of zero<\/strong>. This confirms that this is the most stable structure.<\/p>\n\n\n\n

          \n\n\n\n

          6. Molecular Shape:<\/strong><\/h3>\n\n\n\n

          Though not required for the Lewis structure itself, it’s worth noting:
          OF\u2082 has a bent shape<\/strong> due to the two lone pairs on oxygen (similar to H\u2082O), and the bond angle is slightly less than 109.5\u00b0 due to lone pair repulsion.<\/p>\n\n\n\n

          \n\n\n\n

          Conclusion:<\/h3>\n\n\n\n

          The correct Lewis structure is the one showing oxygen in the center, with two single bonds to fluorine atoms, and lone pairs properly distributed:
          :F\u2013O\u2013F:<\/code><\/strong><\/p>\n\n\n\n

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

          Question 25 2.5 pts What is the correct Lewis structure for oxygen difluoride molecule, OF?F::O::FF::O::FF::O::FF::O::F:F::O::F: The Correct Answer and Explanation is: ChatGPT said: The correct Lewis structure for the oxygen difluoride (OF\u2082) molecule is the last option (fifth one): :F\u2013O\u2013F:Each fluorine (F) atom has three lone pairs, and the oxygen (O) atom has two lone […]<\/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-229817","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/229817","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=229817"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/229817\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=229817"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=229817"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=229817"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}