The Lewis dot structure for diatomic oxygen (O2) can be drawn as follows:<\/p>\n\n\n\n
O=O<\/strong> with each oxygen atom having 6 valence electrons, and each shared pair of electrons forming a covalent bond between the two oxygen atoms. Here’s a breakdown:<\/p>\n\n\n\n Each oxygen atom has 6 valence electrons (since oxygen is in Group 16 of the periodic table). So for O2, the total number of valence electrons is:6 electrons\u00d72 atoms=12 electrons.6 \\text{ electrons} \\times 2 \\text{ atoms} = 12 \\text{ electrons}.6 electrons\u00d72 atoms=12 electrons.<\/p>\n\n\n\n Oxygen atoms form a double bond in the O2 molecule. We place the two oxygen atoms next to each other and draw two shared electron pairs between them, symbolized as a double line (O=O). This uses 4 of the 12 available electrons.<\/p>\n\n\n\n After forming the double bond, we have 8 electrons left (12 total – 4 for the bond). Each oxygen atom has 4 electrons left to be distributed as lone pairs. Each oxygen will have two lone pairs (each lone pair is 2 electrons), so that both oxygen atoms now have 8 electrons around them: 2 electrons from the double bond and 4 electrons as lone pairs.<\/p>\n\n\n\n :O=O:\\text{:O=O:}:O=O:<\/p>\n\n\n\n Where the colon (:) represents lone pairs of electrons. Each oxygen atom has 2 lone pairs (on top and bottom), and the two oxygen atoms share 2 pairs of electrons in the double bond.<\/p>\n\n\n\n This is the correct Lewis dot structure for diatomic oxygen, O2, and ensures that both oxygen atoms satisfy the octet rule.<\/p>\n\n\n\n Which choice presents the Lewis dot structure for diatomic oxygen The Correct Answer and Explanation is: The Lewis dot structure for diatomic oxygen (O2) can be drawn as follows: O=O with each oxygen atom having 6 valence electrons, and each shared pair of electrons forming a covalent bond between the two oxygen atoms. Here’s a […]<\/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-240374","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/240374","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=240374"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/240374\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=240374"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=240374"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=240374"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Step 1: Count the total valence electrons<\/h3>\n\n\n\n
Step 2: Connect the two oxygen atoms<\/h3>\n\n\n\n
Step 3: Distribute the remaining electrons<\/h3>\n\n\n\n
Final Lewis structure:<\/h3>\n\n\n\n
Explanation:<\/h3>\n\n\n\n
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